Chemistry: Atoms First
Julia Burdge & Jason Overby
Chapter 5
Naming Ionic and
Covalent Compounds
Homework: Chapter 5. 23, 25, 27,
55, 61, 63, 99 and 111
Kent L. McCorkle
Cosumnes River College
Sacramento, CA
Copyright (c) The McGraw-Hill Companies, Inc. Permission required for reproduction or display.
5.1
Compounds
A compound is a substance composed of two or more elements
combined in a specific ratio and held together by chemical bonds.
Familiar examples of compounds are water and salt (sodium
chloride).
Ionic Compounds and Bonding
The resulting electrically neutral compound, sodium chloride, is
represented with the chemical formula NaCl.
The chemical formula, or simply formula, of an ionic compound
denotes the constituent elements and the ratio in which they
combine.
5.4
Naming Ions and Ionic Compounds
A monatomic ion is named by changing the ending of the element’s
name to –ide.
Cl– is chloride
O2– is oxide
Some metals can form cations of more than one possible charge.
Fe2+ : ferrous ion [Fe(II)]
Fe3+ : ferric ion [Fe(III)]
Mn2+ : manganese(II) ion
Mn3+ : manganese(III) ion
Mn4+ : manganese(IV) ion
Naming Ions and Ionic Compounds
Naming Ions and Ionic Compounds
Formulas for ionic compounds are generally empirical formulas.
Ionic compounds are electronically neutral.
Formulas of Ionic Compounds
In order for ionic compounds to be electronically neutral, the sum
of the charges on the cation and anion in each formula must be
zero.
Aluminum oxide:
Al3+
O2–
Al2O3
Sum of charges:
2(+3) + 3(–2) = 0
Formulas of Ionic Compounds
Naming Ions and Ionic Compounds
To name ionic compounds:
1) Name the cation
 omit the word ion
 use a Roman numeral if the cation can have more than one
charge
2) Name the anion
 omit the word ion
Examples:
NaCN sodium cyanide
FeCl2 iron(II) chloride
FeCl3 iron(III) chloride
5.7
Covalent Bonding in Ionic Species
Polyatomic ions consist of a combination of two or more atoms.
Formulas are determined following the same rule as for ionic
compounds containing only monatomic ions: ions must combine in
a ratio that give a neutral formula overall.
Calcium phosphate:
Ca2+
PO43–
Ca3(PO4)2
Sum of charges:
3(+2) + 2(–3) = 0
Covalent Bonding in Ionic Species
Covalent Bonding in Ionic Species
Worked Example 5.9
Name the following ionic compounds: (a) Fe2(SO4)3, (b) Al(OH)3, and (c) Hg2O.
Strategy Begin by identifying the cation and anion in each compound, and then
combine the names for each, eliminating the word ion.
Solution (a) Fe2(SO4)3 is iron(III) sulfate.
(b) Al(OH)3 is aluminum hydroxide.
(c) Hg2O is mercury(I) oxide.
Think About It Be careful not to confuse the subscript in the formula with the
charge in the metal ion. In part (a), for example, the subscript on Fe is 2, but this
is an iron(III) compound.
Covalent Bonding in Ionic Species
Oxoanions are polyatomic anions that contain one or more oxygen
atoms and one atom (the “central atom”) of another element.
Starting with the oxoanions that end in –ate, we can name these
ions as follows:
1) The ion with one more O atom than the –ate ion is called the
per…ate ion. Thus, ClO3- is the chlorate ion, so ClO4- is the
perchlorate ion.
2) The ion with one less O atom than the –ate ion is called the –ite
ion. Thus, ClO2- is the chlorite ion.
3) The ion with two fewer O atom than the –ate ion is called the
hypo…ite ion. Thus, ClO- is the hypochlorite ion.
At minimum, memorize the oxoanions that end in –ate so you can
apply these guidelines when necessary.
Covalent Bonding in Ionic Species
perchlorate
chlorate
chlorite
hypochlorite ClO-
ClO4ClO3ClO2-
nitrate
nitrite
NO3NO2-
phosphate
phosphite
PO43PO33-
sulfate
sulfite
SO42SO32-
Worked Example 5.10
Name the following species: (a) BrO4-, (b) HCO3-, and (c) H2CO3.
Strategy Each species is either an oxoanion or an oxoacid. Identify the
“reference oxidation” (the one with the –ate ending) for each, and apply the rules
to determine appropriate names.
Think
It Remembering
all these
names
and formulas
Solution
(a)About
BrO4- has
one more O atom
than the
bromate
ion (BrOis3-), so BrO4greatly facilitated
is the perbromate
ion. by memorizing the common ions that end in –ate.
chlorate
ClO3nitrate
(b) CO32- is the carbonateNO
ion.
3 Because HCO3 has one ionizable hydrogen atom,
iodate carbonateIOion.
it is called the hydrogen
3
carbonate
CO32bromatehydrogen atoms
BrO3- and no charge on the oxalate
(c) With two ionizable
compound, H2CO3 is
C2O42carbonic acid.
sulfate
SO42chromate
Think About It Make sure
2- the charges sum to zero in each compound
CrO4that
formula. In partphosphate
(a), for example, PO
Hg2+3- + 2Cl- = (+2) + 2(-1) =
0; in part (b),
permanganate
4
(+2) + 2(-1) = 0;MnO
and in
- part (c), 3(+1) + (-3) = 0.
4
Worked Example 5.11
Determine the formula of sulfurous acid.
Strategy The –ous ending in the name of an acid indicates that the acid is
derived from an oxoanion ending in –ite. The oxoanion must be sulfite, SO32-, so
add enough hydrogen ions to make a neutral formula.
Solution The formula of sulfurous acid is H2SO3.
Think About It Remembering all these names and formulas is greatly facilitated
by memorizing the common ions that end in -ate.
Hydrates
A hydrate is a compound that has a specific number of water
molecules within its solid structure.
For example, in its normal state, copper(II) sulfate has five water
molecules associated with it.
Systematic name: copper(II) sulfate pentahydrate
Formula: Cu(SO)4 ∙ 5H2O
Some other hydrates are
BaCl2 ∙ 2H2O
LiCl ∙ H2O
MgSO4 ∙ 7H2O
Sr(NO3)2 ∙ 4H2O
Hydrates
When the water molecules are driven off by heating, the resulting
compound, Cu(SO)4, is sometimes called anhydrous copper(II)
sulfate.
Anhydrous means the compound no longer has water molecules
associated with it.
Familiar Inorganic Compounds
Covalent Bonding and Molecules
Covalent Bonding and Molecules
A chemical formula denotes the
composition of the substance.
A molecular formula shows the exact
number of atoms of each element in a
molecule.
Some elements have two or more distinct
forms known as allotropes.
 For example, oxygen (O2) and ozone
(O3) are allotropes of oxygen.
A structural formula shows not only the
elemental composition, but also the
general arrangements.
Covalent Bonding and Molecules
Molecular substances can also be represented using empirical
formulas, the whole-number ratio of elements.
While, the molecular formulas tell us the actual number of atoms (the
true formula), the empirical formula gives the simplest formula.
Molecular formula: N2H4
Empirical formula: NH2
The molecular and empirical formulas are often the same.
Covalent Bonding and Molecules
5.6
Naming Molecular Compounds
Remember that binary molecular compounds are substances that
consist of just two different elements.
Nomenclature:
1)
Name the first element that appears in the formula.
2)
Name the second element that appears in the formula,
changing
its ending to –ide.
Examples:
HCl
HI
hydrogen chloride
hydrogen iodide
Naming Molecular Compounds
Greek prefixes are used to denote the number of atoms of each
element present.
Naming Molecular Compounds
The prefix mono- is generally omitted for the first element.
For ease of pronunciation, we usually eliminate the last letter of a
prefix that ends in “o” or “a” when naming an oxide.
Example: N2O5 is dinitrogen pentoxide not dinitrogen
pentaoxide
Worked Example 5.7
Name the following binary molecular compounds: (a) NF3 and (b) N2O4.
Strategy Each compound will be named using the systematic nomenclature
including, where necessary, appropriate Greek prefixes.
Solution (a) nitrogen trifluoride
(b) dinitrogen tetroxide
Think About It Make sure that the prefixes match the subscripts in the
molecular formulas and that the word oxide is not preceded immediately by an
“a” or an “o”.
Worked Example 5.8
Write the chemical formulas for the following binary molecular compounds:
(a) sulfur tetrafluoride and (b) tetraphosphorus decasulfide.
Strategy The formula for each compound will be deduced using the systematic
nomenclature guidelines.
Solution (a) SF4
(b) P4S10
Think About It Double-check that the subscripts in the formulas match the
prefixes in the compound names: (a) 4 = tetra and (b) 4 = tetra and 10 = deca.
Compounds Containing Hydrogen
The names of molecular compounds containing hydrogen do not
usually conform to the systematic nomenclature guidelines.
Many are called by the common, nonsystematic names or by names
that do not indicate explicitly the number of H atoms present.
Examples:
B2H6
SiH4
NH3
PH3
H2O
H2S
Diborane
Silane
Ammonia
Phosphine
Water
Hydrogen sulfide
Compounds Containing Hydrogen
One definition of an acid is a substance that produces hydrogen
ions (H+) when dissolved in water.
HCl is an example of a binary compound that is an acid when
dissolved in water.
To name these types of acids:
1) remove the –gen ending from hydrogen
2)
change the –ide ending on the second element to –ic.
hydrogen chloride → hydrochloric acid
Compounds Containing Hydrogen
A compound must contain at least one ionizable hydrogen atom to
be an acid upon dissolving.
Organic Compounds
Our nomenclature discussion so far has focused on inorganic
compounds, generally defined as those without carbon.
Organic compounds contain carbon and hydrogen, sometimes in
combination with other atoms.
Hydrocarbons contain only carbon and hydrogen.
The simplest hydrocarbons are called alkanes.
Organic Compounds
Organic Compounds
Organic Compounds
Many organic compounds contain groups of atoms known as
functional groups, which often determine a molecule’s reactivity.
A molecule is an aggregate of two or more atoms in a
definite arrangement held together by chemical bonds
H2
H2O
NH3
CH4
A diatomic molecule contains only two atoms
H2, N2, O2, Br2, HCl, CO
A polyatomic molecule contains more than two atoms
O3, H2O, NH3, CH4
Writing Chemical Formals
There are 7 elements that occur in nature as a diatomic molecule
One way to remember these
elements is:
Mr. BrINClHOF
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-
2.5
Guidelines for Writing Chemical Formulas
for Binary Compounds
1. Except for Hydrogen, the element farther to the left in the
periodic table appears first. Ie: KCl, PCl3, Al2S3, and Fe3O4
2. If hydrogen is present, it appears last except when the other
element is from group 16 or 17. Ie: LiH, NH3, B2H6, CH4
H2O, HCl and HI
3. If both elements are from the same group, the lower one
appears first. Ie: SiC and BrF3
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
molecular
empirical
H2O
H2O
C6H12O6
CH2O
O3
O
N2H4
NH2
ionic compounds consist of a combination of cations
and an anions
• the formula is always the same as the empirical formula
• the sum of the charges on the cation(s) and anion(s) in each
formula unit must equal zero
The ionic compound NaCl
Formula of Ionic Compounds
2 x +3 = +6
3 x -2 = -6
Al2O3
Al3+
1 x +2 = +2
Ca2+
1 x +2 = +2
Na+
O22 x -1 = -2
CaBr2
Br1 x -2 = -2
Na2CO3
CO32-
M
Ion
Name (common name)
Ion
Name (Common name)
NH4+
Ammonium
CO32-
Carbonate
H3O+
Hydronium
HCO3-
OH-
Hydroxide
SO32-
Hydrogen carbonate
(bicarbonate)
Sulfite
CN-
Cyanide
HSO3-
Hydrogen sulfite
NO2-
Nitrite
SO42-
Sulfate
NO3-
Nitrate
HSO4-
Hydrogen sulfate
Thiocyanate
ClO2-
Hypochlorite (often
written OCl-)
Chlorite
SCNS2O32-
Thiosulfate
ClO3-
Chlorate
CrO42-
Chromate
ClO4-
Perchlorate
Cr2O72-
Dichromate
MnO4-
Permanganate
PO43-
Phosphate
CH3CO
Acetate (can be written
C2H3O2-)
Oxalate
HPO42-
Hydrogen phosphate
H2PO4-
Dihydrogen phospate
ClO-
2
C2O42-
U
S
T
K
N
O
W
Recognizing Ionic Compounds
A compound is ionic if it contains a metal from group 1
Or group 2 or one of the polyatomic ions. Binary metal
Oxides and sulfides also have ionic character
F ig 2 -2 3
Pg 59
C ou rtes y K en K arp
P u re w ater(left)
an d a so lu tion
o f su gar(righ t)
d o n o t co nd u ct
electricity
b ecau se th ey
co n tain virtu ally
n o io n s. A
so lu tio n o f salt
(cen ter)
co n du cts
electricity w ell
b ecau se it
co n tain m o b ile
catio n s and
an io n s.
Chemical Nomenclature
• Ionic Compounds
– often a metal + nonmetal
– anion (nonmetal), add “ide” to element name
BaCl2
barium chloride
K2O
potassium oxide
Mg(OH)2
magnesium hydroxide
KNO3
potassium nitrate
Cations of Variable Charge
Transition metals such as copper may form cations
Of different charge. This is represented by placing a
Roman numeral after the transition metal in
Parentheses after the name of the metal.
CuO Copper(II) oxide
Cu2O Copper(I) oxide
• Transition metal ionic compounds
– indicate charge on metal with Roman numerals
FeCl2
2 Cl- -2 so Fe is +2
iron(II) chloride
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
• 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
Molecular Compounds
HI
hydrogen iodide
NF3
nitrogen trifluoride
SO2
sulfur dioxide
N2Cl4
dinitrogen tetrachloride
NO2
nitrogen dioxide
N2O
dinitrogen monoxide
TOXIC!
Laughing Gas
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
nitric acid
H2CO3
carbonic acid
H2SO4
sulfuric acid
HNO3
A base can be defined as a substance that yields
hydroxide ions (OH-) when dissolved in water.
NaOH
sodium hydroxide
KOH
potassium hydroxide
Ba(OH)2
barium hydroxide
Hydrates
A hydrate is an ionic compound that has water molecules
Incorporated into their solid structures
Writing the formula: name of ionic compound-# H2O
Pg 89
The Hydrate of copper
sulfate is the pentahydrate,
and the anhydrous copper
sulfate will absorb water
to form the Hydrate.
.
CuSO4 5 H2O
Copper(II)sulfate.pentahydrate
Olmsted Williams
Writing Chemical Formulas
For non ionic compounds with more than 2 atoms
Write Carbon first
Hydrogen second
All other elements in alphabetical order
Let’s try some………………
4 Hydrogen
2 Carbons
4 oxygens
1 Fluorine
1 Sulfur
C2H4FlO4S
4 Carbons
1 Bromine
8 Hydrogen
1 Chlorine
2 Nitrogen
4 Oxygens
C4H8BrClN2O4
4 Iodines
6 Carbons
10 Hydrogens
C6H10I4
Structural Formulas
for Carbon Containing Compounds
Draw a line to show a connection between all elements in a molecule
Carbon makes 4 connections (this makes them central or inside atoms)
Oxygen and Sulfur make 2
Halogens and Hydrogen make 1 (terminal atoms)
Nitrogen makes 3
Let’s try some…………………
C2H5FlO
(This molecule contains
an alcohol (OH)
Fl H
H-C-C-O-H
H H
C4H7ClN (This molecule contains
An amine, NH2)
H H HH
Cl-C-C-C-C-N
HH H H
H
H
Line Formulas
for Carbon Containing Compounds
All ends and corners represent a Carbon
Hydrogens on Carbons are NOT shown
All other elements and Hydrogens not on a Carbon are shown
Let’s try some…………………
(It always helps to draw the structural formula first)
C2H5FlO
(This molecule contains
an alcohol (OH)
Fl H
H-C-C-O-H
H H
O
F
H
C4H7ClN (This molecule contains
An amine, NH2)
H H HH
H
Cl-C-C-C-C-N
H
HH H H
H
N
Cl
H
Naming Carbon Compounds
Prefixes for number of carbons
1
2
3
4
5
6
7
8
9
10
MethEthPropButPentHexHeptOxtNonDec-
If there are only single bonds
The ending is ane
Hydrogens are understood
All other groups attached to a carbon
are listed before the carbon based name
If the compound is circular the
Prefix cyclo is attached
If there is an –OH group attached
The compound ends in ol
Let’s try some problems……………………….