CHEM 10113, Quiz 5 October 26, 2011
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1 CHEM 10113, Quiz 5 October 26, 2011 Name (please print) All equations must be balanced and show phases for full credit. Significant figures count, show charges as appropriate, and please box your answers! IA Periodic Table of the Elements VIIIA (1) (18) H IIA IIIA IVA VA VIA VIIA He (2) (13) (14) (15) (16) (17) Li Be B C N O F Ne Na Mg IIIB IVB VB VIB VIIB VIIIB IB IIB Al Si P S Cl Ar (3) (4) (5) (6) (7) (8) (9) (10) (11) (12) K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Uuu Uub Uug (261) (262) (266) (264) (270) (268) (281) Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr (2 points) Draw the Lewis electron dot symbols for a) P 3, b) Sr. 2. (7 points) In each blank write >, < or = as appropriate. electron of carbon electron of fluorine Lattice energy of BaI Lattice energy of CaO Reactivity of Li Reactivity of Rb size of As 3 size of Ga IE of Mg IE of Rb Covalent radius of P Van der Waals radius of P C=C double bond length C-C single bond length
2 3. (3 points) Write the chemical equation for the reaction of rubidium with water. 4. (3 points) Briefly explain why Ca prefers to have a +2 charge rather than a +3 charge. Show the appropriate electron configurations to support your answer. 5. (3 points) Write the chemical equation that corresponds to the lattice energy of calcium chloride. 6. (2 points) Write the valence electron configuration for Mn (2 points) Write the valence orbital diagram for arsenic. 8. (3 points) Use Lewis symbols to illustrate the formation of an ionic compound of K and N (as in lecture).
3 CHEM 10113, Quiz 5 October 26, 2011 Name (please print) All equations must be balanced and show phases for full credit. Significant figures count, show charges as appropriate, and please box your answers! IA Periodic Table of the Elements VIIIA (1) (18) H IIA IIIA IVA VA VIA VIIA He (2) (13) (14) (15) (16) (17) Li Be B C N O F Ne Na Mg IIIB IVB VB VIB VIIB VIIIB IB IIB Al Si P S Cl Ar (3) (4) (5) (6) (7) (8) (9) (10) (11) (12) K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Uuu Uub Uug (261) (262) (266) (264) (270) (268) (281) Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr (2 points) Draw the Lewis electron dot symbols for a) Se 2, b) Al. 2. (7 points) In each blank write >, < or = as appropriate. Size of Na + ion Size of P 3 ion EA of Nb Reactivity of sulfur electron of Ca Van der Waals radius of Co Lattice energy of SrBr 2 O=O double bond length EA of As Reactivity of neon electron of Se Nonbonding radius of Co Lattice energy of RbBr O-O single bond length
4 3. (3 points) Write the chemical equation for the reaction of gallium with bromine. 4. (3 points) Briefly explain why S prefers to have a 2 charge rather than a 3 charge. Show the appropriate electron configurations to support your answer. 5. (3 points) Write the chemical equation that corresponds to the first ionization energy of selenium. 6. (2 points) Write the valence electron configuration for Mo (2 points) Write the valence orbital diagram for antimony. 8. (3 points) Use Lewis symbols to illustrate the formation of an ionic compound of Ca and Br (as in lecture).
5 CHEM 10113, Quiz 5 October 26, 2011 Name (please print) All equations must be balanced and show phases for full credit. Significant figures count, show charges as appropriate, and please box your answers! IA Periodic Table of the Elements VIIIA (1) (18) H IIA IIIA IVA VA VIA VIIA He (2) (13) (14) (15) (16) (17) Li Be B C N O F Ne Na Mg IIIB IVB VB VIB VIIB VIIIB IB IIB Al Si P S Cl Ar (3) (4) (5) (6) (7) (8) (9) (10) (11) (12) K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe Cs Ba La Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn Fr Ra Ac Rf Db Sg Bh Hs Mt Ds Uuu Uub Uug (261) (262) (266) (264) (270) (268) (281) Ce Pr Nd Pm Sm Eu Gd Tb Dy Ho Er Tm Yb Lu Th Pa U Np Pu Am Cm Bk Cf Es Fm Md No Lr (2 points) Draw the Lewis electron dot symbols for a) Ba, b) N (7 points) In each blank write >, < or = as appropriate. Nonbonding radius of Ta covalent radius of Ta electron of Sr Lattice energy of BaCl 2 IE of S atomic radius of Bi Reactivity of K N-N single bond strength electron of Sr 2+ Lattice energy of KCl IE of Hg atomic radius of Si Reactivity of Ar N=N double bond strength
6 3. (3 points) Write the chemical equation for the reaction of calcium with iodine. 4. (3 points) Briefly explain why I prefers to have a 1 charge rather than a +1 charge. Show the appropriate electron configurations to support your answer. 5. (3 points) Write the chemical equation that corresponds to the electron affinity of barium. 6. (2 points) Write the valence electron configuration for Ir (2 points) Write the valence orbital diagram for tin. 8. (3 points) Use Lewis symbols to illustrate the formation of an ionic compound of Li and P (as in lecture).
(please print) (1) (18) H IIA IIIA IVA VA VIA VIIA He (2) (13) (14) (15) (16) (17)
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K. 27 Co. 28 Ni. 29 Cu Rb. 46 Pd. 45 Rh. 47 Ag Cs Ir. 78 Pt.
1 IA 1 H Hydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 H 1.01 IIA IIIA IVA VA VIA VIIA 2 He 4.00 Metalloids 3 Li 6.94 4 Be 9.01 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F
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1 IA 1 ydrogen 1.01 Atomic number Element symbol Element name Atomic mass VIIIA 1 1.01 IIA IIIA IVA VA VIA VIIA 2 e 4.00 Metalloids 3 Li 6.94 4 Be 9.01 5 B 10.81 6 C 12.01 7 N 14.01 8 O 16.00 9 F 19.00
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