2.7. Atomic and ionic rad i 2.8. Ionization energy: the first, second,.. ionization energy 2.9. Electron affinity (Note here we use a different definition of the electron affinity from the textbook.) 2.10. Exothermic and Endothermic reactions 3. Chemical Bonds, Valence Bond, and Molecular Shape(Chapter 9) 31. Valence electrons 3.2. Ionic bond 33. Covalent bond 3. 4. Lewis structures (a). Octet rule (b). Single, double, and triple bonds (c). Bond order, bond length, and bond energy Be able to calculate the heat of a reaction from the given bond energies (d). Lone pair electrons, Coordinate bond (e). Be able to write Lewis structures of common molecules ( f. Exception of the octet rule: more than 8 e"; fewer than 8e"; odd number of e (g). Resonance structures (h ). Formal charges -a way to select the most effective Lewis structure(s) (. Failure of Lewis structure: octet rule exception; resonance structure; paramagnetism 3.5. Electronegativity 3.6. Nonpolar and polar covalent bonds 3.7. Valence Bond (VB)method (a). Definition of the valence bond method (b). g bond andπbond How o bond and T bond are made from S, px, py, pz orbitals? How o bond and bond relate to single/double/triple bonds (c). Hybrid orbitals(only applied to central atoms ): sp, sp, sp, spd (d ). Bond angle and the shape of molecules (e). Cis-and Trans-isomerism(sp- hybrid f). VSEPR method: predict the electron pair shapes and molecular shapes How to calculate the hybrid type of the central atom(s) How to arrange lone pair electrons and bonding electrons (g). Advantages and disad vantages of the Vb method 3.8. Molecule's polarity: sum of all bonds' dipoles 3.9. Brief introduction to organic molecules2.7．Atomic and ionic radii 2.8．Ionization energy: the first, second, … ionization energy 2.9．Electron affinity (Note here we use a different definition of the electron affinity from the textbook.) 2.10．Exothermic and Endothermic reactions 3．Chemical Bonds, Valence Bond, and Molecular Shape (Chapter 9) 3.1．Valence electrons 3.2．Ionic bond 3.3．Covalent bond 3.4．Lewis structures (a)．Octet rule (b)．Single, double, and triple bonds (c)．Bond order, bond length, and bond energy:  Be able to calculate the heat of a reaction from the given bond energies (d)．Lone pair electrons, Coordinate bond (e)．Be able to write Lewis structures of common molecules (f)．Exception of the octet rule: more than 8 e- ; fewer than 8 e- ; odd number of e- (g)．Resonance structures (h)．Formal charges – a way to select the most effective Lewis structure(s) (i)．Failure of Lewis structure: octet rule exception; resonance structure; paramagnetism 3.5．Electronegativity 3.6．Nonpolar and polar covalent bonds 3.7．Valence Bond (VB) method (a)．Definition of the valence bond method (b)．σ bond and π bond  How σ bond and π bond are made from s, px, py, pz orbitals?  How σ bond and π bond relate to single/double/triple bonds? (c)．Hybrid orbitals (only applied to central atoms): sp, sp2 , sp3 , sp3d (d)．Bond angle and the shape of molecules (e)．Cis- and Trans- isomerism (sp2 hybrid) (f)．VSEPR method: predict the electron pair shapes and molecular shapes  How to calculate the hybrid type of the central atom(s)  How to arrange lone pair electrons and bonding electrons (g)．Advantages and disadvantages of the VB method 3.8．Molecule’s polarity: sum of all bonds’ dipoles 3.9．Brief introduction to organic molecules