Bonding Review

A mutual electrical attraction between the nuclei and valence electrons of different atoms that binds the atoms together is called a(n):

• chemical bond.

• dipole.

• London force.

• Lewis structure.

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The electrons involved in the formation of a chemical bond are called:

• s electrons.

• valence electrons.

• dipoles.

• Lewis electrons.

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When atoms share electrons, the electrical attraction of an atom for the electrons is called the atom's

• electronegativity.

• electron affinity.

• hybridization.

• resonance.

If the atoms that share electrons have an unequal attraction for the electrons, the bond is called

• nonpolar.

• dipolar.

• polar.

• ionic.

A covalent bond results when (a)   are shared.

• electrons

• ions

• Lewis structures

• dipoles

Most chemical bonds are:

• purely covalent.

• partly ionic and partly covalent.

• metallic.

• purely ionic.

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Nonpolar covalent bonds are not common because:

• A) ions always form when atoms join.

• B) one atom usually attracts electrons more strongly than the other.

• C) dipoles are rare in nature.

• D) the electrons usually remain equally distant from both atoms.

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The greater the electronegativity difference between two bonded atoms, the greater the percentage of:

• covalent character

• ionic character

• electron sharing

• metallic character

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A bond that is less than 5% ionic is considered

• nonpolar covalent.

• ionic.

• metallic.

• polar covalent.

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The pair of elements that forms a bond with the least ionic character is

• Na and Cl.

• Br and Cl.

• H and Cl.

• O and Cl.

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