CHAPTER 2: BONDING AND PROPERTIES

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1 CHAPTER 2: BONDING AND PROPERTIES ISSUES TO ADDRESS... What promotes bonding? What types of bonds are there? What properties are inferred from bonding? Chapter 2 1

Fundamental concepts Proton and electron, charged Neutron Nucleus Electron Protons QuarksGluon 1.60 x10 19 C Mass of electron 9.11x10 31 kg Mass of protons and neutrons 1.

2 Fundamental concepts Proton and electron, charged Neutron Nucleus Electron Protons QuarksGluon 1.60 x10 19 C Mass of electron 9.11x10 31 kg Mass of protons and neutrons 1.67 x kg Atomic number: the number of protons Atomic mass =protons+neutrons Isotope Atomic mass unit(amu): 1amu=1/12 C One mole = 6.023x10 23 atoms(avogadro s) Chapter 2

3 BOHR ATOM orbital electrons: n = principal quantum number n=3 2 1 Adapted from Fig. 2.1, Callister 6e. Nucleus: Z = # protons = 1 for hydrogen to 94 for plutonium N = # neutrons Atomic mass A Z + N Chapter 2 2

4 ELECTRON ENERGY STATES Electrons... n l m l Orbital # of orbitals s s 4 have discrete energy states tend to occupy lowest available energy state p 1 0 2p 0 1 2p s p 1 0 3p 0 1 3p d 2 1 3d 1 0 3d 0 1 3d 1 2 3d 2 Chapter 2 3

5 Relative energies of the electrons for various shells and subshells Energy 5p 5s 4p 4s 3p 3s 2p 2s 4d 3d 1s s p d 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f 5s 5p 5d 5f 5g 6s 6p 6d 6f 6g Chapter 2

6 STABLE ELECTRON CONFIGURATIONS Stable electron configurations... have complete s and p subshells tend to be unreactive. Adapted from Table 2.2, Callister 6e. Chapter 2 4

SURVEY OF ELEMENTS Most elements: Electron configuration not stable. Electron configuration 1s 1 1s 2 (stable) 1s 2 2s 1 1s 2 2s 2 1s 2 2s 2 2p 1 1s 2 2s 2 2p 2.

7 SURVEY OF ELEMENTS Most elements: Electron configuration not stable. Electron configuration 1s 1 1s 2 (stable) 1s 2 2s 1 1s 2 2s 2 1s 2 2s 2 2p 1 1s 2 2s 2 2p s 2 2s 2 2p 6 (stable) 1s 2 2s 2 2p 6 3s 1 1s 2 2s 2 2p 6 3s 2 1s 2 2s 2 2p 6 3s 2 3p s 2 2s 2 2p 6 3s 2 3p 6 (stable)... 1s 2 2s 2 2p 6 3s 2 3p 6 3d 10 4s Adapted from Table 2.2, Callister 6e. (stable) Why? Valence (outer) shell usually not filled completely. Chapter 2 5

8 THE PERIODIC TABLE Columns: Similar Valence Structure Adapted from Fig. 2.6, Callister 6e. Electropositive elements: Readily give up electrons to become + ions. Electronegative elements: Readily acquire electrons to become ions. Chapter 2 6

ELECTRONEGATIVITY Ranges from 0.7 to 4.0, Large values: tendency to acquire electrons. Smaller electronegativity Larger electronegativity Adapted from Fig. 2.7, Callister 6e.

9 ELECTRONEGATIVITY Ranges from 0.7 to 4.0, Large values: tendency to acquire electrons. Smaller electronegativity Larger electronegativity Adapted from Fig. 2.7, Callister 6e. (Fig. 2.7 is adapted from Linus Pauling, The Nature of the Chemical Bond, 3rd edition, Copyright 1939 and 1940, 3rd edition. Copyright 1960 by Cornell University. Chapter 2 7

10 Group Ia IIa IIIa IVa Va VIa VIIa 0 Elements Na Mg Al Si P S Cl Ar Atomic # Outer shell e 3s 1 3s 2 3s 2 3p 1 3s 2 3p 2 3s 2 3p 3 3s 2 3p 4 3s 2 3p 5 3s 2 3p 6 Crystal structure bcc hcp fcc diamond complex fcc Electrical resistivity at RT (10 4 ohmm) metal x10 5 semicon 1x10 17 insulator 2x10 23 insulator gas gas Bond strength ? 2.86? 0.08 (in ev) Melting point C Boiling point C Chapter 2

11 IONIC BONDING Occurs between + and ions. Requires electron transfer. Large difference in electronegativity required. Example: NaCl Chapter 2 8

12 Predominant bonding in Ceramics H 2.1 Li 1.0 Na 0.9 K 0.8 Rb 0.8 Cs 0.7 Fr 0.7 EXAMPLES: IONIC BONDING Be 1.5 Mg 1.2 Ca 1.0 Sr 1.0 Ba 0.9 Ra 0.9 Ti 1.5 Cr 1.6 Fe 1.8 NaCl MgO CaF2 CsCl Ni 1.8 Zn 1.8 As 2.0 O 3.5 F 4.0 Cl 3.0 Br 2.8 I 2.5 At 2.2 He Ne Ar Kr Xe Rn Give up electrons Acquire electrons Adapted from Fig. 2.7, Callister 6e. (Fig. 2.7 is adapted from Linus Pauling, The Nature of the Chemical Bond, 3rd edition, Copyright 1939 and 1940, 3rd edition. Copyright 1960 by Cornell University. Chapter 2 9

13 Requires shared electrons Example: CH4 C: has 4 valence e, needs 4 more H: has 1 valence e, needs 1 more COVALENT BONDING Electronegativities are comparable. Ground state C 1s 2 2s 2 2p 2 C* 4 H CH 4 H H C H H Symmetric no net P CH 3 Cl Cl H C H H No loger symmetric P Chapter 2 10

14 column IVA H 2.1 Li 1.0 Na 0.9 K 0.8 Rb 0.8 Cs 0.7 Fr 0.7 EXAMPLES: COVALENT BONDING Be 1.5 Mg 1.2 Ca 1.0 Sr 1.0 Ba 0.9 Ra 0.9 H2 Ti 1.5 Cr 1.6 Fe 1.8 H2O C(diamond) SiC Ni 1.8 Zn 1.8 Ga 1.6 C 2.5 Si 1.8 As 2.0 GaAs Adapted from Fig. 2.7, Callister 6e. (Fig. 2.7 is adapted from Linus Pauling, The Nature of the Chemical Bond, 3rd edition, Copyright 1939 and 1940, 3rd edition. Copyright 1960 by Cornell University. Ge 1.8 Sn 1.8 Pb 1.8 O 2.0 F 4.0 Cl 3.0 Br 2.8 I 2.5 At 2.2 He Ne Ar Kr Xe Rn F2 Cl2 Molecules with nonmetals Molecules with metals and nonmetals Elemental solids (RHS of Periodic Table) Compound solids (about column IVA) Chapter 2 11

15 METALLIC BONDING Arises from a sea of donated valence electrons (1, 2, or 3 from each atom). Adapted from Fig. 2.11, Callister 6e. Primary bond for metals and their alloys Chapter 2 12

SECONDARY BONDING Arises from interaction

case: Adapted from Fig. 2.14, Callister 6e.

16 SECONDARY BONDING Arises from interaction between dipoles Fluctuating dipoles Adapted from Fig. 2.13, Callister 6e. Permanent dipolesmolecule induced general case: Adapted from Fig. 2.14, Callister 6e. ex: liquid HCl Adapted from Fig. 2.14, Callister 6e. ex: polymer Chapter 2 13

17 SUMMARY: BONDING Type Ionic Covalent Metallic Secondary Bond Energy Large! Variable largediamond smallbismuth Variable largetungsten smallmercury smallest Comments Nondirectional (ceramics) Directional semiconductors, ceramics polymer chains) Nondirectional (metals) Directional interchain (polymer) intermolecular Chapter 2 14

18 Force between atoms (+) Bonding forces and energies F n =F A +F R E 0 bonding energy large bonding E, high melting point stiffness shape of fr curve thermal expansion Er curve Chapter 2

19 HW assignment change: Please do 2.14 instead of 2.13 Chapter 2

20 PROPERTIES FROM BONDING: T M Bond length, r Melting Temperature, Tm F r F Bond energy, Eo Tm is larger if Eo is larger. Chapter 2 15

21 PROPERTIES FROM BONDING: E Elastic modulus, E Elastic modulus F DL A = E o L o E ~ curvature at ro Energy unstretched length r o r E is larger if Eo is larger. smaller Elastic Modulus larger Elastic Modulus Chapter 2 16

22 PROPERTIES FROM BONDING: a Coefficient of thermal expansion, a coeff. thermal expansion DL Lo = a (T 2 T 1 ) a ~ symmetry at ro a is larger if Eo is smaller. Chapter 2 17

SUMMARY: PRIMARY BONDS Ceramics (Ionic & covalent bonding): Large bond energy large Tm large E small a Metals (Metallic bonding): Variable bond energy

23 SUMMARY: PRIMARY BONDS Ceramics (Ionic & covalent bonding): Large bond energy large Tm large E small a Metals (Metallic bonding): Variable bond energy moderate Tm moderate E moderate a Polymers (Covalent & Secondary): Directional Properties Secondary bonding dominates small T small E large a Chapter 2 18

Atomic Structure. Atomic weight = m protons + m neutrons Atomic number (Z) = # of protons Isotope corresponds to # of neutrons

Atomic Structure. Atomic weight = m protons + m neutrons Atomic number (Z) = # of protons Isotope corresponds to # of neutrons Atomic Structure Neutrons: neutral Protons: positive charge (1.6x10 19 C, 1.67x10 27 kg) Electrons: negative charge (1.6x10 19 C, 9.11x10 31 kg) Atomic weight = m protons + m neutrons Atomic number (Z)