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Formula Sheets / Chemistry

Chapter 1

Some Basic Concepts of Chemistry

Revise with flashcards Download this chapter (PDF) All Chemistry formulas (PDF)

Mole concept Concentration terms Empirical formula and stoichiometry Laws of chemical combination

Mole concept

$n = \frac{mass}{M} = \frac{N}{N _{A}} = \frac{V _{gas}}{22.4 L}$ (at STP) $,$ $N_{A} = 6.022 \times 1 0^{23}$
Average atomic mass
$\overset{ˉ}{A} = \frac{\sum ( % abundance \times mass )}{100}$

Concentration terms

$M = \frac{n _{solute}}{V _{soln} ( L )},$ $m = \frac{n _{solute}}{kg solvent},$ $N = M \times n$ -factor
Mole fraction
$x_{A} = \frac{n _{A}}{n _{A} + n _{B}},$ $x_{A} + x_{B} = 1$
Molarity from % (w/w)
$M = \frac{10 \times d \times % w}{M _{solute}}$
Dilution / mixing
$M_{1} V_{1} = M_{2} V_{2};$ $M_{mix} = \frac{M _{1} V _{1} + M _{2} V _{2}}{V _{1} + V _{2}}$

Empirical formula and stoichiometry

Molecular formula
molecular formula $= n \times$ empirical formula $,$ $n = \frac{molar mass}{empirical formula mass}$
Limiting reagent
the reactant with the smallest $\frac{moles}{coefficient}$
Equivalents
equivalents $= n \times n$ -factor $;$ equivalents of A $=$ equivalents of Bin a reaction

Laws of chemical combination

conservation of mass; definite proportions; multiple proportions; Gay-Lussac's gaseous volumes; Avogadro's law

Structure of Atom