Question 1

Which type of chemical bond is present in sodium chloride (NaCl)?

Accepted Answer

Ionic bond

Question 2

What is the primary intermolecular force present in liquid water (H$$_2O$$)?

Accepted Answer

Hydrogen bonding

Question 3

Which of the following best explains why NaCl has a much higher melting point than water?

Accepted Answer

NaCl is held together by strong ionic bonds, while water is held together by weaker intermolecular forces.

Question 4

Which property of water makes it an excellent solvent for ionic compounds like NaCl?

Accepted Answer

Its high electronegativity difference between hydrogen and oxygen, making it highly polar

Question 5

How does the difference in electronegativity between sodium and chlorine atoms influence the bonding in NaCl?

Accepted Answer

It causes electrons to be transferred from sodium to chlorine, forming an ionic bond.

Question 6

Which of the following statements best describes the polarity of a water molecule?

Accepted Answer

Water is polar because oxygen is more electronegative than hydrogen, creating a partial negative charge on oxygen.

Question 7

Why does NaCl dissolve readily in water?

Accepted Answer

The polar water molecules surround and stabilize the Na$$^+$$ and Cl$$^-$$ ions, overcoming the ionic lattice.

Question 8

Which of the following best explains why water has a relatively high melting point for a molecule of its size?

Accepted Answer

Water molecules are held together by strong hydrogen bonds.

Question 9

A student claims that NaCl is a polar molecule. Which statement best evaluates this claim?

Accepted Answer

The claim is incorrect because NaCl is an ionic compound, not a molecule with covalent bonds.

Question 10

Which of the following equations correctly represents the dissolution of NaCl in water?

Accepted Answer

$$\mathrm{NaCl_{(s)} \rightarrow Na^+_{(aq)} + Cl^-_{(aq)}}$$

Question 11

Which factor most directly contributes to the high solubility of NaCl in water?

Accepted Answer

The strong ion-dipole interactions between water molecules and Na$$^+$$ and Cl$$^-$$ ions.

Question 12

Which of the following best describes the effect of electronegativity on the polarity of a molecule?

Accepted Answer

A large difference in electronegativity between atoms leads to a polar bond.

Question 13

Which of the following statements is true regarding the melting points of NaCl and H$$_2O$$?

Accepted Answer

NaCl has a higher melting point than H$$_2O $$due to strong ionic bonds.

Question 14

A patient is given an intravenous solution containing NaCl. Which property of NaCl and water allows this solution to be effective in the body?

Accepted Answer

NaCl dissolves in water due to ion-dipole interactions, allowing ions to be transported in the body.

Question 15

Which of the following best explains why water can dissolve many ionic compounds?

Accepted Answer

Water is polar and can stabilize ions through ion-dipole interactions.

Question 16

Which of the following is a consequence of the polarity of water molecules?

Accepted Answer

Water can form hydrogen bonds, leading to high surface tension.

Question 17

Which of the following best describes the role of electronegativity in determining the type of bond formed between two atoms?

Accepted Answer

If the electronegativity difference is large, an ionic bond forms.

Question 18

Which of the following is NOT a property of ionic compounds like NaCl?

Accepted Answer

Forms discrete molecules

Question 19

Which of the following best explains why water is a liquid at room temperature while other similar-sized molecules are gases?

Accepted Answer

Water molecules form strong hydrogen bonds with each other.

Question 20

Which of the following best describes the interaction between Na$$^+$$ ions and water molecules in solution?

Accepted Answer

Na$$^+$$ ions are surrounded by the partially negative oxygen atoms of water.

Bonding, Properties, and Solubility: Sodium Chloride (NaCl) vs. Water (H₂O)

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