Atoms, Elements, Molecules, and Compounds

Naming convention: Prefix Element + Prefix Element + -ide

• Mono = 1
• Di = 2
• Tri = 3
• Tetra 4
• Penta = 5
• Sexta = 6
• Septa = 7
• Octa = 8
• Nona = 9
• Deca = 10

ex) Cobalt Tetrachloride (CCl4)

Indicates the last component of a molecular compound

Anions composed of oxygen and another element

• -ate
• An oxyanion in a series with more oxygen (ex: NO₃^- nitrate)

• -ite
• An oxyanion in a series with less oxygen (ex: NO₂^- nitrite)

• Hypo-
• The oxyanion with the least oxygen in a series of >2 members (ex: ClO^- hypochlorite)

• Per-
• The oxyanion with the most oxygen in a series of >2 members (ex: ClO₄^- perchlorate)

• (g) Gas
• (l) Liquid
• (s) Solid
• (aq) Aqueous

Reactants (state) -> Products (state)

Type One:

X - A

• Type Two:
• ^A
• X
• Z
• Z = Atomic #
• A = Atomic Mass (P + N)
• X = Chemical Symbol

• Name (if charge variant - roman numerals)
• ex 1: Iron (III) Hydroxide vs Iron (II) Hydroxide
• ex 2: Magnesium nitrate

• X^charge
• ex 1: Fe³⁺ , OH^- -> Fe(OH)₃
• ex 2: MG²⁺ , NO^3- ->Mg(NO₃)₂

Note: Superscripts show charge, subscripts show ions

1) Main group metals lose electrons, forming a cation with the same number of electrons as the nearest noble gas, with nearest signifying the number of electrons closest to that element.

2) Main group non-mentals gain electrons, forming an anion with the same number of electrons as the nearest noble gas.

• 1)
• ____ g x 1 mol/compound molar mass = molar mass (mols)

• 2)
• molar mass (mols) x ratio A/ratio B = _____ mols

• 3)
• ______ mols x N_A/1 mol = ions

g -> mol

____ mol x g/1 mol = ____ gram

• mol -> g
• ____ g x 1 mol/g = ____ mol

_____ g x 1 mol/molar mass (g) x Na/mol = atoms

______ mol x molar mass(g)/1 mol = grams

6.022 x 10²³

Note: This is equivalent to 12g ¹²₆ C

Molecular compounds that release hydrogen ions (H+) when dissolved in water as their bonds are sufficiently polar to cleave apart. They have a pH <7.

• Types
• Binary: Hydrogen + Nonmetal
• ex) HCl/Hydrochloric, HF/Hydrofluoric, HBr/Hydrobromic
• Oxyacids: Hydrogen + oxyanion/polyatomic ion
• ex) H₂SO₄/Sulfuric, HNO₃/Nitric, H₂PO₄/Phosphoric, H₂CO₃/Carbonic

Note: Not every hydrogen compound is acidic, an example being alcohols such as ethanol

Ions composed of 2 or more atoms. These bear a charge. ex) ClO^-

• Atomic Element: Exists in nature as single atoms i.e. they are not diatomic
• ex) Xenon
• Ionic Compound: Metal/Cation + Nonmetal/Anion OR Polyatomic Ion
• ex) NiCL₂, NaNO₃
• Molecular Element: Diatomic Molecules
• ex) Bromine
• Molecular Compound: Nonmetal/Anion + Nonmetal/Anion
• ex) NO₂

Ionic compounds that crystallize with a fixed amount of water in the spaces of their crystal matix.

• ex) CuSO₄ 5H₂O
• Copper (II) Sulfate Pentahydrate

Hydrogen ion (H+) receptors that release hydroxide (OH-) when dissolved in water. They have a pH >7.

ex) NaOH, KOH, NH₃ (ammonium), CO₃^-2 (carbonate), HCO₃^-(bicarbonate)

Note: Alcohols are not bases despite the OH group presence as they will not disassociate to OH^- ions.

• Ionic Compounds
• * Metal + Nonmetal
• * Any compound with a polyatomic ion
• * Conducts electricity (is an electrolyte) ie: Disassociates into ions in water
• * High melting points
• * Many are water soluble.
• * They are held together by electrostatic attraction between + and - ions (ionic bonds). This bond is very strong.

• Molecular Compounds
• * Nonmetal + Nonmetal OR Metalloid
• * Lower melting points as bonds between molecules are generally weak
• * The are insulators not electrolytes
• * Electrons are "tied up" in bonds or are in nonbonding pairs, so no conducting bonds exist
• * Some are water soluble
• * They are covalently bonded i.e they share electrons