Periodic Trends and Index of Boron Lewis Acidity

Size: px
Start display at page:

Download "Periodic Trends and Index of Boron Lewis Acidity"

Transcription

1 Periodic Trends and Index of Boron Lewis Acidity Joshua A. Plumley and Jeffrey D. Evanseck * Contribution from the Center for Computational Sciences and the Department of Chemistry and Biochemistry, Duquesne University, 600 Forbes Avenue, Pittsburgh, Pennsylvania * Corresponding author: Hevanseck@duq.eduH Supporting Information Contents Other Electronegativities Considered... 8 Figure S1: Allen... 8 Figure S2: Sanderson... 8 Figure S3: Allred Rochow... 9 Figure S4: Mulliken Jaffe... 9 Figure S Figure S Figure S Figure S Figure S Figure S Figure S Figure S Coefficients of Partial Determination Optimized Structures and Thermodynamic Data: B3LYP/6 31G(d) NH BH

2 BH 2 F BHF BF BClF BCl 2 F BCl BHCl BH 2 Cl B(OH) BH(OH) BH 2 (OH) B(CH 3 ) BH(CH 3 ) BH 2 (CH 3 ) B(SH) BH(SH) BH 2 (SH) B(SiH 3 ) BH(SiH 3 ) BH 2 (SiH 3 ) BH 3 NH BH 2 F NH BHF 2 NH BF 3 NH BClF 2 NH BCl 2 F NH BCl 3 NH BHCl 2 NH BH 2 Cl NH B(OH) 3 NH

3 BH(OH) 2 NH BH 2 (OH) NH B(CH 3 ) 3 NH BH(CH 3 ) 2 NH BH 2 (CH 3 ) NH B(SH) 3 NH BH(SH) 2 NH BH 2 (SH) NH B(SiH 3 ) 3 NH BH 2 (SiH 3 ) NH BH(SiH 3 ) 2 NH Optimized Structures and Counterpoise Corrections: QCISD(T),MP2, M06 2X NH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BH 2 F MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BHF MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BF MP2/ G(3df,2p)

4 QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BClF MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BCl 2 F MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BCl MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BHCl MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BH 2 Cl MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) B(OH) M06 2X/ G(3df,2p) BH(OH) M06 2X/ G(3df,2p) BH 2 (OH) M06 2X/ G(3df,2p) B(CH 3 ) M06 2X/ G(3df,2p)

5 BH(CH 3 ) M06 2X/ G(3df,2p) BH 2 (CH 3 ) M06 2X/ G(3df,2p) B(SH) M06 2X/ G(3df,2p) BH(SH) M06 2X/ G(3df,2p) BH 2 (SH) M06 2X/ G(3df,2p) B(SiH 3 ) M06 2X/ G(3df,2p) BH(SiH 3 ) M06 2X/ G(3df,2p) BH 2 (SiH 3 ) M06 2X/ G(3df,2p) BH 3 NH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BH 2 F NH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BHF 2 NH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BF 3 NH MP2/ G(3df,2p)

6 QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BClF 2 NH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BCl 2 F NH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BCl 3 NH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BHCl 2 NH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) BH 2 Cl NH MP2/ G(3df,2p) QCISD(T)/aug cc pvqz//mp2/ G(3df,2p) M06 2X/ G(3df,2p) B(OH) 3 NH M06 2X/ G(3df,2p) BH(OH) 2 NH M06 2X/ G(3df,2p) BH 2 (OH) NH M06 2X/ G(3df,2p) B(CH 3 ) 3 NH M06 2X/ G(3df,2p)

7 BH(CH 3 ) 2 NH M06 2X/ G(3df,2p) BH 2 (CH 3 ) NH M06 2X/ G(3df,2p) B(SH) 3 NH M06 2X/ G(3df,2p) BH(SH) 2 NH M06 2X/ G(3df,2p) BH 2 (SH) NH M06 2X/ G(3df,2p) B(SiH 3 ) 3 NH M06 2X/ G(3df,2p) BH 2 (SiH 3 ) NH M06 2X/ G(3df,2p) BH(SiH 3 ) 2 NH M06 2X/ G(3df,2p) References

8 Other Electronegativities Considered Figure S1: Allen Boron Valence Deficiency 2.0 R² = Allen Electronegativity Figure S 1. Boron s valence deficiency (electrons) vs. the average Allen electronegativitity 1 of the atoms coordinated to boron. Second and third period atoms as well as hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/cc-pVQZ//M06-2X// G(3df,2p). Figure S2: Sanderson Boron Valence Deficiency 2.0 R² = Sanderson Electronegativity Figure S 2. Boron s valence deficiency (electrons) vs. the average Sanderson electronegativitiy 2 of the atoms coordinated to boron. Second and third period atoms as well as hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/cc-pVQZ//M06-2X// G(3df,2p). 8

9 Figure S3: Allred Rochow Boron Valence Deficiency R² = Allred-Rochow Electronegativity Figure S 3. Boron s valence deficiency (electrons) vs. the average Allred-Rochow electronegativity 3 of the atoms coordinated to boron. Second and third period atoms as well as hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO HF/ccpVQZ//M06-2X// G(3df,2p). Figure S4: Mulliken Jaffe Boron Valence Deficiency 2.0 R² = Mulliken-Jaffe Electronegativity Figure S 4. Boron s valence deficiency (electrons) vs. the average Mulliken-Jaffe electronegativity 4-6 of the atoms coordinated to boron. Second and third period atoms as well as hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/cc-pVQZ//M06-2X// G(3df,2p). 9

10 Figure S5 Boron Valence Deficiency BF 3 BHF 2 BH 2 F BH 2 OH B(OH) 3 BH(OH) 2 BH 3 BH 2 (CH 3 ) R² = 0.33 B(CH 3 ) 3 BH(CH 3 ) Atomic Radii Figure S 5. Boron s valence deficiency (electrons) vs. the sum of atomic radii (Å) coordinated to boron. Only second period atoms and hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/cc-pVQZ//M06-2X// G(3df,2p). Figure S6 Boron Valence Deficiency 1.0 (B) R² = BH 2 Cl BCl 3 BHCl BH 2 3 BH 2 (SH) B(SH) BH(SH)2 3 BH 2 (SiH 3 ) BH(SiH 3 ) 2 B(SiH 3 ) Atomic Radii Figure S 6. Boron s valence deficiency (electrons) vs. the sum of atomic radii (Å) coordinated to boron. Only third period atoms and hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/cc-pVQZ//M06-2X// G(3df,2p). 10

11 Figure S7 Boron Valence Deficiency 1.0 R² = BH 2 (SH) BH 2 Cl BH 3 BHCl 2 BCl 3 BH 2 (SiH 3 ) B(SH) 3 BH(SiH 3 ) 2 B(SiH3)3 BH(SH) Electronegativity Figure S 7. Boron s valence deficiency (electrons) vs. the average Pauling electronegativity of the atoms coordinated to boron. Only third period atoms and hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/cc-pVQZ//M06-2X// G(3df,2p). Figure S8 Boron Valence Deficiency BH 2 (CH 3 ) B(CH 3 ) 3 BH(CH 3 ) 2 R² = 0.68 BH 3 BH 2 (SiH 3 ) BH(SiH 3 ) 2 B(SiH 3 ) Atomic Radii Figure S 8. Boron s valence deficiency (electrons) vs. the sum of atomic radii (Å) coordinated to boron. Only Group 14 atoms (carbon periodic group) and hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/ccpVQZ//M06-2X// G(3df,2p). 11

12 Figure S9 Boron Valence Deficiency BH 2 (OH) BH(OH) 2 BH 3 BH 2 (SH) BH(SH) 2 B(SH) 3 R² = 0.76 B(OH) Electronegativity Figure S 9. Boron s valence deficiency (electrons) vs. the average Pauling electronegativity of the atoms coordinated to boron. Only Group 16 atoms (oxygen periodic group) and hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/cc-pVQZ. Figure S10 Boron Valence Deficiency BH 2 (OH) B(OH) 3 BH(OH) 2 BH 3 BH 2 (SH) Figure S 10. Boron s valence deficiency (electrons) vs. the sum of atomic radii (Å) coordinated to boron. Only Group 16 atoms (oxygen periodic group) and hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/ccpVQZ//M06-2X// G(3df,2p). 12 R² = 0.65 BH(SH) 2 B(SH) Atomic Radii

13 Figure S11 Boron Valence Deficiency 2.0 R² = BF 3 BClF 2 BHF 2 BH 2 F BCl2F BH 3 BCl 3 BH 2 Cl BHCl Electronegativity Figure S 11. Boron s valence deficiency (electrons) vs. the average Pauling electronegativity of the atoms coordinated to boron. Only Group 17 atoms (fluorine periodic group) and hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/cc-pVQZ//M06-2X// G(3df,2p). Figure S12 Boron Valence Deficiency BF 3 BHF 2 BH 2 F BClF 2 BCl 2 F BH BCl 3 3 BH 2 Cl BHCl 2 R² = Atomic Radii Figure S 12. Boron s valence deficiency (electrons) vs. the sum of atomic radii (Å) coordinated to boron. Only Group 17 atoms (fluorine periodic group) and hydrogen are considered. Boron s valence deficiency is the formal valence of three minus the valence electrons predicted by NBO employing HF/ccpVQZ//M06-2X// G(3df,2p). 13

14 Coefficients of Partial Determination 7 The coefficient of partial determination (r 2 ) has been analyzed in order to determine the importance of each independent variable (substituent electronegativity and atomic radii) when modeling the dependent variable s variance (boron s valence deficiency). The coefficient of partial determination measures the contribution of one independent variable when added to a model containing other independent variables. For example, the regarding a multiple linear regression containing a dependent variable ( ) and two independent variables ( and ) would take the following form:., Where is defined as the error sum of squares of the regression incorporating the independent variables within the parentheses. The entries to the right of the dot within the subscript of. indicate the variable that is already within the model where the entries to the left indicate the dependent variable as well as the independent variable being introduced to the model. Multiplying the result by 100 yields a percent decrease in the error sum of squares when is added to the model that already contains. Comparing coefficients of partial determination allows the importance of each variable to be assessed. For example, if is added to a model that contains only, and the error sum of squares is decreased to a greater extent than when is added to the model that contains only, than is more important than when modeling the variance of. Table S1 summarizes the coefficients of partial determination for each multiple linear regression discussed. 14

15 Table S1. Partial coefficients of determination regarding boron s valence deficiency (Y) vs. a linear combination of substituent electronegativity (EN) and atomic radii (AR). Plot.. Figure 4 a Figure 6 b Figure 7 c a Only third period atoms and hydrogen are considered. b Only group sixteen atoms (oxygen periodic group) and hydrogen are considered. c Only group seventeen atoms (fluorine periodic group) and hydrogen are considered. The data indicates that when substituent electronegativity or atomic radii is added to a model that contains the other variable, the error sum of squares decreases to about the same extent. This suggests that each is equally important when modeling the boron valence deficiency. 15

16 Optimized Structures and Thermodynamic Data: B3LYP/6 31G(d) NH (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) H3N1 PCUSER 29-Jan #N Geom=A llcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq H3B-NH3 0, 1 N X,1,1. H,1,B1,2,A1 H,1,B1,2,A1,3,D1,0 H,1,B1,2,A1,4,D2,0 B1= A1= D1=-120. D2=-120. Version=IA32W-G03RevD.01 Stat e=1-a1 HF= RMSD=4.490e-011 RMSF=4.317e-005 ZeroPoint= Thermal= Dipole=0.,0., DipoleDeriv= ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., , , , , , , , , , , , , , , , , , , Polar= ,0., , ,0., PG=C03V [C3(N1),3SGV(H1)] NImag=0 BH (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1H3 PCUSER 18-Dec #P Geom=A 16

17 llcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq Title Card Required 0,1 B H,1,B1 H,1,B2,2,A1 H,1,B3,3,A2,2,D1,0 B1= B 2= B3= A1= A2= D1=180. Ve rsion=ia32w-g03revd.01 State=1-A1' HF= RMSD=8.535e-011 RMSF =3.725e-005 ZeroPoint= Thermal= Dipole=0.,0.,0. Dipo lederiv= ,0.,0.,0., ,0.,0.,0., , ,0.,0.,0., ,0.,0.,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., Polar= ,0., ,0.,0., PG=D03H [O(B1),3C2(H1)] NImag=0 BH2F (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1F1H2 PCUSER 15-Sep #P Geom =AllCheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq title 0, 1 B F,1,B1 H,1,B2,2,A1 H,1,B2,2,A1,3,D1,0 B1= B2= A1= D1=180. Version=IA32W-G03RevD.01 State=1-A1 HF= RMSD=1.003e-009 RMSF=4.363e-005 ZeroPoint= Thermal= Dipole=0.,0., DipoleDeriv= ,0.,0.,0., ,0.,0.,0., , ,0.,0.,0., ,0.,0.,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., Polar = ,0., ,0.,0., PG=C02V [C2(B1F1),SGV(H2)] N Imag=0 BHF (Hartree/Particle) Thermal correction to Energy=

18 Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1F2H1 PCUSER 15-Sep #P Geom =AllCheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq Title Car d Required 0,1 B H,1,B1 F,1,B2,2,A1 F,1,B2,2,A1,3,D1,0 B1= B2= A1= D1=180. Version=IA32W-G03RevD.01 State =1-A1 HF= RMSD=7.274e-011 RMSF=1.623e-005 ZeroPoint= Thermal= Dipole=0.,0., DipoleDeriv= ,0., 0.,0., ,0.,0.,0., , ,0.,0.,0., ,0.,0.,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., Polar= ,0., ,0.,0., PG=C02V [C2(B1H1 ),SGV(F2)] NImag=0 BF BClF (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= \1\GINC-NEWTON\Freq\RB3LYP\6-31G(d)\B1F3\JOSH\19-Dec-2006\1\\#P GEOM= ALLCHECK GUESS=READ SCRF=CHECK GENCHK RB3LYP/6-31G(D) FREQ\\Title Card Required\\0,1\B\F,1,B1\F,1,B2,2,A1\F,1,B3,3,A2,2,D1,0\\B1= \ B2= \B3= \A1= \A2= \D1=180.\\V ersion=ia64-linux-g03revb.05\state=1-a1'\hf= \rmsd=7.184e-1 0\RMSF=2.767e-05\Dipole=0.,0.,0.\DipoleDeriv= ,0.,0.,0., ,0.,0.,0., , ,0.,0.,0., ,0.,0.,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., \Polar = ,0., ,0.,0., \PG=D03H [O(B1),3C2(F1)]\NImag =0\\

19 (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1Cl1F2 PCUSER 17-Sep #P Geo m=allcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq title 0,1 B Cl,1,B1 F,1,B2,2,A1 F,1,B2,2,A1,3,D1,0 B1= B2= A1= D1=180. Version=IA32W-G03RevD.01 State=1-A1 HF= RMSD=2.412e-010 RMSF=5.165e-005 ZeroPoint= Thermal= Dipole=0.,0., DipoleDeriv= ,0.,0.,0., ,0.,0.,0., , ,0.,0.,0., ,0.,0.,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., Polar= ,0., ,0.,0., PG=C02V [C2(B1Cl1),SGV(F2)] NImag=0 BCl2F (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1Cl2F1 PCUSER 17-Sep #P Geo m=allcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq Title Ca rd Required 0,1 B F,1,B1 Cl,1,B2,2,A1 Cl,1,B2,2,A1,3,D1,0 B1= B2= A1= D1=180. Version=IA32W-G03RevD.01 Sta te=1-a1 HF= RMSD=7.958e-010 RMSF=2.450e-005 ZeroPoint= Thermal= Dipole=0.,0., DipoleDeriv= , 0.,0.,0., ,0.,0.,0., , ,0.,0.,0., ,0.,0.,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., Polar= ,0., ,0.,0., PG=C02V [C2(B 1F1),SGV(Cl2)] NImag=0 19

20 BCl (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1Cl3 PCUSER 10-Sep #P Geom= AllCheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq Title Card Required 0,1 B Cl,1,B1 Cl,1,B2,2,A1 Cl,1,B3,3,A2,2,D1,0 B1= B2= B3= A1= A2= D1=180. Version=IA32W-G03RevD.01 State=1-A1' HF= RMSD=6.233e-009 RMSF=6.110e-007 ZeroPoint= Thermal= Dipole=0.,0.,0. DipoleDeriv= ,0.,0.,0., ,0.,0.,0., , ,0.,0.,0., ,0.,0.,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., Polar= ,0., ,0.,0., PG=D03H [O(B1),3C2(Cl1)] NImag=0 BHCl (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1Cl2H1 PCUSER 15-Sep #P Geo 20

21 m=allcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq Title Ca rd Required 0,1 B H,1,B1 Cl,1,B2,2,A1 Cl,1,B2,2,A1,3,D1,0 B1= B2= A1= D1=180. Version=IA32W-G03RevD.01 Sta te=1-a1 HF= RMSD=8.796e-010 RMSF=1.179e-005 ZeroPoint= Thermal= Dipole=0.,0., DipoleDeriv= ,0.,0.,0., ,0.,0.,0., , ,0.,0.,0., ,0., 0.,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., Polar= ,0., ,0.,0., PG=C02V [C2(B 1H1),SGV(Cl2)] NImag=0 BH2Cl (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= \1\GINC-NEWTON\Freq\RB3LYP\6-31G(d)\B1Cl1H2\JOSH\15-Sep-2007\1\\#P Ge om=allcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq\\title\\ 0,1\B\Cl,1,B1\H,1,B2,2,A1\H,1,B2,2,A1,3,D1,0\\B1= \B2= \A1= \D1=180.\\Version=IA64L-G03RevD.01\State=1-A1\HF= \RMSD=1.051e-09\RMSF=5.720e-05\ZeroPoint= \Thermal= \Dipole=0.,0., \DipoleDeriv= ,0.,0.,0., ,0.,0.,0., , ,0.,0.,0., ,0.,0.,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., \Polar = ,0., ,0.,0., \PG=C02V [C2(B1Cl1),SGV(H2)] \NImag=0\\ B(OH)

22 (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= \1\GINC-PAULING\Freq\RB3LYP\6-31G(d)\B1H3O3\JOSH\26-Aug-2008\0\\#p b3 LYP/6-31G(d) freq\\title Card Required\\0,1\B,0., ,0.\O, , ,0.\H, , ,0.\O, , ,0.\H, , ,0.\O, , ,0.\H, , ,0.\\Version=IA64L-G03Rev E.01\State=1-A'\HF= \RMSD=7.205e-09\RMSF=6.583e-05\ZeroPoin t= \thermal= \dipole=0.,0.,0.\dipolederiv= , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0., 0.,0., , , ,0., , ,0.,0.,0., \Polar= , , ,0.,0., \PG=C 03H [O(B1),SGH(H3O3)]\NImag=0\\ BH(OH) (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1H3O2 PCUSER 26-Aug #p b3ly P/6-31G(d) freq Title Card Required 0,1 B, , , 0. O, , ,0. H, , ,0. O, , ,0. H, , ,0. H, , ,0. Version=IA32W-G03RevE.01 State=1-A' HF= RMSD=8.275e-009 RMSF=6.576e-005 ZeroPoint= Thermal= Dipole= , ,0. DipoleDeriv= , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0., 0.,0., , , ,0., , ,0.,0.,0., Polar= , , ,0.,0., PG=C 22

23 S [SG(B1H3O2)] NImag=0 BH2(OH) (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1H3O1 PCUSER 26-Aug #p b3ly P/6-31G(d) freq Title Card Required 0,1 B, , , 0. O, , ,0. H, , ,0. H, , ,0. H, , ,0. Version =IA32W-G03RevE.01 State=1-A' HF= RMSD=8.687e-009 RMSF=3.20 2e-005 ZeroPoint= Thermal= Dipole= , ,0. DipoleDeriv= , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., Polar= , , ,0.,0., PG=CS [SG(B1H3O1)] NImag=0 B(CH3)

24 BH(CH3) (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) C3H9B1 PCUSER 22-Dec #P Geom =AllCheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq Title Car d Required 0,1 B C,1,r1 C,1,r1,2,a1 C,1,r1,2,a1,3,d1,0 H,2,r2,1,a2,3, d2,0 H,2,r2,1,a2,3,-d2,0 H,2,r3,1,a3,3,d1,0 H,3,r2,1,a2,4,d2,0 H,3,r2, 1,a2,4,-d2,0 H,3,r3,1,a3,4,d1,0 H,4,r2,1,a2,2,d2,0 H,4,r2,1,a2,2,-d2,0 H,4,r3,1,a3,2,d1,0 r1= r2= r3= a1= a2= a3= d2= d1=180. Version =IA32W-G03RevD.01 State=1-A' HF= RMSD=5.941e-009 RMSF=3.88 7e-005 ZeroPoint= Thermal= Dipole=0.,0.,0. DipoleDeri v= ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., , , , , , , , , , , , , , , , , , , , ,0., ,0., ,0., ,0., , , , , , , , , , , , , , , , , , , , ,0., ,0., ,0., ,0., , , , , , , , , , , , , , , , , , , , ,0., ,0., ,0., ,0., Polar= ,0., , ,0., PG=C03H [O(B1),SGH(C3H3),X(H6)] NImag= (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies=

25 1\1\GINC-PAULING\Freq\RB3LYP\6-31G(d)\C2H7B1\JOSH\26-Aug-2008\0\\#p fr eq rb3lyp/6-31g(d)\\title Card Required\\0,1\B, , , \H, , , \C, , , \H, , , \ H, , , \H, , , \C, , , \H, , , \H, , , \H, , , \\Version=IA64L-G03RevE. 01\State=1-A\HF= \RMSD=8.490e-09\RMSF=2.875e-06\ZeroPoint= \Thermal= \Dipole= , , \Dipo lederiv= , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , \Polar= , , , , , \PG=C01 [X(C2H7B1)]\NImag=0\\ BH2(CH3) (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= \1\GINC-PAULING\Freq\RB3LYP\6-31G(d)\C1H5B1\JOSH\26-Aug-2008\0\\#p fr eq rb3lyp/6-31g(d)\\title Card Required\\0,1\B, , , \H, , , \H, , , \C, , , \H, , , \H, , , \H, , , \\Version= IA64L-G03RevE.01\State=1-A'\HF= \RMSD=4.510e-09\RMSF=2.368e- 05\ZeroPoint= \Thermal= \Dipole= , , \DipoleDeriv= , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , ,- 25

26 , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , \Polar= , , , , , \PG=CS [SG(C1H1B1),X(H 4)]\NImag=0\\ B(SH) (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1H3S3 PCUSER 26-Aug #p b3ly P/6-31G(d) freq Title Card Required 0,1 B,0., ,0. S, , ,0. H, , ,0. S, , ,0. H, , ,0. S, , ,0. H, , ,0. Version=IA32W-G03RevE. 01 State=1-A' HF= RMSD=1.560e-009 RMSF=1.326e-004 ZeroPoi nt= Thermal= Dipole=0.,0.,0. DipoleDeriv= , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0., 0.,0., Polar= , , ,0.,0., PG=C03H [O(B1),SGH(H3S3)] NImag=0 BH(SH)

27 (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1H3S2 PCUSER 26-Aug #p b3ly P/6-31G(d) freq Title Card Required 0,1 B, , , 0. S, , ,0. H, , ,0. S, , ,0. H, , ,0. H, , ,0. Version=IA32W-G03RevE.01 State=1-A' HF= RMSD=1.860e-009 RMSF=1.337e-004 ZeroPoint= Thermal= Dipole= , ,0. DipoleDeriv= , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., Polar= , , ,0.,0., PG=CS [SG(B1H3S2)] NImag=0 BH2(SH) (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1H3S1 PCUSER 26-Aug #p b3ly P/6-31G(d) freq Title Card Required 0,1 B, , , 0. S, , ,0. H, , ,0. H, , ,0. H, , ,0. Version =IA32W-G03RevE.01 State=1-A' HF= RMSD=1.272e-009 RMSF=8.08 7e-005 ZeroPoint= Thermal= Dipole= , ,0. DipoleDeriv= , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., Polar= , , ,0.,0., PG=CS [SG(B1H3S1)] NImag =0 27

28 B(SiH3) (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= \1\GINC-PAULING\Freq\RB3LYP\6-31G(d)\B1H9Si3\JOSH\27-Aug-2008\0\\#P G eom=allcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq\\Title Card Required\\0,1\B, , ,0.\Si, , ,0.\Si, , , \Si, , , \H, , ,0.\H, , , \H, , , \H, , , \H, , , \H, , , \H, , , \H, , , \H, , , \\Version=IA64L-G0 3RevE.01\State=1-A'\HF= \RMSD=5.557e-09\RMSF=1.541e-06\Zero Point= \Thermal= \Dipole= , ,0.\Dipol ederiv= , ,0., , ,0.,0.,0., , , ,0., , ,0.,0.,0., , , , , , , , , , , , , , , , , , , , , ,0., , ,0.,0.,0., , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , \Polar= , , , , , \PG=CS [SG(B1H1Si1),X(H8Si2)]\NImag=0\\ 28

29 BH(SiH3) (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1H7Si2 PCUSER 27-Aug #P Geo m=allcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq Title Ca rd Required 0,1 B, , , H, , , Si, , , H, , , H, , , H, , , Si, , , H, , , H, , , H, , , Version=IA32W-G03RevE.01 State=1-A HF= RMSD=3.783e-009 RMSF=6.613e-006 ZeroPoint= Thermal= Dipole= , , DipoleDeriv= , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , Polar= , , , , , PG=C01 [X(B1H7Si2)] NImag=0 BH2(SiH3)

30 (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1H5Si1 PCUSER 27-Aug #P Geo m=allcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq Title Ca rd Required 0,1 B, , , H, , , H, , , Si, , , H, , , H, , , H, , , Version=IA32W-G03RevE.01 State=1-A HF= RMSD=4.752e-010 RMSF=5.972e-005 ZeroPoint= T hermal= Dipole= , , DipoleDeriv= , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , , Polar= , , , , , PG=C01 [X(B1H5Si1)] NImag=0 BH3 NH (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies=

31 Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1H6N1 PCUSER 29-Jan #N Geom =AllCheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq H3B-NH3 0,1 B N,1,r1 H,1,r2,2,a1 H,1,r2,2,a1,3,120.,0 H,1,r2,2,a1,3,-120.,0 H, 2,r3,1,a2,3,180.,0 H,2,r3,1,a2,3,60.,0 H,2,r3,1,a2,3,-60.,0 r1= r2= r3= a1= a2= Vers ion=ia32w-g03revd.01 State=1-A1 HF= RMSD=5.146e-010 RMSF=4. 753e-005 ZeroPoint= Thermal= Dipole=0.,0., DipoleDeriv= ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., , , , , , , , , , , , , , , , , , , , ,0., ,0., ,0., ,0., , , , , , , , , , , , , , , , , , , Polar= ,0., , ,0., PG=C03V [C3(B1N1),3SGV(H2)] NImag=0 BH2F NH (Hartree/Particle) Thermal correction to Energy= Thermal correction to Enthalpy= Thermal correction to Gibbs Free Energy= Sum of electronic and zero-point Energies= Sum of electronic and thermal Energies= Sum of electronic and thermal Enthalpies= Sum of electronic and thermal Free Energies= UNPC-UNK Freq RB3LYP 6-31G(d) B1F1H5N1 PCUSER 15-Sep #P Ge om=allcheck Guess=Read SCRF=Check GenChk RB3LYP/6-31G(d) Freq Title C ard Required 0,1 B N,1,r1 F,1,r4,2,a3 H,1,r2,2,a1,3,d1,0 H,1,r2,2,a1, 3,-d1,0 H,2,r5,1,a4,3,180.,0 H,2,r3,1,a2,3,d2,0 H,2,r3,1,a2,3,-d2,0 r 1= r2= r3= r4= r5= a 1= a2= a3= a4= d1= d2= Version=IA32W-G03RevD.01 State=1-A' HF= RMSD=4.181e-010 RMSF=5.668e-005 ZeroPoint= Thermal= Dipole= ,0., DipoleDeriv= ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., , ,0., ,0., ,0., ,0., , , , , , , , , , , , , , , , , , , , ,0., ,0., ,0., ,0.,

Reduction of 4-Styrylpyridine by SmI 2 : An Inner Sphere ET Case where the Binding Site Differs from the Reaction Center

Reduction of 4-Styrylpyridine by SmI 2 : An Inner Sphere ET Case where the Binding Site Differs from the Reaction Center Supporting Information Reduction of 4-Styrylpyridine by SmI 2 : An Inner Sphere ET Case where the Binding Site Differs from the Reaction Center Ramesh Yella, Shmaryahu Hoz* Department of Chemistry, Bar-Ilan

More information

Electronegativity (MHR Text p ) Draw an electron dot formula for HCl.

Electronegativity (MHR Text p ) Draw an electron dot formula for HCl. http://www.youtube.com/user/kosasihiskandarsjah#p/u/45/kj3o0xvhvqq Electronegativity (MHR Text p. 174 175) Draw an electron dot formula for HCl. The formula suggests that the pair of electrons, which constitutes

More information

Bonding/Lewis Dots Lecture Page 1 of 12 Date. Bonding. What is Coulomb's Law? Energy Profile: Covalent Bonds. Electronegativity and Linus Pauling

Bonding/Lewis Dots Lecture Page 1 of 12 Date. Bonding. What is Coulomb's Law? Energy Profile: Covalent Bonds. Electronegativity and Linus Pauling Bonding/Lewis Dots Lecture Page 1 of 12 Date Bonding What is Coulomb's Law? Energy Profile: Covalent Bonds Electronegativity and Linus Pauling 2.1 H 1.0 Li 0.9 Na 0.8 K 0.8 Rb 0.7 Cs 0.7 Fr 1.5 Be 1.2

More information

QUANTUM CHEMISTRY PROJECT 3: PARTS B AND C

QUANTUM CHEMISTRY PROJECT 3: PARTS B AND C Chemistry 460 Fall 2017 Dr. Jean M. Standard November 6, 2017 QUANTUM CHEMISTRY PROJECT 3: PARTS B AND C PART B: POTENTIAL CURVE, SPECTROSCOPIC CONSTANTS, AND DISSOCIATION ENERGY OF DIATOMIC HYDROGEN (20

More information

Chemical bonding is the combining of elements to form new substances.

Chemical bonding is the combining of elements to form new substances. Name Covalent Bonding and Nomenclature: Unit Objective Study Guide Class Period Date Due 1. Define chemical bonding. What is chemical bonding? Chemical bonding is the combining of elements to form new

More information

All chemical bonding is based on the following relationships of electrostatics: 2. Each period on the periodic table

All chemical bonding is based on the following relationships of electrostatics: 2. Each period on the periodic table UNIT VIII ATOMS AND THE PERIODIC TABLE 25 E. Chemical Bonding 1. An ELECTROSTATIC FORCE is All chemical bonding is based on the following relationships of electrostatics: The greater the distance between

More information

Chemical Bonding I: Covalent Bonding. How are atoms held together in compounds?

Chemical Bonding I: Covalent Bonding. How are atoms held together in compounds? I: Covalent Bonding How are atoms held together in compounds? IONIC or COVALENT bonds or forces For most atoms, a filled outer shell contains 8 electrons ----- an octet Atoms want to form octets when they

More information

1. Following Dalton s Atomic Theory, 2. In 1869 Russian chemist published a method. of organizing the elements. Mendeleev showed that

1. Following Dalton s Atomic Theory, 2. In 1869 Russian chemist published a method. of organizing the elements. Mendeleev showed that 20 CHEMISTRY 11 D. Organizing the Elements The Periodic Table 1. Following Dalton s Atomic Theory, By 1817, chemists had discovered 52 elements and by 1863 that number had risen to 62. 2. In 1869 Russian

More information

Houston Community College System. Chemistry EXAM # 3A Sample

Houston Community College System. Chemistry EXAM # 3A Sample Houston Community College System Chemistry 1411 EXAM # A Sample 1 CHEM 1411 EXAM # (Chapters 8, 9,10,and 11) Name: Score: Directions- please answer the following multiple-choice questions next to each

More information

Review Package #3 Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding

Review Package #3 Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding Chemistry 11 Review Package #3 Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding 1. Atomic Models and Subatomic Particles: A. Subatomic Particles and Average Atomic Mass: - Subatomic

More information

Chemical Bonding 4.8. Valence Bond Theory Hybrid Orbital Theory Multiple Bonds High School Chem Solutions. All rights reserved.

Chemical Bonding 4.8. Valence Bond Theory Hybrid Orbital Theory Multiple Bonds High School Chem Solutions. All rights reserved. Chemical Bonding 4.8 Valence Bond Theory Hybrid Orbital Theory Multiple Bonds Valence Bond Theory Combines Lewis theory of filling octets by sharing pairs of electrons with the electron configuration of

More information

Acid-Base Strength. Chapter 6. Monday, November 2, 2015

Acid-Base Strength. Chapter 6. Monday, November 2, 2015 Acid-Base Strength Chapter 6 Monday, November 2, 2015 Acid-Base Strength We ve seen that the reactivity of acids and bases can be viewed through the HSAB Model or the EC Model. Both of these models try

More information

Bond Atoms Electron behavior Ionic Metal + nonmetal Electrons transferred Covalent Nonmetal + nonmetal Electrons shared

Bond Atoms Electron behavior Ionic Metal + nonmetal Electrons transferred Covalent Nonmetal + nonmetal Electrons shared ch9blank Page 1 Chapter 9: Chemical Bonding I: Lewis Theory Three types of chemical bonding: Bond Atoms Electron behavior Ionic Metal + nonmetal Electrons transferred Covalent Nonmetal + nonmetal Electrons

More information

Three types of chemical bonding: Recall that we can use dots to show valence electrons - these are called Lewis electron-dot structures:

Three types of chemical bonding: Recall that we can use dots to show valence electrons - these are called Lewis electron-dot structures: Chapter 9: Chemical Bonding I: Lewis Theory Three types of chemical bonding: Bond Atoms Electron behavior Ionic Metal + nonmetal Electrons transferred Covalent Nonmetal + nonmetal Electrons shared Metallic

More information

NPA/NBO-Analysis. Examples POP =

NPA/NBO-Analysis. Examples POP = NPA/NBO-Analysis Examples POP = NBO Requests a full Natural Bond Orbital analysis, using NBO version 3 NPA Requests just the Natural Population Analysis phase of NBO. NBORead Requests a full NBO analysis,

More information

Compare the strength of IMFs present in three liquids. The liquids are in separate containers. A. CH 3 CH 2 NH 2 (liquid) B. CH 3 CH 2 F (liquid)

Compare the strength of IMFs present in three liquids. The liquids are in separate containers. A. CH 3 CH 2 NH 2 (liquid) B. CH 3 CH 2 F (liquid) Compare the strength of IMFs present in three liquids. The liquids are in separate containers. A. CH 3 CH 2 NH 2 (liquid) B. CH 3 CH 2 F (liquid) C. CH 3 CH 2 OH (liquid) Draw two 3D Lewis Structures of

More information

CHEM 172 EXAMINATION 1. January 15, 2009

CHEM 172 EXAMINATION 1. January 15, 2009 CHEM 17 EXAMINATION 1 January 15, 009 Dr. Kimberly M. Broekemeier NAME: Circle lecture time: 9:00 11:00 Constants: c = 3.00 X 10 8 m/s h = 6.63 X 10-34 J x s J = kg x m /s Rydberg Constant = 1.096776 x

More information

The wavefunction that describes a bonding pair of electrons:

The wavefunction that describes a bonding pair of electrons: 4.2. Molecular Properties from VB Theory a) Bonding and Bond distances The wavefunction that describes a bonding pair of electrons: Ψ b = a(h 1 ) + b(h 2 ) where h 1 and h 2 are HAOs on adjacent atoms

More information

Chapter 7 Chemical Bonding and Molecular Structure

Chapter 7 Chemical Bonding and Molecular Structure Chapter 7 Chemical Bonding and Molecular Structure Three Types of Chemical Bonding (1) Ionic: formed by electron transfer (2) Covalent: formed by electron sharing (3) Metallic: attraction between metal

More information

CHEM 130 Exp. 8: Molecular Models

CHEM 130 Exp. 8: Molecular Models CHEM 130 Exp. 8: Molecular Models In this lab, we will learn and practice predicting molecular structures from molecular formulas. The Periodic Table of the Elements IA 1 H IIA IIIA IVA VA VIA VIIA 3 5

More information

CHEMISTRY - BURDGE-ATOMS FIRST 3E CH.6 - REPRESENTING MOLECULES.

CHEMISTRY - BURDGE-ATOMS FIRST 3E CH.6 - REPRESENTING MOLECULES. !! www.clutchprep.com CONCEPT: ELECTRON-DOT SYMBOLS Before we look at the first two bonding models, we have to figure out how to depict the valence electrons of bonding atoms. In the electron-dot symbol,

More information

Chapter 2: Acids and Bases

Chapter 2: Acids and Bases 1. Which of the following statements is a correct definition for a Brønsted-Lowry acid? A) Proton acceptor C) Electron pair acceptor B) Electron pair donor D) Proton donor 2. Which of the following statements

More information

Name: Block: Date: Atomic Radius: the distance from the center of the nucleus to the outer most electrons in an atom.

Name: Block: Date: Atomic Radius: the distance from the center of the nucleus to the outer most electrons in an atom. Name: Block: Date: Chemistry 11 Trends Activity Assignment Atomic Radius: the distance from the center of the nucleus to the outer most electrons in an atom. Ionic Radius: the distance from the center

More information

Chapter 8. Chemical Bonding I: Basic Concepts

Chapter 8. Chemical Bonding I: Basic Concepts Chapter 8 Chemical Bonding I: Basic Concepts Topics Lewis Dot Symbols Ionic Bonding Covalent Bonding Electronegativity and Polarity Drawing Lewis Structures Lewis Structures and Formal Charge Resonance

More information

CH 222 Chapter Seven Concept Guide

CH 222 Chapter Seven Concept Guide CH 222 Chapter Seven Concept Guide 1. Lewis Structures Draw the Lewis Dot Structure for cyanide ion, CN -. 1 C at 4 electrons = 4 electrons 1 N at 5 electrons = 5 electrons -1 charge = + 1 electron Total

More information

Chapter 8. forces of attraction which hold atoms or ions together. 3 fundamental types of bonding. Ionic - metals & nonmetals

Chapter 8. forces of attraction which hold atoms or ions together. 3 fundamental types of bonding. Ionic - metals & nonmetals Chapter 8 Basic Concepts of Chemical Bonding Chemical Bonds forces of attraction which hold atoms or ions together 3 fundamental types of bonding Ionic - metals & nonmetals Covalent - nonmetals (semimetals)

More information

Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics.

Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. Ch. 9 NOTES ~ Chemical Bonding NOTE: Vocabulary terms are in boldface and underlined. Supporting details are in italics. I. Review: Comparison of ionic and molecular compounds Molecular compounds Ionic

More information

Polarity main concepts

Polarity main concepts POLARITY Polarity main concepts A polar molecule has opposite charged ends (+ & -) The polarity of a bond is the result of a difference in electronegativity between the two bonded atoms A molecule can

More information

AP CHEMISTRY CHAPTERS 5 & 6 Problem Set #4. (Questions 1-13) Choose the letter that best answers the question or completes the statement.

AP CHEMISTRY CHAPTERS 5 & 6 Problem Set #4. (Questions 1-13) Choose the letter that best answers the question or completes the statement. NAME: AP CHEMISTRY CHAPTERS 5 & 6 Problem Set #4 (Questions 1-13) Choose the letter that best answers the question or completes the statement. (Questions 1-2) Consider atoms of the following elements.

More information

Chapter 8. Chemical Bonding: Basic Concepts

Chapter 8. Chemical Bonding: Basic Concepts Chapter 8. Chemical Bonding: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely

More information

Chapter 9 Ionic and Covalent Bonding

Chapter 9 Ionic and Covalent Bonding Chem 1045 Prof George W.J. Kenney, Jr General Chemistry by Ebbing and Gammon, 8th Edition Last Update: 06-April-2009 Chapter 9 Ionic and Covalent Bonding These Notes are to SUPPLIMENT the Text, They do

More information

AIM: HOW TO FORM COVALENT BONDS

AIM: HOW TO FORM COVALENT BONDS AIM: HOW TO FORM COVALENT BONDS DO NOW: EXPLAIN THE DIFFERENCE BETWEEN IONIC BONDING AND COVALENT BONDS. INCLUDE HOW THE PROPERTIES DIFFER IN SALTS AND MOLECULES, AND WHICH ELEMENTS ARE INVOLVED IN EACH

More information

2. Write the electron configuration notation and the electron dot notation for each: (a) Ni atom (b) Ni 2+ ion (c) Ni 3+ ion

2. Write the electron configuration notation and the electron dot notation for each: (a) Ni atom (b) Ni 2+ ion (c) Ni 3+ ion EXTRA HOMEWORK 2A 1. Predict whether each of the following types of matter will be bonded with ionic, covalent, or metallic bonds, and identify whether each will be composed of atoms, ions, or molcules

More information

Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons

Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons Covalent Bonds Ch. Why do atoms bond? Atoms want noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons For covalent bonds there is a of electrons to get an

More information

Periodic Trends. Atomic Radius: The distance from the center of the nucleus to the outer most electrons in an atom.

Periodic Trends. Atomic Radius: The distance from the center of the nucleus to the outer most electrons in an atom. Periodic Trends Study and learn the definitions listed below. Then use the definitions and the periodic table provided to help you answer the questions in the activity. By the end of the activity you should

More information

REVIEW: VALENCE ELECTRONS CHEMICAL BONDS: LEWIS SYMBOLS: CHEMICAL BONDING. What are valence electrons?

REVIEW: VALENCE ELECTRONS CHEMICAL BONDS: LEWIS SYMBOLS: CHEMICAL BONDING. What are valence electrons? REVIEW: VALENCE ELECTRONS 13 CHEMICAL BONDING What are valence electrons? Which groups on the periodic table readily give up electrons? What group readily accepts electrons? CHEMICAL BONDS: What are chemical

More information

CP Covalent Bonds Ch. 8 &

CP Covalent Bonds Ch. 8 & CP Covalent Bonds Ch. 8 & 9 2015-2016 Why do atoms bond? Atoms want stability- to achieve a noble gas configuration ( ) For bonds there is a transfer of electrons to get an octet of electrons For covalent

More information

Concepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds. David A. Katz Pima Community College Tucson, AZ

Concepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds. David A. Katz Pima Community College Tucson, AZ Concepts of Chemical Bonding and Molecular Geometry Part 1: Ionic and Covalent Bonds David A. Katz Pima Community College Tucson, AZ Chemical Bonds Three basic types of bonds: Ionic Electrostatic attraction

More information

Chapter 8. Bonding: General Concepts. Copyright 2017 Cengage Learning. All Rights Reserved.

Chapter 8. Bonding: General Concepts. Copyright 2017 Cengage Learning. All Rights Reserved. Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents (8.1) (8.2) (8.3) (8.4) (8.5) (8.6) (8.7) (8.8) Types of chemical bonds Electronegativity Bond polarity and dipole moments Ions: Electron

More information

Name Honors Chemistry / /

Name Honors Chemistry / / Name Honors Chemistry / / Lewis Structures & Resonance Structures Last chapter we studied ionic compounds. In ionic compounds electrons are gained or lost. In this chapter we are going to study covalent

More information

! Chemical!Bond!! Lewis!Diagram!(HI!#13)! o Ionic!and!covalent!bond!(M!+!NM!or!NM!+!NM)!(Complete!transfer!of!e S!or!sharing!of!e S )!

! Chemical!Bond!! Lewis!Diagram!(HI!#13)! o Ionic!and!covalent!bond!(M!+!NM!or!NM!+!NM)!(Complete!transfer!of!e S!or!sharing!of!e S )! !! Unit*2.*Atomic*Theory*! Molar!mass!calculation!using!the!abundance!of!isotopes!of!an!element!!!! Electron!configuration!(both!full!notation!and!core!notation)!(HI!#12)! o Neutral!atom,!anion,!cation!(ensure!you!know!the!rules!associated!with!ions)!

More information

Group 13 Elements ( Boron Family)

Group 13 Elements ( Boron Family) Unit -11 The p- Block Elements Total no. of groups- 6 ( Group 13-18) General electronic configuration- ns 2 np 1-6 ( except for He) The first member of p-block differs from remaining members of their corresponding

More information

Chemistry 1 1. Review Package #3. Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding

Chemistry 1 1. Review Package #3. Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding Chemistry 1 1 Review Package #3 Atomic Models and Subatomic Particles The Periodic Table Chemical Bonding properties 1. Atomic Models and Subatomic Particles: A. Subatomic Particles and Average Atomic

More information

Electronic supplementary information (ESI) for. Completing a family: LiCN 3 H 4, the lightest alkali metal guanidinate

Electronic supplementary information (ESI) for. Completing a family: LiCN 3 H 4, the lightest alkali metal guanidinate Electronic supplementary information (ESI) for Completing a family: LiCN 3 H 4, the lightest alkali metal guanidinate Peter Klaus Sawinski, a Volker L. Deringer a and Richard Dronskowski a,b, * a Institute

More information

Chapter 8 Test Study Guide AP Chemistry 6 points DUE AT TEST (Wed., 12/13/17) Date:

Chapter 8 Test Study Guide AP Chemistry 6 points DUE AT TEST (Wed., 12/13/17) Date: Chapter 8 Test Study Guide Name: AP Chemistry 6 points DUE AT TEST (Wed., 12/13/17) Date: Topics to be covered on the December 13, 2017 test: bond bond energy ionic bond covalent bond polar covalent bond

More information

Chemical Bonding Chapter 9

Chemical Bonding Chapter 9 Chemical Bonding Chapter 9 Covalent Bonds and Ionic Bonds: Octet Rule Explain each of the following observations in terms of the "octet rule": Na atoms and Cl atoms will combine to form NaCl. Why does

More information

Name: Hr: 8 Basic Concepts of Chemical Bonding

Name: Hr: 8 Basic Concepts of Chemical Bonding 8.1-8.2 8.3-8.5 8.5-8.7 8.8 Name: Hr: 8 Basic Concepts of Chemical Bonding 8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule State the type of bond (ionic, covalent, or metallic) formed between any

More information

Honors Chemistry - Unit 4 Bonding Part I

Honors Chemistry - Unit 4 Bonding Part I Honors Chemistry - Unit 4 Bonding Part I Unit 4 Packet - Page 1 of 8 Vocab Due: Quiz Date(s): Test Date: UT Quest Due: Bonding Vocabulary: see separate handout assignment OBJECTIVES: Chapters 4-8 Be able

More information

Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules

Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Fructose Water Ch 10 Chemical Bonding, Lewis Structures for Ionic & Covalent Compounds, and Predicting Shapes of Molecules Carbon Dioxide Ammonia Title and Highlight TN Ch 10.1 Topic: EQ: Right Side NOTES

More information

Atomic Structure and Bonding. Chapter 1 Organic Chemistry, 8 th Edition John McMurry

Atomic Structure and Bonding. Chapter 1 Organic Chemistry, 8 th Edition John McMurry Atomic Structure and Bonding Chapter 1 Organic Chemistry, 8 th Edition John McMurry 1 Common Elements Groups First row Second row In most organic molecules carbon is combined with relatively few elements

More information

I. Multiple Choice Questions (Type-I)

I. Multiple Choice Questions (Type-I) I. Multiple Choice Questions (Type-I) 1. Isostructural species are those which have the same shape and hybridisation. Among the given species identify the isostructural pairs. (i) [NF 3 and BF 3 ] [BF

More information

Chapter 6 Chemical Bonding

Chapter 6 Chemical Bonding Chapter 6 Chemical Bonding Section 6-1 Introduction to Chemical Bonding Chemical Bonds Valence electrons are attracted to other atoms, and that determines the kind of chemical bonding that occurs between

More information

CHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols

CHEMICAL BONDING. Chemical Bonds. Ionic Bonding. Lewis Symbols CHEMICAL BONDING Chemical Bonds Lewis Symbols Octet Rule whenever possible, valence electrons in covalent compounds distribute so that each main-group element is surrounded by 8 electrons (except hydrogen

More information

Chapter 8. Bonding: General Concepts

Chapter 8. Bonding: General Concepts Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.2 Electronegativity 8.3 Bond Polarity and Dipole Moments 8.4 Ions: Electron Configurations and Sizes 8.5 Energy

More information

Test Bank for Introductory Chemistry Essentials 5th Edition by Tro

Test Bank for Introductory Chemistry Essentials 5th Edition by Tro Test Bank for Introductory Chemistry Essentials 5th Edition by Tro Sample Introductory Chemistry, 5e (Tro) Chapter 10 Chemical Bonding 10.1 True/False Questions 1) Bonding theories are used to predict

More information

Polarity main concepts

Polarity main concepts POLARITY Polarity main concepts 1. A polar molecule has opposite charged ends (+ & -) 2. The polarity of a bond is the result of a difference in electronegativity between the two bonded atoms 3. A molecule

More information

Chapter 9. Ionic Compounds

Chapter 9. Ionic Compounds Chapter 9 Bonding Ionic Compounds Formed between metal and nonmetal Ionic solids: ions are arranged in a regular lattice Strong forces: attraction of ions for each other 1 Lattice Energy A measure of the

More information

Review for Chapter 4: Structures and Properties of Substances

Review for Chapter 4: Structures and Properties of Substances Review for Chapter 4: Structures and Properties of Substances You are responsible for the following material: 1. Terms: You should be able to write definitions for the following terms. A complete definition

More information

Name: 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron

Name: 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron Chemistry Section Name: MID TERM STUDY GUIDE Date: A. Multiple Choice. 1. The mass of a proton is approximately equal to the mass of (1) an alpha particle (2) a beta particle (3) a positron (4) a neutron

More information

Intramolecular Bonding. Chapters 4, 12 Chemistry Mr. McKenzie

Intramolecular Bonding. Chapters 4, 12 Chemistry Mr. McKenzie Intramolecular Bonding Chapters 4, 12 Chemistry Mr. McKenzie What determines the type of intramolecular bond? An intramolecular bond is any force that holds two atoms together to form a compound; 3 types

More information

Please pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED

Please pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED CHM-201 General Chemistry and Laboratory I Unit #4 Take Home Test Due December 13, 2018 Please pass in only this completed answer sheet on the day of the test. LATE SUBMISSIONS WILL NOT BE ACCEPTED CHM-201

More information

Chapter 8. Bonding: General Concepts

Chapter 8. Bonding: General Concepts Chapter 8 Bonding: General Concepts Chapter 8 Table of Contents 8.1 Types of Chemical Bonds 8.3 Bond Polarity and Dipole Moments 8.5 Energy Effects in Binary Ionic Compounds 8.6 Partial Ionic Character

More information

CHAPTER 8: BASIC CONCEPTS OF CHEMICAL BONDING. Bond-an attractive interaction between two or more atoms.

CHAPTER 8: BASIC CONCEPTS OF CHEMICAL BONDING. Bond-an attractive interaction between two or more atoms. CHAPTER 8: BASIC CONCEPTS OF CHEMICAL BONDING Bond-an attractive interaction between two or more atoms. Bonding is the "glue" that holds molecules together. Two extreme types: Ionic (transfer) Covalent

More information

Polar bonds, polar molecules and the shape of molecules.

Polar bonds, polar molecules and the shape of molecules. Chapter 3 Polar bonds, polar molecules and the shape of molecules. Polar and non-polar bonds In homonuclear diatomic molecules such as H 2 or Cl 2 electrons are shared equally between equal atoms. The

More information

Chapter 8: Bonding. Section 8.1: Lewis Dot Symbols

Chapter 8: Bonding. Section 8.1: Lewis Dot Symbols Chapter 8: Bonding Section 8.1: Lewis Dot Symbols The Lewis electron dot symbol is named after Gilbert Lewis. In the Lewis dot symbol, the element symbol represents the nucleus and the inner electrons.

More information

CHAPTER 12 CHEMICAL BONDING

CHAPTER 12 CHEMICAL BONDING Chemistry Name Hour Chemistry Approximate Timeline Students are expected to keep up with class work when absent. CHAPTER 12 CHEMICAL BONDING Day Plans for the day Assignment(s) for the day 1 Begin Chapter

More information

Chemistry Standard level Paper 1

Chemistry Standard level Paper 1 Chemistry Standard level Paper 1 Thursday 12 May 2016 (morning) 45 minutes Instructions to candidates Do not open this examination paper until instructed to do so. Answer all the questions. For each question,

More information

INTRODUCTION TO CHEMICAL BONDS

INTRODUCTION TO CHEMICAL BONDS INTRODUCTION TO CHEMICAL BONDS Chemical Bonds A general comparison of metals and nonmetals. Chemical Bonds Types of Chemical Bonding 1. Metal with nonmetal: electron transfer and ionic bonding 2. Nonmetal

More information

End of chapter exercises

End of chapter exercises End of chapter exercises Problem 1: Give one word/term for each of the following descriptions. 1. The distance between two adjacent atoms in a molecule. 2. A type of chemical bond that involves the sharing

More information

Chapter 8. Bonding: General Concepts

Chapter 8. Bonding: General Concepts Chapter 8 Bonding: General Concepts Chapter 8 Questions to Consider What is meant by the term chemical bond? Why do atoms bond with each other to form compounds? How do atoms bond with each other to form

More information

sharing or transferring electrons between atoms covalent ionic polar covalent Quantitative description: Quantum mechanics

sharing or transferring electrons between atoms covalent ionic polar covalent Quantitative description: Quantum mechanics Chapter. 3 Chemical Bonding: The Classical Description Two or more atoms approach -> their electrons interact and form new arrangements of electrons with lower total potential energy than isolated atoms

More information

properties) YOU NEED TO KNOW THESE!!!!

properties) YOU NEED TO KNOW THESE!!!! 4.2.A ReIntro to Bonding I Pledge : ( Initial ) DON T FORGET WHAT THIS REPRESENTS. Instructions: Provide a response for each question that is well thought out, satisfies the prompt, is clearly explained,

More information

Topic 4: Chemical Bonds. IB Chemistry SL Ms. Kiely Coral Gables Senior High

Topic 4: Chemical Bonds. IB Chemistry SL Ms. Kiely Coral Gables Senior High Topic 4: Chemical Bonds IB Chemistry SL Ms. Kiely Coral Gables Senior High 5th PERIOD Bell Ringer - review of 4.1 Quiz (revised) 1. What is the formula of a compound formed by magnesium and phosphate?

More information

Advanced Chemistry. Mrs. Klingaman. Chapter 5: Name:

Advanced Chemistry. Mrs. Klingaman. Chapter 5: Name: Advanced Chemistry Mrs. Klingaman Chapter 5: The Periodic Law Name: _ Mods: Chapter 5: The Periodic Law Reading Guide 5.1 History of the Periodic Table (pgs. 125-129) 1) What did Dimitri Mendeleev notice

More information

Atoms and The Periodic Table

Atoms and The Periodic Table Atoms and The Periodic Table A. Early Models of the Atom 1. The earliest models of the atom came in the 5 th century B.C. when In the 4 th century, B.C., rejected this idea and proposed that earthly matter

More information

Covalent Bonding. a. O b. Mg c. Ar d. C. a. K b. N c. Cl d. B

Covalent Bonding. a. O b. Mg c. Ar d. C. a. K b. N c. Cl d. B Covalent Bonding 1. Obtain the number of valence electrons for each of the following atoms from its group number and draw the correct Electron Dot Notation (a.k.a. Lewis Dot Structures). a. K b. N c. Cl

More information

Chapter 8: Concepts of Chemical Bonding

Chapter 8: Concepts of Chemical Bonding Chapter 8: Concepts of Chemical Bonding Learning Outcomes: Write Lewis symbols for atoms and ions. Define lattice energy and be able to arrange compounds in order of increasing lattice energy based on

More information

Funsheet 8.0 [SCIENCE 10 REVIEW] Gu 2015

Funsheet 8.0 [SCIENCE 10 REVIEW] Gu 2015 Funsheet 8.0 [SCIENCE 10 REVIEW] Gu 2015 1. Fill in the following tables. Symbol # # protons electrons # neutrons Atomic number Mass Number Atomic Mass Charge 56 54 83 18 16 32 35 47 1 19 40 1+ 92 241

More information

Chapter 8. Chemical Bonding: Basic Concepts

Chapter 8. Chemical Bonding: Basic Concepts Chapter 8. Chemical Bonding: Basic Concepts Chemical bond: is an attractive force that holds 2 atoms together and forms as a result of interactions between electrons found in combining atoms We rarely

More information

CHEM 110 Exam 2 - Practice Test 1 - Solutions

CHEM 110 Exam 2 - Practice Test 1 - Solutions CHEM 110 Exam 2 - Practice Test 1 - Solutions 1D 1 has a triple bond. 2 has a double bond. 3 and 4 have single bonds. The stronger the bond, the shorter the length. 2A A 1:1 ratio means there must be the

More information

Chemistry 1A Spring 1999 Exam #4 KEY Chapters 9 & 10

Chemistry 1A Spring 1999 Exam #4 KEY Chapters 9 & 10 H 2.2 Chemistry 1A Spring 1999 Exam #4 KEY Chapters 9 & 10 Electronegativities Li Be B C N O F 0.98 1.57 2.04 2.55 3.04 3.44 3.98 Na Mg Al Si P S Cl 0.93 1.31 1.61 1.9 2.19 2.58 3.16 K Ca Ga Ge As Se Br

More information

M11/4/CHEMI/SPM/ENG/TZ2/XX CHEMISTRY STANDARD LEVEL PAPER 1. Monday 9 May 2011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES

M11/4/CHEMI/SPM/ENG/TZ2/XX CHEMISTRY STANDARD LEVEL PAPER 1. Monday 9 May 2011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES M11/4/CHEMI/SPM/ENG/TZ/XX 116116 CHEMISTRY STANDARD LEVEL PAPER 1 Monday 9 May 011 (afternoon) 45 minutes INSTRUCTIONS TO CANDIDATES Do not open this examination paper until instructed to do so. Answer

More information

Unit 5: Bonding Part 2 (Covalent Bonds/Bond & Molecular Polarity/IMF)

Unit 5: Bonding Part 2 (Covalent Bonds/Bond & Molecular Polarity/IMF) Unit 5: Bonding Part 2 (Covalent Bonds/Bond & Molecular ity/imf) The following pages are practice questions for this unit, and will be submitted for homework! You must complete: Ionic vs. Covalent Properties

More information

Chapter 1: Structure and Bonding

Chapter 1: Structure and Bonding 1. What is the ground-state electronic configuration of a carbon atom? A) 1s 2, 2s 2, 2p 5 B) 1s 2, 2s 2, 2p 2 C) 1s 2, 2s 2, 2p 6 D) 1s 2, 2s 2, 2p 4 2. What is the ground-state electronic configuration

More information

Lecture 14. Professor Hicks Inorganic Chemistry (CHE151) Shapes of Molecules. The shape of most molecules is not flat as they are drawn on paper

Lecture 14. Professor Hicks Inorganic Chemistry (CHE151) Shapes of Molecules. The shape of most molecules is not flat as they are drawn on paper Lecture 14 Professor Hicks Inorganic Chemistry (CHE151) Shapes of Molecules The shape of most molecules is not flat as they are drawn on paper The three dimensional arrangement of atoms is called the Geometry

More information

Name (printed): Signature:

Name (printed): Signature: CHEM Lab Section Number: Name (printed): Signature: This exam consists of 36 questions all of equal value for a total of 225 points. Make sure that your test has all of the pages. Please read each problem

More information

GENERAL CHARACTERISTICS OF THE P-BLOCK ELEMENTS

GENERAL CHARACTERISTICS OF THE P-BLOCK ELEMENTS 18 GENERAL CHARACTERISTICS OF THE P-BLOCK ELEMENTS The p-block of the periodic table consists of the elements of groups 13,14, 15, 16, 17 and 18. These elements are characterised by the filling up of electrons

More information

Essential Organic Chemistry. Chapter 1

Essential Organic Chemistry. Chapter 1 Essential Organic Chemistry Paula Yurkanis Bruice Chapter 1 Electronic Structure and Covalent Bonding Periodic Table of the Elements 1.1 The Structure of an Atom Atoms have an internal structure consisting

More information

Chemical Bonding Chapter 8

Chemical Bonding Chapter 8 Chemical Bonding Chapter 8 Get your Clicker, 2 magnets, goggles and your handouts Nov 15 6:15 PM Recall that: Ionic-Involves the transfer of electrons - forms between a metal and a nonmetal Covalent-Involves

More information

Supporting Information

Supporting Information Supporting Information Nitroxide-Mediated Polymerization of Vinyl Chloride at Low Temperature: Kinetic and Computational Studies Carlos M. R. Abreu, Patrícia V. Mendonça, Arménio C. Serra, Benjamin B.

More information

Chemistry 1000 Lecture 15: Covalent bonding and Lewis structures

Chemistry 1000 Lecture 15: Covalent bonding and Lewis structures Chemistry 1000 Lecture 15: Covalent bonding and Lewis structures Marc R. Roussel October 3, 2018 Marc R. Roussel Covalent bonding October 3, 2018 1 / 24 Lewis diagrams Covalent bonding Covalent bond: a

More information

November 18, Oct 23 5:37 PM. Oct 23 5:30 PM. Oct 23 5:39 PM. Oct 23 5:38 PM. Oct 23 5:53 PM. Oct 23 5:57 PM

November 18, Oct 23 5:37 PM. Oct 23 5:30 PM. Oct 23 5:39 PM. Oct 23 5:38 PM. Oct 23 5:53 PM. Oct 23 5:57 PM Electron Configurations of Ions of the Representative Elements Sample Exercise 8.2 Predict the ion generally formed by (a) Sr (b) S (c) Al Oct 23 5:30 PM Oct 23 5:37 PM Transition Metal Ions Practice Exercise

More information

CHEMICAL BONDS. Determining Percentage Composition, Empirical, and Molecular Formulas for Compounds:

CHEMICAL BONDS. Determining Percentage Composition, Empirical, and Molecular Formulas for Compounds: CHEMICAL BONDS Chemical Bonds: The strong electrostatic forces of attraction holding atoms together in a unit are called chemical bonds (EU 2.C). Reflect a balance in the attractive and repulsive forces

More information

CHEM 101 Fall 08 Exam III(a)

CHEM 101 Fall 08 Exam III(a) CHEM 101 Fall 08 Exam III(a) On the answer sheet (scantron) write you name, student ID number, and recitation section number. Choose the best (most correct) answer for each question and enter it on your

More information

Chapter 8 Basic concepts of bonding

Chapter 8 Basic concepts of bonding Chapter 8 Basic concepts of bonding 8.1 Chemical Bonds, Lewis Symbols, and the Octet Rule When atoms or ions are strongly attracted to one another, we say that there is a chemical bond between them. Types

More information

Intramolecular Bonding. Chapters 4, 12 Chemistry Mr. McKenzie

Intramolecular Bonding. Chapters 4, 12 Chemistry Mr. McKenzie Intramolecular Bonding Chapters 4, 12 Chemistry Mr. McKenzie What determines the type of intramolecular bond? An intramolecular bond is any force that holds two atoms together to form a compound; 3 types

More information

Electronegativity is a very useful concept for the explanation or understanding of chemical reactivity throughout the periodic table.

Electronegativity is a very useful concept for the explanation or understanding of chemical reactivity throughout the periodic table. 1.6. Review of Electronegativity (χ) CONCEPT: Electronegativity is a very useful concept for the explanation or understanding of chemical reactivity throughout the periodic table. There are many definitions

More information

A. 24 B. 27 C. 30 D. 32 E. 33. A. It is impossible to tell from the information given. B. 294 mm C. 122 mm D. 10 mm E. 60 mm A. 1 H B. C. D. 19 F " E.

A. 24 B. 27 C. 30 D. 32 E. 33. A. It is impossible to tell from the information given. B. 294 mm C. 122 mm D. 10 mm E. 60 mm A. 1 H B. C. D. 19 F  E. CHEMISTRY 110 EXAM 1 Sept. 24, 2012 FORM A 1. A microwave oven uses 2.45! 10 9 Hz electromagnetic waves to heat food. What is the wavelength of this radiation in mm? A. It is impossible to tell from the

More information

NAME: SECOND EXAMINATION

NAME: SECOND EXAMINATION 1 Chemistry 64 Winter 1994 NAME: SECOND EXAMINATION THIS EXAMINATION IS WORTH 100 POINTS AND CONTAINS 4 (FOUR) QUESTIONS THEY ARE NOT EQUALLY WEIGHTED! YOU SHOULD ATTEMPT ALL QUESTIONS AND ALLOCATE YOUR

More information

Biotech 2: Atoms and Molecules OS Text Reading pp Electron cloud Atoms & Nucleus 2e Subatomic Particles Helium Electron cloud

Biotech 2: Atoms and Molecules OS Text Reading pp Electron cloud Atoms & Nucleus 2e Subatomic Particles Helium Electron cloud 9/4/017 Biotech : Atoms and Molecules OS Text Reading pp. 34-4 Atoms & Subatomic Particles Nucleus Helium e cloud cloud e Protons Neutrons Mass number = 4 s Nucleus Carbon atomic number = # of protons

More information