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.

metals are good conductor of electricity. it has free electrons on their surface. according to electron pool theory, each atom present in a metal crystal losses all of its valence electron and as a result a pool of free is form. these pool of electrons are free to move and   conduct electricity easily   while making metal as good conductor.

the correct answer is a. the ability of electrons to flow throughout the metal.

if it's not useful, feel free to report for mistake in answer.

you did not give any options thus this is the best answer i can give to you with this little information you have given

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