Chemical Bonding 4

Chemical bonding in metals is

• the same as ionic bonding.

• the same as covalent bonding.

• a combination of ionic and covalent bonding.

• different from ionic or covalent bonding.

The valence electrons in a metallic bond

• move freely throughout the network of metal atoms.

• are held tightly by the most positively charged atom.

• are shared equally between two metal atoms.

• continuously move from one energy level to another.

Within a metal, the vacant orbitals in the atoms' outer energy levels

• repel valence electrons.

• attract other metal atoms.

Which of the following properties is not explained by metallic bonding?

• electrical conductivity

• thermal conductivity

• brittleness

• ductility

Which of the following is the result of visible light absorbed by a metal?

• Electrons move to higher energy levels and remain there.

• Light at a frequency similar to the absorbed frequency is emitted.

• Electrons fill the vacant orbitals.

• Light is given off as a line spectrum.

Metals are malleable because when struck, one plane of metal atoms

• can slide past another plane without breaking bonds.

• cannot easily move out of the way.

• moves in a way that maximizes the repulsive forces within the metal.

• bonds to the plane directly beneath it.

Which is a measure of metallic bond strength?

• electron affinity

• electronegativity

• specific heat capacity

• enthalpy of vaporization

In general, as you move from right to left across any row of the periodic table, the strength of a metallic bond

• increases.

• decreases.

• stays the same.

• shows no trend.

Which of these is responsible for the good electrical conductivity of metals?

• the arrangement of metal atoms in separate layers

• the high density of metals atoms in the crystal lattice

• the ability of electrons to move freely about the crystal structure

• the fact that metal atoms contain many orbitals separated by very small energy

The arrangement of valence electrons in a metallic bond is best described as

• fixed positions in a lattice.

• a sea of free-moving electrons.

• concentrated electron density around specific atoms.

• electron pairs existing in multiple bonds.