Question

question 6 (0.5 points)
part 2 draw the attraction between a water molecule and a molecule of pcl3
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
k. 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 the symmetry of \(H_2O\): The water molecule has a bent shape (\(H - O - H\) bond angle is about \(104.5^{\circ}\)), so it is asymmetrical.
• For the polarity of \(H_2O\): Due to its asymmetrical shape and the difference in electronegativity between \(O\) (electronegativity = 3.44) and \(H\) (electronegativity = 2.20), \(H_2O\) is a polar molecule.
• For the partial charges: In \(H_2O\), \(H\) has a lower electronegativity than \(O\). So each \(H\) has a \(\delta+\) (partial positive) charge and \(O\) has a \(\delta-\) (partial negative) charge.
• For the attractive force: \(PCl_3\) has a trigonal - pyramidal shape (as \(P\) has a lone pair and three \(P - Cl\) bonds) and is polar. The strongest force between two polar molecules (\(H_2O\) and \(PCl_3\)) is dipole - dipole force.

Answer:

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