Unit 2: Describing Matter - Nomenclature & Formula Writing

Flashcards covering periodic table organization, group charges, phase changes, physical and chemical properties, bonding, nomenclature of ionic, covalent, acid, and hydrate compounds, and required polyatomic ions.

Alkali Metals

The elements located in Group 1 of the periodic table, possessing a common ion charge of $+1$.

Alkaline Metals

The elements located in Group 2 of the periodic table, possessing a common ion charge of $+2$.

Transition Metals

The elements located in Groups 3 through 12 of the periodic table.

Inner Transition Metals

The elements located in the two rows at the very bottom of the periodic table.

Halogens

The elements located in Group 17 of the periodic table, possessing a common ion charge of $-1$.

Noble Gases

The elements located in Group 18 of the periodic table, having a neutral charge of $0$.

Groups

The vertical columns on the periodic table.

Periods

The horizontal rows on the periodic table.

Transition Metal Charge Exceptions (Ag, Zn, Pb, Sn)

Specific metals that do not vary in the standard transition way: $\text{Ag}$ is always $+1$, $\text{Zn}$ is always $+2$, and $\text{Pb}$ and $\text{Sn}$ are always $+2$ or $+4$.

Solid

A phase of matter characterized by tightly packed molecules and little movement of atoms.

Liquid

A phase of matter characterized by less tightly packed molecules and some movement of atoms.

Gas

A phase of matter characterized by molecules that are not tightly packed and display free movement of atoms.

Melting

The phase change from solid to liquid.

Sublimation

The phase change directly from solid to gas (e.g., dry ice).

Freezing

The phase change from liquid to solid.

Vaporization

The phase change from liquid to gas.

Condensation

The phase change from gas to liquid.

Deposition

The phase change directly from gas to solid (e.g., formation of frost).

Physical Properties

Characteristics of matter that you can see and observe directly.

Chemical Properties

Characteristics of matter that can only be seen or observed chemically.

Physical Change

A change in the form, shape, and/or phase of matter without altering the chemical composition.

Chemical Change

A change in chemical composition involving the altering of atomic and molecular positions within the substance.

Metals

Elements that are lustrous, malleable, ductile, good conductors of heat and electricity, and have high melting points.

Nonmetals

Elements that are dull, brittle, poor conductors of heat and electricity, and have lower melting points.

Metalloids

Elements that have a mix of metal and nonmetal properties.

Ionic Compounds

Compounds formed between a metal and a nonmetal via electron transfer; they exhibit no solid conductivity, are brittle, and have aqueous solubility and aqueous conductivity.

Covalent Compounds

Compounds formed between nonmetals via electron sharing; they exhibit no solid conductivity, are brittle, have aqueous solubility, and have no aqueous conductivity.

Covalent Prefixes

Prefixes used in molecular naming: mono- ($1$), di- ($2$), tri- ($3$), tetra- ($4$), penta- ($5$), hexa- ($6$), hepta- ($7$), octa- ($8$), nona- ($9$), and deca- ($10$).

Acid Naming: -ite Ending

An acid derived from an anion ending in '-ite' is named as '(stem)ous acid' (e.g., nitrite becomes nitrous acid, $\text{HNO}_2$).

Acid Naming: -ate Ending

An acid derived from an anion ending in '-ate' is named as '(stem)ic acid' (e.g., acetate becomes acetic acid, $\text{C}_2\text{H}_4\text{O}_2$).

Acid Naming: -ide Ending

An acid derived from an anion ending in '-ide' is named as 'hydro(stem)ic acid'.

Hydrate

A compound containing water molecules, named as Compound/Element + (prefix)hydrate (e.g., $\text{CuSO}_4 \cdot 5\text{H}_2\text{O}$, copper(II) sulfate pentahydrate).

Ammonium

A polyatomic cation with the formula $\text{NH}_4^{+1}$.

Acetate

A polyatomic anion with the formula $\text{C}_2\text{H}_3\text{O}_2^{-1}$.

Bicarbonate

A polyatomic anion with the formula $\text{HCO}_3^{-1}$.

Chlorate

A polyatomic anion with the formula $\text{ClO}_3^{-1}$.

Hydroxide

A polyatomic anion with the formula $\text{OH}^{-1}$.

Nitrate

A polyatomic anion with the formula $\text{NO}_3^{-1}$.

Nitrite

A polyatomic anion with the formula $\text{NO}_2^{-1}$.

Perchlorate

A polyatomic anion with the formula $\text{ClO}_4^{-1}$.

Permanganate

A polyatomic anion with the formula $\text{MnO}_4^{-1}$.

Cyanide

A polyatomic anion with the formula $\text{CN}^{-1}$.

Carbonate

A polyatomic anion with the formula $\text{CO}_3^{-2}$.

Chromate

A polyatomic anion with the formula $\text{CrO}_4^{-2}$.

Dichromate

A polyatomic anion with the formula $\text{Cr}_2\text{O}_7^{-2}$.

Oxalate

A polyatomic anion with the formula $\text{C}_2\text{O}_4^{-2}$.

Sulfate

A polyatomic anion with the formula $\text{SO}_4^{-2}$.

Sulfite

A polyatomic anion with the formula $\text{SO}_3^{-2}$.

Phosphate

A polyatomic anion with the formula $\text{PO}_4^{-3}$.

Arsenate

A polyatomic anion with the formula $\text{AsO}_4^{-3}$.

Law of Multiples

The principle stating that the same two elements can be used to make different compounds with whole-number ratios (e.g., hydrogen and oxygen forming both $\text{H}_2\text{O}$ and $\text{H}_2\text{O}_2$).

Law of Definite Proportions

The principle that a given chemical compound will always contain elements in the exact same whole-number ratio regardless of source (e.g., both Fiji Water and Poland Springs contain $\text{H}_2\text{O}$ with two hydrogens to one oxygen).