Transcript Chemical Nomenclature


Ionic Bonds
› Metal + Non-Metal
› Metal (CATION) always first followed by Non-metal
(ANION)
› Electrons are Transferred

Covalent Bonds (Sometimes called Molecular)
› Non-metal + Non-metal
› Electrons are Shared

We will talk more about how these bonds
form, their properties, etc next semester
Smallest
piece
Types of
elements
State
Melting
Point
Ionic
Molecular
Formula Unit
Molecule
Metal and
Nonmetal
Nonmetals
solid
High
>300ºC
Solid, liquid or
gas
Low
<300ºC
Ionic
Nomenclature
Binary
Compounds
Ternary
Compounds
Ionic
Compounds
with Transition
Metals

Binary = 2 elements total in the cmpd

Naming Binary Compounds
› Take the cation (metal) and name it just like
the element on the periodic table
› Take the anion (non-metal) and change the
ending of the element to –ide
› Ex: Al2O3 = Aluminum Oxide
Oxygen = Oxide
 Sulfur = Sulfide
 Hydrogen = Hydride
 Phosphorus = Phosphide
 Nitrogen = Nitride
 Silicon = Silicide
 Selenium = Selenide
 Carbon = Carbide


NaCl

Mg3N2

K2S

LiH

SrBr2

AlP
Step 1
Step 2
Step 3
• Write elements with their
charges (M first, then NM)
• Cross charges and make
subscripts from them (remove
+ or - ) Write elements together
as compound
• If necessary, simplify subscripts
to lowest terms

Al+3 O2-

Al2O3

Step 3 not necessary
Step 1
Step 2
Step 3
• Write elements with their
charges (M first, then NM)
• Cross charges and make
subscripts from them (remove
+ or - ) Write elements together
as compound
• If necessary, simplify subscripts
to lowest terms

Al+3 N3-

Al3O3

AlO
› (3 & 3 both divisible
by 3 to give 1)
Step 1
Step 2
Step 3
• Write elements with their
charges (M first, then NM)
• Cross charges and make
subscripts from them (remove
+ or - ) Write elements together
as compound
• If necessary, simplify subscripts
to lowest terms

Mn+4 O2-

Mn2O4

MnO2
› (2 & 4 both divisible
by 4 to give 1 & 2)

Ternary = 3 or more elements in compound

Naming Ternary Ionic Compounds
› Name like Binary (element name + --ide)EXCEPT
when POLYATOMIC IONS are used as metals or
non-metals
› You will need to memorize the most common
polyatomic Ions
NH4Cl
 Mg(OH)2
 NaNO3
 AlPO4
 K2SO4
 H2O2

1.
Still… cation FIRST, anion SECOND
Na+ OH-
2.
Criss-cross the superscript charge to get the
subscripts.
Na1 OH1
3.
Reduce the subscript to the least whole
number ratio if needed.
NaOH
4.
If polyatomic ion has a subscript in the formula greater
than 1, you must put parentheses around the
polyatomic ion and place the subscript outside the
parenthesis.
Al(OH)3
Example: Barium nitrate
1. Write the symbols/formulas for
the cation and anion, including
CHARGES!
2. Cross Charges.
3. Simplify subscripts. Use
parentheses if you need more
than one of a polyatomic ion.
Example: Ammonium sulfate
1. Write the formulas for the cation
and anion, including CHARGES!
2. Cross Charges.
3. Simpifly subscripts. Use
parentheses if you need more
than one of a polyatomic ion.
Magnesium carbonate
 Strontium hydroxide
 Aluminum phosphate


Remember Transition Metals are called
transition because they can have
varying oxidation states!!!
The name of metals with two or more positive ions
(cations) use a Roman numeral to identify ionic
charge.
Lead
Pb2+
lead(II)
Pb4+
lead(IV)
Copyright © 2005 by Pearson Education, Inc.
Publishing as Benjamin Cummings
21

Step 1:
The easiest way to do this is to
uncross the subscripts back to
charges.
› ALWAYS MOVE THE ANION’S
CHARGE BACK FIRST! CHECK &
MAKE SURE THE ANION CHARGE IS
WHAT IT SHOULD BE!
› Ex. Fe3N2 uncrossed: Fe2+ N3 What we expect on N
› Ex. MnO2 uncrossed: Mn+2 O-1
 NOT WHAT WE EXPECT ON O! WE KNOW O
should be a -2 which meant the subscripts
simplified. So….
 REAL ANSWER: MnO2 uncrossed: Mn+4 O2-



Step 2-4
Once you know the charges, now
name the transition metal with
Roman Numerals:
I
II
III
IV V
VI
Ex: Fe+3 O2› Iron (III) Oxide

Ex: Mn+4 O2› Manganese (IV) Oxide

Just like Binary & Ternary Rules
› Now the metal charge is given to you, you
don’t need to remember it or look it up!
› Don’t forget ONLY transition metals use
roman numerals
› Don’t forget about your polyatomics
Mn2O7
NbCl5
TiP
Pd(SO4)2
PtF2
Os2O3
Ir(NO3)4
Co(ClO)2
Fe2S3
AuI3
Manganese (VII) Oxide
Niobium (V) Chloride
Titanium (III) Phosphide
Palladium (IV) Sulfate
Platinum (II) Fluoride
Osmium (III) Oxide
Iridium (IV) Nitrate
Cobalt (II) Hypochloride
Iron (III) Sulfide
Gold (III) Iodide

You will see Transition metals named by
their classical/traditional names.

I want you to be aware of the following,
but you won’t be tested over them in this
class
Ion
Fe3+
Systematic
(STOCK)
Name
Iron (III)
Traditional
(Classical)
Name
Ferric
Fe2+
Iron (II)
Ferrous
Cu2+
Copper (II)
Cupric
Cu1+
Copper (I)
Cuprous
Sn4+
Tin (IV)
Stannic
Sn2+
Tin (II)
Stannous
Pb4+
Lead (IV)
Plumbic
Pb2+
Lead (II)
Plumbous
Name the metal first; use Latin names of
metals.
 In binary compounds the nonmetal takes
the suffix –ide. (Like before)
 The ion with the lower charge takes the
suffix
–ous
 The ion with the higher charge takes the
suffix –ic.

Covalent
Nomenclature
Diatomic
Molecules
Binary
Molecules
Remember, covalent bonds form between a
non-metal and a non-metal and the electrons
are shared!
When some elements are by themselves,
with no other element, they pair up with
other elements that are like them.
 They are called diatomic molecules!
 We name them just by the element
name on the periodic table

Br2I2N2Cl2H2O2F2




Br2
H2
Oxygen
Chlorine




Bromine
Hydrogen
O2
Cl2
If these 7 elements are paired with other elements, they will NOT be named
like this! They will be named like we talk about later!


Covalent Compounds use
Prefixes to name
compounds
ALWAYS use prefixes
except:
› Only use mono on the
second element
› If you have a diatomic
molecule

1st: (prefixelementname)
2nd:(prefixelementendinide)
PREFIXES
1-mono
2-di
3-tri
4-tetra
5-penta
6-hexa
7-hepta
8-octa
9-nona
10-deca
P2O5 diphosphorous pentoxide
OF2 oxygen difluoride
PBr3 phosphorous tribromide
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
CO2
CO
P2O5
N2O
SiO2
CBr4
SO2
PBr5
ICl3
NI3
N2O3
B2H6
NBr3
SCl6
P4O10
S7O2
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
Carbon dioxide
Carbon monoxide
Diphosphorous pentaoxide
Dinitrogen monoxide
Silicon dioxide
Carbon tetrabromide
Sulfur dioxide
Phosphorous pentabromide
Iodine trichloride
Nitrogen triiodide
Dinitrogen trioxide
Diboron hexahydride
Nitrogen tribromide
Sulfur hexachloride
Tetraphosphorous decaoxide
Heptasulfur dioxide
1. Silicon tetrafluoride
2. Dinitrogen trisulfide
3. Sulfur trioxide
4. Dinitrogen tetroxide
5. Nitrogen monoxide
6. Nitrogen dioxide
7. Tetraphosphorous octaoxide
8. Tetraphosphorous nonasulfide
9. Diarsenic pentoxide
10. Phosphorous trichloride
11. Carbon tetrachloride
12. Dihydrogen monoxide
13. Selenium hexafluoride
14. Iodine heptafluoride
15. Tetraarsenic decoxide
16. Carbon disulfide
17. Oxygen difluoride
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
SiF4
N2S3
SO3
N2O4
NO
NO2
P4O8
P4S9
As2O5
PCl3
CCl4
H2O
SeFl6
IF7
As4O10
CS2
OF2
Acid formulas usually begin with H
 We name them according to how the
ANION name ends!
 Common Acids we use:

› HCl: Hydrochloric Acid
› HNO3: Nitric Acid
› H2SO4: Sulfuric Acid
Anion Ending
Acid Name
Example
Binary Acids
(no oxygen in
formula)
-ide
Hydro-(stem) –ic
Acid
HCl:
Hydrochloric
Acid
(from chloride)
Ternary Acids
(oxygen in the
formula)
-ate
(stem)-ic acid
HNO3:
Nitric Acid
(from nitrate)
-ite
(stem)-ous Acid
H2SO3
Sulfurous Acid
(from sulfite)
(per)-ic
per-stem-ic
Acid
HClO4
Perchloric
Acid
Hypo-ite
per-stem-ous
Acid
HClO
Hypochlorous
Acid
ACIDS
start with 'H'
2 elements
3 elements
hydro- prefix
-ic ending
no hydro- prefix
-ate ending
becomes
-ic ending
-ite ending
becomes
-ous ending
• HBr (aq)
•No oxygen, -ide
• H2CO3
•Has oxygen, -ate
• H2SO3
•Has oxygen, -ite
 hydrobromic
acid
 carbonic
acid

sulfurous acid
• hydrofluoric acid
•2 elements
 H+ F-
 HF (aq)
• sulfuric acid
•3 elements, -ic
 H+ SO42-  H2SO4
• nitrous acid
•3 elements, -ous
 H+ NO2-  HNO2

HI (aq)

HCl

H2SO3

HNO3

HIO4

Hydrobromic
acid

Nitrous acid

Carbonic acid

Phosphoric acid

Hydrotelluric acid
 Some compounds contain H2O in their
› These compounds are called hydrates.
structure.
 This
is different from (aq) because the H2O is part of
the molecule (not just surrounding it).
 The
H2O can usually be removed if heated.
separates water: e.g. CuSO4•5H2O is
copper(II) sulfate pentahydrate.
 A dot
 Name
the ionic part (the salt) just the way you would
as before; a greek prefix indicates the # of H2O
groups.
Na2SO4•10H2O
NiSO4•6H2O
sodium sulfate decahydrate
nickel(II) sulfate hexahydrate
carbonate monohydrate Na2CO3•H2O
BaCl2•2H2O
barium chloride dihydrate
sodium
Nomenclature Summary
Flowchart