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Science > Semester 1 Study Guide > Flashcards

Semester 1 Study Guide Flashcards

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1
Q

Scientific Method

A

a sequence of events used to test a question

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2
Q

Hypothesis

A

an explanation of how something happens

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3
Q

Independent Variable

A

a factor that changes in an experiment

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4
Q

Dependent Variable

A

a factor that changes as a result of the IV changing

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5
Q

Constant

A

a factor the remains the same in an experiment

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6
Q

Control Group

A

an unchanged experiment that is used to compare to other experiments

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7
Q

Bar/column graph is used for ________

A

comparing data

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8
Q

Line graph is used for _________

A

data over time

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9
Q

Pie chart is used for ___________

A

comparing data that is part of a whole

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10
Q

What are the three types of models?

A
  1. physical
  2. mathematical
  3. conceptual
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11
Q

Identify the benefits and limitations of models.

A

benefits: can model things that don’t exists; can be kind of like a hypothesis
limitations: don’t act like what it models

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12
Q

Length (and tool)

A

measures how long something is

ruler

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13
Q

Mass (and tool)

A

measures how heavy something is

triple beam balance

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14
Q

Volume (and tool)

A

measures the amount of space something takes up

graduated cylinder

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15
Q

Temperature (and tool)

A

measures how hot or cold something is

thermometer

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16
Q

Density (and tool)

A

measures how dense something is (hydrometer)

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17
Q

Matter

A

anything that is a solid, liquid, or gas and takes up space

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18
Q

Physical Changes

A

a change of matter from one form to another without a change in chemical properties

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19
Q

Chemical Changes

A

a change in matter that turns into a different substance

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20
Q

Characteristic Properties

A

properties most useful in identifying a substance

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21
Q

Reactivity

A

how two or more substances combine to create one or more new substances

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22
Q

Thermal Conductivity

A

the rate at which a substance transfers heat

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23
Q

Explain the rule used to decide what is or is not matter.

A

It has to be a sold, liquid, or gas and it has to be made of atoms

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24
Q

Explain the molecular difference between the three states of matter.

A

solids - the atoms are very close together and retains its shape
liquids - the atoms are moderately spaced and it takes the form of its container
gas - the atoms are far apart and are moving quickly and will take the shape of its container

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25
Q

Discuss why the mercury in a thermometer rises when heated.

A

The molecules expand which also expands the actual mercury.

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26
Q

Contrast chemical and physical changes.

A

chemical - a change that affects the object on a chemical level and sometimes changes the substance
physical - a change that affects the object on a physical level and sometimes changes the object’s appearance

27
Q

Tell why scientists use characteristic properties to identify substances.

A

because they are the same for each substance;

ex: a large chunk of iron has the same characteristic properties as a tiny piece of iron

28
Q

Be able to analyze and interpret data on the properties of substances before and after the substances interact to determine if a chemical reaction has occurred.

A

PRACTICE!

29
Q

Atom

A

smallest unit of matter; made up of proton, neutrons, and electrons

30
Q

Isotopes

A

an atom with a different amount of neutrons than normal

31
Q

Atomic Number

A

the number of protons in an atom

32
Q

Atomic Mass

A

the number of both protons and neutrons

33
Q

Ions

A

an atom with a different amount of protons or electrons than normal

34
Q

Ionic Board

A

M to NM / a bond in which atoms transfer electrons

35
Q

Covalent Bond

A

NM to NM / a bond in which atoms share electrons

36
Q

Reactants

A

participants in a chemical reaction

37
Q

Products

A

created in a chemical reaction

38
Q

Law of Conservation of Mass

A

states that mass is neither created nor destroyed

39
Q

List 5 things that describe an atom.

A
  1. composed of protons, neutrons, and electrons
  2. always moving
  3. mostly empty space
  4. very small
  5. has mass
40
Q

How can you use the periodic table to identify protons, neutrons, and electrons in an atom?

A 
P = Atomic Number
E = Same as P
Neutron = Atomic Mass-Atomic Number
41
Q

Discuss the rules for creating isotopes.

A 
isotopes = uneven amount of neutrons
ions = uneven amount of protons and electrons
42
Q

How can you use the periodic table to determine the number of electron shells and valence electrons for atoms?

A

groups and periods:
periods = vertical
groups = horizontal

43
Q

Contrast an ionic bond with a covalent bond. Determine if a molecule/compound is formed by an ionic or covalent bond.

A 
ionic = electrons giving to another atom
covalent = electrons being share with another atom
ionic = nonmetal ---> metal
covalent = nonmetal ---> nonmetal
44
Q

Describe the relationship between the reactants and the products in a chemical reaction.

A

You start with reactants. When in contact, the reactants begin reacting to each other. This creates a new substance which is called the product.

45
Q

Explain the law of conservation of mass as demonstrated in your lab experiences.

A

The law of conservation of mass states that mass is neither created nor destroyed in a chemical reaction. For example, if you put two different reactive substances in a bag, weigh them, and get 120 grams. Then you mix them together and weigh them after the reaction, it still weighs 120 grams.

46
Q

Energy

A

the ability to do work

47
Q

Kinetic Energy

A

energy of motion

48
Q

Potential Energy

A

energy an object has due to its position

49
Q

Mechanical Energy

A

the sum of PE and KE

50
Q

Thermal Energy

A

heat energy due to the random motion of particles

51
Q

Chemical Energy

A

energy of a compound that changes as its atoms are rearranged

52
Q

Electrical Energy

A

energy of moving electrons

53
Q

Light Energy

A

energy produced by the vibrations of electrically charged particles

54
Q

Nuclear Energy

A

energy produced from the changes in the nucleus of an atom

55
Q

Energy Conservation

A

the act of changing one type of energy to another

56
Q

Law of Conservation of Energy

A

a law that states that energy cannot be created or destroyed, but can change from one form to another

57
Q

Contrast kinetic and potential energy.

A 
kinetic = energy of movement/highest at high speeds
potential = energy of an object from its position that could become kinetic/highest at high altitudes
58
Q

Identify the factors that affect the amount of potential and kinetic energy.

A 
speed = kinetic
height = potential
friction = reduces both
59
Q

Explain the relationship between kinetic, potential, and mechanical energy.

A

NO ANSWER

60
Q

Describe the energy conversions that take place on a roller coaster, and explain how energy is conserved.

A

potential —> kinetic (going downhill)
kinetic —> potential (going uphill)
electric —> kinetic (turning wheels to move uphill)
The amount of mechanical energy is always the same, never created or destroyed, so energy is conserved.

61
Q

Give three examples of one form of energy being converted into another form.

A

electric —> light (flashlight)
chemical —> kinetic (walking or running)
electric —> sound (radio)

62
Q

Explain the Law of Conservation of Energy.

A

States that energy can neither be created nor destroyed.

Example: 
person going downhill
p=100 k=250 350
person near top of hill
p=300 k=50 350
It stays the same.
63
Q

Open Response/Short Answer
Support a claim, using evidence, that when kinetic energy of an object changes, energy is transferred to or from the object.

A 
**PRACTICE WRITING THIS.**
Three parts:
A - answer the question
B - draw a model and label
C - total amount of energy

Science (3 decks)

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