metallic and ionic bonding

Metallic bonding occurs between __ of metallic elements.

atoms

In metallic bonding, valence electrons move freely throughout the structure, creating a __.

sea of delocalized electrons

Metal atoms lose their outer electrons and form __.

positive metal ions (cations)

The delocalized electrons in metallic bonding are held together by __ attraction.

electrostatic

High electrical conductivity in metals is due to __ moving easily and carrying charge.

free electrons

Delocalized electrons in metals can transfer __ energy quickly.

kinetic

One of the properties of metallic bonding allowing layers of atoms to slide over each other is __.

malleability

The strong electrostatic forces in metallic bonding lead to __ melting and boiling points.

high

Copper is an example of a metal that serves as an excellent __ due to freely moving electrons.

conductor

Ionic bonding is the electrostatic attraction between __ charged ions.

oppositely

Ionic bonding typically occurs between a __ that loses electrons and a nonmetal that gains electrons.

metal

When a metal atom donates electrons to a nonmetal atom, it forms a __ from the metal.

positive ion (cation)

The nonmetal atom gains electrons and forms a __.

negative ion (anion)

Ionic compounds typically have a __ structure, maximizing attraction and minimizing repulsion.

crystalline

Ionic compounds have high melting and boiling points due to strong __ forces.

ionic

Most ionic compounds __ in water, such as sodium chloride (NaCl).

dissolve

In solid form, ionic compounds are __ conductors because ions are fixed.

poor

Ionic compounds become good conductors when in __ or dissolved state.

molten

If the ionic lattice is disturbed, it can become __ due to like charges being forced together.

brittle

An example of an ionic compound is __, which forms a cubic lattice of Na⁺ and Cl⁻ ions.

sodium chloride (NaCl)