IBC MIDTERM Flashcards
science
a way of learning about the natural world based on evidence and logic
scientific law
the description of an observed phenomenaa
scientific theory
a widely accepted broad phenomena that is supported by evidence
chemistry
the study of matter and the changes matter undergoes
physical chemistry
how matter behaves, how chemical reactions occur
organic chemistry
carbon containing compounds
inorganic chemistry
properties and behaviors of non-carbon substances
analytical chemistry
identifying composition and structure of matter
biochemistry
chemical structures and processes in living organisms
inductive reasoning
the process of drawing a general conclusion based on many pieces of evidence
scientific method
a logical, systematic approach to the solution of a scientific problem
observation
any info gathered by the senses
hypothesis
an educated guess that can be tested with observations
experiment
a controlled scientific study with specific variables
manipulated variable(independent variable)
a variable changed by the researcher
dependent variable
a variable the researcher predicts will change
what is the difference between a scientific theory and a scientific law??
scientific laws state what always happen, while scientific theories state why things happen
what are the steps of the scientific method and how can you remember them?
observation
research
hypothesis
experiment
analyze data
report results
(ORHEAR)
what are the main areas of chemistry?
physical, organic, analytical, biochemistry, inorganic
list 5 lab safety rules
- No food or drink
- wear safety goggles when instructed
- tie back hair
- report any accidents to the teacher
- clean area when you are finished
mass
measure of the amount of matter in a substance or an object
volume
measure of the amount of space a substance or an object takes up
physical property
properties that can be measured without changing the substance into an entirely different substance
extensive property
properties that depend on the amount of matter present
intensive property
properties that do not depend on the amount of matter present
physical change
a change in one or more properties without any change in the chemical properties
solid
a state of matter in which particles of matter are tightly packed together
liquid
a state of matter in which particles slip past on another and take the shape of their container
gas
a state of matter in which particles can pull apart from one another and spread out
vapor
a substance that is suspended as a gas
states of matter
a physical property of matter. A given kind of matter has the same chemical makeup regardless of state
substance
a form of matter that has a specific chemical composition and distinct properties
mixture
a physical blend of 2 or more components each of which retains its own identity and properties in the mixture
solution
a homogeneous mixture where one substance is dissolved into a different substance
homogeneous mixture
a mixture in which the composition is uniform throughout the mixture
heterogeneous mixture
a mixture in which the composition is not uniform throughout the mixture
phase
a layer in a heterogeneous mixture
chromatography
separates 2 substances using a mobile phase and a stationary phase
distillation
separates 2 liquids by their differences in boiling points
filtration
separation of a mixture’s components through difference in particle size
element
a pure substance that cannot be broken down into any other substance
compound
a pure substance formed when 2+ elements have chemically combined through a chemical reactions to form a new substance
molecule
the smallest particle of a compound that still has the compound’s properties
chemical change
occurs whenever matter changes into an entirely different substance with different chemical properties
chemical property
properties that can only be measured or observed when matter undergoes a change to become an entirely different kind of matter
chemical symbol
a one or two letter designation of an element
flammability
the ability of matter to burn
precipitate
a solid that forms and settles out of a liquid mixture
product
products produced in a chemical reaction
reactant
substances that start a chemical reaction
reactivity
the ability of matter to react chemically with other substances
list at least 3 chemical properties of matter
reactivity, flammability, and the ability of matter to rust
list at least 3 physical properties of matter
color, hardness, state of matter, boiling point, odor
explain the difference between intensive and extensive properties
extensive properties depend on the amount of matter present, while intensive properties do not
list atleast 4 examples of chemical changes
burning, rusting, milk souring, baking a cake
list atleast 4 examples of physical changes
whipping eggs, boiling water, dicing vegetables, folding paper
what are the 4 common states of matter
liquid, solid, gas, plasma
describe the difference between a homogeneous and a heterogeneous mixture
homogeneous mixtures are evenly mixed and uniform throughout, while heterogeneous mixtures are not
list 4 method for separating mixtures
distillation, magnetism, filtration, chromatography
name an example of a field of chemistry being used in the real world
analytical chemists made COVID tests
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
what is the law of conservation of mass
matter cannot be created or destroyed
what are signs of a chemical reaction
change in color or temperature, creation of bubbles, formation of a precipitate or a gas
accuracy
how close a measurement comes to an actual value
precision
how close a series of measurements come to eachother
accepted value
the value that is widely accepted to be correct
experimental value
the value that has been measured
error
the difference between the experimental value and the accepted value
percent error
what percentage your experimental value is different from the accepted value
significant figures
a way of making sure measured numbers are not too precise
scientific notation
an easier way to look at very large numbers
international system of units
the measurement system used by most scientists and engineers
English system
measurement system used by americans
metric system
measurement system used in science and engineering and by countries other than the United states
dimensional analysis
a logical process of converting from one unit to another
temperature
the average kinetic energy of the particles in matter
Kelvin scale
a temperature scale based on molecular motion
celsius scale
temperature scale based on the boiling and freezing point of water
absolute zero
the point where all molecular motion stops
conversion factor
a fraction made from an equivalency
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
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
what is the equation for percent error
|experiment-accepted|over accepted
x 100
what are the rules for determining if a zero is a significant number?
- when the zero is in between nonzero digits
- 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
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
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
what is the equation for calculating density?
d=m/v
free card :)
:)
what is a CER
claim evidence and reasoning
