(a) Arrange the following pairs of covalently bonded atoms in expected order of
increasing bond polarity: C-N, P-Cl, I-Cl, and C-O. (b) for each pair, indicate the direction of
the polarity of the bond, using the symbol +.
Look up the electronegativities and subtract to find the polarity.
Dr. Bob is dum
To determine the expected order of increasing bond polarity for the given pairs of covalently bonded atoms, we need to analyze the electronegativity values of the atoms involved. Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond.
(a) To compare the bond polarities, we can calculate the difference in electronegativity values between the two atoms in each pair. The greater the difference, the more polarized the bond.
The electronegativity values for the elements involved in each pair are as follows:
C (carbon) = 2.5
N (nitrogen) = 3.0
P (phosphorus) = 2.2
Cl (chlorine) = 3.2
I (iodine) = 2.7
O (oxygen) = 3.5
Now, let's calculate the differences in electronegativity for each pair:
C-N: 3.0 - 2.5 = 0.5
P-Cl: 3.2 - 2.2 = 1.0
I-Cl: 3.2 - 2.7 = 0.5
C-O: 3.5 - 2.5 = 1.0
The pairs can be arranged in expected order of increasing bond polarity based on the magnitude of the electronegativity differences:
C-N < I-Cl < C-O < P-Cl
(b) To indicate the direction of bond polarity, we can use the symbol "+" followed by an arrow pointing towards the more electronegative atom.
C-N: C + N
I-Cl: I + Cl
C-O: C + O
P-Cl: P + Cl
Remember, the direction of bond polarity always points from the less electronegative atom towards the more electronegative one.