Transcript chemrat.com

Intro to Inorganic Chemical Nomenclature
Part 1, Binary Compounds
This lesson was divided into two parts
Part 1 Binary Compounds
• In this first video we are studying the nomenclature of Binary
Compounds
• There is also a second video dealing with the nomenclature of
Polyatomic Compounds.
• Youtube ‘Inorganic Chemical Nomenclature Part 2 Polyatomic Compounds’
1
Intro to Inorganic Chemical Nomenclature
Part 1 Binary Compounds
Chemical Nomenclature = writing the formulas and names of chemicals.
Using three systems of inorganic nomenclature …
• the Stock system
• the Prefix system
• the Ous-Ic system
This requires that you learn the names, formulas and oxidation numbers (Ox #’s) of a
variety of monatomic elements and polyatomic ions needed for binary and polyatomic
compounds.
This lesson is designed for a 1st semester college chemistry student and assumes that
the student already has a working knowledge of electron configuration,
electronegativity, chemical bonding, and acid ionization.
2
Intro to Inorganic Chemical Nomenclature
Chemical Formulas of Binary Compounds:
Binary compounds are made of two different kinds of atoms.
A chemical formula tells us which atoms and how many atoms of each kind are
present in a chemical compound.
Look at the structure of a water molecule.
Each water molecule contains 2 hydrogen atoms and 1 oxygen atom.
symbol for oxygen
symbol for hydrogen
subscript indicates
2 hydrogen atoms
H2O
implied subscript of 1
indicating 1 oxygen atom
A subscript of ‘1’ is never written in formulas.
Look at the formulas on the right and identify the error in each.
H2O/1
H2O
/(H)/2O
OH2
3
1A
1H (2.1)
Electronegativity (EN) values of A-group Elements
EN:
hydrogen
1
-1
3Li (1.0)
lithium
1
--11Na (1.0)
sodium
1
--19K (0.9)
2A
4Be(1.5)
beryllium
2
--12Mg (1.2)
magnesium
1
--37Rb (0.9)
2
--20Ca (1.0)
calcium
2
--38Sr (1.0)
rubidium
strontium
1
--55Cs (0.8)
cesium
1
--87Fr (0.8)
2
--56Ba (1.0)
barium
2
--88Ra (1.0)
radium
2
---
potassium
francium
1
---
3A
5B (2.0)
4A
6C
5A
(2.5)
7N (3.0)
boron
carbon
nitrogen
3
2, 4
2,3,4,5
---4
-3
14Si (1.8)
13Al (1.5)
15P (2.1)
aluminum
silicon phosphorus
+3
3, 4, 5
4
---3
--31Ga (1.7)
33As (2.1)
32Ge (1.9)
gallium germanium arsenic
4
3
3, 5
-----3
50Sn (1.8)
49In (1.6)
51Sb (1.9)
indium
antimony
tin
1, 3
3, 5
2, 4
---3
--82Pb (1.7)
83Bi (1.8)
81Tl (1.6)
thallium
lead
bismuth
1, 3
2, 4
3, 5
-------
6A
8O
(3.5)
oxygen
---2
16S (2.5)
sulfur
2, 4, 6
-2
34Se (2.4)
selenium
4, 6
-2
52Te
(2.1)
tellurium
4, 6
-2
84Po
(1.9)
polonium
2, 4
---
7A
9F
(4.0)
fluorine
---1
17Cl (3.0)
chlorine
1,3,5,7
-1
35Br (2.8)
bromine
1, 5
-1
53I (2.5)
iodine
1, 5, 7
-1
85At
(2.1)
astatine
H2O
2.1 (H) < 3.5 (O)
The less EN atom is listed first.
Practice:
Write the formula of a
compound made of …
• one S & two Na atoms
Na2S
1.0 (Na) < 2.5 (S)
• one P & three Br atoms
PBr3
2.1 (P) < 2.8 (Br)
• two Cl’s & one Mg atom
MgCl2 1.2 (Mg) < 3.0 (Cl)
In formulas of ionic compounds, symbols of metals precede nonmetals
because all metals have lower EN values than any nonmetal.
4
Chemical Formulas of Binary Compounds
Use the table of EN values to write the chemical formulas of the compounds shown
below…
EN:
Al (1.5) < O (3.5)
Al2O3
C (2.5) < O (3.5)
CO2
Ca (1.0) < F (4.0)
CaF2
5
Some Exceptions in Chemical Formulas of Binary Compounds
The least Electronegative atom in binary compounds are usually listed first, but there
are a few historical exceptions …
• In the formulas of hydrocarbon compounds (abbreviated HC’s), which are
compounds containing only hydrogen and carbon, C (EN=2.5) is listed before
H (EN=2.1), even though C has the higher EN value.
CH4, methane, is the
major component of
natural gas.
C2H6, ethane is the 2nd
largest component of
natural gas
• Most formulas of binary compounds, in which H is listed first, are acids, such as
hydrochloric acid, HCl and hydrofluoric acid, HF.
• HC’s are not acidic so their H’s are listed last.
6
More Exceptions in Chemical Formulas of Binary Compounds
• In the formulas of binary compounds containing nitrogen, N is usually
listed first regardless of its EN value.
In N2O5,
N (3.0) < O (3.5)
N is less EN and
written first.
In ammonia, NH3,
EN N (3.0) > H (2.1),
but N is written first.
• Ammonia, NH3, is not acidic. It’s a moderately strong base.
• Listing H first would make ammonia look acidic … H3N
/
7
Naming Binary Compounds
There are three systems for naming binary compounds
1. The Stock System (the most comprehensive)
e.g., sodium chloride
2. The Prefix System (for nonmetal compounds only)
e.g., carbon monoxide, carbon dioxide
3. The ous-ic system (has limited use)
e.g., ferrous oxide, ferric oxide
8
The Stock System for Naming Binary Compounds
CaCl2 = calcium chloride
name of less
name of more EN
EN atom first
atom ends in ‘ide’
a space
between
chlorine  chloride
•
•
•
Al2O3 = aluminum oxide
name of less
name of more EN
EN atom first
atom ends in ‘ide’
a space
between
oxygen  oxide
In ionic compounds (made of metal cations, ⊕ and nonmetal anions, ⊖), the less
EN atom is a metal cation, and the more EN atom is a nonmetal anion.
The name of the metal cation is the same as the element’s name but the anion’s
name ends in ‘ide’.
Note that the Stock system name does not tell us the relative number of atoms in
the formula. This will be explained later.
9
Learn the anion names & charges.
1A
1H (2.1)
8A
He
hydrogen
1
-1
3Li (1.0)
lithium
1
--11Na (1.0)
sodium
1
--19K (0.9)
2A
4Be(1.5)
beryllium
2
--12Mg
(1.2)
magnesium
1
--37Rb (0.9)
2
--20Ca (1.0)
calcium
2
--38Sr (1.0)
rubidium
strontium
1
---
2
---
potassium
3A
5B (2.0)
4A
6C
5A
(2.5)
7N (3.0)
boron
carbon
nitrogen
3
2, 4
2,3,4,5
---4
-3
14Si (1.8)
13Al (1.5)
15P (2.1)
aluminum
silicon phosphorus
+3
3, 4, 5
4
---3
--31Ga (1.7)
33As (2.1)
32Ge (1.9)
gallium germanium arsenic
4
3
3, 5
-----3
50Sn (1.8)
49In (1.6)
51Sb (1.9)
indium
antimony
tin
1, 3
3, 5
2, 4
---3
---
6A
8O
(3.5)
oxygen
---2
16S (2.5)
sulfur
2, 4, 6
-2
34Se (2.4)
selenium
4, 6
-2
52Te
(2.1)
tellurium
4, 6
-2
7A
9F
(4.0)
fluorine
---1
17Cl (3.0)
chlorine
1,3,5,7
-1
35Br (2.8)
bromine
1, 5
-1
53I (2.5)
iodine
1, 5, 7
-1
Nonmetal anions gain enough
electrons to fill their valence
shell to become isoelectronic
with the nearest noble gas.
Helium
Ne
Neon
Ar
Argon
Anions typically have
only 1 possible Ox #,
which is easy to
learn if you know
their Group number
on the PD table
Kr
Krypton
Xe
Xenon
10
Practice naming these binary compounds using the Stock system:
K3P
potassium phosphide
BaBr2
barium bromide
MgO
magnesium oxide
CaH2
calcium hydride
Al2S3
aluminum sulfide
Na2Se
sodium selenide
Ca3N2
calcium nitride
SrCl2
strontium chloride
MgF2
magnesium fluoride
B2O3
boron oxide
LiI
lithium iodide
SiC
silicon carbide
Be2C
beryllium carbide
HF
hydrogen fluoride
Note that the last three examples are not ionic compounds. They are composed of metalloids and/or
nonmetals only, yet the Stock system names all compounds as if they were ionic.
The less EN atom is first (using the atom’s name). The more EN atom is last (using the anion’s ‘ide’ name).
11
Writing Chemical Formulas of Binary Compounds
In order to write formulas and name compounds, you will need the
‘oxidation numbers’ (Ox #’s) of the atoms/ions in a compound.
Ox #’s are explained in detail in a video entitled ‘Oxidation Numbers’ and
will only be discussed briefly in this lesson.
What is an oxidation number (Ox #)?
Ox # is a charge assigned to an atom or ion in a compound.
All pure elements have an Ox # = 0, e.g., Ox # Cu=0, H2=0, S8=0.
About 20 elements have only one Ox # (fixed Ox #’s), other than 0, and
they must be memorized, but it is easy to do so if you learn their position
on the periodic table.
The Ox #’s of other atoms/ions are calculated from the chemical formula.
12
Fixed Ox #’s are highlighted (red and yellow). Metals cannot have ⊖ Ox #’s (they never gain e’s).
Most nonmetals can have ⊖ or ⊕ Ox #’s, e.g., Cl in ICl (Cl = -1), Cl in ClF (Cl = +1), Cl in ClO2 (Cl = +4), Cl in ClF7 (Cl = +7).
Note that the nonmetal with higher EN always gets a ⊖ Ox #
1H
(2.1)
symbol & proton number
hydrogen
Key
1
-1
Li (1.0)
electronegativity (EN)
2A
Be(1.5)
3
4
lithium
beryllium
1
---
2
---
11
Fixed Ox #’s are easily memorized by knowing
their A-Group number on the PD table.
Other Ox #’s can all be calculated.
7
N (3.0)
3A
-3
6
7
boron
carbon
negative oxidation numbers
3
---
2, 4
-4
nitrogen oxygen
2,3,4,5
---
Al (1.5)
13
sodium
magnesium
aluminum
1
---
2
---
3
---
3B
4B
5B
6B
7B
6A
B (2.0)
Na (1.0) 12Mg (1.2)
8B
8B
8B
1B
2B
C (2.5)
5A
positive oxidation numbers
5
nitrogen
2,3,4,5
4A
Si (1.8)
14
N (3.0)
O (3.5)
8
-3
P (2.1)
15
7A
F (4.0)
9
fluorine
---1
-2
S (2.5)
16
Cl (3.0)
17
silicon
phosphorus
4
---
sulfur
2, 4, 6
chlorine
3, 4, 5
-3
-2
-1
1,3,5,7
Cr (1.6) 25Mn (1.6) 26Fe (1.7) 27Co (1.7) 28Ni (1.8) 29Cu (1.8) 30Zn (1.6) 31Ga (1.7) 32Ge (1.9) 33As (2.1) 34Se (2.4) 35Br (2.8)
potassium calcium scandium titanium vanadium chromium manganese
iron cobalt nickel copper zinc gallium germanium arsenic selenium bromine
2,3,4,6,7
4
2,3,4,5
2, 3, 6
1
3
3, 4
4, 6
3, 5
2
3
1, 5
2, 3
2, 3
1, 2
2, 3
2
---------3
-2
-------1
--------------19
K (0.9)
Ca (1.0)
20
Sc (1.3)
21
Ti (1.4)
22
23
V (1.5)
24
Zr (1.3) 41Nb (1.5) 42Mo (1.6) 43Tc (1.7) 44Ru (1.8) 45Rh (1.8) 46Pd (1.8) 47Ag (1.9) 48Cd (1.6) 49In (1.6)
rubidium strontium yttrium zirconium niobium molybdenum technetium ruthenium rhodium palladium silver cadmium indium
2,3,4
2, 4
--1
2
3
4
3,5
2
1, 3
2, 3, 4
2,3,4,5,6
1
--------------------------Rb (0.9)
37
Sr (1.0)
38
Cs (0.8) 56Ba (1.0)
cesium barium
1
2
-----
55
Y (1.2)
39
La (1.1)
57
lanthanum
3
---
40
Sn (1.8) 51Sb (1.9)
antimony
tin
3, 5
2, 4
-3
---
50
Au(1.9) 80Hg (1.7) 81Tl (1.6) 82Pb (1.7) 83Bi (1.8)
halfnium tantalum tungsten rhenium osmium iridium platinum gold
mercury thallium
lead bismuth
4
5
1,
3
2,3,4,5,6 1,2,4,6,7 2,3,4,6,8 2,3,4,6
3, 5
2, 4
1,
2
1, 3
2, 4
------------------------Hf (1.3)
72
Ta (1.4)
73
W (1.5)
74
75
Re (1.7) 76Os (1.9)
Ir (1.9)
77
78
Pt (1.8)
79
Te (2.1)
52
tellurium
4, 6
-2
I (2.5)
iodine
53
1, 5, 7
-1
Po (1.9) 85At (2.1)
84
polonium
2, 4
---
astatine
13
Writing the Formulas of Binary Compounds
•Chemical formulas represent the smallest whole number ratio of atoms/ions in a compound.
•The positive and negative charges (Ox #’s) must add up to zero; the charges balance.
Steps
calcium chloride boron bromide
1. Obtain ion symbols
& Ox #’s (charges)
calcium: Ca+2
hydrogen sulfide
magnesium phosphide
magnesium: Mg+2
chloride: Cl-
B+3 (2.0EN) hydrogen: H+ (2.1EN)
bromide: Br - (2.8EN) sulfide: S-2 (2.5EN)
2. Find the total
charge needed to
balance + & - charges
Ca+2
B+3
Mg+2
3. Find the ratio of +
and - ions
1 Ca+2 ion for
every 2 Cl- ions
4. Use subscripts to
write the formulas
Cl-
= +2
-1 -1 = -2
CaCl2
boron:
= +3
H+1
+1 +1 = +2
Br - -1 -1 -1 = -3
S-2
= -2
1 B+3 ion for
every 3 Br - ions
2 H+ ions for every
1 S-2 ion
BBr3
H2S
phosphide: P-3
P-3
+2 +2 +2 = +6
-3 -3 = -6
3 Mg+2 ions for every
2 P-3 ions
Mg3P2
Nonmetals such as Cl, Br, H, S and P can have ⊕ or ⊖ Ox #’s. An atom is assigned a ⊕ Ox # when it
is the less EN atom in a compound and a ⊖ Ox # when it is the more EN atom in a compound.
14
Practice writing the chemical formulas of binary compounds:
name
ions
formula
magnesium oxide
potassium nitride
Mg+2
O-2
MgO
K+
N-3
K3N
barium fluoride
silicon iodide
beryllium carbide
Ba+2
F-
BaF2
Si+4
I-
SiI4
Be+2
C-4
Be2C
calcium hydride
lithium selenide
sodium phosphide
Ca+2
H-
CaH2
Li+
Se-2
Li2Se
Na+
P-3
Na3P
zinc phosphide
aluminum sulfide
boron oxide
Zn+2
P-3
Zn3P2
Al+3
S-2
Al2S3
B+3
O-2
B2O3
A chemical formula shows the lowest whole
number ratio of ions such that the total
positive and negative charges are equal.
The ‘Inverse rule’ is an easy way to find this
ratio.
Consider zinc phosphide.
Zn+2
P-3  Zn3P2
The number of Zn cations (3) equals the
charge of the anion (-3), and the number of
P anions (2) equals the charge of the cation
(+2).
But remember to reduce this to the lowest
whole number ratio.
Consider beryllium carbide.
Be+2 C-4  Be4C2  Be2C
15
Finding an Ox # in Compounds Containing a Multivalent Ion
water = H2O
water ≠ HO2 or H3O or HO, etc.
because the Ox # H = +1 and Ox # O = -2
In order to combine elements in a chemical formula in the correct ratio, you need to know the Ox #’s of
each element. You will also need to know these Ox #’s for writing chemical names.
However many elements are ‘multivalent’; they have more than one possible Ox #.
Fortunately, it is always true that at least one of the elements in a binary compound will have an Ox #
that is known for certain and so the other element’s Ox # can be calculated.
Example 1: Manganese has 5 different Ox #’s in its compounds, i.e., +2, +3, +4, +6 and +7.
Calculate the Ox # of Mn in MnCl2.
Answer: Mn = +2
Here’s why: The Ox # of Cl is -1 because it is more EN than Mn. Chloride is always -1.
The total negative charge in MnCl2 = (Cl-1 × 2) = -2.
So the total positive charge of Mn must be +2, and the Ox # of Mn must be +2.
16
Example 2: Calculate the Ox # of Mn in Mn2O3
Answer: Mn = +3
Here’s why: The Ox # of O is always -2.
The total negative charge of three O’s = (-2 × 3) = -6
The total positive charge of both Mn ions must be +6 (total ⊕ = total ⊖).
So each Mn has a charge of (+6/2) = +3
or solve as a math equation:
Let Ox # of Mn = x
The sum of all Ox #’s = 0
Mn2O3 = 0
(x)*2 + (-2)*3 = 0
2x – 6 = 0
x = +6/2 = +3  Mn+3
or use the Inverse Rule:
+3
-2
Mn2O3
17
Practice:
Calculate the Ox # of the underlined ion in each formula
Formula
MnO2
MnO3
Mn2O7
V3N5
Fe4C3
anion charge
-2
-2
-2
-3
-4
cation charge
Formula
anion charge
cation charge
+4
+6
+7
+5
+3
Cu3P
PbF4
PCl5
Mo2S5
NiH3
-3
-1
-1
-2
-1
+1
+4
+5
+5
+3
18
Naming Binary Compounds Containing a Multivalent Ion:
Iron (Fe), like manganese (Mn) can exhibit more than one Ox #.
There are two kinds of iron chloride, FeCl2 and FeCl3. The name ‘iron chloride’ is thus ambiguous.
In binary compounds containing cations with more than one Ox #, the Ox # of the cation is written in Roman
numerals (in parentheses) immediately after the cation.
Thus FeCl2 is named iron(II) chloride and FeCl3 is named iron(III) chloride.
+2
FeCl2
=
Fe
FeCl3
=
Fe+3
-
Cl
= iron(II) chloride
Cl-
= iron(III) chloride
no space between the cation
name and its Ox # but always
leave a space immediately
before the anion name
There are two different forms of iron chloride.
Iron(II) chloride is green.
Iron(III) chloride is yellow/rusty colored.
Each different chemical compound must have its own,
unique, unambiguous name.
19
Look at the formulas and names of two kinds of iron oxide, FeO and Fe2O3.
Please read carefully: The Ox # listed immediately after the cation indicates the
charge on the cation, not necessarily the number of anions in the formula.
+2
O-2
FeO = Fe
Fe2O3 = Fe+3
= iron(II) oxide
FeO is black
O-2 = iron(III) oxide
The Ox #, e.g., (II) or (III)
indicates the charge on the
cation, not necessarily the
number of anions present.
Fe2O3 is rusty/red
To name a compound, write the ion symbols and determine their Ox #’s from the
combining ratio given in the formula.
The anion usually has only one possible Ox #, so calculate the Ox # of the cation
remembering that the total ⊕ charge and ⊖ charges in compounds are equal.
20
Naming Binary Compounds Containing a Multivalent Ion:
Steps
1. Identify the Ox # that is known for
certain (usually the anion’s).
Au3N
Cl2O5
nitride: N-3 (Group 5A)
oxide: O-2 (Group 6A)
(N is more EN than Au, so it uses its O is more EN than Cl,
negative Ox #)
O always has an Ox # of -2
2. If allowed, check the periodic table
for the possible charges of the
other ion.
Au+ or Au+3
Cl+, Cl+3, Cl+5 or Cl+7
3. Determine the ratio of ions in the
formula
Au3N means 3 gold ions for every
1 nitride ion.
Cl2O5 means 2 chlorines for every
5 oxide ions.
4. Find what charge must be on the
multivalent ion to balance all
charges
Au+
+1 +1 +1 = +3
N-3
= -3
3 Au+ ions are needed for every
1 N-3 ion
Cl+5:
+5 +5 = +10
O 2-:
-2 -2 -2 -2 -2 = -10
2 Cl+5 atoms are needed for every
5 O-2 ions.
5. Write the name of the compound
gold(I) nitride
chlorine(V) oxide
21
Practice Naming Binary Compounds Containing a Multivalent Ion:
Determine Ox #’s of the ions in the compounds below.
Use these Ox #’s to write Stock system names of the compounds.
name
formula
ions
name
formula
ions
iron(II) oxide
FeO
Fe+2
O-2
iron(III) oxide
Fe2O3
Fe+3 O-2
chromium(VI) oxide
CrO3
Cr+6
O-2
manganese(IV) sulfide
MnS2
Mn+4 S-2
nickel(III) fluoride
NiF3
Ni+3 F-
cobalt(III) chloride
CoCl3
Co+3 Cl-
copper(II) oxide
CuO
Cu+2 O-2
cobalt(II) oxide
CoO
Co+2 O-2
copper(I) oxide
Cu2O
Cu+
tin(IV) nitride
Sn3N4
Sn+4 N-3
gold(III) bromide
AuBr3
Au+3 Br-
tin(II) nitride
Sn3N2
Sn+2 N-3
O-2
22
Practice Writing Formulas of Binary Compounds Containing Multivalent Ions:
name
formula
ions
chromium(III) oxide
Cr2O3 Cr+3 O-2
name
formula
ions
cobalt(III) phosphide
CoP
Co+3 P-3
nickel(II) fluoride
NiF2
Ni+2 F-
vanadium(V) chloride
VCl5
V+5 Cl-
titanium(IV) oxide
TiO2
Ti+4 O-2
tungsten(IV) carbide
WC
W+4 C-4
Note: The formula of a binary compounds does not show the charge of the cation or
the anion. Do not write any charges in binary compound formulas.
For example, sodium chloride’s formula is NaCl, not Na+Cl-.
23
Binary Acids:
Binary acids contain hydrogen, H, that is covalently bonded to a non metal.
Hydrogen chloride, HCl, is an example of a binary acid.
When dissolved in water, hydrogen chloride is named hydrochloric acid because it
releases an acidic H+ ion when it ionizes.
Learn the names and formulas of the five common binary acids, listed below.
name (anhydrous)
name (in water)
formula
reaction in water
hydrogen fluoride
hydrofluoric acid
HF
HF  H+ + F-
hydrogen chloride
hydrochloric acid
HCl
HCl  H+ + Cl-
hydrogen bromide
hydrobromic acid
HBr
HBr  H+ + Br-
hydrogen iodide
hydroiodic acid
HI
HI  H+ + I-
hydrogen sulfide
hydrosulfuric acid
H2S
H2S  2H+ + S-2
24
Summary of Stock System Nomenclature for Binary Compounds
SnO
tin(II) oxide
NaCl
sodium chloride
SnO2
tin(IV) oxide
CaCl2
calcium chloride
Cr2O3
chromium(III) oxide
Al2O3
aluminum oxide
CrO3
chromium(VI) oxide
ZnS
zinc sulfide
CuBr
copper(I) bromide
Ag3P
silver phosphide
CuBr2
copper(II) bromide
There is > 1 tin oxide, chromium oxide, copper
bromide.
Sn, Cr, Cu have > 1 Ox #
Sn (+2, +4), Cr (+2, +3, +6), Cu (+1, +2)
Ox #’s must be included in the name (written in
Roman numerals).
There is only one sodium chloride, calcium
chloride, aluminum oxide, zinc sulfide, and silver
phosphide.
Na, Ca, Al, Zn, Ag have only 1 Ox # each.
Na & Ag (+1), Ca & Zn (+2), Al (+3)
The Ox # is not stated in the name.
25
The Prefix System for Binary Compounds
For binary compounds containing two non-metals, a Greek or Latin prefix is attached to the
name of an element to indicate the number of atoms of that element in the compound.
Number
1
2
3
4
5
6
Prefix
mono
di
tri
tetra
penta
hexa
Formula
CO
CO2
SO3
CCl4
PCl5
SF6
Prefix System Name
carbon monoxide
carbon dioxide
sulfur trixode
carbon tetrachloride
phosphorus pentachloride
sulfur hexafluoride
7 = hepta, 8 = octa, 9 = ennea, 10 = deca
Although this system is used almost exclusively for non-metal/non-metal compounds,
occasionally, it is used when a metal is present.
Attach a prefix to the 2nd atom in the formula (always).
Attach a prefix to the 1st atom in the formula (only if there is more than one of them).
26
Name the following compounds using both the Prefix system and the Stock system:
Formula
N2O
NO
NO2
N2O3
N2O4
N2O5
ICl
CS2
SO2
PCl3
P2O5
SCl6
MnO2
Prefix System Name
dinitrogen monoxide
nitrogen monoxide
nitrogen dioxide
dinitrogen trioxide
dinitrogen tetr(a)oxide
dinitrogen pent(a)oxide
iodine monochloride
carbon disulfide
sulfur dioxide
phosphorus trichloride
diphosphorus pent(a)oxide
sulfur hexachloride
manganese dioxide
Stock System Name
nitrogen(I) oxide
nitrogen(II) oxide
nitrogen(IV) oxide
nitrogen(III) oxide
nitrogen(IV) oxide
nitrogen(V) oxide
iodine(I) chloride
carbon(IV) sulfide
sulfur(IV) oxide
phosphorus(III) chloride
phosphorus(V) oxide
sulfur(VI) chloride
manganese(IV) oxide
27
The “Ous-Ic” System
For binary compounds in which the cation usually has only 2 oxidation states, the old “ous-ic” system is
sometimes used.
In a few cases, when the English name of the metal atom is awkward, the Latin name of the metal is
used instead.
Then the suffix “ous” is added for the lower oxidation number and “ic” for the higher oxidation number.
Symbol
Cu
Fe
Pb
Sn
Au
Hg
Pt
Co
Name
copper
iron
lead
tin
gold
mercury
platinum
cobalt
Latin Name
cuprum
ferrum
plumbum
stannum
aurum
-------
Ion Charge & Name
Cu+ = cuprous, Cu+2 = cupric
Fe+2 = ferrous, Fe+3 = ferric
Pb+2 = plumbous, Pb+4 = plumbic
Sn+2 = stannous, Sn+4 = stannic
Au+ = aurous,
Au+3 = auric
Hg+ = mercurous, Hg+2 = mercuric
Pt+2 = platinous, Pt+4 = platinic
Co+2 = cobaltous, Co+3 = cobaltic
28
Name the following compounds using the “ous-ic” system.
Formula
PbCl2
PbCl4
SnBr2
SnBr4
Cu2O
CuO
FeO
Fe2O3
Au2S3
PtF2
PtS2
Hg4C
Hg3N2
Ous-Ic Name
plumbous chloride
plumbic chloride
stannous bromide
stannic bromide
cuprous oxide
cupric oxide
ferrous oxide
ferric oxide
auric sulfide
platinous fluoride
platinic sulfide
mercurous carbide
mercuric nitride
Stock System Name
lead(II) chloride
lead(IV) chloride
tin(II) bromide
tin(IV) bromide
copper(I) oxide
copper(II) oxide
iron(II) oxide
iron(III) oxide
gold(III) sulfide
platinum(II) fluoride
platinum(IV) sulfide
mercury(I) carbide
mercury(II) nitride
29
Peroxides:
•
A reactive type of compound, called ‘peroxides’, has important commercial and industrial
applications. The most familiar example is hydrogen peroxide, H2O2.
H2O2
hydrogen peroxide
‘per’ means one more O than the
normal oxide.
H2O
hydrogen oxide
H
H
O
•
•
•
•
•
H
O
O
H
H2O2 is one of the strongest oxidizers known.
35 – 50% aqueous solutions are used industrially for pulp and paper bleaching.
Up to 12% H2O2 is used as hair bleach and 3% H2O2 is sold as a household disinfectant.
Peroxides are unusual, in that the ‘O’ in a peroxide has an Ox # = -1 and the formula of the
peroxide anion is written O2-2 (because the peroxide anion is a bonded pair of O’s).
Recall that ‘O’ is in Group 6A, it will be stable when it gains 2 electrons and becomes oxide, O-2,
so it is not surprising that peroxide, O2-2, is so reactive (unstable).
30
Group 1A and 2A metal peroxides have some interesting applications.
For example, sodium peroxide, Na2O2, converts carbon dioxide to oxygen and sodium carbonate.
Na2O2 + CO2  Na2CO3 + ½ O2
Both lithium peroxide and sodium peroxide have been used to regenerate oxygen from exhaled air in
confined spaces, such as submarines and spacecraft.
Peroxide Practice: Write the name or formula of the following compounds. Spelling counts.
Formula
H2O
H2O2
BaO2
K2O2
K2O
CaO2
Stock System Name
hydrogen oxide (Prefix name: dihydrogen monoxide)
hydrogen peroxide
barium peroxide
potassium peroxide
potassium oxide
calcium peroxide
Ox # & Charges
H+
O-2
H+
O2-2
Ba+2
O2-2
K+
O2-2
K+
O-2
Ca+2
O2-2
Note that peroxide formulas, such as H2O2, Na2O2, etc. are not reduced to the lowest whole number ratio.
Do not write HO or NaO. All peroxides contain a pair of bonded O’s.
Finished Part 1.
31
Congrats, you just completed inorganic chemical nomenclature
part 1 on Binary Compounds
There is also a second video dealing with the nomenclature of
Polyatomic Compounds.
Youtube
‘Inorganic Chemical Nomenclature Part 2 Polyatomic Compounds’
32
Intro to Inorganic Chemical Nomenclature
Part 2, Polyatomic Compounds
This lesson was divided into two parts
Part 2 Polyatomic Compounds
• In this video we will study the nomenclature of Polyatomic
Compounds
• There is also a first video in which I presented the nomenclature of
Binary Compounds. You should complete that video first.
• Youtube ‘Inorganic Chemical Nomenclature Part 1 Binary Compounds’
33
Inorganic Nomenclature Part 2 Polyatomic Compounds
Oxy Acids:
Oxyacids contain H, O and another nonmetal atom.
Many oxyacids are commonly found in cleaning products, fruits, food
ingredients, industrial chemicals, etc.
•
•
•
•
Phosphoric acid, H3PO4, is used to pickle steel and is the flavour in
root beers and colas.
Sulfuric acid, H2SO4, is the electrolyte in the automobile lead-acid
battery (35% H2SO4).
Carbonic acid, H2CO3, is formed when carbon dioxide, CO2, is
dissolved in water (H2O + CO2  H2CO3).
Carbonated beverages contain carbonic acid.
A 5% solution of acetic acid, CH3COOH, in water is sold as vinegar.
34
Here are eight important oxyacids. Some of these exist with varying numbers of oxygen atoms.
The ‘main’ oxyacids, the –ic acids, and their names are highlighted.
A
Car
Acetic Carbonic
ic acids
per … ic
H2CO3
… ic CH3COOH
… ous
hypo … ous
Never
Stays
Perfectly
Nitric
Sulfuric
Phosphoric
HNO3
HNO2
H2SO4
H2SO3
H3PO4
H3PO3
H3PO2
Clean
Chloric
HClO4
HClO3
HClO2
HClO
Bromic
HBrO4
HBrO3
HBrO2
HBrO
Iodic
HIO4
HIO3
HIO2
HIO
When oxyacids react, they release hydrogen ions, H+, and leave behind polyatomic anions.
HNO3  H+ + NO3and
H2SO4  2H+ + SO4-2
and
H3PO4  3H+ + PO4-3
A
ate anions
per … ate
… ate
… ite
hypo … ite
Car
Never
Acetate Carbonate Nitrate
CH3COO-
CO3-2
NO3NO2-
* H3PO3 only has 2 acidic H’s, so phosphite is HPO3-2
Stays
Perfectly
Clean
Sulfate
Phosphate
SO4-2
SO3-2
PO4-3
* HPO3-2
** H2PO2-
Chlorate
ClO4ClO3ClO2ClO-
Bromate
BrO4BrO3BrO2BrO-
Iodate
IO4IO3IO2IO-
** H3PO2 only has 1 acidic H, so hypophosphite is H2PO2-
35
Practice: Study the structures and learn the formulas and names of the acids and their anions.
+1
-2
+
-1
CH3COOacetate
CH3COOH
acetic acid
+1
2
+
H2SO4
sulfuric acid
SO4-2
sulfate
-3
2
+1
+
CO3-2
carbonate
H2CO3
carbonic acid
+1
HNO3
nitric acid
-2
+
+
PO4-3
phosphate
H3PO4
phosphoric acid
+1
-1
NO3nitrate
+1
3
HClO3
chloric acid
+
-1
ClO3chlorate
36
Practice: Study the Lewis structures and learn the formulas & names of the acids and their anions.
H
H
O
C
C
O
H
H+
H
+
H
H
O
C
C
-
H
O
CH3COOacetate
C
O
H
2H
+
-
O
C
O
H
-
N+ O
O
HNO3
nitric acid
H
H+
-
+
O
NO3nitrate
O
O
O
O
P
O
O
H
Cl O
HClO3
chloric acid
-
SO4-2
sulfate
H
3 H+
-
+
O
P
O
O
-
-
PO4-3
phosphate
O
-
O
S
O
O
N+ O
+
2 H+
H3PO4
phosphoric acid
O-
O-
H
O
CO3-2
carbonate
H2CO3
carbonic acid
O
H2SO4
sulfuric acid
O
+
S
O
O
O
O
O
H
CH3COOH
acetic acid
H
O
H
H+
+
O
Cl O
-
ClO3chlorate
37
Other Polyatomic Ions: A few other important polyatomic ions are shown below.
+1
-1
+
CNcyanide
HCN
hydrocyanic acid
-1
+1
OHhydroxide
H2O
water
+
NH3
ammonia
+
+1
+1
NH4+
ammonium
HCN, hydrogen cyanide is acidic.
In water it is called hydrocyanic acid.
Although it is a weak acid and has a sweet
almond odour, it is highly toxic when ingested.
HCN  H+ + CN-
The formula of water, H2O, looks like other binary
acids, but water is completely neutral.
When a H+ ion is removed from water, hydroxide
ion, OH-, a strong base is formed.
Ammonia, NH3, is a moderately strong base with
a pungent odour – the smell of Windex.
When NH3 reacts with H+, an ammonium cation,
NH4+, is formed: NH3 + H+  NH4+
NH4+ (ammonium ion) is the only polyatomic ion
listed that is a cation. Its ‘ium’ ending indicates
that it is a cation. The polyatomic anions have
endings ‘ate’, ‘ite’, and ‘ide’.
38
Other Polyatomic Ions: A few other important polyatomic ions are shown below.
H
C
H+
N
-
+
C
N
CNcyanide
HCN
hydrocyanic acid
H+
H O H
-
+
O H
OHhydroxide
H2O
water
H
H
N
H
NH3
ammonia
+
H
H
+
H
N+
H
H
NH4+
ammonium
HCN, hydrogen cyanide is acidic.
In water it is called hydrocyanic acid.
Although it is a weak acid and has a sweet
almond odour, it is highly toxic when ingested.
HCN  H+ + CN-
The formula of water, H2O, looks like other binary
acids, but water is completely neutral.
When a H+ ion is removed from water, hydroxide
ion, OH-, a strong base is formed.
Ammonia, NH3, is a moderately strong base with
a pungent odour – the smell of Windex.
When NH3 reacts with H+, an ammonium cation,
NH4+, is formed: NH3 + H+  NH4+
NH4+ (ammonium ion) is the only polyatomic ion
listed that is a cation. Its ‘ium’ ending indicates
that it is a cation. The polyatomic anions have
endings ‘ate’, ‘ite’, and ‘ide’.
39
Monoprotic and Polyprotic Acids:
Acids like CH3COOH, HNO3, HNO2, HClO4, HClO3, HClO2, HClO, etc. have only one ionizable H+ ion per
molecule; these are called monoprotic acids.
The three H’s bonded to C in CH3COOH are not ionizable.
Acids like H2CO3, H2SO4, H2SO3 and H3PO4 can release more than one H+ ion per molecule; they are called
polyprotic acids because they can release more than one H+ (proton).
When polyprotic acids lose some but not all of their ionizable H’s, important polyatomic anions form.
H2CO3 
HCO3- 
H2SO4 
HSO4- 
H2SO3 
HSO3- 
H3PO4 
H2PO4- 
HPO4-2 
H+
H+
H+
H+
H+
H+
H+
H+
H+
+
+
+
+
+
+
+
+
+
HCO3CO3-2
HSO4SO4-2
HSO3SO3-2
H2PO4HPO4-2
PO4-3
bicarbonate or monohydrogen carbonate
carbonate
bisulfate or monohydrogen sulfate
sulfate
bisulfite or monohydrogen sulfite
sulfite
dihydrogen phosphate
monohydrogen phosphate
phosphate
40
The stepwise ionization of some polyprotic acids is shown.
O
H
O
O
P
O
O
H
H+
H
H3PO4
phosphoric acid
+
H
O
H
O
P
O
O
H
-
H
P
O
O
H
H+
-
+
H
O
O
-
O
O
P
O
O
-
HPO4-2
monohydrogen phosphate
H
+
-
O
P
O
H
H+
+
H
O
S
O
S
O
HSO4bisulfate
O
O
H+
-
-
+
O
S
PO4-3
phosphate
O
SO4-2
sulfate
O
O
H
O
S
-
O
HSO4bisulfate
-
-
-
O
O
O
O
+
H
-
HPO4-2
monohydrogen phosphate
-
O
O
P
O
S
H2SO4
sulfuric acid
O
H2PO4dihydrogen phosphate
H
O
O
H2PO4dihydrogen phosphate
O
O
O
O
H2SO3
sulfurous acid
H
H+
+
H
O
S
O
-
HSO3bisulfite
41
Formulas and Names Involving Polyatomic Ions:
Compounds containing polyatomic ions are named the same as binary compounds.
Formulas containing polyatomic ions are written the same as binary compounds, with one
difference …
sodium chloride is NaCl
calcium chloride is CaCl2
Parentheses are not placed around monatomic ions
like Cl-, even when several are present in the formula.
sodium hydroxide is NaOH
calcium hydroxide is Ca(OH)2
Parentheses are placed around polyatomic ions like
OH-, only when several are present in the formula.
Ammonium hydroxide, NH4OH, contains two polyatomic ions, the ammonium cation, NH4+, and
the hydroxide anion, OHIn ammonium cyanide, NH4CN, the N atom occurs twice.
They remain separate so that the both the ammonium cation, NH4+, and the cyanide anion, CN-,
are recognized.
42
Practice: Write names or formulas in the empty cells. Use the Stock System.
Formula
Zn(C2H3O2)2
Fe(C2H3O2)3
Cr(NO2)6
Mn(NO3)7
Al2(SO4)3
Al(HSO4)3
K2SO3
Fe(HSO3)2
Ni(ClO4)2
Sn(ClO3)2
Pb(ClO2)4
HgBrO
Co(BrO3)3
Cr(BrO4)3
Name
zinc acetate
iron(III) acetate
chromium(VI) nitrite
manganese(VII) nitrate
aluminum sulfate
aluminum bisulfate
potassium sulfite
iron(II) bisulfite
nickel(II) perchlorate
tin(II) chlorate
lead(IV) chlorite
mercury(I) hypobromite
cobalt(III) bromate
chromium(III) perbromate
ions & Ox #’s
Zn+2 CH3COOFe+3 CH3COOCr+6 NO2Mn+7 NO3Al+3 SO4-2
Al+3
HSO4K+
SO3-2
Fe+2
HSO3Ni+2
ClO4Sn+2
ClO3Pb+4
ClO2Hg+
BrOCo+3 BrO3Cr+3
BrO443
Practice: Write names or formulas in the empty cells. Use the Stock System.
Formula
Sr(IO2)2
(NH4)2SO4
LiIO
Be(IO3)2
Cu(BrO2)2
Al2(CO3)3
Cu(HCO3)2
Ba3(PO4)2
Cd(IO4)2
W(CN)6
Mo(CO3)3
V2(SO3)5
Pt3(PO4)4
Hg(HSO4)2
Name
strontium iodite
ammonium sulfate
lithium hypoiodite
beryllium iodate
copper(II) bromite
aluminum carbonate
copper(II) bicarbonate
barium phosphate
cadmium periodate
tungsten(VI) cyanide
molybdenum(VI) carbonate
vanadium(V) sulfite
platinum(IV) phosphate
mercury(II) bisulfate
ions & Ox #’s
Sr+2
IO2NH4+ SO4-2
Li+
IOBe+2
IO3Cu+2
BrO2Al+3
CO3-2
Cu+2 HCO3Ba+2
PO4-3
Cd+2
IO4W+6
CNMo+6 CO3-2
V+5
SO3-2
Pt+4
PO4-3
Hg+2
HSO444
In most oxyacids, adding or subtracting O’s to a formula does not change the number of ionizable H’s.
HNO3 and HNO2 are both monoprotic acids.
H2SO4 and H2SO3 are both diprotic acids.
HClO4, HClO3, HClO2 and HClO are all monoprotic acids.
The oxyacids of P are unique. H3PO4 is triprotic, but H3PO3 is only diprotic, and H3PO2 is monoprotic.
Examine the structures of these oxyacids and note that acidic H’s are bonded to O, not to P.
O
H
O
acidic H
O
P
O
O
H
H3PO4
phosphoric acid
triprotic
H
H
O
acidic H
bonded to O
P
O
H
O
H
H
H3PO3
phosphorous acid
diprotic
P
O
H
H
nonacidic H
not bonded to O
H3PO2
hypophosphorous acid
monoprotic
45
O
H
O
O
P
O
O
H
H
H3PO4, phosphoric acid
- H+
H
O
O
P
O
O
H
- H+
-
H
O
P
O
H2PO4-, dihydrogen phosphate
O
O
- H+
-
-
O
P
-
O
HPO4-2, monohydrogen phosphate
O
-
-
PO4-3, phosphate
Because phosphorous acid (H3PO3) has only two ionizable H’s, HPO3-2 is fully ionized and can be named
monohydrogen phosphite or simply ‘phosphite’.
O
H
O
P
O
- H
H
O
O
+
H
H
O
P
O
-
- H+
-
O
P
-
H
H
HPO3-2, monohydrogen phosphite
or simply ‘phosphite’
H2PO3-, dihydrogen phosphite
H3PO3, phosphorous acid
O
Because hypophosphorous acid (H3PO2) has only one ionizable H, H2PO2- is fully ionized and can be named
dihydrogen hypophosphite or simply ‘hypophosphite’.
O
O
H
P
O
H
H
H3PO2, hypophosphorous acid
H+
+
H
P
O
-
H
H2PO2-, dihydrogen hypophosphite
or simply ‘hypophosphite’
46
As we are seeing, there are several conventions for naming the anions of partly ionized polyprotic acids.
The student has latitude here, however, any correct name must identify the compound unambiguously.
Try naming the following compounds using more than one correct name.
Formula
H3PO4
NaH2PO4
K2HPO4
LiH2PO3
Ag2HPO3
NaH2PO2
(NH4)2HPO4
(NH4)2HPO3
NH4H2PO4
(NH4)2KPO4
Name
phosphoric acid or hydrogen phosphate
sodium dihydrogen phosphate or monosodium phosphate
potassium monohydrogen phosphate or dipotassium phosphate
lithium dihydrogen phosphite or monolithium phosphite
silver monohydrogen phosphite or silver phosphite
sodium dihydrogen hypophosphite or sodium hyposphosphite
diammonium monohydrogen phosphate or diammonium phosphate
diammonium monohydrogen phosphite or ammonium phosphite
ammonium dihydrogen phosphate or monoammonium phosphate
diammonium potassium phosphate
ions & Ox #’s
H+
PO4-3
Na+
H2PO4K+
HPO4-2
Li+
H2PO3Ag+
HPO3-2
Na+
H2PO2NH4+ HPO4-2
NH4+ HPO3-2
NH4+ H2PO4NH4+ K+ PO4-3
The number of H’s need not be stated, provided the number of other cations is explicitly stated in the name.
Prefixes like ‘di’ or ‘tri’ should only be used when partially ionized polyprotic acids are being named.
47
For compounds of monovalent cations (Li+, Na+, K+, NH4+, etc.) we have seen that there are several
acceptable names …
e.g., K2HPO4 = dipotassium monohydrogen phosphate or potassium monohydrogen phosphate
or dipotassium phosphate
However, when polyvalent cations, like Ca+2, Al+3, etc. are combined with partially ionized acids, the
convention is to state the number of H’s but not the number of polyvalent metal cations, as follows …
Ca(H2PO4)2
CaHPO4
Al(H2PO4)3
Al2(HPO4)3
Fe2(HPO4)3
SnHPO4
Pb(H2PO3)4
Pd(H2PO2)4
Pd(H2PO2)2
calcium dihydrogen phosphate
calcium monohydrogen phosphate
aluminum dihydrogen phosphate
aluminum monohydrogen phosphate
iron(III) monohydrogen phosphate
tin(II) monohydrogen phosphate
lead(IV) dihydrogen phosphite
palladium(IV) dihydrogen hypophosphite or palladium(IV) hypophosphite
palladium(II) dihydrogen hypophosphite or palladium(II) hypophosphite
Ca+2
Ca+2
Al+3
Al+3
Fe+3
Sn+2
Pb+4
Pd+4
Pd+2
H2PO4HPO4-2
H2PO4HPO4-2
HPO4-2
HPO4-2
H2PO3H2PO2H2PO248
Practice: Write the name or formula of the following compounds. Spelling counts.
The column on the right will not be marked.
Formula
Mg(CH3COO)2
(NH4)2SO4
Fe2(CO3)3
Ba(NO3)2
Mn(ClO2)7
Cd(IO4)2
AlH3
Be3N2
Hg(BrO)2
H2SO3
HClO3
(NH4)2HPO4
Zn(H2PO2)2
Stock System Name
magnesium acetate
ammonium sulfate
iron(III) carbonate
barium nitrate
manganese(VII) chlorite
cadmium periodate
aluminum hydride
beryllium nitride
mercury(II) hypobromite
sulfurous acid
chloric acid
ammonium monohydrogen phosphate or diammonium phosphate
zinc dihydrogen hypophosphite or zinc hypophosphite
Ox # & Charges
Mg+2
CH3COONH4+
SO4-2
Fe+3
CO3-2
Ba+2
NO3Mn+7
ClO2Cd+2
IO4Al+3
HBe+2
N-3
Hg+2
BrOH+
SO3-2
H+
ClO3NH4+ HPO4-2
Zn+2
H2PO249
Other Common Acids: A few other inorganic acids are commonly encountered in the laboratory. Study the
structures and names of these acids and their anions.
O
O
Mn
O
H+
H
+ O
O
Mn
permanganate, MnO4-
O
O
Cr
O
H
2
H+
-
+
O
Cr
O
Cr
O
O
-
O
chromate, CrO4-2
chromic acid, H2CrO4
O
Chromic acid, H2CrO4, is a diprotic acid and strong
oxidizer. Its potassium salt, potassium chromate,
K2CrO4, is used as an indicator for measurement of
chloride by silver nitrate titration.
Cr is in its highest oxidation state, +6, (which
contributes to its strength as an oxidizer).
O
O
H
-
O
O
permanganic acid, HMnO4
H
Permanganic acid, HMnO4, is monoprotic.
Its potassium salt, potassium permanganate (KMnO4) is
a dark purple-colored reagent that is often used in the
lab as a strong oxidizing titrant.
Mn is in its highest oxidation state, +7, (which
contributes to its strength as an oxidizer).
O
O
O
O
Cr
O
O
dichromic acid, H2Cr2O7
H
2
H+
+
-
O
Cr
O
O
O
Cr
O
-
O
dichromate, Cr2O7-2
Dichromic acid, H2Cr2O7 is another
strongly oxidizing diprotic acid. Its
potassium salt, potassium dichromate
( K2Cr2O7) is a common lab reagent.
Can you calculate the Ox # of Cr in it?
50
Potassium permanganate, KMnO4, is a very dark purple,
crystalline solid.
The permanganate ion, MnO4-, is released when dissolved in
water, giving rise to bright purple solutions.
Potassium chromate, K2CrO4, is a bright yellow, crystalline
solid.
Aqueous solutions of this reagent are bright yellow owing to
the presence of the chromate ion, CrO4-2.
Bright orange potassium dichromate, K2Cr2O7, when dissolved
in water, releases the dichromate ion, Cr2O7-2.
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Practice: Write the name or formula of the following compounds. Spelling counts.
Formula
Fe(MnO4)3
Ag2CrO4
ZnCr2O7
Al2(CrO4)3
Na2Cr2O7
V2(Cr2O7)5
Mn2(SO4)7
Cr(PO4)2
Mo(MnO4)6
Cd(IO4)2
Co(BrO3)3
Ni(ClO2)2
Mg(BrO)2
Almost Finished
Stock System Name
iron(III) permanganate
silver chromate
zinc dichromate
aluminum chromate
sodium dichromate
vanadium(V) dichromate
manganese(VII) sulfate
chromium(VI) phosphate
molybdenum(VI) permanganate
cadmium periodate
cobalt(III) bromate
nickel(II) chlorite
magnesium hypobromite
Ox # & Charges
Fe+3
MnO4Ag+
CrO4-2
Zn+2
Cr2O7-2
Al+3
CrO4-2
Na+
Cr2O7-2
V+5
Cr2O7-2
Mn+7
SO4-2
Cr+6
PO4-3
Mo+6
MnO4Cd+2
IO4Co+3
BrO3Ni+2
ClO2Mg+2
BrO52
Name the following compounds using the “ous-ic” system.
Formula
PbCl2
PbCl4
SnBr2
SnBr4
Cu2O
CuO
FeO
Fe2O3
Au2S3
PtF2
Pt(NO3)4
Hg(ClO4)2
Hg2SO3
Ous-Ic Name
plumbous chloride
plumbic chloride
stannous bromide
stannic bromide
cuprous oxide
cupric oxide
ferrous oxide
ferric oxide
auric sulfide
platinous fluoride
platinic nitrate
mercuric perchlorate
mercurous sulfite
Stock System Name
lead(II) chloride
lead(IV) chloride
tin(II) bromide
tin(IV) bromide
copper(I) oxide
copper(II) oxide
iron(II) oxide
iron(III) oxide
gold(III) sulfide
platinum(II) fluoride
platinum(IV) nitrate
mercury(II) perchlorate
mercury(I) sulfite
53
Congrats, you just completed inorganic chemical nomenclature
part 2 on Polyatomic Compounds
There is also a previous video dealing with the nomenclature of
Binary Compounds.
Youtube
‘Inorganic Chemical Nomenclature Part 1 Binary Compounds’
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