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21 Cards in this Set

  • Front
  • Back

Element

Substance made up of only one kind of atom and cant be broken down further into a simpler substance by chemical means

Atom

Smallest particle of an element that can take part in a chemical reaction

Mixture

Substances made up of two or more elements not chemically combined

Compound

Substance made up of two or more elements that are chemically combined

Isotope

Atom of the same element with the same number of protons and electrons but different number of neutrons

Relative Atomic Mass

The weighted average mass of all natural known isotopes of an element compared with C12 where one atom C12 has a mass up exactly 12 units

Relative Isotopic Mass

The mass of a particular isotope of an element compared with C12 where one atom of C12 has a mass of exactly 12 units

Rlative Molecular Mass

Weighted average mass of 1 molecule of a compound compared with C12 where one atom of C12 has a mass of exactly 12 units

Relative Formula Mass

The weighted average mass of the formula of a compound compared with C12 where 1 atom of C12 has a mass of exactly 12 units

The Mole

Amount of substance in grams which has the same number of particles as there are in 12 grams of Carbon

Avagadro's Constant

Number of atoms, ions, molecules or electrons in a mole = 6.023x10^23 (atoms)

Mass and Moles Formula

Moles = Mass of substance (g) / Molecular mass (Mr)

Dm^3 to cm^3

1 dm^3 = 1000 cm^3

Gas and Moles

Moles = Volume of gas (dm^3) / Molar mass (24)

Concentration (g/dm^3)

Concentration = Mass (g) / Volume (dm^3)

Concentration (mol/dm^3)

Concentration = moles / Volume (dm^3)

Percentage Yield (%)

Percentage yeild = [ Amount you make (measured) / Maximum amount (calculated) ] x100

Ar From a Mass Spectra Diagram

Ar = mass x relative abundance / 100

Empirical Formula

Simplest whole number ratio of the elements present in 1 molecule of a compound

Molecular Formula Def.

Total number of atoms present in each element in a molecule

Molecular Formula

Molecular formula = n(Empirical Formula)



n = molecular mass (given) / molecular mass of Empirical formula