Transcript Ch. 7 (Con`t.) Formula Writing & Naming of Compunds

Ch. 7 (Con’t.)
Formula Writing & Naming
of Compounds
Oxidation numbers
Oxidation numbers
• Oxidation numbers are used to describe
the distribution of electrons among
bonded atoms.
• Covalent bonds involve sharing of
electrons, but oxidation numbers show
what the distribution would be if the
electrons were completely transferred.
Guidelines for Assigning Oxidation Numbers
• The oxidation of any free (uncombined) element
is zero.
• The oxidation number of a monatomic ion is
equal to the charge of the ion.
– e.g. The oxidation number of K+ is +1.
• The oxidation number of each hydrogen atom is
+1, unless it is combined with a metal, then it
has a state of -1.
• The oxidation number of fluorine is always -1.
• The oxidation number of each oxygen atom in
most of its compounds is -2.
Predicting Charges on Monatomic Ions
KNOW THESE !!!!
+1 +2
-3 -2 -1
Cd+2
0
Guidelines for Assigning Oxidation Numbers
• The sum of the oxidation numbers
for all the atoms in a compound is
zero.
• The sum of the oxidation numbers
for all the atoms in a polyatomic
ion is equal to the charge on that
ion.
Example: Determine the oxidation numbers
for each atom in KMnO4
• This compound is made up of a K+ cation and an MnO4anion.
• The K+ is a monatomic ion with a charge of +1, so its
oxidation number is +1.
• Assume that each O atom has an oxidation number of 2.
• The MnO4- has a total charge of -1. There are 4 O
atoms, each with an oxidation number of -2
• The oxidation number of the Mn may be found by the
equation:
– Mn + 4(-2) = -1
• Therefore, the oxidation number of Mn in this compound
is +7.
Example: Determine the oxidation numbers
for each atom in Co(NO2)2
• The anion is the nitrite ion, NO2-.
• Assume that each O atom in the nitrite ion has an
oxidation number of -2.
• The NO2- has a total charge of -1. There are 2 O atoms,
each with an oxidation number of -2
• The oxidation number of the N may be found by the
equation:
– N + 2(-2) = -1
• Therefore, the oxidation number of N in this compound is
+3.
• Since there are two nitrate ions, each with a charge of 1, the charge on the Co must be +2. As an ion, its
oxidation number is equal to its charge.
Chemical Formulas
• Chemical formula– Consists of element symbols and subscripts
C6H12O6
– Formula Units – simplest whole # ratios of ions
present in a compound (for ionic compounds)
– Molecular Formulas- used for covalently bonded
compounds.
• (show EVERY atom present in a molecule)
• Ex. H2O
Water has 2 hydrogen atoms and 1 oxygen atom
Step 1:
Writing Balanced Chemical Formulas
Criss-Cross Rule for Ionic Compounds
Example: Aluminum Chloride
write symbols & charge of elements
Cation (metal) always written 1st!
Step 2:
criss-cross charges as subscripts
Aluminum
Chloride
1-
3+
Cl
Al1
Cl
Al
Step 3:
AlCl3
combine as formula unit
(“1” is never shown) (use smallest whole # ratio)
Make sure you remove charges!!
3
charge on cation “becomes” subscript of anion
charge on anion “becomes” subscript of cation
** Warning: Reduce subscripts to lowest terms.
Ones are not included in formulas!!
Al3+ and O2–
Ba2+ and S2–
In3+ and Br1–
Al2 O3
Ba2 S2
In1 Br3
Al2O3
BaS
InBr3
aluminum oxide
barium sulfide
indium bromide
Criss-Cross Rule
Example: Magnesium Oxide
Step 1:
Magnesium
Step 2:
Mg2+
O2-
Step 3:
Mg 2
O2
Step 4:
Step 5:
Mg2O2
MgO
Oxide
Putting Ions Together
Na+ + Cl- = NaCl
Ca+2 + Cl- = CaCl2
Ca+2 + O-2= CaO
Na+ + O-2 = Na2O
Al+3 + S-2 = Al2S3
Ca+2 + N-3 = Ca3N2
You try these!
Li+ + Br- = LiBr
Mg+2 + F- =
Al+3 + I- =
K+ + Cl- =
AlI3
Sr+2 + P-3 = Sr3P2
MgF2
KCl
Crisscross
• Switch the numerical value of the charges
33
2
2+
Ba N
Ba3 N2
• Reduce ratio if possible
Learning Check
Write the correct formula for the
compounds containing the following ions:
1. Na+, S2a) NaS
b) Na2S
c) NaS2
2. Al3+, Cla) AlCl3
b) AlCl
c) Al3Cl
3. Mg2+, N3a) MgN
b) Mg2N3
c) Mg3N2
Solution
1. Na+, S2b) Na2S
2. Al3+, Cla) AlCl3
3. Mg2+, N3c) Mg3N2
Polyatomic Ions
There are some ions that are made up of more
than one type of atom, these are called
Polyatomic ions – groups of covalently bonded
atoms with a charge
For example, the polyatomic ion known as
ammonium NH4+ has 4 atoms of hydrogen and one
atom of nitrogen, HOWEVER, the whole “group”
has an overall charge of +1
** you need to memorize the formulas & the
charges of many polyatomic ions!
Polyatomic
Ions
-
NO3
nitrate ion
NO2nitrite ion
Naming Ternary Ionic Compounds
 contain at least 3 elements & the 1st is a
metal:
 there MUST be at least one polyatomic ion
(it helps to circle the ions)
 Examples:
NaNO3
Sodium nitrate
K2SO4
Potassium sulfate
Al(HCO3)3
Aluminum bicarbonate
or
Aluminum hydrogen carbonate
What About. . .
What if I have to put multiple polyatomic ions in
a compound, for example, magnesium nitrate?
Magnesium has a charge of +2
Nitrate is polyatomic ion and has a charge of -1
Therefore, we need 2 nitrate ions for each
magnesium
In this case, we put the entire polyatomic ion in
parenthesis and put the subscript outside the
parenthesis
Our answer would be Mg(NO3)2
IONIC COMPOUNDS
remember: they have oppositely-charged ions
in a rigid 3-D pattern
NH4
+
Cl-
ammonium chloride, NH4Cl
Ternary Ionic Nomenclature
Sodium Sulfate
Na+ and SO4 -2
Na2SO4
Iron (III) hydroxide
Fe+3 and OHFe(OH)3
Ammonium carbonate
NH4+ and CO3 –2
(NH4)2CO3
Writing Formulas w/Polyatomic Ions
Reminder! Parentheses are required only
when you need more than one “bunch” of a
particular polyatomic ion.
Ba2 and SO42–
BaSO4
Mg2+ and NO21–
Mg(NO2)2 magnesium nitrite
NH41+ and ClO31–
Sn4+ and SO42–
NH4ClO3 ammonium chlorate
Fe3+ and Cr2O72–
NH41+ and N3–
barium sulfate
Sn(SO4)2
Fe2(Cr2O7)3
(NH4)3N
tin (IV) sulfate
iron (III) dichromate
ammonium nitride
Learning Check
1. aluminum nitrate
a) AlNO3
b) Al(NO)3
c) Al(NO3)3
2. copper(II) nitrate
a) CuNO3
b) Cu(NO3)2
c) Cu2(NO3)
3. Iron (III) hydroxide
a) FeOH
b) Fe3OH
c) Fe(OH)3
4. Tin(IV) hydroxide
a) Sn(OH)4 b) Sn(OH)2
c) Sn4(OH)
• Many polyatomic ions with the same
endings on their names have a different
number of oxygen atoms attached to
the central atom.
• For example
chlorate ClO3-1
sulfate SO4-2
phosphate PO4-3
acetate C2H3O2-1
Polyatomic Ion:
a group of atoms that stay together and have a single, overall charge.
BrO41-
Perbromate ion
CO42ClO41IO41NO41-
PO53SO521 more oxygen
BrO31-
BrO1-
Bromate ion
BrO21-
Bromite ion
CO32-
CO22-
CO2-
ClO31-
ClO21-
ClO1-
IO31-
IO21-
IO1-
NO31-
NO21-
NO1-
PO43-
PO33-
PO23-
SO42-
SO32-
SO22-
“normal”
1 less oxygen
Carbonate ion
Chlorate ion
Iodate ion
Nitrate ion
Phosphate ion
Sulfate ion
Hypobromite ion
2 less oxygen
The table below shows the prefixes and suffixes
that tell the number of oxygen atoms present in
the negative ion.
Salt
metal
polyatomic ion
# Oxygen
atoms
________
per_____ate
1 more O
________
_____ate
common
________
_____ite
1 less O
________ hypo_____ite
________
_____ide
2 less O’s
0 O’s
The oxy-ions of chlorine & bromine all
have these trends in common. Look for
them below……
perchlorate
chlorate
chlorite
Hypochlorite
ClO4-1
ClO3-1
ClO2-1
ClO-1
Perbromate
BrO4-1
Bromate
BrO3-1
Bromite
BrO2-1
Hypobromite BrO-1
The most productive method of committing
these ions to memory is first memorize the
ones that have the -ate ending. This is the
most common ending.
Practice Problem #2
sodium chlorite
Choose the correct formula for the compound
1. NaCl
2. NaClO
3. NaClO2
4. Na(ClO)2
5. none of the above
Periodic Chart
Prefixes
next problem
Naming Compounds
What's in a name? That which we call a rose
by any other name would smell as sweet."
- William Shakespeare, Romeo and Juliet (II, ii)
Naming Compounds
Binary Ionic Compounds (metal & nonmetal):
• 1. Cation first, then anion
• 2. Monatomic cation = name of the
element
• Ca2+ = calcium ion
• 3. Monatomic anion = root + -ide
• Cl- = chloride
• CaCl2 = calcium chloride
Name these ions
Cl1-
N3Br1O2Ga3+
Chloride ion
Nitride ion
Bromide ion
Oxide ion
Gallium ion
Naming Binary Ionic Compounds

Examples:
NaCl
sodium chloride
ZnI2
zinc iodide
Al2O3
aluminum oxide
Formulas to Names: Ternary Compounds
1. Write the names of the ions
KMnO4
I’m a
polyatomic
ion
potassium permanganate
Final Name
If the positive ion has a fixed charge, you are finished.
Formulas to Names: Ternary Compounds
1. Write the names of the ions
NH4NO3
I’m a
polyatomic
ion
ammonium nitrate
Final Name
If the positive ion has a fixed charge, you are finished.
Learning Check
Match each set with the correct name:
1.
Na2CO3
a) magnesium sulfite
MgSO3
b) magnesium sulfate
MgSO4
c) sodium carbonate
2.
Ca(HCO3)2
CaCO3
a) calcium carbonate
b) calcium phosphate
Ca3(PO4)2
c) calcium bicarbonate
Practice Naming Ionic Compounds
• Na2CO3 --
• CaSO4 -• KBr -• MgS -• BeCl2 --
• NH4F --
Multiple Oxidation Numbers
• When the metal in an ionic compound is
multi-valent (has more than 1 charge) there
are 2 naming methods:
– Latin & Stock Systems
• Latin is older (not useful for some
compounds)
• The metal is named with it’s Latin or English
root and ends in -ic or –ous to denote
charge.
• E.g. Cu+1 is cuprous, E.g. Cu+2 is cupric
• Lower = ous, Higher = ic
Write the balanced formula for
copper chloride & name it:
Cu+2 + Cl-1 = CuCl2
= cupric chloride
Cu+1 + Cl-1 = CuCl
= cuprous chloride
For Latin naming: know rules, possible
charges, Latin names, & suffixes
Examples of Older Names of Cations formed from
Transition Metals
Multiple valence: Stock System
• The oxidation number (charge) of the metal
is indicated in parentheses using Roman
numerals
• E.g. Cu1+ is copper(I), Cu2+ is copper(II)
• Numbers refer to charges not to #s of
atoms
• Try: Cu2++Cl-1 & Cu1++Cl-1,
• Cu+2++Cl-1 = CuCl2 = copper (II) chloride
Cu+1 + Cl-1 = CuCl = copper (I) chloride
Formula to Name:
How do I figure out the Roman Numeral??
Hint: We’ve already learned this!
• 1) Assign the element with the unknown
charge a charge of x
• 2) Multiply the charge of each element by
the number of atoms of that element to
get the total charge.
• 3) Add the products from step 2 and set
them equal to zero because compounds are
neutral- zero charge
• 4) Solve for the unknown charge.
Binary Compounds
Containing a Metal of Variable Oxidation Number
To name these compounds, give the name of the metal (Type II
cations) followed by Roman numerals in parentheses to indicate
the oxidation number of the metal, followed by the name of the
nonmetal, with its ending replaced by the suffix –ide.
Examples
Stock System
Traditional (OLD) System
FeCl2
FeCl3
Iron (II) chloride
Iron (III) chloride
Ferrous chloride
Ferric chloride
SnO
SnO2
Tin (II) oxide
Tin (IV) oxide
Stannous oxide
Stannic oxide
(“ic” ending = higher oxidation state;
“ous” is lower oxidation state)
Ternary Ionic Nomenclature
Writing Formulas
• Write each ion, cation first. Don’t show
charges in the final formula.
• Overall charge must equal zero.
– If charges cancel, just write symbols.
– If not, use subscripts to balance charges.
• Use parentheses to show more than one
of a particular polyatomic ion.
• Use Roman numerals indicate the ion’s
charge when needed (Stock System)
How do I figure out the Roman
Numeral?
Solving for the roman numeral
(charge) of Fe2O3
• (2x) + (3)(-2) = 0
– # of Fe atoms times charge of Fe + number of
O atoms times charge of O = zero because
compounds are neutral, no charge
•
•
•
•
•
2x + (-6) = 0
2x – 6 = 0
2x = 6
x= 3
Answer for the name: Iron (III) oxide
Examples #6- Formulas to Names
1. Write the names of the ions
2. Determine the charge of
the positive ion
X = +1
2X + (-2) = 0
2Cux (S)-2 = 0
Cu2S
I’m not a
polyatomic
ion
copper (I) sulfide
Final Name
Examples #1- Formulas to Names
1. Write the names of the ions
CuSO3
x
+2
2. Determine the charge of
the positive ion
Cu
The
the positive
You sum
mustofknow
the
and
negative
charges
charge
on the
sulfite
must
ion isequal
-2 zero
-2 = 0
SO3
X + (- 2)I’m
= 0a
+2
+2
polyatomic
X =
+2
ion
copper (II) sulfite
Final Name
Next
Examples #4- Formulas to Names
1. Write the names of the ions
2. Determine the charge of
the positive ion
X = +2
X + 2(-1) = 0
Snx (F-1)2 = 0
SnF2
tin (II) fluoride
Final Name
Example #3-Names to Formulas
1. Write symbols of elements
X 1
Y= 3
3X = 1y
X(+3) + y(-1) = 0
2. Determine number of ions
(Ni+3)x(C2H3O2-1)y=
0
nickel(III) acetate
Choose the lowest
set of integers that
satisfies the equation
C2H3O2)3
Ni1(C
Formula
If thereFinal
is only
one atom
the “1” is not shown
Next
Practice Problem #1
Fe(NO3)3
Choose the correct name for the compound
1. Iron trinitrate
2. iron(I) nitrate
3. iron(III) nitrite
4. iron(III) nitrate
5. none of the above
Periodic Chart
Polyatomic Ions
next problem
Learning Check
Complete the names of the following binary
compounds with variable metal ions:
FeBr2
iron (_____) bromide
CuCl
copper (_____) chloride
SnO2
___(_____ ) ______________
Fe2O3
________________________
Hg2S
________________________
Nomenclature
for molecular (Covalent) binary
compounds (two nonmetals)
• Uses a Prefix System
• 1 .Less electronegative atom
comes first. (towards left side of P.T.)
• 2. Add numerical prefixes to indicate
# of atoms of each element.
3. Change the ending of the second
element to –ide (since it’s binary)
In order to be effective in using prefixes
to name compounds containing two nonmetals, these prefixes must be
committed to memory:
monoditritetrapentahexa-
1
2
3
4
5
6
heptaoctanonadeca-
7
8
9
10
Naming covalent compounds
1 mono
• prefix refers to # of atoms - not charge
2 di
N2O4 = dinitrogen tetroxide
3 tri • Exception: don’t use mono for first
4 tetra element
CO2 = carbon dioxide
5 penta
6 hexa • The first vowel is often dropped to
avoid the combination of “ao” or “oo”.
7 hepta
CO = carbon monoxide (monooxide)
8 octa
P4O10= tetraphosphorus decoxide
9 nona
(decaoxide)
10 deca
Covalent Compounds: Name to Formula
You’ll like this!
For covalent compounds, simply use the
numerical prefixes to tell you the number
(subscript) of each element
(No charges, No criss-cross, No balancing
needed!):
What is the formula for dinitrogen trioxide?
dinitrogen monoxide?
N2O
N2O3
Example #1-Names to Formulas
Two Non metals:
I’m a Binary
Compound
Sulfur trioxide
1. Write symbols of elements
2. Write number of atoms
S1O3
Final Formula
If no prefix, then 1 is
implied and not written
Example #2-Names to Formulas
I’m a Binary
Compound
dichlorine heptaoxide
1. Write symbols of elements
2. Write number of atoms
Cl2O7
Final Formula
Example #3-Names to Formulas
I’m a Binary
Compound
oxygen difluoride
1. Write symbols of elements
2. Write number of atoms
O1F2
If no prefix, then 1 is
Formula
implied Final
and not
written
Example #4-Names to Formulas
I’m a Binary
Compound
dinitrogen tetraoxide
1. Write symbols of elements
2. Write number of atoms
N2O4
Final Formula
Example #5-Names to Formulas
I’m a Binary
Compound
phosphorus pentachloride
1. Write symbols of elements
2. Write number of atoms
P1Cl5
If no prefix, then 1 is
Final
implied
andFormula
not written
Examples #2- Formulas to Names
1. Write names of elements –
last element ends in -ide
2. Write prefix for number of
atoms
monoxenon
XeF3
I’m a Binary
Compound
tri fluoride
If first prefix is mono, it is
Final Name
implied and not written
Example - Formulas
to Names
1. Write names of elements
(-ide on last)
2. Write number of atoms
AsI3
I’m a Binary
Compound
monoarsenic triiod ide
If first prefix is mono, it is
Final Name
implied and not written
Examples #1-
Formulas to Names
1. Write names of elements
Two Non metals:
2. Write number of atoms
CCl4
I’m a Binary
Compound
monocarbon tetra chlor ide
If first prefix is mono, it is
implied and not written
Final Name
Write and name the following
covalent compounds (IUPAC)
CCl4
carbon tetrachloride
P2O3
diphosporus trioxide
IF7
iodine heptafluoride
For more lessons, visit
www.chalkbored.com
Molecular Nomenclature:
Examples
• CF4
– carbon tetrafluoride
• N 2O
– dinitrogen monoxide
• SBr6
– sulfur hexabromide
More Molecular Examples
• arsenic trichloride
– AsCl3
• dinitrogen pentoxide
– N2O5
• tetraphosphorus decoxide
– P4O10
Learning Check
Fill in the blanks to complete the following
names of covalent compounds.
CO
carbon ______oxide
CO2
carbon _______________
PCl3
phosphorus _______chloride
CCl4
carbon ________chloride
N2O
_____nitrogen _____oxide
Learning Check
1.
P2O5
a) phosphorus oxide
b) phosphorus pentoxide
c) diphosphorus pentoxide
2.
Cl2O7
a) dichlorine heptoxide
b) dichlorine oxide
c) chlorine heptoxide
3.
Cl2
a) chlorine
b) dichlorine
c) dichloride
Practice Problem #1
ClF3
Choose the correct name for the compound
1. carbon iodine trifluoride
2. chlorine trifluorine
3. chlorine trifluoride
4. chlorine tetrafluoride
5. none of the above
Practice Problem #2
arsenic pentabromide
Choose the correct formula for the compound
1. AsBr5
2. ArBr5
3. AsBr7
4. As5Br
5. none of the above
Element List
Prefixes
next problem
Practice Problem #3
N2O3
Choose the correct name for the compound
1. nitrogen trioxide
2. dinitride trioxide
3. dinitrogen trioxygen
4. dinitrogen trioxide
5. none of the above
Prefixes
next problem
Practice Problem #6
dichlorine monoxide
Choose the correct formula for the compound
1. ClO
2. Cl2O
3. ClO2
4. Cl2O2
5. none of the above
Prefixes
next problem
Acid Nomenclature
• Acids
– Compounds that form H+ in water.
– Formulas usually begin with ‘H’.
– In order to be considered an acid, they
must be aqueous (dissolved in water –
formulas end in aq)
• Examples:
– HCl
(aq)
– hydrochloric acid
– HNO3 (aq) – nitric acid
– H2SO4 (aq) – sulfuric acid
We will look at
binary &
ternary acids!
Naming Binary Acids
• H + 1 other element HX(aq)
• If the anion attached to hydrogen
ends in -ide, add the prefix hydroand change -ide to -ic acid
• HCl - hydrogen chloride becomes
• hydrochloric acid
• H2S - hydrogen sulfide becomes
• hydrosulfuric acid
Naming Ternary Acids
• H + a polyatomic ion – HXO(aq)
• change the suffix -ate to -ic acid
• HNO3(aq) not hydrogen nitrate, but
– nitric acid
• change the suffix -ite to -ous acid
• HNO2(aq) not hydrogen nitrite, but
– nitrous acid
• Ternary Acid names DO NOT begin
with “hydro-”!
Examples #1-
Formulas to Names
1. The hydrogen out front &
the (aq) subscript indicates
an acid
2. Determine the ion and it’s
acid ending.
HBrO2(aq)
bromite
bromous
____________
acid
Final Name
Acid Nomenclature
Anion
Ending
Binary 
Acid Name
-ide
hydro-(stem)-ic acid
-ate
(stem)-ic acid
-ite
(stem)-ous acid
Ternary
To remember which goes with which…
“In the cafeteria, you ATE something ICky”
Writing Acid Formulas
• Hydrogen will always be first
• The name will tell you the anion
• If it starts with hydro- it’s binary • H + a non-metal,
• If it doesn’t start with hydro-, it’s ternary
– H + a polyatomic ion.
• Remember: -ate comes from -ic, -ite
comes from –ous
• Balance charges.
Example #1-Names to Formulas
chloric acid
1. Determine the formula &
charge of the polyatomic ion
2. Add hydrogen ions
3. Balance charge with ions
4. Add the subscript: (aq)
chlorate
+1
H
-1 =0
ClO3 (aq)
Final Formula
Aqueous Acid
Salt
hydrogen
Hydrogen + polyatomic ion
hydrogen
per_____ate
hydrogen
_____ate
hydrogen
_____ite
hydrogen
hypo_____ite
hydrogen
_____ide
polyatomic ion
per_____ic acid
_____ic acid
_____ous acid
hypo______ous acid
hydro______ic acid
To transform the hydrogen _____ide salt into its
corresponding aqueous acid name:
1) The name hydrogen is replaced with the prefix hydro2) The -ide ending is replaced with ____ic
3) The word acid is added to the name
For example: hydrogen bromide > hydrobromic acid
HBr(s) > HBr(aq)
Salt
Hydrogen + polyatomic ion
Aqueous Acid
hydrogen + polyatomic ion
hydrogen
per_____ate
per_____ic acid
hydrogen
_____ate
_____ic acid
hydrogen
_____ite
_____ous acid
hydrogen
hypo_____ite
hypo______ous acid
hydrogen
_____ide
hydro______ic acid
To transform the hydrogen _____ate salt into its
corresponding aqueous acid name:
1) The name hydrogen is dropped
2) The -ate ending is replaced with –ic
3) The word acid is added to the name
For example:
hydrogen acetate > acetic acid
HC2H3O2(s) > HC2H3O2(aq)
Salt
Hydrogen + polyatomic ion
Aqueous Acid
hydrogen
polyatomic ion
per_____ic acid
hydrogen
per_____ate
hydrogen
_____ate
_____ic acid
hydrogen
_____ite
_____ous acid
hydrogen
hypo_____ite
hypo______ous acid
hydrogen
_____ide
hydro______ic acid
To transform the hydrogen per____ate salt into its
corresponding aqueous acid name:
1) The name hydrogen is dropped
2) The -ate ending is replaced with –ic
3) The word acid is added to the name
For example: hydrogen perchlorate > perchloric acid
HClO4(s) > HClO4 (aq)
Aqueous Acid
Salt
Hydrogen + polyatomic ion
hydrogen
hydrogen
polyatomic ion
per_____ic acid
per_____ate
_____ic acid
hydrogen
_____ate
hydrogen
_____ite
_____ous acid
hydrogen
hypo_____ite
hypo______ous acid
hydrogen
_____ide
hydro______ic acid
To transform the hydrogen _____ite salt into its
corresponding aqueous acid name:
1) The name hydrogen is dropped
2) The -ite ending is replaced with –ous
3) The word acid is added to the name
For example:hydrogen nitrite > nitrous acid
HNO2(s) > HNO2(aq)
Aqueous Acid
Salt
Hydrogen + polyatomic ion
hydrogen
polyatomic ion
per_____ic acid
hydrogen
per_____ate
hydrogen
_____ate
_____ic acid
hydrogen
_____ite
_____ous acid
hydrogen
hypo_____ite
hypo______ous acid
hydrogen
_____ide
hydro______ic acid
To transform the hydrogen hypo_____ite salt into its
corresponding aqueous acid name:
1) The name hydrogen is dropped
2) The -ite ending is replaced with –ous
3) The word acid is added to the name
For example:
hydrogen hypoiodite > hypoiodous acid
HIO (s) > HIO (aq)
Practice Problem #1
HIO4(aq)
Choose the correct name for the compound
1. iodoic acid
2. iodous acid
3. periodoic acid
4. hydrogen periodate
5. none of the above
Ion list
next problem
Acid Nomenclature
• hydrofluoric acid
– 2 elements
 H+ F-
 HF (aq)
• sulfuric acid
– 3 elements, -ic
 H+ SO42-  H2SO4
• nitrous acid
– 3 elements, -ous
 H+ NO2-
 HNO2
Acid Nomenclature
• HBr (aq)
– 2 elements, -ide

hydrobromic acid

carbonic acid

sulfurous acid
• H2CO3
– 3 elements, -ate
• H2SO3
– 3 elements, -ite
Practice Problem
hydrobromic acid
Choose the correct formula for the compound
1. HBrO(aq)
2.
HBr(aq)
3. HBrO3(aq)
4. HBrO2(aq)
5. none of the above
Ion list
next problem
Acid Nomenclature Flowchart
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
A flow chart for naming binary compounds.
Mixed Review
Name the following compounds:
1.
CaO
a) calcium oxide
c) calcium (II) oxide
2.
3.
SnCl4
a) tin tetrachloride
c) tin(IV) chloride
b) calcium(I) oxide
b) tin(II) chloride
N2O3
a) nitrogen oxide
c) nitrogen trioxide
b) dinitrogen trioxide
Solution
Name the following compounds:
1.
CaO
a) calcium oxide
2.
SnCl4
c) tin(IV) chloride
3.
N2O3
b) Dinitrogen trioxide
Mixed Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
Dinitrogen monoxide
Potassium sulfide
Copper (II) nitrate
Dichlorine heptoxide
Chromium (III) sulfate
Iron (III) sulfite
Calcium oxide
Barium carbonate
Iodine monochloride
Mixed Practice
1.
2.
3.
4.
5.
6.
7.
8.
9.
BaI2
P4S3
Ca(OH)2
FeCO3
Na2Cr2O7
I2O5
Cu(ClO4)2
CS2
B2Cl4
Name ‘Em!
• HI (aq)
• HCl
• H2SO3
• HNO3
• HIO4
Write the Formula!
• Hydrobromic acid
• Nitrous acid
• Carbonic acid
• Phosphoric acid
• Hydrotelluric acid
Naming Ternary Compounds
from Oxyacids
The following table lists the most common families of oxy acids.
one more
oxygen atom
HClO4
perchloric acid
most
“common”
HClO3
chloric acid
H2SO4
sulfuric acid
H3PO4
phosphoric acid
HNO3
nitric acid
one less
oxygen
HClO2
chlorous acid
H2SO3
sulfurous acid
H3PO3
phosphorous acid
HNO2
nitrous acid
two less
oxygen
HClO
hypochlorous acid
H3PO2
hypophosphorous acid
(HNO)2
hyponitrous acid
Naming Simple Chemical Compounds
Ionic (metal and nonmetal)
Metal
Forms
only one
positive
ion
Use the
name of
element
Forms
more than
one positive
ion
Covalent (2 nonmetals)
Nonmetal
Single
Negative
Ion
Use element
Use the name
name followed
of the
by a Roman
element, but
numeral to
end with ide
show the charge
First
nonmetal
Second
nonmetal
Before
element name
use a prefix
to match
subscript
Use a prefix
before
element name
and end
with ide
Polyatomic
Ion
Use the
name of
polyatomic
ion (ate or
Ite)
Nomenclature
PO43phosphate ion
HC2H3O2
Acetic Acid
C2H3O2acetate ion
Two nonmetals
PRACTICE
Multiple-charge cation
Everything else
carbon
sulfurN
tetrabromide
dichloride
NCl
O35
2
vanadium
niobiumMn
Pt(IO
(V)
(II)
perchlorate
)4
2S
53chromate
rubidium
sulfate
NH4KI
ClO
barium
oxide
3
Greek prefixes
Roman numeral
for name only
Roman
numeral
Charge
Polyatomic ions OK
CrissCross
Rule
Roman
numeral
Polyatomic ions OK
Where would you file this?
VCrO4
dinitrogen pentoxide
BaO
platinum (IV) iodate
CBr4
ammonium chlorate
Nb(ClO4)5
potassium iodide
SCl2
nitrogen trichloride
Rb2SO4
manganese (V) sulfide
Learning Check
Complete the names of the following binary
compounds:
Na3N
sodium
________________
KBr
potassium ________________
Al2O3
aluminum ________________
MgS
_________________________
Compounds containing polyatomic ions
Ca(OH)2
CuSO4
NH4NO3
Co2(CO3)3
- calcium hydroxide
- copper(II) sulfate
- ammonium nitrate
- cobalt(III) carbonate