Order of Covalent bond;A. KF>KI; LiF>KFB. KF<KI; LiF>KFC. SnCl4>SnCl2; CuCl>NaClD. LiF>KF; CuCl<NaClE. KF<KI; CuCl>NaClC, E OnlyB, C OnlyB, C, E OnlyA, B Only

To determine the order of covalent bonds from the given options, we need to analyze the factors that affect bond strength, including ionic and covalent character, ion size, and electronegativity differences.

Break Down the Problem

1. Identify the order of bond strength for each comparison given in the options.
2. Analyze the ionic and covalent characteristics of each compound.

Relevant Concepts

1. Ionic vs. Covalent Character: The greater the difference in electronegativity between two atoms, the more ionic the bond is likely to be.
2. Ionic Radius: Larger ionic radii generally lead to weaker ionic bonds.
3. Covalent Character: Smaller cations and highly electronegative anions typically lead to stronger covalent bonds.

Analysis and Detail

1. Comparison A: KF > KI, LiF > KF

   • KF is stronger than KI because fluoride is smaller and more electronegative than iodide, leading to stronger ionic bonds.
   • LiF is stronger than KF because Li is a smaller cation than K.

2. Comparison B: KF < KI, LiF > KF

   • This contradicts established trends. Therefore, this comparison is incorrect.

3. Comparison C: SnCl4 > SnCl2, CuCl > NaCl

   • SnCl4 is stronger than SnCl2 due to the higher oxidation state leading to stronger covalent character.
   • CuCl is generally stronger than NaCl due to the smaller and more polarizable cation (Cu) compared to Na.

4. Comparison D: LiF > KF, CuCl < NaCl

   • This is consistent. LiF is stronger than KF.
   • However, CuCl being weaker than NaCl contradicts conventional wisdom since CuCl usually has a more covalent character.

5. Comparison E: KF < KI, CuCl > NaCl

   • Again, this contradicts as KF > KI based on size, and CuCl usually has a stronger bond than NaCl.

Verify and Summarize

Comparing the options based on the analysis:

• A and C are valid comparisons according to ionic and covalent character trends.
• B, D, and E contain contradictions based on expected ionic and covalent bond strengths.

Final Answer

Based on the analysis, the correct selections are: C, E Only (as B contains contradictions).