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Chemistry Key Concepts: Chapters 6 & 7 - Atomic Structure and Periodic Trends - Prof. Zeld, Assignments of Chemistry

Material Type: Assignment; Professor: Ziegler; Class: General Chemistry I; Subject: Chemistry ; University: Central Oregon Community College; Term: Fall 2006;

Typology: Assignments

Pre 2010

Uploaded on 08/18/2009

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CH 221 – Ziegler KEY CONCEPTS Chapters 6,7
Fall 06 10th Ed.
Class period 1 – Reading pp. 216-225.
1. Relate wavelength, frequency, and energy of light. Problem 6.15 a, b
2. State, or recognize, a brief explanation as to why excited atoms emit only certain wavelengths of
light.
3. Rank the energy difference between energy levels in the hydrogen atom. See Figure 6.13
Class period 2 – Reading pp. 225m -228(m); 231-233; 234-238(t), 238(m) – 245 (m)
4. Use the Bohr model to calculate wavelength of lines in the hydrogen spectrum. Problems 6.35
5. State the physical significance of ψ2 for an electron in an atom.
6. Identify the quantum numbers and capacities of energy levels, sublevels, and orbitals. Problems
6.49, 6.63, 6.67, 6.54.
7. Write electron configurations of atoms and ions. Problems 6.65, 6.67.
Class period 3 – Reading pp.; 239 – 249 (m); 274 ( a short but important section of Chapter 7)
8. Write orbital diagrams for atoms and ions. Problem 6.68 a-f.and this: Write electron
configurations for Na0, Na+, Cl0, Cl-, Ne, C0, N0, Al0, Al+3, Ti+2, Ti+4
9. State the number of unpaired electrons in the ground state of an atom or ion. Problem 6.68 a-f
(again), 7.45.
10. Identify periodic trends in radii, ionization energy, and electron affinity. Problems 7.21, 7.23,
7.25, 7.28, 7.33, 7.49.
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CH 221 – Ziegler Fall 06 KEY CONCEPTS Chapters 6,7 10 th Ed.

Class period 1 – Reading pp. 216-225.

  1. Relate wavelength, frequency, and energy of light. Problem 6.15 a, b
  2. State, or recognize, a brief explanation as to why excited atoms emit only certain wavelengths of light.
  3. Rank the energy difference between energy levels in the hydrogen atom. See Figure 6. Class period 2 – Reading pp. 225m -228(m); 231-233; 234-238(t), 238(m) – 245 (m)
  4. Use the Bohr model to calculate wavelength of lines in the hydrogen spectrum. Problems 6.
  5. State the physical significance of ψ^2 for an electron in an atom.
  6. Identify the quantum numbers and capacities of energy levels, sublevels, and orbitals. Problems6.49, 6.63, 6.67, 6.54.
  7. Write electron configurations of atoms and ions. Problems 6.65, 6.67. Class period 3 – Reading pp.; 239 – 249 (m); 274 ( a short but important section of Chapter 7)
  8. Write orbital diagrams for atoms and ions. Problem 6.68 a-f.and this: Write electronconfigurations for Na (^0) , Na+, Cl (^0) , Cl-, Ne, C (^0) , N (^0) , Al (^0) , Al+3, Ti+2, Ti+
  9. State the number of unpaired electrons in the ground state of an atom or ion. Problem 6.68 a-f(again), 7.45.
  10. Identify periodic trends in radii, ionization energy, and electron affinity. Problems 7.21, 7.23,7.25, 7.28, 7.33, 7.49.

CH 221 – Ziegler Fall 06 KEY CONCEPTS Chapters 6,7 10 th Ed.

Answers to Assigned problems not in the back of the book 6.54 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. In general, for each principle quantum number,there are n kinds of orbitals, and n (^2) total orbitals. n, there are n ℓ- values and n^2 mℓ - values. For each shell,

6.62 a) Ga: [Ar] 4s^2 3d^10 4p^1 Outer shells look like this: (^) ↑↓ 4 s ↑↓ ↑↓ ↑↓ 3 d ↑↓ ↑↓ ↑ (^4) p 1 unpaired electron b) Ca: 20 electrons [Ar] 4s^2 outer shell looks like this:

↑↓ 4 s

no unpaired electrons c) V: [Ar] 4s^2 3d^3

outer shells look like this: ↑↓ 4 s ↑ ↑ ↑ 3 d 3 unpaired electrons

d) I: [Kr] 5s^2 4d^10 5p^5 outer shells look like this: ↑↓ 5 s ↑↓ ↑↓ ↑↓ 4 d ↑↓ ↑↓ ↑↓ ↑↓ 5 p ↑ 1 unpaired electron e) Y: 39 electrons [Kr] 5s^2 4d^1

Outer shells look like this: ↑↓ 5 s ↑ 4 d 1 unpaired electron

f) Pt: 78 electrons outer shells look like this: [Xe] 6s^2 4f^14 5d^8

↑↓ 6 s ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ ↑↓ 4 f ↑↓ ↑↓ ↑↓ ↑ 5 d ↑ 2 unpaired electrons

Na^0 1s^2 2s^2 2p^6 3s^1 Na Cl 0 + (^) 1s1s (^22) 2s2s (^22) 2p2p (^66) 3s3s (^20) 3p 5 Cl-^ 1s^2 2s^2 2p^6 3s^2 3p^6 Ne C 0 1s1s^22 2s2s^22 2p2p^62

N^0 1s^2 2s^2 2p^3 Al Al^0 +3^ 1s1s^22 2s (^) 2s^2 2 2p (^) 2p^6 6 3s^2 3p^1 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

7.22 Ca>Ca+2>Mg+