Question 1

Which type of chemical bonding is most commonly found within a molecule of water ($$\mathrm{H_2O}$$)?

Accepted Answer

Covalent bonding

Question 2

Which element is expected to have the highest melting point due to its bonding type?

Accepted Answer

Carbon ($$\mathrm{C}$$, as diamond)

Question 3

What is the primary reason that diamond (a form of carbon) has such a high melting point?

Accepted Answer

It is held together by covalent network bonds.

Question 4

Which of the following best describes the bonding in sodium chloride ($$\mathrm{NaCl}$$)?

Accepted Answer

Ionic bonding

Question 5

Which element from the following list is most likely to form a metallic bond in its pure elemental state?

Accepted Answer

Magnesium ($$\mathrm{Mg})$$

Question 6

Which of the following substances is most likely to be a solid with a high melting point and poor electrical conductivity in both solid and molten states?

Accepted Answer

Diamond ($$\mathrm{C}$$, network covalent)

Question 7

Which of the following best explains why metals are good conductors of electricity?

Accepted Answer

They have delocalized electrons that can move freely.

Question 8

Which type of bonding is responsible for the structure and properties of quartz ($$\mathrm{$$SiO_2$$}$$)?

Accepted Answer

Network covalent bonding

Question 9

Which of the following elements is most likely to form a diatomic molecule with covalent bonding?

Accepted Answer

Oxygen ($$\mathrm{O_2$})$$

Question 10

A student claims that bromine ($$\mathrm{Br_2$}) $$has a higher melting point than magnesium ($$\mathrm{Mg}) $$because bromine is heavier. Is this claim correct? Why or why not?

Accepted Answer

No, because magnesium has metallic bonding which is stronger than the intermolecular forces in bromine.

Question 11

Which of the following best describes the trend in melting points for main group elements with network covalent bonding compared to those with metallic or molecular bonding?

Accepted Answer

Network covalent elements generally have higher melting points.

Question 12

Which of the following is a property of substances with network covalent bonding?

Accepted Answer

They are hard and have high melting points.

Question 13

Which of the following best explains why sodium ($$\mathrm{Na}) is a $$good conductor of electricity in the solid state, but sodium chloride ($$\mathrm{NaCl}) is $$not?

Accepted Answer

Sodium has delocalized electrons, while sodium chloride does not.

Question 14

Which of the following elements is most likely to form a network covalent solid?

Accepted Answer

Carbon ($$\mathrm{C}$$, as diamond)

Question 15

Which of the following statements about covalent bonding is correct?

Accepted Answer

Covalent bonds involve the sharing of electrons between atoms.

Main Group Elements: Bonding Types and Properties

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