Respuesta :
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)
[tex]\boxed{{\text{N and Cl}}}[/tex] 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 [tex]\left({\Delta {\text{EN}}}\right)[/tex]. [tex]\Delta{\text{EN}}[/tex] is the electronegativity difference between the two atoms that are bonded to each other.
The formula to calculate [tex]\Delta{\text{EN}}[/tex] in XY bond is as follows:
[tex]{{\Delta {\text{EN}}=\left( {{\text{electronegativity of Y}}} \right) - \left( {{\text{electronegativity of X}}} \right)[/tex] .......(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 [tex]\Delta\text{EN}}[/tex] is less than 0.4, the bond formed will be non-polar covalent bond.
2. If [tex]\Delta{\text{EN}}[/tex] is between 0.4 and 1.7, the bond formed will be polar covalent bond.
3. If [tex]\Delta{\text{EN}}[/tex] 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.
[tex]\begin{aligned}\Delta \text{EN}_{\text{Na-Cl}}&=3-0.9\\&=2.1\end{aligned}[/tex]
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.
[tex]\begin{aligned}\Delta \text{EN}_{\text{C-O}}&=3.5-2.5\\&=1\end{aligned}[/tex]
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.
[tex]\begin{aligned}\Delta \text{EN}_{\text{B-O}}&=3.5-2\\&=1.5\end{aligned}[/tex]
The electronegativity difference between boron and oxygen is between 0.4 and 1.7. So B and O will form a polar covalent bond.
N and Cl
The electronegativity of nitrogen and chlorine is nearly equal so N and Cl will form a non-polar covalent bond.
Learn more:
1. Identification of ionic bonding: https://brainly.com/question/1603987
2. Which is a covalent compound? https://brainly.com/question/2083444
Answer details:
Grade: High School
Subject: Chemistry
Chapter: Ionic and covalent compounds
Keywords: electronegativity difference, electropositive, electronegative, polar, non-polar, ionic, 0.4, 1.7, N, Cl, O, C, B.
