Question

the elements c and se have the same electronegativity value, 2.55. which of the following claims about the compound that forms from c and se is most likely to be true?
a the carbon - to - selenium bond is unstable.
b the carbon - to - selenium bond is nonpolar covalent.
c the compound has the empirical formula cse.
d a molecule of the compound will have a partial negative charge on the carbon atom.

Explanation:

• Option A: Since carbon (C) and selenium (Se) have the same electronegativity (2.55), the carbon - selenium bond is non - polar covalent. Non - polar covalent bonds are stable as there is equal sharing of electrons. So, the claim that the bond is unstable is incorrect.
• Option B: When two atoms have the same electronegativity, the electrons in the covalent bond are shared equally. This results in a non - polar covalent bond. Since \( \text{EN}(C)=\text{EN}(Se) = 2.55\), the \(C - Se\) bond is non - polar covalent.
• Option C: The empirical formula is the simplest whole - number ratio of atoms in a compound. For a compound formed by \(C\) and \(Se\), if it is \(CSe\), we need to check if there are simpler ratios. But in reality, based on bonding (each \(C\) has 4 valence electrons and each \(Se\) has 6 valence electrons), the formula is more likely \(CSe_2\) (using the criss - cross method for valence electrons: \(C^{4+}\) and \(Se^{2 -}\)). So, the claim of empirical formula \(CSe\) is wrong.
• Option D: In a polar covalent bond (where \( \Delta\text{EN}

eq0\)), there is a partial negative charge (\(\delta-\)) on the more electronegative atom and a partial positive charge (\(\delta+\)) on the less electronegative atom. Since \( \Delta\text{EN}(C - Se)=0\), there are no partial charges on either \(C\) or \(Se\) atoms.

Answer:

B. The carbon - to - selenium bond is nonpolar covalent.