CH1120
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Solid
◦ Definite shape and volume
◦ Cannot be compressed
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Liquid
◦ Definite volume but takes shape of container
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Gas
◦ No fixed volume or shape
◦ Uniformly fills container
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Physical state that involves moving from one
state to another
Occurs when energy is added or removed
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Melting: phase change from solid to liquid
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Freezing: phase change from liquid to solid
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Temperature where liquid and solid phases
coexist at equilibrium is:
◦ Melting point of the solid
◦ Freezing point of the liquid
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Vapour: gas
Vapour pressure: pressure exert by a gas on
its container when it is at equilibrium with its
condensed phases (solid or liquid)
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Boiling: the process of molecules in the liquid
phase breaking apart from neighbouring
molecules to enter the gas phase
Boiling point: temperature when a liquid’s
vapour pressure equals the external pressure
acting on the liquid surface
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Evaporation: liquid  gas
Condensation: gas  liquid
Sublimation: solid  gas
Deposition: gas  solid
Melting: solid  liquid
Freezing: liquid  solid
Boiling: liquid  gas
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Temperature is a measure of the average
kinetic energy of the molecules of a
substance
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Adding energy heats up substances
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Energy causes more movement of molecules
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Altering molecular movement alters the state
of substances
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Remember, molecules do not lose their
structure when they undergo a phase change
◦ H2O is still H2O
 Steam, water, ice
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Molecules simply have more space between
them
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Atoms bond together to obtain a stable
electron configuration
Atoms gain, lose, or share electrons until they
are surrounded by eight valence electrons
Some elements require 2 valence electrons
(not 8)
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Think of your orbital diagrams
◦ Elements want to look like the closest noble gas
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We use Lewis dot diagrams to show valence
electrons and help us see how bonding
occurs
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Remember, electrons repel each other
(negative charge)
◦ They don’t want to fill the same orbital if it can be
avoided
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Electrons are negative
◦ Gaining electrons makes charge more negative
◦ Losing electrons makes charge more positive
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Main group elements are lazy and want to
look like the closest noble gas
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Metals want to lose electrons
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Non-metals want to gain electrons
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In ionic bonding atoms gain and lose
electrons
◦ Charge (ions)
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In covalent bonding atoms share electrons
◦ No charge (atoms)
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Ionic bonds contain a metal and one or more
non-metals
Covalent bonds contain only non-metals
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Atoms form ions by gaining and losing
electrons
Ionic bonds form a crystal lattice
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Contain a metal and one or more non-metals
Contain ions (charged atoms) due to transfer
of electrons
NO sharing electrons
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Electrons are transferred from the metal ion
to the non-metal ion
Smallest unit is the formula unit
◦ 1Na and 1Cl bonded together is one formula unit of
NaCl
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Very high melting and boiling points
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Crystalline and can be cleaved
◦ Broken along smooth flat surfaces
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Brittle
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Conduct electricity when dissolved
◦ Break into ions
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We begin by drawing the individual atoms
involved in the bonds
◦ NaCl
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Then we show the transfer of electrons
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Our final structure has square brackets and
the charge of the ions
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Type 1 metals only have one possible charge
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Metals keep their name from the table
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Non-metal is named ending in -ide
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MgCl2
◦ Magnesium chloride
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NaCl
◦ Sodium chloride
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AgBr
◦ Silver bromide
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Put the symbols for each element
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Balance charges (criss cross)
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Cesium bromide
◦ CsBr
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Cadmium fluoride
◦ CdF2
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Aluminum sulfide
◦ Al2S3
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Zinc sulfide
◦ ZnS
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I=1
II=2
III=3
IV=4
V=5
VI=6
VII=7
VIII=8
IX=9
X=10
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Type 2 metals can have more than one charge
◦ We must tell other people which form we are talking
about
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Use roman numerals to differentiate metals
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Name as you did type 1 compounds
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Add roman numeral in brackets after name of
the metal
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AuCl3
◦ Gold (III) chloride
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NbN
◦ Niobium (I) nitride
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VBr5
◦ Vanadium (V) bromide
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Important to remember the roman numeral
tells you CHARGE not how many atoms
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Write symbols for the metal and non-metal
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Put roman numeral as charge
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Balance charges (criss cross)
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Iron (II) bromide
◦ FeBr2
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Nickel (III) nitride
◦ CuN
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Lead (IV) oxide
◦ PbO2
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In your booklet
Charged chemical species composed of two
or more atoms
Act as a unit
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Follow the rules for the type of compound
you are using
If there are multiples of the polytomic ion,
use brackets
◦ Remember they act as a unit
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Copper (II) carbonate
◦ CuCO3
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Magnesium permanganate
◦ Mg(MnO4)2
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Silver phosphate
◦ Ag3PO4
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Name by following the rules for the type of
compound you are using
Don’t change the name of the polyatomic ion
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AgCN
◦ Silver cyanide
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Cu3(PO3)2
◦ Copper (II) phosphite
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Mn(HCO3)2
◦ Manganese (II) hydrogen carbonate
◦ Manganese (II) bicarbonate
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Formed by the addition of water or its
components to another substance
Substances without water are called
anhydrous
Water molecules form
lattice around central
compound
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Mono=1
Di=2
Tri=3
Tetra=4
Penta=5
Hexa=6
Hepta=7
Octa=8
Nona=9
Deca=10
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Tell you the number of
water molecules that
are present
Example:
◦ Hexahydrate = 6 water
molecules
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Name the base compound by following rules
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Add “hydrate” with the appropriate prefix
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LiClO4 • 3H2O
◦ Lithium perchlorate trihydrate
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NiSO4 • 6H2O
◦ Nickel (II) sulfate hexahydrate
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Write the formula for the base compound by
following previous rules
Separate water molecules from central
compound with “•”
Write H2O with appropriate coefficient
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Copper (II) sulfate pentahydrate
◦ CuSO4 • 5H2O
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Magnesium carbonate pentahydrate
◦ MgCO3 • 5H2O
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Bonds made between non-metal atoms
Electron sharing due to similar affinities for
electrons
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No transfer of electrons
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Smallest unit is the molecule
◦ 1C and 4H bonded together is one molecule
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Low melting and boiling points
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Pliable in solid form
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Do not conduct electricity when dissolved
◦ Do not ionize in solution
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We begin by drawing the individual atoms
involved in bonding
◦ Atom needing the most electrons goes in the
middle
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We circle the electrons that will be shared by
the atoms
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Where there are 2 electrons circled by 2
atoms we replace the electrons with a line
◦ Represents a bond
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When 2 electrons are shared it is a single
bond (1 shared pair)
Can have multiple bonds
4 electrons shared (2 shared pairs) = double
bond
6 electrons shared (3 shared pairs)= triple
bond
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For more complicated compounds:
◦ Add up total valence electrons of bonding atoms
 This is the number of electrons we need in our final
structure
◦ Draw one bond between the central atom and the other
bonding atoms
 Each bond counts as using up 2 of the electrons we started
with
◦ Draw in the valence electrons on the atoms
◦ Borrow electrons to give the central atom a full octet
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Draw the Lewis Structure of the following:
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CO2
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HCN
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COS
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Prefixes
Mono=1
Di=2
Tri=3
Tetra=4
Penta=5
Hexa=6
Hepta=7
Octa=8
Nona=9
Deca=10
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Write the names of the elements present
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Change ending to –ide for last element
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Add prefixes to match the number of atoms
of each element
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CH4
◦ Carbon tetrahydride
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CO
◦ Carbon monoxide
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N2S3
◦ Dinitrogen trisulfide
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Write the symbols for each element in the
compound
Use the prefixes as the subscripts in the
formula
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NCl3
◦ Nitrogen trichloride
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CS2
◦ Carbon disulfide
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BrCl
◦ Bromine monochloride