Section 2.2—Naming Chemicals

Section 2.2—Naming Chemicals

We need to be able to name the chemicals in the antacids!

The Language of Chemistry

Chemistry has a language all of its own

Each element symbol starts with a capital letter

EnglishChemistry

Element Symbols Letters

Chemical Formulas Words

Chemical Equations Sentences

Binary Ionic compounds

Definitions

Binary Ionic Compound- compound containing two elements—one metal and one non-metal

+Cation

+Cation

-Anion

-Anion Ionic Compound

Ionic bond- bond formed by attraction between + and - ions

Metals & Non-Metals

Ionic Bonds are between metals & non-metals

H He

Li Be B C N O F Ne

Na Mg Al Si P S Cl Ar

K Ca Sc Ti V Cr Mn Fe Co Ni Cu Zn Ga Ge As Se Br Kr

Rb Sr Y Zr Nb Mo Tc Ru Rh Pd Ag Cd In Sn Sb Te I Xe

Cs Ba Lu Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn

Fr Ra Lr Rf Db Sg Bh Hs Mt Uun Uuu Uub Uut

Metals Metalloids Non-metals

These compounds have:2 elements (“binary”)A metal & a non-metal (“ionic”)

To name these compounds:Write the name of the metal (the cation)Write the name of the non-metal (the anion) with

the suffix “-ide”

Identifying & Naming Binary Ionic

The subscripts in the formula do not matter when naming this type

Example #1

NaCl

Example #1

NaCl

Cation

Anion

“Sodium”

“Chlorine” becomes “Chloride”

Sodium Chloride

Example #2

CaBr2

Example #2

Cation

Anion

“Calcium”

“Bromine” becomes “Bromide”

CaBr2

Calcium Bromide

Example #3

K2O

Example #3

K2O

Cation

Anion

“Potassium”

“Oxygen” becomes “Oxide”

Potassium Oxide

Let’s Practice

Example:Write the name for the following

compounds

CaF2

Na3P

NaCl

SrBr2

Let’s Practice

Calcium fluoride

Sodium phosphide

Sodium chloride

Strontium bromide


compounds

CaF2

Na3P

NaCl

SrBr2

Polyatomic Ionic Compounds

Definition

Polyatomic Ion- more than one atom that together have a charge

+Cation

+Cation

Polyatomic Ionic Compound- compound containing at least one polyatomic ion

-Polyatomic

Anion

Polyatomic IonicCompound

Common Polyatomic Ions

COMMON POLYATOMIC IONS

Acetate, CH3COO-1 or C2H3O2-1

Ammonium NH4+1

Bromate, BrO3-1

Bromite, BrO2-1

Carbonate, CO3-2

Carbonite, CO2-2

Chlorate, ClO3-1

Chlorite, ClO2-1

Chromate, CrO4-2

Cyanide, CN-1

Dichromate, Cr2O7-2

Dihydrogen phosphate, H2PO4-1

Hydrogen carbonate or bicarbonate, HCO3

-1

Hydrogen phosphate or biphosphate, HPO4

-2

Hydrogen sulfate or bisulfate, HSO4-1

Hydroxide, OH-1

Hypochlorite, ClO-1

Iodate, IO3-1

Iodite, IO2-1

Nitrate, NO3-1

Nitrite, NO2-1

Oxalate, C2O4-2

Perchlorate, ClO4-1

Permanganate, MnO4

-1

Peroxide, O2-2

Phosphate, PO4-3

Phosphite, PO3-3

Silicate, SiO3-1

Sulfate, SO4-2

Sulfite, SO3-2

The Appendix of your book (Page A-2) has the following chart

The only cation (front-half) polyatomic ion is “NH4”

All other polyatomic ions are anions (back-half)

The subscripts within the polyatomic ion is important (it must match exactly with the one on your ion list)

If there are parenthesis, the polyatomic ion is inside (ignore the number outside)

Help Identifying Polyatomic Ions

Practice Identifying Polyatomic Ions

Example:Identify and name the

polyatomic ion in each

compound

NaNO3

NH4Cl

Ca(OH)2

(NH4)3PO4

K2CO3

Practice Identifying Polyatomic Ions

Example:Identify and name the

polyatomic ion in each

compound

NaNO3

NH4Cl

Ca(OH)2

(NH4)3PO4

K2CO3

Nitrate

Ammonium

Hydroxide

Ammonium & phosphate

Carbonate

These compounds have:More than 2 capital letters (non starting with H)Contain at least 1 metal & 1 non-metal

To name these compounds:Write the name of the cation (the metal element

name or “Ammonium” for “NH4”)

If the anion is a polyatomic ion, write the polyatomic ion’s name just as it is

If the anion is a single non-metal element, write its name with the suffix “-ide”

Identifying & Naming Polyatomic Ionic

Example #4

NaNO3

Example #4

NaNO3

Cation

PolyatomicAnion

“Sodium”

“Nitrate”

Sodium Nitrate

Example #5

K2SO4

Example #5

Cation

PolyatomicAnion

“Potassium”

“sulfate”

K2SO4

Potassium sulfate

Example #6

Ca(OH)2

Example #6

Ca(OH)2

Cation

PolyatomicAnion

“Calcium”

“hydroxide”

Calcium hydroxide

Example #7

(NH4)2S

Example #7

PolyatomicCation

Anion

“Ammonium”

“sulfur” becomes “sulfide”

(NH4)2S

Ammonium sulfide

Let’s Practice


compounds

Ca(NO3)2

Na3PO4

NH4ClO

K2CO3

Let’s Practice

Calcium nitrate

Sodium phosphate

Ammonium hypochlorite

Potassium carbonate


compounds

Ca(NO3)2

Na3PO4

NH4ClO

K2CO3

Multivalent Metals

Definition

Multivalent Metal- metal that has more than one possibility for cationic charge


Common multivalent metals and their charges

Cobalt Co+2 Co+3

Copper Cu+1 Cu+2

Iron Fe+2 Fe+3

Lead Pb+2 Pb+4

Manganese Mn+2 Mn+3

Mercury Hg2+2 Hg+2

Tin Sn+2 Sn+4

These compounds have:One of the multi-valent metals in that chart

To name these compounds:Write the name of the metal element (cation)Write the name of the anion (element name with “-ide” or

polyatomic ion name)Determine the total negative chargeTotal negative charge = total positive charge for all

neutral compoundsDetermine the charge on each metal atomWrite the charge in roman numerals in parenthesis after

the metal’s name

Identifying & Naming Multivalent Metals

Common Ions

N3-

O2-

F-

P3-

S2-

Cl-

Se2-

Br-

I-

Periodic table--Charges of common ions

Use the periodic table to determine charges on common elemental anions

Example #8

CuCl

Example #8

CuCl

Cation

Anion

“Copper”


Copper Chloride

Example #8

CuCl

Cation

Anion

“Copper”


Copper Chloride

Chloride has a –1 charge

-1 charge * 1 ion = -1

A –1 charge needs a +1 charge

Therefore, copper must be +1

(I)

Example #9

Fe2(CO3)3

Example #9

Fe2(CO3)3

Cation

Polyatomic Anion

“Iron”

“Carbonate”

Iron carbonate

Example #9

Fe2(CO3)3

Cation

Polyatomic Anion

“Iron”

“Carbonate”

Iron carbonate

Carbonate has a –2 charge

-2 charge * 3 ions = -6

A –6 charge needs a +6 charge and there are 2 iron ions

Therefore, iron must be +3

(III)

Let’s Practice


compounds

PbCl2

PbCl4

MnO

Mn2O3

Let’s Practice

Lead (II) chloride

Lead (IV) chloride

Manganese (II) oxide

Manganese (III) oxide


compounds

PbCl2

PbCl4

MnO

Mn2O3

Binary Covalent Compounds

Definition

Binary Covalent Compound compound made from two non-metals that share electrons

Nonmetal

Nonmetal

Nonmetal

Nonmetal Covalent compound

Covalent bond atoms share electrons

These compounds have:2 elements (“binary”)Both non-metals (“covalent”)

To name these compounds:Write the name of the first element with the

prefix indicating the number of atoms (except don’t use “mono-”)

Write the name of the second element with the prefix indicating the number of atoms (including “mono-”) and the suffix “ide”

Identifying & Naming Binary Covalent

Covalent Prefixes


PREFIXES USED IN MOLECULAR COMPOUNDS1. mono-

2. di-3. tri-

4. tetra-5. penta-6. hexa-7. hepta-8. octa-9. nona-10.deca-

Example #10

P2O5

Example #10

P2O5

Phosphorus

Oxygen

2 = “di-”

5 = “penta-”Use “-ide”

Diphosphorus pentaoxide

Example #11

SiO2

Example #11

Silicon

Oxygen

Don’t use “mono-” on first element

2 = “di-”Use “-ide”

SiO2

Silicon dioxide

Let’s Practice


compounds

CO2

N2O4

P4O10

CO

Let’s Practice

Carbon dioxide

Dinitrogen tetraoxide

Tetraphosphorus decaoxide

Carbon monoxide


compounds

CO2

N2O4

P4O10

CO

Nomenclature Summary

Naming Chemical Formulas

Starts with a metal or NH4

Does not contain a metal = Binary

Covalent compound

2 capital letters = Binary Ionic

More than 2 elements = Polyatomic Ionic

Mixed Practice


compounds

Na2O

K3PO4

Cu(OH)2

(NH4)2S

MgCl2

Mixed Practice

Sodium oxide

Potassium phosphate

Copper (II) hydroxide

Ammonium sulfide

Magnesium chloride


compounds

Na2O

K3PO4

Cu(OH)2

(NH4)2S

MgCl2

Documents

Section 2.2—Naming Chemicals