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Magazine Chapter 1: PROBLEM 1.5 (page 47)
Question: Use electronegativities to predict the direction of the dipole moments of the following bonds.
- C-Br
- C-I
- C-Si
- B-Cl
- B-F
- N-F
- N-Br
- Si-Br
- Si-Cl
- Si-F
Short Answer
Answer
The symbols 鈥�鈥� and 鈥�鈥� indicate bond polarity by showing a partial charge. (In arrow symbolism, the arrow should point to the partial negative charge.)
The dipole moment for the given bonds are:
a.
b.
c.
d.
e.
f.
g.
No dipole moment in.
h.
i.
j.
Step by step solution
Definition of lone pair
A non-polar covalent bond is one where the electrons are shared equally between two atoms, and a polar covalent bond is defined as an unequally shared pair of bonding electrons. The bonding electrons are drawn more strongly to one of the two nuclei in most bonds between two distinct elements.
Dipole moment of C-Br bond
The given bond is C-Br. Electronegativity of carbon and bromine are 2.5 and 3.0, respectively. Therefore, the dipole moment of the given bond is as follows:
Dipole moment of C-Br bond
Dipole moment of C-I bond
The given bond is C-I. Electronegativity of carbon and iodine are 2.5 and 2.7, respectively. Therefore, the dipole moment of the given bond is as follows
Dipole moment of C-I bond
Dipole moment of C-Si bond
The given bond is C-Si. Electronegativity of carbon and silicon are 2.5 and 1.9, respectively. Therefore, the dipole moment of the given bond is as follows:
Dipole moment of C-Si bond
Dipole moment of B-Cl bond
The given bond is B-Cl. Electronegativity of boron and chlorine are 2.0 and 3.2, respectively. Therefore, the dipole moment of the given bond is as follows:
Dipole moment of B-Cl bond
Dipole moment of B-F bond
The given bond is B-F. Electronegativity of carbon and fluorine are 2.0 and 4.0, respectively. Therefore, the dipole moment of the given bond is as follows
Dipole moment of B-F bond
Dipole moment of N-F bond
The given bond is N-F. Electronegativity of nitrogen and fluorine are 3.0 and 4.0, respectively. Therefore, the dipole moment of the given bond is as follows:
Dipole moment of N-F bond
Dipole moment of N-Br bond
The given bond is N-Br. Electronegativity of nitrogen and bromine are 3.0 and 3.0, respectively. Therefore, there is no dipole moment in the given bond:
No dipole moment in N-Br
Dipole moment of Si-Br bond
The given bond is Si-Br. Electronegativity of silicon and bromine are 1.9 and 3.0, respectively. Therefore, the dipole moment of the given bond is as follows:
Dipole moment of Si-Br bond
Dipole moment of Si-Cl bond
The given bond is Si-Cl. Electronegativity of silicon and chlorine are 1.9 and 3.2, respectively. Therefore, the dipole moment of the given bond is as follows:
Dipole moment of Si-Cl bond
Dipole moment of Si-F bond
The given bond is Si-F. Electronegativity of silicon and fluorine are 1.9 and 4.0, respectively. Therefore, the dipole moment of the given bond is as follows:
Dipole moment of Si-F bond
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