Semester Exam Review Flashcards
which SI prefix means “one million” or 10^6?
mega-
which SI prefix means “one billionth” ore 10^-9
nano-
which SI prefix means “one millionth” or 10^-6?
micro-
meters in a kilometer
1000
a millimeter is what fraction of a meter?
1/1000
centimeters in a meter
100
a lowercase letter m is the symbol of which SI prefix
milli-
symbol for the prefix centi-
c
carbon
C
chlorine
Cl
aluminum
Al
hydrogen
H
oxygen
O
iron
Fe
potassium
K
sodium
Na
calcium
Ca
neon
Ne
Cu
copper
Ag
silver
Si
silicon
He
helium
Zn
zinc
Co
cobalt
U
uranium
Pb
lead
Hg
mercury
F
fluorine
subatomic particle of the atom that has no electric charge
neutron
phenomenon that consists of electrons flowing between electrodes in a vacuum tube
cathode rays
type of particle that nucleons are believed to be made of
quarks
if there is a + after an element, than there will one ______________ electron than proton
LESS
equation to determine number of neutrons in an element
N= A (top number) - Z (lower number)
proposed the planetary model of the atom
Rutherford
experiment used to determine the electron’s charge
oil-drop experiment
this value is the number of nucleons in an atom
mass number
atoms of the same element that have different numbers of nucleons
isotopes
the prefix deca- in a molecular formula indicates that ___________ atoms of that element are present in each molecule
10
hepta-
7
nona-
9
octa
8
compound consisting of two nitrogen atoms and four oxygen atoms is named
dinitrogen tetroxide
compound consisting of two nitrogen atoms and five oxygen atoms
dinitrogen pentoxide
compound consisting of a carbon atom and four fluorine atoms is named
carbon tetrafluoride
compound consisting of a sulfur atom and six fluorine atoms is
sulfur hexafluoride
diphosphorus tetraiodide
P2 I4
diiron hexachloride
Fe2 Cl6
hydroxide
OH-
nitrate
NO3-
chlorate
ClO3-
ammonium
NH4+
bicarbonate
HCO3-
sulfate
SO4 2-
carbonate
CO3 2-
iron (III)
Fe 3+
silicate
SiO3 2-
phosphate
PO4 3-
the principle requiring that chemical reactions be balanced is the law of conservation of
mass
a symbolic representation of a chemical reactions is a
chemical equation
when writing a chemical reaction, the _________ are on the left and the _____________ are on the right
reactants- left
products- right
A + B —–> AB
combination reaction
AB ————-> A + B
decomposition reaction
AB + CD —————-> AD + CB
double-displacement reaction
AB + C ————–> A + BC
single-displacement reaction
According to Boyle’s law, if the pressure upon a gas INCREASES, the volume will
decrease (indirect proportioned)
According to Charle’s law, if the temperature of a gas is INCREASES, the volume will
increase (direct proportioned)
if the temperature of a gas is increases while its volume remains constant, its pressure will
increase
in the ideal gas law, the constant R is the ___________
universal gas constant
According to _________________ law, equal volumes of gases at the same temperature and pressure have the same number of molecules
Avogadro’s law
the acronym STP stands for
standard temperature and pressure
the molar volume of an ideal gas under STP conditions is about
22.4 L/mol
law that says that when gases react the volumes of reactants and products are in small, whole-number ratios
Gay-Lussac’s Law
the number of this type of particle identifies an atom as a given element
protons
type of chemist that would most likely study alcohols, which consist of carbon, hydrogen, and oxygen
organic chemist
indicates a chemical change
- change in color
- formation of gas
- formation of precipitate
group of two or more atoms linked together by chemical bonds
molecule
relative charge of an electron
-1
developed the atomic theory of matter
John Dalton
a homogenous part of a system that is in contact with but physically distinct from other parts of the system
phase
a measure of the force of gravity upon an object is
weight
as the internal kinetic energy of a substance increases, the substance’s temperature
INCREASES
the discovery of the nucleus and the development of the planetary model of the atom were results of the
gold-foil experiment
the smallest particles into which a compound may be broken down without changing it into another substance are
molecules
the general term for techniques of separating liquids based on their boiling points is
distillation
an ion that 3 protons, 4 neutrons, and 2 electrons is a
cation
best explanation as to why liquid becomes a gas at the boiling point
the kinetic energy of the particles is great enough to overcome their attraction of each other
term refers to the ration of an object’s mass to its volume
density
refers to energy that is possessed by matter due to its motion
kinetic
which of the three main particles composing that atom has the smallest mass
electron
value of Avogadro’s number
6.022 x 10^23
if the empirical formula of a substance is known, what additional information is needed to calculate the molecular formula
molar mass
unit that is equivalent to Avogadro’s number of objects
molle
set of symbols that tells how many of each type of atom are found in a molecule
formula
sum of the atomic masses of all the atoms in a molecule
mass
the smallest particles into which an element may be broken down without changing the identity of the element
atoms
1 millimeter of mercury is equal to
1 torr
number of protons in an atom
atomic number
standard atmosphere equals
760 torr
the isotope that the atomic mass unit is relative to
carbon-12
standard pressure and temperature
273.15 K and 760 torr
number of atoms in exactly one mole of atoms
6.022 x 10^23
the instrument used to measure atmospheric pressure
barometer
amount of force exerted upon a surface per unit area is
pressure
in the ___________ state of matter, particles have enough energy to move freely but not enough energy to overcome their attraction for each other
liquid
how closely a measured value matches the actual value is
accuracy
the dense central portion of an atom is called the
nucleus
the link between the microscopic and the macroscopic levels of chemistry is
Avogadro’s number
which law implies that at constant temperature and pressure, the molar volume of an ideal gas is constant
Avogadro’s law
negatively charged subatomic particles in an atom
electrons
the type of energy associated with motion is called
kinetic energy
the type of energy associated with the position of an object relative to the forces upon it is known as
potential energy
in thermodynamics, the portion of the universe of the sample of matter being studied is referred to as the
system
according to the first law of thermodynamics, the change in internal energy is the sum of
heat and work
the SI unit of work and energy
joule
the thermodynamic function denoted by the symbol H, which takes into account internal energy (E), volume (V), and pressure (P), is
enthalpy
a chemical reaction that can be summarized by the formula
reactants + heat ———————-> products is an
endothermic equation
reactants——————–> products + heat
exothermic reaction
heat required to raise the temperature of a unit mass of a substance by a unit temperature is the
specific heat
device in which energy changes during a chemical reaction may be measured is the
calorimeter
the highest or peak point on a wave is the wave’s
crest
the distance between any two corresponding points on successive waves is the
wavelength
the number of complete waves that pass by a point in a given time is the wave’s
frequency
individual “bundles” or quanta of light energy are called
photons
an arrangement of all forms of electromagnetic radiation in order of frequency and wavelength
electromagnetic spectrum
SI unit of frequency
Hertz
height of the wave
amplitude
the particle theory of light was first propsed by
Isaac Newton
the amount of energy an individual quantum of light contains depends on its
frequency
the speed of light in a vacuum is approximately
3.00 x 10^8 m/s
quantum number that describes the orientation of an orbital in space
magnetic quantum number (ml)
quantum number describes the shell in which an electron is located
principal quantum number (n)
states that no two electrons in the same atom have the same four quantum numbers
Pauli exclusion principle
states that a single electron occupies each orbital within a subshell before electrons begin pairing
Hund’s rule
specifies the order in which subshells fill with electrons
aufbau principle
type of orbital that has a spherical shape
s
the second shell from the center of an atom can hold up to ______________ electrons
8
the complete arrangement of electrons in an atom is the atom’s
electron configuration
the outermost electrons which are involved in chemical reactions
valence electrons
how many electrons are in the 2p subshell of a nitrogen atom?
1s^2 2s^2 2p^3
3
the energy required to remove an electron from an atom
ionization energy
describes how strongly a chemically combined atom draws electrons to itself
electronegativity
which are larger, simple cations or the neutral atoms from which they were formed?
neutral atoms
periodic trend: decreases down, increases across
ionization energy, electron affinity, electronegativity
periodic trend: increases down, decreases across
atomic radii, metallic character
refers to the randomness of a substance or system
entropy
internal energy of a system plus the product of its pressure and volume
enthalpy
energy is commonly defined as
the ability to do work
device used to measure heat flow during physical processes or chemical reactions
calorimeter
the change in a system’s internal energy is the sum of the heat added to the system and the work done on the system is the ____________ law of thermodynamics
1st
chemical and physical changes that release heat are known as
exothermic processes
the field of chemistry that deals with the energy changes in chemical reactions is chemical
thermodynamics
chemical reactions and physical changes that absorb heat are known as
endothermic processes
type of energy associated with position relative to a force is
potential energy
an endothermic reaction is characterized by ______________ change in enthalpy
positive
the enthalpy of formation for any element in its standard state is
0
when a cup of water evaporates into water vapor, the entropy change in the system is
positive
at constant pressure, enthalpy change equals
heat
the heat per unit mass required to vaporize a substance at its normal boiling point is
heat of vaporization
the total amount of heat liberated or absorbed because of a chemical reaction
heat of reaction
the heat per unit mass required to melt a substance at its normal melting point
heat of fusion
the amount of heat required to cause a unit rise in temperature of a unit mass of a substance
specific heat
individual packets of light energy
photons
amplitude of wave is the measure of its
strength
if the wavelength of a light wave decreases, how must its frequency change
increase
light consists of
electromagnetic waves
photons
developed the periodic table of the elements
Mendeleev
unit wave frequency is measured in
hertz
the lines in the hydrogen spectrum represent
photons emitted as electrons drop from higher to lower energy levels
consists of elements that usually exist as 2+ ions
alkaline earth metals
the lowest energy state of an atom
ground state
the elements in column 1 are the
alkali metals
the elements in column 2 are the
alkaline earth metals
the elements in column 17 are the
halogens
the elements in column 18
noble gases
elements in columns 1, 2, and 13-18 are all classified as
main-group elements
probable formula for the bromide of beryllium
1234321 (Br= 1; Be= 2) therefore BeBr2
not an alkali metal
calcium
when an element is vaporized and heated in a flame or an electric arc, the light emitted forms a
line spectrum
characterized by the transfer of electrons from one atom to another
ionic bond
characterized by the sharing of a “sea” of delocalized electrons among many atoms
metallic bond
produces substances that are characteristically malleable and ductile
metallic bond
bond in which cations are attracted to anions
ionic bond
states that atoms tend to react to achieve a noble-gas electron configuration
octet rule
unequal sharing of electrons produces a
polar bond
a bond that involves sharing of four electrons
double covalent bond
a bonding situation in which electrons are shared by more than two atoms is known as
delocalization
electrons that circulate freely through a molecule instead of being bound to a single atom or pair of atoms are said to be
delocalized (resonant)
a molecule that has a symmetrical distribution of polar covalent bonds will be ______________ as a whole
nonpolar
a formula in which nonbonding electrons are shown as dots around atoms and bonds are shown as lines or dots between atoms is a
Lewis structure
tetrahedral
4 bonds
0 nonbonds
polar or nonpolar
trigonal pyramidal
3 bonding
1 nonbonding
always polar
trigonal planar
3 bonding
0 nonbonding
polar or nonpolar
angular
2 bonding
2 nonbonding
always polar
linear
1 or 2 bonding
0 nonbonding
polar or nonpolar
why one group would be polar and the other not
arranged symmetrically vs. asymmetrically
superior system of measurement because of its divisibility
metric system
metric unit of mass
kilogram
metric unit of length
meter
10^-3
milli-
temperature scale for scientific measurement
Kelvin
makes numbers more manageable
scientific notation
numbers that are always significant
1-9
most abundant state of matter in the universe
plasma
smallest whole/complete particle
atoms
subatomic particles
proton (+)
electron (-)
neutron
chemical grouping of different types of atoms
compounds
mixture that is the same throughout
homogenous
mixture that is different throughout
heterogenous
change in state of matter
physical change
burn wood
chemical change
boil water into gas
physical change
processes used to separate mixture
distillation, chromatography
discovered the electrons
Thompson
discovered proton
Rutherford
discovered the neutron
Chadwick
shows number of protons
atomic number (Z)
the sum of neutrons and protons
mass number (A)
average mass of all isotopes
atomic mass
two types of chemical formulas
molecular, empirical
1 mole of substance =
Avogadro’s number
chemical changes caused by collisions between atoms/ molecules
chemical reaction
reactants on the ______________
products on the ______________
left
right
the reactant giving the smallest amount of production is the
limiting reactant
solid to liquid
heat of fusion
absorbs heat; cold to touch
endo-
product; releases energy
exo-
increases entropy
exothermic
reverse processes that don’t seem natural
spontaneity
states you can’t simultaneously know position and momentum of an electron
uncertainty principle
3D regions of probability
orbitals
2D pathway
orbit
tells chem properties and where the electrons are located
electron configuration
V and T are _______________ related
directly
units of pressure
pascal, torr atmosphere
measures pressure but does not require fluid
aneroid barometer
standard pressure
1 atm, 760 torr
measure pressure of gas sample
monometer
P and V are inversely related at constant T
Boyle’s Law
T and V are directly related at constant P
Charle’s law
temperature scale needed for the gas laws
Kelvin
constant T, P, V
Avogadro’s law
small whole number ratios
Gay-Lusac’s law
1 mole of gas at STP =
22.4 L
combines Boyle, Charles, and Avogadro’s law
ideal gas law
PVnRT
n= number of moles
R= universal gas constant (o.0821 L x atm/K x mol
mixing of gas by random molecular motion
diffusion
states that the heavier the gas the slower the rate of diffusion
Graham’s law of diffusion
states that the total pressure of gas = sum of all individual parts of pressure
Dalton’s law of partial pressure
1 calorie =
4.184 J
states that energy of the unierse is conserve
1st law of thermodynamics
total heat energy content of the system
enthalpy
exothermic has _ enthalpy
negative
a negative change in enthalpy is in ________________ in entropy
increase
specific heat of water
4.18 J/g x C
when the word heat is added
thermochemical equation
in fusion and vaporization, the _____________ does not change; the _________________ changes the ______________
temperature not change
energy changes state
Gibbs free energy helps determine
spontaneity
delta G is 0
equilibrium
-delta G
spontaneous
+ delta G
nonspontaneous
at a constant speed, wavelength and frequency are
inverse
max displacement
amplitude
particle theory of light
Newton
wave theory of light
Huygens
wave-particle duality
Einstein
electromagnetic waves
Maxwell
causes light to be emitted in LINE spectrum
excited and dropped to ground state
Bohr’s model proposed
energy levels
Schrodinger model
wave-mechanical model
Born’s Model
electron-cloud model
subshel shapes
s, p, d, f
determines the number of valence electrons
group
filling up from lowest to highest
aufbau
high EN
high ability to pull electrons to self
hydrogen bonded to _______ _____________ or __________ makes it a hydrogen bond
N, O, F
strongest intermolecular force
hydrogen bond
weakest intermolecular force; occurs in all atoms, molecules etc
London forces
present when molecules are polar; EN
dipole-dipole force
bonding present when greater than 1.7
ionic
bonding present when less than 1.7
covalent
determines type of bonding
electronegativity difference
only elements that do not require 8 valence electrons
hydrogen H
helium HE
states that nonbonding pairs have more force than bonding
VSEPR (valence-shell electron-pair repulsion)
Atoms will tend to react chemically so as to achieve a noble-gas electron configuration, either by losing or gaining electrons with other atoms
Octet rule
How do ionic and covalent bonds differ in the electron rearrangements involved?
Ionic bonding- electrons transferred
Covalent bonding- electrons shares
Why do covalent networks such as diamond and silicon carbide tend to be very hard?
Billions and trillions of atoms are joined into one unit by strong covalent bonds.
Primary difference between covalent and metallic bonding—
Covalent bonding involves the sharing of electrons
Metallic bonding involves the sharing of delocalized electrons among large number of atoms
Type of covalent bond that forms a dipole
Polar bond
How is resonance indicated when drawing Lewis structures?
Double-headed arrows between Lewis structures
How does an intermolecular force differ from a chemical bond?
Intermolecular forces physically attract molecules to each other without transfer or sharing of electrons
Chemical bonds chemical bond atoms into compounds through the transfer or sharing of electrons
What is the difference between crystalline and amorphous solids at the molecular level? How does this affect the properties of the substances?
Crystalline solid has particles arranged in a regular and repeated 3D pattern; definite melting point
Amorphous solids have no ordered arrangement or pattern for the particles that compose it; has not definite melting point.
Three main types of cubic unit cells
Body-centered cubic
Face-centered cubic
Simple unit cell
Cubic close packing
Face-centered cubic
The bcc’s atoms has ________ identical neighbors
8
The fcc’s and hcp’s atoms have _____________ identical neighbors
12
The simplest repeating unit in a crystal is called the
Unit cell
