Chemical Bonds

What is a chemical bond? Why do chemical bonds form?

• A chemical bond is a type of attractive force that forms between atoms.

• All atoms react to obtain a stable and full outer electron configuration.

• Only noble gases naturally possess a stable arrangement that includes a perfect balance and distance between the positive protons and negative electrons.

The Octet Rule• All noble gases except He has an s2p6 configuration (Note:

2 + 6 = 8….”octet” means the number 8)

• Octet rule: atoms tend to gain, lose, or share electrons until they are surrounded by 8 valence electrons (4 electron pairs).

• Caution: there are many exceptions to the octet rule. For example; H, He Li and Be follow “duet rule.”

The Octet RuleThe Octet Rule

How do atoms achieve a full “octet?”

• Atoms will gain, lose or share electrons to achieve a stable, completely full outer electron shell. (called valence shell).

• The gaining or losing of valence electrons is a CHEMICAL REACTION!!

• The difference in electronegativity values of atoms, when placed into contact with each other, determines the loss or gain of electrons.

Bonding and ElectronegativityBonding and Electronegativity

Electronegativity• Electronegativity: The ability of one atom or group of

atoms to attract electrons to itself.• Pauling set electronegativities on a scale from 0.7 (Cs) to

4.0 (F).• Electronegativity increases

• across a period and • down a group.

Electronegativities of ElementsElectronegativities of ElementsElectronegativity

http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/reaction/bonding1.swfAnimation of electron transfer between selected atoms.

Lewis Structures

-Chemical reactions involve valence electrons.

-Lewis structures are shorthand version of atoms showing only their valence electrons.

-Why?? Only valence electrons transferred

during most chemical reactions.

Lewis Symbols

Examples of Longhand and Lewis Electron SymbolsExamples of Longhand and Lewis Electron Symbols

http://www.mhhe.com/physsci/chemistry/chang7/esp/folder_structure/bo/m2/s1/index.htmAnimation of Lewis Diagrams

Chemical Bonding

…atoms share electrons to get a full valence shell

Covalent Bonds

C 2s2 2p2 (4 v.e–)

F 2s2 2p5 (7 v.e–)

both need 8 valence electrons for a full outer shell(octet rule)

1s2

1s2

Covalent bonding

F F

• Fluorine has seven valence electrons• A second F atom also has seven• By sharing electrons• Both end with full orbitals (stable octets)

8 Valence electrons

8 Valence electrons

Chemical Bonding

Ionic Bonds:atoms give up or gain electrons and are attracted to each other by coulombic attraction

Na loses an e–

Na Na1+ + e–

Cl gains an e–

Cl + e– Cl1–

ionic compounds = salts Na1+ + Cl1– NaCl

K1+ + NO31– KNO3

where NO31– is a polyatomic ion: a charged group of atoms

that stay together

Ionic Bonding

-

-

-

-

-

- -

-

-

-

-

- -

-

- -

n = 2

Na[Ne]3s1

n = 3

n = 3

+

-

-

-

-

-

- -

--

-

- -

-

- -

-

Cl[Ne]3s23p5

Na+

[Ne]Cl-

[Ne]3s23p6

NaCl

Transfer of electrons to achieve a stable octet (8 electrons in valence shell).

Copyright © 2007 Pearson Benjamin Cummings. All rights reserved.

Na + Cl2 NaCl

sodium metal and chlorine gas react to form sodium chloride

2 2

Covalent Bonding

-

-

-

-

n = 1

O[He]2s22p4

n = 2

+

-

----

-

-

O2

Sharing of electrons to achieve a stable octet (8 electrons in valence shell).

-

-

-

-

-

-

-

-

-

-

-

-

-

-

-

-

-

O[He]2s22p4

Properties of Salts

VERY HARD each ion is bonded to several oppositely-charged ions

HIGH MELTING POINTS many bonds must be broken

BRITTLE with sufficient force, like atoms are brought next to each other and repel

Vocabulary

• Chemical Bond

– attractive force between atoms or ions that binds them together as a unit

– bonds form in order to…• decrease potential energy (PE)

• increase stability

Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Vocabulary

CHEMICAL FORMULA

molecularformula

formulaunit

IONIC COVALENT

COCO22NaClNaClCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Vocabulary

COMPOUND

ternarycompound

binarycompound

2 elementsmore than 2

elements

NaNONaNO33NaClNaClCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Vocabulary

ION

polyatomicIon

monatomicIon

1 atom 2 or more atoms

NONO33--NaNa++

Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

IONIC COVALENT

Bond Formation

Type of Structure

Solubility in Water

Electrical Conductivity

OtherProperties

e- are transferred from metal to nonmetal

high

yes (solution or liquid)

yes

e- are shared between two nonmetals

low

no

usually not

MeltingPoint

crystal lattice true molecules

Types of Bonds

Physical State

solid liquid or gas

odorousCourtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

“electron sea”

METALLIC

bond formation

type of structure

solubility in water

conductivity

other properties

melting point

Types of Bonds

physical state

electrons are delocalized among metal atoms

very high

yes (any form)

no

malleable, ductile, lustrous

solid

Courtesy Christy Johannesson www.nisd.net/communicationsarts/pages/chem

Ionic Bonding - Crystal Lattice

Types of Bonds

Table salt

Ionic Bonding - Crystal Lattice

Types of Bonds

Table salt

Covalent Bonding - True Molecules

Types of Bonds

Diatomic Molecule

Ammonia

Nitrogen

Water

Lewis Structure

Lewis structure: a model of a covalent molecule thatshows all of the valence electrons

1. Two shared electrons make a single covalent bond,

four make a double bond, etc.

2. unshared pairs: pairs of un-bonded valence electrons

3. Each atom needs a full outer shell, i.e., 8 electrons. Exception: H needs 2 electrons

Lewis Structure

carbon tetrafluoride (CF4)

o

Co

o

o x

xx

x

x x

F x

o

Co

o

ox

xx

x

x x

F x

x x

x

x

x x

F x

x

xx

x

x

F x

x

x

xx

x x

F x

xCx

xx

x

x x

F

x x

x

x x

F x

x

xx

x F x

x

xx

x x

F x

x

covalent compounds = molecular compounds(have lower melting points than do ionic compounds)

Lewis Structure

o

Co

o o

x

Ho

Co

o oH x

x

H

xH

x H CH

H

H

H

x

xxx

x x

I x

o

No

o o

o o

No

o ox

xxx

x x

I x

x x

xx

x x

I x

xxx

x x I

x

x

o o

Nx

xxx

x x

I

x xx

x x

I x

xx

x x I

x

x

o

o

Co

o o x

xxx

xO x

x

xxx

xO x

x

xxx

xO x

o

Co

o o O = C = O

x x

x x x x

x x

methane (CH4)

carbon dioxide (CO2)

nitrogen triiodide (NI3)

Properties of Metalsconduct heat and electricity; ductile; malleable

Other Types of Bondsdipole-dipole forceshydrogen bondsLondon dispersion forces ion-dipole forces (solutions)

Writing Formulas of Ionic Compounds

chemical formula: has neutral charge;shows types of atoms and how many of

each

To write an ionic compound’s formula, we need:1. the two types of ions2. the charge on each ion

Na1+ and F1–

Ba2+ and O2–

Na1+ and O2–

Ba2+ and F1–

NaF

BaO

Na2O

BaF2

sodium fluoride

barium oxide

sodium oxide

barium fluoride

Ca3P2

Formula Unit

Ca2+

Ca2+

Ca2+

P3-

P 3-

Ca2+

P3- Ca2+

P3- Ca2+

Ca2+ and P3– Ca3P2 calcium phosphide

InBr3BaS

Criss-Cross Rule

criss-cross rule: charge on cation / anion

“becomes” subscript of anion / cation

** Warning: Reduce 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

(NH4)3N

Fe2(Cr2O7)3

Sn(SO4)2

NH4ClO3

Mg(NO2)2

BaSO4

Writing Formulas w/Polyatomic Ions

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

Ba2+ and SO4

2–

Mg2+ and NO2

1–

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

?

Compounds Containing Polyatomic Ions

Insert name of ion where it should go in the compound’s name.

Write formulas:

iron (III) nitrate

ammonium phosphide

ammonium chlorite

zinc phosphate

lead (II) permanganate

Fe(NO3)3

(NH4)3P

NH4ClO2

Zn3(PO4)2

Pb(MnO4)2

Fe3+ NO31–

NH41+ P3–

NH41+ ClO2

1–

Zn2+ PO43–

Pb2+ MnO41–

3

3

3 2

2

Write names:

(NH4)2S2O3

AgBrO3

(NH4)3N

U(CrO4)3

Cr2(SO3)3

Writing Formulas of Ionic Compounds

ammonium thiosulfate

silver bromate

ammonium nitride

uranium (VI) chromate

chromium (III) sulfite

CrO42–

SO32–

3

32 Cr

U?

?

6+

3+

Writing Formulas of Covalent Molecules

Covalent Moleculescontain two types of nonmetals

Key: FORGET CHARGES

What to do:Use Greek prefixes to indicate how many atoms

of each element, but don’t use “mono” on first element.

1 – mono 6 – hexa2 – di 7 – hepta3 – tri 8 – octa4 – tetra 9 – nona5 – penta 10 – deca

Writing Formulas of Covalent Molecules

EXAMPLES:

carbon dioxide

CO

dinitrogen trioxide

N2O5

carbon tetrachloride

NI3

CO2

carbon monoxide

N2O3

dinitrogen pentoxide

CCl4

nitrogen triiodide

Cu 2 Br1–

Cu Br1–

2 Fe 3 O2–

Fe O2–

Stock Systemof nomenclature

4. Write name of anion.

FeO

Fe2O3

CuBr

CuBr2

iron (II) oxide

iron (III) oxide

copper (I) bromide

copper (II) bromide

?

?

?

?

A. To name, given the formula:

1. Figure out charge on cation.

2. Write name of cation.

3. Write Roman numerals in ( ) to show cation’s charge.

Pb2+/Pb4+,Sn2+/Sn4+,transition elements (not Ag or Zn)

Multiple-Charge Cations with Elemental Anions

2+

3+

1+

2+

B. To find the formula, given the name:

2. Balance charges to write formula.

cobalt (III) chloride Co3+ Cl1– CoCl3

tin (IV) oxide Sn4+ O2– SnO2

tin (II) oxide Sn2+ O2– SnO

1. Write symbols for the two types of ions.

Element Latin root -ic -ous

gold, Au aur- Au3+ Au1+

lead, Pb plumb- Pb4+ Pb2+

tin, Sn stann- Sn4+ Sn2+

copper, Cu cupr- Cu2+ Cu1+

iron, Fe ferr- Fe3+ Fe2+

Traditional (OLD) System of Nomenclature…used historically (and still some today) to

name compounds w/multiple-charge cations

To use:1. Use Latin root of cation. 2. Use -ic ending for higher charge

“ -ous “ “ lower “ 3. Then say name of anion, as usual.

; (“icky” food is good for you!); (“delicious” food is not good for you!)

Cu2S

AuN

FeF2

plumbic phosphide

plumbous phosphide

stannic chlorideFe2+

Write formulas: Write names:

cuprous sulfide

auric nitride

ferrous fluoride

Pb3P4 3 Pb? 4 P3–

Cu1+

Pb3P2 3 Pb? 2 P3–

Au3+

SnCl4 Sn? 4 Cl1–

S2–

N3–

F1–

copper (I) sulfide

gold (III) nitride

iron (II) fluoride

lead (IV) phosphide

lead (II) phosphide

tin (IV) chloride

O2-

K1+

K1+

Mg2+

Br1-

Br1-

K Br

potassium atom bromine atom

e- e- Br1-K1+

potassium ion bromide ionpotassium bromide

K Br

potassium atom bromine atom

e-

Br1-K1+

potassium ion bromide ion

KBr

MgBr2 K2Omagnesium bromide potassium oxide

Ca2+

Al3+

K1+

Pb4+

Br1-

O2-

N3-

K1+

K1+

Mg2+

Br1-

Br1-

PO43-

S2-

Cu2+

OH1-

OH1-NH41+

NO31-

?

Chemical Bonding Activity

Ca2+

Al3+

Na1+

Pb4+

OH1-

N2-

N3-

M1+

Mg2+

OH1-

OH1-

N3-

Pb4+

N3-

N3-

Pb4+

N3-

Pb4+

N3-

?

(nonmetal)M1+

(metal)

Pb4+ N3-

(metal)(metal)

M2+

(metal)

Pb3N4

lead (IV) nitrideor

plumbic nitride

Key

Cu2+

Al3+

K1+ Pb4+Br1-

O2-

N3-

K1+

K1+

Mg2+

Br1-

Br1-

N3-

N3-

Pb4+

N3-

Pb4+

N3-

1.

2.

3.

4. 5.

6. OH1-

OH1-

NH41+

NO31-

7.

KBr

K2O

MgBr2

AlN

Cu(OH)2

NH4NO3

Pb3N4

http://www.unit5.org/christjs/4bondingact.doc

Key

Fe2+

8. 9. 10.

Ca2+

Ca2+

Ca2+

PO43-

PO43-

PO43-

NH41+

NH41+

NH41+

O2-

Al3+

Al3+

O2-

O2-

O2-

11.

Ca3(PO4)2

(NH4)3PO4

FeOAl2O3

Key

12.

15.

O2-

O2-

Fe3+

Fe3+

O2-

O2-

O2-

13.

Pb4+

S2-

S2-

Pb4+

S2-

S2-

Pb2+ S2-

14.

Cu2+

Cu1+

Cu1+

16.

Fe2O3

Pb2S3

PbS

CuO

Cu2OPb2S4PbS2

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

Type II CationsCommon Type II Cations

Ion Stock System Traditional System

Fe 3+ iron (III) ferric Fe 2+ iron (II) ferrous Cu 2+ copper (II) cupric Cu 1+ copper (I) cuprous Co 3+ cobalt (III) cobaltic Co 2+ cobalt (II) cobaltous Sn 4+ tin (IV) stannic Sn 2+ tin (II) stannous Pb 4+ lead (IV) plumbic Pb 2+ lead (II) plumbous Hg 2+ mercury (II) mercuric Hg2 2+ mercury (I) mercurous

*Mercury (I) ions are always bound together in pairs to form Hg2 2+

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 90

Naming Binary Compounds

Formula Name

1 Hg2O ____________________

2 HgO ____________________

3 ________________ copper (II) fluoride

4 ________________ copper (I) sulfide

5 Cr2O3 ____________________

6 ________________ lead (IV) oxide

mercury (I) oxide

PbO2

mercury (II) oxide

CuF2

Cu2S

chromium (III) oxide

Li

3

H

1

He

2

C

6

N

7

O

8

F

9

Ne

10

Na

11

B

5

Be

4

H

1

Al

13

Si

14

P

15

S

16

Cl

17

Ar

18

K

19

Ca

20

Sc

21

Ti

22

V

23

Cr

24

Mn

25

Fe

26

Co

27

Ni

28

Cu

29

Zn

30

Ga

31

Ge

32

As

33

Se

34

Br

35

Kr

36

Rb

37

Sr

38

Y

39

Zr

40

Nb

41

Mo

42

Tc

43

Ru

44

Rh

45

Pd

46

Ag

47

Cd

48

In

49

Sn

50

Sb

51

Te

52

I

53

Xe

54

Cs

55

Ba

56

Hf

72

Ta

73

W

74

Re

75

Os

76

Ir

77

Pt

78

Au

79

Hg

80

Tl

81

Pb

82

Bi

83

Po

84

At

85

Rn

86

Fr

87

Ra

88

Rf

104

Db

105

Sg

106

Bh

107

Hs

108

Mt

109

Mg

12

Ce

58

Pr

59

Nd

60

Pm

61

Sm

62

Eu

63

Gd

64

Tb

65

Dy

66

Ho

67

Er

68

Tm

69

Yb

70

Lu

71

Th

90

Pa

91

U

92

Np

93

Pu

94

Am

95

Cm

96

Bk

97

Cf

98

Es

99

Fm

100

Md

101

No

102

Lr

103

La

57

Ac

89

1

2

3

4

5

6

7

Single-charge cationsMultiple-charge cations

Elemental anions

1+

2+

1+ 2+

3+ 1-2-3-

Periodic Table with

charges

Periodic Table with

charges

Binary Compounds Containing Two Nonmetals

To name these compounds, give the name of the less electronegative element first with the Greek prefix indicating the number of atoms of that element present, followed by the name of the more electronegative non-metal with the Greek prefix indicating the number of atoms of that element present and with its ending replaced by the suffix –ide.

Prefixes you should know:

Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca

1 2 3 4 5 6 7 8 9 10

Binary CompoundsContaining Two Nonmetals (Type III Compounds)

1. ________________ diarsenic trisulfide

2. ________________ sulfur dioxide

3. P2O5 ____________________

4. ________________ carbon dioxide

5. N2O5 ____________________

6. H2O ____________________

As2S3

SO2

diphosphorus pentoxide

CO2

dinitrogen pentoxide

dihydrogen monoxide

Prefixes – Binary Molecular CompoundsGreek Prefixes for Two Nonmetals

Number Indicated Prefixes

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

Binary Molecular Compounds

N2O dinitrogen monoxideN2O3 dinitrogen trioxideN2O5 dinitrogen pentoxide

ICl iodine monochlorideICl3 iodine trichloride

SO2 sulfur dioxideSO3 sulfur trioxide

Naming Binary CompoundsBinary Compound?

Metal Present?

Does the metal formmore than one cation?

Type IIIUse Greek

Prefixes

Type IUse the elementname for the cation.

Type IIDetermine the charge of the cation; use a Romannumeral after the cationname.

Yes

Yes

YesNo

No

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 98

Ternary Compounds

Ternary compounds are those containing three different elements. (NaNO3, NH4Cl, etc.). The naming of ternary compounds involves the memorization of several positive and negative polyatomic ions, (two or more atoms per ion), and adding these names to the element with which they combine.

i.e., Sodium ion, Na1+ added to the nitrate ion, NO31-, to give

the compound, NaNO3, sodium nitrate.

Binary rules for indicating the oxidation number of metals and for indicating the numbers of atoms present are followed. The polyatomic ions that shouldbe learned are listed in a separate handout.

(PO4)3-

Phosphate

PO43-

1 P 4 O @ 2- = 8-

@ 3- = 3-

11-

?@ 5+ = 5+

3-

Fluorine and oxygenoxygen are highly electronegative and will attractelectrons very strongly. Generally, phosphorus will be 3- oxidation state: however, when combining with oxygen, phosphorus will lose

five electrons and take on a 5+ oxidation charge.

phosphate

sulfate

carbonate

chlorate

nitrate

Polyatomic Ions - Memorize

phosphATE

sulfATE

carbonATE

chlorATE

nitrATE

PO43- ……………

SO42- ……………

CO32- …………..

ClO31- …………..

NO31- ………..….

Eight “-ATE’s”

Exceptions:

ammonium

hydroxide

cyanide

NH41+ ……………

OH1- ……………

CN1- …………..

Pattern to Memorizing Nomenclature

XY“-ide”

XYO3“-ate”

XYO2“-ite”

XYO“hypo___-ite”

XYO4“per___-ate”

normal 1 less oxygen 2 less oxygen1 more oxygen

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

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

Ternary Compounds

NaNO2 sodium nitrite

KClO3 potassium chlorate

Ca3(PO4)2 calcium phosphate

Fe(OH)3 iron (III) hydroxide

NaHCO3 sodium bicarbonate ‘sodium hydrogen carbonate’

ideCalcium hydroxide

Ca2+ OH1-

CaOH2

Ca(OH)2

Ca - OH

H

HO - Ca - OH

vs.

Common Polyatomic Ions

Names of Common Polyatomic Ions

Ion Name Ion Name

NH4 1+ ammonium CO3 2- carbonate

NO2 1- nitrite HCO3 1- hydrogen carbonate NO3 1- nitrate (“bicarbonate” is a widely SO3 2- sulfite used common name) SO4 2- sulfate ClO 1- hypochlorite HSO4 1- hydrogen sulfateClO2 1- chlorite

(“bisulfate” is a widely ClO3 1- chlorate used common name) ClO4 1- perchlorate OH 1- hydroxide C2H3O2 2- acetate CN 1- cyanide MnO4 1- permanganate PO4 3- phosphate Cr2O7 2- dichromate HPO4 2- hydrogen phosphate CrO4 2- chromate H2PO4 1- dihydrogen phosphate O2 2- peroxide

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 100 Print Version

Ternary Compounds

1. ________________ calcium phosphate

2. ________________ ammonium carbonate

3. ________________ aluminum sulfate

4. Na2SO4 ____________________

5. LiCN ____________________

6. Ba(ClO3)2 ____________________

7. ________________ copper (II) hydroxide

Ca3(PO4) 2

(NH4)2CO3

Al2(SO4)3

sodium sulfate

lithium cyanide

barium chlorate

Cu(OH)2

Magnesium Phosphate

Step 1: Magnesium Phosphate

Step 2: Mg2+ PO43-

Step 3: Mg (PO4)3 2

Step 4: Mg3(PO4)2

fluoride

sulfide

sulfide

chloride

bromide

phosphide

fluoride

iodide

chloride

oxide

phosphide

iridium (III)

calcium

titanium (IV)

platinum (II)

barium

strontium

potassium

zinc

manganese (IV)

gold (III)

sodium

dichromate

hydroxide

chromate

acetate

bromate

sulfate

cyanide

nitrite

chlorate

phosphate

nitrate

2(Cr2O7)3

(OH)2

(CrO4)2

(CH3COO)2

(BrO3)2

SO4

CN

(NO2)2

(ClO3)4

PO4

NO3

Ir

Ca

Ti

Pt

Ba

Sr

K

Zn

Mn

Au

Na

F3

S

S2

Cl2

Br2

3P2

F

I2

Cl4

2O3

3P

Ir2+,3+,4+,6+

Ca2+

Ti3+,4+

Pt2+,4+

Ba2+

Sr2+

K1+

Zn2+

Mn2,3,4,6,7+

Au1+,3+

Na1+

variable

fixed

variable

variable

fixed

fixed

fixed

fixed

variable

variable

fixed

fluoride

sulfide

sulfide

chloride

bromide

phosphide

fluoride

iodide

chloride

oxide

phosphide

iridium (III)

calcium

titanium (IV)

platinum (II)

barium

strontium

potassium

zinc

manganese (IV)

gold (III)

sodium

Ir

Ca

Ti

Pt

Ba

Sr

K

Zn

Mn

Au

Na

F3

S

S2

Cl2

Br2

3P2

F

I2

Cl4

2O3

3P

Ir2+,3+,4+,6+

Ca2+

Ti3+,4+

Pt2+,4+

Ba2+

Sr2+

K1+

Zn2+

Mn2,3,4,6,7+

Au1+,3+

Na1+

variable

fixed

variable

variable

fixed

fixed

fixed

fixed

variable

variable

fixed

dichromate

hydroxide

chromate

acetate

bromate

sulfate

cyanide

nitrite

chlorate

phosphate

nitrate

iridium (III)

calcium

titanium (IV)

platinum (II)

barium

strontium

potassium

zinc

manganese (IV)

gold (III)

sodium

2(Cr2O7)3

(OH)2

(CrO4)2

(CH3COO)2

(BrO3)2

3SO4

CN

(NO2)2

(ClO3)4

PO4

NO3

Ir

Ca

Ti

Pt

Ba

Sr

K

Zn

Mn

Au

Na

Ir2+,3+,4+,6+

Ca2+

Ti3+,4+

Pt2+,4+

Ba2+

Sr2+

K1+

Zn2+

Mn2,3,4,6,7+

Au1+,3+

Na1+

variable

fixed

variable

variable

fixed

fixed

fixed

fixed

variable

variable

fixed

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

SCl2

Rb2SO4

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

Two nonmetals Multiple-charge cation Everything else

Romannumeral

Polyatomic ions

Roman numeralfor name only

Polyatomic ions

Greek prefixes

Charge

Criss-CrossRule

Romannumeral

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

Write the total number of atoms that make up each compound.

Write the compound formed by the following ions:1) Al3+ S2-

2) Mg2+ PO43-

When a formula is given…write the proper name. When a name is given…write the proper formula.

3) BaO

4) lithium bromide

5) Ni2S3

6) triphosphorus heptoxide

7) N2O5

8) molybdenum (VI) nitride

9) trinitrotoluene (TNT)… CH3C6H2(NO2)3

10) phosphoric acid H3PO4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)

Write the total number of atoms that make up each compound.

Write the compound formed by the following ions:1) Al3+ S2-

2) Mg2+ PO43-

When a formula is given…write the proper name. When a name is given…write the proper formula.

3) BaO

4) lithium bromide

5) Ni2S3

6) triphosphorus heptoxide

7) N2O5

8) molybdenum (VI) nitride

9) trinitrotoluene (TNT)… CH3C6H2(NO2)3

10) phosphoric acid H3PO4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)

POP QUIZ

Write the total number of atoms that make up each compound.

Write the compound formed by the following ions:1) Al3+ S2-

2) Mg2+ PO43-

When a formula is given…write the proper name. When a name is given…write the proper formula.

3) BaO

4) lithium bromide

5) Ni2S3

6) triphosphorus heptoxide

7) N2O5

8) molybdenum (VI) nitride

9) trinitrotoluene (TNT)… CH3C6H2(NO2)3

10) phosphoric acid H3PO4 Extra credit: What is the formula for plumbic iodide? (Hint: lead is Pb2+ or Pb4+)

Answer Key

Al2S3

Mg3(PO4)2

barium oxide

nickel (III) sulfide

LiBr

dinitrogen pentoxide

MoN2

8

21

PbI4

P3O7

aluminum sulfide

magnesium phosphate

Polyatomic Ions - Quiz

oxalate

chromate

dichromate

permanganate

acetate

C2O42- ……………

CrO42- ……………

Cr2O72- …………..

MnO41- …………..

CH3COO1- …….

K2O

Exceptions!Two exceptions to the simple –ide ending are the diatomic oxide ions, O2

2- and O21-.

O22- is called peroxide

O21- is called superoxide.

Note the differences.

barium oxide __________barium peroxide __________

sodium oxide __________sodium peroxide __________

potassium oxide __________potassium superoxide __________

BaO

Na2O

Do Not Reduce to lowest terms!

KO2

Ba2+

Na1+

K1+

BaO2

Na2O2

Naming Chemical Compounds

Binary Compound?

Use the strategysummarized

earlier

Polyatomic ions present?

This is a compound for which naming procedures have not yet been considered.

Name the compound using procedures similar to those for naming binary ionic compounds.

Yes

YesNo

No

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 102

Nomenclature Review Flow Chart

Metal + Nonmetal?

Formula Name?

Ionic

Covalent

Two Nonmetals?

Multiple Single

Use Prefixes!!!

*Mono* HexaDi HeptaTri OctaTetra NonaPenta Deca

1. Write name of cation (metal)

2. Determine the charge on the metal by balancing the (-) charge from the anion

3. Write the charge of the metal in Roman Numerals and put in parentheses

4. Write name of anion(Individual anions need –ide ending!)

Steps 1 & 4 ONLY

d,f-blockPb,Sn

Columns 1, 2, 13Ag+, Zn2+

(Except: NH4+)

Name Formula?

No Prefixes? Prefixes?

1. Determine the ions present and the charge on each (Roman Numeral = cation charge, otherwise use PT)

2. Balance formula (criss-cross)

3. Reduce subscripts (if needed)

1. FORGET CHARGES!!!

2. Use prefixes to determine subscripts

3. Do NOT reduce subscripts!

Ionic Covalent

Binary Hydrogen Compoundsof Nonmetals When Dissolved in Water

(These compounds are commonly called acids.)

The prefix hydro- is used to represent hydrogen, followed by the nameof the nonmetal with its ending replaced by the suffix –ic and the wordacid added.

Examples:

*HCl

HBr

*The name of this compound would be hydrogen chloride if it was NOT dissolved in water.

Hydrochloric acid

Hydrobromic 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)

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

An acid with aname ending in

A salt with aname ending in

-ic

-ous

-ate

-iteforms

forms

Hill, Petrucci, General Chemistry An Integrated Approach1999, page 60

Oxyacids Oxysalts If you replace hydrogen with a metal, you have formed an oxysalt.A salt is a compound consisting of a metal and a non-metal. If thesalt consists of a metal, a nonmetal, and oxygen it is called anoxysalt. NaClO4, sodium perchlorate, is an oxysalt.

HClO4

perchloric acid

HClO3

chloric acid

HClO2

chlorous acid

HClOhypochlorous acid

NaClO4

sodium perchlorate

NaClO3

sodium chlorate

NaClO2

sodium chlorite

NaClOsodium hypochlorite

OXYACID OXYSALT

ACID SALT

per stem ic changes to per stem ate

stem ic changes to stem ate

stem ous changes to stem ite

hyper stem ous changes to hypo stem ite

HClO3 + Na1+ NaClO3 + H1+

acid cation salt

Suffixes have meaning“-ide” binary compound

sodium chloride (NaCl)

“-ite” or “-ate” polyatomic compoundsulfite (SO3

2-)

sulfate (SO42-) “-ate” means one more

oxygen than “-ite”

“-ol” alcoholmethyl alcohol (methanol)

“-ose” sugarsucrose

“-ase” enzymesucrase

Oxidation States in Formulas and Names

dinitrogen monoxide N2O nitrogen (I) oxide

dinitrogen trioxide N2O3 nitrogen (III) oxide

dinitrogen pentoxide N2O5 nitrogen (V) oxide

sulfur dioxide SO2 sulfur (IV) oxide

sulfur trioxide SO3 sulfur (VI) oxide

Traditional System Stock System

+1 -2

+3 -2

+5 -2

+4 -2

+6 -2

(Two non-metals)

stock system is NOT preferred for two non-metals

% Mg = x 10024 g95 g

Percentage Composition

Mg

magnesium

24.305

12

Cl

chlorine

35.453

17

Mg2+ Cl1-

MgCl2

1 Mg @ 24.305 amu = 24.305 amu2 Cl @ 35.453 amu = 70.906 amu 95.211 amu

25.52% Mg

74.48% Cl

(by mass...not atoms)

It is not 33% Mg and 66% Cl

% = x 100part

whole

Empirical and Molecular Formulas

A pure compound always consists of the same elements combined in the same proportions by weight.

Therefore, we can express molecular composition as PERCENT BY WEIGHTPERCENT BY WEIGHT.

Ethanol, C2H6O 52.13% C 13.15% H 34.72% O

Empirical FormulaQuantitative analysis shows that a compound contains 32.38% sodium, 22.65% sulfur, and 44.99% oxygen.

Find the empirical formula of this compound.

= 1.408 mol Na

= 0.708 mol S

= 2.812 mol O

/ 0.708 mol

/ 0.708 mol

/ 0.708 mol

= 2 Na

= 1 S

= 4 O

Na2SO4

32.38% Na

22.65% S

44.99% O

32.38 g Na

22.65 g S

44.99 g O

Na g 23

Na mol 1

S g 32

S mol 1

O g 16

O mol 1

sodium sulfate

Step 1) % g Step 2) g molStep 3) mol mol

Na2SO4

Empirical FormulaA sample weighing 250.0 g is analyzed and found to contain the following:

27.38% sodium 1.19% hydrogen14.29% carbon57.14% oxygen

Determine the empirical formula of this compound.

Step 1) convert % gram

Step 2) gram moles

Step 3) mol / mol

Assume sample is 100 g.

27.38 g Na 1.19 g H14.29 g C57.14 g O

Na mol 1.1904 Na g 23Na mol 1Na g 27.38 Na molx

H mol 1.19 H g 1H mol 1H g 1.19 H molx

C mol 1.1908 C g 12C mol 1C g 14.29 C molx

O mol 3.5712 O g 16O mol 1O g 57.14 O molx

/ 1.19 mol = 1 Na

/ 1.19 mol = 1 H

/ 1.19 mol = 1 C

/ 1.19 mol = 3 O

NaHCO3

Empirical & Molecular FormulaA 175 g hydrocarbon sample is analyzed and found to contain ~83% carbon.The molar mass of the sample is determined to be 58 g/mol. Determine the empirical and molecular formula for this sample.

Determine the empirical formula of this compound.

Step 1) convert % gram

Step 2) gram moles

Step 3) mol / mol

Assume sample is 100 g.

C mol 6.917 C g 12C mol 1C g 83 C molx

H mol 17 H g 1H mol 1H g 17 H molx

/ 6.917 mol = 1 C

/ 6.917 mol = 2.5 H (2.4577 H)

CH2.5

Then, 83 g carbon and 17 g hydrogen.

C2H5

MMmolecular = 58 g/mol

58/29 = 2

Therefore 2(C2H5) = C4H10

MMempirical = 29 g/mol

2 C @ 12 g = 24 g5 H @ 1 g = 5 g 29 g

butane

(~17% hydrogen)(contains only hydrogen + carbon)

1 mol S

1 mol Zn

Common Mistakes when Calculating Empirical Formula

Given: Compound consists of 36.3 g Zn and 17.8 g S.

Find: empirical formula

36.3 g Zn

65.4 g Zn

= 2 Zn

17.8 g S

17.8

17.8= 1 S

Zn2S

36.3 g Zn

17.8 g S

32.1 g S

= 0.555 mol Zn

= 0.555 mol S

Chemical formulaindicates MOLE ratio,

not GRAM ratio

0.555 mol

0.555 mol

1

1

Zn

SZnS

zinc sulfide

Empirical Formula of a Hydrocarbon

CxHy

g H2O

g CO2

mol H2O

mol CO2

mol Cmol H

burnin O2

1 mol CO2

44.01 gx

1 mol H2O 18.02 g

x 2 mol H 1 mol H2O

x

2 mol C 1 mol CO2

x

Empiricalformula

Kotz & Treichel, Chemistry & Chemical Reactivity, 3rd Edition , 1996, page 224

Find the molar mass and percentage composition of zinc acetate

acetate = CH3COO1-

Zn2+ CH3COO1-

Zn(CH3COO)2

1 Zn @ 65.4 g/mol = 65.4 g

4 C @ 12 g/mol = 48 g

6 H @ 1 g/mol = 6 g

4 O @ 16 g/mol = 64 g

Zn(CH3COO)2183.4 g

/ 183.4 g x 100% = 35.6 % Zn

/ 183.4 g x 100% = 26.2 % C

/ 183.4 g x 100% = 3.3 % H

/ 183.4 g x 100% = 34.9 % O

1 mol Cl

35.5 g Cl

1 mol Y

88.9 g Y

A compound is found to be 45.5% Y and 54.5% Cl.

Its molar mass (molecular mass) is 590 g.

a) Find its empirical formula

b) Find its molecular formula

Assume a 100 g sample sizeAssume a 100 g sample size

45.5 g Y

54.5 g Cl

= 0.5118 mol Y

= 1.535 mol Cl

/ 0.5118 mol

/ 0.5118 mol

= 1 Y

= 3 Cl

YCl3

1 Y @ 88.9 g/mol = 88.9g

3 Cl @ 35.5 g/mol = 106.5 g

YCl3 195.4 g590 / 195.4 = 3

3 (YCl3) Y3Cl9

Molar Mass vs. Atomic Mass

6.02x1023

H2 = _______H2 = _____

H2O = ________H2O = _____

MgSO4 = ________MgSO4 = _____

(NH4)3PO4 = _____ (NH4)3PO4 = ________

Percentage Composition

Empirical vs. Molecular Formula

% g g mol mol mol

Empirical Formula

2 amu

18 amu

120 amu

149 amu

2 g

18 g

120 g

149 g

% = x 100 % partwhole

(lowest ratio)

(by mass)

Subscripts, Superscripts and Coefficients

Al3(SO4 )2coefficient

subscripts

superscripts

ALUMINUM SULFATE

SO43- Al2+

5

Subscripts, Superscripts and Coefficients

MgSO4 MAGNESIUM SULFATE

SO42- Mg2+

3

Subscripts, Superscripts and Coefficients

subscript

MAGNESIUM NITRATE

NO31- Mg2+

42

MgNO3 Mg(NO3)2

Interpretation of a Chemical Formula

Sulfuric Acid

H2SO4

Two atomsof hydrogen

One atom of sulfur

Four atoms of oxygen

S

O

O

O

O H

H

Chemical Formulas

C8H18 Subscript indicates that there are 8 carbon atoms in a molecule of octane.

Subscript indicates thatthere are 18 hydrogen atoms

in a molecule of octane.

Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 203

Stock System of Nomenclature

CuCl2 Name of Roman cation numeral

indicating charge

Name of anion+

copper (II) chloride

Chemical Formulas

Al2(SO4)3Subscript 2

refers to2 aluminum

atoms.

Subscript 4refers to4 oxygenatoms in

sulfate ion.

Subscript 3 refers toeverything inside parentheses.Here there are 3 sulfate ions, with a total of 3 sulfur atoms

and 12 oxygen atoms.

Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 204

Naming Binary Ionic Compounds

Al2O3

Name of cation Name of anion

aluminum oxide

Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 207

The OLD System of Nomenclature

CuCl2Name of Name of anion cation

Cupric chloride

-ic higheroxidation #

-ous loweroxidation #

+

Davis, Metcalfe, Williams, Castka, Modern Chemistry, 1999, page 208

Centrum Multi-VitaminIngredients: ascorbic acid, beta carotene, biotin, calcium pantothenate, calciumphosphate, carnauba wax, chromium chloride, crospovidone, cupric sulfate,cyanocobalamin, dl-alpha tocopheryl acetate, FD & C blue no. 2 aluminum lake,hydroxypropyl cellulose, ferrous fumarate, hydroxypropyl methylcellulose, lactose, Magnesium oxide, magnesium stearate, manganese sulfate, microcrystalline cellu-lose,niacinamide, nickel sulfate, phytonandione, polyethylene glycol, potassium chloride, potassium citrate, potassium iodide, povidone, pyridoxine hydrochloride, riboflavin, silica gel, sodium borate, sodium metavanadate, sodium molybdate,sodium selenate, stannous chloride, stearic acid, thiamin mononitrate, titaniumdioxide, triacetin, vitamin A acetate, vitamin D3, zinc oxide. PC7563-46-00

Warning: Accidental overdose of iron-containing products is a leading cause of fatal poisoning in children under 6. Keep this product out of reach of children.In case of accidental overdose, call a doctor or poison control immediately.

Chromium (III) Chloride

Step 1: Chromium (III) Chloride

Step 2: Cr3+ Cl1-

Step 3: Cr Cl1 3

Step 4: CrCl3

RECALL: Chromium forms oxides in which metal exhibits oxidationstates of +3 and +2. STOCK system indicates oxidation state of compound. Assume Cr3+ (chromium (III) chloride).

Return to Centrum Bottle

Cupric Sulfate

Step 1: Cupric Sulfate

Step 2: Cu2+ SO42-

Step 3: Cu (SO4)2 2

Step 4: Cu2(SO4)2

Step 5: CuSO4

RECALL: “ic” higher oxidation & “ous” lower oxidation Cu2+ (higher) Cu1+ (lower)

Return to Centrum Bottle

Manganese (III) Sulfate

Step 1: Manganese (III) Sulfate

Step 2: Mn3+ SO42-

Step 3: Mn (SO4)2 3

Step 4: Mn2(SO4)3

RECALL: Manganese forms oxides in which metal exhibits oxidationstates of +2, +3, +4, and +7. STOCK system indicates oxidation state of compound. Assume Mn3+ (manganese (III) sulfate).

Return to Centrum Bottle

Stannous Chloride

Step 1: Stannous (tin) Chloride

Step 2: Sn2+ Cl1-

Step 3: Sn Cl1 2

Step 4: SnCl2

RECALL: “ic” higher oxidation & “ous” lower oxidation Sn4+ (higher) Sn2+ (lower)

Return to Centrum Bottle

Stannic Chloride

Step 1: Stannic (tin) Chloride

Step 2: Sn4+ Cl1-

Step 3: Sn Cl1 4

Step 4: SnCl4

RECALL: “ic” higher oxidation & “ous” lower oxidation Sn4+ (higher) Sn2+ (lower)

Return to Centrum Bottle

Chromium Chloride

Step 1: Chromium (II) Chloride

Step 2: Cr2+ Cl1-

Step 3: Cr Cl1 2

Step 4: Cr1Cl2

Step 5: CrCl2

RECALL: Chromium has multiple oxidation states. Name with STOCK system.

Assume Chromiun (II).

Return to Centrum Bottle

Calcium Phosphate

Step 1: Calcium Phosphate

Step 2: Ca2+ PO43-

Step 3: Ca (PO4)3 2

Step 4: Ca3(PO4)2

Return to Centrum Bottle

Zinc Oxide

Step 1: Zinc Oxide

Step 2: Zn2+ O2-

Step 3: Zn O2 2

Step 4: Zn2O2

Step 5: ZnO

Return to Centrum Bottle

Common Polyatomic Ions

Ion Name Ion Name

NH4+ ammonium

nitrite

nitrate

phosphate

hydrogen phosphate

dihydrogen phosphate

carbonate

hydrogen carbonate(bicarbonate is a widelyused common name)

sulfite

sulfate

hydrogen sulfate(bisulfate is a widelyused common name)

hydroxide

cyanide

hypochlorite

chlorite

chlorate

perchlorate

acetate

permanganate

dichromate

chromate

peroxide

NO2-

NO3-

SO32-

HSO4-

OH-

CN-

PO43-

CO32-

SO42-

MnO4-

O22-

Cr2O72-

HPO42-

H2PO4-

ClO2-

ClO3-

ClO-

HCO3-

ClO4-

C2H3O2-

CrO42-

Names of Common Polyatomic Ions

1

2

3

4

5

6

1

2

3

4

5

6

Electronegativities

7

Be

1.5

Al

1.5

Si

1.8

Ti

1.5

V

1.6

Cr

1.6

Mn

1.5

Fe

1.8

Co

1.8

Ni

1.8

Cu

1.9

Zn

1.7

Ga

1.6

Ge

1.8

Nb

1.6

Mo

1.8

Tc

1.9

Ag

1.9

Cd

1.7

In

1.7

Sn

1.8

Sb

1.9

Ta

1.5

W

1.7

Re

1.9

Hg

1.9

Tl

1.8

Pb

1.8

Bi

1.9

1.5 - 1.9

N

3.0

O

3.5

F

4.0

Cl

3.0

3.0 - 4.0

C

2.5

S

2.5

Br

2.8

I

2.5

2.5 - 2.9

Na

0.9

K

0.8

Rb

0.8

Cs

0.7

Ba

0.9

Fr

0.7

Ra

0.9

Below 1.0

H

2.1

B

2.0

P

2.1

As

2.0

Se

2.4

Ru

2.2

Rh

2.2

Pd

2.2

Te

2.1

Os

2.2

Ir

2.2

Pt

2.2

Au

2.4

Po

2.0

At

2.2

2.0 - 2.4

Per

iod

Actinides: 1.3 - 1.5

Li

1.0

Ca

1.0

Sc

1.3

Sr

1.0

Y

1.2

Zr

1.4

Hf

1.3

Mg

1.2

La

1.1

Ac

1.1

1.0 - 1.4

Lanthanides: 1.1 - 1.3

1A

2A

3B 4B 5B 6B 7B 1B 2B

3A 4A 5A 6A 7A

8A

Hill, Petrucci, General Chemistry An Integrated Approach 2nd Edition, page 373

8B

Metal (fixed) + Non-metal

binary -ide NaCl sodium chloride

Metal (variable) + Non-metal

STOCK system (Roman Numeral)

CrCl2 chromium (II) chloride

OLD system [-ic (higher) & -ous (lower)]

CuCl2 cupric chloride

Sn stannumPb plumbumCu cuprumAu aurumFe ferrum

Polyatomic Ions [-ate (one more O) & -ite (one less O)]

LiNO3 lithium nitrate

LiNO2 lithium nitrite

Li3N lithium nitride

TWO Elements

Three or more Elements

ReviewReview

Cu1+ or Cu2+

Group 1, Group 2, Ag, Zn, Al

Transition Elements

Cr2+ Cl1-

Ternary Compounds

(binary compound)

Polyatomic Ions [-ate (one more O) & -ite (one less O)]

per____ate NORMAL _____ite hypo_____ite

chloratenitratecarbonatesulfatephosphate

ammonium, cyanide, hydroxide

Nonmetal & Nonmetal (Greek prefixes)……DO NOT REDUCE!

Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca

1 2 3 4 5 6 7 8 9 10

ClO31-

NO31-

CO32-

SO42-

PO43-

NH41+ CN1- OH1-

chloritenitritecarbonitesulfitephosphite

ClO21-

NO21-

CO22-

SO32-

PO33-

perchloratepernitratepercarbonatepersulfateperphosphate

ClO41-

NO41-

CO42-

SO52-

PO53-

2 less oxygen1 less oxygen1 more oxygen

ClO1-

NO1-

CO2-

SO22-

PO23-

hypochloritehyponitritehypocarbonitehyposulfitehypophosphite

Memorize

How many atoms are in a formula unit of ammonium hypophosphite?NH4

1+ PO23-

(NH4)3PO2

318

_____ate

Molecular Models Activity

ammonia

hydrogen monochloride

trichloromethane

urea

propane

butane

nitrogen triiodide (video)

carbon tetrachloride

methane

water

ethane

ethyne

dihydrogen monosulfide

carbon dioxide

supplies

Bonding and Shape of Molecules

Number of Bonds

Number of Unshared Pairs Shape Examples

2

3

4

3

2

0

0

0

1

2

Linear

Trigonal planar

Tetrahedral

Pyramidal

Bent

BeCl2

BF3

CH4, SiCl4

NH3, PCl3

H2O, H2S, SCl2

-Be-

B

C

N

:

O

:

:

CovalentStructure

Lewis Structures

1) Count up total number of valence electrons

2) Connect all atoms with single bonds

- “multiple” atoms usually on outside

- “single” atoms usually in center;

C always in center,

H always on outside.

3) Complete octets on exterior atoms (not H, though)

4) Check

- valence electrons match with Step 1

- all atoms (except H) have an octet; if not, try multiple bonds

- any extra electrons? Put on central atom

- no unpaired electrons (free radicals)

Gilbert Lewis

Carbon tetrachloride

C ClClCl

Cl

CCl4

C109.5o

Cl

ClClCl

Carbon tetrachloride – “carbon tet” had been used as dry cleaning solventbecause of its extreme non-polarity.

Tetrahedral geometry

Methane

CHH

HH

C109.5o

H

HHH

Methane –The first member of the paraffin (alkane) hydrocarbons series. a.k.a. (marsh gas, CH4).

Tetrahedral geometry

Water

....

H HOBent

geometry

SO2

(-)

(+)

Polar molecule

Ethane

CH

CHH

HHH

space-filling molecule

ball-and-stickLewis dot notation

C2H6

molecular formula

C = 1s22s22p2

Ethene

CH

CHH

HHH

space-filling molecule

ball-and-stickLewis dot notation

C2H4

molecular formula

Ethyne

CCH H CCH H

No octet

Stable octet

6 electrons = triple bond

CCH H

C2H2

CCH H

each C “feels” 6 electrons

each C “feels” 7 carbons

Ethyne – a.k.a. “acetylene”

Dihydrogen monosulfide

....

H HS

Bent

SO2

Carbon dioxide

O OC

Lineargeometry

C OOCO2

C OO

Ammonia

NH HH

N107o HH

H

..

NH3

..

HH

H

N

TrigonalPyramidalgeometry

NH HH

H

Amino Acids – Functional Groups

Amine Carboxylic AcidBase Pair

NH21- R- COOH

NH3NH21- NH4

1+

amine ammonia ammonium ion

NH

HH

:

NH

HH

H : 1+

NH

H

:

1-

:

H+ lose H+ H+

+

Hydrogen monochloride

H ClHCl

H Cl

(-)(+)

H Cl

Polar molecule

HCl(g) + H2O(l) HCl(aq)

hydrogenchloride

water hydrochloric acid

Trichloromethane

C ClClCl

H

CHCl3

C109.5o

H

ClClCl

C ClClCl

H

(-)

(+)

Polar molecule

Tetrahedral geometry

Urea

CON HH

NH H

CON HH

NH H

CO(NH2)2

NOT “di-urea”

Urea – The first organic compound to be synthesized (Wohler, 1828).

Propane

CH

CHH

CH

HHHH

C C C

HH

H

HH H H

H

C3H8

Butane

CH

CHH

CH

C HH

HHHHH - C - C - C - C - H

H H H H

H H H H

C4H10 C C C

HH

H

HH H H

HC

H

H

Nitrogen triiodide

NI II N

107o III

..

NI3

TrigonalPyramidalgeometry

Video clip:

(slow motion)

detonation of NI3

Supplies

15 black (carbon) 8 green (chlorine and iodine) 1 yellow (sulfur) 4 blue (oxygen) 4 red (nitrogen) 42 hydrogen (hydrogen) 67 bonds (bonds)

C Cl I S O N H

C ClClCl

ClCH

H HH

C OO

SH HC C HH

C ClClCl

H

H Cl

CCl4 CH4

CO2

C2H2

HClCHCl3

SH2

CH

CHH

CH

C HH

HHHHCH

CHH

CH

HHHH

NH HH

NI II

Decomposition of Nitrogen Triiodide

Decomposition of Nitrogen Triiodide

2 NI3(s) N2(g) + 3 I2(g)

NI3 I2

N2

C109.5o

H

HHH

N107o HH

H

..

O104.5o H

H

..

..

CH4, methane NH3, ammonia H2O, water

..

O

O

O

lone pairelectrons

OOO

O3, ozone

......

The VSEPR Model

O OC

Linear

The Shapes of Some Simple ABn Molecules

O OS

BentO O

S

O

Trigonalplanar

FF

F

N

Trigonalpyramidal

T-shaped Squareplanar

F FCl

F

F F

Xe

F FF

F

FP

F

F

Trigonalbipyramidal

Octahedral

FF

F

S

F

F

F

AB6

SO2

Brown, LeMay, Bursten, Chemistry The Central Science, 2000, page 305

Resources - Nomenclature

ObjectivesObjectives

Worksheet - binary cmpds: single charge cationWorksheet - binary cmpds: single charge cation

Worksheet - ions in chemical formulasWorksheet - ions in chemical formulas

Worksheet - ionic cmpds: polyatomic ions w multiple-charge cationWorksheet - ionic cmpds: polyatomic ions w multiple-charge cation

Worksheet - ionic formulas (binary, polyatomic, transition)Worksheet - ionic formulas (binary, polyatomic, transition)

Worksheet - traditional system of nomenclatureWorksheet - traditional system of nomenclature

Worksheet - covalent binary cmpds: non-metal - non-metal Worksheet - covalent binary cmpds: non-metal - non-metal

Worksheet - ionic cmpds: polyatomic ionsWorksheet - ionic cmpds: polyatomic ions

Outline (general)(general)

Worksheet - empirical and molecularWorksheet - empirical and molecular

Worksheet - vocab (bonding)Worksheet - vocab (bonding)

Activity - bonding piecesActivity - bonding pieces

Activity - molecular modelsActivity - molecular models

Activity - mole patternActivity - mole pattern

Worksheet - binary compoundsWorksheet - binary compounds

Worksheet - ions in chemical compoundsWorksheet - ions in chemical compounds

Textbook - questionsTextbook - questions

Worksheet - ionic binary cmpds: multiple charge cationWorksheet - ionic binary cmpds: multiple charge cation

Worksheet - oxidation numbers and ionic cmpdsWorksheet - oxidation numbers and ionic cmpds

Worksheet - names and formulas of cmpdsWorksheet - names and formulas of cmpds

Worksheet - errors in chemical formulas and nomenclatureWorksheet - errors in chemical formulas and nomenclature

General Chemistry PP