honors naming compounds notes

NAMING COMPOUNDS

Chemical Formulaindicates the relative number of atoms of each kind in a chemical compound.

Identify the number of atoms in each of the following compounds:

1. KCl= _____________________

2. C6H12O6=__________________

3. NH3=__________________

Finding the number of atoms in a compound with polyatomic ions

Compound What does it look like Numbers of expanded? atoms

1. MgCO3

2. Al(ClO4)3

Compound What does it look like Numbers of expanded? atoms

3. Zn3(PO4)2

4. (NH4)2S

Law of Definite Proportions

• Law stating that every pure substance always contains the same elements combined in the same proportions by weight.

• For example: H2O, will always have the same percent by weight, ex. 11.2% H and 88.8% O

Molecular FormulaRepresents the number and kind of atoms

in a molecule (not necessarily the smallest whole number ratio).

Structural Formulastructural formula indicates two-

dimensional arrangement of the bonds and lone pairs of electrons in a molecule.

Empirical Formula for Molecules (have covalent bonds)

• The chemical formula that represents the simplest (lowest) atomic ratio in which elements can combine.

• Formulas for molecular compounds are NOT NECESSARILY the empirical formula

Molecular Formula Empirical Formula

C2H6

C6H12O6

C4H8

C3H8

C6H10

C4H6

C2H4

C5H10

Empirical Formula for Ionic Compounds

ALWAYS WRITTEN IN EMPIRICAL FORM• The chemical formula that represents the simplest (lowest) atomic ratio

in which elements can combine.• Formulas for ionic compounds are the empirical formula because they are

ALWAYS written in the expressed as the lowest possible ratios.

Empirical Form

Ca2O2

Fe2O2

Pb2O4

Mg2O2

Empirical Formula for Ionic Compounds with Polyatomic Ions

Empirical Form

Fe2(CO3)2

Fe2(HSO4)2

Zn2(SO4)2

Pb2(SO3)2

Empirical or Molecular Formula

If written in molecular formula what is the empirical formula?

Type of Bond

C6H12O6

LiNO3

H2O2

C11H22O11

To determine how many atoms combine with one another in a compound we must

determine each elements OXIDATION NUMBER.

OXIDATION NUMBER

Predicting Ionic ChargesGroup 1:

H+

Li+Na+

K+

Predicting Ionic ChargesGroup 2:

Be2+

Mg2+

Ca2+

Sr2+

Ba2+

Predicting Ionic ChargesGroup 13:

B3+

Al3+

Ga3+

Predicting Ionic ChargesGroup 14:

Predicting Ionic ChargesGroup 15:N3-

P3-

As3-

Nitride

PhosphideArsenide

Predicting Ionic ChargesGroup 16:O2-

S2-

Se2-

Oxide

SulfideSelenide

Predicting Ionic ChargesGroup 15:N3-

P3-

As3-

Nitride

PhosphideArsenide

Predicting Ionic ChargesGroup 16:O2-

S2-

Se2-

Oxide

SulfideSelenide

Predicting Ionic ChargesGroup 17:F1-

Cl1-Br1-Fluoride

Chloride

Bromide

I1- Iodide

Predicting Ionic ChargesGroup 18:

Predicting Ionic ChargesGroups 3 - 11: Many transition elements

have multiple oxidation states.Iron(II) = Iron(III) =

Predicting Ionic ChargesGroups 3 - 11: Some metals

have only one possible oxidation state.Zinc = Zn2+Silver = Ag+

Rules for assigning Oxidation Numbers

1. The atoms in a pure element have an oxidation number of zero.2. Alkali metals always have an oxidation number of +1; alkaline

earth metals always have an oxidation number of +2.3. Fluorine always has an oxidation number of -1.4. Oxygen has an oxidation number of -2 in almost all compounds.

Exceptions are in compounds with a halogen, when it has an oxidation number of +2, and in peroxides (H2O2), when it has an oxidation number of -1.

5. Hydrogen has an oxidation number of +1 in almost all compounds except when combined with a metal when it has an oxidation number of -1.

6. The sum of all the oxidation numbers in a neutral compound is zero.

7. The sum of all the oxidation numbers in a polyatomic ion is equal to the charge of the ion.

ASSIGNING OXIDATION NUMBERS

• A compound has a total charge of ZERO so set your equation equal to ZERO.

• Assign the variable X to your unknown oxidation number.

Given a compound, find the oxidation number of every element you know for certain. Then solve for others using algebra.

a. KMnO4

b. CaCO3

What is in common with the elements in the compound?

H2+1 O1

-2 Mg1+2F2

-1

Al2+3S3-2 Cu3

+1P1-3

Ca1+2Cl2-1 Fe2

+3O3-2

CRISS-CROSS METHOD to determine the chemical formula

1. Write the symbols for the elements side by side.2. Write the oxidation states of each element to the

top right of the symbol.When the nonmetal is combines with a metal, the oxidation state will always be the first number (the negative one) in the list of oxidation states.

3. Criss cross the charges DOWN and use the absolute values (-2 becomes 2).

4. Check to make sure the subscripts are the lowest ratio.

Practice Criss-Cross Method

1. Na and S

2. K and P

3. Al and S

4. Mg and Br

5. Al and O

Write down the only cations on Table E: (positively charges ions)

Write down the only polyatomic ions that end in –ide.

Find the charge of the polyatomic ion using Table E

Put parenthesis around the polyatomic ion.

1. PO4

2. CO3

3. SO3

4. NH4

5. ClO

6. ClO2

7. HSO4

8. ClO4

9. CN

10. OH

11. S2O3

12. SCN

• If you see a group of atoms together with a charge it is a polyatomic ion from Table E.• Put the polyatomic ion within Parenthesis.• Find the charge of the polyatomic ion.• Use the criss-cross method to determine subscripts.

Na +1 CO3-2

How many atoms are present in the compound?

NH4+1 S-2

How many atoms are present in the compound?

Write the formula of the compound composed of the ions shown:a. Place all Polyatomic Ions in Parenthesis (Table E)b. Determine all oxidation numbers of elements and polyatomic ionsc. Use Criss-Cross Methodd. Reduce to Empirical Form if necessary

1. NH4 S

2. Na NO3

3. Cu Br

4. Al SO4

5. Fe CO3

6. Pb PO4

7. Ag ClO

8. Ca F

9. NH4 SO3

10. Cu OH

11. Ni I

12. Zn SO4

13. Pb ClO2

14. H I

15. Fe HSO4

16. Cu CO3

17. NH4 O

18. Ag S

19. Al ClO4

WELCOME BACK!!

HAPPY NEW YEAR!!!!

What is the topic we are learning?

NAMING IONIC COMPOUNDS

• An Ionic compound can quickly be determined if a METAL is bonded to a NONMETAL.

• Naming Ionic compounds with metals that have only ONE oxidation state is fairly simple.

Of the following metals listed below, check off all the elements that have more than one oxidation state:

a. Mn___ b. Zn ___ c. K ____ d. Pb___

e. Mg___ f. Au ___ g. Ag ___ h. Ga ___

i. Sn __ j. Li ____ k. U ____ l. Cr ___

Naming Ionic Compounds that contain metals with only 1

oxidation state.

Binary Ionic CompoundsIonic compounds with only 2 different elements.

Name the metal and end the nonmetal in –ide.

For example: CaBr2 =

1. MgO= ________________________

2. CaCl2 = _______________________

3. AlBr3 = _______________________

4. Ag3N = _______________________

5. Al2O3 = ______________________

6. LiI = _________________________

7. BaF2 = _______________________

8. Zn2C = _______________________

9. Ba3N2 = ______________________

10. CdO = _Cadnium oxide__________Cadmium Oxide

11. Ga2S3 = _______________________

12. K3N = ________________________

13. SrO = ________________________

Ternary Ionic CompoundsIonic Compounds with 3

different elements.They usually contain Polyatomic

Ions (Table E)Name the following Polyatomic Ions:A. NO3

- _________ d. SO42- ___________

B. ClO2- _________ e. S2O3

2- __________

C. CO32- _________ f. SCN- ____________

How to name Ternary Compounds:

Name the metal and then name the polyatomic ion.

For example: KNO3 =

Name the following Ternary compounds:

1. NaC2H3O2 _____________________

2. AgHCO3 _______________________

3. LiNO2 _________________________

4. Ga2(S2O3)3 ____________________

5. Ca3(PO4)2 _____________________

6. ZnSO3 __________________________

7. KClO3 ___________________________

8. Al(OH)3 _________________________

9. RbSCN __________________________

10. SrCO3 _________________________

Naming Ionic Compounds with Metals with Multiple oxidation

states (multiple charges): STOCK SYSTEM

1. Determine the oxidation state of the metal in the compound.

2. Name the metal, put the oxidation state in ROMAN NUMERALS in parenthesis and end the nonmetal in –ide.

Criss-Cross Find Empirical formula

Pb+4 O-2

Cu+2 (SO4) -2

Sn+2(CO3) -2

Work Backwards and Start with the Empirical Formula to determine the Oxidation state of a Metal with

Multiple Oxidation StatesEmpirical Formula Write in the oxidation

number for the nonmetal or polyatomic ion you are sure of and criss-cross.

Non-reduced form with Oxidation States

Fe1O1 Fe O

Fe1(SO4)1 Fe (SO4)

Cu1(SO4)1 Cu (SO4)

Work Backwards and Start with the Empirical Formula to determine the Oxidation state of a Metal with

Multiple Oxidation States

Empirical Formula

Write in the oxidation number for the nonmetal or polyatomic ion you are sure of and criss-cross.

Non-reduced form with Oxidation States

Sn1(SO3)1 Sn (SO3)

Mn1(SO4)2 Mn (SO4)

Cr1(PO4)2 Cr (PO4)

Name the following compound using the Stock System:

1. Fe O ____________________________

2. Fe Cl2 ___________________________

3. Cu SO4 __________________________

4. Pb Cl2 ___________________________

5. Pb O2 ___________________________

6. Cu3(PO4)2 ________________________

7. Cu2 S ___________________________

8. Fe2(CrO4)3 ______________________

19. Sn CO3 _________________________

10. Sn F4 ___________________________

Name each of the following compounds, use Roman Numerals

only when necessary.Put a check next to every compound that begins

with a metal with more than 1 oxidation state.Put parenthesis around all the polyatomic ions.1. NH4 Cl _________________________

2. Pb SO4 _________________________

3. Co Cl3 __________________________

4. Ba (NO3)2 ______________________

5. Co2 (SO3)3 _____________________

6. KH ____________________________

7. NH4 F _________________________

8. K2Cr2O7 _______________________

9. Cu S __________________________

10. Cu ClO2 ______________________

11. Ag NO3 _______________________

12. Fe Cl3 ________________________

13. Cr F2 _________________________

14. Na Cl _________________________

15. Fe PO4 ______________________

16. Li F _________________________

17. Fe F3 _______________________

18. Al (OH)3 _____________________

19. Mg I2 ________________________

20. Fe Cl3 _______________________

Formula Writing for Ionic Compounds

1. All ionic compounds must be in empirical form. (Reduced Form)

2. If the compound ends in –ide, most likely it is a binary compound. Except for cyanide and hydroxide.

3. If the substance ends in –ate or –ite it contains a polyatomic ion. Put the polyatomic ion in parenthesis before you criss-cross.

4. Put the oxidation states on top and criss-cross the numbers.For example: Aluminum Sulfide =

Write the formulas for each of the following compounds:

Make sure you reduce it to empirical form.1. Aluminum Chloride ___________________

2. Silver Phosphate _____________________

3. Lithium Hydride ______________________

4. Magnesium Acetate __________________

5. Potassium Sulfite _____________________

6. Zinc Thiosulfate ____________________

7. Strontium Nitride ____________________

8. Calcium Oxide _______________________

9. Gallium Oxalate ______________________

10. Ammonium Hydroxide ________________

Writing formulas for compounds with metals with more than one oxidations state:

(Roman Numerals will be given)1. If there are Roman Numerals with the name, the Roman Numeral is

the charge of the metals.For example: Iron (II) Oxide= Fe+2O-2=Fe2O2=FeO

2. If the compound ends in –ate or –ite, most likely you should look on the polyatomic ion chart.

3. Write the metal, then look up the polyatomic ion and place it in parenthesis. Put the charges on top and criss-cross. Reduce if necessary.

For example: Zinc Carbonate=

Gold (III) Thiocyanate =

For each compound listed below, write the correct formula using the stock

system.1. Iron (II) Chloride _____________________

2. Lead (IV) Phosphide __________________

3. Tin (II) Oxide ________________________

4. Copper (I) Iodide _____________________

5. Nickel (III) Sulfide ____________________

6. Cobalt (II) Thiocyanate ______________

7. Manganese (IV) Oxide _________________

8. Titanium (IV) Chromate _________________

9. Iron (III) Sulfate _______________________

10. Lead (II) Nitrate ______________________

11. Tin (IV) Carbonate ______________

12. Copper (II) Acetate _____________

Naming Molecular Compounds

• What types of bonds are in molecular compounds? _____________________

• How can we tell if a formula has a covalent bond? ___________________________

Prefix System

Most nonmetals have more than 1 oxidation state, therefore you can use the Stock System (Roman Numerals) or the prefix system.

Molecular Prefix Number of Atoms12345678910

HOW TO NAME MOLECULAR COMPOUNDS

According to the number of atoms of each element, state the prefix for the number of each atom before the name of the element and end the nonmetal in –ide.

For example:P2O5 =CO2 =

The prefix mono only need to be used for the second half of the compound NOT the first element.

Name the following covalent compounds:

1. CI4 ________________________________

2. PCl5 ______________________________

3. SI6 _______________________________

4. P2S6 ______________________________

5. N3O4 ______________________________

6. SO2 ____________________________

7. N2O4 ___________________________

8. CO _____________________________

9. NF3 ____________________________

10. ICl5 ___________________________

11. H2S3 __________________________

12. N2O3 _________________________

13. ClF7 __________________________

14. SO3 ___________________________

15. NI5 ___________________________

16. BN2 __________________________

17. P2O5 _________________________

18. IF7 ___________________________

Many chemical compounds have common names:

Example:–Water

–Ammonia

–Table salt

Naming Acids

1. Elements that begin with hydrogen are normally acids.

2. Naming Binary Acidsa. Begin with the word HYDRO- and end with

the non metal in –ICb. Then add the word ACID

For example: HCl= Hydrochloric acid

3. Naming Ternary Acidsa. Cover the hydrogen and look up the polyatomic ion being used.

b. If the polyatomic ion ends in –ITE change the ending to –OUS and add the word ACID.For example: HClO2 = chlorite = Chlorous Acid

c. If the polyatomic ion ends in –ATE change the ending to –IC and add the word acid.

For example: H2SO4 = sulfate = Sulfuric Acid

Name the following acids:

1. HCl _______________________________

2. HBr _______________________________

3. HF _______________________________

4. H2S ______________________________

5. H3P ______________________________

6. H2Se ___________________________

7. HI ______________________________

8. H2CO3 __________________________

9. H2C2O7 _________________________

10. HNO2 __________________________

11. H3PO4_________________________

12. H2SO3_________________________

13. H2S2O3________________________

For each of the following acids below, write the correct formula.

1. Sulfuric Acid ________________________

2. Hydrochloric Acid ____________________

3. Clorous Acid ________________________

4. Cloric Acid __________________________

5. Thiocyanic Acid _______________________

6. Acetic Acid _______________________

7. Nitric Acid ___________________________

8. Dichromic Acid _______________________

9. HydroIodic Acid ______________________

10. Nitrous Acid ________________________

How can you tell the difference between a binary acid and a ternary acid from its name?

Naming Ionic Compounds using the FormulaDetermining subscripts of elements or polyatomic in ionic compounds

Use Criss-cross method Example:

Naming ionic compounds with metals with only 1 oxidation state

Binary Ionic CompoundsIonic compounds with only 2 different elements.

Name the metal and end the nonmetal in –ide.

For example: CaBr2 = Calcium Bromide

Ternary Ionic CompoundsIonic Compounds with 3 different elements.•Name the metal and then name the polyatomic ion.

For example: KNO3 = Potassium Nitrate

Naming ionic compounds with metals with multiple oxidation state

1. Determine the oxidation state of the metal in the compound.

2. Name the metal, put the oxidation state in ROMAN NUMERALS in parenthesis and end the nonmetal in –ide.

Example: FeO= Iron (II) Oxide

Writing the Formula of Ionic Formulas using the name of the Ionic Compound

Formula Writing for Ionic Compounds

All ionic compounds must be in empirical form. (Reduced Form)If the compound ends in –ide, most likely it is a binary compound. Except for cyanide and hydroxide.If the substance ends in –ate or –ite it contains a polyatomic ion. Put the polyatomic ion in parenthesis before you criss-cross.Put the oxidation states on top and criss-cross the numbers.

For example:Zinc Carbonate= Zn+2(CO3) -2 =

Zn2(CO3)2 =Zn(CO3)

Gold (III) Thiocyanate = Au+3 (SCN) -1 = Au(SCN)3

Writing formulas for compounds with metals with more than one oxidations state:(Roman Numerals will be given)

If there are Roman Numerals with the name, the Roman Numeral is the charge of the metals.

2. If the compound ends in –ate or –ite, most likely you should look on the polyatomic ion chart.

3. Write the metal, then look up the polyatomic ion and place it in parenthesis. Put the charges on top and criss cross. Reduce if necessary.

For example: Iron (II) Oxide= Fe+2O-2=Fe2O2=FeO

THE END