Naming Compounds

Hypochlorous Acid

Overview

• Determine names from formulas.

• Determine formulas from names.

How do we know...

• it’s formula is HClO. Why does it have that name?

• quantities of atoms in hypochlorous acid?

What is a chemical name?...

• Common names include - laughing gas (N2O), quicksilver (Hg), lime (CaO), and saltpeter (NaNO3).

• Chemical names are those agreed upon by IUPAC (International Union of Pure and Applied Chemistry).

• We can determine many of their names by using standard conventions.

Naming Compounds

Ionic Covalent Acid

Naming Compounds

Ionic Covalent Acid

Disclaimer: What you will learn is useful, but will not apply to the over 11 million possible compounds.

Naming Compounds

Ionic Covalent Acid

Determine name based on

ending

Put Elements in order

add “-ide”

use greek

prefixes

Name the anion

Name the

cation

Naming Compounds

Ionic Covalent Acid

Determine name based on

ending

Put Elements in order

add “-ide”

use greek

prefixes

Name the anion

Name the

cation

First we need to determine the

bond...

How do we tell ionic, covalent, and acids apart?

• Ionic has a metal and a non-metal. They can also be formed with polyatomic ions acting as cation(s) and anion(s).

• Covalent has two or more metals.

• Acids begin with H and are aqueous solutions.

Ionic, Covalent, (or Acid)

• AlBr3 =

• NaNO3 =

• CO2 =

• KHSO4 =

• H2SO4 =

Ionic, Covalent, (or Acid)

• AlBr3 = ionic, metal and non-metal.

• NaNO3 = ionic, note the nitrate is a polyatomic ion.

• CO2 = covalent, both non-metals.

• KHSO4 = ionic, metal and non-metal(s).

• H2SO4 = acid, begins with H. Why not covalent?

Molecular Compounds

1. Identify metal(s) and non-metal(s).

2. The name of the element farthest to the left in the periodic table is written first. If both elements are in the same group, the lower one is written first.

3. The name of the last element is given with an “-ide” ending.

4. Place the prefix that applies to the number of atoms.

PrefixesNumber Prefix Example

1 None (or mon-) chloride2 di- dichloride3 tri- trichloride4 tetra- tetrachloride5 penta- pentachloride6 hexa- hexachloride7 hepta- heptachloride8 octa- octachloride9 nona- nonachloride10 deca- decachloride

Molecular Compounds1. Identify metal(s) and non-metal(s). Note: there should be only non-

metals.

2. The name of the element farthest to the left in the periodic table is written first. If both elements are in the same group, the lower one is written first. WHY?

•1. There are occasional exceptions to this rule (most commonly oxygen except when written with fluorine).

3. The name of the last element is given with an “-ide” ending.

4. Place the prefix that applies to the number of atoms.

Practice

• CF4 =

1. Identify metal(s) and non-metal(s).

2. The name of the element farthest to the left in the periodic table is written first. If both elements are in the same group, the lower one is written first.

3. The name of the last element is given with an “-ide” ending.

4. Place the prefix that applies to the number of atoms.

Practice

• CF4 = Carbon Tetrachloride.

Practice

• N2F2 =

1. Identify metal(s) and non-metal(s).

2. The name of the element farthest to the left in the periodic table is written first. If both elements are in the same group, the lower one is written first.

3. The name of the last element is given with an “-ide” ending.

4. Place the prefix that applies to the number of atoms.

Practice

• N2F2 = dinitrogen difluoride

Practice

• PCl5 =

Practice

• PCl5 = Phosphorus Pentachloride.

Practice

• N2O5 =

Practice

• N2O5 = dinitrogen pentoxide

• Note: you drop the a in “penta”. You can drop the last vowel of the prefix always before “oxide.”

Examples of Molecular Compounds

• Cl2O = dichlorine monoxide

• NF3 = nitrogen trifluoride

• N2O4 = dinitrogen tetrafluoride

• P4S10 = tetraphosphorus decasulfide

Practice Molecular Compounds

• Cl2O = dichlorine monoxide

• NF3 = nitrogen trifluoride

• N2O4 = dinitrogen tetrafluoride

• P4S10 = tetraphosphorus decasulfide

Practice Molecular Compounds

• Cl2O =

• NF3 =

• N2O4 =

• P4S10 =

Molecular Practice

1. SO2 =

2. PCl5 =

3. N2O3 =

4. SF6 =

5. IF5 =

6. XeO3 =

Molecular Practice

1. SO2 = Sulfur Dioxide

2. PCl5 = Phosphorus Pentachloride

3. N2O3 = Dinitrogen Trioxide

4. SF6 = Sulfur Hexafluoride

5. IF5 = Iodine Pentafluoride

6. XeO3 = Xenon Trioxide

Homework

• Review your notes and the section on covalent compounds.

• Complete the practice sheet.

• Preview the section on ionic compounds.

Ionic Compounds

1. Name the cation.

2. Name the anion.

3. Name the compound.

Ionic Compounds - Cation

1. Name the cation.

1.1.Cations formed from metals have the same name as the metal. e.g. Sodium Chloride.

2. Name the anion.

3. Name the compound.

Ionic Compounds - Cation1. Name the cation.

1.1.Cations formed from metals have the same name as the metal. e.g. Sodium Chloride.

1.2.If a metal can form ions with dif’t charges, specify the charge with a roman numeral. e.g. Iron (11) Chloride. Note: sometimes you’ll see a classical name - ferric chloride.

2. Name the anion.

3. Name the compound.

Ionic Compounds - Cation1. Name the cation.

1.1.Cations formed from metals have the same name as the metal. e.g. Sodium Chloride.

1.2.If a metal can form ions with dif’t charges, specify the charge with a roman numeral. e.g. Iron (11) Chloride. Note: sometimes you’ll see a classical name - ferric chloride.

1.3.Cations formed from nonmetals have names ending in “-ium”. These are uncommon. Common(nest) examples are Hydronium ion (H30+) and Ammonium ion (NH4+).

2. Name the anion.

3. Name the compound.

Ionic Compounds - Anion

1. Name the cation.

2. Name the anion.

2.1.Monatomic ions have names formed by replacing the end of the element with an “-ide”. e.g. Lithium Bromide (LiBr). Note: some simple polyatomic ions also end in “-ide” e.g. hydroxide (OH-).

3. Name the compound.

Ionic Compounds - Anion1. Name the cation.

2. Name the anion.

2.1.Monatomic ions have names formed by replacing the end of the element with an “-ide”. e.g. Lithium Bromide (LiBr). Note: some simple polyatomic ions also end in “-ide” e.g. hydroxide (OH-).

2.2.Most polyatomic ions contain oxygen and end in “-ate” to denote the most common form. The ending “-ite” is used for ions that have the same charge but one less oxygen. e.g. Sulfate (SO42-) and sulfite (SO32-). These are referred to as oxyanions.

3. Name the compound.

Ionic Compounds - Anion1. Name the cation.

2. Name the anion.

2.1.Monatomic ions have names formed by replacing the end of the element with an “-ide”. e.g. Lithium Bromide (LiBr). Note: some simple polyatomic ions also end in “-ide” e.g. hydroxide (OH-).

2.2.Most polyatomic ions contain oxygen and end in “-ate” to denote the most common form. The ending “-ite” is used for ions that have the same charge but one less oxygen. e.g. Sulfate (SO42-) and sulfite (SO32-). These are referred to as oxyanions.

2.3.When H+ is added on the front of an oxyanion, write hydrogen before the name. e.g. hydrogen carbonate ion (HCO3-) as opposed to carbonate (CO32-). Note: prefixes apply to the H.

3. Name the compound.

Ionic Compounds - Putting it together...

1. Name the cation.

2. Name the anion.

3. Name the compound. Simply put the names of the ions together with the cation first. e.g. Calcium Chloride (CaCl2)

Ionic Practice

• LiI =

Ionic Practice

• LiI = Lithium Iodide

Ionic Practice

• CaBr2 =

Ionic Practice

• CaBr2 = Calcium Bromide

Ionic Practice

• Ag2O=

Ionic Practice

• Ag2O= Silver Oxide

Ionic Practice

• CuCl =

Ionic Practice

• CuCl = Copper (I) Chloride

Ionic Practice

• FeCl2 = Iron (II) Chloride

Ionic Practice

• FeCl2 =

Ionic Practice

• FeCl2 = Iron (II) Chloride

More Ionic Practice

• Ba(OH)2 =

• K2SO4 =

• Cr2O3 =

• KHSO4 =

More Ionic Practice

• Ba(OH)2 = Barium Hydroxide

• K2SO4 = Potassium Sulfate

• Cr2O3 = Chromium (III) Oxide

• KHSO4 = Potassium Hydrogen Sulfate

Acids

1. Acids based on anions whose name ends in “-ide”

a. “-ide” = “hydro-” + ______ + “-ic” + “acid”

Acid Practice

• HCl =

• H+ and Cl-

• Note: contains the chloride ion.

• “hydro”+________+”ic”+”acid”

Acid Practice

• HCl = Hydrochloric Acid

Acid Practice

• H2S =

• H+ and S2-

• Note: contains the sulfide ion.

Acid Practice

• H2S = Hydrosulfuric acid

Acids1. Acids based on anions whose name ends in “-ide”

a. “-ide” “hydro-” + “-ic” + “acid”

2. Acids based on anions whose name ends in “-ate” or “-ite”

a. “-ate” “-ic” + “acid”

b. “-ite” “-ous” + “acid”

c. If there is a “per-” or “hypo-”, these prefixes are retained.

Acid Practice

• H3PO4 =

• H+ and PO43-

• Note: contains the phosphate ion

• _____ + “ic” + “acid”

Acid Practice

• H3PO4 = Phosphoric Acid

Acid Practice

• H3PO3 =

• H+ and PO33-

• Note: contains the phosphite ion

• _____ + “ous” + “acid”

Acid Practice

• H3PO3 = Phosphorous Acid

Acid Practice

• HClO =

• H+ and ClO-

• Note: contains the hypochlorite ion

• _____ + “ous” + “acid”

Acid Practice

• HClO = Hypochlorous Acid

Assorted Acid Practice

• HI =

• HBr =

• HNO3 =

• HNO2 =

• H2CO3 =

Assorted Acid Practice

• HI = Iodic Acid

• HBr = Bromic Acid

• HNO3 = Nitric Acid

• HNO2 = Nitrous Acid

• H2CO3 = Carbonic Acid

Note about Acids

• The previous compounds are H2O solutions.

• When the compounds are not in water, they are named “hydrogen” + stem name of the nonmetal + “-ide”.

• e.g. Hydrogen Sulfide, H2S

Homework

• Complete the practice sheet.

• Be sure to have read pages 108-120.