6.1 Introduction to Chemical Bonding

Ionic bonds form as a result of the electrostatic attraction between

• dipoles

• electrons

• ions

• nuclei

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

Choose the pair of elements that will most likely have the least ionic character. Na=0.9, O=3.5, Cl=3.0, H=2.1

• Na and Cl

• O and Cl

• H and O

• Na and O

Choose the pair of elements that will most likely have the greatest ionic character.

K=0.8

N=3.0

Br=2.8

S=2.5

• K and N

• K and S

• N and Br

• S and Br

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-

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.

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.