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Module 1 - Pharmacy Licensure Exam (Phil) > General Chemistry > Flashcards

General Chemistry Flashcards

1
Q

A branch of physical science that studies the composition, structure, properties and change of matter

A

Chemistry

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2
Q

Deals with chemical processes that occur in living organisms

A

Biochemistry

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3
Q

Works with fundamental principles of physics and chemistry

A

Physical Chemistry

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4
Q

Separation and identification of chemical substances

A

Analytical Chemistry

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5
Q

Focuses on substances that contain carbon and hydrogen in combination with a few other elements

A

Organic Chemistry

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6
Q

Focuses on most of the elements other than carbon

A

Inorganic Chemistry

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7
Q

Anything that occupies space (or has volume), displays a property known as mass, and possess inertia; can be a pure chemical substance or a mixture of substances

A

Matter

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8
Q

Refers to the parts or components of a sample of matter and their relative proportions

A

Composition

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9
Q

The qualities or attributes that can be used to distinguish one sample of matter from others

A

Properties

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10
Q

one that a sample of matter displays without changing its composition

A

Physical property

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11
Q

a physical property of a system that does not depend on the system size or the amount of material in the system

A

Intensive property (bulk property)/intrinsic property

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12
Q

one that is additive for independent, non-interacting subsystems

A

Extensive property/extrinsic property

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13
Q

the ability (or inability) of a sample of matter to undergo a change in composition under stated conditions

A

Chemical property

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14
Q

a modern version of the metric system; a decimal system

A

SI = Système Internationale d’Unités (International System of Units)

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15
Q

Refers to how close a measured value is tothe accepted, or “real,” value

A

Accuracy

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16
Q

Refers to the degree of reproducibility of ameasured quantity

A

Precision

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17
Q

Not determined by chance but is introduced by an inaccuracy (as of observation ormeasurement) inherent in the system

A

Systematic Errors

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18
Q

Caused by inherently unpredictablefluctuations in the readings of a measurement apparatus or in the experimenter’s interpretation of the instrumental reading

A

Random errors

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19
Q

describes the QUANTITY OF METTER in an object; SI unit, kilogram (kg)

A

Mass (𝒎)

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20
Q

the force of gravity on an object 𝑊=𝑔×𝑚

A

Weight (𝑾)

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21
Q

those of length, mass, time, temperature, amount of substance, electric current, and luminous intensity (SI units)

A

Fundamental (base) quantities

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22
Q

combinations of certain of these fundamental quantities; e.g., velocity (m/s), volume (cm3 or cc or mL), density (g/mL)

A

Derived units

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23
Q

term applied to elements and compounds (whose composition and properties are uniform throughout a given sample and from one sample to another)

A

Substance

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24
Q

a substance made up of only a single type of atom distinguished by its atomic number, which is the number of protons in its atomic nucleus; divided into metals, metalloids, and nonmetals; 118 known chemical elements (as of 2010); 98 chemical elements occur naturally on earth

A

Element

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25
Q

the smallest constituent unit of ordinary matter that has the properties of a chemical element

A

Atom

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26
Q

substance in which atoms of different elements are combined with one another

A

Compound

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27
Q

the smallest entity having the same proportions of the constituent atoms as does the compound as a whole

A

Molecule

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28
Q

made of two or more types of substances

A

Mixtures

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29
Q

uniform in composition and properties throughout a given sample, but the composition and properties may vary from one sample to another

A

Solutions (homogeneous mixtures)

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30
Q

whose components separate into distinct regions; the composition and physical properties vary from one part of the mixture to another

A

Heterogeneous mixtures

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31
Q

occurs when a sample of matter changes its physical appearance; its composition remains unchanged; includes changes in texture, color, temperature, shape, state

A

Physical change

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32
Q

when one or more samples of matter are converted to new samples with different compositions; indications include change in temperature, change in color, noticeable odor, formation of a precipitate, formation of bubbles

A

Chemical change

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33
Q

State of matter that maintains a fixed volume and shape,with component particles (atoms, molecules or ions) [IFA] close together and fixed into place

Molecular Motion: Vibration

A

Solid

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34
Q

States of Matter that maintains a fixed volume, but has a variable shape that adapts to fit its container. Its particles [IFA] are still close together but move freely

Molecular Motion: Gliding

A

Liquid

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35
Q

States of Matter: has both variable volume and shape, adapting both to fit its container. Its particles [IFA] are neither close together nor fixed in place

Molecular Motion: Constant random motion

A

Gas

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36
Q

States of Matter: has variable volume and shape, but as well as neutral atoms, it contains a significant number of ions and electrons, both of which can move around freely

A

Plasma

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37
Q

The state or phase of a given set of matter can change depending on pressure and temperature conditions.

A

State of Matter

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38
Q

Phase Transitions: Solid to Liquid

A

Melting (Fusion)

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39
Q

Phase Transitions: Liquid to Gas

A

Vaporization

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40
Q

Phase Transitions: Gas to Plasma

A

Ionization

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41
Q

Phase Transitions: Plasma to Gas

A

Deionization

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42
Q

Phase Transitions: Gas to Liquid

A

Condensation

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43
Q

Phase Transitions: Liquid to Solid

A

Freezing

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44
Q

Phase Transitions: Solid to Gas

A

Sublimation

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45
Q

Phase Transitions: Gas to Solid

A

Deposition

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46
Q

Chemical Reaction: two or more simple substances combine to form a more complex substance

A

Synthesis

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47
Q

Chemical Reaction: when a more complex substance breaks down into its more simple parts

A

Decomposition

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48
Q

Chemical Reaction: a single uncombined element replaces another in a compound, one element trades places with another element in a compound

A

Single Replacement

49
Q

Chemical Reaction: the anions and cations of two compounds switch places and form two entirely different compounds

A

Double Replacement

50
Q

Chemical Reaction: involves a transfer of protons (H+) from one species (the acid) to another (the base)

A

Neutralization (acid-base reaction)

51
Q

Chemical Reaction: the formation of a solid in a solution or inside another solid during a chemical reaction

A

Precipitation

52
Q

Chemical Reaction: when ligands (with lone pairs) react with a metal atom (with empty orbitals) to form a coordination complex

A

Complexation

53
Q

Chemical Reaction: transfer of electrons from one involved species (reducing agents) to another (oxidizing agent); the former species is oxidized and the latter is reduced

A

Reduction and oxidation (redox reaction)

54
Q

Chemical Reaction: when atoms and molecules absorb energy (photons) of the illumination light and convert into an excited state; energy is released by breaking chemical bonds

A

Photochemical reaction

55
Q

Chemical Reaction: very slow reaction between solids

A

Solid-state reaction

56
Q

Chemical Reaction: surfaces at very low pressure such as ultra-high vacuum

A

Reaction at the solid-gas interphase

57
Q

The total mass of substances present after a chemical reaction is the same as the total mass of substances before the reaction.

A

Law of Conservation of Mass

58
Q

All samples of a compound have the same composition—the same proportions by mass of the constituent elements.

A

Law of Constant Composition (Law of Definite Proportions)

59
Q

If two elements can be combined to form a number of possible compounds, then the ratios of the masses of the second element which combine with a fixed mass of the first element will be ratios of small whole numbers.

A

Law of Multiple Proportions

60
Q

Atomic Models: all matter was composed of small indivisible particles called atoms (atomos, Gr. “uncuttable”)

A

Democritus

61
Q

Atomic Models: “billiard ball model” (1808); proposed that each chemical element is composed of atoms of a single, unique type, and though they cannot be altered or destroyed by chemical means, they can combine to form more complex structures

A

John Dalton

62
Q

Atomic Models: “plum pudding model” (1903); discovered the electron through his work on cathode rays

A

J.J. Thomson

63
Q

Atomic Models: “nuclear/planetary model” (1911); discovered that most of the mass and positive charge of an atom is concentrated in a very small fraction of its volume, which he assumed to be at the very center

A

Ernest Rutherford

64
Q

A type of particle that carry two fundamental units of charge; same mass as He

A

Alpha (α) particles

65
Q

A type of negatively charged particles produced by changes occurring within the nuclei of radioactive atoms; same properties as electrons

A

Beta (β) particles

66
Q

Atomic Models: “shell model” (1923); electrons are arranged around the nucleus in discrete energy levels or shells

A

Neils Bohr

67
Q

Atomic Models: “electron cloud model”; assumes that the electron is a wave and tries to describe the regions in space, or orbitals, where electrons are most likely to be found

A

Erwin Schrödinger

68
Q

made the first cathode ray tube (CRT)

A

Michael Faraday

69
Q

determined the electronic charge e through a series of “oil drop” experiments; e = –1.6022x10^-19 C me = 9.1094x10^-28 g

A

Robert Millikan

70
Q

discovered X-rays

A

Wilhelm Roentgen

71
Q

discovered radioactivity

A

Antoine Henri Becquerel

72
Q

discovered gamma (γ) radiation, which is not made of particles

A

Paul Villard

73
Q

discovered transmutation (fundamental changes at the subatomic level in which one element is changed into another in radioactive decay

A

Frederick Soddy (and Rutherford)

74
Q

(1932) discovered neutral particles called neutrons that originate from the nuclei of atoms

A

James Chadwick

75
Q

The more precisely the position is determined, the less precisely the momentum is known in this instant, and vice versa.

A

Heisenberg’s Uncertainty Principle

76
Q

the sets of numerical values which give acceptable solutions to the Schrödinger wave equation for the hydrogen atom

A

Quantum Numbers

77
Q

Quantum Numbers: the electron shell, or energy level, of an atom

A

Principal quantum number (n)

78
Q

Quantum Numbers: describes the subshell: l = 0 (s orbital); 1 (p orbital), 2 (d orbital), 3 (f orbital)

A

Azimuthal quantum number (l)/ angular quantum number or orbital quantum number;

79
Q

Quantum Numbers: describes the specific orbital (or “cloud”) within that subshell; orientation of the subshell’s shape; range from −l to l

A

Magnetic quantum number (ml)

80
Q

Quantum Numbers: describes the spin (intrinsic angular momentum) of the electron within that orbital

A

Spin projection quantum number (ms)

81
Q

States that it is impossible for two electrons of an atom to have the same values of the four quantum numbers (n, l, ml and ms).

A

Pauli’s Exclusion Principle (Wolfgang Pauli (1925))

82
Q

-coined by Robert Mulliken in 1932 as an abbreviation for one-electron orbital wave function - mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom - the region in space where an electron is most likely to be found

A

Atomic Orbitals: sharp (s orbital, l = 0) principal (p orbital, l = 1) diffuse (d orbital, l = 2) fundamental/fine (f orbital, l = 3)

83
Q

The distribution of electrons of an atom or molecule in atomic or molecular orbitals

A

Electron Configuration

84
Q

Electron Configuration: (from the German aufbau, “building up, construction”) – the lowest-energy orbitals are filled before electrons are placed in higher-energy orbitals

A

Aufbau’s principle

85
Q

“bus seat rule”; the orbitals of the subshell are each occupied singly with electrons of parallel spin before double occupation occurs

A

Hund’s rule of maximum multiplicity

86
Q

exactly 1/12 of the mass of an unbound neutral atom of carbon-12 in its nuclear and electronic ground state; equivalent to 1 Da (dalton)

A

Unified atomic mass unit (amu or u)

87
Q

the number of protons in an atom

A

Atomic number (proton number, Z)

88
Q

the total number of protons and neutrons (nucleons)

A

Mass number (A)

89
Q

the number of neutrons; A – Z

A

Neutron number

90
Q

the average of the isotopic masses weighted according to the naturally occurring abundances of the isotopes of the element

A

Atomic mass (atomic weight)

91
Q

the general term used to describe an atom with a particular atomic number and mass number

A

Nuclides

92
Q

two or more atoms having the same atomic number (Z) or number of protons, but different mass numbers (A) or number of neutrons

A

Isotopes

93
Q

nuclides of equal number of neutrons, but different number of protons

A

Isotones

94
Q

atoms of different chemical elements that have the same number of nucleons; differ in atomic number, but have the same mass number

A

Isobars

95
Q

nuclides with equal proton number and equal mass number, but different states of excitation

A

Nuclear isomers

96
Q

neutron and proton number exchanged

A

Mirror nuclei

97
Q

unstable and radioactive nuclides

A

Radionuclides

98
Q

decay products

A

Radiogenic nuclides

99
Q

an elementary particle and a fundamental constituent of matter

A

Quark

100
Q

composite particles made of quarks, e.g., protons (2 up quarks + 1 down quark) and neutrons (3 quarks)

A

Hadron

101
Q

composite subatomic particles made up of 3 quarks; e.g., neutron

A

Baryon

102
Q

any baryon containing on or more strange quarks, but no charm, bottom, or top quark

A

Hyperon

103
Q

composed of one quark and one antiquark, bound together by a strong interaction; about 2/3 the size of a proton or neutron; charged mesons decay to form electrons and neutrinos; uncharged mesons may 67 decay to photons

A

Meson

104
Q

an elementary, half-integer spin particle that does not undergo strong interactions; e.g., electron

A

Lepton

105
Q

neutral leptons

A

Neutrino

106
Q

a tabular arrangement of the chemical elements, organized on the basis of their atomic number, electron configurations, and recurring chemical properties

A

Periodic Table of Elements

107
Q

Periodic Table of Elements: places similar elements

A

vertical groups (or families)

108
Q

Periodic Table of Elements: horizontal rows

A

periods

109
Q

published a list of 33 elements grouped into gases, metals, nonmetals, and earths

A

Antoine Lavoisier

110
Q

Law of Triads (1829), e.g., Li, Na, K were grouped together as soft, reactive metals

A

Johann Wolfgang Döbereiner

111
Q

(1858) observed valency

A

August Kekulé

112
Q

(1862) first noticed the periodicity of elements; published an early form of periodic table called the telluric helix (or screw)

A

Alexandre-Emile Béguyer de Chancourtois

113
Q

Law of Octaves (1863 to 1866)

A

John Newlands

114
Q

Categories of Elements: generally malleable and ductile; good conductors of heat and electricity; lustrous and shiny

A

Metals

115
Q

Categories of Elements: “opposite” properties of metals

A

Nonmetals

116
Q

Categories of Elements: have some metallic and some nonmetallic properties; e.g., B, Si, Ge, As, Sb, Te, Po, At

A

Metalloids

117
Q

Categories of Elements: have complete octet; e.g., He, Ne, Ar, Kr, Xe, Rn

A

Noble gas

118
Q

Categories of Elements: the series of 14 elements that follow 57La at Period 6

A

Lanthanides

119
Q

Categories of Elements: the series of 14 elements that follow 89Ac at Period 7

A

Actinides

Module 1 - Pharmacy Licensure Exam (Phil) (9 decks)

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