ch. 7 (con’t.) formula writing & naming of compunds

Ch. 7 (Con’t.)Formula Writing &

Naming of Compunds

Predicting Charges on Monatomic IonsPredicting Charges on Monatomic IonsKNOW THESE !!!!KNOW THESE !!!!

+1 +2 -3 -2 -1 0

Cd+2

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

Example: Aluminum ChlorideStep 1:

Step 2:

1 3

Step 3:

Al Cl

Al Cl

3+ 1-

write symbols & charge of elements

criss-cross charges as subscripts

combine as formula unit(“1” is never shown) (use smallest whole # ratio)Make sure you remove charges!!

Aluminum Chloride

AlCl3

Cation (metal) always written 1st!

Writing Balanced Chemical FormulasCriss-Cross Rule for Ionic Compounds

InBr3BaS

charge on cation “becomes” subscript of anion charge on anion “becomes” subscript of cation

** Warning: Reduce subscripts to lowest terms.

Al2O3

Al3+ and O2–

Al2 O3

Ba2+ and S2–

Ba2 S2

In3+ and Br1–

In1 Br3

aluminum oxide barium sulfide indium bromide

Ones are not included in formulas!!

Example: Magnesium Oxide

Step 1: Magnesium Oxide

Step 2: Mg2+ O2-

Step 3: Mg O2 2

Step 4: Mg2O2

Step 5: MgO

Criss-Cross Rule

Putting Ions Together

Na+ + Cl- = NaCl

Ca+2 + O-2= CaO Na+ + O-2 = Na2O

Al+3 + S-2 = Al2S

3Ca+2 + N-3 = Ca

3N

2

Ca+2 + Cl- = CaCl2

You try these!

Mg+2 + F- =

K+ + Cl- = Al+3 + I- =

Sr+2 + P-3 =

Li+ + Br- =

Sr3P

2

AlI3

MgF2

KCl

LiBr

Crisscross

• Switch the numerical value of the charges

Ba2+ N3-2 3

Ba3N2• Reduce ratio if possible

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

Solution

1. Na+, S2-

b) Na2S

2. Al3+, Cl-

a) AlCl3

3. Mg2+, N3-

c) Mg3N2

Polyatomic IonsThere 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!

NO3-

nitrate ion

NO2-

nitrite ion

Polyatomic Ions

Polyatomic Ions

Naming Ternary Ionic Compoundscontain 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 COMPOUNDSremember: they have oppositely-charged

ions in a rigid 3-D pattern

IONIC COMPOUNDSremember: they have oppositely-charged

ions in a rigid 3-D pattern

NH4+

Cl-

ammonium chloride, NHammonium chloride, NH44ClCl

Ternary Ionic Nomenclature

Sodium SulfateNa+ and SO4 -2

Na2SO4

Iron (III) hydroxideFe+3 and OH-

Fe(OH)3

Ammonium carbonateNH4

+ and CO3 –2

(NH4)2CO3

(NH4)3N

Fe2(Cr2O7)3

Sn(SO4)2

NH4ClO3

Mg(NO2)2

BaSO4

Writing Formulas w/Polyatomic Ions

Reminder! Parentheses are required only when you need more than one “bunch” of a particular polyatomic ion.

Ba2 and SO4

2–

Mg2+ and NO21–

NH41+ and ClO3

1–

Sn4+ and SO42–

Fe3+ and Cr2O72–

NH41+ and N3–

barium sulfate

magnesium nitrite

ammonium chlorate

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

BrO31-

Bromate ion

BrO21-

Bromite ion

BrO1-

Hypobromite ion

CO42- CO3

2-

Carbonate ion

CO22- CO2-

ClO41- ClO3

1-

Chlorate ion

ClO21- ClO1-

IO41- IO3

1-

Iodate ion

IO21- IO1-

NO41- NO3

1-

Nitrate ion

NO21- NO1-

PO53- PO4

3-

Phosphate ion

PO33- PO2

3-

SO52- SO4

2-

Sulfate ion

SO32- SO2

2-

1 more oxygen “normal” 1 less oxygen 2 less oxygen

Salt metal polyatomic ion # Oxygen

atoms

________ per_____ate 1 more O ________ _____ate common ________ _____ite 1 less O

________ hypo_____ite 2 less O’s

________ _____ide 0 O’s

The table below shows the prefixes and suffixes that tell the number of oxygen atoms present in the negative ion.

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.

Practice Problem #2sodium chlorite

Choose the correct formula for the compound

1. NaCl

2. NaClO

3. NaClO2

4. Na(ClO)2

5. none of the above

next problem

PrefixesPeriodic Chart

Naming CompoundsNaming 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)

Naming CompoundsNaming Compounds

• 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

Binary Ionic Compounds (metal & nonmetal):Binary Ionic Compounds (metal & nonmetal):

Name these ions

Cl1- Chloride ion N3- Nitride ion Br1- Bromide ion O2- Oxide ion Ga3+ Gallium ion

Naming Binary Ionic Compounds

Examples:

NaCl

ZnI2

Al2O3

sodium chloride

zinc iodide

aluminum oxide

Formulas to Names: Ternary Compounds

KMnO4

potassium

I’m a polyatomi

c ion

1. Write the names of the ions

Final Name permanganate

If the positive ion has a fixed charge, you are finished.

Formulas to Names: Ternary Compounds

NH4NO3

ammonium

I’m a polyatomi

c ion


Final Name

nitrate

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 a) calcium carbonate

CaCO3 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

Cu+2 + Cl-1 = CuCl2

= cupric chloride

Cu+1 + Cl-1 = CuCl = cuprous chloride

For Latin naming: know rules, possible charges, Latin names, & suffixes

Write the balanced formula for copper chloride & name it:

Examples of Older Names of Cations formed from Transition Metals

• 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

Co+1 + Cl-1 = CuCl = copper (I) chloride

Multiple valence: Stock System

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 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

FeCl2

(“ic” ending = higher oxidation state; “ous” is lower oxidation state)

SnO Tin oxideSnO2 Tin oxide

(II)(III)

(II)(IV)

Traditional (OLD) System

Ferrous chlorideFerric chloride

Stannous oxideStannic oxide

Iron chlorideIron chlorideFeCl3

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

Cu2S

copper

I’m not a polyatomi

c ion

2. Determine the charge of the positive ion


Final Name

sulfide(I)

2Cux (S)-2 = 0

2X + (-2) = 0

X = +1


CuSO3

copper

I’m a polyatomi

c ion


Final Name

sulfite(II)

x

X + (- 2) = 0

X = +2

Cu SO3

= 0

You must know the charge on the sulfite ion is -2

The sum of the positive and negative charges must equal zero


-

2

+2 +2

Next

+2


SnF2

tin



Final Name

fluoride(II)

Snx (F-1)2 = 0

X + 2(-1) = 0

X = +2

Example #3-Names to Formulas

nickel(III) acetate

Ni C2H3O2

2. Determine number of ions

1. Write symbols of elements

Final Formula

(Ni+3)x(C2H3O2-1)y

= 0

3X = 1y

X(+3) + y(-1) = 0

X 1Y 3=

1Choose the lowest set of integers that

satisfies the equation

(C2H3O2)3

If there is only one atom the “1” is not shown

Next

Practice Problem #1Fe(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 abovenext

problemPolyatomic

IonsPeriodic Chart

Learning Check

Complete the names of the following binary

compounds with variable metal ions:

FeBr2 iron (_____) bromide

CuCl copper (_____) chloride

SnO2 ___(_____ ) ______________

Fe2O3 ________________________

Hg2S ________________________

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 it’s binary)

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

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

Naming covalent compounds1 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 chargeN2O4 = dinitrogen tetroxide

• Exception: don’t 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

(decaoxide)

Covalent Compounds: Name to FormulaYou’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?

N2O3

dinitrogen monoxide?

N2O


Sulfur trioxide

S O1 3

I’m a Binary Compound

2. Write number of atoms


Final Formula

If no prefix, then 1 is implied and not written

Two Non metals:


dichlorine heptaoxide

Cl O2 7




Final Formula


oxygen difluoride

O F1 2




Final FormulaIf no prefix, then 1 is

implied and not written


dinitrogen tetraoxide

N O2 4




Final Formula


phosphorus pentachloride

PCl1 5




Final FormulaIf no prefix, then 1 is

implied and not written


XeF3

xenonmono

tri

I’m a Binary

Compound

2. Write prefix for number of atoms

1. Write names of elements –last element ends in -ide

Final Name

fluorideIf first prefix is mono, it is implied and not written

Example - Formulas to Names

AsI3

arsenic

mono

tri

I’m a Binary

Compound


1. Write names of elements

(-ide on last)

Final Name

iodideIf first prefix is mono, it is implied and not written


CCl4

carbon

mono

tetra

I’m a Binary

Compound


1. Write names of elements

Final Name

chlorideIf first prefix is mono, it is implied and not written

Two Non metals:

Write and name the following covalent compounds (IUPAC)

carbon tetrachloride

diphosporus trioxide

iodine heptafluoride

CCl4

P2O3

IF7

For more lessons, visit www.chalkbored.com

• CF4

• N2O

• SBr6

–carbon tetrafluoride

–dinitrogen monoxide

–sulfur hexabromide

Molecular Nomenclature: Examples

• arsenic trichloride

• dinitrogen pentoxide

• tetraphosphorus decoxide

–AsCl3

–N2O5

–P4O10

More Molecular Examples

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 #1ClF3


1. carbon iodine trifluoride

2. chlorine trifluorine

3. chlorine trifluoride

4. chlorine tetrafluoride


Practice Problem #2arsenic pentabromide


1. AsBr5

2. ArBr5

3. AsBr7

4. As5Br5. none of the above

next problem

PrefixesElement List

Practice Problem #3N2O3


1. nitrogen trioxide

2. dinitride trioxide

3. dinitrogen trioxygen

4. dinitrogen trioxide


problemPrefixes

Practice Problem #6dichlorine monoxide


1. ClO

2. Cl2O

3. ClO2

4. Cl2O2


next problem

Prefixes

Acid Nomenclature• AcidsAcids

– Compounds that form HCompounds that form H++ in water. in water.

– Formulas usually begin with ‘H’.Formulas usually begin with ‘H’.

– In order In order to be considered an acidto be considered an acid, , they they

must be aqueous (dissolved in water – must be aqueous (dissolved in water –

formulas end in aq)formulas end in aq)

• Examples:Examples:

– HCl HCl (aq)(aq) – hydrochloric acid – hydrochloric acid

– HNOHNO3 3 (aq)(aq) – nitric acid – nitric acid

– HH22SOSO4 4 (aq)(aq) – sulfuric acid – 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 hydro- and 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-”!

Anion Ending Acid Name

-ide hydro-(stem)-ic acid

-ate (stem)-ic acid

-ite (stem)-ous acid

Acid Nomenclature

Binary Binary

Ternary Ternary

To remember which goes with which…To remember which goes with which…

““In the cafeteria, you ATE something ICky”In the cafeteria, you ATE something ICky”

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 > hydrobromic acid HBr(s) > HBr(aq)

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 –ic3) The word acid is added to the name

For example: hydrogen acetate > acetic acid HC2H3O2(s) > HC2H3O2(aq)

SaltHydrogen + polyatomic ion


hydrogen _____ate

hydrogen _____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 per____ate salt into its corresponding aqueous acid name:

1) The name hydrogen is dropped 2) The -ate ending is replaced with –ic3) The word acid is added to the name

For example: hydrogen perchlorate > perchloric acid HClO4(s) > HClO4 (aq)


per_____ic acid

_____ic acid

_____ous acid

hypo______ous acid

hydro______ic acid

Salt



hydrogen _____ate

hydrogen _____ite


hydrogen _____ide

Salt



hydrogen _____ate

hydrogen _____ite


hydrogen _____ide


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 –ous3) The word acid is added to the name

For example:hydrogen nitrite > nitrous acidHNO2(s) > HNO2(aq)

Salt



hydrogen _____ate

hydrogen _____ite


hydrogen _____ide


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 –ous3) The word acid is added to the name

For example: hydrogen hypoiodite > hypoiodous acid HIO (s) > HIO (aq)


2. Determine the ion and it’s acid ending.

1. The hydrogen out front & the (aq) subscript indicates an acid

Final Name

HBrO2(aq)

bromous acid

bromite

____________ acid

Practice Problem #1HIO4(aq)


1. iodoic acid

2. iodous acid

3. periodoic acid

4. hydrogen periodate


problemIon list

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.


HClO3

2. Add hydrogen ions

1. Determine the formula & charge of the polyatomic ion

Final Formula

chloric acid

(aq)

chlorate

-1+1

3. Balance charge with ions

4. Add the subscript: (aq)

=0

• hydrofluoric acidhydrofluoric acid

• sulfuric acidsulfuric acid

• nitrous acidnitrous acid

– 2 elements2 elements

– 3 elements, 3 elements, -ic-ic

– 3 elements, 3 elements, -ous-ous

HF HF (aq)(aq)

HH22SOSO44

HNOHNO22

Acid Nomenclature

HH++ F- F-

HH++ SO SO442-2-

HH++ NO NO22--

• HBr HBr (aq)(aq)

• HH22COCO33

• HH22SOSO33

– 2 elements, 2 elements, --ideide

– 3 elements, 3 elements, -ate-ate

– 3 elements, 3 elements, -ite-ite

hydrohydrobromic bromic

acidacid

carboncarbonicic

acidacid

sulfursulfurousous

acidacid

Acid Nomenclature

Practice Problemhydrobromic acid


1. HBrO(aq)

2. HBr(aq)

3. HBrO3(aq)

4. HBrO2(aq)


next problem

Ion list

Acid Nomenclature Flowchart

h yd ro - p re fix-ic en d in g

2 e lem en ts

-a te en d in gb ecom es-ic en d in g

-ite en d in gb ecom es

-o u s en d in g

n o h yd ro - p re fix

3 e lem en ts

AC ID Ss ta rt w ith 'H '

A flow chart for naming binary compounds.

Mixed Review

Name the following compounds:

1. CaOa) calcium oxide b) calcium(I) oxidec) calcium (II) oxide

2. SnCl4

a) tin tetrachloride b) tin(II) chloride

c) tin(IV) chloride

3. N2O3

a) nitrogen oxide b) dinitrogen trioxidec) nitrogen trioxide

Solution

Name the following compounds:

1. CaO

2. SnCl4

3. N2O3

a) calcium oxide

c) tin(IV) chloride

b) Dinitrogen trioxide

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

Mixed Practice

1.1. BaIBaI22

2.2. PP44SS33

3.3. Ca(OH)Ca(OH)22

4.4. FeCOFeCO33

5.5. NaNa22CrCr22OO77

6.6. II22OO55

7.7. Cu(ClOCu(ClO44))22

8.8. CSCS22

9.9. BB22ClCl44

Name ‘Em!

• HI HI (aq)(aq)

• HClHCl

• HH22SOSO33

• HNOHNO33

• HIOHIO44

Write the Formula!

• Hydrobromic acidHydrobromic acid

• Nitrous acidNitrous acid

• Carbonic acidCarbonic acid

• Phosphoric acidPhosphoric acid

• Hydrotelluric acidHydrotelluric acid

Naming Ternary Compounds from Oxyacids

The following table lists the most common families of oxy acids.

one moreoxygen atom

most“common”

one lessoxygen

two lessoxygen

HClO4

perchloric acid

HClO3

chloric acid

HClO2

chlorous acid

HClOhypochlorous acid

H2SO4

sulfuric acid

H2SO3

sulfurous acid

H3PO4

phosphoric acid

H3PO3

phosphorous acid

H3PO2

hypophosphorous acid

HNO3

nitric acid

HNO2

nitrous acid

(HNO)2

hyponitrous acid

Naming Simple Chemical Compounds

Ionic (metal and nonmetal) Covalent (2 nonmetals)

Metal

Formsonly onepositive

ion

Formsmore than

one positiveion

Nonmetal

Use the name of element

Use elementname followed

by a Romannumeral to

show the charge

Firstnonmetal

Secondnonmetal

Beforeelement name

use a prefixto matchsubscript

Use a prefixbefore

element name and end with ide

SingleNegative

Ion

Polyatomic Ion

Use the nameof the

element, butend with ide

Use thename of

polyatomicion (ate or

Ite)

NomenclaturePOPO44

3-3-

phosphate ionphosphate ion

CC22HH33OO22--

acetate ionacetate ion

HC2H3O2

Acetic Acid

Two nonmetals Multiple-charge cation Everything else

Romannumeral

Polyatomic ions OK

Roman numeralfor name only

Polyatomic ions

Greek prefixes

Charge

Criss-CrossRule

Romannumeral

OK

Where would you file this?

VCrO4

BaO

CBr4

Nb(ClO4)5

SCl2Rb2SO4

dinitrogen pentoxide

platinum (IV) iodate

ammonium chlorate

potassium iodide

nitrogen trichloride

manganese (V) sulfide

vanadium (II) chromate

VCrO4

N2O5

dinitrogen pentoxide

barium oxide

BaO

Pt(IO3)4

platinum (IV) iodate

carbon tetrabromide

CBr4

NH4ClO3

ammonium chlorate

niobium (V) perchlorate

Nb(ClO4)5

KI

potassium iodide

sulfur dichloride

SCl2

NCl3

nitrogen trichloride

rubidium sulfate

Rb2SO4

Mn2S5

manganese (V) sulfide

PRACTICE

Learning Check

Complete the names of the following binary compounds:

Na3N sodium ________________

KBr potassium ________________

Al2O3 aluminum ________________

MgS _________________________

- calcium hydroxide

- copper(II) sulfate

- ammonium nitrate

- cobalt(III) carbonate

Ca(OH)2

CuSO4

NH4NO3

Co2(CO3)3

Compounds containing polyatomic ions

ch. 7 (con’t.) formula writing & naming of compunds

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