Question 1

Which of the following best describes the type of bonding present in sodium chloride ($$\mathrm{NaCl}) $$and explains its high melting point?

Accepted Answer

Ionic bonding; strong electrostatic attraction between oppositely charged ions

Question 2

Diamond and graphite are both forms of carbon. Which statement best explains why diamond is much harder than graphite?

Accepted Answer

Diamond has a giant molecular structure with each carbon atom covalently bonded to four others, while graphite has layers held together by weak forces.

Question 3

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

Accepted Answer

Electrons are shared equally between all atoms, forming a delocalized 'sea' that allows metals to conduct electricity.

Question 4

Which property of metals is best explained by the presence of delocalized electrons in metallic bonding?

Accepted Answer

Electrical conductivity

Question 5

Which of the following molecules has a linear molecular geometry according to VSEPR theory?

Accepted Answer

$$\mathrm{CO_2$}$$

Question 6

A student dissolves table salt ($$\mathrm{NaCl}) in $$water. Which type of bonding is broken and which is formed during this process?

Accepted Answer

Ionic bonds are broken; ion-dipole interactions are formed between ions and water molecules.

Question 7

Which of the following statements about covalent bonds is correct?

Accepted Answer

Covalent bonds involve the sharing of electron pairs between atoms.

Question 8

Which of the following best explains why graphite can conduct electricity but diamond cannot?

Accepted Answer

Graphite has delocalized electrons within its layers, while diamond does not.

Question 9

Which of the following is a property of giant molecular (network covalent) solids such as silicon dioxide ($$\mathrm{$$SiO_2$$}$$)?

Accepted Answer

High melting point due to strong covalent bonds throughout the structure

Question 10

Which of the following best describes the bonding and structure in magnesium metal ($$\mathrm{Mg}$$)?

Accepted Answer

Metallic lattice with positive ions surrounded by a sea of delocalized electrons

Question 11

Which of the following best explains why ionic compounds conduct electricity when molten but not when solid?

Accepted Answer

Ions are free to move in the molten state but fixed in the solid state.

Question 12

Which of the following statements about the strength of metallic bonds is correct?

Accepted Answer

The strength increases with the number of delocalized electrons and the charge of the metal ion.

Question 13

Which of the following best describes the structure of a typical ionic solid such as sodium chloride ($$\mathrm{NaCl}$$)?

Accepted Answer

A lattice of positive and negative ions held together by electrostatic forces

Question 14

Which of the following is a correct statement about the melting points of ionic, covalent, and metallic solids?

Accepted Answer

Ionic and metallic solids generally have high melting points due to strong forces, while simple molecular covalent solids have low melting points.

Question 15

Which of the following best explains why water ($$\mathrm{H_2O}) $$has a bent molecular geometry?

Accepted Answer

The two lone pairs on oxygen repel the bonding pairs, creating a bent shape.

Question 16

Which of the following is the best explanation for the high melting point of magnesium oxide ($$\mathrm{MgO}) $$compared to sodium chloride ($$\mathrm{NaCl}$$)?

Accepted Answer

$$\mathrm{MgO}$$ has ions with higher charges, leading to stronger electrostatic attractions.

Study Notes: Chemical Bonding and Structure (General Chemistry)

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