Question 1

Which of the following best describes the difference between ionic, covalent, and metallic bonding?

Accepted Answer

Ionic bonding involves the transfer of electrons, covalent bonding involves the sharing of electrons, and metallic bonding involves pooling of electrons in a 'sea' shared by all atoms.

Question 2

A solid substance is hard, brittle, has a high melting point, and conducts electricity when molten but not as a solid. What type of bonding is most likely present?

Accepted Answer

Ionic bonding

Question 3

Which of the following compounds is most likely to be metallic based on its properties: malleable, ductile, and a good conductor of electricity?

Accepted Answer

Copper (Cu)

Question 4

Given the following bond energies and lengths: $$\mathrm{C-C} (154 pm$$, 347 kJ/mol), $$\mathrm{C=C} (134 pm$$, 611 kJ/mol), $$\mathrm{C\equiv C} (120 pm$$, 837 kJ/mol), which statement is correct?

Accepted Answer

As bond order increases, bond length decreases and bond energy increases.

Question 5

Which of the following best explains why the formation of NaCl from its elements is highly exothermic?

Accepted Answer

A large amount of energy is released when the oppositely charged ions coalesce into the solid lattice.

Question 6

Which of the following statements about lattice energy is correct?

Accepted Answer

Lattice energy increases with increasing ionic charge and decreasing ionic radius.

Question 7

Which of the following pairs of elements will form a compound with the greatest lattice energy?

Accepted Answer

MgO

Question 8

Which of the following best describes a polar covalent bond?

Accepted Answer

A bond in which electrons are shared unequally between two atoms with different electronegativities.

Question 9

Arrange the following bonds in order of increasing polarity: N–F, Be–F, O–F.

Accepted Answer

$$\mathrm{O-F} \u003c \mathrm{N-F} \u003c \mathrm{Be-F}$$

Question 10

Which of the following best explains why metals are malleable and ductile?

Accepted Answer

The non-directional nature of metallic bonding allows metal atoms to slide past each other without breaking bonds.

Question 11

Which of the following substances is most likely to be a molecular compound?

Accepted Answer

CO2

Question 12

Which of the following best describes the trend in electronegativity across a period and down a group in the periodic table?

Accepted Answer

Electronegativity increases across a period and decreases down a group.

Question 13

A molecule has a large dipole moment. Which of the following is most likely true about the atoms in the molecule?

Accepted Answer

There is a large difference in electronegativity between the atoms.

Question 14

Which of the following best explains why ionic compounds have high melting points?

Accepted Answer

Strong electrostatic forces between ions in the lattice require a large amount of energy to overcome.

Question 15

Which of the following is the correct empirical formula for glucose ($$\mathrm{C_6H_{12}O_6$}$$)?

Accepted Answer

$$\mathrm{CH_2O}$$

Question 16

Which of the following best describes the relationship between bond energy and bond length?

Accepted Answer

Shorter bonds are generally stronger (higher bond energy) than longer bonds.

Question 17

Which of the following best describes the electron-sea model of metallic bonding?

Accepted Answer

Valence electrons are delocalized and move freely throughout the metal lattice.

Question 18

Which of the following best explains why ionic compounds are brittle?

Accepted Answer

When a force is applied, like-charged ions are forced next to each other, causing repulsion and the crystal to shatter.

Question 19

Which of the following is the correct formula for the compound formed between calcium and nitrogen?

Accepted Answer

$$\mathrm{Ca_3N_2}$$

Question 20

Which of the following best describes the difference between a molecular formula and an empirical formula?

Accepted Answer

A molecular formula gives the actual number of atoms of each element in a molecule, while an empirical formula gives the lowest whole-number ratio of atoms.

Chemical Bonding: Ionic, Covalent, and Metallic Bonds

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