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Math  /  Data & Statistics

QuestionClassify each bond as nonpolar covalent, polar covalent, or ionic. \begin{tabular}{|cc} \hline Atom & Electronegativity \\ \hline C & 2.5 \\ S & 2.5 \\ I & 2.5 \\ Cl & 3.0 \\ Se & 2.4 \\ \hline \end{tabular}
Clear A
C-Se S−Cl\mathrm{S}-\mathrm{Cl} ionic C-I

Studdy Solution

STEP 1

1. Electronegativity differences determine bond types.
2. Nonpolar covalent bonds have an electronegativity difference of 0 to 0.4.
3. Polar covalent bonds have an electronegativity difference of 0.5 to 1.7.
4. Ionic bonds have an electronegativity difference greater than 1.7.

STEP 2

1. Calculate the electronegativity difference for each bond.
2. Classify each bond based on the electronegativity difference.

STEP 3

Calculate the electronegativity difference for C-Se:
∣2.5−2.4∣=0.1 |2.5 - 2.4| = 0.1

STEP 4

Calculate the electronegativity difference for S-Cl:
∣2.5−3.0∣=0.5 |2.5 - 3.0| = 0.5

STEP 5

Calculate the electronegativity difference for C-I:
∣2.5−2.5∣=0 |2.5 - 2.5| = 0

STEP 6

Classify C-Se bond:
Since the electronegativity difference is 0.10.1, it is a nonpolar covalent bond.

STEP 7

Classify S-Cl bond:
Since the electronegativity difference is 0.50.5, it is a polar covalent bond.

STEP 8

Classify C-I bond:
Since the electronegativity difference is 00, it is a nonpolar covalent bond.
The classifications are: - C-Se: Nonpolar Covalent - S-Cl: Polar Covalent - C-I: Nonpolar Covalent

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