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Exam 9: Models of Chemical Bonding

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Question 21

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Arrange the following bonds in order of increasing bond strength.

A) C-I < C-Br < C-Cl < C-F
B) C-F < C-Cl < C-Br < C-I
C) C-Br < C-I < C-Cl < C-F
D) C-I < C-Br < C-F< C-Cl
E) None of these choices are correct.

F) B) and E)
G) A) and D)

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Question 22

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A Born-Haber cycle applied to the formation reaction of an ionic solid

A) is normally used to calculate ionization energy.
B) is normally used to calculate electron affinity.
C) is normally used to calculate bond energy.
D) is normally used to determine the overall enthalpy change.
E) is an application of Hess's Law.

F) None of the above
G) C) and D)

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Question 23

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Which of the following elements is the least electronegative?

Electronegativity is a measure of

Nitrogen and hydrogen combine to form ammonia in the Haber process. Calculate (in kJ) the standard enthalpy change ΔH° for the reaction written below, using the bond energies given. N₂(g) + 3H₂(g) → 2NH₃(g)

Bond energy increases as bond order increases, for bonding between a given pair of atoms.

Analysis of an unknown substance showed that it has a moderate melting point and is a good conductor of heat and electricity in the solid phase. Which of the following substances would have those characteristics?

Calculate the lattice energy of magnesium sulfide from the data given below. Mg(s) → Mg(g) ΔH° = 148 kJ/mol Mg(g) → Mg²⁺(g) + 2e⁻ ΔH° = 2186 kJ/mol S₈(s) → 8S(g) ΔH° = 2232 kJ/mol S(g) + 2e⁻ → S²⁻(g) ΔH° = 450 kJ/mol 8Mg(s) + S₈(s) → 8MgS(s) ΔH° = −2744 kJ/mol Mg²⁺(g) + S²⁻(g) → MgS(s) ΔH°_lattice = ?

Arrange aluminum, boron, nitrogen, and phosphorous in order of increasing electronegativity.

The more C-O and O-H bonds there are in a substance, the greater will be the amount of heat released when a fixed mass of the substance is burned.

Covalently bonded substances do not necessarily exist as separate molecules.

No real bonds are 100% ionic in character.

As a measure of the strength of metallic bonding, the boiling point of a metal is a better indicator than its melting point.

The electrostatic energy of two charged particles is inversely proportional to the distance between them.

For which of the following elements (in their normal, stable, forms) would it be correct to describe the bonding as involving "electron pooling"?

Arrange oxygen, sulfur, calcium, rubidium, and potassium in order of decreasing electronegativity.

In which of these substances are the atoms held together by polar covalent bonding?

The electrostatic energy of two charged particles is inversely proportional to the square of the distance between them.

Based on electronegativity trends in the periodic table, predict which of the following compounds will have the greatest % ionic character in its bonds.

The stronger the bonds in a fuel, the more energy it will yield.