Introduction to Bonding

Ionic bonds form as a result of the electrostatic attraction between

• dipoles.

• electrons.

• ions.

• nuclei.

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A single covalent bond involves the sharing of

• only one electron.

• two electrons.

• three electrons.

• a variable number of electrons, which depends on the bonding atoms.

The measure of an atom’s ability to attract electrons is its

• electronegativity

• polarization.

• ionization

• electron affinity

Atoms that are bonded with an electronegativity difference of 0 to 0.3 are generally considered to be

• negatively charged compounds.

• nonpolar-covalent compounds.

• polar-covalent compounds.

• ionic compounds.

What is the apparent charge on the chlorine atom in the molecule HCl?

• +1

• -1

• δ+

• δ-

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Atoms seldom exist as independent particles in nature because

• as single particles, most atoms have low potential energy.

• their electronegativity is much lower when they combine with other atoms.

• atoms are more stable when they combine with other atoms.

• neutral particles are rare.

When an atom completely gives up its valence electrons to another atom, they form a bond that is considered to be

• purely ionic.

• partially ionic.

• polar-covalent.

• nonpolar-covalent.

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You can estimate the degree to which a bond between two atoms is ionic or covalent by calculating the

• distance between the atoms’ nuclei.

• difference in the atoms’ electronegativities.

• atoms’ atomic radii.

• number of atoms in the compound.

Use the table below to choose the pair of elements that will most likely have the least ionic character

• Na and Cl

• O and Cl

• H and O

• Na and O

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Use the table below to choose the pair of elements that will most likely have the greatest ionic character.

• K and N

• K and S

• N and Br

• S and Br

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