1. Review of the Fundamentals
(strap on your seat belt)

2. Nomenclature Ionic MNm TmNm MXO MNm – Name the ions
Cations – no change
Anions – end in –ide
KCl
MgBr2
CaS
For fomulas make them electrically neutral by crisscrossing charges
Barium oxide
Sodium phosphide
Aluminum fluoride

3. TmNm Roman numeral indicates charge Chromium (III) oxide Zinc iodide
Lead (II) sulfide
Silver chloride
Tin (II) oxide

4. Naming – have to calculate the charge of the Tm
FeCl2
FeCl3
CuO
Co2O3

5. Binary Acids Hydro___________-ic acid HCl H2S H3P Hydrobromic acid
Hydroiodic acid

6. Ternary Compounds MXO or TmXO
Name metal name polyatomic ion
KClO3
Na2SO4
Al(NO2)3
Crisscross charges to make electrically neutral
Ammonium dichromate
Calcium actetate
Sodium carbonate
Magnesium phosphate
Potassium nitrite

7. Ternary Acids HXO (oxyacids)
-ate changes to –ic and add the word acid
-ite changes to –ous and add the word acid
HNO3
HNO2
H3N
Perchloric acid
Hypochlorous acid
Bromous acid

8. Non-organic Covalent compounds NmNm
1st element sometimes gets a prefix (if subscript > 1)
2nd element always gets a prefix
2nd element always ends in –ide CO
CO2
N2O
NO2
Sulfur trioxide
Diphosporus pentachloride

9. Notes on polyatomic ions
-ate vs ite
Prefixes
Bi-
Hypo-
Per-
Elements in the same family bond the same way chlorate bromate

10. Some New Stuff Organic compounds (carbon “chains)
Organic compounds are defined by functional groups
Some functional groups you will need to know for this class
Acids (carboxylic acids) – C(=O)-OH
Alcohols –OH
Keytones – R1-C(=O)-R2
Aldehydes R-C(=O)-H
Esters R1-C(=O)-O-R2

11. Hydrocarbons Alkanes CnH2n+2 Alkenes CnH2n Alkynes CnH2n-2
(saturated – all single bonds)
Alkenes CnH2n
(unsaturated- double bonds)
Alkynes CnH2n-2
(unsaturated- triple bonds)

12. Hydrocarbon nomenclature
Prefixes
Meth
Eth
Prop
But
Pent
Hex
Hept
Oct
Suffixes
ane
ene
yne
-ol
-oic

13. Practice Practice C2H6 C2H5OH C2H5COOH C3H6 C3H7OH C4H6 C4H5OH butene
Butanol
Propanoic
Methanoic
Cyclobutane
cyclohexane

14. Keytones
ketones are named by changing the suffix -ane of the parent alkane to -anone.
The position of the carbonyl group is usually denoted by a number.
C H3-CO-CH3 2-propanone (acetone)

15. Aldehydes
The name is formed by changing the suffix -e of the parent alkane to -al, so that HCHO is named methanal, and CH3CH2CH2CHO is named butanal.

16. Chemical Laws Laws of Conservation Of Mass Lavoisier
Matter is not created or destroyed
Application – balancing equations
Atoms are conserved

17. Law of Definite Composition
Proust
“Every compound always contains the mass proportions of elements”
Ex : water mass proportions will always be a multiple of 2.02gH: 16.0g O
Law of Multiple Proportions
Dalton
“When two elements form different compounds, the ratio of masses of element A combined with 1.00 g of element B is a whole number”
Ex.
Compound
Mass of oxygen that combines with 1.0g Carbon 1
1.33g 2
2.66g

18. Historic Models Daltons model pg 46 Dalton, Thomson, Rutherford, Bohr
(chapter two)

19. Subatomic Particles A-Z format Atomic number (Z number)
Equal to the number of protons in an atom
Atomic Mass
Since electrons have insignificant mass, the mass atomic mass is the sum of protons and neutrons
Isotopes- have the same number of protons, but different numbers of neutrons
A-Z format

20. Mass spectrometer
Used to determine the isotopes of an element and there fore the Average atomic mass
Data is measured in percent deflection

22. Average Atomic Mass Weighted average
Takes into considerations how common the isotopes are
Ex. There are 3 common isotopes of Uus. The mass spectrometer produced the data below. What is the average atomic mass of Uus
Mass
percent
283.4 amu
34.60
284.7 amu
21.20
287.8 amu
44.20

23. All the ways you learned to get moles Last Year
Solids
Gases
Moles
Liquids
Solutions

24. Given: 0.6331g ammonium sulfate
_______ mol
_______ mol H atom
_______ Formula units
_______ N atoms
_______ g Oxygen

25. Percentage Composition Empirical and Molecular Formula
Example 1:
What is the percentage composition of potassium dichromate?
Example 2:
Determine the percentage composition of copper (II) sulfate pentahydrate.

26. Empirical Formula
Molecular Formula CH
C2H2 or C3H3 or C6H6
C6H12O6

27. Example 3.
A sample of an unknown compound with a mass of g was analyzed and found to contain g of carbon and 1.469g of oxygen. What is the empirical formula of this compound?

28. Example 4.
A white powder used in paints, enamels and ceramics had the following composition: % Ba, 6.090% C, and 24.32% O. Determine the empirical formula.

29. Example 5
An oxide of phosphorus is 43.7% phosphorus and has a molecular weight of 284 g/mol. Determine the molecular formula for this compound.

30. Combustion Analysis
Combustion Analysis is used to determine the empirical/molecular formula for hydrocarbons. (CxHy) CxHy + O2 → CO2 + H2O CxHyOz + O2 → CO2 + H2O The formula of the hydrocarbon can be assayed when considering the amounts of carbon dioxide and water collected from the combustion.

31. Example 1:
A compound contains only carbon and hydrogen. A 1.45g sample is burned and produces 2.25g of water and 4.40g of carbon dioxide. Determine the empirical formula for the hydrocarbon.

32. Example 2:
5.00g of an oxygen containing hydrocarbon is combusted to yield 9.57g carbon dioxide and 5.87g water. What is the empirical formula?

33. Composition vs. Reaction Stoichiometry
Composition deals with—
Reaction deals with--

34. Reaction Stoichiometry
Balancing Equations: Ex. 1: (NH4)2Cr2O7 (s)  Cr2O3 (s) + N2 (g) + H2O (l) Ex. 2: H2O (l)  Ex. 3: CaCl2 (aq) + Na3PO4 (aq)  Ex. 4: C3H8 (g) + O2 

35. Ex. 1. What mass of potassium iodide is necessary to completely react with g of lead (II) nitrate in a double replacement reaction?

36. Ex. 2. What mass of solution that is 22
Ex. 2. What mass of solution that is 22.5% potassium iodide is needed to completely precipitate 0.28 g of lead (II) iodide?

37. Ex. 3. In an experiment performed in the classroom, a student collects 12.7 L of ammonia from the reaction of 9.0 g of nitrogen with excess hydrogen. What is the percent yield?

38. Yield
Theoretical Yield:
Percent Yield:

39. Make it Real
Limiting Reactant: Excess Reactant:

40. Ex. 4: Consider the synthesis of Zinc and sulfur If 25
Ex. 4: Consider the synthesis of Zinc and sulfur If 25.0g of zinc and 30.0 g of sulfur are mixed, How many grams of zinc sulfide could be produced? How many grams of excess reactant should remain after the reaction is over?

41. Ex. 5: In a reaction between 38. 0g of chromium (III) oxide and 9
Ex. 5: In a reaction between 38.0g of chromium (III) oxide and 9.00 g of aluminum metal, 15.2 g of chromium metal were collected along with an unmeasured amount of aluminum oxide. What was the percent yield for this experiment?