Ionic bonding is formed when one atom donates electrons to another, resulting in the formation of positively and negatively charged ions.

Covalent bonding involves the sharing of electrons between atoms, resulting in a strong attraction between them.

Metallic bonding is formed between metal atoms, where the valence electrons are delocalized and can move freely throughout the metal lattice.

The strength of an ionic bond is influenced by the size, charge, and distance between the ions.

H₂O is held together by covalent bonds between hydrogen and oxygen atoms.

Na has a metallic bond, where the valence electrons are delocalized and can move freely throughout the metal lattice.

The bond between hydrogen and oxygen in water is a covalent bond, where the electrons are shared between the atoms.

HCl has a polar covalent bond due to the difference in electronegativity between hydrogen and chlorine.

Non-metal atoms typically form covalent bonds by sharing electrons.

CH₄ has a nonpolar covalent bond due to the equal sharing of electrons between carbon and hydrogen atoms.

When a metal and a non-metal react, they typically form an ionic bond, where the metal loses electrons to the non-metal.

NaCl has an ionic bond between sodium and chlorine, where sodium donates an electron to chlorine.

Metal atoms typically form metallic bonds, where the valence electrons are delocalized and can move freely throughout the metal lattice.

Fe has a metallic bond, where the valence electrons are delocalized and can move freely throughout the metal lattice.

Hydrogen atoms typically form covalent bonds with non-metal atoms by sharing electrons.