Which pair of atoms forms a nonpolar covalent bond? which pair of atoms forms a nonpolar covalent bond? na and cl c and o n and

Question

posledela

4 years ago

13

Which pair of atoms forms a nonpolar covalent bond? which pair of atoms forms a nonpolar covalent bond? na and cl c and o n and

cl b and o?

Chemistry

2 answers:

adelina 88 [10] · Answer 1 · 2022-02-03T06:29:15+03:00

Types of Bonds can be predicted by calculating the difference in electronegativity.

If, Electronegativity difference is,

Less than 0.4 then it is Non Polar Covalent

Between 0.4 and 1.7 then it is Polar Covalent

Greater than 1.7 then it is Ionic

For Na and Cl,

E.N of Chlorine = 3.16

E.N of Sodium = 0.93

________

E.N Difference 2.23 (Ionic Bond)

For C and O,

E.N of Oxygen = 3.44

E.N of Carbon = 2.55

________

E.N Difference 0.89 (Polar Covalent Bond)

For N and Cl,

E.N of Chlorine = 3.16

E.N of Notrogen = 3.04

________

E.N Difference 0.12 (Non-Polar Covalent Bond)

For B and O,

E.N of Oxygen = 3.44

E.N of Boron = 2.04

________

E.N Difference 1.40 (Polar Covalent Bond)

IrinaK [193] · Answer 2 · 2022-02-03T08:20:53+03:00

$\boxed{{\text{N and Cl}}}$ will form a non-polar covalent compound.

Further Explanation:

Electronegativity:

It is the tendency of an atom to attract the shared electrons in the bond towards itself. More the electronegativity of the atom, higher will be its tendency to attract the bonding electrons towards itself. The electronegative atom develops a partial negative charge and the electropositive atom develops a partial positive charge.

The polarity of the bond can be determined by the electronegativity difference $\left({\Delta {\text{EN}}}\right)$ . $\Delta{\text{EN}}$ is the electronegativity difference between the two atoms that are bonded to each other.

The formula to calculate $\Delta{\text{EN}}$ in XY bond is as follows:

${{\Delta {\text{EN}}=\left( {{\text{electronegativity of Y}}} \right) - \left( {{\text{electronegativity of X}}} \right)$ .......(1)

Here,

X is the electropositive atom.

Y is the electronegative atom.

Higher the electronegativity difference between the two atoms, more will be the polarity of the bond and vice-versa.

1. If $\Delta\text{EN}}$ is less than 0.4, the bond formed will be non-polar covalent bond.

2. If $\Delta{\text{EN}}$ is between 0.4 and 1.7, the bond formed will be polar covalent bond.

3. If $\Delta{\text{EN}}$ is more than 1.7, the bond formed will be an ionic bond.

Na and Cl

Chlorine is more electronegative than sodium. Substitute 3 for the electronegativity of Y and 0.9 for the electronegativity of X in equation (1) to calculate the electronegativity difference between Na and Cl.

$\begin{aligned}\Delta \text{EN}_{\text{Na-Cl}}&=3-0.9\\&=2.1\end{aligned}$

The electronegativity difference between sodium and chlorine comes out to be greater than 1.7. So Na and Cl will form an ionic bond.

C and O

Oxygen is more electronegative than carbon. Substitute 3.5 for the electronegativity of Y and 2.5 for the electronegativity of X in equation (1) to calculate the electronegativity difference between C and O.

$\begin{aligned}\Delta \text{EN}_{\text{C-O}}&=3.5-2.5\\&=1\end{aligned}$

The electronegativity difference between carbon and chlorine is between 0.4 and 1.7. So C and O will form a polar covalent bond.

B and O

Oxygen is more electronegative than boron. Substitute 3.5 for the electronegativity of Y and 2 for the electronegativity of X in equation (1) to calculate the electronegativity difference between B and O.

$\begin{aligned}\Delta \text{EN}_{\text{B-O}}&=3.5-2\\&=1.5\end{aligned}$