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Chemistry Flashcards

1
Q

Chemistry

A

The physical science that deals with the composition, properties, and changes in matter

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2
Q

Observation

A

A direct form of knowledge obtained by means of one of your five senses

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3
Q

Qualitative observation

A

Qualities of matter or changes in matter

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4
Q

Quantitive observation

A

Quantities of matter or the degree of change in matter

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5
Q

Interpretation

A

An indirect form of knowledge that builds on a concept or an experience to further describe or explain an observation

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6
Q

Empirical knowledge

A

Knowledge gained through observation

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7
Q

Theoretical knowledge

A

Explains and describes scientific observations in terms of ideas; not observable

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8
Q

Graphs

A

Visual presentations of observations

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9
Q

Empirical hypotheses

A

Preliminary generalizations that require further testing

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10
Q

Empirical definitions

A

Statements that define an object or a process in terms of observable properties

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11
Q

Generalizations

A

Statements that summarize a limited number of empirical results

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12
Q

Scientific laws

A

Statements of major concepts based on a large body of empirical knowledge

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13
Q

The law of conservation of mass

A

In any physical or chemical change, the total initial mass of reactant(s) is equal to the total final mass of product(s)

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14
Q

Technology

A

Skills, processes, and equipment required to manufacture useful products or perform useful tasks

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15
Q

Science

A

The study of the natural world with the goal of describing, explaining, and predicting substances and changes

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16
Q

Homogeneous Mixtures

A

Mixtures that contain pure substances evenly distributed throughout the mixture - Uniform, only one phase

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17
Q

Heterogeneous Mixtures

A

Mixtures that have an uneven distribution of pure substances - Non-uniform, may be more than one phase

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18
Q

Element

A

A simple pure substance that cannot be broken down into simpler substances by ordinary chemical means

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19
Q

Matter

A

Anything that has mass and occupies space

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20
Q

Pure substances

A

Composition is constant and uniform

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21
Q

Mixtures

A

Composition is variable and may or may not be uniform throughout the sample

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22
Q

Entity

A

A general term including particles (sub-atomic entities such as protons, electrons, neutrons), atoms, ions, molecules, and formula units.

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23
Q

Atom

A

Theoretically the smallest entity of an element that is still characteristic.

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24
Q

Compounds

A

Theoretically contain atoms of more than one element combined in a definite fixed proportion

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25
Q

Chemical formula

A

Consists of element symbols representing the entities and their proportions present in the substance

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26
Q

Who created a periodic table?

A

Dmitri Mendeleev, a Russian chemist

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27
Q

Periodic law

A

Chemical and physical properties of elements repeat themselves in regular intervals, when the elements are arranged in order of increasing atomic number

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28
Q

Family/Group of elements

A

Has similar chemical properties and includes the elements in a vertical column in the main part of the table

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29
Q

Period

A

A horizontal row of elements whose properties gradually change from metallic to nonmetallic from left to right along the row

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30
Q

Where are metals located on the periodic table?

A

To the left of the staircase line

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31
Q

Where are non-metals located on the periodic table

A

To the right of the staircase line

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32
Q

What are semi-metals (Metalloids) and where are they located on the periodic table?

A

A class of elements that are distributed along the staircase line

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33
Q

IUPAC

A

International Union of Pure and Applied Chemistry

A governing body for scientific communication and has defined a set of standard conditions

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34
Q

SATP

A

Standard Ambient Temperature and Pressure

Under these ambient (surrounding) conditions, the materials are at a temperature of 25ºC and a pressure of 100kPa

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35
Q

Properties of metals

A

Shiny, bendable, good conductors of heat and electricity

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36
Q

Properties of nonmetals

A

Not shiny, not bendable, generally not good conductors of heat and electricity in their solid form
At SATP most nonmetals are gases and few are solids Solid nonmetals are brittle and lack lustre
Most nonmetals consist in compounds

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37
Q

Alkali metals

A

Group 1 elements. They are soft, silver-colored metals that react violently with water to form basic solutions. The most reactive alkali metals are cesium and francium

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38
Q

Alkaline-earth metals

A

Group 2 elements. They are light-reactive metals that form oxide coatings when exposed to air

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39
Q

Halogens

A

Elements in Group 17. They are all extremely reactive, with fluorine being the most reactive

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40
Q

Noble Gases

A

Elements in Group 18. They are special because of their extremely low chemical reactivity

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41
Q

Main Group Elements

A

The elements in Groups 1, 2, and 12 to 18. Of all the elements, the main group elements best follow the periodic law

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42
Q

Transition elements

A

The elements in Groups 3 to 11. These elements exhibit a wide range of chemical and physical properties

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43
Q

Lanthanoids

A

Elements with atomic numbers 58 to 71

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44
Q

Rare earth elements

A

Include lanthanoids and yttrium and scandium

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45
Q

Actinoids

A

Elements with atomic numbers 90 to 103

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46
Q

Transuranic elements

A

The synthetic elements that have atomic numbers of 93 or greater (Beyond Uranium)

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47
Q

Electronegativity

A

A number that describes the relative ability of an atom to attract a pair of bonding electrons in its valence level

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48
Q

Theoretical descriptions

A

Specific descriptive statements based on theories or models

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49
Q

Theoretical hypotheses

A

Ideas that are untested or extremely tentative

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50
Q

Theoretical Definitions

A

General statements that characterize the nature of a substance or process in terms of a non-observable idea

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51
Q

Theories

A

Comprehensive sets of ideas based on general principles that explain a large number of observations

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52
Q

Analogies

A

Comparisons that communicate an idea in more familiar or recognizable terms

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53
Q

Models

A

Physical, graphic, or mental representations used to communicate an abstract idea

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54
Q

What characteristics must a theory have in order to be accepted by the scientific community?

A

Must:
Describe observations in terms of non-observable ideas
Explain observations by means of ideas
Predict results in future experiments that have not yet been tried
Be as simple as possible in concept and application

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55
Q

Mass number

A

The number of protons plus neutrons in their nucleus

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56
Q

Atomic number

A

The characteristic number of protons in the nucleus of atoms of that element

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57
Q

Ions

A

Have an electrical charge

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58
Q

Monatomic ions

A

Single atoms that have gained or lost electrons

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59
Q

Cations

A

Positively charged ions

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60
Q

Negatively charged ion

A

Anions

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61
Q

Verified prediction

A

If the evidence agrees within reasonable experimental error with the prediction

62
Q

Falsified

A

If the evidence obviously contradicts the prediction

63
Q

What are three possible strategies concerning unacceptable theories?

A

Restrict - Treat the conflicting evidence as an exception and use the existing theory within a restricted range of situations
Revise - The new evidence becomes part of an improved theory (most common)
Replace - Replace the existing theory with a totally new concept.

64
Q

Ionic compounds

A

Metal-Nonmetal combinations

65
Q

Molecular compounds

A

Nonmetal-Nonmetal combinations

66
Q

Metal-Metal combinations

A

Alloys and inter-metallic compounds

67
Q

Diagnostic test

A

Laboratory procedure conducted to identify or classify chemicals

68
Q

Empirical definitions

A

A list of empirical properties that define a class of chemicals

69
Q

Difference between Ionic compounds and Molecular compounds

A

At SATP:
Ionic solids
Molecular varied

When dissolved in water:
Ionic conducts
Molecular generally not

70
Q

Acids

A

Pure compounds at SATP that form conducting aqueous solutions that turn blue litmus paper red
Acids exhibit properties only when dissolved
Have properties of molecular compounds
Start with hydrogen or end in COOH

71
Q

Bases

A

Compounds whose aqueous solutions make red litmus paper turn blue

72
Q

Neutral

A

Compounds whose aqueous solutions do not affect litmus paper

73
Q

Multi-valent

A

More than one type of ion

74
Q

Polyatomic ions

A

Ions containing a group of atoms with a net positive or negative charge

75
Q

Formula unit

A

Of an ionic compound is a representation of the simplest whole number ratio of ions

76
Q

Empirical formula

A

The simplest ratio formula

77
Q

Molecule

A

Nonmetal atoms share electrons and the sharing holds the atoms together

78
Q

Molecular formula

A

Indicates the number of atoms of each kind in a molecule

79
Q

Water

A

H2O/HOH

80
Q

Hydrogen peroxide

A

H2O2

81
Q

Ammonia

A

NH3

82
Q

Glucose

A

C6H12O6

83
Q

Sucrose

A

C12H22O11

84
Q

Methane

A

CH4

85
Q

Propane

A

C3H8

86
Q

Octane

A

C8H18

87
Q

Methanol

A

CH3OH

88
Q

Ethanol

A

C2H5OH

89
Q

Hydrogen sulfide

A

H2S

90
Q

Which perspective leads to researching and explaining natural phenomena?

A

Scientific

91
Q

Which perspective is concerned with the development and use of machines, instruments, and processes that have a social purpose?

A

Technological

92
Q

Which perspective considers relationships between living organisms and the environment?

A

Ecological

93
Q

Which perspective focuses on the production, distribution, and consumption of wealth?

A

Economical

94
Q

Which perspective involves governments, vote-getting actions or arguments based on ideology?

A

Political

95
Q

Physical change

A

Fundamental entities remain the same

96
Q

Chemical change

A

Change in chemical bonding

97
Q

Nuclear change

A

Create entirely new atomic entities

98
Q

Kinetic molecular theory

A

Smallest entities of a substance are in continuous motion

99
Q

Diagnostic test

A

Short, specific test with expected evidence to see if a substance is present

100
Q

Avogadro’s number

A

6.02 x 10^23

101
Q

mol

A

Abbreviation for mole, one substance in the atomic quantity of Avogadro’s number

102
Q

Solution

A

Homogeneous mixture of a solute

103
Q

Solute

A

A substance dissolved

104
Q

Solvent

A

Substance (usually liquid) doing the dissolving

105
Q

Solubility

A

Maximum quantity of a substance that will dissolve in a solvent at a given temperature

106
Q

Precipitate

A

Solid substances formed from reactions in solution

107
Q

Structural formula

A

The illustration of a dash between bonding atoms

108
Q

Valence electrons

A

Bind in a covalent bond

109
Q

Orbital

A

Specific volume of space in which an electron of certain energy is likely to be found

110
Q

Valence orbitals

A

The volumes of space that can be occupied by electrons in an atom’s highest energy level

111
Q

Bonding electron

A

An electron shared with another atom

112
Q

Lone pair

A

Two electrons occupying the same orbital

113
Q

Octet rule

A

Energy levels above the first four contain orbitals, that is, eight electrons maximum. The noble gases have this valence electronic structure; their lack of reactivity indicates that a structure with eight electrons filling a valence level is very stable

114
Q

Lewis symbol

A

The valence electrons, which do not change, are shown as dots around the central symbol, with the entire diagram showing (for an atom) a net charge of zero

115
Q

Covalent bond

A

The simultaneous attraction of two nuclei for a shared pair of bonding electrons

116
Q

Ionic bond

A

The attraction between any specific cation and any specific anion

117
Q

Bonding capacity

A

The maximum number of single covalent bonds that an atom can form

118
Q

Coordinate covalent bond

A

A covalent bond in which one of the atoms donates both electrons

119
Q

Stereochemistry

A

The study of the 3D spatial configuration of molecules and how this affects their reactions.

120
Q

VSEPR Theory

A

The valence-shell-electron-pair-repulsion theory

121
Q

Nonpolar covalent bond

A

If the bonded atoms have the same electronegativity

122
Q

Polar covalent bond

A

If the bonded atoms have different electronegativities

123
Q

Bond dipole

A

The charge separation that occurs when the electronegativity difference of two bonded atoms shifts the shared electrons, making one end of the bond partially positive and the other partially negative

124
Q

London force

A

The more electrons a molecule has, the more easily momentary dipoles will form, and the greater effect of the London force sill be.
Note: London force is necessarily present between all molecules, whether or not any other types of attractions are present.

125
Q

Dipole-dipole force

A

Attraction between dipoles

126
Q

Pressure

A

Force per unit area

127
Q

Atmospheric pressure

A

Force per unit area exerted by air on all objects

128
Q

STP

A

Standard temperature and pressure (0ºC, 101.325 kPa)

129
Q

SATP

A

Standard ambient temperature and pressure 25ºC and 100 kPa

130
Q

Boyle’s Law

A

As the pressure on a gas increases, the volume of the gas decreases proportionally, provided that the temperature and chemical amount of gas remain constant.
(P1V1) (2P1, 1/2V1) (4P1, 1/3V1) etc PV=K

131
Q

Absolute zero

A

The lowest possible temperature of a gas (-273ºC)

132
Q

Absolute/Kelvin Temperature Scale

A

Absolute zero (-273ºC) = Zero Kelvin (0ºK)

133
Q

Charles’ Law

A

As the temperature of a gas increases, the volume increases proportionally, provided that the pressure and chemical amount of a gas remain constant.
V1/T1 = V2/T2

134
Q

Combined Gas Law

A

The product of the pressure and volume of a gas sample is proportional to its absolute temperature in kelvin: PV=kT
P1V1/T1 = P2V2/T2

135
Q

Explain the kinetic molecular theory in brief

A

q smallest particles (ie. atoms, molecules, ions) are in constant, random motion

q the higher the temp., the faster the motion (ie. the larger the kinetic energy)

q motion stops (ie. kinetic energy is zero) at absolute zero or 0 Kelvin

136
Q

The law of combining volumes

A

When measured at the same temperature and pressure, volumes of gaseous reactants and products of chemical reactions are always in simple ratios of whole numbers.

137
Q

Avogadro’s theory

A

Equal volumes of gasses at the same temperature and pressure contain equal numbers of molecules.

138
Q

Molar volume

A

The volume that one mole of a gas occupies at a specified temperature and pressure

139
Q

The molar volume of a gas at STP

A

22.4 L/mol

140
Q

The molar volume of gas at SATP

A

24.8 L/mol

141
Q

Ideal gas law

A

PV = nRT

142
Q

Universal gas constant

A

The constant, R in the ideal gas law
Its value can be obtained by substituting STP (or SATP) conditions for one mole of an ideal gas into the ideal gas law and solving for R.
8.314 L·kPa/mol·K

143
Q

Solution

A

A homogeneous mixture of two or more substances

144
Q

Solvent

A

A substance present in larger quantity within a solution

145
Q

Solute

A

A substance present in smaller quantity within a solution; dissolved within the solvent

146
Q

Electrolytes

A

Aqueous solutions that conduct electricity

147
Q

Non-electrolytes

A

Aqueous solutions that do not conduct electricity

148
Q

Dissociation

A

The separation of ions that occurs when an ionic compound dissolves in water

149
Q

Ionization

A

The process by which a neutral atom or molecule is converted to an ion.

150
Q

Stock ssolution

A

An initial, usually concentrated, solution from which samples are taken for a dilution

High School (8 decks)

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