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Consider the molecules CH4,NH3 and H2O. Which of the given statements is false ?
medium
Organic Chemistry Some Basic Principles and Techniques
2016
chemistry
The H – C – H bond angle in CH4, the H – N – H bond angle in NH3, and the H – O – H bond angle in H2O
Explanation
To determine which statement is false, we need to analyze the bond angles in CH4,NH3, and H2O.
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Sign up / Login are all greater than
The H – O – H bond angle in H2O is larger than the H – C – H bond angle in CH4.
The H – O – H bond angle in H2O is smaller than the H – N – H bond angle in NH3.
The H – C – H bond angle in CH4 is larger than the H – N – H bond angle in NH3.
1.
(methane) has a tetrahedral geometry with bond angles of
109.5∘. 2.
(ammonia) has a trigonal pyramidal geometry due to the lone pair on nitrogen,
resulting in bond angles of approximately
107∘. 3.
(water) has a bent geometry due to two lone pairs on oxygen,
resulting in bond angles of approximately
104.5∘. Now, let's evaluate each option:
Option 1: The H – C – H bond angle in
the H – N – H bond angle in
and the H – O – H bond angle in
are all greater than
- This is true because all the mentioned bond angles are greater than
Option 2: The H – O – H bond angle in
is larger than the H – C – H bond angle in
- This is false because
104.5∘ (H – O – H) is smaller than
109.5∘ (H – C – H).
Option 3: The H – O – H bond angle in
is smaller than the H – N – H bond angle in
- This is true because
104.5∘ (H – O – H) is smaller than
(H – N – H).
Option 4: The H – C – H bond angle in
is larger than the H – N – H bond angle in
- This is true because
109.5∘ (H – C – H) is larger than
(H – N – H).
Therefore, the false statement is Option 2.