Temporary CYCLE TEST preparations for Physical Science Flashcards
core electrons
Electrons in the energy levels below the outermost energy level.
covalent bond
Sharing of at least one pair of electrons by two non-metal atoms.
electron affinity
Electron affinity is the quantity of energy released when an electron is
added to an atom in the ground state.
electronegativity
A measure of the tendency of an atom to attract a bonding pair of
electrons.
ionic bond
A transfer of electrons and subsequent electrostatic attraction.
ionisation energy
The amount of energy required to remove one electron from an atom in
the gaseous phase.
isotopes
Atoms of the same element having the same atomic number
but different numbers of neutrons.
metallic bonding
Bonding between a positive kernel and a sea of delocalised electrons.
non-polar covalent
An equal sharing of electrons.
polar covalent
Unequal sharing of electrons leading to a dipole forming.
valence electrons
Electrons in the outermost energy level of an atom.
condensation
The process of a gas becoming a liquid.
deposition
The process of a gas becoming a solid.
evaporation
The process of a liquid becoming a gas.
freezing
The process of a liquid becoming a solid.
melting
The process of a solid becoming a liquid.
sublimation
The process of a solid becoming a gas.
boiling point
The temperature at which a liquid starts to become a gas.
freezing point
The temperature at which a liquid starts to become a solid.
melting point
The temperature at which a solid starts to become a liquid.
compound
A compound consists of particles that are made up of more than one type
of atom, and the different types of atoms are joined together chemically.
element
An element cannot be broken down into simpler substances.
heterogenous
mixture
A heterogeneous mixture is a mixture where we can still see the different
components of the mixture.
homogenous
mixture
A homogeneous mixture is a mixture which exists as only one phase so
that we cannot distinguish visually between the different components of
the mixture.
mixture
A mixture consists of two or more pure substances that can be mixed
together in any ratio.
pure substance
A pure substance consists of the same type of particles throughout.
law of conservation
of mass
In a chemical reaction, the total mass of all the reactants equals the total
mass of all the products.
law of constant
composition
A specific chemical compound always contains the same elements in the
same ratio.
solute
The substance that is dissolved in the solution.
solvent
The substance in which another substance is dissolved, forming a solution.
solution
A homogeneous mixture of a solute and a solvent.
dissociation
The splitting of an ionic compound into its ions.
ionisation
The reaction of a molecular substance with water to produce ions.
hydration
Hydration is the process in which ions are surrounded by water molecules
in a water solution.
electrolyte
A substance that can conduct electricity by forming free ions when molten
or dissolved in solution.
ammonium
NH4+
carbonate
CO[3]2-
bicarbonate
HCO3-
dichromate
Cr[2]O[7]2-
hydroxide
OH-
hydronium
H[3]O+
nitrate
NO[3]-
nitrite
NO2-
permanganate
MnO4-
phosphate
PO[4]3-
sulphate
SO[4]2-
sulphite
SO[3]2-
water
(water) H[2]O
table salt
(sodium chloride) NaCℓ
vinegar
(ethanoic acid) CH[3]COOH
baking soda
(sodium bicarbonate) NaHCO[3]
battery acid
(sulphuric acid) H[2]SO[4]
swimming pool acid
(hydrochloric acid) HCℓ
ammonia
(ammonia) NH[3]
soda water
(carbonic acid) H[2]CO[3]
caustic soda
(sodium hydroxide) NaOH
marble/chalk
(calcium carbonate) CaCO[3]
epsom salts
(magnesium sulphate) MgSO[4]
Does nitric acid (HNO[3]) have a common name?
No.
