Unit 4: Concept 3 Metallic Bonds

Multiple Choice

Metals are strong absorbers and reflectors of light.When light is shone on to the surface of a metal, its electrons absorb small amounts of energy and become excited into one of its many empty orbitals. The electrons immediately fall back down to lower energy levels and emit light.

This process is responsible for which property of metals?

• conductivity

• malleability

• luster

• ductility

Multiple Choice

What is a metallic bond?

• The attraction between metal atoms in which a new compound is formed

• The attraction of stationary metal cations to mobile electrons

• The repulsion between metal ions within a pool of shared electrons

Multiple Choice

In metallic bonds, do metal atoms lose their valence electrons?

• No

• Yes

• Sometimes

Multiple Choice

Do metallic bonds result in the formation of compounds?

• No

• Yes

• Sometimes

Multiple Choice

What type of structures do metals like to form in metallic bonds?

• Lattice

• Ionic

• Compounds

Multiple Choice

How does the "Sea of Electrons" model explain the malleability of metals?

• Electrons are fixed, allowing layers to slide

• Electrons are localized, preventing layers from sliding

• Electrons are delocalized, allowing layers to slide

Multiple Choice

Melting point is the temperature at which a substance changes state from solid to liquid (melts).

Solubility is the ability of a substance to be dissolved in water.

Which of the following do you think is a result of the "Sea of Electrons" in metals?

• High melting point

• High solubility

• Low melting point

• low solubility

Multiple Select

Which types of energy can metals conduct?

• Electrical

• Nuclear

• Chemical

• Thermal

Multiple Choice

What is a key characteristic of a metallic bond?

• Valence electrons are transferred from one metal atom to another.

• Valence electrons are in a shared pool among all metal atoms.