Question:
Which of the following species is not tetrahedral?
Which of the following species is not tetrahedral?
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A perfect tetrahedral geometry requires four bonding atoms around the central atom with no lone pairs. Molecules with lone pairs, like \( \text{SF}_4 \), deviate from tetrahedral geometry.
Updated On: Jun 30, 2026
- \( \text{CH}_4 \)
- \( \text{SF}_4 \)
- \( \text{NH}_4^+ \)
- \( \text{SiCl}_4 \)
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The Correct Option is B
Solution and Explanation
Step 1: Recognize the geometry of tetrahedral molecules.
In a tetrahedral molecule, the central atom is bonded to four other atoms arranged symmetrically in three-dimensional space, forming a tetrahedral shape with bond angles of 109.5°. The common tetrahedral species include \( \text{CH}_4 \) (methane), \( \text{NH}_4^+ \) (ammonium ion), and \( \text{SiCl}_4 \) (silicon tetrachloride).
Step 2: Analyze the species \( \text{SF}_4 \).
Sulfur tetrafluoride \( \text{SF}_4 \) has a central sulfur atom bonded to four fluorine atoms. However, \( \text{SF}_4 \) does not have a perfect tetrahedral geometry because it has one lone pair of electrons on the sulfur atom. This results in a see-saw geometry rather than a tetrahedral geometry. Therefore, \( \text{SF}_4 \) is not tetrahedral.
Step 3: Conclusion.
Thus, \( \text{SF}_4 \) is not tetrahedral, making option (B) the correct answer.
\[ \boxed{\text{(B) \( \text{SF}_4 \)}} \]
In a tetrahedral molecule, the central atom is bonded to four other atoms arranged symmetrically in three-dimensional space, forming a tetrahedral shape with bond angles of 109.5°. The common tetrahedral species include \( \text{CH}_4 \) (methane), \( \text{NH}_4^+ \) (ammonium ion), and \( \text{SiCl}_4 \) (silicon tetrachloride).
Step 2: Analyze the species \( \text{SF}_4 \).
Sulfur tetrafluoride \( \text{SF}_4 \) has a central sulfur atom bonded to four fluorine atoms. However, \( \text{SF}_4 \) does not have a perfect tetrahedral geometry because it has one lone pair of electrons on the sulfur atom. This results in a see-saw geometry rather than a tetrahedral geometry. Therefore, \( \text{SF}_4 \) is not tetrahedral.
Step 3: Conclusion.
Thus, \( \text{SF}_4 \) is not tetrahedral, making option (B) the correct answer.
\[ \boxed{\text{(B) \( \text{SF}_4 \)}} \]
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