Unit 1 Chapters 1, 2, and 3 Labs for this unit should include: Vernier labs 1 and 2, and possibly the carbonate mixture inquiry lab.

What Is Chemistry? Chemistry is the study of matter and how it changes. Elements: Atoms: Molecules and Compounds:

States of Matter Solid: Liquid: Gas:

Matter

Pure Substnaces Pure substance: Mixture: Heterogeneous: Homogeneous:

Properties of Matter Physical Properties: Chemical Properties:

Intensive Properties: Extensive Properties:

Atomic Theory Subatomic Particles: Electrostatic Forces: Stress the importance of electrostatic forces.

Radioactivity Radio activity: Spontaneous emission of radiation.

The Nuclear Atom Nucleus: Electronic Charge: Atomic Mass: Give charge of electron and proton

Atomic Size: Talk about angstorms and how they relate to meters.

Isotopes Isotope: Average Atomic Mass: show example from chapter notes of average atomic mass of C. Cover mass spectroscopy in advanced lab skills. Show example of average atomic mass problem page 47

Naturally occurring chlorine is 75 Naturally occurring chlorine is 75.78 % 35Cl, which has an atomic mass of 34.969 amu, and 24.22 % 37Cl, which has an atomicmass of 36.966 amu. Calculate the average atomic mass of chlorine. sample exercise 2.4 p 47

The Periodic Table How it’s arranged: go over basic sections of the periodic table.

Law of Definite Proportions

The Law of Multiple Proportions

Ions and Ionic Compounds Cation: Anion:

Common Ions and their charges Group 1: H+, Li+, Na+ Group 2: Be2+, Mg2+, Ca2+ Group 15: N3-, P3-, As3- Group 16: O2-, S2-, Se2- Group 17: F-, Cl-, Br- Transition elements can usually have more than one charge. Example Fe2+ and Fe3+

Transition Metal Ions Most transition metals can have a few different charges. Example: Fe2+, Fe3+ Fe2O3 FeO

Polyatomic Ions Ammonium: NH4+ Nitrite: NO2- Nitrate: NO3- Hydroxide: OH- Hypochlorite: ClO-

Chlorite: ClO2- Chlorate: ClO3- Perchlorate: ClO4- Carbonate: CO32- Sulfite: SO32- Sulfate: SO42- Peroxide: O22- Phosphate: PO43-

Naming Ionic Compounds

Practice NH4Cl Fe(NO3)3 TiBr3 Pb(SO4)2 Chromium (VI) Phosphate Tin (II) Nitrate Cobalt (III) Oxide Chromium (III) Hydroxide

Chromium (III) Sulfite Barium Carbonate Aluminum Hydroxide Copper (I) Sulfide Lead (II) Phosphate Zinc (II) Iodide Chromium (III) Sulfite NH4Br NaClO3 Fe2S3 AgNO3 CuF2 Ni(ClO)3 Ru3(PO4)4

Naming Molecular Compounds

Practice Naming practice worksheets

The Mole

Molar Mass

Percent Mass Show empirical formula example, molecular formula example and give out formula packet

Hydrates good time to do vernier lab 2.

Empirical And Molecular Formula

Chemical Reactions Chemical Equations: Highlight the difference between coefficients and subscripts. Give out a balancing worksheet

C6H12O6(s) + 6 O2(g)  6 CO2(g) + 6 H2O(l) Stoichiometry How many grams of water are produced in the combustion of 1.00 g of glucose? C6H12O6(s) + 6 O2(g)  6 CO2(g) + 6 H2O(l) Have a bunch of stoichiometry practice ready!

Limiting Reactants Use bread and cheese example.

Consider the reaction that occurs in a fuel cell: 2 H2(g) + O2(g)  2 H2O(g) Suppose the fuel cell is set up with 150 g of hydrogen and 1500 g of oxygen. How many grams of water can be formed?

Theoretical Yield and Percent Yield show 3.14 on page 105

6 C6H12(l) + 5 O2(g)  2 H2C6H8O4(l) + 2 H2O(g) Adipic acid (H2C6H8O4) is used to produce nylon. The acid is made commercially by a controlled reaction between cyclohexane (C6H12) and O2: 6 C6H12(l) + 5 O2(g)  2 H2C6H8O4(l) + 2 H2O(g) a.) Assume that you carry out this reaction starting with 25.0 g of cyclohexane and that cyclohexane is the limiting reactant. What is the theoretical yeild of adipic acid? b.) If you obtain 33.5 g of adipic acid from your reaction, what is the percent yeild?

Example AP Questions Complete combustion of a sample of a hydrocarbon in excess oxygen produces equimolar quantities of carbon dioxide and water. Which of the following could be the molecular formula of the compound? C2H2 C2H6 C4H8 C6H6

The mass percent of carbon in pure glucose, C6H12O6, is 40. 0% The mass percent of carbon in pure glucose, C6H12O6, is 40.0%. A chemist analyzes an impure sample of glucose and determines that the mass percent of carbon is 38.2 %. Which of the following impurities could account for the low mass percent of carbon in the sample? Water, H2O Ribose, C5H10O5 Fructose, C6H12O6. An isomer of glucose Sucrose, C12H22O11

How many protons, neutrons, and electrons are in a 5626Fe atom? Protons Neutrons Electrons 26 30 26 26 56 26 30 26 30 56 26 26 56 82 56

Atoms of Mg combine with atoms of F to from a compound Atoms of Mg combine with atoms of F to from a compound. Atoms of which of the following elements combine with atoms of F in the same ratio? Li Ba Al Cl Ne

C3H8(g) + 5 O2(g)  3 CO3(g) + 4 H2O(l) In the reaction represented above, what is the total number of moles of reactants consumed when 1.00 mole of CO2(g) is produced? 0.33 mol 1.33 mol 1.50 mol 2.00 mol 6.00 mol

LiHCO3(aq) + H2SO4(aq)  Li2SO4(aq) + H2O(l) + CO2(g) When the equation above is balanced and the coefficients are reduced to lowest whole-number terms, what is the coefficient of H2O 1 2 3 4 5

When a 3. 22 g sample of an unknown hydrate of sodium sulfate, Na2SO4 When a 3.22 g sample of an unknown hydrate of sodium sulfate, Na2SO4 * x H2O(s) is heated, H2O (molar mass 18) is driven off. The mass of the anhydrous Na2SO4(s) (molar mass 142 g) that remains is 1.42 g. The value of x in the hydrate is 0.013 1.8 6.0 10.0 20.0

What is the empirical formula of an oxide of chromium that is 48 percent oxygen by mass? CrO CrO2 CrO3 Cr2O Cr2O3