What is the relationship between electronegativity and bond type? put another way, how could you predict whether a compound would be ionic or covalent if given a list of the elements’ electronegativities?

The greater the difference in electronegativity (ΔEN) between two atoms, the greater the degree in ionic character in the bond.

If you have a bond between atoms A and B (A-B),

ΔEN = |EN_A - EN_B|

The rules for the type of bond are:

•If ΔEN < 0.5, the bond is nonpolar covalent

•If 0.5 ≤ΔEN < 1.7, the bond is polar covalent

•If ΔEN ≥ 1.7, the bond is ionic

Examples:

C-H: ΔEN = |2.55 – 2.20| = 0.35; nonpolar covalent

C-F: ΔEN = |2.55 – 3.98| = 1.43; polar covalent

Na-F: ΔEN = |0.93 – 3.98| = 3.05; ionic

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explanation:

the best answer is d because the strong cohesion is caused by the ability of water molecules to undergo hydrogen bonding.

a is incorrect because when water solidifies, it becomes   ice, which expands and occupies a bigger volume for the same mass of water in its liquid state.

b is incorrect because water has high surface tension. besides bonding to itself it hydrogen bonds to other molecules at the top decreasing possibility for breaking of attractive forces.

c is incorrect because the water molecule has oxygen which is highly electronegative and so pulls the electron pair towards itself creating a dipole moment, making the molecule polar.

e is incorrect because water has strong adhesion, ability to stick to other molecules such as glass because of this molecules having stronger hydrogen bonding than water.