Question

1. predict which bond is the most polar (has electrons that are pulled most strongly to one side of the bond): c—f, si—f, ge—f.

Explanation:

Step1: Recall Electronegativity Trend

Electronegativity decreases down a group. Carbon (C), Silicon (Si), Germanium (Ge) are in Group 14, with C at top, Si below, Ge below Si. Fluorine (F) is highly electronegative.

Step2: Calculate Electronegativity Difference

Polarity depends on electronegativity difference (\(\Delta EN\)) between bonded atoms. \(\Delta EN = |EN_{F} - EN_{other}|\). As we go down Group 14 (C → Si → Ge), \(EN\) of the metal decreases. So \(EN_{C} > EN_{Si} > EN_{Ge}\). Thus, \(\Delta EN\) for Ge - F is largest (since \(EN_{Ge}\) is smallest, \(|EN_{F}-EN_{Ge}|\) is biggest), making Ge - F the most polar.

Answer:

Ge - F