Question

part 2 draw the attraction between a water molecule and a molecule of nf₃
h₂o has 4 reds and is symmetrical/asymmetrical (answer is 1) making it a
polar/nonpolar (answer is 2) molecule.
each h has a 3 charge and the o has a 4 charge.
the strongest possible attractive force between these two molecules is 5.
a. nonpolar covalent b. polar covalent c. ionic d. polar
e. nonpolar f. 0.97 g. 0 h. 0.01 i. 0.94 j. 0.40
j. 1.24 l. diatomic m. bent n. pyramidal o. planar trigonal
p. tetrahedral q. symmetrical r. asymmetrical
s. londons t. dipole - dipole u. hydrogen bond v. ion - dipole
w. δ+ x. δ- y. no partial charge

Explanation:

• For question 1: The water molecule (\(H_2O\)) has a bent shape. Due to the presence of two lone pairs on the oxygen atom, the distribution of electron - density is not symmetric. So, it is asymmetrical.
• For question 2: Since the molecule is asymmetrical and oxygen is more electronegative than hydrogen, the molecule has a net dipole moment. So, it is polar.
• For question 3: Hydrogen is less electronegative than oxygen. In a polar \(H - O\) bond, hydrogen has a partial positive (\(\delta+\)) charge.
• For question 4: Oxygen is more electronegative than hydrogen. In a polar \(H - O\) bond, oxygen has a partial negative (\(\delta-\)) charge.
• For question 5: Both \(H_2O\) and \(NF_3\) are polar molecules. The strongest intermolecular force between two polar molecules is dipole - dipole interaction.

Answer:

1. R. asymmetrical
2. D. polar
3. W. \(\delta+\)
4. X. \(\delta-\)
5. T. dipole - dipole