Chapter 2Chapter 2

Chemical NamesChemical Names

and Formulasand Formulas

Naming Ions

IE X + energy X+ + e-

Atom Ion

Cation

• CationCation• Positive IonPositive Ion

• MetalMetal

• Loses ElectronsLoses Electrons

Cation t looks like a + Cation t looks like a +

Naming Ions

EA X + e- X- + energy

Atom Ion

Anion

• AnionAnion • Negative IonNegative Ion

• NonmetalNonmetal

• Gains ElectronsGains Electrons

Anion n in middle stands for negativeAnion n in middle stands for negative

Monoatomic IonMonoatomic Ion

Monatomic IonMonatomic Ion – Ion that consists of a – Ion that consists of a single atomsingle atom• CationCation

• Positive IonPositive Ion

• MetalMetal

• Loses ElectronsLoses Electrons

• AnionAnion• Negative IonNegative Ion

• NonmetalNonmetal

• Gain ElectronsGain Electrons

Rules for Ion Names/Symbols: Cation

Metals = use element name

= use symbol with superscript charge

= superscript is written in air

Alkali Metals Transition Metals

Hydrogen H+1 Silver Ag+1

Lithium Li+1 Gold Au+1

Sodium Na+1

Potassium K+1

Rules for Ion Names/Symbols: Cation

Metals = use element name

= use symbol with superscript charge

= superscript is written in air

Alkaline Earth Metals Transition Metals

Magnesium Mg+2 Cobalt Co+2

Calcium Ca+2 Nickel Ni+2

Strontium Sr+2 Zinc Zn+2

Barium Ba+2

Rules for Ion Names/Symbols: Cation

Some metals have multiple charges.

Stock System uses Roman numerals.

Roman numerals = charge!!

1 I 6 VI

2 II 7 VII

3 III 8 VIII

4 IV 9 IX

5 V 10 X

.

Rules for Ion Names/Symbols: Cation

Copper (I) Cu+1 Tin (II) Sn+2

Copper (II) Cu+2 Tin (IV) Sn+4

Iron (II) Fe+2 Manganese (II) Mn+2

Iron (III) Fe+3 Manganese (IV) Mn+4

Lead (II) Pb+2

Lead (IV) Pb+4

Rules for Ion Names/Symbols: Anion

Nonmetals = use element name with ‘ide’

= use symbol with superscript charge

= superscript is written in air

Halogens

Fluorine Fluoride F-1

Chlorine Chloride Cl-1

Bromine Bromide Br-1

Iodine Iodide I-1

Rules for Ion Names/Symbols: Anion

Nonmetals = use element name with ‘ide’

= use symbol with superscript charge

= superscript is written in air

Oxygen Family Nitrogen Family

Oxygen Oxide O-2 Nitrogen Nitride N-3

Sulfur Sulfide S-2 Phosphorus

Carbon Family Phosphide P-3

Carbon Carbide C-4

Rules for Ion Names/Symbols: Cation or Anion ?

Multiples can be cation or anion.

It depends on what other ion is around it.

Cation Anion

Carbon C+4 Carbide C-4

Nitrogen N+5 Nitride N-3

Phosphorus P+5 Phosphide P-3

Binary CompoundsBinary Compounds

Composed of 2 elementsComposed of 2 elements• Can be either ionic or molecularCan be either ionic or molecular

Binary Ionic CompoundsBinary Ionic Compounds

Consist of IonsConsist of Ions• Metallic IonsMetallic Ions bonded to bonded to Nonmetal ionsNonmetal ions

oror

• CationsCations bonded to bonded to AnionsAnions

Writing Names forBinary Ionic Compounds

Steps

1. Use ION names.

2. Write the CATION name.

3. Then write the ANION name.

For example,

NaCl becomes Sodium Chloride

MgBr2 becomes Magnesium Bromide

CuO becomes Copper (II) Oxide

Writing Formulas for Writing Formulas for Binary Ionic CompoundsBinary Ionic Compounds

StepsSteps1.1. USEUSE the the IONS.IONS.

2.2. Write the symbol for the Write the symbol for the CATIONCATION..

3.3. Then write the symbol for the Then write the symbol for the ANION.ANION.

4.4. Balance the charges to zero. The Balance the charges to zero. The subscripts denotes the number of ions subscripts denotes the number of ions needed to balance the charges to zero.needed to balance the charges to zero.

Example Example ((Level 1Level 1))

Sodium ChlorideSodium Chloride

NaNa+1+1 ClCl-1-1

NaNaClCl

Example Example (Level 1)(Level 1)

Magnesium OxideMagnesium Oxide

OO-2-2MgMg+2+2

MgMgOO

Example Example (Level 1)(Level 1)

Aluminum NitrideAluminum Nitride

AlAl+3+3

AlAlNN

NN-3-3

PracticePractice

1.1. Potassium IodidePotassium Iodide

2.2. Calcium SulfideCalcium Sulfide

3.3. Aluminum PhosphideAluminum Phosphide

4.4. Gold FluorideGold Fluoride

5.5. Barium OxideBarium Oxide

6.6. Sodium BromideSodium Bromide

7.7. Strontium SulfideStrontium Sulfide

Example Example (Level 2)(Level 2)

Lithium OxideLithium Oxide

LiLi+1+1 OO-2-2

LiLi22OO

LiLi+1+1

Example Example (Level 2)(Level 2)

Calcium FluorideCalcium Fluoride

CaCa+2+2 FF-1-1

CaCaFF22

FF-1-1

Example Example (Level 2)(Level 2)

Aluminum IodideAluminum Iodide

AlAl+3+3 II-1-1

AlAlII33

II-1-1II-1-1

Practice

1.1. Potassium OxidePotassium Oxide

2.2. Strontium BromideStrontium Bromide

3.3. Aluminum ChlorideAluminum Chloride

4.4. Gold SulfideGold Sulfide

5.5. Silver NitrideSilver Nitride

6.6. Barium FluorideBarium Fluoride

7.7. Calcium IodideCalcium Iodide

Example Example (Level 3)(Level 3)

Aluminum SulfideAluminum Sulfide

AlAl+3+3 SS-2-2

AlAl22SS33

SS-2-2 SS-2-2AlAl+3+3

Example Example (Level 3)(Level 3)

Tin (IV) NitrideTin (IV) Nitride

SnSn+4+4 NN-3-3

SnSn33NN44

NN-3-3 NN-3-3SnSn+4+4SnSn+4+4 NN-3-3

Polyatomic IonsPolyatomic Ions

Polyatomic IonsPolyatomic Ions – Ions composed of – Ions composed of more than one atommore than one atom • Most end in Most end in iteite or or ateate

Polyatomic Ions

Ammonium NH4+1

Cyanide CN-1

Hydroxide OH-1

Nitrite NO2-1 Nitrate NO3

-1

Carbonate CO3-2

Sulfite SO3-2 Sulfate SO4

-2

Phosphite PO3-3 Phosphate PO4

-3

Example Example (Level 1)(Level 1)

Ammonium ChlorideAmmonium Chloride

ClCl--

NHNH44ClCl

NHNH44+1+1

Example Example (level 1)(level 1)

Barium SulfateBarium Sulfate

BaBa+2+2 SOSO44-2-2

BaBaSOSO44

Polyatomic Ions OnlyPolyatomic Ions Only

When writing compounds if you need When writing compounds if you need more than one polyatomic ion you more than one polyatomic ion you must add must add parenthesisparenthesis

Example Example (Level 2)(Level 2)

Ammonium SulfateAmmonium Sulfate

NHNH44+1+1 SOSO44

-2-2

NHNH4422SOSO44

NHNH44+1+1

((NHNH44))22SOSO44

Example Example (Level 2)(Level 2)

Barium HydroxideBarium Hydroxide

BaBa+2+2 OHOH-1-1

BaBaOHOH22 BaBa((OHOH))22

OHOH-1-1

Practice

1. Ammonium Phosphate

2. Calcium Hydroxide

3. Aluminum Nitrate

4. Magnesium Sulfate

5. Tin (IV) Carbonate

6. Strontium Sulfate

7. Barium Nitrate

Nomenclature Nomenclature of Ionic Compoundsof Ionic Compounds

StepsSteps

1.1. Use the names of the Use the names of the ionsions..

2.2. Write the Write the metalmetal first followed by the first followed by the nonmetalnonmetal

3.3. The The subscriptssubscripts take care of themselves take care of themselves

Example Example

NaClNaCl

NaNa+1+1

SodiumSodium ChlorideChloride

ClCl-1-1

ExampleExample

CaClCaCl22

CaCa+2+2

CalciumCalcium ChlorideChloride

ClCl-1-1 ClCl-1-1

Example Example

CuSOCuSO44

CuCu+2+2

Copper (II) Copper (II) SulfateSulfate

SOSO44-2-2

Practice

1.1. NaINaI

2.2. (NH(NH44))22SOSO44

3.3. MgBrMgBr22

4.4. AlAl22(CO(CO33))33

5.5. CuOCuO

6.6. FeFe22OO33

7.7. CaCa33PP22

Formula Writing and NomenclatureFormula Writing and NomenclatureCovalent (Molecular) CompoundsCovalent (Molecular) Compounds

StepsSteps

1.1. Write the first Write the first nonmetalnonmetal symbol followed symbol followed by the second by the second nonmetal nonmetal symbolsymbol..

2.2. The Greek prefixes denote the The Greek prefixes denote the subscriptssubscripts..

3.3. Do not need to balance the charges.Do not need to balance the charges.

Greek PrefixesGreek Prefixesfor Molecular Compoundsfor Molecular Compounds

1 Mono 6 Hexa

2 Di 7 Hepta3 Tri 8 Octa4 Tetra 9 Nona5 Penta 10 Deca

ExampleExampleCarbonCarbon DiDioxideoxide

CC

CCOO22

OO22

ExampleExample

Dinitrogen Monoxide

NN

NN22OO

OO22 11

PracticePractice

1.1. Sulfur DioxideSulfur Dioxide

2.2. Trichlorine TetraiodideTrichlorine Tetraiodide

3.3. Pentaphosphorus HexasulfidePentaphosphorus Hexasulfide

4.4. Heptaoxygen OctaselenideHeptaoxygen Octaselenide

5.5. Nonafluorine DecanitrideNonafluorine Decanitride

6.6. Dinitrogen PentoxideDinitrogen Pentoxide

7.7. Carbon TetrachlorideCarbon Tetrachloride

Naming Molecular CompoundsNaming Molecular Compounds

RulesRules

1.1. Write the 1Write the 1st st element name.element name.

2.2. Write the 2Write the 2ndnd element name with an element name with an ending of “ending of “ideide””

3.3. Add Add Greek prefixes Greek prefixes to both names. The to both names. The Greek prefix Greek prefix denotes the subscript.denotes the subscript.

4.4. Do not use a mono on the 1Do not use a mono on the 1stst element element name. name.

Example

SiSiOO22

SiliconSilicon OxygenOxygen

SiliconSilicon DiDioxideoxide

DiDiideide

ExampleExample

PP44FF66

PhosphorusPhosphorus FluorineFluorine

TetraTetraphosphorusphosphorus HexaHexafluoridefluoride

HexaHexaideide

TetraTetra

PracticePractice

1.1. COCO

2.2. SiSi22FF

3.3. OO33BrBr77

4.4. ISIS

5.5. ONON44

6.6. FF44HH33

7.7. PP77SS99

Halogenated Oxyanions

Name:

Prefix Suffix

Hypo root ite

root ite

root ate

Per root ate

Example:

Chlorine

Hypochlorite ClO-1

Chlorite ClO2-1

Chlorate ClO3-1

Perchlorate ClO4-1

Try Bromine and Iodine.

Polyatomic Oxyacids

Example:

Chlorine

Hypochlorite ClO-1

Chlorite ClO2-1

Chlorate ClO3-1

Perchlorate ClO4-1

Example:

Chlorine

Hypochlorous acid HClO

Chlorous acid HClO2

Chloric acid HClO3

Perchloric acid HClO4

Binary Acids

Formula: Hydrogen w Halogen

Name: Hydro+Root+ic Acid

HCl Hydrochloric Acid

HBr Hydrobromic Acid

HI Hydroiodic Acid

HF Hydrofluoric Acid

Alkanes

Methane Ethane Propane Butane Pentane

Alcohols

Methanol Ethanol Propanol Butanol Pentanol

Other functional groups?

Alcohols Ethers Aldehydes Ketones Carboxylic acid Ester Amine Amide

Formula weights/Molar Mass

The sum of atomic weights for a compound (in amu)

The number of grams in one mole of a substance (in g)

Lewis Dot Structures

For atoms For ionic

compounds For molecular

compounds

LDS: Neutral Molecules

Draw the dot structures of each atom Share one atom for each element (to make

a single bond between each element) Count electrons around each atom If octets are incomplete, share more

electrons between atoms

LDS: Negatively Charged Molecules

Repeat procedure for uncharged molecules Add one electron for each negative charged

atom

LDS: Positively charged molecules

Same procedure as negative… except remove one electron

Web Practice Site

http://www.fernbank.edu/Chemistry/nomen.html