1. Chemistry (5/8) Due Today: Stoichiometry Worksheet Gas Laws Graphs
Objectives:
Complete Stoichiometry Quiz
Interpret and discuss the Gas Laws graphs by answering the questions in your packet.

2. Chemistry (5/9) Due Today: Stoichiometry Worksheet-late
Gas Laws Graphs
Objectives:
Discuss the Gas Laws you read about from the text and applied to graphs.
Discuss Stoichiometry Quiz
Homework:
Study for Stoichiometry Re-Take Quiz

3. Gas Laws Assignment Chapter 14.2 in Text
Graph each set of data using a line graph.
Interpret each graph by answering the questions in the packet.

4. Gas Laws Behavior of a gas when two of the following variables change:
temperature of a gas (oC or K)
pressure of a gas (atm, mmHg, Pa)
volume of a gas ( mL, cm3)
Illustrate in your notes how a sample of gas in a balloon would be affected by a change in each variable above.

5. Gas Laws
Volume vs. Pressure Graph

6. Boyle’s Law
If temperature is held constant, what is the relationship between the volume
and pressure of a gas?
blog.cencophysics.com 

7. Gas Laws
2. Temperature vs. Volume Graph

8. Charles’ Law If pressure is held constant,
what is the relationship between temperature and volume of a gas?

9. Gas Laws
3. Temperature vs. Pressure of a Gas

10. Gay-Lussac’s Law If volume is held constant, what is the
relationship between temperature and
pressure?

11. Combined Gas Law
Establishes a relationship between pressure, volume, and temperature of a gas if the amount of gas is held constant.
P1V1/T1= P2V2/T2

12. Ideal Gas Law
Establishes a relationship between pressure, volume, temperature, and quantity of a gas.
PV=nRT,where P= pressure (atm)
V= volume (Liters)
n= quantity of gas (moles)
R= gas constant: L-atm/mol-K
T= temperature (Kelvin)

13. Chemistry Introduction: Measurement and Scientific Method

14. Measurement and Scientific Method: Precision vs. Accuracy
Label each picture as precise, accurate, both, or neither.

15. Matter and Change

16. Phase Changes and Kinetic Energy

17. Atomic Structure

18. Electromagnetic Spectrum

19. Bohr’s Model of the Atom
The electron cloud consists of energy levels.
Electrons reside and move around in these energy levels.
Electrons can move to other energy levels when absorb photons. 19

20. Electron Movement Ground state of H Atom (lowest energy level for e-)
Ground state of H Atom (lowest energy level for e-)
A photon (light particle) is absorbed by H’s electron.
Electron becomes excited and jumps to higher energy level.
3. E- returns to ground state and emits (releases) the photon.
Emitted photon’s wavelength can be detected by scientists.
(Infrared region at room temp; Visble region at higher temps.)

21. Electron Properties and Arrangement

22. Electron Properties and Arrangement

23. Electron Properties and Arrangement

24. Periodic Table

25. Periodic Table: Atomic Radius

26. Periodic Table: Ionization Energy

27. Chemical Bonding

28. Chemical Reactions

29. Types of Chemical Reactions
1. Synthesis (A+ B ----> AB)
2. Decomposition (AB------> A + B)
3. Single Replacement (A+ BC ---> B + AC)
4. Double Replacement (AB + CD ---> CB + AD)
5. Combustion (CxHx + O > CO2 + H2O)
6. Neutralization (Acid + Base--> H2O + Salt)

30. Chemical Reaction Energy Diagram: Exothermic

31. Chemical Reaction Energy Diagram Endothermic

32. Chemical Reactions Rates
Reaction Rates = how fast the reactants chemically change into the products.
Collision Theory: Reactant particles will form products when reactants collide:
at the right position.
and exchange the right amount of kinetic energy.

33. Nuclear Chemistry

34. Nuclear Band of Stability
*Big Misconception: Stable nucleus means equal number of protons and neutrons. From
graph, students confirmed that most elements with a stable nucleus needs more neutrons to minimize the repulsion force between protons with a similar charge.

35. Nuclear Chemistry: Radioactive Decay

36. Chemical Quantities

37. Stoichiometry

38. What does Chemistry study?
Chemistry Final
What does Chemistry study?

39. Convert to scientific notation: 2,350,921

40. Scientific Notation
Convert to scientific notation .

41. Metric Conversion Kilo-, Hecto-, Deka-, Base, Deci- Centi-, Milli-
5 kg = ________cg

42. Metric Conversion Kilo-, Hecto-, Deka-, Base, Deci- Centi-, Milli-
3.5cL= ______ L

43. Metric and English Conversions
How many seconds is in hrs?

44. Metric and English Conversions
Sara ran 2 miles in 16 minutes. How far did she run in kilometers? (1mi= 1600m)

45. Density
What is the equation for density?

46. Density
A solution has a mass of 1200 g and a density of 1.2 g/mL. What is the volume?

47. Density
What is the density of a 50mL sample of water that has a mass of 49.6 g?

48. Scientific Method
What are the 5 main steps to the scientific method?

49. Scientific Method
What is the difference between qualitative and quantitative results?

50. Scientific Method
What is the difference between accuracy and precision?

51. Scientific Method
Determine which of the following sets of data is most precise.
2.5, 6.0, 4.0
2.5, 3.0, 2.0
2.5, 2.4, 2.3

52. Scientific Method
A student wanted to know how temperature affected the rate of a chemical reaction. She observed and recorded the time it took for a chemical reaction to occur at three different temperatures.
What is the independent variable?
What is the dependent variable?

53. Significant Figures
How many significant figures?
g ________

54. Significant Figures
How many signficant figures?
2.104_______

55. Calculating using Significant Figures
How many significant figures are in the answer?
1.21 g x 0.50g =

56. Calculating using Signficant Figures
How many significant figures are in the answer?
0.45m m g+ 4g =

57. Matter
What are the two broad classes of matter?

58. Classification of Matter58

59. Matter
What is the big difference between substances and mixtures?

60. Mixtures
Determine if the following mixtures are heterogenous or homogenous mixtures.
Saltwater
b. Vegetable soup

61. Compounds True or False: Compounds composition is always varied.
True or False: A compound’s properties are similar to the elements making up the compound.

62. Physical Properties
Give me example of physical properties.

63. Chemical properties
Give me example of chemical properties.

64. Physical or Chemical Change
Determine if the following are chemical or physical changes
Boiling water
b. Digesting food
Burning fire wood
d. Dissolving sugar in water

65. Mixture or Compound?
air
Na(OH)
lead
Na(OH)solution

66. Atomic Theory
Who believed matter consisted of air, wind, fire, and earth?
Who was the first to propose that matter is composed of atoms?

67. Atomic Theory
Who was the first person to confirm using the scientific method that matter was composed of atoms?

68. Dalton’s Atomic Theory
Identify important concepts of Dalton’s Atomic Theory.

69. The Atom
What are the two subatomic particles that have charge?

70. The Atom
What are the two subatomic particles that contribute mass to an atom?

71. The Atom
What is the difference between mass number and atomic mass?

72. Atomic Subparticles
Nitrogen is a neutral atom. It has 7neutrons and 7 electrons.
What is Nitrogen’s number of protons?
What is Nitrogen’s atomic number?
What is Nitrogen’s mass number?

73. Atomic Subparticles
Ca 2+ has a mass number of 40 and an atomic number of 20.
How may protons does Ca 2+ have?
How many electrons does Ca 2+ have?
How many neutrons does Ca 2+ have?

74. The Atom
What is an isotope?

75. Bell Ringer How many significant figures? 0.040020____ 1.0200_____
10,840______
24.09/ 4.2______
= ______

76. Isotope C-12 and C-13 are isotopes.
What subatomic particle has the same value with each isotope of carbon above?
What subatomic particle has different values with each isotope of carbon above?

77. Radioisotope What is a radioisotope?
What are the three types of radioisotope particles we talked about?

78. Nuclear Radiation Radiation charges Radiation Penetration paper wood
concrete or lead

79. Alpha Particles Alpha rays(α) = Emission of a He nucleus.
alpha particles are (+) charged .
large mass and charge prevents alpha particles from traveling and penetrating far. 1.
parent decays α daughter isotope
isotope particle (stable)
(unstable) (He nucleus)

80. Nuclear Decay with α Particles
Mass number decreases by four
Atomic Number decreases by two
(Daughter isotope that is more stable)

81. Nuclear Decay: Beta Particles
Beta Rays (β) = A neutron breaks into a p+ and e-
p+ remains in nucleus and e- is emitted.
Beta rays have a (-) charge.
Beta rays travel and penetrate farther because smaller charge and no mass. 81

82. Nuclear Decay with β particles
Mass number remains the same
(proton switches with a neutron)
Atomic number increases by one.
(proton formed in nucleus; stable daughter isotope).

83. Nuclear Decay: Gamma +ϒ
Gamma Rays(ϒ) = high energy particle with no mass or charge.
Does not have a charge or mass, therefore travels and penetrates the farthest.
Most dangerous rays because penetrates skin.
Usually emitted with alpha and beta particles. +ϒ
parent decays α daughter isotope + ϒ
isotope particle (stable)
(unstable) (He nucleus)

84. Nuclear Decay with ϒ rays
Mass number remains the same
(ϒ rays has no mass)
Atomic number remains the same
(ϒ rays has no mass or charge)

85. Periodic Table
Who organized the periodic table based on atomic mass?

86. Periodic Table
Who organized the periodic table based on atomic number?

87. Periodic Table
How is the modern periodic table
Organized?

88. Periodic Table
What is another name for rows on the periodic table?

89. Periodic Table
What is another name for the columns on the periodic table?

90. Periodic Table
Give me an example of a metal, non-metal, and a metalloid

91. Periodic Table
What is the difference between transitional and representative groups?