Download Honours

2/24/2014 Symbols for Atoms, Molecules, and Ions
Nomenclature
—  Isotope form:
The top number represents the
mass number.
CHEMISTRY 11
4
2
He
The bottom number represents the
atomic number.
Molecules and Ions
—  Recall:
¡  The bottom number is always the number
of protons.
¡  The bottom number is also usually the
number of electrons, but only in a neutral
element.
¡  The number of neutrons is always the top
number minus the bottom number.
2.  One taking electrons from the other (produces an IONIC SALT
or FORMULA UNIT having ionic bonds).
—  Consider NaCl:
¡  Chlorine has a higher affinity for electrons than Sodium, and
so it takes one away as shown by the following:
Cl + e - → Cl - ¡ 
The electron joins up with the chlorine, and becomes a
negatively charged ion (also known as an ANION).
—  Compounds are made up of two or more atoms held
together 2 different methods:
1.  Both sharing electrons (produces a MOLECULE having
covalent bonds).
—  Take water for example:
Each H shares its electron with
the O, so that the O has two
shared electrons, completing
its valence shell.
¡ 
The electron came from the sodium atom:
Na → Na + + e –
The normal Sodium atom gives off an electron and becomes a
positively charged ion in the process (also known as a
CATION).
¡  Since these charges have opposite signs, they attract to form
the ionic solid.
¡ 
1 2/24/2014 Review of Naming
—  Ions don't have to be just one atom; they can be
—  From Science 10 Honours…
¡  Naming:
polyatomic (consisting of many atoms).
—  For Example:
÷  Ionic
Compounds
and Polyatomic
¢  Hydrates
¢  Multivalent Cations
¢  Binary
•  Using Stock Method and Common Name
÷  Covalent
÷  Acids
¡ 
Name
Formula
Aluminum chloride
AlCl3
Compound
K2O
Magnesium hydride
MgH2
Common Name
Mg(OH)2
Fe2O3
Ferric oxide
Iron (III) oxide
Ammonium sulphate
NaClO
Hydrates?
Stock Name
Magnesium hydroxide
(NH4)2SO4
Na2S
Potassium oxide
You
know the
drill…
Counting Atoms
Again, with multivalent cations…
Ionic Compounds…
Sodium sulphide
Compounds
and Bases
Sodium hypochlorite
CrF2
Chromous fluoride
CuCl2
Cupric chloride
Chromium (II) fluoride
Copper (II) chloride
Ca(HCO3)2
Calcium bicarbonate
KHC2O4
Potassium binoxalate
Dissociation of Ionic Salts
Iron (III) phosphate octahydrate
FePO4 · 8H2O
Nickel (II) chloride hexahydrate
NiCl2 · 6H2O
Calcium nitrate tetrahydrate
Ca(NO3)2 · 4H2O
Sodium sulphate decahydrate
Na2SO4 · 10H2O
Magnesium hydrogen phosphate heptahydrate
MgHPO4 · 7H2O
Nickel (II) phosphate octahydrate
Ni3(PO4)2 · 8H2O
—  Electrolyte:
¡  A substance which dissolves to give an electrically conducting
solution containing ions.
¡  Produced from an ionic salt.
¡  For example:
(NH4)2SO4(s) è 2 NH4+(aq) + SO42-(aq)
Dissociation equation: salt è ions.
2 2/24/2014 NO dissociation for covalent!
Try some covalent…
you’ll be better for it!
Tetraphosphorus trisulphide
P4S3
Trisilicon tetranitride
Si3N4
Oxygen diflouride
OF2
Bromine monofluoride
BrF
Tetrasulphur dinitride
S4N2
Diphosphorus hexaoxide
P2O6
—  Molecular:
¡  Compounds made up of a non-metal and a non-metal will be
molecular in solution (do not form ions, stay as a molecule in
solution).
¡  For example:
CH3OH(l) è CH3OH(aq)
¡  Usually organic compounds (more to come later).
¡  Beware of acetate (CH3COO-) and other organic ions. They will
form ionic solutions.
And last, but not least, ACIDS!!!
Name
Formula
Hydrochloric Acid
HCl
Nitric Acid
HNO3
Sulphurous Acid
H2SO3
Chlorous Acid
HClO2
Counting Atoms… remember?
When we are given a molecule, it’s
easy to count how many atoms are
present.
—  For Example:
¡ 
AgNO3(s)
5 atoms
¡ 
KCl(aq)
2 atoms
¡ 
Pb(SO4)2(s)
11 atoms
¡ 
Al(CH3COO)3(s)
22 atoms
Transition metals (a.k.a. “The Weirdo's”)
—  Exhibit the following characteristics:
¡  Form more than one oxidation state (charge).
¡  The cations are often complex ions.
¡  The transition metal is surrounded by a certain number of
LIGANDS (molecules or ions that bond to a metal ion).
¡  For example:
—  Unlike other metals, transition metals show great
[Co(NH3)6]Cl3
similarities within a given period and group.
3 2/24/2014 Coordination Compounds
—  Most compounds produce coloured solutions.
—  Formed by transition metal ions.
—  Consists of a
(a transition
metal with its attached ligands) and
(ions to balance out
charge).
—  For example:
[Co(NH3)5Cl]Cl2
Ligands
—  When these compounds dissolve in water, they
usually produce coloured solutions that act as ionic
compounds:
[Co(NH3)5Cl]Cl2(s) → Co(NH3)5Cl2+(aq) + 2Cl-(aq)
—  A neutral molecule or ion having a lone electron pair
that can be used to form a bond to a metal ion.
—  Monodentate Ligand:
¡  Also called unidentate ligand.
¡  Can form one bond to a metal ion.
—  Bidentate Ligand:
¡  Can form two bonds to a metal ion.
—  Chelating Ligand or Chelates:
¡  A ligand that is attached to a central metal ion by bonds from
two or more donor atoms.
Coordination Number
—  The number of bonds formed by metal ions to ligands
varies from two to sixteen.
—  Depends upon the size, charge, and electron configuration
of the transition metal ion.
Chelating
ligand
—  Each coordination number will produce a
different geometry (more to come later).
4 2/24/2014 Nomenclature
—  For Example:
¡  For each of the following, determine the coordination number:
÷  [Zn(NH3)4]2+
÷  [Co(CN)6]3÷  [Ag(NH3)2]+
Name these…
—  [Cr(NH3)3(H2O)3]Cl3
¡  triamminetriaquachromium(III) chloride
—  [Pt(NH3)5Cl]Br3
¡  pentaamminechloroplatinum(IV) bromide
—  [Pt(H2NCH2CH2NH2)2Cl2]Cl2
¡  dichlorobis(ethylenediamine)platinum(IV) chloride
—  [Co(H2NCH2CH2NH2)3]2(SO4)3
¡  tris(ethylenediamine)cobalt(III) sulfate
—  K4[Fe(CN)6]
¡  potassium hexacyanoferrate(II)
—  Na2[NiCl4]
¡  sodium tetrachloronickelate(II)
Write the formulas for the following:
—  Hexaammineiron(III) nitrate
¡  [Fe(NH3)6](NO3)3
—  Ammonium tetrachlorocuprate(II)
¡  (NH4)2[CuCl4]
Homework:
—  Do:
¡  Nomenclature
¡  Study for your quiz (in two classes)!!!
÷  Naming
Compounds
—  Sodium chloropentacyanoferrate(III)
¡  Na3[Fe(CN)5Cl]
—  Potassium hexafluorocobaltate(III)
¡  K3[CoF6]
5 2/24/2014 What is on the exam?
—  The Classification of
Matter
¡ 
Atoms, Molecules, and
Ions
—  Classifying Matter
¡  Heterogeneous,
Homogeneous, etc.
—  The Physical Separation
of Substances
¡ 
Distillation,
Chromatography, etc.
—  Nomenclature
¡  Symbols for atoms, ions,
and molecules
¡  Naming and Formulas for:
÷  Ionic
Compounds
Compounds
÷  Hydrates
÷  Acids
÷  Complex Ions
÷  Covalent
—  Counting Atoms
6