Ch. 7 (Con

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Ch. 7 (Cont.)Formula Writing Naming of
Compounds
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Oxidation numbers
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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.

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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.

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Predicting Charges on Monatomic Ions KNOW THESE
!!!!
1 2
-3 -2 -1 0
Cd2
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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.

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Example Determine the oxidation numbers for
each atom in KMnO4

• This compound is made up of a K cation and an
  MnO4- anion.
• 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.

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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.

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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

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Example Aluminum Chloride
Writing Balanced Chemical Formulas
Criss-Cross Rule for Ionic Compounds
Step 1
write symbols charge of elements
Cation (metal) always written 1st!
Aluminum Chloride
1-
Al Cl
3
Step 2
criss-cross charges as subscripts
Al Cl
1
3
AlCl3
combine as formula unit (1 is never shown) (use
smallest whole ratio) Make sure you remove
charges!!
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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
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Example Magnesium Oxide
Criss-Cross Rule
Step 1 Magnesium Oxide
Step 2 Mg2 O2-
Step 3 Mg O
2
2
Step 4 Mg2O2
Step 5 MgO
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Putting Ions Together
Na Cl- NaCl
Ca2 Cl- CaCl2
Ca2 O-2 CaO
Na O-2 Na2O
Al3 S-2 Al2S3
Ca2 N-3 Ca3N2
You try these!
Mg2 F-
Li Br-
MgF2
LiBr
Al3 I-
AlI3
K Cl-
KCl
Sr3P2
Sr2 P-3
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Crisscross

• Switch the numerical value of the charges

Ba2
N3-
3
2
Ba3
N2

• Reduce ratio if possible

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Learning Check

• Write the correct formula for the compounds
  containing the following ions
• 1. Na, S2-
• a) NaS b) Na2S c) NaS2
• 2. Al3, Cl-
• a) AlCl3 b) AlCl c) Al3Cl
• 3. Mg2, N3-
• a) MgN b) Mg2N3 c) Mg3N2

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Solution

• 1. Na, S2-
• b) Na2S
• 2. Al3, Cl-
• a) AlCl3
• 3. Mg2, N3-
• c) Mg3N2

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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!
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Polyatomic Ions

• NO3-
• nitrate ion
• NO2-
• nitrite ion

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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

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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
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IONIC COMPOUNDSremember they have
oppositely-charged ions in a rigid 3-D pattern
ammonium chloride, NH4Cl
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Ternary Ionic Nomenclature

• Sodium Sulfate
• Na and SO4 -2
• Na2SO4
• Iron (III) hydroxide
• Fe3 and OH-
• Fe(OH)3
• Ammonium carbonate
• NH4 and CO3 2
• (NH4)2CO3

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Writing Formulas w/Polyatomic Ions
Reminder! Parentheses are required only when
you need more than one bunch of a particular
polyatomic ion.
BaSO4
Ba2 and SO42
barium sulfate
Mg(NO2)2
Mg2 and NO21
magnesium nitrite
NH4ClO3
NH41 and ClO31
ammonium chlorate
Sn4 and SO42
Sn(SO4)2
tin (IV) sulfate
Fe2(Cr2O7)3
Fe3 and Cr2O72
iron (III) dichromate
(NH4)3N
NH41 and N3
ammonium nitride
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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)

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• 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

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Polyatomic Ion a group of atoms that stay
together and have a single, overall charge.
BrO41- Perbromate ion BrO31- Bromate ion BrO21- Bromite ion BrO1- Hypobromite ion
CO42- CO32- Carbonate ion CO22- CO2-
ClO41- ClO31- Chlorate ion ClO21- ClO1-
IO41- IO31- Iodate ion IO21- IO1-
NO41- NO31- Nitrate ion NO21- NO1-
PO53- PO43- Phosphate ion PO33- PO23-
SO52- SO42- Sulfate ion SO32- SO22-
1 more oxygen normal 1 less oxygen 2 less oxygen
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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 2 less
Os ________ _____ide 0 Os
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• The oxy-ions of chlorine bromine all have
  these trends in common. Look for them below

perchlorate ClO4-1 chlorate
ClO3-1 chlorite ClO2-1 Hypochlorite 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.
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Practice Problem 2

• sodium chlorite

Choose the correct formula for the compound
1. NaCl
No, you need to review prefixes
2. NaClO
No, you need to review prefixes
3. NaClO2
Very good, click arrow to continue
No, you have several errors
4. Na(ClO)2
No, there is a correct answer
5. none of the above
next problem
Prefixes
Periodic Chart
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Naming Compounds
What's in a name? That which we call a roseby
any other name would smell as sweet." -
William Shakespeare, Romeo and Juliet (II, ii)
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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

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Name these ions

• Cl1-

Chloride ion

• N3-

Nitride ion

• Br1-

Bromide ion
Oxide ion

• O2-

Gallium ion

• Ga3

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Naming Binary Ionic Compounds

• Examples
• NaCl
• ZnI2
• Al2O3

sodium chloride zinc iodide aluminum oxide
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Formulas to Names Ternary Compounds
1. Write the names of the ions
Im a polyatomic ion

• KMnO4

potassium
permanganate
Final Name
If the positive ion has a fixed charge, you are
finished.
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Formulas to Names Ternary Compounds
1. Write the names of the ions
Im a polyatomic ion

• NH4NO3

ammonium
nitrate
Final Name
If the positive ion has a fixed charge, you are
finished.
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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 a) calcium carbonate
• CaCO3 b) calcium phosphate
• Ca3(PO4)2 c) calcium bicarbonate

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Practice Naming Ionic Compounds

• Na2CO3 --
• CaSO4 --
• KBr --
• MgS --
• BeCl2 --
• NH4F --

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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 its Latin or English
  root and ends in -ic or ous to denote charge.
• E.g. Cu1 is cuprous, E.g. Cu2 is cupric
• Lower ous, Higher ic

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Write the balanced formula for copper chloride
name it
Cu2 Cl-1 CuCl2 cupric chloride Cu1
Cl-1 CuCl cuprous chloride For Latin
naming know rules, possible charges, Latin
names, suffixes
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Examples of Older Names of Cations formed from
Transition Metals
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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 Cu2Cl-1 Cu1Cl-1,
• Cu2Cl-1 CuCl2 copper (II) chloride
• Cu1 Cl-1 CuCl copper (I) chloride

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Formula to NameHow do I figure out the Roman
Numeral??Hint Weve 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.

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Binary CompoundsContaining 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
(II)
FeCl2
Ferrous chloride
Iron chloride
Iron chloride
FeCl3
(III)
Ferric chloride
(II)
SnO Tin oxide SnO2 Tin oxide
Stannous oxide
(IV)
Stannic oxide
(ic ending higher oxidation state ous
is lower oxidation state)
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Ternary Ionic Nomenclature

• Writing Formulas
• Write each ion, cation first. Dont 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 ions charge when
  needed (Stock System)

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How do I figure out the Roman Numeral?
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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

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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
Im not a polyatomic ion

• Cu2S

copper
sulfide
(I)
Final Name
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Examples 1- Formulas to Names

• CuSO3

1. Write the names of the ions
0
-2
2. Determine the charge of the positive ion
Cu
SO3
2
x
X (- 2) 0
Im a polyatomic ion
You must know the charge on the sulfite ion is -2
The sum of the positive and negative charges must
equal zero
2 2
X 2
copper
sulfite
(II)
Final Name
Next
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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
fluoride
(II)
Final Name
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Example 3-Names to Formulas
1. Write symbols of elements
3X 1y
X(3) y(-1) 0
2. Determine number of ions
(Ni3)x(C2H3O2-1)y 0

• nickel(III) acetate

Choose the lowest set of integers thatsatisfies
the equation
(C2H3O2)3
C2H3O2
Ni
1
Final Formula
If there is only one atom the 1 is not shown
Next
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Practice Problem 1

• Fe(NO3)3

Choose the correct name for the compound
1. Iron trinitrate
No, you do not use prefixes
2. iron(I) nitrate
No, you have the wrong oxidation number
3. iron(III) nitrite
No, you need to review polyatomic ions
4. iron(III) nitrate
Very good, click arrow to continue
5. none of the above
No, there is a correct answer
next problem
Polyatomic Ions
Periodic Chart
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Learning Check

• Complete the names of the following binary
  compounds with variable metal ions
• FeBr2 iron (_____) bromide
• CuCl copper (_____) chloride
• SnO2 ___(_____ ) ______________
• Fe2O3 ________________________
• Hg2S ________________________

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Nomenclaturefor 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 its binary)

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In order to be effective in using prefixes to
name compounds containing two non-metals, these
prefixes must be committed to memory

• mono- 1 hepta- 7
• di- 2 octa- 8
• tri- 3 nona- 9
• tetra- 4 deca- 10
• penta- 5
• hexa- 6

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Naming covalent compounds
1 mono
2 di
3 tri
4 tetra
5 penta
6 hexa
7 hepta
8 octa
9 nona
10 deca

• prefix refers to of atoms - not charge
• N2O4 dinitrogen tetroxide
• Exception dont use mono for first element
• CO2 carbon dioxide
• The first vowel is often dropped to avoid the
  combination of ao or oo.
• CO carbon monoxide (monooxide)

P4O10 tetraphosphorus decoxide (decaoxid
e)
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Covalent Compounds Name to Formula Youll 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? N2O3 dinitrogen
monoxide? N2O
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Example 1-Names to Formulas
Im a Binary Compound
Two Non metals

• Sulfur trioxide

1. Write symbols of elements
S
O
1
3
2. Write number of atoms
Final Formula
If no prefix, then 1 is implied and not written
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Example 2-Names to Formulas
Im a Binary Compound

• dichlorine heptaoxide

1. Write symbols of elements
Cl
O
2
7
2. Write number of atoms
Final Formula
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Example 3-Names to Formulas
Im a Binary Compound

• oxygen difluoride

1. Write symbols of elements
O
F
1
2
2. Write number of atoms
If no prefix, then 1 is implied and not written
Final Formula
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Example 4-Names to Formulas
Im a Binary Compound

• dinitrogen tetraoxide

1. Write symbols of elements
N
O
2
4
2. Write number of atoms
Final Formula
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Example 5-Names to Formulas
Im a Binary Compound

• phosphorus pentachloride

1. Write symbols of elements
P
Cl
5
1
2. Write number of atoms
If no prefix, then 1 is implied and not written
Final Formula
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Examples 2- Formulas to Names
1. Write names of elements last element ends in
-ide
2. Write prefix for number of atoms
Im a Binary Compound

• XeF3

xenon
mono
fluor
tri
ide
If first prefix is mono, it is implied and not
written
Final Name
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Example - Formulas to Names

• Write names of elements
• (-ide on last)

Im a Binary Compound
2. Write number of atoms

• AsI3

ide
arsenic
mono
tri
iod
If first prefix is mono, it is implied and not
written
Final Name
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Examples 1- Formulas to Names
Two Non metals
1. Write names of elements
2. Write number of atoms
Im a Binary Compound

• CCl4

carbon
mono
tetra
chlor
ide
If first prefix is mono, it is implied and not
written
Final Name
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Write and name the following covalent compounds
(IUPAC)

• carbon tetrachloride
• diphosporus trioxide
• iodine heptafluoride

CCl4 P2O3 IF7
For more lessons, visit www.chalkbored.com
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Molecular Nomenclature Examples

• CF4
• N2O
• SBr6

• carbon tetrafluoride

• dinitrogen monoxide

• sulfur hexabromide

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More Molecular Examples

• arsenic trichloride
• dinitrogen pentoxide
• tetraphosphorus decoxide

• AsCl3

• N2O5

• P4O10

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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

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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

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Practice Problem 1

• ClF3

Choose the correct name for the compound
1. carbon iodine trifluoride
No, "Cl" is not carbon iodine, see element list
2. chlorine trifluorine
No, all binary compounds end with "ide"
3. chlorine trifluoride
Very good, click arrow to continue
4. chlorine tetrafluoride
No, you need to review prefixes
5. none of the above
No, there is a correct answer
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Practice Problem 2

• arsenic pentabromide

Choose the correct formula for the compound
1. AsBr5
Very good, click arrow to continue
2. ArBr5
No, "Ar" is not correct, see element list
3. AsBr7
No, you need to review prefixes
No, the subscript is with the wrong element
4. As5Br
No, there is a correct answer
5. none of the above
next problem
Prefixes
Element List
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Practice Problem 3

• N2O3

Choose the correct name for the compound
1. nitrogen trioxide
No, you need to use more prefixes
2. dinitride trioxide
No, only the last element ends with "ide"
3. dinitrogen trioxygen
No, all binary compounds end in "ide"
4. dinitrogen trioxide
Very good, click arrow to continue
5. none of the above
No, there is a correct answer
next problem
Prefixes
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Practice Problem 6

• dichlorine monoxide

Choose the correct formula for the compound
1. ClO
No, you don't have any subscripts
2. Cl2O
Very good, click arrow to continue
3. ClO2
No, you have the wrong subscripts
No, you have the wrong subscripts
4. Cl2O2
No, there is a correct answer
5. none of the above
next problem
Prefixes
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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!
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Naming Binary Acids

• H 1 other element HX(aq)
• If the anion attached to hydrogen ends in -ide,
  add the prefix hydro- and change -ide to -ic acid
• HCl - hydrogen chloride becomes
• hydrochloric acid
• H2S - hydrogen sulfide becomes
• hydrosulfuric acid

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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-!

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Examples 1- Formulas to Names
HBrO2(aq)
1. The hydrogen out front the (aq) subscript
indicates an acid
bromite
2. Determine the ion and its acid ending.
bromous acid
____________ acid
Final Name
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Acid Nomenclature
Binary ?
Ternary
To remember which goes with which In the
cafeteria, you ATE something ICky
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Writing Acid Formulas

• Hydrogen will always be first
• The name will tell you the anion
• If it starts with hydro- its binary -
• H a non-metal,
• If it doesnt start with hydro-, its ternary H
  a polyatomic ion.
• Remember -ate comes from -ic, -ite comes from
  ous
• Balance charges.

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Example 1-Names to Formulas
chloric acid

1. Determine the formula charge of the polyatomic
   ion

chlorate
2. Add hydrogen ions
-1
1
0
H
ClO3
(aq)
3. Balance charge with ions
Final Formula
4. Add the subscript (aq)
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Salt Hydrogen polyatomic ion hydrogen
per_____ate hydrogen _____ate hydrogen
_____ite hydrogen
hypo_____ite hydrogen _____ide
Aqueous Acid hydrogen 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 hydro-
2) The -ide ending is replaced with ____ic 3)
The word acid is added to the name For example
hydrogen bromide gt hydrobromic acid
HBr(s) gt HBr(aq)
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Salt Hydrogen polyatomic
ion hydrogen per_____ate hydrogen
_____ate hydrogen
_____ite hydrogen hypo_____ite hydrogen
_____ide
Aqueous Acid hydrogen polyatomic
ion per_____ic acid _____ic acid
_____ous acid hypo______ous acid 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 gt
acetic acid HC2H3O2(s)
gt HC2H3O2(aq)
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Aqueous Acid hydrogen polyatomic
ion per_____ic acid _____ic acid
_____ous acid hypo______ous acid hydro______ic
acid
Salt Hydrogen polyatomic
ion hydrogen per_____ate hydrogen
_____ate hydrogen _____ite hydrogen
hypo_____ite hydrogen _____ide
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 gt
perchloric acid
HClO4(s) gt HClO4 (aq)
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Salt Hydrogen polyatomic ion hydrogen
per_____ate hydrogen _____ate hydrogen
_____ite hydrogen
hypo_____ite hydrogen _____ide
Aqueous Acid hydrogen polyatomic
ion per_____ic acid _____ic acid
_____ous acid hypo______ous acid 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 examplehydrogen nitrite gt
nitrous acid HNO2(s) gt HNO2(aq)
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Salt Hydrogen polyatomic ion hydrogen
per_____ate hydrogen _____ate hydrogen
_____ite hydrogen
hypo_____ite hydrogen _____ide
Aqueous Acid hydrogen polyatomic
ion per_____ic acid _____ic acid
_____ous acid hypo______ous acid 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 gt
hypoiodous acid HIO
(s) gt HIO (aq)
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Practice Problem 1

• HIO4(aq)

Choose the correct name for the compound
1. iodoic acid
No, it contains more oxygen atoms
2. iodous acid
No, it contains more oxygen atoms
3. periodoic acid
Very good, click arrow to continue
4. hydrogen periodate
No, you need to use the acid name
5. none of the above
No, there is a correct answer
next problem
Ion list
89
Acid Nomenclature

• hydrofluoric acid
• sulfuric acid
• nitrous acid

• 2 elements

? HF (aq)
? H F-

• 3 elements, -ic

? H2SO4
? H SO42-
? HNO2
? H NO2-

• 3 elements, -ous

90
Acid Nomenclature

• HBr (aq)
• H2CO3
• H2SO3

? hydrobromic acid

• 2 elements, -ide

• 3 elements, -ate

? carbonic acid
? sulfurous acid

• 3 elements, -ite

91
Practice Problem

• hydrobromic acid

Choose the correct formula for the compound
1. HBrO(aq)
No, it has too many oxygen atoms
2. HBr(aq)
Very good, click arrow to continue
3. HBrO3(aq)
No, you have too many oxygen atoms
No, you have too many oxygen atoms
4. HBrO2(aq)
No, there is a correct answer
5. none of the above
next problem
Ion list
92
Acid Nomenclature Flowchart
93
A flow chart for naming binary compounds.
94
Mixed Review

• Name the following compounds
• 1. CaO
• a) calcium oxide b) calcium(I) oxide c)
  calcium (II) oxide
• 2. SnCl4
• a) tin tetrachloride b) tin(II) chloride
• c) tin(IV) chloride
• 3. N2O3
• a) nitrogen oxide b) dinitrogen trioxide
• c) nitrogen trioxide

95
Solution

• Name the following compounds
• 1. CaO
• 2. SnCl4
• 3. N2O3

a) calcium oxide
c) tin(IV) chloride
b) Dinitrogen trioxide
96
Mixed Practice

1. Dinitrogen monoxide
2. Potassium sulfide
3. Copper (II) nitrate
4. Dichlorine heptoxide
5. Chromium (III) sulfate
6. Iron (III) sulfite
7. Calcium oxide
8. Barium carbonate
9. Iodine monochloride

97
Mixed Practice

1. BaI2
2. P4S3
3. Ca(OH)2
4. FeCO3
5. Na2Cr2O7
6. I2O5
7. Cu(ClO4)2
8. CS2
9. B2Cl4

98
Name Em!

• HI (aq)
• HCl
• H2SO3
• HNO3
• HIO4

99
Write the Formula!

• Hydrobromic acid
• Nitrous acid
• Carbonic acid
• Phosphoric acid
• Hydrotelluric acid

100
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
101
(No Transcript)
102
Naming Simple Chemical Compounds
Ionic (metal and nonmetal)
Covalent (2 nonmetals)
Metal
Nonmetal
First nonmetal
Second nonmetal
Forms only one positive ion
Forms more than one positive ion
Single Negative Ion
Polyatomic Ion
Use the name of element
Use element name followed by a Roman numeral
to show the charge
Before element name use a prefix to
match subscript
Use a prefix before element name and end with
ide
Use the name of the element, but end with ide
Use the name of polyatomic ion (ate or Ite)
103

• Nomenclature

PO43- phosphate ion
HC2H3O2 Acetic Acid
C2H3O2- acetate ion
104
PRACTICE
Two nonmetals
Multiple-charge cation
Everything else
N2O5
barium oxide
carbon tetrabromide
NH4ClO3
KI
sulfur dichloride
NCl3
rubidium sulfate
vanadium (II) chromate
Pt(IO3)4
niobium (V) perchlorate
Mn2S5
Greek prefixes
Roman numeral for name only
Roman numeral
Charge
Polyatomic ions OK
Polyatomic ions
OK
Where would you file this?
Criss- Cross Rule
VCrO4
dinitrogen pentoxide
VCrO4
dinitrogen pentoxide
BaO
platinum (IV) iodate
BaO
platinum (IV) iodate
CBr4
ammonium chlorate
CBr4
ammonium chlorate
Roman numeral
Nb(ClO4)5
potassium iodide
Nb(ClO4)5
potassium iodide
SCl2
nitrogen trichloride
SCl2
nitrogen trichloride
Rb2SO4
Rb2SO4
manganese (V) sulfide
manganese (V) sulfide
105
Learning Check

• Complete the names of the following binary
  compounds
• Na3N sodium ________________
• KBr potassium ________________
• Al2O3 aluminum ________________
• MgS _________________________

106
Compounds containing polyatomic ions
- calcium hydroxide - copper(II) sulfate -
ammonium nitrate - cobalt(III) carbonate
Ca(OH)2 CuSO4 NH4NO3 Co2(CO3)3