Unit 4 Chem

Ionic Compounds

Formed from the electrostatic attraction between ions, typically consisting of metals and nonmetals.

Naming Ionic Compounds

Name the metal (cation) first followed by the non-metal (anion) with the suffix -ide.

Covalent Compounds

Made from the sharing of electrons between nonmetals.

Prefixes for Covalent Compounds

Indicate the number of atoms: 1=mono, 2=di, 3=tri, 4=tetra, 5=penta, 6=hexa, 7=hepta, 8=octa, 9=nona, 10=deca.

Oxyacids

Formed from H + polyatomic ion; change suffix -ate to -ic and -ite to -ous.

Criss-Cross Method

Method to balance charges of cations and anions to write correct formula for ionic compounds.

VSEPR Theory

Predicts the geometry of molecules based on the repulsion between electron pairs in the valence shell of the central atom.

Electronegativity

The ability of an atom to attract electrons in a bond; determines bond type.

Hybridization

The mixing of atomic orbitals to form new hybrid orbitals that are degenerate.

Polyatomic Ions

Ions that consist of two or more atoms bonded together and carry a net charge.

Nitrate

NO3^-; commonly found in fertilizers and explosives.

Sulfate

SO4^2-; used in various industrial processes.

Phosphate

PO4^3-; essential for energy transfer in biological systems.

Hydroxide

OH^-1 ; important in acid-base chemistry.

-ate and -ite Suffixes

The suffix -ate denotes more atoms compared to the -ite form which has one less oxygen.

Per- and Hypo- Prefixes

Per-, indicates one more oxygen than -ate; hypo-, indicates one less oxygen than -ite.

Ammonium

NH4^+1 ; a positively charged polyatomic ion commonly found in fertilizers.

Sulfite

SO3^-2; a polyatomic ion containing sulfur and oxygen, with one less oxygen than sulfate.

Nitrite

NO2^-1; a polyatomic ion containing nitrogen and oxygen, with one less oxygen than nitrate.

Carbonate

CO3^-2; a polyatomic ion composed of carbon and oxygen, commonly found in rocks and minerals.