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Consider the molecules CH4ā,NH3ā and H2āO. Which of the given statements is false ?
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Organic Chemistry Some Basic Principles and Techniques
2016
chemistry
The H ā C ā H bond angle in CH4ā, the H ā N ā H bond angle in NH3ā, and the H ā O ā H bond angle in H2āO
Explanation
To determine which statement is false, we need to analyze the bond angles in CH4ā,NH3ā, and H2āO.
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The H ā O ā H bond angle in H2āO is larger than the H ā C ā H bond angle in CH4ā.
The H ā O ā H bond angle in H2āO is smaller than the H ā N ā H bond angle in NH3ā.
The H ā C ā H bond angle in CH4ā is larger than the H ā N ā H bond angle in NH3ā.
1.
(methane) has a tetrahedral geometry with bond angles of
109.5ā. 2.
(ammonia) has a trigonal pyramidal geometry due to the lone pair on nitrogen,
resulting in bond angles of approximately
107ā. 3.
(water) has a bent geometry due to two lone pairs on oxygen,
resulting in bond angles of approximately
104.5ā. Now, let's evaluate each option:
Option 1: The H ā C ā H bond angle in
the H ā N ā H bond angle in
and the H ā O ā H bond angle in
are all greater than
90ā. - This is true because all the mentioned bond angles are greater than
90ā. Option 2: The H ā O ā H bond angle in
is larger than the H ā C ā H bond angle in
- This is false because
104.5ā (H ā O ā H) is smaller than
109.5ā (H ā C ā H).
Option 3: The H ā O ā H bond angle in
is smaller than the H ā N ā H bond angle in
- This is true because
104.5ā (H ā O ā H) is smaller than
107ā (H ā N ā H).
Option 4: The H ā C ā H bond angle in
is larger than the H ā N ā H bond angle in
- This is true because
109.5ā (H ā C ā H) is larger than
107ā (H ā N ā H).
Therefore, the false statement is Option 2.