which of these molecules do not contain polar bonds? (reference p 240 of your textbook.)
a xef₂
b clf₃
c pcl₃
d tecl₄

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Accepted Answer

# Brief Explanations:
- Polar bonds occur when there is a significant difference in electronegativity between the atoms forming the bond.
- In $XeF_2$, $Xe - F$ bonds are polar due to the difference in electronegativity between $Xe$ and $F$.
- In $ClF_3$, $Cl - F$ bonds are polar as $Cl$ and $F$ have different electronegativities.
- In $PCl_3$, $P - Cl$ bonds are polar because of the electronegativity difference between $P$ and $Cl$.
- In $TeCl_4$, $Te - Cl$ bonds are polar due to the difference in electronegativity between $Te$ and $Cl$.

Wait, there is a mistake in the above analysis. Let's re - analyze:
- A polar bond is formed when two different atoms (with different electronegativities) are bonded.
- All the given molecules ($XeF_2$, $ClF_3$, $PCl_3$, $TeCl_4$) have bonds between different atoms. However, if we consider the question again, maybe there is a mis - understanding. Wait, no, all of these have polar bonds. But if we assume that there is a typo and maybe one of them is a diatomic molecule of the same atom (but in the given options, there is no such case). Wait, another approach: maybe the question is about non - polar molecules (but the question clearly asks about non - polar bonds). Wait, no, all bonds in these molecules (since they are between different atoms) are polar. But if we check the electronegativity values:
    - For $XeF_2$: $Xe$ has an electronegativity of approximately $2.6$ and $F$ has $4.0$. The $Xe - F$ bond is polar.
    - For $ClF_3$: $Cl$ (electronegativity $\sim3.0$) and $F$ ($4.0$), $Cl - F$ bond is polar.
    - For $PCl_3$: $P$ (electronegativity $\sim2.1$) and $Cl$ ($3.0$), $P - Cl$ bond is polar.
    - For $TeCl_4$: $Te$ (electronegativity $\sim2.1$) and $Cl$ ($3.0$), $Te - Cl$ bond is polar.

Wait, maybe the original question was about non - polar molecules (a common confusion). But if we strictly follow the question (non - polar bonds):
- A non - polar bond is between two identical atoms (e.g., $H_2$ ($H - H$ bond), $O_2$ ($O=O$ bond)). Since all the given molecules have bonds between different atoms, there is an error in the problem. But if we assume that it was a misprint and the question was about non - polar molecules:
    - $XeF_2$ has a linear geometry ($F - Xe - F$), and the bond dipoles cancel out (molecule is non - polar), but the $Xe - F$ bonds are still polar.
    - $ClF_3$ has a T - shaped geometry, and the bond dipoles do not cancel (molecule is polar).
    - $PCl_3$ has a trigonal pyramidal geometry, and the bond dipoles do not cancel (molecule is polar).
    - $TeCl_4$ has a see - saw geometry, and the bond dipoles do not cancel (molecule is polar).

If we assume that the question was misphrased (should be non - polar molecules), then $XeF_2$ (molecule is non - polar, but bonds are polar). But if we follow the question (non - polar bonds), there is no correct answer. But if we consider the electronegativity difference:
- For $PCl_3$: $P$ ($2.1$) and $Cl$ ($3.0$), $\Delta EN=3.0 - 2.1 = 0.9$
- For $TeCl_4$: $Te$ ($2.1$) and $Cl$ ($3.0$), $\Delta EN = 3.0-2.1=0.9$
- For $ClF_3$: $Cl$ ($3.0$) and $F$ ($4.0$), $\Delta EN=4.0 - 3.0=1.0$
- For $XeF_2$: $Xe$ ($2.6$) and $F$ ($4.0$), $\Delta EN=4.0 - 2.6 = 1.4$

All have polar bonds. But if we consider that in some textbooks, a small electronegativity difference ($<0.5$) is considered non - polar. But in these cases, the differences are $>0.5$.

Alternatively, if we check the structure for symmetry (for molecule polarity, but again, question is about bond polarity):
- A bond is polar if $EN_1
eq EN_2$. Since all these are between different elements ($Xe - F$, $Cl - F$, $P - Cl$, $Te - Cl$), all bonds are polar. But if we assume that the question was about non - polar molecules (a common error in such questions):
    - $XeF_2$ has a linear shape ($F - Xe - F$), and the bond dipoles ($\mu_{Xe - F}$) cancel each other out (molecule is non - polar), but the $Xe - F$ bonds are polar.
    - $ClF_3$ (T - shaped, asymmetric, molecule is polar)
    - $PCl_3$ (trigonal pyramidal, asymmetric, molecule is polar)
    - $TeCl_4$ (see - saw, asymmetric, molecule is polar)

If we follow the mis - phrased (but common) question (non - polar molecules), then $XeF_2$ (molecule is non - polar). But if we follow the exact question (non - polar bonds), there is no correct answer. But since the options are given and considering common textbook problems (mis - labeled as bond polarity instead of molecule polarity):

# Answer:
A. $XeF_2$ (assuming the question was about non - polar molecules, as all bonds in the given options are polar. If strictly about non - polar bonds, there is no correct answer, but following common textbook errors)

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