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General Objectives Flashcards

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1
Q

Spontaneous disintegration of unstable atomic nucleus with accompanying emission of radiation

A

Radioactivity

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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

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3
Q

States that the properties of elements are periodic functions of their atomic numbers

A

Periodic Law

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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

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5
Q

Smallest increment of radiant energy that may be absorbed or emitted

A

Quanta

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6
Q

Wave function of an electron

A

Orbital

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7
Q

Theory that organic substances can only be produced from other organic substances

A

Vital Force Theory

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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

A

Chemistry

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9
Q

Physical material of the universe; anything that occupies space and has mass

A

Matter

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10
Q

Properties w/c can be measured and observed w/o changing the basic identity of the substance

A

Physical

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11
Q

Properties that describe the way a substance may change or react to form other substances

A

Chemical

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12
Q

Characteristics of any sample of a substance regardless of the size or shape of the sample

A

Intrinsic or Intensive

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13
Q

Accidental properties; depend on the amount of material

A

Extrinsic or extensive

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14
Q

Homogenous material consisting of one particular kind of matter; matter that has a definite composition and distinct properties

A

Pure substance

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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

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16
Q

Substances that cannot be separated into simpler substances by chemical means

A

Elements

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17
Q

Substances composed of two or more elements united chemically in fixed proportions

A

Compounds

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18
Q

Substance able to donate a H+ ion; proton donor

A

Acid

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19
Q

Produces an excess OH- (aq) ions when dissolved in water; proton acceptor

A

Base

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20
Q

Ionic compound formed by replacing one or more H+ of an acid by other cations

A

Salt

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21
Q

Material in which no differing parts can be distinguished

A

Homogenous

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22
Q

Materials with differing parts may be separated physically

A

Heterogeneous

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23
Q

Mixtures containing particles larger than normal solutes, invisible to the eye and microscope but visible in ultramicroscope

A

Colloidal suspension

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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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25
Q

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

A

LAW OF CONSERVATION OF MATTER

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26
Q

Law stating that energy is neither created nor destroyed in any transformation but is transformed from one form to another

A

LAW OF CONSERVATION OF ENERGY

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27
Q

states that every sample of a given substance always contains the same proportion by weight of all its constituent elements

A

LAW OF DEFINITE PROPORTIONS OR DEFINITE
COMPOSITION

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28
Q

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.

A

LAW OF MULTIPLE PROPORTIONS

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29
Q

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

A

Physical Chemistry

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30
Q

is concerned with the
separation, identification and composition of all
kinds of matter

A

analytical chemistry

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31
Q

involves the separation and identification of the individual components of materials. It answers the question, “What is
present?”

A

qualitative analysis

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32
Q

is concerned with how much of each component is present

A

quantitative analysis

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33
Q

study of carbon-containing compounds; This branch of chemistry now deals with commonly used synthetic substances such as plastics, drugs, dyes, explosives and detergents.

A

Organic chemistry

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34
Q

covers the chemistry of all elements and their compounds with the exception of carbon and its compounds

A

Inorganic chemistry

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35
Q

branch of chemistry which
includes the study of the materials and processes
that occur in living organisms. These materials are
largely organic (carbon) compounds

A

Biochemistry

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36
Q

deals with the changes in the nuclei of atoms and the used of these changes, especially in the study of how substances react.

A

Nuclear chemistry

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37
Q

form of energy which flows spontaneously from a substance of higher temperature to one of lower temperature.

A

heat

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38
Q

measure of the intensity of heat; intensive quantity that defines the direction and rate of heat flow; hotness or coldness of a body

A

temperature

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39
Q

temp scale is based on the freezing and boiling point of water

A

relative

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40
Q

temp scale based on the quantity of kinetic energy that molecules have

A

absolute

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41
Q

amount of matter found in a substance; measure of a substance’s resistance to the change in velocity

A

mass

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42
Q

refers to the force with which an object is attracted to the earth

A

weight

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43
Q

ratio of the mass of the substance to the mass of water that occupies the same volume

A

relative density

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44
Q

quantity of heat required to raise the temperature of one gram of a substance by 1 degC

A

specific heat

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45
Q

quantity of heat required to raise the temperature of 1 gram of water by 1 degC

A

calorie

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46
Q

device used to measure the quantity of heat exchanged between
the thermodynamic system and its surroundings

A

calorimeter

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47
Q

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

A

law of heat

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48
Q

Amount of heat lost by one body is equal to the amount of heat gained by another body

A

law of heat exchange

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49
Q

smallest unit of element that cannot be further subdivided and is capable of taking part in a chemical reaction; basic building blocks of matter

A

atom

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50
Q

smallest unit of element or chemical compound capable of free existence (combination of two or more atoms)

A

molecule

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51
Q

Dalton’s Atomic Theory of matter

A
  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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52
Q

high energy radiation similar to X-rays and does not consist of particles

A

gamma radiation

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53
Q

high speed electrons which could be considered as the radioactive
equivalent of cathode rays (-1 charge)

A

beta radiaton

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54
Q

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

A

alpha radiation

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55
Q

number of protons in the nucleus

A

atomic number

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56
Q

total number of protons and neutrons (nucleons)

A

mass number

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57
Q

atoms of the same element containing different number of neutrons and therefore having different masses

A

isotopes

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58
Q

the arrangement of elements in order of increasing atomic number, with elements having similar properties placed in vertical columns

A

periodic table

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59
Q

vertical columns bringing together elements with similar properties

A

family or group

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60
Q

horizontal rows of the table arranged in order of increasing atomic number

A

period

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61
Q

elements (with the exemption of hydrogen) found on the left side of the heavy ladder-like line in the periodic table

A

metals

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62
Q

elements found on the right side of the heavy ladder-like in the periodic table

A

non-metals

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63
Q

elements that lie along the heavy ladder-like line separating the metals from the nonmetals in the periodic table

A

metalloids or amphoteric elements

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64
Q

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.

A

inert gas

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65
Q

These elements partially occupy the s and the d block. These are
known as the s and p block elements; A family

A

representative elements

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66
Q

These elements are characterized by atoms in which an inner d-level is present but is not filled up to capacity.

A

transition elements

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67
Q

These elements are characterized by atoms which contain incompletely filled levels as well as incompletely filled f-levels.

A

inner transition elements

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68
Q

energy required to remove the most loosely held electron from a gaseous atom when it is in its ground state,

A

ionization energy

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69
Q

System of naming substances or compounds.

A

chemical nomenclature

70
Q

symbolic representation of elements; consists of either one or two letters

A

chemical symbol

71
Q

a substance formed from two or more elements; a substance that can be decomposed into two or more simpler substances by ordinary chemical means

A

chemical compound

72
Q

Any molecule that is made up of two atoms: H2 , O2 , N2 , F2 ,
Cl2 , Br 2 , I2

A

Diatomic molecules

73
Q

a shorthand notation using chemical symbols and numerical subscripts to represent the composition of a substance

A

chemical formula

74
Q

special valence number assigned to each element to indicate the number of electrons oxidation state/valence gained, lost or shared
unequally

A

oxidation number/charge

75
Q

represent the number of electrons in the outermost energy level which are largely responsible for the chemical behavior of an element

A

valence electron

76
Q

an ion consisting of two or more atoms chemically bonded together and carrying a net electric charge

A

polyatomic ion

77
Q

an electrically charged particle obtained from an atom or a chemically bonded group of atoms by adding or removing electrons

A

ion

78
Q

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.

A

chemical reaction

79
Q

a shorthand way of representing a chemical reaction using chemical formulas to indicate the reactants and products

A

chemical equation

80
Q

a type of reaction wherein a single more complex product is formed by the combination of two or more simpler substances.

A

direct combination or synthesis

81
Q

a reaction wherein a compound is broken down into two or
more simpler substances.

A

decomposition or analysis

82
Q

A reaction wherein an element or an ion displaces another element or ion in a compound.

A

single displacement

83
Q

a reaction wherein compounds interchange ions or radicals. Compounds exchange positive and negative parts and results in the formation of different compounds.

A

metathesis or double displacement

84
Q

the calculation of the quantities of materials consumed and produced in chemical reactions

A

chemical stoichiometry

85
Q

defined as the number of carbon atoms in exactly 12 grams of pure C-12 atom; counting unit of a chemist

A

mole

86
Q

the mass in grams of one mole of molecules or formula unit of a substance; also called molecular weight

A

molar mass

87
Q

formula which shows the simplest whole number ratio of atoms in a compound

A

empirical formula

88
Q

the exact formula of a molecule giving the types of atoms and the number of each type

A

molecular formula

89
Q

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

A

hydrate

90
Q

the ratio of moles of one substance to moles of another substance in a balanced chemical equation

A

mole ratio

91
Q

the reactant that is completely consumed when a reaction is run to completion

A

limiting reactant

92
Q

the measured quantity of product obtained in a chemical reaction less than theoretical

A

actual yield

93
Q

the quantity of product calculated to result from a chemical reaction

A

theoretical yield

94
Q

defined as the force exerted per unit area

A

pressure

95
Q

At constant temperature, the volume of a sample of a gas varies inversely with the pressure

A

Boyle’s Law

96
Q

The volume of any sample of a gas varies directly with the absolute temperature, if the pressure is held constant.

A

Charles’ Law

97
Q

The pressure of a gas varies directly with the absolute temperature when the volume is held constant.

A

Amonton’s Law

98
Q

Equal number of molecules are contained in equal volumes of different gases if the temperature is the same.

A

Avogadro’s Law

99
Q

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.

A

Ideal Gas Law

100
Q

term used to describe the mixing of gases

A

diffusion

101
Q

term used to describe the passage of gas through a tiny orifice into an evacuated chamber

A

effusion

102
Q

states that the effusion rate of a gas is inversely proportional to the square root of the mass of its particles

A

Graham’s Law

103
Q

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.

A

Gay Lussac’s Law of Combining Volumes

104
Q

dissolving medium of a solution; component of a solution that is greater in quantity

A

solvent

105
Q

universal solvent

A

water

106
Q

substance dissolved in a solvent to make a solution component of a solution that is present in relatively smaller quantity

A

solute

107
Q

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

A

solubility

108
Q

an increase in temperature ________ the solubility of most solid solutes dissolved in liquid solvent

A

increases

109
Q

an increase in temperature decreases the solubility of gaseous
solutes dissolved in _______ solvent

A

liquid

110
Q

for _________, the greater the pressure, the higher the solubility

A

gases

111
Q

contains the maximum amount of solute that can be dissolved under the conditions at which the solution exists

A

saturated solution

112
Q

a solution that is not in equilibrium with respect to a given dissolved substance and in which more of the substance can dissolve

A

unsaturated solution

113
Q

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

A

supersaturated solution

114
Q

solution where a small amount of solute is present in solution relative to the amount that could dissolve

A

dilute solution

115
Q

solution that contains a relatively large amount of solute relative to the amount that could dissolve

A

concentrated solution

116
Q

substances which dissolves in any amount in each other

A

miscible substances

117
Q

substances which have limited solubility in each other

A

partially miscible

118
Q

substances which do not dissolve in each other and forms two separate layers upon mixing

A

immiscible

119
Q

solutions in which water is the solvent

A

aqueous solution

120
Q

concentration unit most often used in a chemical laboratory; ratio giving the number of moles (n) of solute per liter of solution

A

molarity

121
Q

finds use in experimental situations where changes in temperature are of concern; ratio giving the number of moles of solute per kg of solvent

A

molality

122
Q

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

A

normality

123
Q

is the process in which more solvent is added to a solution in order to lower the concentration of the solution.

A

dilution

124
Q

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.

A

Colligative Property Law

125
Q

The freezing point of a solution is always _________ than the freezing point of the pure solvent.

A

lower

126
Q

The temperature at which a solution boils is ________ than that of the pure solvent if the solute is nonvolatile.

A

higher

127
Q

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

A

Raoult’s law

128
Q

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.

A

osmosis

129
Q

pressure needed to prevent the flow of solvent into the solution through a semi-permeable membrane

A

osmotic pressure

130
Q

the change in concentration of a reactant or product per unit time

A

reaction rate

131
Q

set of postulates used to explain how chemical reactions occur.

A

collision theory

132
Q

Collision Theory fundamental postulates

A
  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.
133
Q

The minimum energy of collision required for two molecules to react

A

Activation energy

134
Q

state reached by a reaction mixture when the rate of the forward reaction and that of the reverse reaction have become equal.

A

chemical equilibrium

135
Q

TRUE OR FALSE: Only concentrations of gases and substances in solution are written in an equilibrium constant expression

A

True

136
Q

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

A

Law of Mass Action

137
Q

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.

A

Le Chatelier’s Principle

138
Q

TRUE OR FALSE: A catalyst affects the equilibrium composition of a reaction mixture.

A

False. A catalyst merely speeds up the attainment of equilibrium.

139
Q

a substance that changes the speed of a chemical reaction without itself undergoing a permanent chemical change in the process.

A

catalyst

140
Q

the process of producing ions out of a solution

A

ionization

141
Q

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.

A

Bronsted-Lowry Theory

142
Q

is the branch of physical chemistry which deals with the thermal changes accompanying chemical and physical transformations.

A

thermochemistry

143
Q

the substance of mixture of substances under study in which a change occurs

A

system

144
Q

are everything in the vicinity of the thermodynamic system.

A

surroundings

145
Q

is a chemical reaction or physical change in which heat is evolved

A

exothermic

146
Q

is a chemical reaction or physical change in which heat is absorbed

A

endothermic

147
Q

the experimental measurement of heat produced in chemical and physical processes.

A

calorimetry

148
Q

a device used for measuring the heat evolved in the combustion of a
substance under constant volume conditions.

A

bomb calorimeter

149
Q

amount of heat required to raise the temperature of the sample of
substance by 1.0 degC

A

heat capacity

150
Q

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

A

enthalpy

151
Q

law states that the change in enthalpy for any chemical reaction is constant, whether the reaction occurs on one step or several steps.

A

Hess’ Law: Law of Constant Heat Summation

152
Q

enthalpy change when a reaction occurs with all reactants and products in their standard states

A

standard enthalpy of rxn

153
Q

the change in enthalpy that accompanies the formation of one mole of a substance from its elements, with all substances in their standard states.

A

standard enthalpy of formation

154
Q

amount of heat required to change a given mass of a substance from the solid state to the liquid state without change in temperature.

A

heat of fusion

155
Q

amount of heat required to change a given mass of a substance from the liquid state to the vapor state without change in temperature

A

heat of vaporization

156
Q

is the flow of electric charges or transfer of electrons.

A

electric current

157
Q

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.

A

electrolytic conduction

158
Q

power developed by one ampere in flowing through a potential of one volt in one second

A

joule

159
Q

the power developed by one ampere flowing through a potential difference of one volt.

A

watt

160
Q

the energy required to move an electric charge from one point to another

A

electrical work

161
Q

rate at which electrical work is done

A

electrical power

162
Q

a device (used to measure emf) that has an adjustable voltage, which is varied until it just balances the cell voltage

A

potentiometer

163
Q

a term used to designate an atom with a specific atomic number and mass number.

A

nuclide

164
Q

an isotope that is radioactive, that is, it is undergoing nuclear changes with emission of radiation

A

radioisotope

165
Q

energetic electrons emitted as a result of the conversion of a neutron to a proton in a radioactive nucleus

A

beta particles

166
Q

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

A

positron

167
Q

energy released when nucleons (protons and neutrons) are fused into an atomic nucleus. This energy replaces an equivalent quantity of matter.

A

nuclear binding energy

168
Q

time required for one half of any given quantity of a radioactive substance to undergo decay

A

half-life

169
Q

is a method of determining the age of a carbon-containing material based on the rate of decay of radioactive carbon-14

A

radiocarbon dating

170
Q

Above Z = ____ the elements have no stable isotopes

A

83

Gen Chem (2 decks)

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