practice
molecule lewis
structure does it
contain polar
bonds? is the
molecule
polar? intermolecular forces present
van der
waals (√)
dipole-dipole
(√)
hydrogen
bonds (√)
pcl₃
f₂
bf₃
ccl₄
hf
h₂o
ch₃cl

Question

Accepted Answer

# Brief Explanations:
- **For $PCl_{3}$**:
    - Lewis structure: Phosphorus is the central atom. It has 5 valence electrons. Three are used to form bonds with chlorine atoms (each chlorine has 7 valence electrons). There is one lone pair on phosphorus. The structure is trigonal pyramidal.
    - Polar bonds: $P - Cl$ bonds are polar (electronegativity difference: $Cl(3.0) - P(2.1)=0.9$).
    - Molecular polarity: The molecule is polar due to the trigonal - pyramidal shape (lone pair causes asymmetry).
    - Intermolecular forces: Van der Waals (all molecules have this), dipole - dipole (because it is polar).
- **For $F_{2}$**:
    - Lewis structure: Each fluorine atom has 7 valence electrons. They share one pair of electrons ($F - F$ single bond).
    - Polar bonds: $F - F$ bond is non - polar (electronegativity difference $=0$).
    - Molecular polarity: Non - polar.
    - Intermolecular forces: Only van der Waals.
- **For $BF_{3}$**:
    - Lewis structure: Boron is the central atom with 3 valence electrons. It forms three $B - F$ bonds (each $F$ has 7 valence electrons). The structure is trigonal planar.
    - Polar bonds: $B - F$ bonds are polar ($F(4.0)-B(2.0)=2.0$).
    - Molecular polarity: Non - polar (trigonal planar symmetry cancels out bond dipoles).
    - Intermolecular forces: Only van der Waals.
- **For $CCl_{4}$**:
    - Lewis structure: Carbon is the central atom with 4 valence electrons. It forms four $C - Cl$ bonds (each $Cl$ has 7 valence electrons). The structure is tetrahedral.
    - Polar bonds: $C - Cl$ bonds are polar ($Cl(3.0)-C(2.5)=0.5$).
    - Molecular polarity: Non - polar (tetrahedral symmetry cancels out bond dipoles).
    - Intermolecular forces: Only van der Waals.
- **For $HF$**:
    - Lewis structure: Hydrogen (1 valence electron) and fluorine (7 valence electrons) share one pair ($H - F$ bond).
    - Polar bonds: $H - F$ bond is polar ($F(4.0)-H(2.1)=1.9$).
    - Molecular polarity: Polar.
    - Intermolecular forces: Van der Waals, dipole - dipole, and hydrogen bonds ($H$ is bonded to highly electronegative $F$).
- **For $H_{2}O$**:
    - Lewis structure: Oxygen (6 valence electrons) is the central atom. It forms two $O - H$ bonds (each $H$ has 1 valence electron). There are two lone pairs on oxygen. The structure is bent.
    - Polar bonds: $O - H$ bonds are polar ($O(3.5)-H(2.1)=1.4$).
    - Molecular polarity: Polar (bent shape causes asymmetry).
    - Intermolecular forces: Van der Waals, dipole - dipole, and hydrogen bonds ($H$ is bonded to highly electronegative $O$).
- **For $CH_{3}Cl$**:
    - Lewis structure: Carbon is the central atom. It forms three $C - H$ bonds ($H$ has 1 valence electron) and one $C - Cl$ bond ($Cl$ has 7 valence electrons). The structure is tetrahedral (asymmetrical due to $Cl$).
    - Polar bonds: $C - Cl$ bond is polar ($Cl(3.0)-C(2.5)=0.5$), $C - H$ bonds are slightly polar ($C(2.5)-H(2.1)=0.4$).
    - Molecular polarity: Polar.
    - Intermolecular forces: Van der Waals, dipole - dipole.

# Answer:
| Molecule | Lewis structure | Does it contain polar bonds? | Is the molecule polar? | Intermolecular Forces present |
|---|---|---|---|---|
| $PCl_{3}$ | Central $P$ with three $P - Cl$ bonds and one lone pair | Yes | Yes | Van der Waals ($\checkmark$), Dipole - dipole ($\checkmark$) |
| $F_{2}$ | $F - F$ single bond | No | No | Van der Waals ($\checkmark$) |
| $BF_{3}$ | Central $B$ with three $B - F$ bonds (trigonal planar) | Yes | No | Van der Waals ($\checkmark$) |
| $CCl_{4}$ | Central $C$ with four $C - Cl$ bonds (tetrahedral) | Yes | No | Van der Waals ($\checkmark$) |
| $HF$ | $H - F$ single bond | Yes | Yes | Van der Waals ($\checkmark$), Dipole - dipole ($\checkmark$), Hydrogen bonds ($\checkmark$) |
| $H_{2}O$ | Central $O$ with two $O - H$ bonds and two lone pairs (bent) | Yes | Yes | Van der Waals ($\checkmark$), Dipole - dipole ($\checkmark$), Hydrogen bonds ($\checkmark$) |
| $CH_{3}Cl$ | Central $C$ with three $C - H$ and one $C - Cl$ bond (asymmetric tetrahedral) | Yes | Yes | Van der Waals ($\checkmark$), Dipole - dipole ($\checkmark$) |

Molecule	Lewis structure	Does it contain polar bonds?	Is the molecule polar?	Intermolecular Forces present
\(F_{2}\)	\(F - F\) single bond	No	No	Van der Waals (\(\checkmark\))
\(BF_{3}\)	Central \(B\) with three \(B - F\) bonds (trigonal planar)	Yes	No	Van der Waals (\(\checkmark\))
\(CCl_{4}\)	Central \(C\) with four \(C - Cl\) bonds (tetrahedral)	Yes	No	Van der Waals (\(\checkmark\))
\(HF\)	\(H - F\) single bond	Yes	Yes	Van der Waals (\(\checkmark\)), Dipole - dipole (\(\checkmark\)), Hydrogen bonds (\(\checkmark\))
\(H_{2}O\)	Central \(O\) with two \(O - H\) bonds and two lone pairs (bent)	Yes	Yes	Van der Waals (\(\checkmark\)), Dipole - dipole (\(\checkmark\)), Hydrogen bonds (\(\checkmark\))
\(CH_{3}Cl\)	Central \(C\) with three \(C - H\) and one \(C - Cl\) bond (asymmetric tetrahedral)	Yes	Yes	Van der Waals (\(\checkmark\)), Dipole - dipole (\(\checkmark\))

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