Atoms
The smallest part of matter.
Proton, Neutron and Electron
subatomic particles
Electrons
The smallest subatomic particle with a negative charge
Protons
The positive subatomic particle that is in the nucleus that contributes to atomic mass
Neutrons
The other subatomic particle with no charge that contributes to atomic mass
charge of an atom
Neutral, protons = electrons
number of elements in periodic table
118
Atomic number
number that goes up by one with each successive element on the periodic table
Mass number
number that tells the average amount of protons and neutrons in an element
Isotopes
Atoms with the same number of protons but different amount of neutrons, e.g Carbon - 14
electron shell maxiums
2, 8, 18 (8), 32
Valence shells/electrons
The outermost electron shell has the least electrostatic attraction to the nucleus
main categories in periodic table
Metals, metalloids, and non-metals
verticle GROUPS
The number of valence electrons of the elements, similar chemical properties
horizontal PERIODS
The number of electron shells
Group 18
Nobel gases, full valence shell
Group 1
Alkali metals, more reactive going down, 1 valence electron
Group 17
Halogens, more reactive going up, 7 valence electrons
Types of chemical bonding
Ionic bonding, metallic bonding, covalent bonding
Ions
Charged atoms that have either gained or lost electrons
Cation, positive charge
Ions that loose electrons
Anion, negative charge
Ions that gain electrons
Transition metals
Metals that have many different ions, e.g Iron (III)
Polyatomic ions
Non-metal ions that have combined to become a anion
Ionic bonding
Bonding that occurs between a non-metal and a metal, balancing ionic charges
Lattice
chemical structure of ionic compound
Ionic lattice pattern
Anions and cations alternating
Ionic lattice properties
hard, brittle, high melting and boiling points, crystalline solid, conducts electricity when not solid
Metallic bonding
Bonding between metals
Metal compounds are in a lattice of cations held together due to what
the delocalised electrons from the cations zooming around creating an electrostatic bond
metal compound properties
lustrous, high melting and boiling points, malleable and ductile, dense, good electrical and heat conductors
3 types of heat treatments on metals
quenching, annealing, tempering
annealing process
making a metal red hot and then cooling slowly
quenching process
making a metal red hot and then shocking it in ice water to cool it down
tempering process
quenched metals, reheated and then cooled slowly
tempering properties
less brittle/more malleable, retaining hardness due to a balance between crystal size and interconnectedness
quenching properties
harder, more brittle due to smaller crystals and larger gaps
annealing properties
softer, more ductile and malleable due to larger crystals with smaller gaps
solvent
the liquid a substance is dissolved into
solute
the dissolved substance that can be a liquid, solid, or gas
in displacement reactions what metals are displaced
the more reactive metal will displace the less reactive metal in the solution
when will a displacement reaction not occur
if the more reactive metal is already in the solution
what are the 3 methods of metal extraction
roasting in air, smelting, and electrolysis
covalent bonding atoms
non-metals
covalent bonds
a shared pair of electrons between non-metals
reactants
the substances before a chemical reaction
products
the substances formed during a chemical reaction
law of conservation of mass
reactants = products
acids
are molecular in structure
acidic solutions
have more H+ ions
basic solution
have more OH- ions
ph scale 0 - 7 - 14
acidic - neutral - basic
indicators
change colour at different ph values
strong acid names
hydrochloric acid, sulfuric acid, nitric acid
strong acids
are completely ionised
weak acids
incomplete ionisation, reversible reaction
molar (M)
concentration of solution
reaction of acids with reactive metals
acid + metal = salt + hydrogen
reaction of acids with metal hydroxides (neutralisation reaction)
acid + metal hydroxide = salt + water
reactions of acids with metal oxides
acid + metal oxide = salt + water
reactions of acids with metal carbonates
acid + metal carbonate = salt + carbon dioxide + water
reactions of acids with metal hydrogen carbonates
acid + metal hydrogen carbonate = salt + carbon dioxide + water
rate of reaction
how fast the reactants are converted into products
rate of reaction formula
-reactants/time or products/time
average rate of reaction
take a segment of the line and calculate the gradient
instantaneous rate of reaction
draw a tangent at the given point and then find gradient of tangent
collision theory requirements
collision, correct orientation, enough energy
activation energy
the amount of energy needed for a successful colllision
factors that can influence the rate of reaction
concentration, temperature, surface area, catalyst
greater concentration in a reaction
more frequent collisions, more successful collisions, faster rate of reaction
greater surface area in a reaction
more surface exposed to collisions, more frequent collisions, more successful collisions, faster rate of reaction
greater temperature in a reaction
increased kinetic energy, more particles with energy >Ea, more frequent collisions, more successful collisions, faster rate of reaction
catalyst in a reaction
lowers activation energy, more particles with energy >Ea, more successful collisions, faster rate of reaction
catalyst effect
weakens bonds within the reactants, does not contribute to the products