Chapter 9 NotesHonors Chemistry

Chapter 9: Chemical Names and Formulas

Section 1: Naming Ions

(read pages 252-259)

Monatomic Ions

  • Ions that consist of a______atom with a ______or ______charge resulting from the ______or ______of ______or more ______electrons
  • Two Types
  • Positive Ions
  • ______
  • Negative Ions
  • ______

Cations

  • ______charged ions
  • Metal atom ______
  • Name ______the ______

Naming Cations Practice

Element / # of valence electrons / Ion formed / Name of cation
Sodium / …………… / ……………………………
…………………… / Ca2+
Magnesium

Anions

  • ______charged ions
  • Nonmetal atom ______
  • Name changes to ______ending

Naming Anions Practice

Element / # of valence electrons / Ion formed / Name of anion
Nitrogen / ………………………..
………………
…… / S2-
Fluoride

Note

  • Groups ______and ______usually ______form ions

Ions of Transition Metals

  • Many of the ______metals form ______than ______cation with ______ionic charges
  • Not ______transition metals have ______than ______charge
  • ______must be determined from the ______of ______

Two Methods to Name Transition Metal Ions

  1. ______
  2. ______

Stock System

  • ______method of ______
  • A ______in ______is placed ______the name of the element to indicate the ______of the ______

Number / 1 / 2 / 3 / 4 / 5 / 6
Roman Numeral

Stock System Naming Practice

Ion Formed / # of Electrons Lost / Stock Name
Cu+ / 1 / Copper (I) ion
Cu2+
Lead (II) ion
Pb4+

Classical Method

  • In the past, scientists used the ______names of elements.

Practice Problems

Name the ions formed by these elements and classify them as anions or cations.

a)Selenium ______

b)Barium ______

c)Phosphorous ______

Polyatomic Ions

  • What does the prefix poly mean?______
  • Polyatomic ions are ______of ______than ______atom
  • ______bound ______of atoms that behave as a ______and carry a ______
  • The names of most polyatomic ions end in ______or______
  • Different Endings
  • Ammonium______
  • ______CN-
  • ______OH-

A Closer Look at a Polyatomic Ion

Name: ______

PO43-

Book Work - Page 258 #3-9

Section 2: Naming and Writing Formulas for Ionic Compounds
(read pages 260-266)

Binary Ionic Compounds

  • What does the prefix bi mean? ______
  • A binary ______compound is composed of ______elements - a ______and a ______

Naming Binary Ionic Compounds

  • If you know the formula of the ionic compound, you can write the name
  • To name any binary ionic compound, place the ______name ______, followed by the ______name.

Naming Binary Ionic Compounds - Examples

  1. Naming a Simple Ionic Compound (1 ______+ 1 ______)
  2. CaCl2______
  1. Naming an Ionic Compound containing a Transition Metal with only ONE possible charge (1 ______+ 1 ______)
  2. ZnS ______
  1. Naming an Ionic Compound containing a Transition Metal with only ONE possible charge (1 ______+ 1 ______)
  2. Cu2O ______b. CuO______

Try It!

Name the following binary ionic compounds:

  1. NaF ______
  2. FeCl3 ______
  3. FeCl2 ______

Writing Binary Ionic Formulas

  • If you know the name of a binary ionic compound, you can write the formula!
  • Write the ______of the ______and then the ______. Then, add the ______that are needed to ______the ______.
  • The ______charge of the ______must balance the ______charge of the ______so that the net ionic charge of the compound is ______.

Remember the Crisscross Method?

  1. ______
  1. ______
  2. ______
  3. ______

Writing Binary Ionic Formulas - Examples

  1. Simple Ionic Compounds:
  2. Sodium Bromide ______
  3. Ionic Compounds with Transition Metals:
  4. Iron (III) Oxide______

Writing Formulas for Binary Ionic Compounds

Write formulas for these binary ionic compounds.

  1. Copper (II) sulfide ______
  2. Potassium nitride ______

11. Write formulas for these compounds

  1. Sodium iodide ______
  1. Potassium sulfide ______
  2. Calcium iodide ______

What is a polyatomic ion?

  • ______bound groups of ______that behave as a ______and carry a ______

Polyatomic Ions behave as a UNIT.

  • You ______change the ______or the ______of ______of each ______in a polyatomic ion or you will change the ______of that ion!!

Naming Compounds with Polyatomic Ions

  • To name a compound containing a polyatomic ion, state the ______, and then the ______.
  • Just like naming binary ______compounds!
  • Except you ______change the anion name!

Naming Compounds with Polyatomic Ions Example

  1. CaSO4______
  2. AlPO4 ______
  3. NaC2H3O2 ______
  4. CuSiO3 ______

Writing the Formula of a Compound containing a Polyatomic Ion

  • Remember: Polyatomic ions ______as a ______.
  • You ______change the assigned ______.
  • Write the ______for the ______, followed by the ______for the ______ion, then ______the charges. Use ______.

Writing Formulas with Polyatomic Ions Example

  1. Aluminum chromate ______
  2. Ammonium sulfide ______
  3. Ammonium sulfate ______
  4. Tin (II) cyanide ______
  5. Magnesium hydroxide ______
  6. Potassium sulfate ______

Try It!
Write the formulas of the following binary ionic compounds:

  1. Tin (IV) sulfide ______
  2. Magnesium nitrate ______
  3. Calcium bromide ______
  4. Sodium hydroxide ______

Book Work - Page 266 #14-19

Section 3: Naming and Writing Formulas for Molecular Compounds
(read pages 268-270)

Binary Molecular Compounds

  • A binary ______compound is composed of ______elements – ______are ______
  • Binary molecular compounds do not contain ______– they are made of… ______

Naming Binary Molecular Compounds

  • Use ______
  • The ______in the name of a binary molecular compound tells how many ______of each ______are present in each ______of the ______

Number / 1 / 2 / 3 / 4 / 5 / 6 / 7 / 8 / 9 / 10
Prefix

Steps for Naming a Binary Molecular Compound

  1. ______that the compound is a binary ______compound.
  2. ______the elements in the ______that they appear in the ______
  3. Use ______to indicate the ______of each kind of atom.
  4. The name of the ______element ______the ______. The ______of the ______element changes to ______

Special Rules

  • If there is only ______atom of the ______element in the formula, drop the ______

Example: CCl4 is called ______, NOTmonocarbon tetrachloride.

  • If the element ______with a ______, drop the ______on the end of the ______.

Example: CO is called ______, NOT carbon monooxide.

Naming Binary Molecular Compounds - Examples

  1. N2O ______
  2. Cl2O8______

Try It!

  1. CBr4 ______
  2. N2H4 ______
  3. PCl5 ______
  4. S2F10 ______

Writing Formulas for Binary Molecular Compounds

  • Use the ______in the name to tell you the ______of each ______in the ______. Then, write the correct ______for the two elements with the appropriate ______.

Writing Formulas for Binary Molecular Compounds – Examples

  1. Dinitrogen trioxide ______
  2. Iodine heptafluoride______

Try It!

  1. Carbon disulfide ______
  2. Tribromineoctoxide ______
  3. Silicon monocarbide ______
  4. Dihydrogen monoxide ______

Book Work - Page 270 #20-25

Section 4: Naming and Writing Formulas for Acids and Bases

(read pages 271-273)

Naming Acids

  • Acid – a ______that contains ______or more ______atoms and produces ______ions (______) when ______in ______
  • ______is most commonly listed ______in the compound
  • Formula: ______
  • NOTE: Acids ______have to have ______first, but ______do.

Rules for Naming Acids

  • ______rules
  • Dependent of the ______(the non ______part)

Rule #1

  • When the name of the ______ends in ______, the ______name begins with ______. The ______of the ______has the suffix ______and is followed by ______.
  • Simply – if there is no ______in the acid formula, the formula for the name is ______
  • Example
  • HCl
  • Cation – ______
  • Anion – ______
  • Name of Acid – ______

Rule #2

  • When the ______name ends in ______, the ______name is the stem of the anion with the suffix ______followed by the word ______.
  • Formula for name: ______
  • Example
  • HClO2
  • Cation – ______
  • Anion – ______
  • Name of Acid – ______

Rule #3

  • When the anion name ______in ______, the ______name is the ______of the anion with the suffix ______followed by the word ______.
  • Formula for name: ______
  • Example
  • HClO3
  • Cation – ______
  • Anion – ______
  • Name of Acid – ______

Practice Problems

  1. H2SO3 ______
  2. HNO3 ______
  3. HBr ______
  4. H3PO3 ______

Writing Formulas for Acids

  • Use the ______in ______
  • Example:
  • Write the formula for hydrocyanic acid.
  • Hydro-root-ic acid means the anion ends in –ide.
  • The cation is ______(______).
  • The anion is ______(______).
  • The formula for the acid is ______.

Practice Problems

Write the formulas for the following acids:

  1. Hydroiodic acid ______
  2. Carbonic acid ______
  3. Carbonous acid ______
  4. Acetic acid ______

Names and Formulas of Bases

  • Base – a ______that produces ______ions (______) when ______in ______
  • Named the ______way as an ______compound: Name of ______, then name of ______.
  • ______is usually ______(_____) but it does not have to be.
  • Example:
  • NaOH
  • Cation: ______
  • Anion: ______
  • Name of Base: ______

Try It!

Provide the appropriate name or formula of the following bases:

  1. Potassium hydroxide ______
  2. Be(OH)2 ______
  3. RbOH ______
  4. Aluminum hydroxide ______

Book Work – Page 273 #26-33

Section 5: The Laws Governing Formulas and Names
(read pages 274-279)

The Law Governing Formulas and Names

  • The ______for naming and writing ______are ______because elements form compounds in ______ways.
  • Two Important ______
  • The Law of ______Proportions
  • The Law of ______Proportions

The Law of Definite Proportions

  • States that in samples of any chemical ______, the ______of the elements are always in the ______.
  • So what does that mean?
  1. What is the formula for water? ______
  2. What is the atomic mass of Oxygen? ______
  3. What is the atomic mass of Hydrogren? ______
  4. What is the mass ratio of Oxygen to Hydrogen in water? ______
  1. What is the formula for Hydrogen Peroxide or Dihydrogen Dioxide? ______
  2. What is the mass ratio of Oxygen to Hydrogen in hydrogen peroxide? ______

The Law of Multiple Proportions

  • Whenever the ______two elements form ______than one ______, the different ______of one element that combine with the ______mass of the other element are in the ______of small ______numbers.

Guidelines for Writing the Chemical Formula of a Compound

  1. An ______ending generally indicates a ______compound.
  2. An ______or ______ending means a ______ion that contains ______is in the formula.
  3. ______in a name generally indicate that the compound is ______.
  4. A ______after the name of a ______shows the ______of the ______.

Naming Review

Naming Practice

Formula / Name / Ionic or Molecular?
Sodium chloride
BrF3
LiNO3
Dinitrogentetrahydride
Potassium hydroxide
Rb2O
Hydrofluoric acid

Book Work - Page 279 #35, 39-41

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