Freshman Science Exam Review

Freshman Science Exam Review

Mrs. Nixon

The review Sheet is for your benefit. You will be allowed to use your journal on the exam, but not your review sheet (hint: Do the review in your journal or prep journal based on review)

CHAPTER 1 - nature of science

·  Science

·  Technology

·  Pseudoscience

·  Scientific method

·  Observation

·  Inference

·  Manipulated (independent) Variable

·  Responding (dependent) variable

·  Controlled variable

·  Constants

·  Scientific theory

·  Scientific law

·  Scientific notation

·  Significant figures

·  Conversion figures

·  Precision

·  Accuracy

·  Dimensional analysis

·  Measurements (logical, performing, estimating)

·  Units of

o  Length

o  Mass

o  Volume

o  Density

·  Graphs

o  Slope

o  Direct proportion

o  Indirect proportion

o  Plot

o  Read and interpretxz007A

Practice (pg. 31, standardized test prep)

CHAPTER 2 – properties of matter

·  Pure substance

·  Solution

·  Element

·  Atom

·  Compound

·  Homogeneous mixture

·  Heterogeneous mixture

·  Suspension

·  Colloid

·  Physical property

·  Physical change

·  Viscosity

·  Conductivity

·  Malleability

·  Melting point

·  Boiling point

·  Filtration

·  Distillation

·  Chemical property

·  Chemical change

·  Flammability

·  Reactivity

·  Precipitate

Practice (pg. 65, standardized test prep)

CHAPTER 3 – states of matter (3.1 and 3.3 only)

·  Solid

·  Liquid

·  Gas

·  Kinetic energy

·  Phase changes

·  Endothermic

·  Exothermic

·  Heat of vaporization

·  Heat of fusion

·  Evaporation

·  Vapor pressure

·  Condensation

·  Sublimation

·  Deposition

Practice (pg.97 (1, 2, 3, 6), standardized test prep)

CHAPTER 4 – atomic structure

·  Proton

·  Electron

·  Neutron

·  Atomic number

·  Atomic mass

·  Mass number

·  Nucleus

·  Isotope

·  Energy levels

·  Electron cloud

·  Electron configuration

·  Orbital

·  Ground state

Practice (pg. 65, standardized test prep)

CHAPTER 5 – periodic table

·  Periodic table

·  Period

·  Group

·  Periodic law

·  Amu

·  Metals

·  Nonmetals

·  Metalloids

·  Transition metals

·  Halogens

·  Noble gases

·  Alkali earth

·  Alkali metals

·  Valence electron

Practice (pg. 153, standardized test prep)

CHAPTER 6 – chemical bonds (6.1, 6.2, 6.3)

·  Electron dot (lewis dot) diagram

·  Ion

·  Anion

·  Cation

·  Chemical bond

·  Ionic bond

·  Chemical formula

·  Covalent bond

·  Molecule

·  Polar covalent bond

·  Nonpolar covalent bond

·  Polyatomic ion

Practice (pg. 189,#1-5, standardized test prep)

CHAPTER 7 – chemical reactions (7.1 and 7.2 only)

·  Reactants

·  Products

·  Chemical equations

·  Coefficients

·  Subscripts

·  Law of conservation of mass

·  Synthesis reaction

·  Decomposition reaction

·  Single replacement reaction

·  Double replacement reaction

·  Combustion reaction

Practice (pg. 225, #1-4, standardized test prep)

CHAPTER 8 – Acids and bases (8.3 and 8.4 only)

·  Acid

·  Base

·  Indicator

·  Neutralization (acid base) Reaction

·  pH

·  buffer

·  electrolyte

Practice (pg. 259, #3-6, standardized test prep)

CHAPTER 10 – nuclear chemistry (10.1, 10.2, and 10.4 only)

·  Radioactivity

·  Nuclear radiation

·  Alpha particles

·  Beta particles

·  Gamma rays

·  Neutron emission

·  Background radiation

·  Half life

·  Fission

·  Fusion

Practice (pg. 321, # 1-6, standardized test prep)

CHAPTER 11 – motion (11.1, 11.2, and 11.3)

·  Frame of reference

·  Distance

·  Displacement

·  Speed

·  Velocity

·  Average speed

·  Acceleration

·  Distance time graphs

·  Speed time graphs

Practice (pg. 353, standardized test prep)

CHAPTER 12 – forces and Motion (12.1, 12.2, 12.3)

·  Force

·  Newton

·  Friction

·  Gravity

·  Newton’s 1st law of motion

·  Newton’s 2nd law of motion

·  Newton’s 3rd law of motion

·  Mass

·  Weight

Practice (pg. 387, standardized test prep)

CHAPTER 15 – energy

·  Energy

·  Kinetic energy

·  Potential energy

·  Law of conservation of energy

·  Mechanical energy

·  Thermal energy

·  Nuclear energy

·  Chemical energy

·  Electromagnetic energy

Practice (pg. 471, standardized test prep)

CHAPTER 16 – thermal energy

·  Heat

·  Temperature

·  Conduction

·  Convection

·  Radiation

·  Insulation

EQUATIONS

D= m/V

F = ma

KE = ½ mv2

GPE = mgh

S= distance/time

Acceleration = speed 2 speed 1 / time 2- time 1

Sample type questions

Safety

1)  List 3 APPROPRIATE lab behaviors.

2)  What does MSDS stand for?

3)  Draw these pieces of lab equipment?

4)  Test Tube / 5)  Test Tube Rack
6)  Test Tube Holder / 7)  Graduated Cylinder

Scientific Method

8)  Are these Observations or Inferences?

The sky is dark and cloudy.______He must be a soccer player. _____

It is going to rain._____ The Dum-Dum sucker is red. ______

He is wearing a blue shirt and yellow tie.____ The liquid is an acid._____

9)  How do you write a hypothesis?

10)  The Independent variable goes on the ___ axis. The Dependent variable goes on the ____ axis.

11)  What is the very first step of the scientific method?

12)  How do you title a graph?

13)  After testing your hypothesis and making observations, may you change your hypothesis and retest it?

14)  What is the last step of the scientific method?

15)  Read the following experiment:

You notice that your neighbor’s tomato plants are twice the size of your family’s. You want to investigate the impact on plant growth of adding various amounts of fertilizer to potted plants. You go buy the supplies—some plants and fertilizer. One plant is given fertilizer, one is not. You believe that if you start fertilizing your tomato plant, then it will grow taller. You record the initial height of each plant, and add fertilizer to one plant. Growth is recorded of each daily. You place two plants of equal size and type in a sunny windowsill and give the plants equal amounts of water – The temperature is kept the same for each plant. The plant given the fertilizer grows to 24 cm, while the other plant grows to 19 cm. As you predicted, the plant given the fertilizer grows taller than the plant without the fertilizer.

What is the….

i)  Control?

ii)  Constants?

iii)  Hypothesis?

iv)  Conclusion?

v)  Independent variable?

vi)  Dependent variable?

Metric System

16)  What is the abbreviation for decimeters? _____ Kilometer? _____ Centimeter? _____

17)  What does “mg” stand for? ____

18)  What does “s” stand for? ______ms? ______

19)  What does “mL” stand for? ______

20)  The standard metric unit for temperature is ______.

21)  The metric unit measured using a stopwatch is the ______.

22)  Bob measured the length of the classroom. The units would be ______.

23)  A graduated cylinder is used to measure ______.

24)  ______is measured using a triple-beam balance.

25)  With a triple beam balance, what is the unit that goes with the measurement number? ______

26)  There are ____ centimeters in one meter.

27)  There are _____ meters in one kilometer.

28)  Every measurement has a number and ______.

29)  Convert these problems into scientific notation:

a)  4978270 = ______

b)  0.000729 = ______

30)  Convert these problems into standard form:

a)  1.01 x 10-6 = ______

b)  31.00 x 104 = ______

31)  How many significant figures are in the following numbers?

a)  7080 = ____ 4.070 = ____ 0.0076 = ____ 80.000 = ____

Graphing

Graph A Graph B

32)  What type of graph is A?

33)  What type of graph is B?

Matter

34)  Solid, liquid, gas, or plasma?

a)  A substance that has a definite volume, but changing (indefinite) shape:

b)  A substance that does NOT have a definite volume nor a definite shape:

c)  A substance that has a definite volume and a definite shape

35)  Fill in the diagram with the processes.

GAS

.

SOLID LIQUID

36)  This phase change diagram is for what substance? ______

37)  What is happening at point 3? ______

38)  What is happening at point 4? ______

39)  According to the diagram below, which beaker contains the densest liquid?

Substance / Melting Point / Boiling Point
A / - 67 C / -10 C
B / 5 C / 234 C
C / 189 C / 191 C

40)  What substance(s) is a gas at 90 C? ______

41)  What substance(s) is a liquid at 186 C? ______

42)  Physical Change or Chemical Change?

i)  Burning wood ______

ii)  Iron rusting ______

iii)  Copper turning green ______

iv)  Ice melting ______

v)  Mashing bananas ______

43)  Two identical graduated cylinders containing different liquids are placed on identical balances. What Conclusion about density can you make based only on what you can observe from the diagram below?

44)  At 25 ºC, water has a density of 1.0 g/mL and vegetable oil has a density of 0.90 g/mL. Substance Z has a density of 0.95 g/mL. Choose which letter best represents Substance Z when it is place in water and oil.

i.  A

ii.  B

iii C

45)  A buckeye has a mass of 17.89 g. When placed in a graduated cylinder with 20.0 mL of water, the water rose to 50.7 mL. What is the density of the buckeye?

46)  A pure diamond has a density of 4.52 g/cm3. Its mass is 7.81g. What is the volume of the diamond?

47)  Matter is defined as anything that…______

Use these words below.

Chemical . Physical / Suspension
Elements Heterogeneous / . / Colloid

48)  Pure substances are either ______or compounds.

49)  In a(an) ______mixture, the parts of a mixture are noticeably different from one another.

50)  If the particles in a mixture, such as fog, scatter light, the mixture is a(an) _____.

51)  A(An) ______change has taken place when the material has changed shape or size, but the composition of the material remains the same.

52)  When the substances in a sample of matter are changing into different or new substances, _____ changes may be observed.

53)  When the parts of a mixture settle into different layers, you have created a(an) ______.

54)  Is this a compound?

Cobalt, Co / sodium, Na
Carbon Dioxide, CO2 / iodine, I

55)  Is this a pure substance?

Elements Compounds / Mixtures

56)  Is this a mixture?

Carbon Dioxide (CO2) Iron (Fe) / Soil

57)  A mixture that appears to contain only one substance (the same throughout) is a(an)

58)  Is this a heterogeneous mixture?

water in a swimming pool / a jar of mixed nuts
sugar water / stainless steel

59)  Is this a physical or chemical change?

water boils at 100 Celsius
an aspirin tablet is crushed
balls of wax form when melted wax is poured into ice water
a gas forms when vinegar and baking soda are mixed

Atoms & The Periodic Table

60)  Which scientist discovered that atoms consist of subatomic, charged particles? ______

61)  Who discovered the nucleus?______

62)  Who thought atoms of a solid were rough and atoms of a liquid were smooth?

63)  Who thought of an atom as a Plum Pudding Model?______

64)  The subatomic particle found in the nucleus and has no charge is…

65)  In order to find the atomic mass of an element, one must add together the number of which 2 subatomic particles?

66)  Elements on the periodic table are arranged according to their ______…

67)  Which element will you find in the 3rd row, 2nd column? ______

68)  How many electrons can the 3rd energy level hold? ______

69)  The number of energy levels an atom has corresponds to the number of…______

70)  Francium and Cesium are both elements in which family of elements? ______

71)  How are elements arranged in the Periodic Table? By increasing ______.

72)  Where is most of the mass of an atom located? ______

73)  What column number are the Halogens? ______

74)  How many families (certain sections we studied) are there in the Periodic Table? ______

75)  How many rows are there in the Periodic Table? ______

76)  What element will you find in row 2, column 14? ______

77)  Which Noble gas is in row 5 of the periodic table? ______

78)  Elements in the middle of the table are the ______.

79)  In a neutral atom, calcium has: How many p? ____n? ____e? ______

80)  In a neutral atom, tin (Sn) has: How many p? ____n? ____e? ______

81)  Draw the Bohr model for each of the following…Draw the Lewis Dot structure, too!

i)  Fluorine Chlorine

ii)  Potassium Magnesium

82)  Describe the characteristics of Noble gases.

83)  What are isotopes?

84)  What is the same between oxygen-17 and oxygen-18? Different?

85)  The charge of an electron is _____

86)  What are valence electrons?

87)  Where would you likely find elements on the periodic table that form negative ions?

88)  How many electrons does an ion of fluorine with a charge of -1 contain? _____

89)  What family are the following elements in?

i)  Chlorine ______

ii)  Calcium ______

iii)  Aluminum ______

90)  How many valence electrons do the following elements contain?

i)  Beryllium ______

ii)  Oxygen ______

iii)  Carbon ______

91)  How many energy levels do the following elements contain?

i)  Lithium ______

ii)  Potassium ______

iii)  Sulfur ______

92)  Ionic or Covalent?

i)  CH4 ______

ii)  NaCl ______

iii)  BaSO4 ______

iv)  electrons are transferred ______

v)  electrons are shared ______

93)  Balance these equations.

i)  ___ Cl2 + ___ NaBr à ___ NaCl + ___Br2

ii)  ___Al2O3 à ___Al + ___O2

iii)  __H2 + ___O2 à ___H2O

94)  An endothermic reaction is one that ______energy, where an exothermic reaction ______energy.

95)  WHY must all chemical reactions be balanced?

96)  Match these to their points.

Neutral Strong acids Strong bases Weak acids Weak bases

97)  Acids taste…______

98)  All acids contain which ion? ______