1. Nomenclature
Chemistry 1

2. The Language of Chemistry
Subscripts indicate the number of atoms of an element in a molecule.
C8H18 or MgCl2
How many atoms of each element are in the following?
CH4
SO2 O2
P4O10
Pb(NO3)2

3. Review What is a cation? What is an anion?
What group of elements typically form +1 cations? Why?
What group of elements typically form +2 cations? Why?
What group of elements typically form -1 anions? Why?
What group of elements typically form -2 anions? Why?

4. Ions and Compounds Binary Compounds Ternary Compounds
Monatomic ions (N3-)
Ions formed from a single atom
Polyatomic ions (SO42-)
Ions formed from more than one atom
See hand-out (purple)
Binary Compounds
Made of two elements
Ternary Compounds
Made of three or more elements (contains polyatomic ion)
**When writing chemical formulas for ionic compounds, the overall charge of the compound must be ZERO/NEUTRAL!**

5. Formula of Ionic Compounds
List the cation (positively charged ion) chemical symbol first.
List the anion (negatively charged ion) chemical symbol after the cation.
If the charges are not the same (sum of the oxidation numbers must equal zero), subscripts must be added to indicate a ratio of positive and negative ions.
-The polyatomic ion acts as an individual ion.
-Because polyatomic ions act as a unit, NEVER CHANGE SUBSCRIPTS OF ANY ATOM WITHIN THE ION.
-Transition metals with more than one oxidation number… the charge is noted using roman numerals!

6. Let’s Practice Writing Formulas
Q: What is the chemical formula for aluminum fluoride?
Symbol for aluminum ion = Al3+
Symbol for fluoride ion = F-
2. Al3+F-
3. Least common multiple is .
4. AlF3
5. Orbital Notation Verification

7. Practice Writing Formulas
Write the correct formula for the following ionic compounds.
Potassium and Iodide
Magnesium and Chloride
Aluminum and Bromide
Cesium and Nitride
Barium and Sulfide

8. Practice Writing Formulas With Polyatomic Ions
Sodium and Nitrate
Calcium and Chlorate
Aluminum and Carbonate
Potassium and Chromate
Magnesium and Carbonate

9. Naming Ionic Compounds
List the name of the cation (watch for transition metals).
List the name of the anion, changing the ending to “ide”
If you have a polyatomic anion, just list its name after the cation.
CaCl2 = calcium chloride
Na2S = sodium sulfide

10. Naming Ionic Compounds With A Transition Metal
Work backwards to determine the charge on the transition metal….
Cr2O3 FeO NiCl2 Mn3(PO4)2
Rules To Name Compound:
1. Name the cation
2. Place the charge of the transition metal as a roman numeral
3. Name the anion by changing the ending to “ide”

11. Review – Binary Compounds
Write the correct chemical formula for each of the following compounds.
potassium bromide
magnesium selenide
sodium phosphide
tin(IV) chloride
aluminum oxide
scandium(III) sulfide
Give the correct names for each of the following compounds listed below. KF
SnI4
SiF4
AlBr3
FeCl3
ZnO

12. Review Ternary Compounds
 Write  the  chemical  formulas  for  the  following  names:
Iron (III) acetate
Gold(III) sulfate
Ammonium phosphate
Calcium nitrate
Write the chemical names for the following chemical formulas:
FeC2O4
Pb(CO3)2
Al(MnO4)3
Ba(OH)2

13. Entrance Ticket
Write the formula for the following compounds. Hint-look up the charges for each element/ion and then balance the charges
Calcium Nitride
Rubidium Sulfide
Lead (II) Nitrate
Iron (III) Oxide
Manganese (III) Chlorate
Write the name for the following compounds.
Cr3P2
Al2 (SO4) 3
BaO
CoN
Cu3 (PO4 ) 2

14. Molecular Compounds Nomenclature (Covalent)
When naming compounds consisting of two nonmetals, the names of the elements are written in the same order as they appear in the formula. (The more metallic element is written first.)
The second element uses the suffix “-ide”. Prefixes are added to the name of each element to indicate the NUMBER of atoms of the element in the molecule.
(If the first element’s prefix is mono-, it will be dropped. For example, monocarbon dioxide (CO2) is simply called carbon dioxide.)
**Note: the “o” or “a” at the end of a prefix is usually dropped when the word following the prefix begins with another vowel…e.g. monoxide or pentoxide.

15. Prefixes –Polyatomic Handout
Number of atoms
Mono- 1
Di- 2
Tri- 3
Tetra- 4
Penta- 5
Hexa- 6
Hepta- 7
Octa- 8
Nona- 9
Deca- 10

16. For the following molecular compounds, write the molecular formula:
Carbon mononitride
Sulfur tribromide
Phosphorus triflouride
Nitrogen dioxide
Carbon tetrachloride
Dihydrogen monoxide
Sulfur trioxide
Dinitrogen hexoxide

17. For the following molecular formulas, write the compound name:
SiO2
CO2
SeF6
N2O5
As2O5
AsI3
PCl5
CF4

18. Flow Chart Challenge
Create a flow chart to use while NAMING Ionic and Covalent Compounds
Hints:
How do you distinguish between an Ionic and Covalent Compound?
Which one uses prefixes?
When do you use Roman Numerals in the name?
What do you do for naming polyatomic ions?

19. Chemical Formulas
Chemistry 1

20. Oxidation Numbers “oxidation states”
The number of electrons that must be added to or removed from an atom in a combined state to convert the atom into the elemental form.

21. Assigning Oxidation States
Rules for Assigning Oxidation States
The Oxidation State of…
An atom in an element is zero
Na(s), O2(g), Hg(l)
A monatomic ion is the same as its charge
Na+, Cl-
Fluorine is -1 in its compounds
HF, PF3
Oxygen is usually -2 in its compounds
H2O, CO2
Exception: Peroxides (containing O22-) in which oxygen is -1
Hydrogen is +1 in its covalent compounds
H2O, HCl, NH3

22. Oxidation Numbers - Model
Assign oxidation numbers to the atoms of each element in the following compounds.
PI3 HF
CS2
As2S3
NO2-

23. Oxidation Numbers Practice
Assign oxidation numbers to the atoms of each element in the following compounds.
CI4
HCl
SO3
IO3
H2CO3
SO42-

24. Percent Composition
The percentage by mass of each element in a compound.

25. Steps For Calculations
Using the periodic table determine the molar mass of the compound.
Take each mass for each element (molar mass times number of atoms) and divide it by the total mass of the compound.
Multiply this value by 100 to obtain a percentage.
Percentages should add up to equal 100%
Steps For Calculations

26. Percent Composition
Determine the percent composition in the following compounds:
PbBr4
Ba(OH)2

27. Percent Composition
Determine the percent composition in the following compounds:
NaOH
(NH4)3PO4
CCl2F2
Pb(NO3)2

28. Bite the Bubble Lab
See handout

29. Empirical Formula: The formula with the smallest whole number ratio of the elements in the compound (simplest formula)
Note: May not always be the same as the molecular formula.
To calculate, convert masses of elements to moles.
If a question gives the percentages of each compound, assume you have 100 g of the sample and then each percentage becomes the mass of the element.
Next, divide each mole by the smallest one.
This gives the ratio of atoms, which you will use to write the formula.
Empirical Formula

30. Empirical Formulas
The percent composition of a compound was found to be 63.5% silver, 8.2% nitrogen, and 28.3% oxygen. Determine this compound’s empirical formula.
Name the compound.

31. Empirical Formulas
A g sample of a compound contains g sodium, g chromium and g oxygen. What is the empirical formula?
Name the compound.

32. Empirical Formula
grams of an organic compound is known to contain grams of carbon, grams of hydrogen, grams of oxygen and the rest is nitrogen. What is the empirical formula of the compound?

33. Molecular Formulas
Molecular Formulas: A formula that specifies the actual number of atoms of each element in one molecule of the substance.
-Molecular formula is a multiple of the empirical formula.
Steps for Solving:
Determine the Empirical Formula first!
Use the formula :
N= The number we will multiply the subscripts in the empirical formula by to obtain the new molecular formula.

34. Empirical and Molecular Formulas
A compound of boron and hydrogen has a percent composition of 78.14% boron and 21.86% hydrogen. If the molar mass is 27.6, what is the empirical and molecular formula?

35. Empirical and Molecular Formulas
A compound with the formula C2H5O is found to have a molar mass of 90g. What is the molecular formula of the compound?

36. Chapter Review Test will cover… New
Ionic, Molecular, and Acid Nomenclature
Oxidation Numbers and Percent Composition
Empirical and Molecular Formulas
Chemical Bonding
Periodic Table Trends, Electron Configuration and Periodic Table History
Chapter Review