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Exam 9: Chemical Bonding I: Lewis Theory

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Question 51

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Which of the following statements is TRUE?

A) An ionic bond is much stronger than most covalent bonds.
B) An ionic bond is formed through the sharing of electrons.
C) Ionic compounds at room temperature typically conduct electricity.
D) Once dissolved in water, ionic compounds rarely conduct electricity.
E) None of the above is true.

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Question 52

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Which of the following resonance structures for OCN⁻ will contribute most to the correct structure of OCN⁻?

A) O(2 lone pairs) =C=N(2 lone pairs)
B) O(1 lone pair) ≡C-N(3 lone pairs)
C) O(1 lone pair) =C(2 lp) =N(1 lone pair)
D) O(3 lone pairs) -C≡N(with 1 lone pair)
E) They all contribute equally to the correct structure of OCN⁻.

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Question 53

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How are electron affinity and electronegativity different?

Using Lewis structures and formal charge, which of the following ions is most stable? OCN⁻ ONC⁻ NOC⁻

Explain why the lattice energy of MgS is approximately four times as large as that of NaCl.

Choose the bond below that is most polar.

Use the data given below to construct a Born-Haber cycle to determine the second ionization energy of Ca. ΔH°(kJ mol^-1) Ca(s) → Ca(g) 193 Ca(g) → Ca⁺(g) + e⁻ 590. 2O(g) → O₂(g) -498 O(g) + e⁻ → O⁻(g) -141 O⁻(g) + e⁻ → O²⁻(g) 878 Ca(s) + O₂(g) → CaO(s) -635 Ca²⁺(g) + O²⁻(g) → CaO(s) -3414

Of the following elements, which has the highest electronegativity?

Which of the following ionic compounds would be expected to have the highest lattice energy?

Choose the bond below that is most polar.

Draw the Lewis structure for the acetate ion CH₃CO₂⁻, including any important resonance structures. Label each atom with its formal charge.

Use the data given below to construct a Born-Haber cycle to determine the lattice energy of CaO. ΔH°(kJ mol^-1) Ca(s) → Ca(g) 193 Ca(g) → Ca⁺(g) + e⁻ 590 Ca⁺(g) → Ca²⁺(g) + e⁻ 1010 2O(g) → O₂(g) -498 O(g) + e⁻ → O⁻(g) -141 O⁻(g) + e⁻ → O²⁻(g) 878 Ca(s) + O₂(g) → CaO(s) -635

Choose the best Lewis structure for CH₂Cl₂.

Choose the best Lewis structure for BF₃.

Draw the Lewis structure for BrO₃⁻. Make sure to include any important resonance structures.

Place the following in order of decreasing XO bond length, where "X" represents the central atom in each of the following compounds or ions: SiO₃²⁻ CO₂ CO₃²⁻

Place the following in order of decreasing magnitude of lattice energy. K₂O Rb₂S Li₂O

Which compound has the highest carbon-carbon bond strength?

Choose the compound below that should have the lowest melting point according to the ionic bonding model.

Using periodic trends, place the following bonds in order of decreasing ionic character. Sb-Cl P-Cl As-Cl