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Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425

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BuyFindarrow_forward

Introductory Chemistry: A Foundati...

9th Edition
Steven S. Zumdahl + 1 other
ISBN: 9781337399425
Textbook Problem
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ompare and contrast the bonding found in the H 2 ( g ) and HF ( g ) molecules with that found in NaF ( s ) .

Interpretation Introduction

Interpretation:

The comparison between the bonding found in H2(g) and HF(g) molecules with that found in NaF(s) is to be stated.

Concept Introduction:

The tendency of an atom to attract electrons towards it is referred to as electronegativity. It aids in the unequal distribution of charges in a molecule. The electronegativity is the primary factor that determines the type of bond formed. The general rule is that if the electronegativity difference is more than 2, then the bond formed will be ionic. The polar covalent bond will be formed if the electronegativity difference is between 0.5 to 2.

There are two types of polar bonds named as polar covalent bonds and non-polar covalent bonds.

Explanation

The valence shell of the hydrogen atom has one electron. In H2(g) molecule, both the hydrogen atoms combine by sharing the electrons to form a stable molecule. Hence, a covalent bond is formed in H2 molecule.

Sodium is electropositive alkali metal which has +1 charge in its valence shell. Fluorine is a nonmetal, which has 7 electrons in its valence shell. It indicates that fluorine has a high tendency to attract one electron for high stability, whereas sodium loses its one electron to get stable. The attraction between the positive charge of sodium and the negative charge of fluorine takes place. Hence, an ionic bond is formed in NaF compound.

Therefore, the H2 molecule is formed by covalent bonding whereas NaF compound is formed by ionic bonding

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