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IBC MIDTERM Flashcards

1
Q

science

A

a way of learning about the natural world based on evidence and logic

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2
Q

scientific law

A

the description of an observed phenomenaa

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3
Q

scientific theory

A

a widely accepted broad phenomena that is supported by evidence

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4
Q

chemistry

A

the study of matter and the changes matter undergoes

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5
Q

physical chemistry

A

how matter behaves, how chemical reactions occur

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6
Q

organic chemistry

A

carbon containing compounds

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7
Q

inorganic chemistry

A

properties and behaviors of non-carbon substances

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8
Q

analytical chemistry

A

identifying composition and structure of matter

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9
Q

biochemistry

A

chemical structures and processes in living organisms

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10
Q

inductive reasoning

A

the process of drawing a general conclusion based on many pieces of evidence

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11
Q

scientific method

A

a logical, systematic approach to the solution of a scientific problem

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12
Q

observation

A

any info gathered by the senses

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13
Q

hypothesis

A

an educated guess that can be tested with observations

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14
Q

experiment

A

a controlled scientific study with specific variables

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15
Q

manipulated variable(independent variable)

A

a variable changed by the researcher

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16
Q

dependent variable

A

a variable the researcher predicts will change

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17
Q

what is the difference between a scientific theory and a scientific law??

A

scientific laws state what always happen, while scientific theories state why things happen

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18
Q

what are the steps of the scientific method and how can you remember them?

A

observation
research
hypothesis
experiment
analyze data
report results

(ORHEAR)

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19
Q

what are the main areas of chemistry?

A

physical, organic, analytical, biochemistry, inorganic

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20
Q

list 5 lab safety rules

A
  1. No food or drink
  2. wear safety goggles when instructed
  3. tie back hair
  4. report any accidents to the teacher
  5. clean area when you are finished
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21
Q

mass

A

measure of the amount of matter in a substance or an object

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22
Q

volume

A

measure of the amount of space a substance or an object takes up

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23
Q

physical property

A

properties that can be measured without changing the substance into an entirely different substance

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24
Q

extensive property

A

properties that depend on the amount of matter present

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25
intensive property
properties that do not depend on the amount of matter present
26
physical change
a change in one or more properties without any change in the chemical properties
27
solid
a state of matter in which particles of matter are tightly packed together
28
liquid
a state of matter in which particles slip past on another and take the shape of their container
29
gas
a state of matter in which particles can pull apart from one another and spread out
30
vapor
a substance that is suspended as a gas
31
states of matter
a physical property of matter. A given kind of matter has the same chemical makeup regardless of state
32
substance
a form of matter that has a specific chemical composition and distinct properties
33
mixture
a physical blend of 2 or more components each of which retains its own identity and properties in the mixture
34
solution
a homogeneous mixture where one substance is dissolved into a different substance
35
homogeneous mixture
a mixture in which the composition is uniform throughout the mixture
36
heterogeneous mixture
a mixture in which the composition is not uniform throughout the mixture
37
phase
a layer in a heterogeneous mixture
38
chromatography
separates 2 substances using a mobile phase and a stationary phase
39
distillation
separates 2 liquids by their differences in boiling points
40
filtration
separation of a mixture's components through difference in particle size
41
element
a pure substance that cannot be broken down into any other substance
42
compound
a pure substance formed when 2+ elements have chemically combined through a chemical reactions to form a new substance
43
molecule
the smallest particle of a compound that still has the compound's properties
44
chemical change
occurs whenever matter changes into an entirely different substance with different chemical properties
45
chemical property
properties that can only be measured or observed when matter undergoes a change to become an entirely different kind of matter
46
chemical symbol
a one or two letter designation of an element
47
flammability
the ability of matter to burn
48
precipitate
a solid that forms and settles out of a liquid mixture
49
product
products produced in a chemical reaction
50
reactant
substances that start a chemical reaction
51
reactivity
the ability of matter to react chemically with other substances
52
list at least 3 chemical properties of matter
reactivity, flammability, and the ability of matter to rust
53
list at least 3 physical properties of matter
color, hardness, state of matter, boiling point, odor
54
explain the difference between intensive and extensive properties
extensive properties depend on the amount of matter present, while intensive properties do not
55
list atleast 4 examples of chemical changes
burning, rusting, milk souring, baking a cake
56
list atleast 4 examples of physical changes
whipping eggs, boiling water, dicing vegetables, folding paper
57
what are the 4 common states of matter
liquid, solid, gas, plasma
58
describe the difference between a homogeneous and a heterogeneous mixture
homogeneous mixtures are evenly mixed and uniform throughout, while heterogeneous mixtures are not
59
list 4 method for separating mixtures
distillation, magnetism, filtration, chromatography
60
name an example of a field of chemistry being used in the real world
analytical chemists made COVID tests
61
explain the difference between an element and a compound
an element is a pure substance represented by a symbol on the periodic table, while a compound is a pure substance made of 2 or more elements that is represented by a formula
62
what is the law of conservation of mass
matter cannot be created or destroyed
63
what are signs of a chemical reaction
change in color or temperature, creation of bubbles, formation of a precipitate or a gas
64
accuracy
how close a measurement comes to an actual value
65
precision
how close a series of measurements come to eachother
66
accepted value
the value that is widely accepted to be correct
67
experimental value
the value that has been measured
67
error
the difference between the experimental value and the accepted value
68
percent error
what percentage your experimental value is different from the accepted value
69
significant figures
a way of making sure measured numbers are not too precise
70
scientific notation
an easier way to look at very large numbers
71
international system of units
the measurement system used by most scientists and engineers
72
English system
measurement system used by americans
73
metric system
measurement system used in science and engineering and by countries other than the United states
74
dimensional analysis
a logical process of converting from one unit to another
75
temperature
the average kinetic energy of the particles in matter
76
Kelvin scale
a temperature scale based on molecular motion
77
celsius scale
temperature scale based on the boiling and freezing point of water
78
absolute zero
the point where all molecular motion stops
79
conversion factor
a fraction made from an equivalency
80
density
the ratio of an object's mass to its volume; the measure of how tightly packed and how heavy the molecules are in an object
81
what is the difference between accuracy and precision
accuracy is how close a measurement comes to an actual value, while precision is how close a series of measurements is to one another
82
what is the equation for percent error
|experiment-accepted|over accepted x 100
83
what are the rules for determining if a zero is a significant number?
1. when the zero is in between nonzero digits 2. at the end of a number that includes a decimal point (not a sig fig if...) before the first nonzero number at the end of a number without a decimal point
84
what are the rules for determining how many sig figs there should be when adding and subtracting
the answer must have the same number of decimal places as the number with the fewest decimal places
85
what are the rules for determining how many significant figures should be in the answer when using multiplication and division
the answer needs to have the same number of sig figs as the number that has the least number of sig figs
86
what is the equation for calculating density?
d=m/v
87
free card :)
:)
88
what is a CER
claim evidence and reasoning

IBC (4 decks)

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