Chapter 4Chapter 4

Section 3 Section 3

Compound names and formulasCompound names and formulas

Naming Ionic CompoundsNaming Ionic Compounds

BiBinary compounds (Compounds with just nary compounds (Compounds with just two elements) Natwo elements) Na22SS

1. Name the first element - Sodium1. Name the first element - Sodium

2. Name the root of the second 2. Name the root of the second element – “Sulf”element – “Sulf”

3. Add the ending “ide” to the root3. Add the ending “ide” to the root

Sodium SulfideSodium Sulfide

ALL binary compounds will end with “ide”. *There is an exception – compounds with ammonium can also end in “ide”….. Ammonium Bromide

Naming ionic compoundsNaming ionic compounds

The first name is the name of the The first name is the name of the cationcation Example: CaClExample: CaCl22 has first name calcium has first name calcium

The last name has the name of the The last name has the name of the anionanion. . (Anion names always end in “ide” unless (Anion names always end in “ide” unless they are from your polyatomic ion chart.)they are from your polyatomic ion chart.)

Example: CaClExample: CaCl22 has last name chloride, has last name chloride, so CaClso CaCl22 is calcium chloride is calcium chloride

Name these ionic Name these ionic compoundscompounds 1. BaF1. BaF22

2. K2. K22SeSe

3. CaS3. CaS 4. AlF4. AlF33

5. LiH5. LiH

Inonic CompoundsInonic Compounds

Some common CationsSome common Cations Name and Symbol Ion chargeName and Symbol Ion charge

Cesium ion, Cs + 1Lithium ion, Li + 1Potassium ion, K + 1Rubidium ion, Rb + 1Sodium ion, Na + 1Barium ion, Ba + 2Beryllium ion, Be + 2Calcium ion, Ca + 2Magnesium ion, Mg + 2Strontium ion, Sr + 2Aluminum ion, Al + 3

Some common AnionsSome common Anions Name and Symbol Ion chargeName and Symbol Ion charge

Fluorine, F FluorIDE - 1Chlorine, Cl ChlorIDE - 1Bromine, Br BromIDE - 1Iodine, I IodIDE - 1

Oxygen, O OxIDE - 2Sulfur, S SulfIDE - 2Nitrogen, N NitrIDE - 3

Some cation names must Some cation names must show their chargeshow their charge

Transition metals may form several Transition metals may form several cations each with a different charge. cations each with a different charge.

These cations must have a Roman These cations must have a Roman Numeral in parenthesis. The Roman Numeral in parenthesis. The Roman Numeral shows the cation’s charge.Numeral shows the cation’s charge.

Formulas with transition Formulas with transition metals………..metals………..

EXAMPLE:EXAMPLE: Fe Fe22OO33 - Look - Look first first at the element at the element

combined with the transition. Oxygen forms a -combined with the transition. Oxygen forms a -2 ion , if there are 3 atoms each with a -2 2 ion , if there are 3 atoms each with a -2 charge there is a total charge of -6 ..So if Iron charge there is a total charge of -6 ..So if Iron has 2 atoms, the total charge must equal +6. has 2 atoms, the total charge must equal +6. Then this is made of Fe +3 ions (+3 X 2 = +6), Then this is made of Fe +3 ions (+3 X 2 = +6), so it is named Iron (III) Oxide; so it is named Iron (III) Oxide;

FeO is made of Fe +2 ions so it is named Iron FeO is made of Fe +2 ions so it is named Iron (II) Oxide.(II) Oxide.

What are the charges on What are the charges on ions?ions?

Ionic compounds that Ionic compounds that contain more than 2 contain more than 2 elementselements

Compounds containing polyatomic Compounds containing polyatomic ions have charges listed on your ions have charges listed on your polyatomic ion chart.polyatomic ion chart.

*Notice that all “ate”and “ite” suffixes are compounds that have oxygen in them.

Writing formulas for Ionic Writing formulas for Ionic CompoundsCompounds

What is the chemical formula for aluminum fluorWhat is the chemical formula for aluminum fluorideide??1.1. List the symbols for each ionList the symbols for each ion

Al +3 F -1Al +3 F -12.2. Write the symbols for the ions with the cation first…. Write the symbols for the ions with the cation first….

Al Al+3+3 F F-1-1

3.3. Find the least common multiple of the ions charges, Find the least common multiple of the ions charges, so that the positive and negative charges will so that the positive and negative charges will balance…… need total of 3 negative charges to balance…… need total of 3 negative charges to balance with Al’s 3 positive charges.balance with Al’s 3 positive charges.

4.4. Write the chemical formula, indicating with subscripts Write the chemical formula, indicating with subscripts how many of each ion are needed to make a neutral how many of each ion are needed to make a neutral compound…… AlFcompound…… AlF3 3 leave the charges offleave the charges off

Practice writing ionic Practice writing ionic formulasformulas

1. Ca1. Ca2+2+ combined with F combined with F--

CaFCaF22

2. Co2. Co3+3+ combined with PO combined with PO443-3-

CoPOCoPO44

3. Ni3. Ni2+2+ combined with OH combined with OH--

Ni(OH) Ni(OH) 22

More practiceMore practice 1. calcium combined with oxygen1. calcium combined with oxygen

CaCa2+2+ OO2-2-

CaOCaO 2. potassium combined with oxalate2. potassium combined with oxalate

KK1+1+ C C22OO442-2-

KK22CC22OO44

3. barium hydrogen sulfate3. barium hydrogen sulfate

BaBa2+ 2+ HSOHSO441-1-

Ba(HSOBa(HSO44))22

Practice makes perfect only Practice makes perfect only if you practice perfect!if you practice perfect! Write formulas for:Write formulas for:

Calcium sulfideCalcium sulfide CaCa2+2+ S S2-2-

CaSCaS Potassium sulfidePotassium sulfide KK+1+1 S S2-2-

KK22SS

Practice makes perfect only Practice makes perfect only if you practice perfect!if you practice perfect! Write formulas for:Write formulas for:

Calcium sulfiteCalcium sulfite CaCa2+2+ SO SO33

2-2-

CaSOCaSO33

Potassium sulfatePotassium sulfate KK+1+1 SO SO44

2-2-

KK22SOSO44

Practice makes perfect only Practice makes perfect only if you practice perfect!if you practice perfect! Write formulas for:Write formulas for:

Gallium oxideGallium oxide GaGa3+3+ O O2-2-

GaGa22OO33

Ammonium PhosphiteAmmonium Phosphite NHNH44

+1+1 PO PO333-3-

(NH(NH44) ) 33POPO33

Some Transition Metal Some Transition Metal CationsCations

Ion name SymbolIon name SymbolCopper (I)Copper (I) Cu +1 Cu +1Copper (II)Copper (II) Cu +2 Cu +2Iron (II) Iron (II) Fe +2 Fe +2Iron (III) Fe +3Iron (III) Fe +3Nickel (II) Ni +2Nickel (II) Ni +2Nickel (III) Ni +3Nickel (III) Ni +3Lead (II)Lead (II) Pb +2 Pb +2Lead (IV) Pb +4Lead (IV) Pb +4Mercury (I)Mercury (I) Hg +1 Hg +1Mercury (II) Hg +2Mercury (II) Hg +2Gold ((I)Gold ((I) Au +1 Au +1Gold (III)Gold (III) Au +3 Au +3

Ion name SymbolIon name SymbolChromium (II)Chromium (II) Cr +2Cr +2Chromium (III)Chromium (III) Cr +3Cr +3Tin (II) Tin (II) Sn +2Sn +2Tin (IV)Tin (IV) Sn +4Sn +4Titanium (II)Titanium (II) Ti +2 Ti +2 Titanium (III)Titanium (III) Ti +3Ti +3Titanium (IV)Titanium (IV) Ti +4Ti +4Manganese (II)Manganese (II) Mn +2Mn +2Manganese (III)Manganese (III) Mn +3Mn +3Manganese (IV)Manganese (IV) Mn +4Mn +4Manganese (VI)Manganese (VI) Mn + 6Mn + 6Manganese (VII)Manganese (VII) Mn + 7Mn + 7

Math Skills…..Math Skills…..

Write formulas for the Write formulas for the following ionic compounds:following ionic compounds:

1.1. Lithium oxide Lithium oxide

2.2. Beryllium chlorideBeryllium chloride

3.3. Titanium (III) nitrideTitanium (III) nitride

4.4. Cobalt (III) hydroxideCobalt (III) hydroxide

LiO2

BeCl2

TiN

Co(OH)3

Naming Covalent Naming Covalent compoundscompounds

Covalent compounds Covalent compounds are named using are named using different rules than different rules than those used to name those used to name ionic compoundsionic compounds

Numerical prefixes Numerical prefixes are used to name are used to name covalent compounds covalent compounds of two elementsof two elements

Number of atoms Prefix 1 Mono 2 Di- 3 Tri- 4 Tetra- 5 Penta- 6 Hexa- 7 Hepta- 8 Octa- 9 Nona- 10 Deca-

Dinitrogen tetroxide N2O4

has 2 Nitrogen atoms and 4 Oxygen atoms.

What about covalent What about covalent compounds?compounds?

Many covalent compounds are named with Many covalent compounds are named with prefixes.prefixes.

Examples:Examples: COCO22

SOSO22

HH22OO55

Many covalent compounds Many covalent compounds are hydrocarbons with are hydrocarbons with special namesspecial names

Examples:Examples: CHCH44

CC22HH66

CC22HH44

CC22HH22

Naming non-binary Naming non-binary compounds (polyatomics)compounds (polyatomics)

Use the first element nameUse the first element name Add the polyatomic nameAdd the polyatomic name

****A ****A hinthint – any time you see a compound – any time you see a compound with three or more elements it is a good with three or more elements it is a good sign that it may include a polyatomic***sign that it may include a polyatomic***

CHECK YOUR LISTCHECK YOUR LIST

Example: NaNOExample: NaNO3 3 - -

Name these…..Name these…..

Mg(NOMg(NO33))22

Pb(OH)Pb(OH)22

CuCOCuCO33

KK33POPO44

NHNH44ClCl

Chemical Formulas for Chemical Formulas for Covalent CompoundsCovalent Compounds

A compound’s simplest formula as its A compound’s simplest formula as its empirical formulaempirical formula

Different compounds can have the same Different compounds can have the same empirical formulaempirical formula

Molecular formulas are determined from Molecular formulas are determined from empirical formulasempirical formulas

Check your Check your understandingunderstanding

ASSIGNMENTSASSIGNMENTS

Writing Binary formulasWriting Binary formulas

Naming Binary Compounds (Ionic)Naming Binary Compounds (Ionic)

Naming Binary Compounds (Covalent)Naming Binary Compounds (Covalent)

Formulas with Polyatomic IonsFormulas with Polyatomic Ions

Naming of Non-Binary CompoundsNaming of Non-Binary Compounds

Naming Compounds (Mixed)Naming Compounds (Mixed)

Compound Names and Compound Names and FormulasFormulas

Empirical formula – the simplest chemical Empirical formula – the simplest chemical formula of a compound that tells the formula of a compound that tells the smallest whole-number ratio of atoms in smallest whole-number ratio of atoms in the compoundthe compound

Molecular formula – a chemical formula Molecular formula – a chemical formula that reports the actual numbers of atoms that reports the actual numbers of atoms in one molecule of a compoundin one molecule of a compound

4.3