General Chemistry I Study Guide Flashcards

Vocabulary practice flashcards covering essential concepts, formulas, subatomic particles, and chemical nomenclature from General Chemistry I Test #1 Study Guide.

Extensive property

A physical property that depends on the amount of matter present, such as mass, volume, or length.

Intensive property

A physical property that does not depend on the amount of matter present, such as density, melting point, boiling point, or color.

Isotopes

Atoms of the same element that have the same number of protons but a different number of neutrons, resulting in different mass numbers.

Ions

Atoms of the same element that have the same number of protons but a different number of electrons, resulting in an electric charge.

Transition metals

Elements located in groups 3–12 of the periodic table.

Halogens

Elements located in group 17 of the periodic table, including F, Cl, Br, I, and At.

Electrolyte

Any compound that dissociates into ions when dissolved in water, including ionic compounds, acids, and bases.

Non-electrolyte

A molecular or covalent compound that stays intact when dissolved in water rather than dissociating into ions.

Oxyanion naming "hypo- -ite"

The naming prefix/suffix combination indicating an oxyanion with the least oxygen level (for example, hypochlorite, $\text{ClO}^-$).

Oxyanion suffix "-ite"

The naming suffix indicating an oxyanion with one less oxygen atom than the standard "-ate" anion (for example, nitrite, $\text{NO}_2^-$).

Oxyanion suffix "-ate"

The naming suffix indicating the "standard" oxygen level for an oxyanion (for example, nitrate, $\text{NO}_3^-$).

Oxyanion naming "per- -ate"

The naming prefix/suffix combination indicating an oxyanion with the most oxygen level (for example, perchlorate, $\text{ClO}_4^-$).

Oxyanion acid naming rule

Rule stating that oxyanions ending in "-ite" become "-ous acid", and oxyanions ending in "-ate" become "-ic acid".

Vanadium

Chemical element represented by the symbol $\text{V}$.

Silicon

Chemical element represented by the symbol $\text{Si}$ (distinct from sulfur, which is $\text{S}$).

Nickel

Chemical element represented by the symbol $\text{Ni}$.

Density to moles to atoms calculation chain

A 3-step calculation method: 1. $\text{Volume} \times \text{Density} = \text{Mass}$; 2. $\text{Mass} \div \text{Molar Mass} = \text{Moles}$; 3. $\text{Moles} \times \text{Avogadro's Number } (6.022 \times 10^{23}) = \text{Atoms}$.

Fahrenheit to Celsius formula

\text{^\circ C} = (\text{^\circ F} - 32) \times \frac{5}{9}

Celsius to Kelvin formula

\text{K} = \text{^\circ C} + 273.15

Subatomic particle rules for neutral atoms

$\text{protons} = \text{atomic number } (Z)$; $\text{neutrons} = \text{mass number } (A) - \text{atomic number } (Z)$; $\text{electrons} = \text{atomic number } (Z)$.

Lead-207 subatomic composition

An isotope with symbol $^{207}\text{Pb}$ ($Z = 82$) containing $82$ protons, $82$ electrons, and $125$ neutrons ($207 - 82 = 125$).

Zinc-68 subatomic composition

An isotope with symbol $^{68}\text{Zn}$ ($Z = 30$) containing $30$ protons, $30$ electrons, and $38$ neutrons ($68 - 30 = 38$).

Iodine-123 subatomic composition

An isotope with symbol $^{123}\text{I}$ ($Z = 53$) containing $53$ protons, $53$ electrons, and $70$ neutrons ($123 - 53 = 70$).

Hydroiodic acid

A binary acid with formula $\text{HI}(aq)$, named using the rule: hydro- + root + -ic acid.

Mercury(II) sulfide

An ionic compound with formula $\text{HgS}$, where $\text{Hg}^{2+}$ is balanced by $\text{S}^{2-}$ and named using a Roman numeral.

Sodium nitride

A binary ionic compound with formula $\text{Na}_3\text{N}$, requiring no numerical prefixes in its name.

Iron(III) carbonate

An ionic compound with formula $\text{Fe}_2(\text{CO}_3)_3$, where two $\text{Fe}^{3+}$ cations balance three $\text{CO}_3^{2-}$ anions.

Tetraselenium dinitride

A covalent compound composed of two nonmetals with formula $\text{Se}_4\text{N}_2$, named using Greek prefixes.

Strontium thiosulfate

An ionic compound with formula $\text{SrS}_2\text{O}_3$, containing the $\text{S}_2\text{O}_3^{2-}$ thiosulfate ion.

Aluminum permanganate

An ionic compound with formula $\text{Al}(\text{MnO}_4)_3$, formed from $\text{Al}^{3+}$ and three $\text{MnO}_4^-$ ions.

Sulfur hexafluoride

A covalent compound with formula $\text{SF}_6$, where the prefix "hexa-" indicates 6 fluorine atoms.

Copper(II) hydrogen sulfate

An ionic compound with formula $\text{Cu}(\text{HSO}_4)_2$, formed from $\text{Cu}^{2+}$ and two $\text{HSO}_4^-$ ions.

Cobalt(II) oxide

An ionic compound with formula $\text{CoO}$, composed of $\text{Co}^{2+}$ and $\text{O}^{2-}$ ions.

Beryllium chlorite

An ionic compound with formula $\text{Be}(\text{ClO}_2)_2$, composed of $\text{Be}^{2+}$ and two $\text{ClO}_2^-$ ions.

Nickel(II) nitrate

An ionic compound with formula $\text{Ni}(\text{NO}_3)_2$, composed of $\text{Ni}^{2+}$ and two $\text{NO}_3^-$ ions.

Hydrogen peroxide

A compound with formula $\text{H}_2\text{O}_2$, memorized as an exception to standard naming rules.

Permanganate

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

Sulfate

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

Nitrate

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

Nitrite

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

Carbonate

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

Phosphate

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

Hydrogen sulfate

A polyatomic ion with the formula $\text{HSO}_4^-$.

Thiosulfate

A polyatomic ion with the formula $\text{S}_2\text{O}_3^{2-}$.

Chlorite

A polyatomic ion with the formula $\text{ClO}_2^-$.

Chlorate

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

Hydroxide

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

Peroxide ion

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

Greek prefixes for covalent naming

Prefixes used to designate atom counts in covalent compounds: mono- (1), di- (2), tri- (3), tetra- (4), penta- (5), hexa- (6), hepta- (7), octa- (8), nona- (9), deca- (10).