Using the given table of electronegativity values, determine whether each bond is nonpolar covalent, polar covalent, or ionic.

Table:

1st column: Element (F, O, Cl, Br, I, S)

2nd Column: Electronegativity (4.0, 3.5, 3.0, 2.9, 2.7, 2.6)

3rd Column: Element (C, Se, H, Al, Na, K)

4th Column: Electronegativity (2.5, 2.5, 2.1, 1.6, 0.9, 0.8)

Drag the appropriate items to their respective bins.

(a. Bond between C and H b. bond between K and Cl c. bond between Na and O d. bond between Br and Br d. bond between C and F e. bond between Na and F f. bond between H and F g. bond between F and F h. bond between Al and Cl i. bond between Br and F)

Nonpolar covalent, Polar covalent, Ionic

Electronegativity (χ) is a property that describes the tendency of an atom to attract a shared pair of electrons. Atoms with higher electronegativity attracts more electrons towards it, electrons are closer to that atom.

When the electronegativity difference is greater, the bond polarity is increasing.

Δχ (C-H) = 2.5 - 2.1 = 0.4; nonpolar covalent.

Δχ (K-Cl) = 3.0 - 0.8 = 2.2; ionic bond.

Δχ (Na-O) = 3.5 - 0.9 = 2.6; ionic bond.

Δχ (Br-Br) = 2.9 - 2.9 = 0; nonpolar covalent.

Δχ (C-F) = 4 - 2.5 = 1.5; polar covalent.

Δχ (Na-F) = 4 - 0.9 = 3.1; ionic bond.

Δχ (H-F) = 4 - 2.1 = 1.9; polar covalent.

Δχ (F-F) = 4 - 4 = 0; nonpolar covalent.

Δχ (Al-Cl) = 3 - 1.6 = 1.4; polar covalent.

Δχ (Br-F) = 4 - 2.9 = 1.1; polar covalent.