General Objectives Flashcards
(170 cards)
1
Q
Spontaneous disintegration of unstable atomic nucleus with accompanying emission of radiation
A
Radioactivity
2
Q
This principle states that it is impossible to determine simultaneously the exact position and the exact momentum of a body as small as the electron
A
Uncertainty Principle
3
Q
States that the properties of elements are periodic functions of their atomic numbers
A
Periodic Law
4
Q
Shows that elements are arranged according to increasing atomic weights, similarities in physical and chemical properties reappear after each interval of 8 elements
A
Law of Octaves
5
Q
Smallest increment of radiant energy that may be absorbed or emitted
A
Quanta
6
Q
Wave function of an electron
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Orbital
7
Q
Theory that organic substances can only be produced from other organic substances
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Vital Force Theory
8
Q
Scientific discipline that treats the composition, properties and transformations of matter; study of structure and changes matter undergoes in natural processes and planned experiments
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Chemistry
9
Q
Physical material of the universe; anything that occupies space and has mass
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Matter
10
Q
Properties w/c can be measured and observed w/o changing the basic identity of the substance
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Physical
11
Q
Properties that describe the way a substance may change or react to form other substances
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Chemical
12
Q
Characteristics of any sample of a substance regardless of the size or shape of the sample
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Intrinsic or Intensive
13
Q
Accidental properties; depend on the amount of material
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Extrinsic or extensive
14
Q
Homogenous material consisting of one particular kind of matter; matter that has a definite composition and distinct properties
A
Pure substance
15
Q
Constituents can be separated by suitable physical means into pure components without changing the identities of the components; combination of two or more substances in w/c each substance retains its own identity and hence its own properties
A
Mixture
16
Q
Substances that cannot be separated into simpler substances by chemical means
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Elements
17
Q
Substances composed of two or more elements united chemically in fixed proportions
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Compounds
18
Q
Substance able to donate a H+ ion; proton donor
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Acid
19
Q
Produces an excess OH- (aq) ions when dissolved in water; proton acceptor
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Base
20
Q
Ionic compound formed by replacing one or more H+ of an acid by other cations
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Salt
21
Q
Material in which no differing parts can be distinguished
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Homogenous
22
Q
Materials with differing parts may be separated physically
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Heterogeneous
23
Q
Mixtures containing particles larger than normal solutes, invisible to the eye and microscope but visible in ultramicroscope
A
Colloidal suspension
24
Q
Consists of particles appearing as huge molecules in a dispersing medium; particles may be visible to the eye and settle rapidly to the bottom if container
A
Coarse suspension
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Law which states that when an ordinary chemical reaction occurs, there is no detectable change in the masses of the substances involved before and after the reaction
LAW OF CONSERVATION OF MATTER
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Law stating that energy is neither created nor destroyed in any transformation but is transformed from one form to another
LAW OF CONSERVATION OF ENERGY
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states that every sample of a given substance always contains the same proportion by weight of all its constituent elements
LAW OF DEFINITE PROPORTIONS OR DEFINITE
COMPOSITION
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states that when two elements are combined
to form two or more different compounds, and if the
amount of one element is constant, the mass of the
other element in the different compounds are in a
ratio of whole numbers.
LAW OF MULTIPLE PROPORTIONS
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among its primary goals is the investigation of
the structure and transformation of matter and the
interrelationships of energy and matter; application of the methods and theories of physics to the study of chemical changes and
properties of matter
Physical Chemistry
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is concerned with the
separation, identification and composition of all
kinds of matter
analytical chemistry
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involves the separation and identification of the individual components of materials. It answers the question, “What is
present?”
qualitative analysis
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is concerned with how much of each component is present
quantitative analysis
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study of carbon-containing compounds; This branch of chemistry now deals with commonly used synthetic substances such as plastics, drugs, dyes, explosives and detergents.
Organic chemistry
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covers the chemistry of all elements and their compounds with the exception of carbon and its compounds
Inorganic chemistry
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branch of chemistry which
includes the study of the materials and processes
that occur in living organisms. These materials are
largely organic (carbon) compounds
Biochemistry
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deals with the changes in the nuclei of atoms and the used of these changes, especially in the study of how substances react.
Nuclear chemistry
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form of energy which flows spontaneously from a substance of higher temperature to one of lower temperature.
heat
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measure of the intensity of heat; intensive quantity that defines the direction and rate of heat flow; hotness or coldness of a body
temperature
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temp scale is based on the freezing and boiling point of water
relative
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temp scale based on the quantity of kinetic energy that molecules have
absolute
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amount of matter found in a substance; measure of a substance’s resistance to the change in velocity
mass
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refers to the force with which an object is attracted to the earth
weight
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ratio of the mass of the substance to the mass of water that occupies the same volume
relative density
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quantity of heat required to raise the temperature of one gram of a substance by 1 degC
specific heat
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quantity of heat required to raise the temperature of 1 gram of water by 1 degC
calorie
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device used to measure the quantity of heat exchanged between
the thermodynamic system and its surroundings
calorimeter
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States that the amount of heat that a body gains or losses depends on the mass and nature of the body and change in temperature of that body
law of heat
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Amount of heat lost by one body is equal to the amount of heat gained by another body
law of heat exchange
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smallest unit of element that cannot be further subdivided and is capable of taking part in a chemical reaction; basic building blocks of matter
atom
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smallest unit of element or chemical compound capable of free existence (combination of two or more atoms)
molecule
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Dalton’s Atomic Theory of matter
1. Elements are composed of extremely small particles called atoms.
2. All atoms of a given element are identical; the atoms of different elements are different and have different properties (including different masses).
3. Atoms of an element are not changed into different types of atoms by chemical reactions: Atoms are neither created nor destroyed in chemical reactions.
4. Compounds are formed when atoms of more than one element combine; a given compound always has the same relative number and kind of atoms.
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high energy radiation similar to X-rays and does not consist of particles
gamma radiation
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high speed electrons which could be considered as the radioactive
equivalent of cathode rays (-1 charge)
beta radiaton
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much more massive than β particles and have a positive rather than a negative charge; has a charge of 2+; combines with electrons to form atoms of helium
alpha radiation
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number of protons in the nucleus
atomic number
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total number of protons and neutrons (nucleons)
mass number
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atoms of the same element containing different number of neutrons and therefore having different masses
isotopes
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the arrangement of elements in order of increasing atomic number, with elements having similar properties placed in vertical columns
periodic table
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vertical columns bringing together elements with similar properties
family or group
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horizontal rows of the table arranged in order of increasing atomic number
period
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elements (with the exemption of hydrogen) found on the left side of the heavy ladder-like line in the periodic table
metals
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elements found on the right side of the heavy ladder-like in the periodic table
non-metals
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elements that lie along the heavy ladder-like line separating the metals from the nonmetals in the periodic table
metalloids or amphoteric elements
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Elements of this type are characterized by atoms in which all subsidiary quantum levels that are present are filled up to capacity. These are members of Group VIII A in the periodic table.
inert gas
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These elements partially occupy the s and the d block. These are
known as the s and p block elements; A family
representative elements
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These elements are characterized by atoms in which an inner d-level is present but is not filled up to capacity.
transition elements
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These elements are characterized by atoms which contain incompletely filled levels as well as incompletely filled f-levels.
inner transition elements
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energy required to remove the most loosely held electron from a gaseous atom when it is in its ground state,
ionization energy
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System of naming substances or compounds.
chemical nomenclature
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symbolic representation of elements; consists of either one or two letters
chemical symbol
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a substance formed from two or more elements; a substance that can be decomposed into two or more simpler substances by ordinary chemical means
chemical compound
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Any molecule that is made up of two atoms: H2 , O2 , N2 , F2 ,
Cl2 , Br 2 , I2
Diatomic molecules
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a shorthand notation using chemical symbols and numerical subscripts to represent the composition of a substance
chemical formula
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special valence number assigned to each element to indicate the number of electrons oxidation state/valence gained, lost or shared
unequally
oxidation number/charge
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represent the number of electrons in the outermost energy level which are largely responsible for the chemical behavior of an element
valence electron
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an ion consisting of two or more atoms chemically bonded together and carrying a net electric charge
polyatomic ion
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an electrically charged particle obtained from an atom or a chemically bonded group of atoms by adding or removing electrons
ion
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a change in which one or more kinds of matter are transformed into a new kind of matter or several new kinds of matter; change in which a new substance with new properties is formed.
chemical reaction
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a shorthand way of representing a chemical reaction using chemical formulas to indicate the reactants and products
chemical equation
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a type of reaction wherein a single more complex product is formed by the combination of two or more simpler substances.
direct combination or synthesis
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a reaction wherein a compound is broken down into two or
more simpler substances.
decomposition or analysis
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A reaction wherein an element or an ion displaces another element or ion in a compound.
single displacement
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a reaction wherein compounds interchange ions or radicals. Compounds exchange positive and negative parts and results in the formation of different compounds.
metathesis or double displacement
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the calculation of the quantities of materials consumed and produced in chemical reactions
chemical stoichiometry
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defined as the number of carbon atoms in exactly 12 grams of pure C-12 atom; counting unit of a chemist
mole
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the mass in grams of one mole of molecules or formula unit of a substance; also called molecular weight
molar mass
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formula which shows the simplest whole number ratio of atoms in a compound
empirical formula
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the exact formula of a molecule giving the types of atoms and the number of each type
molecular formula
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a compound in which a fixed number of water molecules are associated with each formula unit; composed of an anhydrous salt and water of hydration
hydrate
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the ratio of moles of one substance to moles of another substance in a balanced chemical equation
mole ratio
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the reactant that is completely consumed when a reaction is run to completion
limiting reactant
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the measured quantity of product obtained in a chemical reaction less than theoretical
actual yield
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the quantity of product calculated to result from a chemical reaction
theoretical yield
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defined as the force exerted per unit area
pressure
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At constant temperature, the volume of a sample of a gas varies inversely with the pressure
Boyle's Law
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The volume of any sample of a gas varies directly with the absolute temperature, if the pressure is held constant.
Charles' Law
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The pressure of a gas varies directly with the absolute temperature when the volume is held constant.
Amonton's Law
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Equal number of molecules are contained in equal volumes of different gases if the temperature is the same.
Avogadro's Law
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The volume of a gas is directly proportional to the number of moles present, n, and to the absolute temperature, T, and is inversely
proportional to the pressure, P.
Ideal Gas Law
100
term used to describe the mixing of gases
diffusion
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term used to describe the passage of gas through a tiny orifice into an evacuated chamber
effusion
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states that the effusion rate of a gas is inversely proportional to the square root of the mass of its particles
Graham's Law
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When measured at constant temperature and pressure, the volume of gases that are produced or used in a chemical reaction can be expressed in ratios of small whole numbers.
Gay Lussac's Law of Combining Volumes
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dissolving medium of a solution; component of a solution that is greater in quantity
solvent
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universal solvent
water
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substance dissolved in a solvent to make a solution component of a solution that is present in relatively smaller quantity
solute
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refers to the amount of substance that dissolves in a given quantity of solvent at a given temperature to form a saturated solution; this characteristic of a substance is the concentration of its saturated solution
solubility
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an increase in temperature ________ the solubility of most solid solutes dissolved in liquid solvent
increases
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an increase in temperature decreases the solubility of gaseous
solutes dissolved in _______ solvent
liquid
110
for _________, the greater the pressure, the higher the solubility
gases
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contains the maximum amount of solute that can be dissolved under the conditions at which the solution exists
saturated solution
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a solution that is not in equilibrium with respect to a given dissolved substance and in which more of the substance can dissolve
unsaturated solution
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solution which contains an amount of solute in excess of that normally possible under existing conditions; unstable solution in which the concentration of the solute is greater than its saturated solution
supersaturated solution
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solution where a small amount of solute is present in solution relative to the amount that could dissolve
dilute solution
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solution that contains a relatively large amount of solute relative to the amount that could dissolve
concentrated solution
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substances which dissolves in any amount in each other
miscible substances
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substances which have limited solubility in each other
partially miscible
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substances which do not dissolve in each other and forms two separate layers upon mixing
immiscible
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solutions in which water is the solvent
aqueous solution
120
concentration unit most often used in a chemical laboratory; ratio giving the number of moles (n) of solute per liter of solution
molarity
121
finds use in experimental situations where changes in temperature are of concern; ratio giving the number of moles of solute per kg of solvent
molality
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most encountered in situations that involve the reactions of acids with bases; ratio giving the number of gram-equivalents of solute present in a liter volume of solution
normality
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is the process in which more solvent is added to a solution in order to lower the concentration of the solution.
dilution
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The vapor pressure, freezing point and boiling point of a solution differs from those of the pure solvent by amounts that are directly proportional to the molal concentration of the solute.
Colligative Property Law
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The freezing point of a solution is always _________ than the freezing point of the pure solvent.
lower
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The temperature at which a solution boils is ________ than that of the pure solvent if the solute is nonvolatile.
higher
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States that the vapor pressure of a solvent above a solution is equal to the vapor pressure of the pure solvent at the same temperature scaled by the mole fraction of the solvent present
Raoult's law
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spontaneous net movement or diffusion of solvent molecules through a selectively-permeable membrane from a region of high water potential to a region of low water potential, in the direction that tends to equalize the solute concentrations on the two sides.
osmosis
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pressure needed to prevent the flow of solvent into the solution through a semi-permeable membrane
osmotic pressure
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the change in concentration of a reactant or product per unit time
reaction rate
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set of postulates used to explain how chemical reactions occur.
collision theory
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Collision Theory fundamental postulates
1. Reactant particles must collide with each other in order for a reaction to occur.
2. Colliding particles must collide with a certain minimum total amount of energy (activation energy), if the collision is to result in a reaction.
3. In some cases, reactants must be oriented in a specific way upon collision if a reaction is to occur.
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The minimum energy of collision required for two molecules to react
Activation energy
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state reached by a reaction mixture when the rate of the forward reaction and that of the reverse reaction have become equal.
chemical equilibrium
135
TRUE OR FALSE: Only concentrations of gases and substances in solution are written in an equilibrium constant expression
True
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relation that states that the values of the equilibrium constant expression, Kc are constant for a particular reaction at a given temperature, whatever equilibrium concentrations are substituted
Law of Mass Action
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If a system in chemical equilibrium is altered by a change of some condition, chemical reaction occurs to shift the equilibrium composition in a way that acts to reduce the effect of that change of condition.
Le Chatelier's Principle
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TRUE OR FALSE: A catalyst affects the equilibrium composition of a reaction mixture.
False. A catalyst merely speeds up the attainment of equilibrium.
139
a substance that changes the speed of a chemical reaction without itself undergoing a permanent chemical change in the process.
catalyst
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the process of producing ions out of a solution
ionization
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Theory stating that a substance can function as an acid only in the presence of a base; similarly, a substance can function as a base only in the presence of an acid.
Bronsted-Lowry Theory
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is the branch of physical chemistry which deals with the thermal changes accompanying chemical and physical transformations.
thermochemistry
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the substance of mixture of substances under study in which a change occurs
system
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are everything in the vicinity of the thermodynamic system.
surroundings
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is a chemical reaction or physical change in which heat is evolved
exothermic
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is a chemical reaction or physical change in which heat is absorbed
endothermic
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the experimental measurement of heat produced in chemical and physical processes.
calorimetry
148
a device used for measuring the heat evolved in the combustion of a
substance under constant volume conditions.
bomb calorimeter
149
amount of heat required to raise the temperature of the sample of
substance by 1.0 degC
heat capacity
150
is a property of a substance that can be used to obtain the heat absorbed or evolved in a chemical reaction (or physical change) at constant pressure
enthalpy
151
law states that the change in enthalpy for any chemical reaction is constant, whether the reaction occurs on one step or several steps.
Hess' Law: Law of Constant Heat Summation
152
enthalpy change when a reaction occurs with all reactants and products in their standard states
standard enthalpy of rxn
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the change in enthalpy that accompanies the formation of one mole of a substance from its elements, with all substances in their standard states.
standard enthalpy of formation
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amount of heat required to change a given mass of a substance from the solid state to the liquid state without change in temperature.
heat of fusion
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amount of heat required to change a given mass of a substance from the liquid state to the vapor state without change in temperature
heat of vaporization
156
is the flow of electric charges or transfer of electrons.
electric current
157
Conduction in which the charge is carried by ions. This will not occur unless the ions of the Electrolytes are free to move. It is exhibited principally by molten salts and by aqueous solutions of electrolytes.
electrolytic conduction
158
power developed by one ampere in flowing through a potential of one volt in one second
joule
159
the power developed by one ampere flowing through a potential difference of one volt.
watt
160
the energy required to move an electric charge from one point to another
electrical work
161
rate at which electrical work is done
electrical power
162
a device (used to measure emf) that has an adjustable voltage, which is varied until it just balances the cell voltage
potentiometer
163
a term used to designate an atom with a specific atomic number and mass number.
nuclide
164
an isotope that is radioactive, that is, it is undergoing nuclear changes with emission of radiation
radioisotope
165
energetic electrons emitted as a result of the conversion of a neutron to a proton in a radioactive nucleus
beta particles
166
particle with the same mass as an electron but with a positive charge; positive electron emitted as a result of the conversion of a proton to a neutron in a radioactive nucleus
positron
167
energy released when nucleons (protons and neutrons) are fused into an atomic nucleus. This energy replaces an equivalent quantity of matter.
nuclear binding energy
168
time required for one half of any given quantity of a radioactive substance to undergo decay
half-life
169
is a method of determining the age of a carbon-containing material based on the rate of decay of radioactive carbon-14
radiocarbon dating
170
Above Z = ____ the elements have no stable isotopes
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