Compounds

Binary CompoundsBinary compounds that contain a metal of fixed oxidation number(group 1, group 2, Al, Zn, Ag, etc.), and a non-metal.

To name these compounds, give the name of metal followed by thename of the non-metal, with the ending replaced by the suffix –ide.

Examples:

NaCl sodium chloride (Na1+ Cl1-)

CaS calcium sulfide (Ca2+ S2-)

AlI3 aluminum iodide (Al3+ I1-)

Cations and AnionsCommon Simple Cations and Anions

Cation Name Anion Name*

H 1+ hydrogen H 1- hydride Li 1+ lithium F 1- fluoride Na 1+ sodium Cl 1- chloride K 1+ potassium Br 1- bromide Cs 1+ cesium I 1- iodide Be 2+ beryllium O 2- oxide Mg 2+ magnesium S 2- sulfide Al 3+ aluminum Ag 1+ silver

*The root is given in color.

Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 86

Example: Aluminum Chloride

Step 1:

Step 2:

Step 3: 1 3

Step 4: AlCl3

Criss-Cross Rule

Al Cl

Al Cl

3+ 1-

write out name with space

write symbols & charge of elements

criss-cross charges as subsrcipts

combine as formula unit(“1” is never shown)

Example: Aluminum Chloride

Step 1: Aluminum Chloride

Step 2: Al3+ Cl1-

Step 3: Al Cl1 3

Step 4: AlCl 3

Criss-Cross Rule

Example: Aluminum Oxide

Step 1: Aluminum Oxide

Step 2: Al3+ O2-

Step 3: Al O2 3

Step 4: Al2O3

Criss-Cross Rule

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

Naming Binary Compounds

Formula Name

1 BaO ____________________

2 ________________ sodium bromide

3 MgI2 ____________________

4 KCl ____________________

5 ________________ strontium fluoride

6 ________________ cesium fluoride

barium oxide

NaBr

magnesium iodide

potassium chloride

SrF2

CsF

Ternary Compounds

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.

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’

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

Ternary Compounds1. ________________ 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

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- …………..

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

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) triphosphorous heptaoxide

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) triphosphorous heptaoxide

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) triphosphorous heptaoxide

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 KeyAl2S3

Mg3(PO4)2

barium oxide

nickel (III) sulfide

LiBr

dinitrogen pentaoxide

MoN2

8

21

PbI4

P3O7

Polyatomic Ions - Quiz

oxalate

chromate

dichromate

permanganate

acetate

C2O42- ……………

CrO42- ……………

Cr2O72- …………..

MnO41- …………..

CH3COO1- …….

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 __________

BaOBaO2

Na2ONa2O2 Do Not Reduce to lowest terms!

K2OKO2

Ba2+

Na1+

K1+

Ionic Compounds:Polyatomic Ions

KeysKeys

Ionic Compounds:  Polyatomic Ions

Chart of the Ions and Polyatomic Ions

Polyatomic Ions Grid to Memorize Ionic Compounds:  Polyatomic Ions

Ionic Binary Compounds:Multiple-Charge Cations

KeysKeys

          Ionic Binary Compounds:  Multiple-Charge Cations

          Ionic Binary Compounds:  Multiple-Charge Cations

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

Oxidation Numbers and Ionic Compounds

KeysKeys

Oxidation Numbers and Ionic Compounds

Oxidation Numbers and Ionic Compounds

Names and Formulas of Compounds

KeysKeys

Names and Formulas of Compounds

Names and Formulas of Compounds

Subscripts, Superscripts and Coefficients

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

Interpretation of a Chemical Formula

Sulfuric Acid

H2SO4

Two atomsof hydrogen

One atom of sulfur

Four atoms of oxygen

HH

O

S

OO

O

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 Stock System of Nomenclature

CuCl2Name of Name of anion cation

Copper (II) chloride

Romannumeral

indicatingcharge

+

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

Bonding Activity

Common Polyatomic Ions

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

Chemical Bonding Activity

KeysKeys

          Chemical Bonding Activity (pink/blue)Chemical Bonding Activity Pieces

          Chemical Bonding Activity (pink/blue)Chemical Bonding Activity Pieces

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

Molecular Models Activity

KeysKeys

Molecular Model's Activity

Molecular Model's Activity

Molecular Models Activityammonia

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

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

C2H4

molecular formula

C = 1s22s22p2

Ethane

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 HC2H2

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

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

FTrigonal

bipyramidalOctahedral

FF

F

S

F

F

F

AB6

SO2

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