Unit 5: Bonding andInorganic Nomenclature

Chemistry

NaClO3

Fe(ClO3)2

lithium nitrate

lithium nitride

lithium nitrite

lead (II) sulfide

barium sulfide

sulfur dioxide

Fe(ClO3)3

NO2

N2O4

N2O5

Outline

PowerPoint Presentation by Mr. John Bergmann

Chemical Bonding Ionic Bonds: atoms give up or gain e– and

are attracted to each other by coulombic attraction

Na Na1+ Cl Cl1–loses e– gains e–

Na1+ + Cl1– NaCl

K1+ + NO31– KNO3

ionic compounds = salts

where NO31– is a polyatomic ion:

a charged group of atoms that stay together

Properties of Salts

1. very hard –

2. high melting points –

3. brittle –

each ion is bondedto several oppositely-charged ions

many bonds must be broken

with sufficient force,like atoms arebrought next toeach other and repel

calcite

Covalent Bonds …atoms share e– to get a full valence shell

Lewis structure:

1. Two shared e– make a single covalent bond,four make a double bond, etc.

2. unshared pairs: pairs of unbonded valence e–

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

a model of a covalent molecule that

shows all of the valence e–

1s2 2s2 2p2 (4 v.e–) 1s2 2s2 2p5 (7 v.e–)

both need 8 v.e– for a full outer shell (octet rule)

CF

x

x

H

x x

xx

x xF x

carbon tetrafluoride (CF4)

o

Co

o o

x

xxx

x xF x

o

Co

o ox

xxx

x xF x

x

xxx

xF x

x

xxx

x xF x

x

x

xxx

x xF x

x

xxx

x xF x

x

xxx

x xF x

methane (CH4)

o

Co

o o

H x

o

Co

o oH x

xH

x H

H x

H x

H x

ooo

oN o

nitrogen triiodide (NI3)

carbon dioxide (CO2)

x x

xx

x x I x

x

xxx

x x I x

x

xxx

x x I x

xxx

x x I x

x

x

xxx

x x I x

x

xxx

x x I xoo

o

oN 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

x

xxx

xO x

butter

(consist of twononmetal elements)

covalent compounds = molecular compounds

-- have lower melting points than do ionic compounds

In insulators (like wood),the v.e– are attachedto particular atoms.

Metallic Bonds

In metals, valence shells of atoms overlap, so v.e– are free to travel between atoms through material.

Not so in metals.

All due to free-moving

v.e–.

Properties of Metals

ductile conduct heat and electricity

malleable

These are much weaker than ionic, covalent, or metallic bonds, but very important in determining states of matter, boiling and melting points, and

molecular shape (among other things).

Other Types of Bonds

dipole-dipole forces hydrogen bonds London dispersion forces ion-dipole forces

DNA

boiling H2O

Writing Formulas of Ionic Compounds

chemical formula:

To write an ionic compound’s formula, we need:1. the two types of ions 2. the charge on each ion

Na1+ and F1–

Ba2+ and O2– Na1+ and O2– Ba2+ and F1–

shows types of atomsand how many of each

NaF

BaONa2OBaF2

(i.e., “pink” and “blue”)

has neutral charge;

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

** Warning:

Al3+ and O2– Ba2+ and S2– In3+ and Br1–

Reduce to lowest terms.

Al O Ba S In Br 2 3 2 2 31

Al2O3 BaS InBr3

criss-cross rule:

Writing Formulas w/Polyatomic Ions

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

Ba2+ and SO42–

Mg2+ and NO21–

NH41+ and ClO3

1–

Sn4+ and SO42–

Fe3+ and Cr2O72–

NH41+ and N3–

BaSO4

Mg(NO2)2

NH4ClO3

Sn(SO4)2

Fe2(Cr2O7)3

(NH4)3N

Inorganic Nomenclature

potassiumnitrateKNO3

sodiumhydroxide

NaOH

dinitrogen monoxideN2O

copper (II)sulfateCu2SO4

Ionic Compounds (cation/anion combos)Single-Charge Cations with Elemental Anions

The single-charge cations are: groups 1, 2, 13, and Ag1+, Cd2+, and Zn2+

i.e., “pulled off the Table” anions

A. To name, given the formula:

2. Use name of anion (it has the ending “ide”).

1. Use name of cation.

NaF

BaO

Na2O

BaF2

sodium fluoride

barium oxide

sodium oxide

barium fluoride

Na

Ba

1. Write symbols for the two types of ions.2. Balance charges to write formula.

silver sulfide

zinc phosphide

calcium iodide

B. To write formula, given the name:

Ag1+ S2– Ag2S

Zn2+ P3– Zn3P2

I1– Ca2+ CaI2

CaAg

Zn

Multiple-Charge Cations with Elemental Anions

The multiple-charge cations are:

i.e., “pulled off the Table” anions

Pb, Sn, and the transition elements (but – of course! – not Ag, Cd, or Zn)

iron oxide

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.4. Write name of anion.

FeO

Fe2O3

CuBr

CuBr2

iron oxide

CuFe

Stock Systemof nomenclature

Fe? O2– iron (II) oxide

Fe? O2– iron (III) oxide

copper bromide

copper bromide

Cu? Br1– copper (I) bromide

Cu2+ Br1– copper (II) bromide

Fe?

Br1–

O2– O2–

Fe2+

Fe3+ Fe3+

Cu1+

Cu?

B. To find the formula, given the name:1. Write symbols for the two types of ions.

2. Balance charges to write formula.

cobalt (III) chloride

tin (IV) oxide

tin (II) oxide

Co

Sn

Co3+ Cl1– CoCl3

Sn4+

O2–

O2–

Sn2+

SnO2

SnO

Compounds Containing Polyatomic Ions Insert name of ionwhere it should goin the compound’sname.

Write formulas:

iron (III) nitrite

ammonium phosphide

ammonium chlorate zinc phosphate lead (II) permanganate

iron (III) nitrite

ammonium phosphide

ammonium chlorate zinc phosphate lead (II) permanganate

Fe3+ NO31– Fe(NO3)3

NH41+

NH41+

P3– (NH4)3P

ClO31– NH4ClO3

Zn2+ PO43– Zn3(PO4)2

Pb2+ MnO41– Pb(MnO4)2

Write names:

(NH4)2S2O3

AgBrO3

(NH4)3N

U(CrO4)3

Cr2(SO3)3

(NH4)2S2O3

AgBrO3

(NH4)3N

U(CrO4)3

Cr2(SO3)3

ammonium thiosulfate

silver bromate

ammonium nitride

U? CrO42–

CrO42–

CrO42–

uranium (VI) chromate

Cr? Cr?

Cr3+ Cr3+ SO3

2– SO32–

SO32– chromium (III) sulfite

U6+

mono

Covalent Compounds -- contain two types of

** Key:

Use Greek prefixes to indicate howmany atoms of each element, but

don’t use “mono” on first element.

nonmetals nonmetals

FORGET CHARGES!

What to do:

1 –2 –3 –4 –5 –

6 –7 –8 –9 –

10 –

ditritetrapenta

hexaheptaoctanonadec

EXAMPLES:

carbon dioxide CO dinitrogen trioxide N2O5

carbon tetrachloride NI3

CO2 carbon monoxide N2O3

dinitrogen pentoxide CCl4

nitrogen triiodide

Dihydrogen Monoxide:A Tale of Danger and

Irresponsibility

-- major component of acid rain

-- found in all cancer cells-- inhalation can be deadly-- excessive ingestion results in acute physical symptoms:

e.g., frequent urination, bloated sensation, profuse sweating

-- often an industrial byproduct of chemical reactions; dumped wholesale into rivers and lakes

4. S F6

5. Fe (NO3)3

1. Ni2 S3

2. N F3

3. Na BrO3

6. Sr SO4

Writing Chemical NamesFormula RN/GP/neither

Use poly.ion sheet? Name

GPRN

RNGPneither

neither

noyes

nonoyes

yes

sulfur hexafluorideiron (III) nitrate

nickel (III) sulfidenitrogen trifluoridesodium bromate

strontium sulfate

10. oxygen difluoride

4. zinc arsenate5. silver nitride

1. copper (II) phosphide2. lithium phosphate3. phosphorus triiodide

7. dinitrogen pentasulfide8. tin (IV) nitride

6. sulfur dibromide

Writing Chemical Formulas

9. rubidium nitrite

11. iron (III) sulfite12. ammonium oxide

Name Charges matter?Use poly.

ion sheet? Formula

yesyes

yesyesno

noyes

no

yes

yesyes

no

yesno

noyesno

nono

no

yes

yesyes

no

Zn3(AsO4)2

Ag3N

Cu3P2

Li3PO4

PI3

N2S5

Sn3N4

SBr2

RbNO2

Fe2(SO3)3

(NH4)2O

OF2

Traditional 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 ending for lower charge. 3. Then say name of anion, as usual.

Cu

Au Pb

Sn

Fe

(i.e., NOT the Stock System)

Write formulas: cuprous sulfide

auric nitrite

ferrous fluoride

Write names: Pb3P4

Pb3P2

Sn(OH)4

Cu1+ S2– Cu2S

Au3+ NO21– Au(NO2)3

Fe2+ F1– FeF2

cuprous sulfide

auric nitrite

ferrous fluoride

Pb3P4

Pb3P2

Sn(OH)4

Pb? P3– Pb? Pb?

Pb? Pb? Pb?

P3– P3– P3–

P3– P3– Pb2+

Pb4+

Pb2+

Pb4+ Pb4+

plumbic phosphidePb2+

plumbous phosphideOH1– Sn4+ Sn? OH1–

OH1– OH1–

stannic hydroxide

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+

10. oxygen difluoride

4. zinc arsenate5. silver nitride

1. copper (II) phosphide2. lithium phosphate3. phosphorus triiodide

7. dinitrogen pentasulfide8. tin (IV) nitride

6. sulfur dibromide

Writing Chemical Formulas

9. rubidium nitrite

11. iron (III) sulfite12. ammonium oxide

Name Charges matter?Use poly.

ion sheet? Formula

yesyes

yesyesno

noyes

no

yes

yesyes

no

yesno

noyesno

nono

no

yes

yesyes

no

Zn3(AsO4)2

Ag3N

Cu3P2

Li3PO4

PI3

N2S5

Sn3N4

SBr2

RbNO2

Fe2(SO3)3

(NH4)2O

OF2

7. S O3

8. Sn Br4

Writing Chemical Names

9. K3 PO4

11. C S2

12. Cu F

10. NH4 OH

Formula RN/GP/neitherUse poly.

ion sheet? Name

GPneitherneither

GPRN

neither

nonoyes

nono

yes

sulfur trioxidetin (IV) bromide

potassium phosphate

carbon disulfidecopper (I) fluoride

ammonium hydroxide

Traditional 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 ending for lower charge. 3. Then say name of anion, as usual.

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+

Write formulas: cuprous sulfide

auric nitrite

ferrous fluoride

Write names: Pb3P4

Pb3P2

Sn(OH)4

Cu1+ S2– Cu2S

Au3+ NO21– Au(NO2)3

Fe2+ F1– FeF2

cuprous sulfide

auric nitrite

ferrous fluoride

Pb3P4

Pb3P2

Sn(OH)4

Pb? P3– Pb? Pb?

Pb? Pb? Pb?

P3– P3– P3–

P3– P3– Pb2+

Pb4+

Pb2+

Pb4+ Pb4+

plumbic phosphidePb2+

plumbous phosphideOH1– Sn4+ Sn? OH1–

OH1– OH1–

stannic hydroxide

Empirical Formula and Molecular Formula

Compound Molecular Formula

EmpiricalFormula

glucose C6H12O6

propane C3H8

butane C4H10

naphthalene C10H8

sucrose C12H22O11

octane C8H18

lowest-termsformula

shows the true numberand type of atoms in a

m’cule

CH2O

C3H8

C2H5

C5H4

C12H22O11

C4H9

0 0

0 0

Resources - Nomenclature

Objectives

Worksheet - binary cmpds: single charge cation

Worksheet - ions in chemical formulas

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

Worksheet - ionic formulas (binary, polyatomic, transition)

Worksheet - traditional system of nomenclature

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

Worksheet - ionic cmpds: polyatomic ions

Outline (general)

Worksheet - empirical and molecular

Worksheet - vocab (bonding)

Activity - bonding pieces

Activity - molecular models

Activity - mole pattern

Worksheet - binary compounds

Worksheet - ions in chemical compounds

Textbook - questions

Worksheet - ionic binary cmpds: multiple charge cation

Worksheet - oxidation numbers and ionic cmpds

Worksheet - names and formulas of cmpds

Worksheet - errors in chemical formulas and nomenclature