Transcript Compounds
Compounds
A compound is a pure substance that contains
two or more elements that are chemically
bonded to each other
Compounds form when the electrons of two
or more elements interact and are composed
of either:
Molecules
water =
H
O
H
Ions
Salt = NaCl
Na , Cl
Molecules
Molecule:
A group of atoms combined in definite
proportions and held together by strong
attractive forces called covalent chemical
bonds
Covalent bonds are formed when atoms
share two or more electrons.
The smallest representative particle of a
molecular compound
Molecular Compounds
Molecular compounds
composed of molecules that contain more
than one type of atom
Most molecular substances are composed
of non-metals only.
Examples:
Water (H2O)
Ethyl alcohol (C2H6O)
Carbon dioxide (CO2)
Ammonia (NH3)
Ionic Compounds
Ionic compounds are composed of ions (both
cations and anions) and usually contain a
metal and one or more nonmetals.
“Salt” (NaCl)
Contains Na+ and Cl- ions
Tums (CaCO3)
Contains Ca2+ and CO32- ions
Milk of Magnesia [Mg(OH)2]
Contains Mg2+ and OH-
Ionic Compounds
Ionic compounds such as NaCl are formed when
one or more electrons are transferred from
one atom to another
the resulting cation and anion are strongly
attracted to each other and are held
together by an ionic bond resulting from
electrostatic forces of attraction
Chemical Formulas
The composition of a compound is generally
shown using a chemical formula:
A shorthand notation that describes the
types and relative (or exact) numbers of
each atom (or ion) present in a pure
substance
Chemical formulas always contain:
Elemental symbols
Subscripts
Show the relative (or exact) number
of each type of atom or ion
Chemical Formulas
Molecular Formula
chemical formula that tells the actual
number of each type of atom in a molecule
Empirical Formula
chemical formula that tells the smallest
whole number ratio of each type of atom
in a molecule
Acetic Acid
Ascorbic Acid
Sodium Sulfate
C2H4O2
C6H8O6
Na2SO4
CH2O
C3H4O3
Ionic Compounds
The ions present in an ionic compound can be
either:
Monoatomic
Polyatomic
Monoatomic ion:
a charged species containing a single atom
that has gained or lost electrons
Al3+
S2-
Predicting Ion Charge – Monoatomic Ions
Many atoms gain or lose electrons in such a
way that they end up with the same number
of electrons as the nearest (closest in atomic
number) noble gas.
“octet” rule
Ca (20p, 20e-) Ca2+ (20p, 18e-) [Ar: 18p,18e-]
O (8p, 8e-) O2- (8p, 10e-) [Ne: 10p, 10e-]
Predicting Ion Charge – Monoatomic Ions
Using the octet rule you can easily determine
the charge on most of the monoatomic ions
formed by the main group elements.
Main group metal cations:
Charge = group number
Main group nonmetal anions:
Charge = group # - 8
(or simply count the number of “spaces” away
from the nearest noble gas and add a
negative sign)
Common Monoatomic Ions
Know These!
P3Zn2+
Ag+
In general:
Metal atoms and hydrogen lose e- and form cations.
Nonmetal atoms gain e- and form anions.
Common Monoatomic Ions
Many transition metals and a few main group
elements form more than one ion.
Main group
Main group
Cr2+ Mn2+ Fe2+ Co2+
Cr3+ Mn3+ Fe3+ Co3+
Cu+
Cu2+
Sn2+
Sn4+
Pb2+ Bi3+
Pb4+ Bi5+
Names of Monoatomic Ions - Cations
Cations formed by a metal have the same
name as the metal.
K+
potassium ion
Ca2+
calcium ion
Al3+
aluminum ion
If a metal forms more than one cation, use
Roman numerals in ( ) after the name of the
metal to show its charge.
Fe2+
Fe3+
Cu+
Cu2+
iron (II) ion
iron (III) ion
copper (I) ion
copper (II) ion
Names of Monoatomic Ions - Anions
Monoatomic anions are named by:
dropping the ending of the element’s name
adding “ide”
N
N3-
nitrogen
O
oxygen
nitride
O2-
oxide
Polyatomic Ions
Polyatomic ion:
an electrically charged group of two or
more atoms that are held together by
covalent bonds
Polyatomic ions cannot be broken into
smaller pieces.
Examples:
-
NO3
SO42HCO3
PO43-
H
H N H
H
Polyatomic Ions
You are responsible for knowing the names
and formulas of all ions listed in your
syllabus, including the common polyatomic
ions:
Ammonium
Hydroxide
Cyanide
Nitrate
Acetate
Sulfate
Bisulfate (Hydrogen sulfate)
Carbonate
Bicarbonate (Hydrogen carbonate)
Phosphate
NH4+
OHCNNO3C2H3O2SO42HSO4CO32HCO3PO43-
Naming Oxyanions
mXOn
Many of the polyatomic anions are oxyanions.
polyatomic anions containing one or more
oxygens attached to a central atom
To name an oxyanion, drop the ending of the
central atom name and add:
“ate”
most common oxyanion
of the element
“ite”
1 less oxygen
NO3- nitrate
NO2- nitrite
SO42- sulfate
SO32- sulfite
CO32- carbonate
PO43- phosphate
PO33- phosphite
Oxyanions
“ate” oxyanions to memorize
4A
5A
2CO3
NO3
carbonate
6A
nitrate
3PO4
2SO4
phosphate sulfate
7A
-
ClO3
chlorate
BrO3
bromate
IO3
iodate
Noble gases
3A
Oxyanions
The halogens typically form 4 different
oxyanions:
“per”
“hypo”
1 more O than the “ate” oxyanion
1 less O than the “ite” oxyanion
ClO4ClO3ClO2ClO-
perchlorate
chlorate
chlorite
hypochlorite
most oxygens
most common
1 less O
fewest oxygens
Oxyanions
Anions derived by adding one or two H+ to an
oxyanion:
add “hydrogen” or “dihydrogen” as prefix
to oxyanion name
CO32HCO3-
carbonate
hydrogen carbonate
(usually called bicarbonate)
PO43H2PO4-
phosphate
dihydrogen phosphate
Writing Formulas for Ionic Compounds
Ionic compounds are always represented using
an empirical formula with the cation shown
first.
The formula for an ionic compound must be
electrically neutral.
Total positive charge = total negative
charge
Although ions are present in an ionic
compound, the formula does NOT explicitly
show the charge of the ions.
NaCl
not
Na Cl
Writing Formulas for Ionic Compounds
Ionic compounds must be electrically neutral.
Total positive charge = total negative
charge
Na+ + Cl-
NaCl
Na+
Cl-
(1 pos, 1 neg)
Writing Formulas for Ionic Compounds
Ca2+ + Cl-
CaCl
(2 pos, 1 neg)
ClCa2+
Ca2+ + 2Cl-
CaCl2 (2 pos, 2 neg)
ClCa2+
Cl-
Writing Formulas for Ionic Compounds
To write the empirical formula of an ionic
compound from its name:
1. Identify the formula including charge for
each ion.
2. Combine the ions in a ratio that gives an
electrically neutral compound.
Writing Formulas for Ionic Compounds
If charges on the ions are equal in magnitude
(but opposite in sign), then combine the ions
in a 1:1 ratio.
calcium sulfate
2+
Ca
2SO4
Ca2+ SO42-
CaSO4
sodium bicarbonate
+
Na
-
HCO3
NaHCO3
Na+
HCO3-
3-
Writing Formulas for Ionic Compounds
If charges on the ions are different, then
flip-flop the charges (i.e. the charge of one
ion becomes the subscript of the other ion).
magnesium nitride
Mg2+
N3-
Mg3N2
calcium hydroxide
2+
Mg3N
Ca
2
OH
1-
Ca(OH)2
Place ( ) around a polyatomic ion IF more
than one is needed.
Writing Formulas for Ionic Compounds
Example: Write the correct formula for the
following ionic compounds.
Zinc bromide
Aluminum carbonate
Iron (II) phosphate
Tin (IV) sulfate
Magnesium hydroxide
Writing Formulas for Ionic Compounds
Example: Write the correct formula for the
following ionic compounds.
Sodium bicarbonate
Ammonium sulfate
Potassium phosphite
Sodium hypochlorite
Copper (I) oxide
Writing Formulas for Ionic Compounds
Remember:
Use empirical formulas
Formulas must be electrically neutral
Do not show the charges of each ion in
the final formula that you write
Use parentheses around polyatomic ions if
more than one is present in the formula
Do not use ( ) around monoatomic ions
Do not use ( ) around a single
polyatomic ion
Naming Ionic Compounds
Ionic compounds are named using the cation
name followed by the anion name
CaBr2
NaClO
Mg3(PO4)2
calcium bromide
sodium hypochlorite
magnesium phosphate
If the cation can form ions with more than
one charge, you must specify the charge:
Fe2S3
PbO2
iron (III) sulfide
lead (IV) oxide
Naming Ionic Compounds
Example: Name the following ionic compounds.
Na2SO4
FeCl3
(NH4)3PO4
KClO4
Cu2CO3
Sn(SO4)2
Common “Household” Chemicals
You are responsible for knowing the names
and formulas for the chemical present in:
Baking soda
sodium bicarbonate
NaHCO3
Table salt
Sodium chloride
NaCl
Bleach
Sodium hypochlorite
NaClO or NaOCl