Transcript Nomenclature

Nomenclature
CH. 3
The Types of Compounds
Ionic
salts, acids and bases (Electrolytes)
Minerals
Covalent
inorganic from non living systems
organic/biological- hydrocarbons, from living systems
polymers - large hydrocarbons
Metallic compound
Pure elements, alloys and amalgams
biometallic - proteins or large compounds with metal
centers
Compounds
IONIC Compounds
COVALENT compounds
Fixed Charge Metals
Multiple charge metals
Acids
Ammonium salts
inorganic
Binary
Ternary
Binary
Ternary
Binary
NaCl
CaCO3
FeO
PbSO4
sodium chloride
calcium carbonate
Iron (II) oxide
lead (II) sulfate
organic
Ternary
ternary
binary
binary
ternary
HCl
H3PO4
NH4NO3
N2S4
hydrochloric acid
phosphoric acid
ammonium nitrate
dinitrogen tetrasulfide
C8H18
octane
CH3COCH3
acetone
COVALENT Compounds
Covalent compounds usually form when two non
metal atoms which both have a desire to gain
electrons create a bond by sharing the electrons
between them.
Neither atoms has full possession of the electron;
therefore neither atom is charged.
Most organic compounds or hydrocarbons would fit
into this category.
With over 10 million compounds, organics comprise
90% of all the known matter.
IONIC Compounds
Ionic Compounds involve the transfer of
electrons from one atom making a cation to
another atom making an anion.
The bond forms when the cation with a
positive charge is attracted to the anion with
a negative charge.
This electrostatic attraction is the ionic bond
and usually occurs between a metal and a
non metal atom.
Balancing Charge
Na+ & O-2
Na+x O-2y
x(+1) + y(-2) = 0
find the smallest common factor
Na2O
Ca+2 & N-3
Ca3N2
x(+2) + y(-3) = 0
Fixed Charge Metals
1A always carries a +1 charge.
Electron configuration - ns1
2A always carries a +2 charge
Electron configuration - ns2
3A metals and 3B always carries +3
electron configuration - ns2np1 or ns2nd1
Naming inorganic compounds
When an element forms only one compound
with a given anion.
name the cation
name the anion using the ending (-ide)
NaCl
sodium chloride
MgBr2
magnesium bromide
Al2O3
aluminum oxide
K3N
potassium nitride
Naming ionic compounds
Many metals form more than one compound with
some anions.
For these, roman numerals are used in the name
to indicate the charge on the metal.
Cu1+
+
O2copper(I)
oxide
Cu2+
+
O2copper(II)
oxide
= Cu2O
copper(I) oxide
= CuO
copper(II) oxide
Metals with multiple charges
Transition metals.
Here it is easier to list the ones that to only
have a single common oxidation state.
All Group 3B - 3+
Ni, Zn, Cd
- 2+
Ag
- 1+
Lanthanides and actinides - 3+
Summary
Simple rules that will keep you out of trouble
most of the time.
Groups IA, 2A, 3A (except Tl) only have a
single oxidation state that is the same as the
group number - don’t use numbers.
Most other metals and semimetals have
multiple oxidation states - use numbers.
If you are sure that a transition group
element only has a single state, don’t use a
number.
Polyatomic Ions
need to know
Nitrate
NO31-
Hydroxide
OH-
Carbonate
CO3-2
Cyanide
CN-
Sulfate
SO4-2
Acetate
C2H3O21-
Phosphate
PO4-3
Chlorate
ClO31- Ammonium
NH4+
Polyatomic ions
When a compound contains a polyatomic ion,
you simply use the given name.
NH4Cl
ammonium chloride
NaOH
sodium hydroxide
KMnO4
potassium permanganate
(NH4)2SO4
ammonium sulfate
Acids and Bases
Acid
HCl
HNO3
H2SO4
H3PO4
NaOH
KOH
Ba(OH)2 Al(OH)3
Base
The bases listed are metal hydroxides and
therefore are named as an ionic compound
Acids
Binary acids
–
–
–
–
the anion is a single element ending in -IDE
the acid is named hydro - root - ic acid
HCl - Hydrogen Chloride or
hydro- chlor - ic acid
Ternary Acids
• Anion ends in -IDE
– hydro - root - ic acid
– HCN, hydrogen cyanide is hydro cyan ic acid
• anion ends in -ATE
– root - ic acid
– HNO3, hydrogen nitrate is nitr ic acid
• anion ends in -ITE
– root -ous acid
– H3PO3, hydrogen phosphite is phosphorous acid
Naming Covalent Molecules
A simple set of rules can be used.
name elements in the order they appear in the
formula.
use prefixes to indicate how many atoms there are
of each type.
mono = 1
di = 2
tri = 3
tetra = 4
penta = 5
hexa = 6
hepta = 7
octa = 8
deca = 10
use the ending (-ide) for the second element listed
in the formula.
Naming covalent compounds
N2O5
CO2
CO
SiO2
ICl3
P2O5
CCl4
dinitrogen pentoxide
carbon dioxide
carbon monoxide
silicon dioxide
iodine trichloride
diphophorous pentoxide
carbon tetrachloride
The rule may be modified to improve how a name
sounds.
Example - use monoxide not monooxide.
Naming Organic Compounds
• Contain Carbon and hydrogen atoms
• Use prefix to count number of carbons
present in the compound
• functional groups
Nomenclature overview
Now that a large number of nomenclature
rules have been introduced, we need to
review them.
Simple binary ionic compounds
Ionic compounds of metals with multiple charges
Compounds containing polyatomic ions
Simple molecular compounds
It’s useful to be able to identify which
system to use by looking at the chemical.
A bit more on nomenclature
When the first element is a metal then usually:
If only one other element is present and
the second element is a non-metal name the metal first - as element.
Name non-metal second with -ide ending
If more than one other element is present name the metal first - as element.
The rest is most likely a polyatomic ion
so use the name from the table in book.
A bit more on nomenclature
Is a metal present
Use prefixes
as the first element? No (mono, di, tri ...)
Yes
Can the metal have
more than one
oxidation state?
No
Roman numerals
are not needed.
Yes
Use Roman numerals
to indicate oxidation state of metal
Naming Activities
• Naming Flowchart