deck_15796904 (1) Flashcards
Molecular Ion
2/more atoms covalently bonded with an overall charge
Avogadro’s Constant
Number of atoms in 12.000g of carbon-12
Mole
the amount of substance which contains the Avogadro constant of atoms, molecules or groups of ions
Molar Mass
The mass of one mole of a substance
Anhydrous (salt)
a salt which contains no water of cryst
Water of Crystallisation
Water chem bonded within a crystal
Atomic Number
the number of protons (in the nucleus of an atom)
Mass Number
The total number of protons and neutrons in the nucleus of an atom
RAM
The average (weighted mean) mass of an atom of an element relative to 1/12th of the mass of an atom of carbon-12
RIM
The mass of an atom of an isotope of an element relative to 1/12th of the mass of an atom of carbon-12
Isotopes
Atoms which have the same atomic number but a different mass number (contain the same number of protons but a different number of neutrons)
RFM
The average (weighted mean) mass of a formula unit relative to 1/12th mass of an atom of carbon-12
RMM
The average (weighted mean) mass of a molecule relative to 1/12th mass of an atom of carbon-12
First Ionisation En
The energy required to convert one mole of gaseous atoms into gaseous ions with a single positive charge
Second ionis En
the energy required to convert one mole of gaseous ions with a single positive charge with gaseous ions with a double positive charge
Third Ionis En
the energy req to convert one mole of gaseous ions with a double positive charge into gaseous ions with a triple positive charge
Covalent Bond
The electrostatic attraction between a shared pair of electrons and nuclei of bonded atoms
Co-ordinate Bond (Dative) bond
A shared pair of electrons between two atoms. One atom provides both electrons
Octet Rule
When reacting, an atom tends to gain, lose or share electrons to achieve 8 in its outer shell
EN
The extent to which an atom attracts the bonding electrons in a covalent bond
Polar Bond
a covalent bond in which there is unequal sharing of the bonding electrons
Delocalised Electrons
Outer electrons do not have fixed positions but move freely
Intermolecular
Between neighbouring molecules (as opposed to intramolecular)
vdwF
the attraction between instantaneous and induced dipoles on neighbouring molecules
