2. Final Review This is an aid. Not an answer key.

3. Measurement Accuracy Precision What are the rules for reading instruments in the lab? How do you decide the best instrument to use in the lab?

4. Significant Figures What are the rules? 0.5260 5.02 5020 0.00502 500.

5. Significant Figures What are the rules for addition and subtraction? 5.20 + 6.2 = 5.21 – 5.234 = What are the rules for multiplication and division? 5.02 x 5.203 = 5.54 x 5.4/5 =

6. Density D M V ensity ass olume D = MVMV M = D x V V = MDMD

7. lecturePLUS Timberlake6 Density Osmium is a very dense metal. What is its density in g/cm 3 if 50.00 g of the metal occupies a volume of 2.22cm 3 ? The density of octane, a component of gasoline, is 0.702 g/mL. What is the mass, in kg, of 875 mL of octane? D = m/V m = D*V V = m/D

8. Conversions How many micrometers are in 5 meters? How many kilometers are in 4.95 x 10 5 millimeters? How many miles are in 4.95 x 10 5 millimeters? How many liters are in 8.95 ounces? How many pounds are in 9.8 milligrams?

9. Matter What is matter? What kinds of pure substances can you have? Definitions. What kinds of mixtures can you have? Define each.

10. Chemical and Physical Change How do we know something is a chemical change? What are some chemical changes? How do we know something is a physical change? What are some physical changes?

11. Chemical and Physical Properties What is a chemical property? Physical property? –Melting point- length –Corrosive- toxicity –Solubility- mass –Density- Flammability –Boiling point- combustibility

12. Atomic Models Describe the atomic models (experiment, evidence, conclusion). –Dalton –Thompson –Rutherford –Bohr –Quantum theory

13. Atomic Structure What is an isotope? How many protons, neutrons, and electrons? Br 80 35 Carbon- 12 S 32 16

14. Atomic Structure ElementAtomic Mass ProtonsNeutronsElectrons Sodium -2411 Oxygen-181810 Calcium-41412018

15. Nuclear Chemistry (Decay Particles) ParticleSymbolWhat is it?Penetratio n Alpha (  ) Helium nucleus (2 p + ) 0.2 mm (paper) Beta (  ) High Speed e - 100 mm (wood) Gamma (  ) High Energy Electromagnetic Wave 500 mm (concrete)

16. Nuclear Chemistry (Decay Particles)

17. Types of Radioactive Decay  alpha production (  ): helium nucleus  beta production (  ): 2 4 He  1 0 e 2+

18. Half-life Concept http://phet.colorado.edu/en/simulation/radio active-dating-game

19. Fission

20. Fusion

21. Electron Configuration

22. What are the quantum numbers? What is the electron configurations for: –Sodium –Fluorine –Phosphorus –Calcium –Iron –Bromine What are the shorthand configurations?

23. Ionization energy, electronegativity Electron affinity INCREASE

24. Atomic size increases, shielding constant Ionic size increases

25. Periodic Trends Which atom is larger and has the greater electronegativity? –Sodium or chlorine –Magnesium or barium –Oxygen or lithium Which ion is smaller? –Calcium or barium –Magnesium or silicon –Chlorine or silicon

26. Compounds Identify each of the following as ionic or covalent. Write the name of each compound. –NaBrF 3 H 9 –P 3 N 7 Mg 3 P 2 –O 4 Br 6 NaCl –Ca 3 N 2 SrI 2 –B 2 I 8 BaBr 2

27. Two Types of Compounds Smallest piece Melting Point State Types of elements Formula UnitMolecule Metal and Nonmetal Nonmetals solid Solid, liquid or gas High >300ºCLow <300ºC IonicMolecular

28. Naming Compounds Identify each of the following as ionic or covalent. Write the name of each compound. –NaBrF 3 H 9 –P 3 N 7 Mg 3 P 2 –O 4 Br 6 NaCl –Ca 3 N 2 SrI 2 –B 2 I 8 BaBr 2

29. Write the formulas for these Lithium sulfide tin (II) oxide tin (IV) oxide Magnesium fluoride Copper (II) sulfate Iron (III) phosphide gallium nitrate Iron (III) sulfide Identify the cations and anions above.

30. Polar-Covalent bonds Nonpolar-Covalent bonds Covalent Bonds  Electrons are unequally shared  Electronegativity difference between.3 and 1.7  Electrons are equally shared  Electronegativity difference of 0 to 0.3

31. Polarity A molecule, such as HF, that has a center of positive charge and a center of negative charge is said to be polar, or to have a dipole moment. A molecule, such as HF, that has a center of positive charge and a center of negative charge is said to be polar, or to have a dipole moment.

32. Draw Lewis Structures Polar/Non-Polar H 2 O O 2 CH 3 Cl HCl CCl 4 N 2 PH 3

33. Table – VSEPR Structures

34. Calculating Formula Mass Calculate the formula mass of magnesium carbonate, MgCO 3. 24.31 g + 12.01 g + 3(16.00 g) = 84.32 g

35. Calculations with Moles: How many grams of lithium are in 3.50 moles of lithium? 3.50 mol Li = g Li 1 mol Li 6.94 g Li 24.29

36. Calculations with Moles: Converting grams to moles How many moles of lithium are in 18.2 grams of lithium? 18.2 g Li = mol Li 6.94 g Li 1 mol Li 2.62

37. Calculations with Moles: Using Avogadro’s Number How many atoms of lithium are in 3.50 moles of lithium? 3.50 mol Li = atoms Li 1 mol Li 6.022 x 10 23 atoms Li 2.11 x 10 24

38. Calculations with Moles: How many atoms of lithium are in 18.2 g of lithium? 18.2 g Li = atoms Li 1 mol Li6.022 x 10 23 atoms Li 1.58 x 10 24 6.94 g Li1 mol Li (18.2)(6.022 x 10 23 )/6.94

39. Experiments Can you identify the independent, dependent, experimental control, and controlled variables? Can you write a hypothesis? If…(what you do)…then….(what will happen)…., because… (scientific reason). Can you graph data? (titles, units, dependent, independent)