Chemical Nomenclature

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Chemical Nomenclature

• Ionic Compounds
• often a metal nonmetal
• anion (nonmetal), add ide to element name

BaCl2
barium chloride
Known as a subscript
K2O
potassium oxide
Mg(OH)2
magnesium hydroxide
KNO3
potassium nitrate
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An ion is an atom, or group of atoms, that has a
net positive or negative charge.
cation ion with a positive charge If a neutral
atom loses one or more electrons it becomes a
cation.
anion ion with a negative charge If a neutral
atom gains one or more electrons it becomes an
anion.
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Forming Cations Anions
A CATION forms when an atom loses one or more
electrons.
An ANION forms when an atom gains one or more
electrons
F e- --gt F-
Mg --gt Mg2 2 e-
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Do You Understand Ions?
13 protons, 10 (13 3) electrons
34 protons, 36 (34 2) electrons
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A monatomic ion contains only one atom
Na, Cl-, Ca2, O2-, Al3, N3-
A polyatomic ion contains more than one atom
OH-, CN-, NH4, NO3-
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Compound Names and Formulas
A. Naming ionic compounds
1. Ionic - transfer of electrons - causing one
element to become a positive ion (cation) and
one element to become a negative ion (anion)
2. the positive ion always come first
NaCl is never written as ClNa
3. The name is derived from the ions that make it
up
a. naming binary ionic compounds - two elements
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i. the positive ion is simply the name ion the
element
ii. Na is sodium
Ba is Barium
b. the negative ions ending is changed to ide
i. chlorine - Cl is changed to Cl- - chloride
c. some polyatomic ions are name according to
their oxygen content
Sulfate and sulfite
SO4-- and SO3--
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d. Some cations must show their charge
Fe is known as the Iron II ion
Feis known as the Iron III ion
e. when writing chemical formulas from their
names - the number of positive ions must equal
the number of negative ions
Sodium fluoride
NaF - - these charges are balanced
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Calcium chloride
CaCl- - these charges are not balanced so we
must adjust the subscripts so the number of
equals the number of -
CaCl2-
Remember - Charges must be balanced - so you must
have 2 -1s to balance the 2
Coefficient
subscript
2NH4 CO3-2 gt (NH4 ) 2 CO3-2
Ammonium
carbonate
carbonate
Ammonium
Use coefficients to balance the total number of
atoms - Always balance charges first using
subscripts
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1 with -1
Ammonium with acetate
NH4 C2H3O2- gt NH4 C2H3O2-
Ammonium
acetate
Ammonium Acetate
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Cu1 C2H3O2- gt Cu1C2H3O2-
copper (I)
acetate
copper (I) acetate
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1 with -2
There is an issue
CO3 --
NH4
NH4

(
)
2
CO3 --
2
Ammonium carbonate
Carbonate
Ammonium
You must make the charges equal
now you must balance it according to the
conservation of mass
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1 with -3
You must always have the charges equal - so
must have 3 1 with the -3
3NH4 PO4 -3 gt (NH4)3PO4-3
Ammonium
phosphate
phosphate
Ammonium
2 with -1
You must always have the charges equal - so must
have 2 -1s to equal the 2
Ca2 2C2H3O2 -1 gt Ca2(C2H3O2-)2
Calcium
acetate
acetate
Calcium
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2 with -2
Since the charges are equal - you simply put them
together
Ca 2 CO3 -2 gt CaCO3
Carbonate
Calcium
Calcium
Carbonate
2 with -3
Since the charges are not equal - you must find
the LCD for 2 and 3 which is 6 so
3Ca 2 2 PO4 -3 gt Ca23(PO4 -3 )2
Calcium
Phosphate
Calcium
Phosphate
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3 with -1
Al3 3 C2H3O2- ? Al3(C2H3O2-)3
Aluminum
Acetate
Aluminum Acetate
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3 with -2
2Al3 3CO3 -- ? Al32 (CO3 --)3
Aluminum
Carbonate
Aluminum Carbonate
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3 with -3
Al PO4 --- ? AlPO4 ---
Aluminum
Phosphate
Aluminum Phosphate
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A molecular formula shows the exact number of
atoms of each element in the smallest unit of a
substance
An empirical formula shows the simplest
whole-number ratio of the atoms in a substance
H2O
CH2O
C6H12O6
O3
O
N2H4
NH2
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• Molecular compounds
• nonmetals or nonmetals metalloids
• common names
• H2O, NH3, CH4, C60
• element further left in periodic table is 1st
• element closest to bottom of group is 1st
• if more than one compound can be formed from the
  same elements, use prefixes to indicate number of
  each kind of atom
• last element ends in ide

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Molecular Compounds
HI
hydrogen iodide
NF3
nitrogen trifluoride
SO2
sulfur dioxide
N2Cl4
dinitrogen tetrachloride
NO2
nitrogen dioxide
N2O
dinitrogen monoxide
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Mixed Practice

• Dinitrogen monoxide
• Potassium sulfide
• Copper (II) nitrate
• Dichlorine heptoxide
• Chromium (III) sulfate
• Iron(III) sulfite
• Calcium oxide
• Barium carbonate
• Iodine monochloride

1. N2O
2. K2S
3. Cu(NO3)2
4. Cl2O7
5. Cr2(SO4)3
6. Fe2(SO3)3
7. CaO
8. BaCO3
9. ICl

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Mixed Practice

• BaI2
• P4S3
• Ca(OH)2
• FeCO3
• Na2Cr2O7
• I2O5
• Cu(ClO4)2
• CS2
• B2Cl4

1. Barium iodide
2. Tetraphosphorus trisulfide
3. Calcium hydroxide
4. Iron (II) carbonate
5. Sodium dichromate
6. Diiodine pentoxide
7. Cupric perchlorate
8. Carbon disulfide
9. Diboron tetrachloride

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Examples of Older Names of Cations formed from
Transition Metals(memorize these!!)
From Zumdahl
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An acid can be defined as a substance that yields
hydrogen ions (H) when dissolved in water.

• HCl
• Pure substance, hydrogen chloride
• Dissolved in water (H Cl-), hydrochloric acid

An oxoacid is an acid that contains hydrogen,
oxygen, and another element.
HNO3
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• Transition metal ionic compounds
• indicate charge on metal with Roman numerals

iron(II) chloride
FeCl2
2 Cl- -2 so Fe is 2
FeCl3
3 Cl- -3 so Fe is 3
iron(III) chloride
Cr2S3
3 S-2 -6 so Cr is 3 (6/2)
chromium(III) sulfide
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Oxidation and reduction
1. Oxidation and reduction (redox reactions)
A. Oxidation - loss of electrons
B. Reduction - gain of electrons
Oxidation-reduction reactions MUST happen at the
same time
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C. Oxidation numbers - number of electrons
gained, lost or shared
1. how to assign oxidation numbers
a. free elements are assigned an oxidation
number of zero
i. free element - any un- combined element -
this includes the 7 diatomics
H2, N2, O2, F2, Cl2, Br2, I2
These 7 elements must be together if they are
alone
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b. mono atomic ion's charge equals their
oxidation number
i. Na1 1
ii. S-2 -2
c. hydrogen's oxidation is 1
d. oxygen's oxidation number is -2 except in
peroxides. In peroxides, the oxidation is -1
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e. the sum of the oxidation numbers of a
compound must add up to be zero
f. the sum of the oxidation numbers of
a polyatomic ion must add up to equal its
charge
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1. The oxidation number of hydrogen is 1 except
   when it is bonded to metals in binary compounds.
   In these cases, its oxidation number is 1.

1. Group IA metals are 1, IIA metals are 2 and
   fluorine is always 1.

6. The sum of the oxidation numbers of all the
atoms in a molecule or ion is equal to the charge
on the molecule or ion.
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1
-2
HCO3-
1
-6
?
-1
4
H 1
O -2
C 4
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Oxidation number
The charge the atom would have in a molecule (or
an ionic compound) if electrons were completely
transferred.

1. Free elements (uncombined state) have an
   oxidation number of zero.

Na, Be, K, Pb, H2, O2, P4 0

1. In monatomic ions, the oxidation number is equal
   to the charge on the ion.

Li, Li 1 Fe3, Fe 3 O2-, O -2

1. The oxidation number of oxygen is usually 2. In
   H2O2 and O22- it is 1.

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Try some
find the oxidation numbers for each element


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Formula of Ionic Compounds
Al2O3
Al3
O2-
CaBr2
Ca2
Br-
Na2CO3
Na
CO32-
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NH4Br-
Ca2Cl-2
NaC2H3O2-
Cu2SO4-
KHCO3-
Ba2(NO3-)2
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Zn2S-2
Li3PO4-3
Al3(HSO4-)3
Fe3 2O-2 3
Zn2CO3-2
HCN-
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Ag 2 Cr2O7 -2
Fe3PO3 -3
H2 O2-2
Ca2 HPO4-2
CuNO2-
Cu2 (NO2- )2
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Hg2C2O4-2
Cr3(OH- )3