Definitions I NEED to know Flashcards
Relative isotopic mass
The mass of an isotope relative to 1/12 of the mass of a carbon-12 atom.
Relative atomic mass (Ar)
The weighted mean mass of an atom of an element relative to 1/12 of the mass of a carbon-12 atom.
Mole
The amount of substance containing as many particles as there are atoms in 12g of the carbon-12 isotope. This is 6.02 x 10^23 particles.
Molar Mass
The mass of one mole of a substance in grams.
Empirical formula
The simplest whole number ratio of atoms of each element in a compound.
Molecular formula
The actual number of atoms of each element in a molecule.
Percentage yield
The actual yield divided by the theoretical yield x100%
Atom economy
Measure of how well atoms have been utilised.
Sum of molar masses of desired products/ Sum of molar masses of all products x100%
Ionic bond
Strong electrostatic force of attraction between oppositely charged ions
Covalent bond
The strong electrostatic force of attraction between a shared pair of electrons and the nuclei of the bonded atoms
Polar covalent bond
A covalent bond where the bonded electron pair are not shared equally between bonded atoms.
Due to differences in electronegativity between bonded atoms.
Hydrogen bond
a strong dipole-dipole attraction between an electron-deficient hydrogen atom and a lone pair of electrons on a highly electronegative atom on a different molecule
Electronegativity
A measure of the ability of an atom to attract a shared pair of electrons in a covalent bond.
Ideal gas equation
pV = nRT
p = pressure *(Pa) V = volume (m³) n = moles of gas (mol) R = gas constant (8.314 JK-¹mol-¹) T = temperature (K)
Hydrogen ion
An ion with no electrons and 1 proton
