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UNIT #1

Have your notes ready. Begin working on the review packet. You will have 10 minutes to complete each unit. Use your time wisely. UNIT #1. MATTER AND CHANGE. 1. List the major differences between the three states of matter (Think about the distance and motion of their particles):.

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UNIT #1

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  1. Have your notes ready. Begin working on the review packet. You will have 10 minutes to complete each unit. Use your time wisely.

  2. UNIT #1 MATTER AND CHANGE

  3. 1. List the major differences between the three states of matter (Think about the distance and motion of their particles): • Solid: the particles are tightly packed together. Solids have a definite shape and volume. • Liquid: the particles can easily pass each other. Liquids have a definite volume, but take the shape of its container. • Gas: the particles are really far from each other and move quickly. Gases do not have a definite volume or shape.

  4. 2. What happens to the particles in matter when energy/heat is added? Particles move more quickly when you add more heat/energy.

  5. 3. Based on their location on the Periodic Table, how do you know that Lithium (Li), Sodium (Na), and Potassium (K) have similar properties? • Lithium, Sodium, and Potassium have similar chemical properties because they are all in the same group and elements in the same group share similar chemical properties.

  6. 4. Label the following elements as metal, nonmetal, or metalloid: • Nitrogen (N)- nonmetal • Boron (B)- metalloid • Calcium (Ca)- metal

  7. 5. Which of the elements in #4 would be: • A good conductor of heat/electricity? Calcium • A semiconductor of heat/electricity? Boron • A poor conductor of heat/electricity? Nitrogen

  8. 6. List 3 differences between metals and nonmetals

  9. 7. Classify the following changes as chemical or physical. • Burning paper CHEMICAL • Tearing paper PHYSICAL • Baking soda and vinegar fizz up when they are reacted CHEMICAL • Ice melting PHYSICAL A physical change does NOT change a substance’s chemical identity. A chemical change changes a substance’s chemical identity.

  10. 8. Explain the difference between a mixture and a pure substance.

  11. 9. Identify the following as a homogenous mixture, heterogenous mixture, or pure substance. • Water (PURE SUBSTANCE because it is a compound by itself) • glucose (sugar) (PURE SUBSTANCE because it is a compound by itself) • a cupcake with sprinkles on top (HETEROGENOUS MIXTURE because it is not the same throughout) • KoolAid (HOMOGENOUS MIXTURE because it is the same throughout) • Magnesium (PURE SUBSTANCE because it is a compound by itself)

  12. Heterogenous Mixture

  13. 10. Which of the following can you break down chemically? • Mercury • Thallium • Sodium hydroxide • Argon Sodium hydroxide is a compound and therefore can be broken down chemically.

  14. UNIT# 2 UNITS AND MEASUREMENT

  15. 1. Write the following measurements in scientific notation: a. 12,300 cm: 1.23 x 104 cm b. 0.000 078 g: 7.8 x 10-5 g c. 675.0 L: 6.750 x 102 L

  16. 2. How many significant figures are in each of the measurements above? a. 12,300 cm 3 significant figures b. 0.000 078 g 2 significant figures c. 675.0 L 4 significant figures

  17. 3. Calculate the following: 4.5 x 105 is divided by 2.25 x 104 = 20 1.2 x 102 is multiplied by 3.2x103 = 384,000 or 3.84 x 105 (Reminder: Don’t forget to use the parentheses if you’re using your calculator.)

  18. 4. A sample of ethanol weighs 2.45 g and has a volume of 3.1mL. Find its density. Density = mass/volume D = m/v m = 2.45 g V = 3.1 mL D = m/v = 2.45 g/3.1 mL = 0.79 g/mL

  19. 5. A sample of ethanol has a volume of 6.2 mL. If its density is 0.78 g/mL, what is the mass of this sample? V = 6.2 mL D = 0.78 g/mL m = V x D m = 6.2 mL x 0.78 g/mL = 4.8 g

  20. 6. How does a hypothesis become a theory? A hypothesis becomes a theory after it is repeatedly supported by experimental data.

  21. How many grams are in 8.29kg? OR

  22. 8. Write your answer from #7 in scientific notation. 8,290 g = 8.29 x 103 g

  23. UNIT 3 Atoms: Building Blocks of Matter

  24. 1. Describe the location, electrical charge, and mass for each of the 3 subatomic particles in an atom. • Proton: nucleus, positive charge, mass = 1 • Electron: in electron clouds around the nucleus, negative charge, mass = 0 • Neutron: nucleus, no charge, mass = 1

  25. 2. For an atom to be electrically neutral, it must have the same number of ___protons____________ and ________electrons_________.

  26. 3. An atom has 8 protons and 7 neutrons. What is its: • Atomic Number: 8 • Element Name: Oxygen • Number of electrons: 8 • Mass Number: 7 neutrons + 8 protons = 15

  27. 4. Isotopes of an element have the same number of _____protons____ but different number of neutrons.

  28. 5. a) How many protons are in each of the following isotopes of Chlorine? • Chlorine-35 ____17__protons___ Chlorine-37______17__protons • Chlorine-36 _____17___protons_

  29. 5. b) How many neutrons are in each of the following isotopes of chlorine? • Chlorine-35: 35 – 17 = 18 • Chlorine-37: 37 – 17 = 20 • Chlorine-36: 36 – 17 = 19 Remember: # of neutrons = mass # - atomic #

  30. 5. c) Circle the isotope with the largest mass number: • Chlorine-35 Chlorine-37 Chlorine-36

  31. 6. The isotopes below are in hyphen notation. Write their nuclear symbols. • Nitrogen-15: 15N 7 • Carbon-14: 14C 6 • Iron-59: 59Fe 26

  32. 7. The diagrams below represent the nucleus of an atom. ( P=proton; N=neutron) How do you know they represent the same element? They represent the same element because they have the same number of protons.

  33. To convert from temperature in Celsius to Kelvin, add 273 and put K or Kelvin as the unit. • 50 degrees Celsius to Kelvin: 50 + 273 = 323 K • 20 degrees Celsius to Kelvin: 20 + 273 = 293 K

  34. An object has a density of 12 g/cm3 and a mass of 6 g. What is its density? • Write down the values that you are given and organize them. • Find out what you need to solve for. • Plug the numbers you know into the equation D = m/V (Density = mass/volume). • Do the math and write your answer using proper units. • D = m/V • M = V x D • V = m/D

  35. Significant Figures Rules • Zeros between nonzero digits are significant. (Example: 50.8 Liters has 3 significant figures) • Zeros in front of all nonzero digits are NOT significant. (Example: 0.00959 grams only has 3 significant figures) • Zeros at the end of a number and to the right of a decimal point are significant. (Example: 8.000 000 000 millimeters have 10 significant figures). • A decimal point after zeros indicates that they are significant. (Example: 2000. meters has four significant figures because of the decimal point explicitly written at the end.)

  36. What is the formula for density?

  37. Density = mass/volume

  38. Drug x has a mass of 100 grams and a volume of 50 cm3. what is its density?(30 seconds)

  39. 2 g/cm3

  40. The density of a substance is 1.97 g/cm3 and you have a 40 cm3 sample. Calculate the mass.(1 minute)

  41. 78.8 grams

  42. Mike has 30 grams of a candy bar with a density of 12.4 grams/cm3. calculate volume.

  43. 2.4 cm3

  44. Write the following in scientific notation96, 000, 000

  45. 9.6 x 107

  46. Write the following in scientific notation90,000 meters(30 seconds)

  47. 9 x 104 meters

  48. Write the following in scientific notation0.00056(30 seconds)

  49. 5.6 x 10-4

  50. Express 12.5kilometers in meters

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