This set of Class 11 Chemistry Chapter 4 Multiple Choice Questions & Answers (MCQs) focuses on “Ionic or Electrovalent Bond”.
1. A chemical bond formation that involves the complete transfer of electrons between atoms is _______
a) ionic bond
b) covalent bond
c) metallic bond
d) partial covalent bond
View Answer
Explanation: Ionic bond, which is otherwise known as electrovalent bond forms between two atoms by the transfer of electrons between them. It generates oppositely charged ions. Positively charged ions are mostly metals and the vice-versa.
2. Formation of a compound through ionic bond ______ the ionization energy of the metal ion.
a) does not depends on
b) depend on
c) is independent regarding
d) may or may not depend on
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Explanation: For the formation of the ionic bond, the metal ion has to overcome to energy for the removal of an electron from its outer shell in order to become a cation, that is ionization energy. Therefore Formation of a compound through ionic bond depends on the ionization energy of the metal ion.
3. The enthalpy change that occurs when an atom in the ground state gains an electron, is electron gain enthalpy.
a) True
b) False
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Explanation: Yes. electron gain enthalpy is the enthalpy change for an atom in the ground state to gain an electron. An atom gains an electron, thus forming negatively charged ion also known as a cation. Symbolic representation is as follows: A(g) + e– → A(g)–.
4. Electron gain enthalpy may be ________
a) exothermic
b) endothermic
c) both exothermic and endothermic
d) always zero
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Explanation: Electron gain enthalpy is the enthalpy change for an atom in the ground state to gain an electron. In the case of an exothermic reaction, the value of electron gain enthalpy is negative, which means that it is releasing energy and vice-versa when it’s positive.
5. Ionic bonds easily form when electron when ionization energy of the metallic atom is _____ comparatively.
a) negative
b) constant
c) more
d) less
View Answer
Explanation: The rate of formation of an ionic bond mainly depends on the tendency to become cation and anion from their original ground states. The tendency is maximum for metallic atoms whose ionization energy is less than the other atoms.
6. What is the energy that is released upon the formation of an ionic compound known as?
a) Ionization energy
b) Lattice energy
c) Electron gain enthalpy
d) Electropositivity
View Answer
Explanation: When the ions are combined to form an ionic compound that is a crystalline solid, a certain amount of energy is released and this is known as the lattice energy. Solubility, volatility, and hardness can be predicted from lattice energy.
7. What’s the amount of lattice energy of NaCl?
a) 788 KJ mol-1
b) 688 KJ mol-1
c) 588 KJ mol-1
d) 488 KJ mol-1
View Answer
Explanation: NaCl’s lattice enthalpy is given by 788 KJ mol-1. To disassociate one mole of NaCl into one mole of Na+ and one mole of Cl-1 into an infinite distance, we need 788 KJ mol-1 of energy. When the ions are combined to form an ionic compound that is a crystalline solid, a certain amount of energy is released and this is known as the lattice energy.
8. Which of the following molecule’s formation doesn’t include ionic bond?
a) LiCl
b) MgO
c) SnCl4
d) H2O
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Explanation: The molecules LiCl, MgO, and SnCl4 are formed by ionic bonds as they transfer electrons from an electropositive atom, that donates to the electronegative atom, that accepts. Whereas H2O has covalent bonds as it shares electrons.
9. Ionization energy is always endothermic in nature.
a) False
b) True
View Answer
Explanation: Ionization energy is the minimum amount of energy that is required to remove an electron from a neutral isolated gaseous atom. The symbolic representation is given by A(g) → A(g)+ + e–. It is always negative as it requires energy that is endothermic in nature.
10. Ionic bond formation depends on the arrangement of __________
a) molecule
b) atom
c) lattice
d) kernal
View Answer
Explanation: Lattice of the crystalline compound is the arrangement of positive and the negative ions inside a substance. It is dependent on the ease of formation of ionic bonds as per Kossel and Lewis Ionic bond formation.
Sanfoundry Global Education & Learning Series – Chemistry – Class 11.
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