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Catalyst 1/31/12

Catalyst 1/31/12. Have your Midterm Review Packet out. I’m going around to check that you’ve done it. On your whiteboards, answer the following : An object has a mass of 25 grams and a volume of 10 cm 3 . What is its density? Convert 4, 500 to scientific notation .

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Catalyst 1/31/12

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  1. Catalyst 1/31/12 Have your Midterm Review Packet out. I’m going around to check that you’ve done it. On your whiteboards, answer the following: • An object has a mass of 25 grams and a volume of 10 cm3. What is its density? • Convert 4, 500 to scientific notation. **Calculators available up front.

  2. Agenda • Catalyst (5 minutes) • Announcements (1 minute) • Guided Review (40 minutes)

  3. Announcements • Midterm Study Session today after school. Let me know if you’re coming. • The following people need to finish/make up their benchmark exams: Suheily Christian M. Michelle L. Jonathan Anthony Maverick

  4. First Marking Period Topics: • Matter and Change • Density Calculations • Scientific Notation • Unit Conversions • Isotopes • Second Marking Period Topics: • Periodic Table Organization • Atomic Structure • Electron Configuration • Naming Binary Ionic and Covalent Compounds/Writing Chemical Formulas

  5. Whiteboards Practice • Cap the marker if not in use. • Do not leave anything written on the whiteboard in the end. • Leave the markers on your desk at the end of class. Tape it so it doesn’t roll over. • Cover the calculators when finished. • Everyone must participate. If you don’t know the answer, write “I don’t know,” but I need you to try.

  6. Order of Review • Measurements and Calculations • Atoms: Building Blocks of Matter • Matter and Change *We will not go over Naming Compounds/Chemical Formulas unless you have a specific question.

  7. Measurements and Calculations

  8. Unit Conversions Refer to staircase chart. Remember: Prefixes kilo = 1000 hecto = 100 deka = 10 --(no prefix) = 1 deci = 1/10 centi = 1/100 milli = 1/1000

  9. 1. Write the following measurements in scientific notation. DON’T FORGET YOUR UNITS: • 12,300 cm • 0.000 078 g • 675.0 L • 90,850 kg

  10. 1. Write the following measurements in scientific notation. DON’T FORGET YOUR UNITS: • 12,300 cm = 1.23 x 104 cm • 0.000 078 g = 7.8 x 10-5 g • 675.0 L = 6.750 x 102 L • 90,850 kg = 9.085 x 104 kg

  11. 2. How many significant figures are in each of the measurements above (in #1)?

  12. Rules for Significant Figures (MEMORIZE THESE) • 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. 2000 meters only has one because there is no decimal point in the end.)

  13. 2. How many significant figures are in each of the measurements above (in #1)? • 12,300 cm = 3 sig figs • 0.000 078 g = 2 sig figs • 675.0 L = 4 sig figs • 90,850 kg = 4 sig figs

  14. Rules for Significant Figures (MEMORIZE THESE) • 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. 2000 meters only has one because there is no decimal point in the end.)

  15. 3. Calculate the following: • 9.5 x 105 is divided by 2.25 x 104 • 1.2 x 102 is multiplied by 3.2x103

  16. 3. Calculate the following: • 9.5 x 105 is divided by 2.25 x 104 = 42.22 • 1.2 x 102 is multiplied by 3.2x103 = 384,000

  17. 4. A sample of ethanol weighs 2.45g and has a volume of 3.1mL. Find its density. (Do on whiteboard)

  18. 5. A sample of alcohol has a volume of 6.2mL. If its density is 0.78g/mL, what is the mass of this sample? (Do on whiteboard.)

  19. 6. How does a hypothesis become a theory?

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

  21. 7. Describe what a hypothesis is.

  22. 7. Describe what a hypothesis is. A hypothesis is a testable statement.

  23. 8. How many grams are in 8.29kg? (Do on whiteboard)

  24. 9. Write your answer from #8 in scientific notation.

  25. 9. Write your answer from #8 in scientific notation. 8.29 x 103 g

  26. 10. How many centigrams are there in 54.5 grams? (Do on whiteboard)

  27. Atoms: The Building Blocks of Matter

  28. 1. A = Atomic Number B = Average Atomic Mass C = Element Symbol D = Element Name

  29. 2. Describe the location and electrical charge (positive, negative, or neutral) for each of the 3 subatomic particles in an atom. • Proton__________________________ • Electron_________________________ • Neutron_________________________

  30. 2. Describe the location and electrical charge (positive, negative, or neutral) for each of the 3 subatomic particles in an atom. • Proton = in the nucleus, positive • Electron = around the nucleus, negative • Neutron = in the nucleus, neutral (no charge)

  31. 3. For an atom to be electrically neutral (no charge), it must have the same number of _______________ and ____________________.

  32. 3. For an atom to be electrically neutral (no charge), it must have the same number of protonsand electrons.

  33. 4. An atom has 9 protons and 10 neutrons. What is its: • Atomic Number ______________________ • Element Name _____________________ • Number of electrons _____________________ • Mass Number ___________________________

  34. 4. An atom has 9 protons and 10 neutrons. What is its: • Atomic Number = 9 • Element Name = Flourine • Number of electrons = 9 electrons • Mass Number = 19

  35. 5. Isotopes of an element have the same number of______, but different number of_____.

  36. 5. Isotopes of an element have the same number of protons, but different number of neutrons.

  37. 6. a) How many protons are in each of the following isotopes of Chlorine? • Chlorine-35 _________ Chlorine-37_________ • Chlorine-36 _________

  38. 6. 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

  39. 6. b) How many neutrons are in each of the following isotopes of chlorine? • Chlorine-35 18 neutrons • Chlorine-37 20 neutrons • Chlorine-36 19 neutrons

  40. Remember: # of neutrons = mass # - atomic #

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

  42. 7. The isotopes below are in hyphen notation. Write their nuclear symbols. • Nitrogen-15 ___________ • Carbon-14 ___________ • Iron-59 ___________ (Do on whiteboard)

  43. 8. The diagrams below represent the nucleus of an atom. (P=proton; N=neutron) How do you know they represent the same element? 2p 3n 2p 2n

  44. 8. They have the same number of protons.

  45. 9. Atom X has 10 protons and 11 neutrons. Atom Y has 10 protons and 13 neutrons. Atom X and Y are considered _____________________ because they have the same number of _______________ but different number of ____________________.

  46. 9. Atom X has 10 protons and 11 neutrons. Atom Y has 10 protons and 13 neutrons. Atom X and Y are considered isotopes because they have the same number of protons but different number of neutrons.

  47. Matter and Change

  48. List the major differences between the three states of matter (Think about the distance and motion of their particles): • Solid • Liquid • Gas

  49. List the major differences between the three states of matter (Think about the distance and motion of their particles): • Solid = particles are closely packed together. They vibrate in place. They have a definite shape and volume. • Liquid = particles can move pass each other and are not as close to each other. Liquids take the shape of their containers. • Gas = particles are moving really quickly and are far apart. Gases do not have a definite shape or volume.

  50. 2. What happens to the particles in matter when energy/heat is added?

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