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chemistry
the study of matter, its properties, the changes that matter undergoes, and the energy associated with these changes
matter
anything with both mass and volume
composition
the types and amounts of simpler substances that make up matter
physical property
properties a substance shows itself without interacting with another substance
color
physical property
melting and boiling point
physical property
density
physical property
chemical property
properties a substance shows as it interacts with other substances
flammability
chemical property
corrosiveness
chemical property
physical change
produces a recognizable difference in the appearance without changing the composition (state change)
chemical change
transformation of a substance by rearranging, removing, replacing, or adding atoms
solid
state of matter with a fixed shape and volume, may be hard or soft, rigid or flexible
liquid
state of matter with varying shape but a fixed volume, shapes conforms to the shape of the container it is in
a liquid has an _________
upper surface
gas
state of matter with no fixed shape or volume and no surface
plasma
gaseous state of matter with an appreciable amount of electrically charge particles
where is plasma found?
certain high temperature environments (stars and lightning)
solid state to liquid state
melting
solid state to gaseous state
deposition
liquid state to solid state
freezing
liquid state to gaseous state
evaporation
gaseous state to liquid state
condensation
gaseous state to solid state
sublimation
true or false: physical changes are reversible
true
energy
the ability to do work
potential energy
energy due to object’s position
kinetic energy
energy due to object’s movement
______ energy states are more stable than _______ energy states
lower; higher
specific heat
the amount of heat needed to raise temperature of 1g of substance 1 degree C
true or false: nonmetals generally have low specific heats
false: they usually have high specific heats
true or false: metals generally have low specific heats
true
if you sleep outside in the winter, would sleeping in a tent or a car be safer?
the tent because nonmetals have higher specific heats
gravitational system
the potential energy gained when a lifted weight is converted to kinetic energy as the weight falls
conversion factor
ratio of equivalent quantities used to express a quantity in different units
If you need 325 cm of wire and the wire sells for $0.15/ft, how much will the wire cost?
$1.60
325 cm x 1in/2.54cm x 1ft/12in x $0.15/1ft = 1.60 dollars
density
mass divided by volume
Celsius degrees
scale based on the freezing and boiling points of water; most common around the world
Kelvin
the “absolute temperature scale”, begins at absolute zero
true or false: the Kelvin scale only has positive numbers
true
Fahrenheit degrees
this scale has a different size and different zero points than other scales
true or false: Celsius and Fahrenheit use the same size degree
false: Celsius and Kelvin share the same size degree
Celsius temperature to Kelvin
C temp + 273.15
Kelvin temperature to Celsius
K temp - 27.15
Celsius temperature to Fahrenheit
9/5(C temp) + 32
Fahrenheit temperature to Celsius
5/9(F temp - 32)
A child has a body temperature of 38.7 degrees Celsius. If the normal body temperature is 98.6 degrees Fahrenheit, do they have a fever? What is their temperature in Kelvin?
yes and 311.8 K
true or false: the rightmost digit of a measurement is always certain
false: it is always estimated
zeros to the ______ of digits are not significant
left
_______ zeros in ________ are significant
trailing; decimal places
true or false: all nonzero digits are significant
true
the significant figures for a multiplication/division answer should have the _____________ as the measurement with the fewest sig. figs.
same number of significant figures
the answer to an addition/subtraction problem should have the ____________ as the measurement with the fewest decimal places
same number of decimal places
exact numbers have _______________ associated with them
no uncertainty
precision
how close measurements in a series are to each other
accuracy
how close each measurement is to the actual value
systematic error
produces values that are either all higher or all lower than the actual value
random error
produces values that are both higher and lower than the actual value
true or false: some results can be precise while also being inaccurate
true
_______ connect the dots on a graph
NEVER
R² value
indicates how close measurements are to a straight line
standard deviaiton
measure used to quantify the amount of variation in a set of data
small standard deviation has _____ precision and is ______ to mean value
high; close
large standard deviation has _____ precision and _______ variation
low; random
atom
basic structural unit of an element that retains its chemical properties
a neutral atom has the same number of what?
protons and electrons
atomic mass
sum of number of protons and neutrons
true or false: the atomic number of an atom is equal to its number of electrons
false: equal to number of protons
If Boron’s (B) atomic mass is equal to 11 and its atomic number is 5, calculate its numbers of protons, electrons, and neutrons.
protons = 5
electrons = 5
neutrons = 6
isotopes
atoms of the same element having different masses (different numbers of neutrons)
excited electron state
promotion of electrons occurs as it absorbs energy
electrons absorb energy when they move to _______ energy levels
higher
relaxation state
electrons release energy as they travel to lower energy states
ground state
the lowest possible energy level
Bohr failed to explain what?
line spectra of atoms with more than one electron
what is a major change from Bohr’s Theory to the Modern Atomic Theory?
electrons do NOT move in orbits
atomic orbitals
regions in space with a high probability of electrons
Dmitri Mendeleev and Lothar Meyer did what?
independently
periodic law
the physical and chemical properties of the elements are periodic functions of their atomic number
period
horizontal row of elements on periodic table
group
(aka “families”) column of elements on periodic table
metals
substances whose atoms tend to lose electrons (positive charge) and mainly found in the left 2/3 of periodic table
high thermal/electrical conductivity
metallic property
high malleability/ductility
metallic property
solid at room temperature
metals
nonmetals
substances whose atoms tend to gain electrons (negative charge) and mainly found on the right 1/3 of the periodic table
brittle and powdery solids/gases
nonmetals
true or false: nonmetals’ properties are the opposite of metallic properties
true
electron configuration
describes the arrangement of electrons in atoms
principle energy levels
regions where electrons may be found (values like n=1,2,3. . . )
sublevel
set of energy-equal orbits within a principle energy level
true or false: s orbitals are spherically symmetrical in shape
true
true or false: p orbitals are shaped like dumbbells
true
how many electrons can a s orbital hold?
2
how many electrons can a p orbital hold?
6
how many electrons can a d orbital hold?
10
Aufbau Principle
electrons will fill the lowest available orbitals first
Pauli Exclusion Principle
each orbital can hold up to two electrons with their spins in the opposite directions
Hund’s Rule
each orbital in a subshell is half-filled before any becomes paired
valence electrons
outermost electrons in an atoms