Question

question 4 (0.5 points)
part 2 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: \(H_2O\) has a bent shape. The oxygen atom has two lone pairs and two bonding pairs. Due to the presence of lone - pairs and the difference in electronegativity between \(O\) and \(H\), the molecule is asymmetrical.
• For polarity: Since the molecule is asymmetrical and there is a significant electronegativity difference (\(O: 3.44\), \(H: 2.20\)) between the atoms in the \(O - H\) bonds, \(H_2O\) is a polar molecule.
• For partial charges: Oxygen is more electronegative than hydrogen. So, hydrogen has a partial positive (\(\delta+\)) charge and oxygen has a partial negative (\(\delta-\)) charge.
• For intermolecular force: The strongest intermolecular force between \(H_2O\) molecules is hydrogen bonding. Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom (\(O\), \(N\), or \(F\)) and interacts with another electronegative atom.

Answer:

1. R. asymmetrical
2. D. polar
3. W. \(\delta+\)
4. X. \(\delta-\)
5. U. hydrogen bond