Definitions Flashcards
Covalent bond
The electrostatic attraction between a shared pair of electrons and the nucleus
Melting point
The temperature at which a solid changes to a liquid
define Oxidation number/ State
The hypothetical charge on an atom assuming that the bonding is ionic
Oxidation in terms of electrons
loss of electrons
Oxidation number
increase in oxidation number
Periodicity
the repeated pattern/trend in properties down or across the periodic table
Mass no. as a letter
A
Atomic no. as a letter
Z
Nucleons
particles within the nucleus (protons + neutrons)
5 stages of mass spectrometry
1) ionisation
2) acceleration
3) ion drift
4) detection
5) analysis
define isoelectronic
same electron configuration but different element
define the first ionisation energy
The energy needed to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions
the second ionisation energy
The energy required to remove 1 electron from 1 mole of 1+ gaseous ions, to form 1 mole of gaseous 2+ ions
ionic bonding
electrostatic attraction between positive and negative ions
metallic bonding
electrostatic attraction between positive ions and delocalised electrons in a layered structure
lattice
regular repeating patteren
symbol for carbonate
CO3 2-
symbol for sulfate
SO4 2-
symbol for nitrate
NO3 -
symbol for hydroxide
OH -
symbol for ammonia
NH3
symbol for ammonium
NH4 +
Coordinate bond (dative bond)
it is formed when one atom donates a shared pair of electrons to another atom/ion
Electronegativity
it is the power of an atom to attract electrons to itself in a covalent bond
permanent dipole
an unequal sharing of electrons in a covalent bond leading to δ+ and δ- ends
How do van der Waal forces form
Random electron movement in the first molecule induces a temporary dipole in another molecule which creates an attraction of δ+ and δ- in different/adjacent molecules
