Questions on Ionic Bond
20 Multiple-Choice Questions: Ionic Bond
Questions
1. What best describes an ionic bond?
A) Sharing of electrons between atoms
B) Attraction between cations and anions
C) Weak interaction between neutral atoms
D) Delocalized electrons in a "sea"
E) Overlap of atomic orbitals
2. Which of the following pairs of elements is most likely to form an ionic bond?
A) Hydrogen and Carbon
B) Oxygen and Nitrogen
C) Sodium and Chlorine
D) Nitrogen and Sulfur
E) Carbon and Hydrogen
3. In an ionic bond, electrons are:
A) Shared equally between atoms
B) Shared unequally between atoms
C) Completely transferred from one atom to another
D) Absent
E) Found in the nucleus
4. What type of elements usually form ionic bonds?
A) Nonmetal with nonmetal
B) Metal with nonmetal
C) Metalloid with metal
D) Noble gas with halogen
E) Metal with noble gas
5. Which of the following compounds is held together by ionic bonds?
A) CO₂
B) CH₄
C) NaCl
D) H₂O
E) NH₃
6. When a metal atom becomes a cation, it:
A) Gains electrons
B) Shares electrons
C) Loses electrons
D) Forms a covalent bond
E) Gains protons
7. Which of the following is a property of ionic compounds?
A) Low melting point
B) Conduct electricity in solid state
C) Form molecules
D) Conduct electricity when dissolved in water
E) Always liquid at room temperature
8. In the formation of NaCl, sodium:
A) Gains one electron
B) Shares one electron with chlorine
C) Loses one electron to chlorine
D) Forms a double bond
E) Gains a proton
9. Ionic compounds are usually:
A) Soft and flexible
B) Liquid at room temperature
C) Gases at room temperature
D) Brittle solids with high melting points
E) Poor conductors when molten
10. Which of the following ions is formed when magnesium loses two electrons?
A) Mg⁰
B) Mg⁻
C) Mg⁺
D) Mg²⁺
E) Mg²⁻
11. Which of the following is not an ionic compound?
A) KBr
B) CaCl₂
C) NaF
D) HCl
E) Li₂O
12. Which of the following best explains the strength of an ionic bond?
A) Shared electrons
B) Overlapping orbitals
C) Opposite charges attract
D) Same charges attract
E) Random motion of electrons
13. The formation of an ionic bond is generally:
A) Endothermic
B) Non-spontaneous
C) Spontaneous and exothermic
D) Driven by entropy
E) Reversible only in gas phase
14. The electrical conductivity of ionic compounds increases when:
A) In solid form
B) Dissolved in water or melted
C) Cooled below 0°C
D) Pressurized
E) Mixed with sugar
15. Which element is most likely to form an ionic bond with fluorine?
A) Carbon
B) Oxygen
C) Potassium
D) Phosphorus
E) Neon
16. Which compound contains an ionic bond?
A) H₂
B) NH₃
C) Na₂O
D) Cl₂
E) CH₄
17. Which is true of electrons in an ionic bond?
A) They are shared
B) They are localized between atoms
C) They are transferred from one atom to another
D) They remain in the nucleus
E) They orbit both atoms equally
18. When calcium forms an ionic bond with chlorine, the formula is:
A) CaCl
B) CaCl₂
C) Ca₂Cl
D) Ca₂Cl₂
E) CaCl₃
19. What charge does an atom typically gain to become an anion in an ionic bond?
A) Positive
B) Negative
C) Neutral
D) Variable depending on state
E) No charge
20. Which statement is false about ionic bonds?
A) They occur between metals and nonmetals
B) Electrons are transferred
C) Ions are formed
D) Ionic compounds have low melting points
E) Ionic compounds are often soluble in water
- Questions on Binary Ionic Compounds (Naming and Formulas)
- Questions on Polyatomic Ions – Naming and Formulas
- Questions on Ternary Ionic Compounds – Naming and Formulas
Answers with Explanations
1. B) Attraction between cations and anions
→ Ionic bonds form from the electrostatic attraction between positively and negatively charged ions.
2. C) Sodium and Chlorine
→ Sodium is a metal, and chlorine is a nonmetal — perfect conditions for ionic bonding.
3. C) Completely transferred from one atom to another
→ This is the hallmark of an ionic bond.
4. B) Metal with nonmetal
→ Metals lose electrons, nonmetals gain them — forming ions.
5. C) NaCl
→ Sodium chloride is a classic ionic compound.
6. C) Loses electrons
→ Metals lose electrons and become positively charged cations.
7. D) Conduct electricity when dissolved in water
→ Dissociation of ions in water allows current to flow.
8. C) Loses one electron to chlorine
→ Sodium gives up one electron to achieve a full outer shell.
9. D) Brittle solids with high melting points
→ Due to the strong electrostatic forces holding ions in place.
10. D) Mg²⁺
→ Losing two electrons gives magnesium a +2 charge.
11. D) HCl
→ Hydrogen chloride is covalent, not ionic.
12. C) Opposite charges attract
→ This explains the force that holds ions together in an ionic bond.
13. C) Spontaneous and exothermic
→ Ionic bond formation releases energy and happens naturally under many conditions.
14. B) Dissolved in water or melted
→ Free-moving ions allow conduction.
15. C) Potassium
→ Potassium is a metal, ready to donate electrons to fluorine.
16. C) Na₂O
→ Sodium oxide is composed of metal and nonmetal ions.
17. C) They are transferred from one atom to another
→ Typical in the formation of cations and anions.
18. B) CaCl₂
→ Calcium (2⁺) pairs with two Cl⁻ to balance charges.
19. B) Negative
→ Anions have more electrons than protons.
20. D) Ionic compounds have low melting points
→ False. Ionic compounds generally have high melting points.
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