Chemical Bonding Types and Naming Ionic Compounds

Three types of chemical bonding exist: ionic, covalent, and metallic.

Ionic, covalent, and metallic are the three main types of chemical bonding.

An ionic bond involves the transfer of valence electrons from one atom to another, creating oppositely charged ions that attract each other.

A covalent bond occurs when two atoms share valence electrons to achieve a stable electron configuration.

A metallic bond involves a 'sea' of delocalized valence electrons that flow freely among a lattice of positively charged metal ions.

A cation is a positively charged ion formed when an atom loses one or more electrons.

An anion is a negatively charged ion formed when an atom gains one or more electrons.

Alkali metals (Group 1), alkaline earth metals (Group 2), Aluminum (Group 13), Gallium (Group 13), and Indium (Group 13) tend to donate valence electrons in ionic bonding.

Halogens (Group 17) and Oxygen (Group 16) often receive valence electrons to complete their outer shell in ionic bonding.

Ionic bonds don't always follow a one-to-one ratio. The ratio depends on the charges of the ions involved to create a neutral compound.

To name an ionic compound, start with the cation (metal) name, followed by the anion (non-metal) name with the '-ide' ending.

The ionic formula for ammonium is [NH4]+. Ammonium is a positively charged polyatomic ion with a charge of +1.

The ionic formula for hydroxide is [OH]-. Hydroxide is a negatively charged polyatomic ion with a charge of -1.

The ionic formula for nitrate is [NO3]-. Nitrate is a negatively charged polyatomic ion with a charge of -1.

The ionic formula for sulfate is [SO4]2-. Sulfate is a negatively charged polyatomic ion with a charge of -2.

The ionic formula for carbonate is [CO3]2-. Carbonate is a negatively charged polyatomic ion with a charge of -2.

The ionic formula for phosphate is [PO4]3-. Phosphate is a negatively charged polyatomic ion with a charge of -3.

Transition metal ions are written with roman numerals indicating their charge. These numerals represent the number of valence electrons they tend to lose or gain.

Roman numerals are used to indicate the charge of transition metal ions. They replace the number of valence electrons lost or gained by the element.

An ionic bond is formed between a metal and a nonmetal.

A covalent bond is formed between two nonmetals or between a nonmetal and a metalloid.

The first rule is to write the name of the electronegative element first in a covalent compound name.

If a covalent compound contains more than one atom of a particular element, use a prefix (di, tri, tetra, etc.) before the element's name. If there's only one atom, you can skip the prefix.

The third rule is to always place the prefix before the name of the electronegative element.

The fourth rule is to change the ending of the second nonmetal element in a covalent compound name to '-ide'.

The prefix 'mono-' is used to indicate one atom of an element in a covalent compound.

The prefix 'di-' is used to indicate two atoms of an element in a covalent compound.

The prefix 'tri-' is used to indicate three atoms of an element in a covalent compound.

The prefix 'tetra-' is used to indicate four atoms of an element in a covalent compound.

The prefix 'penta-' is used to indicate five atoms of an element in a covalent compound.

The prefix 'hexa-' is used to indicate six atoms of an element in a covalent compound.

The prefix 'hepta-' is used to indicate seven atoms of an element in a covalent compound.

The prefix 'octa-' is used to indicate eight atoms of an element in a covalent compound.

The prefix 'nona-' is used to indicate nine atoms of an element in a covalent compound.

The prefix 'deca-' is used to indicate ten atoms of an element in a covalent compound.

Hydrogen (H) has zero dots and one line in its Lewis dot structure.

Carbon (C) has zero dots and four lines in its Lewis dot structure.

Nitrogen (N) has two dots and three lines in its Lewis dot structure.

Oxygen (O) has four dots and two lines in its Lewis dot structure.

Fluorine (F) has six dots and one line in its Lewis dot structure.

Neon (Ne) has eight dots and zero lines in its Lewis dot structure.

Ionic compounds are typically hard, brittle solids with high melting points and dissolve in water. Covalent compounds are often soft or hard, have lower melting points, and are less likely to dissolve in water.