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CH 221 – Ziegler KEY CONCEPTS Fall 04
Chapters 6,7 9 th^ edition
Class period 1 – Reading pp. 199-201.
- Relate wavelength, frequency, and energy of light. Problem 6.8 a, b
Class period 2 – Reading pp. 202-209; 212-
- State, or recognize, a brief explanation as to why excited atoms emit only certain wavelengths of light.
- Rank the energy difference between energy levels in the hydrogen atom. See Figure 6.
- Use the Bohr model to calculate wavelength of lines in the hydrogen spectrum. Problems 6.
Class period 3 – Reading pp. 215m-217, 218 – 224 (m); 225(m) – 226; 249 - 250 (b) (short section of Chapter 7)
- State the physical significance of ψ^2 for an electron in an atom.
- Identify the quantum numbers and capacities of energy levels, sublevels, and orbitals. Problems 6.42, 6.44, 6.46, 6.55.
- Write electron configurations of atoms and ions. Problems 6.57, 6.60 a-e.
- Write orbital diagrams for atoms and ions. Problem 6.61 and this: Write electron configurations for Na^0 , Na+, Cl^0 , Cl-, Ne, C^0 , N^0 , Al^0 , Al+3, Ti+2, Ti+
- State the number of unpaired electrons in the ground state of an atom or ion. Problem 6.62 a-d.
Class period 4 – Reading pp. 239 – 249 (m).
- Identify periodic trends in radii, ionization energy, and electron affinity. Problems 7.16 b), 7.18*, 7.20, 7.22, 7.31, 7.43.
*The answer for 7.18 a is wrong in the answer book.
CH 221 – Ziegler KEY CONCEPTS Fall 04
Chapters 6,7 9 th^ edition
Answers to Assigned problems 6.8 a) ν = 5.02 x 10^14 s-
b) λ = 2.5 x 10-5^ m
6.28 a) ∆E = 2.09 x 10-18J ; ν= 3.15 x 10^15 s-1^ ; λ = 9.49 x 10-8^ m (emitted)
b) ∆E = 4.09 x 10-19^ J; ν= 6.16 x 10^14 s-1^ ; λ = 4.87 x 10-7^ m (emitted) c) ∆E = 7.57 x 10-20^ J; ν= 1.14 x 10^14 s-1^ ; λ = 2.63 x 10-6^ m (absorbed)
6.42 a) For n =3, there are 3 ℓ values (2,1,0) and 9 mℓ values (ℓ=2; mℓ = -2, -1, 0,1,2; ℓ=1; mℓ = -1, 0,1; ℓ=0; mℓ = 0)
b) For n =5, there are 5 ℓ values (4,3,2,1,0) and 25 mℓ values (ℓ=4; mℓ = -4,-3,-2, -1, 0,1,2,3,4;
(ℓ=3; mℓ = -3,-2,-1, 0,1,2,3; ℓ=2; mℓ = -2,-1, 0,1,2; ℓ=1; mℓ = -1, 0,1; ℓ=0; mℓ = 0)
In general, for each principle quantum number, n , there are n ℓ- values and n^2 mℓ - values. For each shell, there are n kinds of orbitals, and n^2 total orbitals. 6.44 a) 2,1,1; 2,1,0; 2,1,- b) 5,2,2; 5,2,1; 5,2,0; 5,2,-1; 5,2,-
6.46 a) permissible, 2p b) forbidden, for ℓ=0; mℓ can only be 0.
c) permissible, 4 d d) forbidden, for n = 3, the largest ℓ value is 2. 6.55 See text page A- 6.57 See text page A- 6.60 a) Al:[Ne]3s^2 3p^1 b) Sc: [Ar]4s^2 3d^1 c) Co: [Ar]4s^2 3d^7 d) Br: [Ar]4s^2 3d^10 4p^5 e) Ba: [Xe]6s^2 Na^0 1s^2 2s^2 2p^6 3s^1 Na+^ 1s^2 2s^2 2p^6 3s^0 Cl^0 1s^2 2s^2 2p^6 3s^2 3p^5 Cl-^ 1s^2 2s^2 2p^6 3s^2 3p^6 Ne 1s^2 2s^2 2p^6 C^0 1s^2 2s^2 2p^2
N^0 1s^2 2s^2 2p^3 Al^0 1s^2 2s^2 2p^6 3s^2 3p^1 Al+3^ 1s^2 2s^2 2p^6 Ti+2^ 1s^2 2s^2 2p^6 3s^2 3p^6 4s^0 3d^2 Ti+4^ 1s^2 2s^2 2p^6 3s^2 3p^6 4s^0 3d^0
6.62 a) Ti: [Ar] 4 s 3 d
↑ ↓ ↑ ↑ 2 unpaired electrons
b) Ga: [Ar] 4 s 3 d 4 p
↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑ 1 unpaired electron
c) Rh: [Kr] 5 s 4 d
↑↓ ↑↓ ↑↓ ↑ ↑ ↑ 3 unpaired electrons
d) I: [Kr] 5 s 4 d
5 p
1 unpaired electron
7.16 b) S<Si<Se<Ge 7.18 a) K<Rb<Cs b) Te<Sn<In c) Cl<P<Sr 7.20 a) More electrons=larger object b) ion sizes increase going down a column
c) More electrons=larger atom/ion; also Fe+ has a half-filled shell, for minimum repulsion and smaller size. 7.22 Ca>Ca+2>Mg+ 7.31 See Text A- 7.43 See Text A-
