Consider the oxides of group 14 elements \(SiO_2,GeO_2,SnO_2,PbO_2,CO\) and \(GeO\). The amphoteric oxides are
- \(GeO, GeO_2\)
- \(SiO_2, GeO_2\)
- \(SnO_2, PbO_2\)
- \(SnO_2, CO\)
The Correct Option is C
Solution and Explanation
The question asks us to identify the amphoteric oxides among the given options of group 14 element oxides. Amphoteric oxides are those that can react both as acids and bases. To solve this, we need to consider the properties of each given oxide.
- \(CO\): This is a neutral oxide, not amphoteric.
- \(SiO_2\): Silicon dioxide is acidic and not amphoteric.
- \(GeO\): Germanium monoxide is a basic oxide, not amphoteric.
- \(GeO_2\): Germanium dioxide is amphoteric.
- \(SnO_2\): Tin dioxide is amphoteric as it can react with both acids and bases.
- \(PbO_2\): Lead dioxide is amphoteric, as it can also react with acids and bases.
Based on the above analysis, the oxides that are amphoteric from the given group 14 elements are \(SnO_2\) and \(PbO_2\). Therefore, the correct answer is:
\(SnO_2, PbO_2\)
These oxides (\(SnO_2\) and \(PbO_2\)) can react with both acids, such as hydrochloric acid, and bases like sodium hydroxide, exhibiting their amphoteric behavior.
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- Given below are two statements:
Statement I: The electronegativity of group 14 elements from Si to Pb gradually decreases.
Statement II: Group 14 contains non-metallic, metallic, as well as metalloid elements.
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(A) Covalent radius decreases down the group from C to Pb in a regular manner.
(B) Electronegativity decreases from C to Pb down the group gradually.
(C) Maximum covalence of C is 4 whereas other elements can expand their covalence due to presence of d orbitals.
(D) Heavier elements do not form ppi-ppi bonds.
(E) Carbon can exhibit negative oxidation states.
Choose the correct answer from the options given below:
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