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Mass number (A)
the total number of protons and neutrons in an atom
Atomic number (Z)
the number of protons in an atom
Isotope
Atoms of the same element with different mass numbers / atoms of the same element with the same atomic number but different mass numbers
Ion
A species in which there is a surplus or lack of electrons
First ionisation energy
The amount of energy required to remove the outer most electron from a gaseous atom in its ground sate
Ionic bond
A transfer of electrons and subsequent electrostatic attraction
Covalent bond
The sharing of at least one pair of electrons between two atoms
Electronegativity
a measure of the tendency of an atom to attract a bonding pair of electrons
non polar covalent bond
An equal sharing of electrons
polar covalent bond
unequal sharing of electrons leading to a dipole forming (as a result of electronegativity difference)
Intermolecular forces
The weak force of attraction between molecules, ions or atoms in noble gases
intramolecular bonds
A bond which occurs between atoms within a molecule
Giant covalent substance
A substance which contains a large network of covalent bonds
Allotrope
different structural forms of the same element
Metallic bond
A bond between a positive kernel and a sea of delocalised electrons
Mole
The amount of any substance that contains the same number of elementary particles as 12g of Carbon-12
Relative atomic mass (Aᵣ)
The average mass of one atom of an element relative to Carbon-12, which has mass exactly 12
Relative molecular mass (Mᵣ)
The average mass of one molecule relative to Carbon-12, which has mass exactly 12
Law of conservation of matter
Matter cannot be created or destroyed, only transferred from one place to another
Molar mass (M)
The mass in grams of one mole of that substance
Empirical formula
The formula that shows the simplest ratio of elements in the compound
Molecular formula
The formula that shows the actual ratio of elements in a compound
Standard solution
A solution of which the concentration is know exactly, and is unlikely to change for a period of time
Solution
A homogenous mixture of solute and solvent
Solute
The substance that is dissolved in the solution
Solvent
the substance in which another substance is dissolved, forming a solution
Concentration
The amount of solute per unit volume of solution
Atomic mass unit (amu)
one twelfth the mass of a carbon-12 atom
grams per mole (g/mol)
unit of molar mass
Molar volume of gas (Vₘ)
22.4 dm³
1dm³ = ____ m³ = ____ cm³ = ____mm³
0,001 AND 1000 AND 1 000 000
