Metallic Bonding

Metallic bonding occurs between atoms of

• Sulfur

• Copper

• Fluorine

• Carbon

Which of the following best describes metallic bonding?

• Some metal atoms gain electrons while others lose electrons

• Valence electrons become delocalized and can move freely between cations

• Metal ions form permanent bonds by sharing electrons to obey the octet rule

• Metal atoms use their positive charge to gain additional electrons until every atom has eight valence electrons

Why are metals malleable?

Which of the following explains why metals are malleable?

• Their high melting points allow them to be flexible

• Metal cations reposition themselves until they can find 8 valence electrons

• Mobile electrons allow for cations to move when struck and take on a new form

• Mobile electrons provide smooth surfaces which are easy to reshape

The ability to conduct electricity in the solid state is a characteristic of metallic bonding. This characteristic is best described by the presence of

• High ionization energies

• High electronegativity

• Mobile electrons

• Mobile protons

What type of bonding do metals have?

Do metals have a regular or irregular structure?

What is the main purpose of alloying metals?

What happens to valence (outer) electrons in a metal?

What forces of attraction hold metal atoms together?