Chemistry: Bonding, Periodic Table, and Quantitative Calculations

Comprehensive vocabulary flashcards covering chemical bonding, periodic table organization, polyatomic ions, and key quantitative chemistry formulas and constants.

Relative Atomic Mass ($A_r$)

The weighted average mass of an atom of an element compared to carbon-12, calculated using isotopic abundances by the equation: $A_r = \frac{\sum (\text{mass} \times \text{abundance})}{100}$.

Groups (Periodic Table)

The vertical columns of elements in the periodic table, representing elements that share similar chemical properties and have the same number of electrons in their outer shell.

Periods (Periodic Table)

The horizontal rows in the periodic table, representing the number of electron shells an atom possesses.

Group 1 Metals

The reactive alkali metals situated in the first column of the periodic table that react readily with water.

Ionic Compound

A compound formed through the transfer of electrons from a metal to a non-metal, producing oppositely charged ions held together by electrostatic attraction (e.g., $Li^+$ and $Cl^-$, or $Na^+$ and $Cl^-$).

Covalent Bonding

A type of chemical bonding that occurs when non-metal atoms achieve stable electron shells by sharing pairs of electrons, as exemplified by water ($H_2O$).

Ammonium Ion

A positively charged polyatomic cation with the formula $NH_4^+$.

Hydroxide Ion

A negatively charged polyatomic anion with the formula $OH^-$.

Carbonate Ion

A divalent polyatomic anion with the formula $CO_3^{2-}$.

Nitrate Ion

A polyatomic anion with the formula $NO_3^-$.

Sulfate Ion

A divalent polyatomic anion with the formula $SO_4^{2-}$.

Phosphate Ion

A trivalent polyatomic anion with the formula $PO_4^{3-}$.

Bicarbonate Ion

A polyatomic anion with the formula $HCO_3^-$.

Relative Molecular Mass ($M_r$)

The sum of the relative atomic masses ($A_r$) of all atoms present in a molecular formula (for example, for $NH_3$: $M_r = (1 \times 14) + (3 \times 1) = 17$).

Avogadro's Constant

The number of representative particles (atoms or molecules) contained in exactly one mole of any substance, defined as $6.02 \times 10^{23}$.

Mole Calculation Formula

The fundamental stoichiometric equation used to determine the quantity in moles of a chemical substance: $\text{Moles} = \frac{\text{Mass}}{M_r}$.

Molar Gas Volume at Room Temperature

The volume occupied by one mole of any gas at standard room temperature and pressure, equal to $24\,dm^3$.

Cubic Decimeter Conversion

The volume equivalence between cubic centimeters and cubic decimeters: $1000\,cm^3 = 1\,dm^3$.

Concentration Formula

The measure of the mass of solute dissolved per unit volume of solution, defined as $C = \frac{\text{Mass}}{\text{Volume}}$ with units of $g\,dm^{-3}$.