Quantum Numbers

Question 1

a. 2s

(n,l,m_l,m_s) = (2,0,0,±½)

b. 2p_x

(n,l,m_l,m_s) = (2,1,±1,±½)

c. 3p_z

(n,l,m_l,m_s) = (3,1,0,±½)

d. 3d_xz

(n,l,m_l,m_s) = (3,2,±1,±½)

e. 4d_z2

(n,l,m_l,m_s) = (4,2,0,±½)

f. 5d_x2-_y2

(n,l,m_l,m_s) = (5,2,±2,±½)

Slater's Rules

Question 1

a. As⁺

(1s²)(2s²,2p⁶)(3s²,3p⁶)(3d¹⁰)(4s²,4p²)

σ = (3 × 0.35) + (18 × 0.85) + (10 × 1.00) = 26.35
Z* = Z – σ = 33 – 26.35 = 6.65

b. S

(1s²)(2s²,2p⁶)(3s²,3p⁴)

σ = (5 × 0.35) + (8 × 0.85) + (2 × 1.00) = 10.55
Z* = Z – σ = 16 – 10.55 = 5.45

c. Cr

(1s²)(2s²,2p⁶)(3s²,3p⁶)(3d⁵)(4s¹,4p⁰)

σ = (13 × 0.85) + (10 × 1.00) = 21.05
Z* = Z – σ = 24 – 21.05 = 2.95

d. Pd²⁺

(1s²)(2s²,2p⁶)(3s²,3p⁶)(3d¹⁰)(4s²,4p⁶)(4d⁸)

σ = (7 × 0.35) + (36 × 1.00) = 38.45
Z* = Z – σ = 46 – 38.45 = 7.55

e. Cu⁺

(1s²)(2s²,2p⁶)(3s²,3p⁶)(3d¹⁰)

σ = (9 × 0.35) + (18 × 1.00) = 21.15
Z* = Z – σ = 29 – 21.15 = 7.85

Oxidation-Reduction (RedOx) Reaction

Question 1

a. 2BrO₃^– + 3N₂H₄ → 2Br^– + 3N₂ + 6H₂O

b. 3UO²⁺ + 2NO₃^– + 2H⁺ → 3UO₂²⁺ + 2NO + H₂O

c. 3P₄ + 20NO₃^– + 8H⁺ + 8H₂O → 12H₂PO₄^– + 20NO

d. 5S₂O₃^2– + 8MnO₄^– + 14H⁺ → 10SO₄^2– + 8Mn²⁺ + 7H₂O

e. 2Ag⁺ + H₂CO + H₂O → 2Ag + HCO₂H + 2H⁺

Question 2

a. 3ClO^– + 2CrO₂^– + 2OH^– → 3Cl^– + 2CrO₄^2– + H₂O

b. 6Fe(OH)₂ + 2CrO₄^2– → 3Fe₂O₃ + 2Cr(OH)₄^– + 2OH^– + H₂O

c. 3CH₃CH₂OH + 4MnO₄^– → 3CH₃COO^– + 4MnO₂ + OH^– + 4H₂O

d. 6ClO₂ + 6OH^– → 5ClO₃^– + Cl^– + 3H₂O

e. 4[Fe(CN)₆]^3– + N₂H₄ + 4OH^– → 4[Fe(CN)₆]^4– + N₂ + 4H₂O

Frost (Oxidation State) Diagrams

Question 1

a. Ni²⁺ + Cu²⁺ → No Reaction

b. VO²⁺ + Cr²⁺ → V³⁺ + Cr³⁺

c. CoO₂ + Cr³⁺ → Co²⁺ + Cr⁶⁺

d. Ti³⁺ + H₃O⁺ → No Reaction

e. H₂O + I₂ → No Reaction