Quarterly 4 review Flashcards
(Ch 1) chemistry is the study of the …, …, and … of matter and the changes that matter undergoes
composition; structure; properties
(Ch 1) a chemical is any substance that has a
definite composition or is used or produced in a chemical process
(Ch 1) basic research is carried out for the sake of
increasing knowledge
(Ch 1) applied research is carried out to
solve practical problems
(Ch 1) technological development involves the use of existing knowledge to
make life easier or more convenient
(Ch 1) all matter has … and …
mass; takes up space
(Ch 1) mass is one measure of the
amount of matter
(Ch 1) chemical properties refer to a substance’s ability to
undergo changes that alter its composition and identity
(Ch 1) an element is composed of one kind of
atom
(Ch 1) compounds are made from two or more
elements in fixed proportions
(Ch 1) all substances have characterisitc properties that enable chemists to tell the
substances apart and to separate the substances
(Ch 1) physical changes do not involve changes in
identity of a substance
(Ch 1) the three major states of matter are
solid, liquid, and gas
(Ch 1) changes of state, such as melting and boiling, are
physical changes
(Ch 1) in a chemical change (chemical reaction) the
identity of the substance changes
(Ch 1) energy changes accompany
physical and chemical changes
(Ch 1) energy may be released or absorbed, but it is neither
created nor destroyed
(Ch 1) matter can be classified into
mixtures and pure substances
(Ch 1) each element has a
unique symbol
(Ch 1) the periodic table shows the elements organized by their
chemical properties
(Ch 1) columns on the table respresent .. or … of elements that have similar …
groups; families; chemical properties
(Ch 1) properties vary across the rows, or
periods
(Ch 1) the elements can be classified as …, …, …, and …
metals, nonmetals, metalloids, noble gases
(Ch 1) these classes occupy different areas of the periodic table. metals tend to be, …., …, and … and tend to be good….
shiny; malleable; ductile; conductors
(Ch 1) nonmetals tend to be … and tend to be poor..
brittle; conductors
(Ch 1) metalloids are intermediate in properties between .. and …., and they tend to be … of electricity
metals; nonmetals; semiconductors
(Ch 1) the noble gases are generally
unreactive elements
(Ch 1) extensive properties depend on the amount of matter that is
present
(Ch 1) intensive properties do not depend on the
amount of matter present
(Ch 1) a physical property is a characteristic that can be observed or measured without changing the
identity of the substance
(Ch 1) a chemical proeprty relates to a substance’s ability to undergo changees that transform it into
different substances
(ch 2) the scientific method is a logical approach to
solving problems that lend themselves to investigation
(ch 2) a hypothesis is a testable statemtn that serves as the
basis for predictions and further experiments
(ch 2) a theory is a broad generalization that explains a body of
known facts or phenomena
(ch 2) the result of nearly every measurement is a
number and a unit
(ch 2) the SI system of measurement has seven base units:
meter (length) kilogram (mass) second (time) kelvin (temperature) mole (amount of substance) ampere (electric current) candela (luminous intensity)
(ch 2) weight is a measure fo the
gravitational pull on matter
(ch 2) derived Si units include the … and the …
square meter (area); cubic meter (volume)
(ch 2) density is the ratio of
mass to volume
(ch 2) conversion factors are used to convert from
one unit to another
(ch 2) accuracy refers to the closeness of a measurement to the
correct or accepted value
(ch 2) precision refers to the closeness of values for a
set of measurements
(ch 2) percentage error is the difference between the experimental and the accepted value that is
divided by the accepted value and then multiplied by 100
(ch 2) the significant figures in a number consist of all digits known with certainty plus
one final digit, which is uncertain
(ch 2) after addition or subtraction, the answer should be rounded so that it has no more digits to the right of the decimal point that there are in the measurement that has the
smallest number of digits to the right of the decimal point
(ch 2) after multiplication or division, the answer should be rounded so that it has no more significant figures than there are in the measurement that has
the fewest number of significant figures
(ch 2) exact conversion factors are completely certain and do not limit the number of
digits in a calculation
(ch 2) a number written in scientific notation is of the form … in which M is greater than or equal to 1 but less than 10 and n is an integer
M x 10^n
(ch 2) two quantities are directly proportional to each other if dividing one by the other
yields a constant value
(ch 2) two quantities are inversely proportional to each other if their product has a
constant value
(ch 2) a system is a specific portion of matter in a given region of space that has been selected for study
during an experiment or observation
(ch 2) a model in science is more than a physical object; it is often an explanation of how phenomena occur and how
data or events are related
(ch 2) a quantity is something that has
magnitude, size, or amount
(ch 2) dimensional analysis is a mathematical technique that allows you to use units to
solve problems involving measurements
(ch 3) john dalton proposed a scientific theory of atoms that can still be used to explain
properties of most chemicals today
(ch 3) matter and its mass cannot be … or …. in chemical reactions
created; destroyed
(ch 3) the mass ratios of the elements that make up a given compound are always the …, regardless of how much of the compound there … or how it …
same; is; was formed
(ch 3) if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element can be expressed as
a ratio of small whole numbers
(ch 3) cathode-ray tubes supplied evidence of the existence of
electrons
(ch 3) electrons are negatively charged subatomic particles that have relatively
little mass
(ch 3) rutherford found evidence for the existence of the atomic nucleus by bombarding gold foil with a
beam of positively charged particles
(ch 3) atomic nuclei are composed of …, which have an electric charge of …, and (in all but one case) neutrons, which have .. electric charge
protons; +1; no
(ch 3) atomic nuclei have radii of about …., and atoms have radii of about …
.001 pm; 40-270 pm
(ch 3) the atomic number of an element is equal to the number of
protons of an atom of that element
(ch 3) the mass number is equal to the total number of protons and neutrons that make up the
nucleus of an atom of that element
(ch 3) the relative atomic mass unit (amu) is based on the … atom and is a convenient unit for measuring the … of atoms
carbon-12; mass
(ch 3) the average atomic mass of an element is found by calculating the …. of the atomic masses of the naturally occuring … of the element
weighted average; isotopes
(ch 3) avogadro’s number is equal to approximately…. a sample that contains a number of particles equal to Avogadro’s number contains a … of those particles
6.022 x 10^23; mole
(ch 3) atom is the smallest particle of an element that retains the
chemical properties of that element
(ch 3) nuclear forces are short range …, …., and … forces that hold the nuclear particles …
proton-neutron, proton-proton, and neutron-neutron; together
(ch 3) isotopes are atoms of the same element that have
different masses
(ch 3) nuclide is a general term for a specific
isotope of an element
(ch 3) a mole is the amount of a substance that contains as many particles as there are atoms in exactly
12 g of carbon-12
(ch 3) molar mass is the mass of … of a pure substance
one mole
(ch 4) in the early 20th century, light was determined to have a dual
wave-partticle nature
(ch 4) quantum theory was developed to explain observations such as the … and the …. of hydrogen
photoelectric effect; line-emission spectrum
(ch 4) quantum theory states that electrons can exist only at specific
atomic energy levels
(ch 4) when an electron moves from one main energy level to a main energy level of lower energy, a …. is emitted. the … energy equals the energy difference between ….
photon; photon’s; the two levels
(ch 4) an electron in an atom can move from one main energy level to a higher main enrgy level only by absorbing an amount of energy exactly equal to the
difference between the two levels
(ch 4) electrons were determined to have a dual
wave-particle nature
(ch 4) the heisenberg uncertainty principle states that it is impossible to determine simultaneously the … and … of an … or any other …
velocity; position; electron; particle
(ch 4) quantization of electron energies is a natural outcome of othe …. which describes the properties of an atom’s …
Schrodinger wave equation; electrons
(ch 4) an orbital, a….., shows the regin in space where an electron is most likely to be …
3d region around the nucleus; found
(ch 4) the four quantum numbers that describe the properties of electrons in atomic orbitals are the:
principal quantum number
angular momentum quantum number:
magnetic quantum number
spin quantum number
(ch 4) the ground-state electron configuration of an atom can be written by using the:
aufbau principle
hund’s rule
pauli exclusion principle
(ch 4) electron configurations can be depicted by using different types of notation such as:
orbital notation
electron-configuration notation
noble-gas notation
(ch 4) electron configurations of some atoms, such as Cr, deviate from the predictions of the Aufbau principle, but the ground-state configuration that results is the configuration with the
minimum possible energy
(ch 4) electromagnetic radiation: form of energy that exhibits
wavelike behavior as it travels through space
(ch 4) electromagnetic spectrum formed by
all forms of electromagnetic radiation
(ch 4) wavelength: the distance between corresponding points on
adjacent waves
(ch 4) frequency: defined as the number of waves that pass a given point in a
specific time, usually one second
(ch 4) photoelectric effect: emission of electrons from a metal when
light shines on the metal
(ch 4) quantum of energy is the minimum quantity of energy that can be
lost or gained by an atom
(ch 4) photon: particle of electromagnetic radiation having
zero mass and carrying a quantum of energy
(ch 4) ground state: lowest … of an atom
energy state
(ch 4) excited state: a state in which an atom has a higher … than it has in its ….
potential energy; ground state
(ch 4) continuous spectrum: emission of a continuous range of
frequencies of electromagnetic radiation
(ch 4) principal quantum number: n, indicates the main
energy level occupied by electron
(ch 4) angular momentum quantum number, l, indicates the
shape of the orbital
(ch 4) magnetic quantum number, m, indicates the orientation of an
orbital around the nucleus
(ch 4) spin quantum number has only two possible values (+1/2, -1/2) which indicate the two fundamental
spin states of an eelctron in an orbital
(ch 4) aufbau principle: an electron ocupies the lowest-energy
orbital that can receive it
(ch 4) pauli exclusion principle: no two electrons in the same atom can have the same
set of four quantum numbers
(ch 4) hund’s rule: orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singlyu occupied orbitals must have
the same spin state
(ch 5) the periodic law states that the physical and chemical properties of the elements are
periodic functionso ftheir atomic numbers
the periodic table is an arrangement of the elements in order of their atomic numbers so that elements with simialr properties
fall in the same column
(ch 5) the columns in the periodic table are referred to as
groups
(ch 5) the rows in the periodic table are called
periods
(ch 5) many chemical properties of the elements can be explained by the configurations of the
elements’ outermost electrons
(ch 5) the nobel gases exhibit unique chemical stability because their highest occupied levels have an
octet of electrons, ns^2np^6
(ch 5) based on the electron configurations of the elements, the periodic table can be divided into four blocks:
s, p, d, and f
(ch 5) the groups and periods of the periodic table display general trends in following proterties:
electron affinity; electronegativity; ionization energy; atomoic radius; ionic radius
(ch 5) the electrons in an atom that are available to lost, gained, or shared in the formation of chemical compounds are
valence electrons
(ch 5) in determining the electron configuration of an ion, the order in which electrons are removed from the atom is the reverse of the order given by the
atom’s electron-configuration notation
(ch 5) lanthanides are 14 elements with atomic numbers from
58 to 71
(ch 5) actinides are 14 elements with atomic numbers from
90 to 103
(ch 5) alkali metals:
group 1
(ch 5) alkaline-earth metals:
group 2
(ch 5) transition elements: d-block elements with typical
metallic properties
(ch 5) main-group elements:
p-block and s-block elements
(ch 5) halogens:
group 17
(ch 5) atomic radius: 1/2 distance between
nucei of identical atoms that are bonded
(ch 5) ion: an atom or group of bonded atoms that has a
postive/ negative charge
(ch 5) ionization: any process that results int he formation of
an ion
(ch 5) ionization energy: energy required to remove
one electron from a neutral atom of an element
(ch 5) electron affinity: energy change that occurs when an electron is
acquired by a neutral atom
(ch 5) cation:
positive ion
(ch 5) anion:
negative ion
(ch 5) electronegativity: measure of the ability of an atom in a chemical compound to attract
electrons from another atom in the compound
(ch 6) most atoms are … to other atoms
chemically bonded
(ch 6) the three major types oc hemical bonding are
ionic, covalent, and metallic
(ch 6) in general, atoms of metals bond ionically with atoms of
nonmetals
(ch 6) atoms of metals bond metallically with
each other
(ch 6) and atoms of nonmetals bond
covalently with each other
(ch 6) atoms in molecules are joined by
covalent bonds
(ch 6) in a covalent bond, two atoms share
one or more pairs of electrons
(ch 6) the octet rule states that many chemical compounds tend to form bonds so that each atom shares or has
eight electrons in its highest occupied energy level
(ch 6) bonding within many molecules and ions can be indicated by a
lewis structure
(ch 6) molecules or ions that cannot be correctly represented by a single Lewis structure are represented by
resonance structures
(ch 6) an ionic compound is a 3d network of
cations and anions mutually attracted to each other
(ch 6) ionic compounds tend to be harder and more brittle and to have higher … than materials containing only ….
boiling points; covalently bonded atoms
(ch 6) the “electron sea” formed in metallic bonding gives metals their properties of …. and … conductivity, …, …, and …
high electrical; thermal; malleability; ductility; luster
(ch 6) vsepr theory is used to predic tthe … of molecules based on the fact that electron pairs strognly
shape; strongly repel each other
(ch 6) hybridization theory is used to predict the shapes of molecules based on the fact that orbitals within an atom can
mix to form orbitals of equal energy
(ch 6) intermolecular forces include … and …
dipole-dipole forces; london dispersion forces
(ch 6) hydrogen bonding is a special case of
dipole-dipole forces
(ch 6) chemical bond: mutual electrical attraction between nuclei and valence electrons of
different atoms that binds the atoms together
(ch 6) ionic bonding: chemical bonding that results from electrical attraction between
cations and anions
(ch 6) covalent bonding: sharing of electron pairs between
two atoms
(ch 6) nonpolar-covalent bond: covalent bond in which bonding electrons are shared equally by the bonded atoms, resulitng in a balanced
distribution of electrical charge
(ch 6) a polar-covalent bond is a covalent bond in whicht he bonded atoms have an
unequal attraction for the shared electrons
(ch 6) molecule: neuttral group of atoms that are held together by
covalent bonds
(ch 6) molecular compound: chemical compound whose simplest units are
molecules
(ch 6) chemical formula: indicates relative numbers of atoms of each kind in a chemical compound by using
atomic symbols and numerical subscripts
(ch 6) molecular formula: shows types and numbers of atoms combined in a single molecule of a
molecular ompound
(ch 6) bond energy: energy required to … a chemical bond and form…
break; neutral isolated atoms
(ch 6) structural formula: indicates…, …, …, and /… but not the unshared pairs of the atoms in a molecule
kind; number; arrangement; bonds
(ch 6) single bond: covalent bond in which one pair of electrons is shared between
two atoms
(ch 6) multiple bonds:
deouble and triple bonds
(ch 6) formula unit: simplest collection of atoms from which an ionic compound’s formula can be
established
(ch 6) lattice enrgy: energy released when one mole of an ionci crystalline compound is
formed from gaseous ions
(ch 6) polyatomic ion: charged group fo
covalently bonded atoms
(ch 6) metallic bonding: chemical bonding that results from the attraction betweern … and the surrounding…
metal atoms; sea of electrons
(ch 6) malleability: ability of a substance to be … or …
hhammered; beaten into sheets
(ch 6) ductility: ability of substance to be ..,…, or …. through a small opening to produce a wire
drawn; pulled; extruded
(ch 6) hybrid orbitals: orbitals of equal energy produced by the combination of two or more
orbitals on the same atom
(ch 6) dipole is created by equal but opposite charges that are
separated by a short distance
(ch 6) hydrogen bonding: intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an ubnshared pair of electrons of an
electronegative atom in a nearby molecule
(ch 6) london dispersion forces: intermolecular attractions resulting fromt he cosntant motion of electrosn and the creation fo
instantaneous dipoles
(ch 7) positive monatomic ion is identified simply by the name of the
appropriate element
(ch 7) a negative monatomic ion is named by dropping parts of the ending of the element’s name and adding
-ide to the root
(ch 7) the charge of each ion in an ionic comjpound may be used to determine the simplest
chemical formula for the compound
(ch 7) binary compounds are composed of
two elemetns
(ch 7) binary ionic compounds are named by combining the names of the
positive and negative ions
(ch 7) the old system of naming binary molecular compounds uses
prefixes
(ch 7) the new system, known ans the Stock system, uses
oxidation numbers
(ch 7) oxidation numbers are useful in …, writing…, and in ….
naming compounds; formulas; balancing chemical equations
(ch 7) compounds containing elements that have more than one oxidation state are named by using the
stock system
(ch 7) stock-system names and prefix-system names are used… for many molecular compounds
interchangeably
(ch 7) oxidation numbers of each element in a compound may be used to determine the compound’s simplest
chemical formula
(ch 7) by knowing oxidation numbers, we can name compounds without knowing whether theya re
ionic or molecular
(ch 7) …,…, and … cnan be calculated form the chemical formula for a compound
formula mass, molar mass, percentage composition
(ch 7) percentage composition of a compound si the percentage by mass of each
element in the compound
(ch 7) molar mass is used as conversion factor between amojunt in moles and mass in grams of a given
compound/ element
(ch 7) an empirical formula shows the simplest whole number ratio of
atoms in a given compound
(ch 7) empirical formulas indicate how many atoms of each elemnt are combined in the simplest
unit of a chemical compound
(ch 7) a molecular formula can be found from the empirical formula if the
molar mass is measured
(ch 7) oxyanion: polyatomic ions that
contian oxygen
(ch 7) salt: an ionic compound composed of a … and the … from an acid
cation; anion
(ch 7) oxidation state: assiged to the atoms composing the
compound or ion
(ch 7) formula mass: sum of the average atomic masses of
all atoms represented in the formula
(Ch 8) four observations that suggest a chemical reaction is taking place are the
evolution of energy as heat and light
production of gas
change in color
formation of a precipitate
(Ch 8) a balanced chemical equation represents, with symbols and formulas, the identities and relative amoutns of
products in a chemical reactio
(Ch 8) synthesis rections equation:
A+X→AX
(Ch 8) decomposition reaction equation
AX→A + X
(Ch 8) single-displacement reactions represented by two equation:
A + BX→AX + B
Y + BX→BY + X
(Ch 8) double diosplacement reaction equatio
AX + BY→AY + BX
(Ch 8) in a combustion reaction, a substance combines with…, realsing energy in the form of … and …
oxygen; heat; light
(Ch 8) activity series list the elements in order of their chemical reactivity and are useful in predicting wither a
chemical reaction will occur
(Ch 8) chemists determine activity series through
experiments
(Ch 8) precipitate: a solid that is produced as a result of a chemical reaction in solution and that
separates from the solutio
(Ch 8) coefficient: small whole number that ppears in front of a
formula in a chemical equation
(Ch 8) word equation: an equation in which the reactants and products in a chemical reactiona represented by
words
(Ch 8) formula equation: represents reactants and products of a chemical reaction by their
symbols or formulas
(Ch 8) electrolysis: decomposition of a substance by an
electric current
(ch 9) reaction stoichiometry involves the mass relationships between
reactants and products in a chemical reaction
(ch 9) relating one substance to another requires expressing the amount of each
substance in moles
(ch 9) a mole ratio is the conversion factor that relates the amount in … of any two substances in a …
moles; chemical reaction
(ch 9) the mole ratio is derived from the
balanced equation
(ch 9) amount of a substance is expressed in…., and mass of a substance is expressed by using mass units such ass…, …, or …
moles; grams; kilograms; milligrams
(ch 9) mass and amount of substance are.., wherars moles and grams are …
quantities; units
(ch 9) a balanced chemical equation is necessary to solve any
stoichiometric problem
(ch 9) in an ideal stoichiometric calculation, the mass or the amount of any reactnat or product can be calculated if the …. and the … or … of any other reactant or product is known
balanced chemical equation; mass; amount
(ch 9) in actual reactions, the reactants may be present in proportions that differ from the stoichiometric proportions required for a complete reaction in which all of
each reactant is converted to product
(ch 9) the limiting reactant controls the …. of product formed
maximum possible amount
(ch 9) for many reactions, the quantity of a product is less than the
theoretical maximum for that product
(ch 9) percentage yield shows the relationship between the … and … for the product of a reaction
theoretical yield; actual yield
(ch 9) composition stochiometry: deals with the mass relationships of
elements in compounds
(ch 9) excess reactant: substance that is not
used up completely in a reaction
(ch 9) theoretical yield: maximum amount of product that can be produced from a
giv en amount of reactant
(ch 9) actual yield: measured amount of a product obtained from a
reaction
(ch 10) the kinetic-molecular theory of matter can be used to explain the properties of
gases, liquids, and solids
(ch 10) the kinetic-molecular theory of gases describes a model of an
ideal gas
(ch 10) gases consist of large numbers of tiny, fast-moving … that are … relative to their sized
particles; far apart
(ch 10) particles of a liquid are … and more … than those of a gas and are less … than those of a solid
closer together; ordered; ordered
(ch 10) liquids have a definite … and a fairly high …, and they are relatively ….
volume; density; incompressible
l(ch 10) like gases, liquids can .. and are thus considered to be …
flow; fluids
(ch 10) the particles of a solid ar enot nearly as free to … as those of a liquid or gas
move about
(ch 10) solids have a definite .. and may be … or …
shape; crystalline; amorphous
(ch 10) solids have a definite … and are generally non…
volume; nonfluid
(ch 10) a crystal structure is the total 3d array of … that describes teh arrangement of the ..
.points; particles of a crystal
(ch 10) unlike crystalline solids, amorphous solids do not have a highly…. or a regular…
ordered structure; shape
(ch 10) a liquid in a closed system will gradually reach a… as the rate at which molecules … equals the rate at which they…
liquid-vapor equilibrium; condense; evaporate
(ch 10) when two opposing changes occur at equal rates in the same closed system, nthe system is said to be in
dynamic equilibrium
(ch 10) water is a
polar covalent compound
(ch 10) the structure and the hydrogen bonding in water are responsible for its relatively high…., molar ….., ….., and molar….
melting point; enthalpy of fusion; boiling point; enthalpy of vaporization
(ch 10) ideal gas: hypothetical gas that perfectly fits all the assumptions of the
kinetic-molecular theory
(ch 10) elastic collision: one in which there is no net loss of
total kinetic energy
(ch 10) diffusion: result of the spontaneous … of the particles of two substances caused by their….
mixing; random motion
(ch 10) effusion: process by which gas particles pass through a
tiny opening
(ch 10) real gas: a gas that does not behave completely according to the assumptions of the
kinetic-molecular theory
(ch 10) fluid: substance that can … and therefore take the … of of its container
flow; shape
(ch 10) surface tension: force that tends to pull adjacent parts of aliquid’s surface …, thereby decreasign
together; surface area to the smallest possible size
(ch 10) capillary action: attraction of the surface of a liquid to the s
surface of a solid
(ch 10) vaporization: process by which a liquid or solid
changes to a gas
(ch 10) evaporation: process by which particles escape from the surface of a nonboiling liquid and
enter the gas state
(ch 10) freezing/ solidification: physical change of a liquid to a solid by
removal of energy as heat
(ch 10) crystalline solids: consist of
crystals
(ch 10) amorphous solid: one in which the particles are
arranged randomly
(ch 10) meltin: physical change of a solid to a liquid by the addition of
nergy as heat
(ch 10) melting point: temperature at which a solid
becomes a liquid
(ch 10) supercooled liquids: substances that retain certain liquid properties even at
temperatures at which they appear to be solid
(ch 10) crystal: a substance in which the particles are arranged in an
orderly, geometric, repeating pattern
(ch 10) unit cell: the smallest portionof a crystal lattice that shows the
3d pattern of the entire lattice
(ch 10) phase; any part of a system that has
uniform composition and properties
(ch 10) condensation: process by which a gas changes to a
liquid
(ch 10) equilibrium: dynamic condition in which two opposing changes occur at
equal rates in a closed system
(ch 10) equilibrium vapor presssure: pressure exerted by a vapor in equilibrium with its
corresponding liquid at a given temeprature
(ch 10) volatile liquids: liquids that
evaporate readily
(ch 10) boiling: conversion of a liquid to a vapor within the liquid as well as
at its surface
(ch 10) boiling point: temeprature at which the equilibrium vapor pressure of the liquid equals
the atmospheric pressure
(ch 10) molar enthalpy of vaporization: amount of energy as heat that is needed to vaporize on mole of liquid at the liquid’s
boiling point at constant pressure
(ch 10) freezing point: temperature at whicht eh solid and liquid are in
equilibrium at 1 atm
(ch 10) molar enthalpy of fusion: amount of energy as heat required to melt one mole of
solid at the soldi’s melting pint
(ch 10) sublimation: change of state from a solid directly to a
gas
(ch 10) deposition: change of state from a gas directly to a
solid
(ch 10) phase diagram: graph of pressure versus temperature that shows the conditions under whicht he
phases of a substance exist
(ch 10) triple point: indicates the temeprature and pressure conditions at which the solid, liquid, and vapor of the substance can
coexist at equilibrium
(ch 10) critical point: indicates the critical
temperature and critical pressure
(ch 10) critical temperature: temperature above which the substance cannot exist in the
liquid state
(ch 10) critical pressure: lowest pressure at which the substance can exist as a liquid at the
critical temperature
(ch 11) kinetic moleculr teory of gases describes an
ideal gas
(ch 11) the behvior of most gases is nearly ideal except at very
high pressures and low temperatures
(ch 11) a barometer measures
atmospheric pressure
(ch 11) dalton’s law of partial pressure states that in a mixture of unreacting gases, the total pressure equals the sum of the
partial pressures of each gas
(ch 11) boyle’s law states the inverse relationship between the volume and pressure of a gas:
PV=k
(ch 11) charles law illustrates the direct relationship between a gas’s … and its … in kelvins:
volume; temperature
V=kT
(ch 11) gay-lussac’s law represents the direct relationshjip betrween a gas’s … and its … in kelvins:
pressure; temperature
P=kT
(ch 11) the combined gas law combines boyle’s, charles’s, and gay-lussac’s law into this epression:
PV/ T=k
(ch 11) gay-lussac’s law of combining volumes states that the volumes of recting gases and their products at the same temperature and pressure can be expressed as
ratios of whole numbers
(ch 11) avogadro’s law states that equal volumes of gases at the same temperature and pressure contain
equal numbers of molecules
(ch 11) the volume occupied by one mole of an ideal gas at STP is called the …, which …
standard molar volume; 22.414 L
(ch 11) charles’s law, Boyle’s law, and Avogadro’s law can be bombined to create the ideal gas law:
PV=nRT
(ch 11) gases diffuse, or become morespread out, due to their
constant random molecular motion
(ch 11) graham’s law of effusion states that the relative rates of effusion of gases at the same temperature and pressurea re inversely proportional to the
square roots of their molar masses
(ch 11) pressure is defined as the force per
unit area on a surface
(ch 11) newton: force that will increase the speed of a 1 kilogram mass by one meter per second each second that the
force is applied
(ch 11) millimeters of mercury: common unit of
pressure
(ch 11) atmosphere of pressure: exactly equivalent to
760 mm Hg
(ch 11) pascal: the pressure exerted by a force of one … acting on an area of one
newton; square meter
(ch 11) partial pressure: pressure of each
gas in a mixture
(ch 11) absolute zero: teh temperature …, given a value of … in the kelvin scale
-273.15 C; zero
(ch 11) ideal gas constant: the constant …, with balues of … atm and …. kPa
R; .082 atm; 8.314 kPa
( ch 12) solutions are
homogenous mixtures
( ch 12) mixtures are classified as:
solutions
suspensions
colloids
( ch 12) the way mixtures are classified depends on the … of the solute particles in the mixture
size
( ch 12) the dissolved substance is the
solute
( ch 12) solutions that have water as a solvent are
aqueous solutions
( ch 12) solutions can consist of solutes and solvents that are
solids, liquids, or gases
( ch 12) suspensions settle out upon
standing
( ch 12) colloids do not settle out, and they scatter
light that’s shined through them
( ch 12) most ionic solutes and some molecular solutes form aqueous solutions that conduct an electric current:
electrolytes
( ch 12) nonelectrolytes are solutes that dissolve in water to form
solutions that do not conduct
( ch 12) a solute dissolves at a rate that depends on the … of the solute, how vigorously the solution is.., and the … of the solvent
surface area; mixed; temperature
( ch 12) the solubility of a substance indicates how much of that substance will dissolve in a specified amount of solvent under
certain conditions
( ch 12) the solubility of a substance depends on the
temeprature
( ch 12) the solubilityof gases in liquids increases with icreases in
pressure
( ch 12) the solubility of gases in liquids decreases wtih
increases in temperature
( ch 12) the overall energy absorbed as heat by the system when a specified amount osf solute dissolved during solution formation is caleld the
enthalpy of solution
( ch 12) two useful expressions of concentration are
molarity and molality
( ch 12) the molar concentration of a solution represents the ratio fo moles of solute to
liters of solutio
n( ch 12) the molal concentration of a solution represents the ratio fo moles of solute to
kilograms of solvent
( ch 12) soluble: capable of being
dissolved
( ch 12) solvent: dissolving
medium
( ch 12) solution equilibrium: physical state in which the opposing processes of … and … of a solute occur at equal rates
dissolution; crystallization
( ch 12) saturated solution: a solution that contains the maximum amount of
dissolved solute
( ch 12) unsaturated solution: solution that contains less solute than a
saturated solution under same conditions
( ch 12) supersaturated solution: contains more dissolved solute that a saturated solution contains under the
same conditions
( ch 12) hydration: solution process with water as the
solvent
( ch 12) immiscible: liquids that are nto
soluble in each other
( ch 12) miscible: liquids that dissolve freely in one another in any
proportion
( ch 12) henry’s law: solubilityof a gas in al iquid is directly proportional to the partial pressure of that gas on the
surface of the liquid
( ch 12) effervescence: rapid escape of a gas from a liquid in which it is
dissovled
( ch 12) solvated: solute particle that is surrounded by
solvent molecules
( ch 12) enthalpy of solution: the net amount of energy absorbed as heat by the solution when a specific amount of
solute dissolves in a solvent
( ch 12) concentration: measure fo the amount of solute in a given amount of
solvent or solution
In general, the atomic radii of the main-group elements… down a group
increase
In general, ionization energies of the main-group elements … across each period.
increase
Among the main-group elements, ionization energies generally… down the groups;
decrease
Ionic radii: cationic radii …across a period
decrease
anionic radii ….across each period
decrease
there is a gradual …of ionic radii down a group
increase
electronegativities tend to …across each period, although there are exceptions;
increase
electronegativities tend to either …down a group or remain about the same
decrease
