Shared Flashcard Set

Details

L to J vocab
vocab
153
Chemistry
11th Grade
05/11/2010

Additional Chemistry Flashcards

 


 

Cards

Term
absolute zero
Definition
the zero point on the kelvin temperature scale, equivalent to -273.15C
Term
accepted value
Definition
a quantity used by general agreement of the scientific community
Term
accuracy
Definition
the closeness of a measurement to the true value of what is being measured
Term
acid
Definition
a compound that produces hydgrogen ions in solution
Term
activity series
Definition
a list of elements in order of decreasing activity
Term
actual yield
Definition
the amount of product that forms whe a reaction is carried out in the labratory
Term
allotrope
Definition
one of two or more differnet molecular forms of an element in the same physical state
Term
alloy
Definition
a misture composed of two or more elements, at least one of which is a metal
Term
amplitude
Definition
the hight of a wave's crest
Term
anion
Definition
any atom or group of atoms with a negative charge
Term
aqueous solution
Definition
water that contains dissolved substances
Term
atomic emission spectrum
Definition
the pattern formed whn light passes through a prism or diffraction grating to separate it into the different frequencies of light it contains
Term
atomic mass
Definition
the weighted average of the masses of the isotopes of an element
Term
atomic mass unit
Definition
a unit of mass equal to one-twelfth the mass of carbon-12 atom
Term
atomic number
Definition
the number of protons in the nucleus of an atom of an element
Term
atomic orbital
Definition
a mathematical expression describing the probability of finding an electron at various locations
Term
atomic radius
Definition
one-half the distance between the nuclei of two atoms of the same element when the atoms are joined
Term
aufbau principle
Definition
the rule that electrons occupy the orbitals of lowest energy first
Term
avagadro's number
Definition
the number representative particles contained in one mole of a substance
Term
balanced equation
Definition
a chemical equation in which mass is conserved
Term
base
Definition
a compound that produces hydroxide ions in solution
Term
binary compound
Definition
a compound composed of two elements
Term
bioling point elevation
Definition
the difference in temperature between the boiling point of a solution and the boiling point of the pure solvent
Term
bonding orbital
Definition
a molecular orbital that can be occupied by two electrons of covalent bond
Term
boyle's law
Definition
for a given mass of gas at constant temp, the volume of the gas varies inversely with pressure
Term
brownian motion
Definition
the chaotic movement of colloidal particles, caused by collision with particles of the solvent in which they are dispersed
Term
calorie
Definition
the quantity of heat needed to raise the temperature of 1 g fo pure water
Term
calorimeter
Definition
an insulated device used to measure the absorption or release of heat in chemical or physical processes
Term
calorimetry
Definition
the precise measurement of heat flow out of a system for chemical and physical processes
Term
catalyst
Definition
a substance that increases the rate of reaction by lowering the activation-energy barrier
Term
cathode ray
Definition
a stream of electrons produced at the negative electrode of a tube containing a gas at low pressure
Term
cation
Definition
any atom or group of atoms with a positve charge
Term
charle's law
Definition
the volume of a fixed mass of gas is directly proportional to its kelvin temperature if the pressure is kept constant
Term
chemical equation
Definition
an expression representing a chemical reaction
Term
chemical formula
Definition
an expression that indicates the number and type of atoms present in the smallest representative unit of substance
Term
coefficients
Definition
a small whole number that appears in front of a formula in a balanced chemical equation
Term
colligative properties
Definition
a property of a solution that depends only upon the number of solute particles, and not upon their identities
Term
combined gas law
Definition
the law that describes the relationship among the pressure, temperature, and volume of an enclosed gas
Term
combustion
Definition
a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light
Term
complete ionic equation
Definition
an equation that shows dissolved ionic compounds as dissociated free ions
Term
composition
Definition
Term
compressibility
Definition
a measure of how much the volume of matter decreases under pressure
Term
concentrated solution
Definition
a solution containing a large amount of solute
Term
concentration
Definition
a measurement of the amount of solute that is dissolved in a given quantity of solvent
Term
conversion factor
Definition
a ratio of equivalent measurements used to convert a quantity from one unit to another
Term
coordinate covalent bond
Definition
a covalent bond in which one atom contributes both bonding electrons
Term
coordination number
Definition
the number of ions of oppisite charge that surround each ion in a crystal
Term
covalent bond
Definition
a bond formed by the sharing of electrons between atoms
Term
decomposition
Definition
a chemical change in which a single compound is broken down into two or more simpler products
Term
diatomic molecule
Definition
a molecule consisting of two atoms
Term
diffusion
Definition
the tendancy of molecules to move toward areas of lower concentration until the concentration is uniform throughout
Term
dilute solution
Definition
a solution that contains a small amount of solute
Term
dimensional analysis
Definition
a technique of problem-solving that uses the units that are part of a measurement to help solve the problem
Term
dipole
Definition
a molecule that has two poles, or regions with opposite charges
Term
dispersion force
Definition
attractions between molecules caused by the electron motion on one molecule affectin g the electron motion on the other trhough electrical forces
Term
distillation
Definition
a process used to separate dissolved solids from a liquid, which is biled to produce a vapor that is then condencsed into a liquid
Term
double covalent bond
Definition
a bond in which two atoms share two pairs of electrons
Term
double displacement
Definition
a chemical change that involves an exchange of positive ions between tow compuonds
Term
effusion
Definition
the process that occurs when a gas escapes through a tiny hole in its container
Term
electrolyte
Definition
a compound that conducts an electric current when it is in a an aqueous solution or in the molten state
Term
electron configuration
Definition
the arrangement of electrons of an atom in its ground state into various orbitals around the nuclei of atoms
Term
electron dot diagram
Definition
a notation that depicts valence electrons as dots areound the atomic symbol of the element
Term
electronegativity
Definition
the ability of an atom to attract electrons when the atom is in a compound
Term
empirical formula
Definition
a formula with the lowest whole number ratio of elements in a compound
Term
endothermic process
Definition
a process that absorbs heat from the surroundings
Term
energy levels
Definition
the specific energies an electron in an atom or other system can have
Term
enthalpy
Definition
the heat content of a system at constant pressure
Term
error
Definition
the difference between the accepted value and the experimental value
Term
excess reactant
Definition
a reactant present in a quantity that is more than sufficent to react with a limiting reactant
Term
exothermic process
Definition
a process that releases heat to its surroundings
Term
experimental value
Definition
a quantitative value measured during an experiment
Term
extensive property
Definition
a property that depends on the amount of matter in a sample
Term
filtration
Definition
a process that separates a solid from the liquid in a heterogeneous mixture
Term
formula unit
Definition
the lowest whole number ratio of ions in an ionic compound
Term
freezing point depression
Definition
the difference in temperature between the freezing point of a solution and the freeaing point of the pure solvent
Term
frequency
Definition
the number of wave cycles that pass a given point per unit of time
Term
Gay-Lussac's Law
Definition
the pressure of a gas is directly proportional to the kelvin temperature if the volume is constant
Term
ground state
Definition
the lowest possible energy of an electron described by quantum mechanics
Term
heat
Definition
energy that transfers from one object to another because of a temperature diffeence between teh objects
Term
heisenberg uncertainty
Definition
it is impossible to know exactly both the velocity and the positio of a particle at the same time
Term
Hund's Rule
Definition
electrons occpy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible
Term
hydrate
Definition
a compound that has a specific number of water molecules bound to each formula unit
Term
hybridization
Definition
the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals
Term
hydrogen bonds
Definition
attractive forces in which a hydrogen covalentlybonded to a very electronegative atom is also weakly bonded to an unshared electron pair of another electronegative atom
Term
intensive property
Definition
a property that depends on the type of matter in a sample, not the amount of matter
Term
intensive property
Definition
a property that depends on the type of matter in a sample, not the amount of matter
Term
ion
Definition
an atom or group of atoms that has a positive or negative charge
Term
ionic bond
Definition
the electrostatic attraction that binds oppositely charged ions together
Term
ionization energy
Definition
the energy required to remove an electron from an atom in its gaseous state
Term
isotope
Definition
atoms of the same element that hve the same atomic number but different atomic masses due to a different number of nuetrons
Term
joule
Definition
the SI unit of energy
Term
law of conservation of energy
Definition
in any chemical or physical process, energy is neither created nor destroyed
Term
law of definite proportions
Definition
in samples of any chemical compound,the masses of elements are always in the same proportion
Term
law of conservation of mass
Definition
in any physical change or chemical reaction, mass is conserved
Term
law of multiple proportions
Definition
whenever two elements form more than one compound
Term
limiting reactant
Definition
any reactant that is used up first in a chemical reaction
Term
mass number
Definition
the total number of the amount of matter that an object contains
Term
melting point
Definition
the temperature at which a substance changes from a solid to a liquid
Term
metallic bond
Definition
the force of attractino that holds metals together
Term
molality
Definition
the concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 kilogram of solvent
Term
molar mass
Definition
a term used to refer to the massof a mole of any substance
Term
molar volume
Definition
the volume occupied by 1 mole of a gas at standard temperature and pressure
Term
molarity
Definition
the concentration of solute in a solution expressed as the numberof moles of solute dissolved in 1 liter of solution
Term
mole
Definition
the amount of a substance that contains 6.o2x1023 representative particles of that substance
Term
molecule
Definition
a neutral group of atoms joined together by covalent bonds
Term
monatomic ion
Definition
a single atom with a positive or negative charge resulting from the loss or gain of one or more valence electrons
Term
net ionic equation
Definition
an equation for a reaction in solution showing only those particles that are directly involved in the chemical change
Term
nonpolar covalent bond
Definition
a covalent bond in which the electrons are shared equally by two atoms
Term
octet rule
Definition
atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually eight valence electrons
Term
pascal
Definition
the SI unit of pressure
Term
Paulie exclusion principle
Definition
an atomic orbital may describe at most two electrons, each with opposite spin direction
Term
percent composition
Definition
the percent by mass of each element in a compound
Term
percent error
Definition
the percent that a measured value differs from the accepted value
Term
percent yeild
Definition
the ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage
Term
periodic law
Definition
when the elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties
Term
phase
Definition
any part of a sample with uniform composition and properties
Term
photon
Definition
a quantum of light
Term
pi bond
Definition
a covalent bond in which the bonding elctrons are most likely to be found in sausage-shaped regions above and below the bond axis of the bonded axis
Term
polar bond
Definition
a covalent bond between atomsin which the electrons are shared unequally
Term
polar molecule
Definition
a molecule in which one side of the molcule is slightly negative and the opposite side is slightly positive
Term
polyatomic ion
Definition
a tightly bound group of atoms that behaves as unit and has a positive or negative change
Term
precipitate
Definition
a solid that forms and settles out of a liquid mixture
Term
product
Definition
a substance produced in a chemical reaction
Term
quantum
Definition
the amount of energy needed to move an electron from one energy level to another
Term
quantum mechanical model
Definition
the modern description, primarily mathematical, of the behavior of electrons in atoms
Term
reactant
Definition
a substance present at the start of a reaction
Term
representative particle
Definition
the smallest unit into which a substance can be broken down without a change in composition, usually atoms, molecules, or ions
Term
saturated solution
Definition
a solution containing the maximum amount of solute for a given amount of solvent at a constant temperature and pressure
Term
sigma bond
Definition
a bond formed when two atomic orbitals combine for form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Term
significant digits
Definition
all the digits that can be known precisely in a measurement, plus a last estimated digit
Term
single covalent bond
Definition
a bond formed when two atoms share a pair of electrons
Term
single displacement reaction
Definition
a chemical change in which one element replaces a second element in a compound
Term
skeletal equation
Definition
a chemical equation that does not indicate the relative amounts of reactants and products
Term
solubility
Definition
the amount of a substance that dissolves in a given quantity of solvent at specified conditions of temperature and pressure to produce a saturated solution
Term
solute
Definition
dissolved particles in a solution
Term
solution
Definition
a homogeneous mixture
Term
solvent
Definition
the dissolving medium in a solution
Term
specific heat
Definition
the amount of heat needed to increase the temperature of 1 g of a substance 1 C
Term
spectator ion
Definition
an ion that is not directly involved in a chemical reaction
Term
spectrum
Definition
wavelengths of visible light that are separated when a beam of light passes through a prism
Term
standard temperature and pressure
Definition
the conditions under which the volume of a gas is usually measured
Term
stoichiometry
Definition
that portion of chemistry dealing with numerical relationships in chemical reactions
Term
structural formula
Definition
a chemical formula that shows the arrangement of atoms in a molecule or a polyatomic ion
Term
supersaturated solution
Definition
a solution that contains more solute than it can theoretically hold at a given temperature
Term
surface tension
Definition
an inward force that tends to minimize the surface area of a liquid
Term
theoretical yield
Definition
the amount of product that could form during a reaction calculated from a balanced chemical equation
Term
triple covalent bond
Definition
a covalent bond in which three pairs of electrons are shared by two atoms
Term
Tyndall effect
Definition
scattering of light by particles in a colloid or suspension, which causes a beam of light to become visible
Term
unsaturated solution
Definition
a solution that contains less solute than a saturated solution at a given temperature and pressure
Term
valence electron
Definition
an electron in the highest occupied energy level of an atom
Term
van der waals force
Definition
the two weakest intermolecular attractions--dispersion interactions and dipole forces
Term
vapor
Definition
describes the gaseous state of a substance that is generally a liquid or solid at room temperature
Term
vapor pressure
Definition
a measure of the force exerted by a gas above a liquid in a sealed container
Supporting users have an ad free experience!