Introduction to Chemical Bonding

Ionic bonds form as a result of the electrostatic attraction between

• dipoles.

• electrons.

• ions.

• nuclei.

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NGSS.HS-PS1-3

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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.

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

 

Element Electronegativity Element Electronegativity

Na 0.9 O 3.5

Cl 3.0 H 2.1

 

• Na and Cl

• O and Cl

• H and O

• Na and O

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

 

Element Electronegativity Element Electronegativity

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.

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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.