Metallic Bonding Review

In metallic bonding, what are the electrons described as being?

• Transferred completely from one atom to another

• Shared equally between atoms

• Delocalized or free to move

• Paired in a hydrogen bond

What type of bond is formed from cations trapped in a sea of mobile ions?

• Metallic Bond

• Nonpolar Covalent Bond

• Ionic Bond

• Polar Covalent Bond

In metallic bonding, the strength of the bond is primarily determined by:

• The size of the metal ions.

• The charge of the metal ions.

• The number of delocalized electrons.

• The electronegativity of the metal atoms.

This type of bonding is characterized by the term "sea of electrons"

• Ionic

• Covalent

• Metallic

• Treasury

In metallic bonding, what is the role of delocalized electrons?

• They form covalent bonds between atoms

• They create a rigid lattice structure

• They allow metals to conduct electricity

• They prevent metals from reacting with acids

Which property of metals is explained by metallic bonding?

• Brittleness

• High melting point

• Poor electrical conductivity

• Transparency

What happens to the electrons in a metallic bond?

• They are shared between two specific atoms

• They are transferred to non-metal atoms

• They are free to move throughout the metal

• They are confined to a single atom

Tags

NGSS.HS-PS2-5

How does metallic bonding contribute to the malleability of metals?

• By forming strong ionic bonds

• By allowing layers of atoms to slide over each other

• By creating directional covalent bonds

• By trapping electrons in fixed positions

Which of the following is a characteristic feature of metallic bonding?

• Localized electron pairs

• Directional bonding

• Sea of delocalized electrons

• Weak van der Waals forces

Why are metals typically good conductors of heat?

• Because of their high density

• Due to the presence of free electrons

• Because they have a crystalline structure

• Due to strong covalent bonds