Homework Answers
1)
Step 1: Find out electronegativity of both elements
Step 2: Find out the difference in electronegativity
Step 3: Use the following table to determine the character of bond. Note that the values in the below table are approximate values and not exact. This is because there is no well defined criteria that when does a polar covalent bond transitions to an ionic one and hence, different people use different table.
| Electronegativity difference | Bond Character |
| Greater than 1.7 | Ionic |
| Lesser than 1.7 but greater than 0.4 | Polar Covalent |
| Lesser than 0.4 | Non-polar Covalent |
a)
Electronegativity of K = 0.82
Electronegativity of Cl = 3.16
Difference = 3.16 - 0.82 = 2.34
Thus, this is an ionic bond
b)
Electronegativity of N = 3.04
Electronegativity of N = 3.04
Difference = 3.04-3.04 = 0
Thus, this is a non-polar covalent bond
c)
Electronegativity of C = 2.55
Electronegativity of S= 2.58
Difference = 2.58-2.55 = 0.03
Thus, this is a non-polar covalent bond
d)
Electronegativity of C = 2.55
Electronegativity of Cl = 3.16
Difference = 3.16-2.55 = 0.61
Thus, this is a polar covalent bond
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A covalent bond is a
bond in which electrons are shared between atoms of elements. A
covalent bond can be polar or nonpolar. In a nonpolar covalent
bond, the bond is between two identical atoms and the electrons are
evenly shared between the atoms.In contrast, in a
polar covalent bond, the bond is between two nonidentical atoms and
the electrons are unevenly shared between the atoms. The uneven
sharing of electrons takes place because of the difference in the
electronegativity...
Critical thinking questions
1) Determne the average electronegativity between EN1 and EN2
for each bond in the table above. Based on the data on table 1,
what combination of ΔEN given and average EN
values leads to ionic bonding?
2) Based on the data in table 1, what combination of
ΔEN and average EN values leads to non polar
covalent bonding?
3) Based on the data in table 1, what combination of
ΔEN and average EN values leads to polar...
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