Reasoning: In a covalent bond, the electron density is shared between the two atoms, and the degree of sharing depends on the electronegativity difference between them.

Both Assertion and Reasoning are true, and Reasoning is the correct explanation of Assertion.

Correct Answer

Wrong Answer

Both Assertion and Reasoning are true, but Reasoning is not the correct explanation of Assertion.

Correct Answer

Wrong Answer

Assertion is true, but Reasoning is false.

Correct Answer

Wrong Answer

Assertion is false, but Reasoning is true.

Correct Answer

Wrong Answer

View Solution

Assertion: The ionic character of a covalent bond increases with an increase in the bond length.

Reasoning: The electronegativity difference between two atoms decreases with an increase in bond length.

Both Assertion and Reasoning are true, and Reasoning is the correct explanation of Assertion.

Correct Answer

Wrong Answer

Both Assertion and Reasoning are true, but Reasoning is not the correct explanation of Assertion.

Correct Answer

Wrong Answer

Assertion is true, but Reasoning is false.

Correct Answer

Wrong Answer

Assertion is false, but Reasoning is true.

Correct Answer

Wrong Answer

View Solution

Assertion: A molecule with a polar covalent bond is always polar.

Reasoning: In a polar covalent bond, the electron pair is unequally shared between the two atoms, resulting in a dipole moment.

Both Assertion and Reasoning are true, and Reasoning is the correct explanation for Assertion.

Correct Answer

Wrong Answer

Both Assertion and Reasoning are true, but Reasoning is not the correct explanation for Assertion.

Correct Answer

Wrong Answer

Assertion is true, but Reasoning is false.

Correct Answer

Wrong Answer

Assertion is false, but Reasoning is true.

Correct Answer

Wrong Answer

View Solution

The property of the halogens to attract the bonded electrons of the covalent bond is known as

Electron affinity

Correct Answer

Wrong Answer

ionization potential

Correct Answer

Wrong Answer

Electronic attraction

Correct Answer

Wrong Answer

Electronegativity

Correct Answer

Wrong Answer

View Solution

Pursue MD/MS in USA

Want to study abroad? Plan your Journey

Apply

Pursue MD/MS in Ireland

Want to study abroad? Plan your Journey

Apply

Which of the following statements is incorrect regarding the ionic character in a covalent bond?

A covalent bond with higher electronegativity difference will have a higher percentage of ionic character.

Correct Answer

Wrong Answer

A covalent bond with a lower electronegativity difference will have a lower percentage of ionic character.

Correct Answer

Wrong Answer

The bond length has a significant effect on the ionic character of a covalent bond.

Correct Answer

Wrong Answer

None of the above.

Correct Answer

Wrong Answer

View Solution

Calculate the percentage of ionic character in a bond between two carbon atoms, given that the bond length is $1.54 A^0$ and the electronegativity values of carbon and hydrogen are 2.55 and 2.20, respectively

Correct Answer

Wrong Answer

9.89%

Correct Answer

Wrong Answer

19.18%

Correct Answer

Wrong Answer

30.31%

Correct Answer

Wrong Answer

View Solution

NEET 2026 Free Mock Test with Solutions

Download the NEET 2026 Free Mock Test PDF with detailed solutions. Practice real exam-style questions, analyze your performance, and enhance your preparation.

Download EBook

Calculate the percentage of ionic character in a bond between two nitrogen atoms, given that the bond length is 1.097 Å and the electronegativity of nitrogen is 3.04. (Take the electronegativity of nitrogen as the average of the electronegativity values of N and N+.)

4.21%

Correct Answer

Wrong Answer

8.42%

Correct Answer

Wrong Answer

16.84%

Correct Answer

Wrong Answer

33.68%

Correct Answer

Wrong Answer

View Solution

Concepts Covered - 1

Ionic Character in Covalent Bond

If the atoms that form a covalent bond are identical, as in H₂, Cl₂, and other diatomic molecules, then the electrons in the bond must be shared equally. We refer to this as a pure covalent bond. Electrons shared in pure covalent bonds have an equal probability of being near each nucleus.

In the case of Cl₂, each atom starts off with seven valence electrons, and each Cl shares one electron with the other, forming one covalent bond:

Cl+Cl⟶Cl₂

When the atoms linked by a covalent bond are different, the bonding electrons are shared, but no longer equally. Instead, the bonding electrons are more attracted to one atom than the other, giving rise to a shift of electron density toward that atom. This unequal distribution of electrons is known as a polar covalent bond, characterized by a partial positive charge on one atom and a partial negative charge on the other. The atom that attracts the electrons more strongly acquires the partial negative charge and vice versa. For example, the electrons in the H–Cl bond of a hydrogen chloride molecule are shifted towards chlorine. Thus, in an HCl molecule, the chlorine atom carries a partial negative charge and the hydrogen atom has a partial positive charge as shown in the figure given below.

(a) The distribution of electron density in the HCl molecule is uneven. The electron density is greater around the chlorine nucleus. (b) Symbols δ+ and δ– indicate the polarity of the H–Cl bond.

When the electronegativity difference is very small or zero, the bond is covalent and nonpolar. When it is large, the bond is polar covalent or ionic. The absolute values of the electronegativity differences between the atoms in the bonds H–H, H–Cl, and Na–Cl are 0 (nonpolar), 0.9 (polar covalent), and 2.1 (ionic), respectively. The degree to which electrons are shared between atoms varies from completely equal (pure covalent bonding) to not at all (ionic bonding). The figure below shows the relationship between electronegativity difference and bond type.