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Physical Science Final Exam Study Guide

I. Chemistry 1. What is the difference between a homogeneous mixture and a heterogeneous mixture? 2. List 2 examples of a homogeneous mixture and 2 examples of heterogenous mixtures. 3. List 2 examples of a pure substance and 2 examples of a mixture. 4. Where are metals, nonmetals, and metalloids located on the periodic table? Be specific! 5. List 2 formulas for an element and 2 formulas for a compound. 6. Compare these phases:

Particle attraction? (how tightly are their molecules packed?)

Particle motion? (How do they move/how much do they move within the substance?)

Explain the gain or loss of heat when going to next phase…

So, what does this gain or loss of heat do to the attraction of the particles?

Solid

Liquid

Gas

7. Phase changes: Please complete this table:

Phase change? (solid to liquid to gas, etc.)

Is energy taken in (endothermic) or released (exothermic)?

Melting

Vaporization

Condensation

Freezing

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8. Compare evaporation, vaporization, and boiling. Watch this Youtube video: http://www.youtube.com/watch?v=9KjMe92gr-o

See this table to help with your comparison

Vaporization Boiling Evaporation

This is the only one that is an ACTUAL phase change

Energy is NOT involved with this process.

This is not technically a phase change, but it is when a liquid changes to a gas due to changes in pressure.

This is when the particles on a surface are exposed to wind and a liquid changes into a gas below its “boiling point”

This is the phase change of a liquid turning to a gas.

9. Compare the formation of a solution and the formation of a compound. Which is a chemical process and

which is a physical process? 10. A solution forms due to forces of (CHOOSE ONE) (gravity, attraction, or energy) between the two types

of particles that make up solutions. These two types of particles are (CHOOSE TWO) (protons, neutrons, solutes, solvents).

11. A material is ___________________________ due to the LACK of ATTRACTION between particles.

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12. Please answer the following questions based on this solubility curve:

a. Which is more soluble, NaNO3 or KCl? b. How does the line drawn for a particular substance relate to the saturation of a solution of that

substance? c. How many grams of NH4Cl will dissolve in 100 grams of 90°C Water? d. How many grams of NH4Cl will dissolve in 50 grams of 90°C water? e. How many grams of KClO3 will dissolve in 300 grams of 30°C water? f. How would you make a saturated solution of KNO3 at 60°C in 50 grams of water? g. If I asked you to make a saturated solution of KCl in 100 grams of water, what other piece of information

would you need before you could start?

13. Complete this table:

Cannot hold any more solute in that given solvent at that given temperature.

Holds more solute than that solvent can usually hold at that temperature.

Holds less solute than that solvent can hold at that particular temperature.

Saturated

Unsaturated

Supersaturated

Dilute

Concentrated

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14. Explain how you could separate a mixture using solubility, density, boiling point, and magnetic properties.

15. Please complete this table:

Metal Nonmetal Metalloid Definition, if necessary

State of matter at room temperature

Density (high or low)

Melting points are normally…

Boiling points are normally…

Lustrous?

Conductive?

Ductile?

Malleable?

Color?

Reactivity?

16. Compare some physical and chemical properties of:

Physical properties Chemical Properties

Salt

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Sugar

Baking soda

Corn starch

Rubbing alcohol

Water

17. Complete this table:

Charge Mass? Location

Proton

Electron

Neutron

18. Compare the number of protons, neutrons, electrons, and mass number in neutral atoms vs. ions 19. Explain how the different mass numbers of isotopes contributes to the average atomic mass for a given

element. 20. Show 3 ways to write the symbol for a carbon isotope that has a mass number of 12. 21. Draw Bohr models of Sodium and Hydrogen. 22. Draw dot diagrams for chlorine, helium, and argon. 23. How many valence electrons do the following atoms have? Be, K, B, Si, As, Te, I, Kr 24. What are these atoms’ oxidation numbers? 25. Why are tin and lead sometimes written Sn (II) and Pb (III) or Pb (II) (having Roman Numerals beside

them)? 26. Which group contains the most reactive metals and which one is the most reactive? 27. Which group contains the most reactive nonmetals and which one in the most reactive? 28. Complete this table:

Their Electrons are (shared/transferred, etc.)

Formed between which type of atoms? (metals, nonmetals, etc.)

NaCl CO2 KBr

Ionic

Covalent

Metallic

29. Write the formulas or the names for the following compounds. Make sure you follow the correct rules for ionic vs. covalent (molecular) compounds.

sodium hydroxide

P4S5

lithium oxide

Si2Br6

iron (III) phosphide

B2Si

chlorine dioxide

MgBr2

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dinitrogen trioxide

Zn(OH)2

iodine pentafluoride

PbO

30. Please BALANCE and CLASSIFY these reactions:

1. 2 K + 2 H2O -----> 2 KOH + H2

2. HCl + NaOH ----> H2O + NaCl

3. KNO3 ----> KNO2 + O2

4. 2 C2H2 + 5 O2 -----> 4 CO2 + 2 H2O

5. C4H8 + 6 O2 ----> 4 CO2 + 4 H2O

6. Hg + O2 ----> HgO

31. How does the Law of Conservation of Matter relate to balancing chemical equations?

32. Match these acids and bases with their formulas:

Calcium Hydroxide

Barium Hydroxide

Sodium bicarbonate

Hydrochloric acid

Nitric Acid

Magnesium Hydroxide

HCl

H2SO4

C2H4O2

HNO3

C6H8O7

NaHCO3

NaOH

KOH

Ca(OH)2

Mg(OH)2

Ba(OH)2

NH4OH

Sodium Hydroxide

Ammonium Hydroxide

Acetic Acid Potassium Hydroxide

Sulfuric Acid

Citric Acid

HCl

H2SO4

C2H4O2

HNO3

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C6H8O7

NaHCO3

NaOH

KOH

Ca(OH)2

Mg(OH)2

Ba(OH)2

NH4OH

35. Arrhenius theory of acids and bases:

Acids Bases Neutral

Produce more OH- ions in solution than H+

Produce more H+ ions in solution than OH- ions

Produce equal amounts of H+ ions and OH- ions in solution

pH below 7

pH above 7

pH equal to 7

Reactive with metals

Reactive with fats/oils

36. What is a neutralization reaction? 37. Which 2 things are formed in a neutralization reaction?

38. Complete the table below with the correct information about each type of radioactive emission.

Charge Atomic Symbol

Can be stopped

by

Mass (large/small)?

This decay Increases the

atomic number by 1

This decay reduces the mass of an atom by 4 and the atomic number by 2

These are Electromagnetic Waves released

from the nucleus with an

alpha or beta particle.

Alpha

Beta

Gamma

39. Complete the following nuclear reactions:

a. 6027Co 0-1e + _____ Radiation type ____________

b. 211___Fr _____ + 207

85_____ Radiation type_________

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c. 8235____ _____ + ___

___Kr Radiation type ____________

40. Complete this table using the concepts you have learned about Fission and Fusion:

Fission Fusion

two or more nuclei join together to form a more-massive nucleus

Uranium

large nucleus splits into two smaller nuclei

energy is released

Chernobyl

not currently used to provide

electrical energy

no radioactive waste products

occurs in the sun’s core

radioactive waste products

requires temperatures over 100,000,000_C

fuels 20 percent of the electrical energy used in the United States

not currently used to provide

electrical energy

41. Complete these half-life problems:

II. Physics 42. Draw and label a diagram which shows the difference between distance and displacement.

43. Which is a scalar quantity and which is a vector quantity:

Scalar quantity V ector quantity

Speed

Velocity

Distance

Displacement

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44. The symbol for velocity is _________________ The symbol for time is ______________

The symbol for distance is _______________ The equation for velocity is __________________

The unit for velocity is ________________ The unit for time is _____________________

The unit for distance is ___________________

45. Please calculate the answers to these problems:

1

2

3

4

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46. Momentum problems: 1. Calculate the momentum of a 0.15 kg ball that is moving toward home plate at a velocity of 40m/s. 2. Which has greater momentum, a 2.0kg hockey puck moving east at 2.5m/s or a 1.3kg hockey puck moving south at 3.0m/s?

47. How do you determine the weight of an object? 48. A small rocket weighs 14.7 N. What is the mass? 49. A net force of 25 N is applied to a 10 kg mass. What is the acceleration given to the mass? 50. How is air resistance related to terminal velocity? 51. Define friction. 52. Give examples of static, sliding, rolling, and fluid friction. 53. What is inertia and how is it related to mass? Think of Newton’s first Law! 54. Draw 1 diagram to show balanced forces and another diagram to show unbalanced forces. 55. Think about the relationship between force, mass, and acceleration to answer these:

a. The greater the force on an object, the greater its change in (acceleration/ motion/mass) (choose one) b. The same amount of force applied to an object with less mass results in greater (acceleration/

motion/mass) (choose one) 56. State Newton’s 2nd Law and give 2 examples. 57. State Newton’s 3rd Law and give 2 examples. 58. Compare thermal energy, heat, and temperature:

Temperature Thermal Energy Heat

TOTAL energy of all of the particles of an object – this includes mass and kinetic energy.

Thermal energy moving from a warmer object to a cooler object

A measure of the average kinetic energy of an object.

59. Compare conduction, convection, and radiation as methods of energy transfer:

Conduction Convection radiation

Involves waves

Involves currents

Involves direct contact

A metal spoon in a pot of soup.

Boiling water

A toaster toasting bread.

60. How are kinetic energy and potential energy related on a roller coaster’s top of the first hill and bottom of the

first hill? 61. Work requires ____________________. 62. When work is done on an object , the result is an increase in its _____________________ and is accompanied by

a decrease in energy somewhere else. 63. What is the equation for calculating the amount of work done on an object? 64. How are power and work related? (give the equation for calculating power)

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65. The 2 simple machines that are a modified version of the inclined plane are ______________________ and _______________________. 66. Which 2 simple machines are variations of a lever? 67. If work input is not equal to work output for a machine, how does the Law of Conservation of Energy explain this

“lost” energy? 68. Why is no machine 100 % efficient, or greater than 100 % efficient? 69. Give the formula for calculating efficiency of a machine. 70. Calculate the efficiency of a machine that places the caps on plastic soda bottles requires 25 kJ of input work.

The output work of the machine is 23 kJ. 71. Determine the ideal and actual mechanical advantage for the following machine: A lever has an effort arm

with a length of 2 m and a resistance arm with a length of 0.5 m. When 900 N of force are applied to the lever, a 1750-N load is raised 0.3 m.

72. Draw and label a longitudinal (compressional) wave with the parts: amplitude, rarefaction, compression, and wavelength.

73. What is the equation for calculating wave problems involving velocity, frequency, and wavelength. 74. How is energy related to the amplitude of a wave? 75. Draw and label a transverse wave with its parts: crest, trough, amplitude, and wavelength 76. How do transverse and longitudinal waves move particles as related to wave direction? 77. Please complete this table comparing wave behaviors:

Reflection Refraction Diffraction

Being able to hear around a corner is due to this wave behavior

SONAR is due to this wave behavior

Things can look bigger, bent, or broken in water

RADAR is due to this wave behavior

78. Opposite charges (attract/repel) and like charges (attract/repel) (choose one in each set of parenthesis) 79. Please complete this table regarding methods of charging objects:

Conduction Friction Induction

Transferred from rubbing

the force field of a highly negatively charged object pushes the electrons away from nearby objects causing them to become + charged

transferred by direct contact w/ another object

Hair standing on end w/ Van de Graff machine

statically charged balloon attracts small pieces of torn up paper

Getting shocked from walking on the carpet

80. Draw both a series and a parallel circuit diagram with resistors and batteries. Please label the parts of the

diagrams

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81. Show the difference between an open circuit and a closed circuit by drawing a simple diagram. Please label which is open and which is closed.

82. List Ohm’s law equation and the Power equation. Explain what each of the letters represent. 83. Explain the difference between a series and a parallel circuit. 84. Explain how the flow of electricity through series and parallel circuits is affected by voltage and

resistance….think about the circuits lab…what happened when you added more light bulbs? What would happen if we added more voltage?

85. More current exists in a wire when (resistance/voltage) is low. 86. Explain how changes in composition, length, temperature, and diameter of a wire would affect the current in a

circuit.

87. Complete this table regarding resistance:

Increases resistance Decreases resistance

Increasing the length of a wire

Increasing the temperature

Increasing the diameter of a wire

88. For a magnet to be magnetized, the Magnetic domains must be (random/lined-up) (choose one). 89. How do you demagnetize a magnet? 90. Magnets (repel/attract) because force comes out of (North/South ) Pole and goes into the (North/South) Pole

(choose one from each set of parenthesis) 91. Magnets (repel/attract) (choose one) because the forces are pushing (toward/away) from each other (choose

one from each set of parenthesis) 92. An electric current produces a magnetic field. (True or False) 93. Describe what an Electromagnet is. 94. An electric generator converts (mechanical/electrical) energy into (mechanical/electrical). 95. A motor converts (mechanical/electrical) energy into (mechanical/electrical). 96. Explain how electricity and magnetism are related to ATM or credit cards, speakers, automatic sprinklers, and

traffic signal triggers.

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