Question:
Identify the element that can exhibit negative oxidation states.
Identify the element that can exhibit negative oxidation states.
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Only highly electronegative Group 14 element (carbon) commonly shows negative oxidation states like -4.
Updated On: Jun 20, 2026
- C
- Ge
- Sn
- Pb
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The Correct Option is A
Solution and Explanation
Step 1: Understand oxidation state behavior in Group 14 elements.
Group 14 elements (C, Si, Ge, Sn, Pb) generally show +4 and +2 oxidation states due to availability of four valence electrons. However, ability to show negative oxidation state depends on electronegativity and tendency to gain electrons.
Step 2: Analyze carbon (C).
Carbon is highly electronegative compared to other Group 14 elements. It can easily gain electrons from more electropositive elements like metals, forming compounds such as carbides (e.g., CH\(_4\), where it is assigned -4 oxidation state). Hence carbon can show negative oxidation states.
Step 3: Analyze Ge, Sn, Pb.
Germanium, tin, and lead are more metallic in nature. They are less electronegative and prefer losing electrons rather than gaining them. Therefore, they rarely or do not show negative oxidation states in typical chemistry.
Step 4: Compare periodic trend.
Down the group, metallic character increases and electronegativity decreases. Thus, tendency to show negative oxidation state decreases from carbon to lead.
Step 5: Final evaluation.
Only carbon has sufficient electronegativity to acquire electrons and exhibit negative oxidation states in compounds with electropositive elements.
Final Answer: \[ \boxed{\text{C}} \]
Group 14 elements (C, Si, Ge, Sn, Pb) generally show +4 and +2 oxidation states due to availability of four valence electrons. However, ability to show negative oxidation state depends on electronegativity and tendency to gain electrons.
Step 2: Analyze carbon (C).
Carbon is highly electronegative compared to other Group 14 elements. It can easily gain electrons from more electropositive elements like metals, forming compounds such as carbides (e.g., CH\(_4\), where it is assigned -4 oxidation state). Hence carbon can show negative oxidation states.
Step 3: Analyze Ge, Sn, Pb.
Germanium, tin, and lead are more metallic in nature. They are less electronegative and prefer losing electrons rather than gaining them. Therefore, they rarely or do not show negative oxidation states in typical chemistry.
Step 4: Compare periodic trend.
Down the group, metallic character increases and electronegativity decreases. Thus, tendency to show negative oxidation state decreases from carbon to lead.
Step 5: Final evaluation.
Only carbon has sufficient electronegativity to acquire electrons and exhibit negative oxidation states in compounds with electropositive elements.
Final Answer: \[ \boxed{\text{C}} \]
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