Solution Found!
1. From what you remember of electronegativities, show the
Chapter 1, Problem 35SP(choose chapter or problem)
Problem 35SP
1. From what you remember of electronegativities, show the direction of the dipole moments of the following bonds.
2. In each case, predict whether the dipole moment is relatively large (electronegativity difference ) or small.
(a) C-Cl
(b) C-H
(c) C-Li
(d) C-N
(e) C-O
(f) C-B
(g) C-Mg
(h) N-H
(i) O-H
(j) C-Br
Questions & Answers
QUESTION:
Problem 35SP
1. From what you remember of electronegativities, show the direction of the dipole moments of the following bonds.
2. In each case, predict whether the dipole moment is relatively large (electronegativity difference ) or small.
(a) C-Cl
(b) C-H
(c) C-Li
(d) C-N
(e) C-O
(f) C-B
(g) C-Mg
(h) N-H
(i) O-H
(j) C-Br
ANSWER:
Solution 35SP :
Step 1:
Electronegativity is the measure of tendency of an atom to attract a bonding pair of electrons towards itself. An atom's electronegativity is affected by its atomic number and the distance at which its valence electrons reside from the charged nucleus.
Dipole moment is a measure of the polarity of the molecule, i.e it is a measure of the separation of two electrically opposite charges. The difference in the electronegativity of the atoms or ions causes the dipole moment. Larger, the difference in electronegativity, larger is the dipole moment.
- If the difference in electronegativity between two atoms or ions is less than 0.5, then the dipole moment is said to be small.
- If the difference in electronegativity between two atoms or ions is greater than 0.5, then the dipole moment is said to be large.
The direction of the dipole moment of a molecule is as shown below :
Here, the arrowhead of the symbol is always pointed towards the negative pole and the positive sign or plus sign is always towards the positive pole of the molecule.