Supplemental packet page 73. carbide ion X- charges nitride ion oxide ion fluoride ion phosphide ion sulfide ion chloride ion phosphate ion sulfate ion

OO

O

monatomic ions oxy ions, XO–

suffix -atessuffix -ides

isoelectronic chargesPO4

3- SO4

2- ClO4

1-

BO33-

CO32-

NO3-

C4±

N-3 O

2- F

1-

P-3 S

2- Cl

1-

MUST learn X— charges!!!

aqueous solutionacid dissolved in H2O

M+ charge NOT calculated

group represents M+ charge

H—XH—O–X

oxy acids hydrohalic acidsatomic acids

suffix -ate changes to —ic

aqueous acids suffix name change

acid as a gas name using

covalent rules

TM+ charge is calculated

from the total number of

X– charges

No ROMAN numeral necessary

Use ROMAN numeral

for TM+ charge

use prefix to indicate the number of nonmetal atoms1 mono2 di3 tri4 tetra5 penta6 hexa7 hepta8 octa9 nona10 deca

use suffix -ide for ending of the last element in the formula

Use of prefixesNO use of prefixes

Acidshydrogen-nonmetals

H—X

TM+ is transition metal

X—XM+ X

–

Nomenclature

Ionic Compounds(cations-anions) nonmetals-nonmetals

Covalent Compounds

M+ is representative metal

NomenclatureSupplemental packet page 73

monatomic ions oxy ions, XO–

suffix -atessuffix -ides

isoelectronic chargesPO4

3- SO4

2- ClO4

1-

BO33-

CO32-

NO3-

C4±

N-3 O

2- F

1-

P-3 S

2- Cl

1-

MUST learn X— charges!!!

carbide ion

X- charges

nitride ionoxide ionfluoride ion

phosphide ionsulfide ionchloride ion

phosphate ionsulfate ionperchlorate ion

borate ioncarbonate ionnitrate ion



hydrogens

hydrogen perchloratedihydrogen sulfate

hydrogen chloridehydrogen nitrate

trihydrogen phosphate

hydrogen acetate

as a gas

Acidsas a pure compoundhydrogen listed first



hydrogens




hydrogen acetate

as a gas

OO

O


H—XH—O–X




acid as a gas name using

covalent rules


H—X

HClO4 > H2SO4 > HCl > HNO3 >> H3PO4 > HC2H3O2

pure compoundAcids named as a

sulfuric acid

nitric acid phosphoric acid

hydrochloric acid

acetic acid

aqueous solutionperchloric acidhydrogen perchlorate

dihydrogen sulfatehydrogen chloridehydrogen nitrate


hydrogen acetate




hydrogen acetate

HClO4 > H2SO4 > HCl > HNO3 >> H3PO4 > HC2H3O2

OO

O


H—XH—O–X





H—X

pure compoundAcids named as a Acids named as an

Acidsas an aqueous solution

Covalent Compounds



Use of prefixes

X—Xnonmetals-nonmetalsCovalent Compounds

CO2

H2S

S2Br6

C4H8

carbon dioxide

dihydrogen sulfide (g)as an acid in aqueous solution

hydrosulfuric acid (aq)

tetracarbon octahydride

disulfur hexabromide

carbon dioxide

Covalent Compounds



Use of prefixes


dinitrogen oxidebetter known as

nitrous oxidelaughing gas

diphosphorus pentaoxide

pentaphosphorus decaoxide

sulfur dioxide(smog)

SO2

P2O5

P5O10

N2O

Covalent Compounds



Use of prefixes


dinitrogen tetraoxide

phosphorus pentafluoride

triarsenic heptaoxide

nitrogen triiodide

NI3

N2O4

PF5

As3O7

Ionic Compounds

NH4+

ammonium ion is M+ like





X– charges


Use ROMAN numeral

for TM+ charge

NO use of prefixes


M+ X

–

Ionic Compounds(cations-anions)


cation anion

= 1-

2+1-

0

Correct Ratios

2+ 2- =

anioncation

0

01+

1+=

anioncation

2-

1

one smilelyw/ two ears

°°2

two ears

°°

one smilely

1 =

the sum of all oxidation numbers in a neutral species is zero, 0,

Ionic Compounds

NH4+






X– charges


Use ROMAN numeral

for TM+ charge

NO use of prefixes


M+ X

–




cation anion

1-= 3-2+

cation anion

1+= 1-2+

Incorrect Ratios

2-3+

2-=

anioncation

1-

Incorrect combinations of ion charge quicklybecomes a headache in chemistry. A unit withoverall charge that is not zero creates a molecule that is lopsided and inbalanced.

= 1

one smilely

°°

one ear

1 °°

one smilelyw/ one ear

duah!

1

?

Ionic Compounds

NH4+






X– charges


Use ROMAN numeral

for TM+ charge

NO use of prefixes


M+ X

–



Fe2+ CO32- = FeCO3

Fe2+ Br- = FeBr2

Li+ CO32- = Li2CO3

Sr2+ OH- = Sr(OH)2

iron (II) carbonate

iron (II) bromide

lithium carbonate

strontium hydroxide

1 2

2 1

11

1 2

TM+ roman numeral

A Roman numeral represents oxidation state:The larger the positive number,The higher the oxidation state of the ion. Only transition metals and heavier post-transition metals (e.g. Sn,Pb) use a Roman numeral in its name


Ion charge calculation in ionic substances

1) Ion charge is called “oxidation state or number”2) memorize the monatomic ions and their charge the “–ides” (C4- , N3- , O2- , F1- ).3) memorize the polyatomic ions and their charge “–ates”( [PO4]3- , [SO4]2- , [ClO4]1- )4) All anions (-ides and -ates) seek out positively charged cations ( Na1+, Ca2+, Al3+ ) to achieve a balance of zero in overall substance charge.

Perhaps the easiest way to calculate an oxidation number for a metal in an ionic compound is to draw a visual. For example, Na2SO4

1) Separate the metal from the nonmetals in the formula,

2) Assign monatomics and polyatomics whose oxidation number was memorized,

3) Knowing the sum of all oxidation numbers in a neutral species is zero (0), solve for the oxidation number of the remaining element.

Na SO4 Na

Na SO4 Na2-

Na SO4 Na2-

1+ 1+

1 + (2-) + 1 = 0

sodium sulfate

Calculate an oxidation number for a metal in an ionic compound of FePO4

1) Separate the metal from the nonmetals in the formula,



Fe PO4

Fe PO4 Na3-

Fe PO4 Na3-

3+ 1+

3 + (3-) = 0

iron (III) phosphate

Calculate an oxidation number for a metal in an ionic compound of Fe3(PO4)2

1) separate the metal from the nonmetals in the formula,



Fe PO4 Fe PO4 Fe

Fe PO4 Fe PO4 Fe3- 3-

Fe PO4 Fe PO4 Fe3- 3-2+ 2+ 2+

2 + (3-) + 2 + (3-) + 2 = 0

iron (II) phosphate

Documents

Supplemental packet page 73. carbide ion X- charges nitride ion oxide ion fluoride ion phosphide ion sulfide ion chloride ion phosphate ion sulfate ion