Unit 5 Nomenclature pp. 95 - 117. Binary Ionic Compounds Monovalent and Multivalent.

Unit 5 Nomenclature

pp. 95 - 117

Binary Ionic Compounds

Monovalent and Multivalent

Ionic Compounds

• Binary Ionic compounds– Monovalent; metal present forms only 1 type of

cation• Na → Na1+

• Mg → Mg2+

– Multivalent; metal present can form 2 or more different cations that have different charges. • Cu → Cu2+

• Cu →Cu3+

• Cr → Cr1+

• Cr → Cr2+

Rules for Naming Monovalent Binary Ionic Compounds

1. The cation is always named first and the anion second.2. A monatomic cation takes its name from the element.

Example; Na1+ is called sodium in the names of compounds containing this ion.

3. A monatomic anion is named by taking the first part of the element name (the root) and adding –ide. Example; Cl1- is called chloride.

4. Write the name of the compound by combining the names of the ions.

Examples of Naming

1. NaCl2. KI3. CaS4. CsBr5. MgO

Examples of Writing Formulas

1. Aluminum chloride2. Magnesium Iodide3. Rubidium oxide4. Strontium iodide5. Potassium sulfide

Remember

• Compounds formed from metals and non-metals are ionic.

• In an ionic compound the cation is always named first.

• The net charge of an ionic compound is always zero.

Multivalent Binary Ionic Compounds

• Multi-valent metals(transition metals) with a monatomic non-metal.

• Gold can form Au1+ and Au3+.• The name Gold chloride could be either AuCl or

AuCl3, but which one? • Roman numerals are used to specify the charge on

the cation. • Except for Ag1+, Cd2+ and Zn2+ which do NOT need a

Roman numeral in the name even though they are transition metals.

Examples of Naming

1. Fe2O3

2. CuCl2

3. PbO2

4. MnO4

5. CrO3

Examples of Writing Formulas

1. Manganese (IV) oxide2. Nickel (III) sulfide3. Iron (VI) selenide 4. Vanadium (III) nitride 5. Silver oxide 6. Cadmium fluoride

Does the compound contain a mono- or multi-

valent cation?

Monovalent Multivalent

Name the cation, using the element

name.

Using the principle of charge balance, determine the cation

charge.

Include in the cation name a Roman numeral indicating the

charge.

Ionic Compounds with Polyatomics

Naming Ionic Compounds that contain Polyatomic ions

• Polyatomic ions; charged entities composed of several atoms covalently(sharing e-) bonded together.

• Most of them are oxyanions with varying number of oxygens in the formula.

Polyatomic ions- p. 109

ION NAME ION NAME

NH4+ Ammonium CO3

2- CarbonateNO2

1- Nitrite ClO1- HypochloriteNO3

1- Nitrate ClO21- Chlorite

SO32- Sulfite ClO3

1- ChlorateSO4

2- Sulfate ClO41- Perchlorate

OH1- Hydroxide Cr2O72- Dichromate

PO43- Phosphate CrO4

2- Chromate

Naming Ionic Compounds that contain Polyatomic ions.

• Pretty much the same rules as with binary ionic compounds but you use the Polyatomics name.

• Need to recognize that it is an ionic compound with a polyatomic.

• Need ( ) around polyatomics if there is more than 1

Binary Compound?

NO YES

Polyatomic ion or ions present?

Use the Naming

Strategy from p. 95

Use the polyatomic ion’s proper name in the name of

the compound. YES

Examples

1. NH4SO4

2. Na2CO3

3. Zn3(PO4)2

4. Co(C2H3O2)2

5. SnSO3

6. Pb(NO3)4

Examples

1. Ammonium oxide2. Copper (II) Sulfate3. Iron (II) nitrate4. Cobalt (III) sulfite5. Zinc permanganate6. Silver nitrate7. Cobalt (II) phosphate

Naming Molecular Compounds

pp. 103-108

Molecular/covalent Compounds• Binary compounds that contain only NONMETALS

share electrons to form a compound. • Rules for naming molecular compounds; – The first element in the formula is named first, and the full

element name is used.– The second element gets an –ide ending. – Prefixes are used to denote # of atoms present. – Mono is never used for naming the first element.– Concerning Vowels;• No “ao” , no “oo” yes to “io”. • Its monoxide; not monooxide• Its pentoxide; not pentaoxide

Prefix Number of atomsMono- 1

Di- 2Tri- 3

Tetra- 4Penta- 5Hexa- 6

Hepta- 7Octa- 8Nona- 9Deca- 10

Examples

1. CCl4

2. NO2

3. IF5

4. SiO2

5. O2F2

6. XeF6

Examples

1. Phosphorus pentachloride2. Tetraphosphorus hexoxide3. Sulfur hexafluoride4. Sulfur trioxide5. Sulfur dioxide6. Pentaphosphorus decoxide7. Dinitrogen trioxide

Naming Acids

pp. 113-116

Naming Acids

• When dissolved in water, certain molecules produce H+ ions (protons).

• 2 types of Acids;• Binary - hydrogen and a monatomic anion.• Oxyacids – hydrogen and a polyatomic anion.

Naming Acids

1. If binary acid; the acid is named with the prefix hydro- and the suffix –ic to the root name for the element.

2. If oxyacid ( with a polyatomic); 1. If the polyatomic anion ends in –ate, then acid ends in

–ic.2. If the polyatomic anion ends in –ite, then acid ends in –

ous. 3. No prefix of hydro-

Examples• HCl is hydrochloric acid• HBr is hydrobromic acid• HI is hydroiodic acid• HCN is hydrocyanic acid• H2SO4 is sulfuric acid

• H2SO3 is sulfurous acid

• HNO3 is nitric acid

• HNO2 is nitrous acid

• H3PO4 is phosphoric acid

• H3PO3 is phosphorous acid

Metal cation Monovalent Use cation full

name and anion with –ide end.

Formula must be neutral.

Subscripts tells how many to make neutral

Metal cation Multivalent. Includes; Sn, Pb

Bi. Does not

Include; Zn, Ag, Cd

Use cation full name with Roman # and anion with –ide end.

Roman # in name NOT formula.

Use math to determine charge of mutlivalent cation.

IONIC All non-metals Use prefixes in

name to tell how many.

Mono- not needed for first element.

Second element uses ALL prefixes, gets –ide ending.

No “ao”, “oo”

Two types; binary and oxy.

Binarys get hydro- and –ide ending. All non-metals

Oxys; “I ate something icky”

Anion ends in –ate, acid ends in –ic

Anion ends in –ite, acid ends in –ous

COVALENT ACIDS