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Chem > Quarterly 4 review > Flashcards

Quarterly 4 review Flashcards

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1
Q

(Ch 1) chemistry is the study of the …, …, and … of matter and the changes that matter undergoes

A

composition; structure; properties

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2
Q

(Ch 1) a chemical is any substance that has a

A

definite composition or is used or produced in a chemical process

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3
Q

(Ch 1) basic research is carried out for the sake of

A

increasing knowledge

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4
Q

(Ch 1) applied research is carried out to

A

solve practical problems

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5
Q

(Ch 1) technological development involves the use of existing knowledge to

A

make life easier or more convenient

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6
Q

(Ch 1) all matter has … and …

A

mass; takes up space

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7
Q

(Ch 1) mass is one measure of the

A

amount of matter

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8
Q

(Ch 1) chemical properties refer to a substance’s ability to

A

undergo changes that alter its composition and identity

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9
Q

(Ch 1) an element is composed of one kind of

A

atom

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10
Q

(Ch 1) compounds are made from two or more

A

elements in fixed proportions

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11
Q

(Ch 1) all substances have characterisitc properties that enable chemists to tell the

A

substances apart and to separate the substances

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12
Q

(Ch 1) physical changes do not involve changes in

A

identity of a substance

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13
Q

(Ch 1) the three major states of matter are

A

solid, liquid, and gas

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14
Q

(Ch 1) changes of state, such as melting and boiling, are

A

physical changes

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15
Q

(Ch 1) in a chemical change (chemical reaction) the

A

identity of the substance changes

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16
Q

(Ch 1) energy changes accompany

A

physical and chemical changes

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17
Q

(Ch 1) energy may be released or absorbed, but it is neither

A

created nor destroyed

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18
Q

(Ch 1) matter can be classified into

A

mixtures and pure substances

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19
Q

(Ch 1) each element has a

A

unique symbol

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20
Q

(Ch 1) the periodic table shows the elements organized by their

A

chemical properties

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21
Q

(Ch 1) columns on the table respresent .. or … of elements that have similar …

A

groups; families; chemical properties

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22
Q

(Ch 1) properties vary across the rows, or

A

periods

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23
Q

(Ch 1) the elements can be classified as …, …, …, and …

A

metals, nonmetals, metalloids, noble gases

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24
Q

(Ch 1) these classes occupy different areas of the periodic table. metals tend to be, …., …, and … and tend to be good….

A

shiny; malleable; ductile; conductors

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25
Q

(Ch 1) nonmetals tend to be … and tend to be poor..

A

brittle; conductors

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26
Q

(Ch 1) metalloids are intermediate in properties between .. and …., and they tend to be … of electricity

A

metals; nonmetals; semiconductors

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27
Q

(Ch 1) the noble gases are generally

A

unreactive elements

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28
Q

(Ch 1) extensive properties depend on the amount of matter that is

A

present

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29
Q

(Ch 1) intensive properties do not depend on the

A

amount of matter present

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30
Q

(Ch 1) a physical property is a characteristic that can be observed or measured without changing the

A

identity of the substance

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31
Q

(Ch 1) a chemical proeprty relates to a substance’s ability to undergo changees that transform it into

A

different substances

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32
Q

(ch 2) the scientific method is a logical approach to

A

solving problems that lend themselves to investigation

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33
Q

(ch 2) a hypothesis is a testable statemtn that serves as the

A

basis for predictions and further experiments

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34
Q

(ch 2) a theory is a broad generalization that explains a body of

A

known facts or phenomena

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35
Q

(ch 2) the result of nearly every measurement is a

A

number and a unit

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36
Q

(ch 2) the SI system of measurement has seven base units:

A 
meter (length)
kilogram (mass)
second (time)
kelvin (temperature)
mole (amount of substance)
ampere (electric current)
candela (luminous intensity)
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37
Q

(ch 2) weight is a measure fo the

A

gravitational pull on matter

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38
Q

(ch 2) derived Si units include the … and the …

A

square meter (area); cubic meter (volume)

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39
Q

(ch 2) density is the ratio of

A

mass to volume

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40
Q

(ch 2) conversion factors are used to convert from

A

one unit to another

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41
Q

(ch 2) accuracy refers to the closeness of a measurement to the

A

correct or accepted value

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42
Q

(ch 2) precision refers to the closeness of values for a

A

set of measurements

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43
Q

(ch 2) percentage error is the difference between the experimental and the accepted value that is

A

divided by the accepted value and then multiplied by 100

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44
Q

(ch 2) the significant figures in a number consist of all digits known with certainty plus

A

one final digit, which is uncertain

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45
Q

(ch 2) after addition or subtraction, the answer should be rounded so that it has no more digits to the right of the decimal point that there are in the measurement that has the

A

smallest number of digits to the right of the decimal point

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46
Q

(ch 2) after multiplication or division, the answer should be rounded so that it has no more significant figures than there are in the measurement that has

A

the fewest number of significant figures

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47
Q

(ch 2) exact conversion factors are completely certain and do not limit the number of

A

digits in a calculation

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48
Q

(ch 2) a number written in scientific notation is of the form … in which M is greater than or equal to 1 but less than 10 and n is an integer

A

M x 10^n

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49
Q

(ch 2) two quantities are directly proportional to each other if dividing one by the other

A

yields a constant value

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50
Q

(ch 2) two quantities are inversely proportional to each other if their product has a

A

constant value

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51
Q

(ch 2) a system is a specific portion of matter in a given region of space that has been selected for study

A

during an experiment or observation

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52
Q

(ch 2) a model in science is more than a physical object; it is often an explanation of how phenomena occur and how

A

data or events are related

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53
Q

(ch 2) a quantity is something that has

A

magnitude, size, or amount

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54
Q

(ch 2) dimensional analysis is a mathematical technique that allows you to use units to

A

solve problems involving measurements

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55
Q

(ch 3) john dalton proposed a scientific theory of atoms that can still be used to explain

A

properties of most chemicals today

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56
Q

(ch 3) matter and its mass cannot be … or …. in chemical reactions

A

created; destroyed

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57
Q

(ch 3) the mass ratios of the elements that make up a given compound are always the …, regardless of how much of the compound there … or how it …

A

same; is; was formed

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58
Q

(ch 3) if two or more different compounds are composed of the same two elements, then the ratio of the masses of the second element combined with a certain mass of the first element can be expressed as

A

a ratio of small whole numbers

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59
Q

(ch 3) cathode-ray tubes supplied evidence of the existence of

A

electrons

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60
Q

(ch 3) electrons are negatively charged subatomic particles that have relatively

A

little mass

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61
Q

(ch 3) rutherford found evidence for the existence of the atomic nucleus by bombarding gold foil with a

A

beam of positively charged particles

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62
Q

(ch 3) atomic nuclei are composed of …, which have an electric charge of …, and (in all but one case) neutrons, which have .. electric charge

A

protons; +1; no

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63
Q

(ch 3) atomic nuclei have radii of about …., and atoms have radii of about …

A

.001 pm; 40-270 pm

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64
Q

(ch 3) the atomic number of an element is equal to the number of

A

protons of an atom of that element

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65
Q

(ch 3) the mass number is equal to the total number of protons and neutrons that make up the

A

nucleus of an atom of that element

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66
Q

(ch 3) the relative atomic mass unit (amu) is based on the … atom and is a convenient unit for measuring the … of atoms

A

carbon-12; mass

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67
Q

(ch 3) the average atomic mass of an element is found by calculating the …. of the atomic masses of the naturally occuring … of the element

A

weighted average; isotopes

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68
Q

(ch 3) avogadro’s number is equal to approximately…. a sample that contains a number of particles equal to Avogadro’s number contains a … of those particles

A

6.022 x 10^23; mole

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69
Q

(ch 3) atom is the smallest particle of an element that retains the

A

chemical properties of that element

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70
Q

(ch 3) nuclear forces are short range …, …., and … forces that hold the nuclear particles …

A

proton-neutron, proton-proton, and neutron-neutron; together

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71
Q

(ch 3) isotopes are atoms of the same element that have

A

different masses

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72
Q

(ch 3) nuclide is a general term for a specific

A

isotope of an element

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73
Q

(ch 3) a mole is the amount of a substance that contains as many particles as there are atoms in exactly

A

12 g of carbon-12

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74
Q

(ch 3) molar mass is the mass of … of a pure substance

A

one mole

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75
Q

(ch 4) in the early 20th century, light was determined to have a dual

A

wave-partticle nature

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76
Q

(ch 4) quantum theory was developed to explain observations such as the … and the …. of hydrogen

A

photoelectric effect; line-emission spectrum

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77
Q

(ch 4) quantum theory states that electrons can exist only at specific

A

atomic energy levels

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78
Q

(ch 4) when an electron moves from one main energy level to a main energy level of lower energy, a …. is emitted. the … energy equals the energy difference between ….

A

photon; photon’s; the two levels

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79
Q

(ch 4) an electron in an atom can move from one main energy level to a higher main enrgy level only by absorbing an amount of energy exactly equal to the

A

difference between the two levels

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80
Q

(ch 4) electrons were determined to have a dual

A

wave-particle nature

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81
Q

(ch 4) the heisenberg uncertainty principle states that it is impossible to determine simultaneously the … and … of an … or any other …

A

velocity; position; electron; particle

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82
Q

(ch 4) quantization of electron energies is a natural outcome of othe …. which describes the properties of an atom’s …

A

Schrodinger wave equation; electrons

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83
Q

(ch 4) an orbital, a….., shows the regin in space where an electron is most likely to be …

A

3d region around the nucleus; found

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84
Q

(ch 4) the four quantum numbers that describe the properties of electrons in atomic orbitals are the:

A

principal quantum number
angular momentum quantum number:
magnetic quantum number
spin quantum number

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85
Q

(ch 4) the ground-state electron configuration of an atom can be written by using the:

A

aufbau principle
hund’s rule
pauli exclusion principle

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86
Q

(ch 4) electron configurations can be depicted by using different types of notation such as:

A

orbital notation
electron-configuration notation
noble-gas notation

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87
Q

(ch 4) electron configurations of some atoms, such as Cr, deviate from the predictions of the Aufbau principle, but the ground-state configuration that results is the configuration with the

A

minimum possible energy

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88
Q

(ch 4) electromagnetic radiation: form of energy that exhibits

A

wavelike behavior as it travels through space

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89
Q

(ch 4) electromagnetic spectrum formed by

A

all forms of electromagnetic radiation

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90
Q

(ch 4) wavelength: the distance between corresponding points on

A

adjacent waves

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91
Q

(ch 4) frequency: defined as the number of waves that pass a given point in a

A

specific time, usually one second

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92
Q

(ch 4) photoelectric effect: emission of electrons from a metal when

A

light shines on the metal

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93
Q

(ch 4) quantum of energy is the minimum quantity of energy that can be

A

lost or gained by an atom

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94
Q

(ch 4) photon: particle of electromagnetic radiation having

A

zero mass and carrying a quantum of energy

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95
Q

(ch 4) ground state: lowest … of an atom

A

energy state

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96
Q

(ch 4) excited state: a state in which an atom has a higher … than it has in its ….

A

potential energy; ground state

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97
Q

(ch 4) continuous spectrum: emission of a continuous range of

A

frequencies of electromagnetic radiation

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98
Q

(ch 4) principal quantum number: n, indicates the main

A

energy level occupied by electron

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99
Q

(ch 4) angular momentum quantum number, l, indicates the

A

shape of the orbital

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100
Q

(ch 4) magnetic quantum number, m, indicates the orientation of an

A

orbital around the nucleus

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101
Q

(ch 4) spin quantum number has only two possible values (+1/2, -1/2) which indicate the two fundamental

A

spin states of an eelctron in an orbital

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102
Q

(ch 4) aufbau principle: an electron ocupies the lowest-energy

A

orbital that can receive it

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103
Q

(ch 4) pauli exclusion principle: no two electrons in the same atom can have the same

A

set of four quantum numbers

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104
Q

(ch 4) hund’s rule: orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron, and all electrons in singlyu occupied orbitals must have

A

the same spin state

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105
Q

(ch 5) the periodic law states that the physical and chemical properties of the elements are

A

periodic functionso ftheir atomic numbers

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106
Q

the periodic table is an arrangement of the elements in order of their atomic numbers so that elements with simialr properties

A

fall in the same column

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107
Q

(ch 5) the columns in the periodic table are referred to as

A

groups

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108
Q

(ch 5) the rows in the periodic table are called

A

periods

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109
Q

(ch 5) many chemical properties of the elements can be explained by the configurations of the

A

elements’ outermost electrons

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110
Q

(ch 5) the nobel gases exhibit unique chemical stability because their highest occupied levels have an

A

octet of electrons, ns^2np^6

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111
Q

(ch 5) based on the electron configurations of the elements, the periodic table can be divided into four blocks:

A

s, p, d, and f

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112
Q

(ch 5) the groups and periods of the periodic table display general trends in following proterties:

A

electron affinity; electronegativity; ionization energy; atomoic radius; ionic radius

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113
Q

(ch 5) the electrons in an atom that are available to lost, gained, or shared in the formation of chemical compounds are

A

valence electrons

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114
Q

(ch 5) in determining the electron configuration of an ion, the order in which electrons are removed from the atom is the reverse of the order given by the

A

atom’s electron-configuration notation

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115
Q

(ch 5) lanthanides are 14 elements with atomic numbers from

A

58 to 71

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116
Q

(ch 5) actinides are 14 elements with atomic numbers from

A

90 to 103

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117
Q

(ch 5) alkali metals:

A

group 1

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118
Q

(ch 5) alkaline-earth metals:

A

group 2

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119
Q

(ch 5) transition elements: d-block elements with typical

A

metallic properties

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120
Q

(ch 5) main-group elements:

A

p-block and s-block elements

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121
Q

(ch 5) halogens:

A

group 17

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122
Q

(ch 5) atomic radius: 1/2 distance between

A

nucei of identical atoms that are bonded

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123
Q

(ch 5) ion: an atom or group of bonded atoms that has a

A

postive/ negative charge

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124
Q

(ch 5) ionization: any process that results int he formation of

A

an ion

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125
Q

(ch 5) ionization energy: energy required to remove

A

one electron from a neutral atom of an element

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126
Q

(ch 5) electron affinity: energy change that occurs when an electron is

A

acquired by a neutral atom

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127
Q

(ch 5) cation:

A

positive ion

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128
Q

(ch 5) anion:

A

negative ion

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129
Q

(ch 5) electronegativity: measure of the ability of an atom in a chemical compound to attract

A

electrons from another atom in the compound

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130
Q

(ch 6) most atoms are … to other atoms

A

chemically bonded

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131
Q

(ch 6) the three major types oc hemical bonding are

A

ionic, covalent, and metallic

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132
Q

(ch 6) in general, atoms of metals bond ionically with atoms of

A

nonmetals

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133
Q

(ch 6) atoms of metals bond metallically with

A

each other

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134
Q

(ch 6) and atoms of nonmetals bond

A

covalently with each other

135
Q

(ch 6) atoms in molecules are joined by

A

covalent bonds

136
Q

(ch 6) in a covalent bond, two atoms share

A

one or more pairs of electrons

137
Q

(ch 6) the octet rule states that many chemical compounds tend to form bonds so that each atom shares or has

A

eight electrons in its highest occupied energy level

138
Q

(ch 6) bonding within many molecules and ions can be indicated by a

A

lewis structure

139
Q

(ch 6) molecules or ions that cannot be correctly represented by a single Lewis structure are represented by

A

resonance structures

140
Q

(ch 6) an ionic compound is a 3d network of

A

cations and anions mutually attracted to each other

141
Q

(ch 6) ionic compounds tend to be harder and more brittle and to have higher … than materials containing only ….

A

boiling points; covalently bonded atoms

142
Q

(ch 6) the “electron sea” formed in metallic bonding gives metals their properties of …. and … conductivity, …, …, and …

A

high electrical; thermal; malleability; ductility; luster

143
Q

(ch 6) vsepr theory is used to predic tthe … of molecules based on the fact that electron pairs strognly

A

shape; strongly repel each other

144
Q

(ch 6) hybridization theory is used to predict the shapes of molecules based on the fact that orbitals within an atom can

A

mix to form orbitals of equal energy

145
Q

(ch 6) intermolecular forces include … and …

A

dipole-dipole forces; london dispersion forces

146
Q

(ch 6) hydrogen bonding is a special case of

A

dipole-dipole forces

147
Q

(ch 6) chemical bond: mutual electrical attraction between nuclei and valence electrons of

A

different atoms that binds the atoms together

148
Q

(ch 6) ionic bonding: chemical bonding that results from electrical attraction between

A

cations and anions

149
Q

(ch 6) covalent bonding: sharing of electron pairs between

A

two atoms

150
Q

(ch 6) nonpolar-covalent bond: covalent bond in which bonding electrons are shared equally by the bonded atoms, resulitng in a balanced

A

distribution of electrical charge

151
Q

(ch 6) a polar-covalent bond is a covalent bond in whicht he bonded atoms have an

A

unequal attraction for the shared electrons

152
Q

(ch 6) molecule: neuttral group of atoms that are held together by

A

covalent bonds

153
Q

(ch 6) molecular compound: chemical compound whose simplest units are

A

molecules

154
Q

(ch 6) chemical formula: indicates relative numbers of atoms of each kind in a chemical compound by using

A

atomic symbols and numerical subscripts

155
Q

(ch 6) molecular formula: shows types and numbers of atoms combined in a single molecule of a

A

molecular ompound

156
Q

(ch 6) bond energy: energy required to … a chemical bond and form…

A

break; neutral isolated atoms

157
Q

(ch 6) structural formula: indicates…, …, …, and /… but not the unshared pairs of the atoms in a molecule

A

kind; number; arrangement; bonds

158
Q

(ch 6) single bond: covalent bond in which one pair of electrons is shared between

A

two atoms

159
Q

(ch 6) multiple bonds:

A

deouble and triple bonds

160
Q

(ch 6) formula unit: simplest collection of atoms from which an ionic compound’s formula can be

A

established

161
Q

(ch 6) lattice enrgy: energy released when one mole of an ionci crystalline compound is

A

formed from gaseous ions

162
Q

(ch 6) polyatomic ion: charged group fo

A

covalently bonded atoms

163
Q

(ch 6) metallic bonding: chemical bonding that results from the attraction betweern … and the surrounding…

A

metal atoms; sea of electrons

164
Q

(ch 6) malleability: ability of a substance to be … or …

A

hhammered; beaten into sheets

165
Q

(ch 6) ductility: ability of substance to be ..,…, or …. through a small opening to produce a wire

A

drawn; pulled; extruded

166
Q

(ch 6) hybrid orbitals: orbitals of equal energy produced by the combination of two or more

A

orbitals on the same atom

167
Q

(ch 6) dipole is created by equal but opposite charges that are

A

separated by a short distance

168
Q

(ch 6) hydrogen bonding: intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an ubnshared pair of electrons of an

A

electronegative atom in a nearby molecule

169
Q

(ch 6) london dispersion forces: intermolecular attractions resulting fromt he cosntant motion of electrosn and the creation fo

A

instantaneous dipoles

170
Q

(ch 7) positive monatomic ion is identified simply by the name of the

A

appropriate element

171
Q

(ch 7) a negative monatomic ion is named by dropping parts of the ending of the element’s name and adding

A

-ide to the root

172
Q

(ch 7) the charge of each ion in an ionic comjpound may be used to determine the simplest

A

chemical formula for the compound

173
Q

(ch 7) binary compounds are composed of

A

two elemetns

174
Q

(ch 7) binary ionic compounds are named by combining the names of the

A

positive and negative ions

175
Q

(ch 7) the old system of naming binary molecular compounds uses

A

prefixes

176
Q

(ch 7) the new system, known ans the Stock system, uses

A

oxidation numbers

177
Q

(ch 7) oxidation numbers are useful in …, writing…, and in ….

A

naming compounds; formulas; balancing chemical equations

178
Q

(ch 7) compounds containing elements that have more than one oxidation state are named by using the

A

stock system

179
Q

(ch 7) stock-system names and prefix-system names are used… for many molecular compounds

A

interchangeably

180
Q

(ch 7) oxidation numbers of each element in a compound may be used to determine the compound’s simplest

A

chemical formula

181
Q

(ch 7) by knowing oxidation numbers, we can name compounds without knowing whether theya re

A

ionic or molecular

182
Q

(ch 7) …,…, and … cnan be calculated form the chemical formula for a compound

A

formula mass, molar mass, percentage composition

183
Q

(ch 7) percentage composition of a compound si the percentage by mass of each

A

element in the compound

184
Q

(ch 7) molar mass is used as conversion factor between amojunt in moles and mass in grams of a given

A

compound/ element

185
Q

(ch 7) an empirical formula shows the simplest whole number ratio of

A

atoms in a given compound

186
Q

(ch 7) empirical formulas indicate how many atoms of each elemnt are combined in the simplest

A

unit of a chemical compound

187
Q

(ch 7) a molecular formula can be found from the empirical formula if the

A

molar mass is measured

188
Q

(ch 7) oxyanion: polyatomic ions that

A

contian oxygen

189
Q

(ch 7) salt: an ionic compound composed of a … and the … from an acid

A

cation; anion

190
Q

(ch 7) oxidation state: assiged to the atoms composing the

A

compound or ion

191
Q

(ch 7) formula mass: sum of the average atomic masses of

A

all atoms represented in the formula

192
Q

(Ch 8) four observations that suggest a chemical reaction is taking place are the

A

evolution of energy as heat and light
production of gas
change in color
formation of a precipitate

193
Q

(Ch 8) a balanced chemical equation represents, with symbols and formulas, the identities and relative amoutns of

A

products in a chemical reactio

194
Q

(Ch 8) synthesis rections equation:

A

A+X→AX

195
Q

(Ch 8) decomposition reaction equation

A

AX→A + X

196
Q

(Ch 8) single-displacement reactions represented by two equation:

A

A + BX→AX + B

Y + BX→BY + X

197
Q

(Ch 8) double diosplacement reaction equatio

A

AX + BY→AY + BX

198
Q

(Ch 8) in a combustion reaction, a substance combines with…, realsing energy in the form of … and …

A

oxygen; heat; light

199
Q

(Ch 8) activity series list the elements in order of their chemical reactivity and are useful in predicting wither a

A

chemical reaction will occur

200
Q

(Ch 8) chemists determine activity series through

A

experiments

201
Q

(Ch 8) precipitate: a solid that is produced as a result of a chemical reaction in solution and that

A

separates from the solutio

202
Q

(Ch 8) coefficient: small whole number that ppears in front of a

A

formula in a chemical equation

203
Q

(Ch 8) word equation: an equation in which the reactants and products in a chemical reactiona represented by

A

words

204
Q

(Ch 8) formula equation: represents reactants and products of a chemical reaction by their

A

symbols or formulas

205
Q

(Ch 8) electrolysis: decomposition of a substance by an

A

electric current

206
Q

(ch 9) reaction stoichiometry involves the mass relationships between

A

reactants and products in a chemical reaction

207
Q

(ch 9) relating one substance to another requires expressing the amount of each

A

substance in moles

208
Q

(ch 9) a mole ratio is the conversion factor that relates the amount in … of any two substances in a …

A

moles; chemical reaction

209
Q

(ch 9) the mole ratio is derived from the

A

balanced equation

210
Q

(ch 9) amount of a substance is expressed in…., and mass of a substance is expressed by using mass units such ass…, …, or …

A

moles; grams; kilograms; milligrams

211
Q

(ch 9) mass and amount of substance are.., wherars moles and grams are …

A

quantities; units

212
Q

(ch 9) a balanced chemical equation is necessary to solve any

A

stoichiometric problem

213
Q

(ch 9) in an ideal stoichiometric calculation, the mass or the amount of any reactnat or product can be calculated if the …. and the … or … of any other reactant or product is known

A

balanced chemical equation; mass; amount

214
Q

(ch 9) in actual reactions, the reactants may be present in proportions that differ from the stoichiometric proportions required for a complete reaction in which all of

A

each reactant is converted to product

215
Q

(ch 9) the limiting reactant controls the …. of product formed

A

maximum possible amount

216
Q

(ch 9) for many reactions, the quantity of a product is less than the

A

theoretical maximum for that product

217
Q

(ch 9) percentage yield shows the relationship between the … and … for the product of a reaction

A

theoretical yield; actual yield

218
Q

(ch 9) composition stochiometry: deals with the mass relationships of

A

elements in compounds

219
Q

(ch 9) excess reactant: substance that is not

A

used up completely in a reaction

220
Q

(ch 9) theoretical yield: maximum amount of product that can be produced from a

A

giv en amount of reactant

221
Q

(ch 9) actual yield: measured amount of a product obtained from a

A

reaction

222
Q

(ch 10) the kinetic-molecular theory of matter can be used to explain the properties of

A

gases, liquids, and solids

223
Q

(ch 10) the kinetic-molecular theory of gases describes a model of an

A

ideal gas

224
Q

(ch 10) gases consist of large numbers of tiny, fast-moving … that are … relative to their sized

A

particles; far apart

225
Q

(ch 10) particles of a liquid are … and more … than those of a gas and are less … than those of a solid

A

closer together; ordered; ordered

226
Q

(ch 10) liquids have a definite … and a fairly high …, and they are relatively ….

A

volume; density; incompressible

227
Q

l(ch 10) like gases, liquids can .. and are thus considered to be …

A

flow; fluids

228
Q

(ch 10) the particles of a solid ar enot nearly as free to … as those of a liquid or gas

A

move about

229
Q

(ch 10) solids have a definite .. and may be … or …

A

shape; crystalline; amorphous

230
Q

(ch 10) solids have a definite … and are generally non…

A

volume; nonfluid

231
Q

(ch 10) a crystal structure is the total 3d array of … that describes teh arrangement of the ..

A

.points; particles of a crystal

232
Q

(ch 10) unlike crystalline solids, amorphous solids do not have a highly…. or a regular…

A

ordered structure; shape

233
Q

(ch 10) a liquid in a closed system will gradually reach a… as the rate at which molecules … equals the rate at which they…

A

liquid-vapor equilibrium; condense; evaporate

234
Q

(ch 10) when two opposing changes occur at equal rates in the same closed system, nthe system is said to be in

A

dynamic equilibrium

235
Q

(ch 10) water is a

A

polar covalent compound

236
Q

(ch 10) the structure and the hydrogen bonding in water are responsible for its relatively high…., molar ….., ….., and molar….

A

melting point; enthalpy of fusion; boiling point; enthalpy of vaporization

237
Q

(ch 10) ideal gas: hypothetical gas that perfectly fits all the assumptions of the

A

kinetic-molecular theory

238
Q

(ch 10) elastic collision: one in which there is no net loss of

A

total kinetic energy

239
Q

(ch 10) diffusion: result of the spontaneous … of the particles of two substances caused by their….

A

mixing; random motion

240
Q

(ch 10) effusion: process by which gas particles pass through a

A

tiny opening

241
Q

(ch 10) real gas: a gas that does not behave completely according to the assumptions of the

A

kinetic-molecular theory

242
Q

(ch 10) fluid: substance that can … and therefore take the … of of its container

A

flow; shape

243
Q

(ch 10) surface tension: force that tends to pull adjacent parts of aliquid’s surface …, thereby decreasign

A

together; surface area to the smallest possible size

244
Q

(ch 10) capillary action: attraction of the surface of a liquid to the s

A

surface of a solid

245
Q

(ch 10) vaporization: process by which a liquid or solid

A

changes to a gas

246
Q

(ch 10) evaporation: process by which particles escape from the surface of a nonboiling liquid and

A

enter the gas state

247
Q

(ch 10) freezing/ solidification: physical change of a liquid to a solid by

A

removal of energy as heat

248
Q

(ch 10) crystalline solids: consist of

A

crystals

249
Q

(ch 10) amorphous solid: one in which the particles are

A

arranged randomly

250
Q

(ch 10) meltin: physical change of a solid to a liquid by the addition of

A

nergy as heat

251
Q

(ch 10) melting point: temperature at which a solid

A

becomes a liquid

252
Q

(ch 10) supercooled liquids: substances that retain certain liquid properties even at

A

temperatures at which they appear to be solid

253
Q

(ch 10) crystal: a substance in which the particles are arranged in an

A

orderly, geometric, repeating pattern

254
Q

(ch 10) unit cell: the smallest portionof a crystal lattice that shows the

A

3d pattern of the entire lattice

255
Q

(ch 10) phase; any part of a system that has

A

uniform composition and properties

256
Q

(ch 10) condensation: process by which a gas changes to a

A

liquid

257
Q

(ch 10) equilibrium: dynamic condition in which two opposing changes occur at

A

equal rates in a closed system

258
Q

(ch 10) equilibrium vapor presssure: pressure exerted by a vapor in equilibrium with its

A

corresponding liquid at a given temeprature

259
Q

(ch 10) volatile liquids: liquids that

A

evaporate readily

260
Q

(ch 10) boiling: conversion of a liquid to a vapor within the liquid as well as

A

at its surface

261
Q

(ch 10) boiling point: temeprature at which the equilibrium vapor pressure of the liquid equals

A

the atmospheric pressure

262
Q

(ch 10) molar enthalpy of vaporization: amount of energy as heat that is needed to vaporize on mole of liquid at the liquid’s

A

boiling point at constant pressure

263
Q

(ch 10) freezing point: temperature at whicht eh solid and liquid are in

A

equilibrium at 1 atm

264
Q

(ch 10) molar enthalpy of fusion: amount of energy as heat required to melt one mole of

A

solid at the soldi’s melting pint

265
Q

(ch 10) sublimation: change of state from a solid directly to a

A

gas

266
Q

(ch 10) deposition: change of state from a gas directly to a

A

solid

267
Q

(ch 10) phase diagram: graph of pressure versus temperature that shows the conditions under whicht he

A

phases of a substance exist

268
Q

(ch 10) triple point: indicates the temeprature and pressure conditions at which the solid, liquid, and vapor of the substance can

A

coexist at equilibrium

269
Q

(ch 10) critical point: indicates the critical

A

temperature and critical pressure

270
Q

(ch 10) critical temperature: temperature above which the substance cannot exist in the

A

liquid state

271
Q

(ch 10) critical pressure: lowest pressure at which the substance can exist as a liquid at the

A

critical temperature

272
Q

(ch 11) kinetic moleculr teory of gases describes an

A

ideal gas

273
Q

(ch 11) the behvior of most gases is nearly ideal except at very

A

high pressures and low temperatures

274
Q

(ch 11) a barometer measures

A

atmospheric pressure

275
Q

(ch 11) dalton’s law of partial pressure states that in a mixture of unreacting gases, the total pressure equals the sum of the

A

partial pressures of each gas

276
Q

(ch 11) boyle’s law states the inverse relationship between the volume and pressure of a gas:

A

PV=k

277
Q

(ch 11) charles law illustrates the direct relationship between a gas’s … and its … in kelvins:

A

volume; temperature

V=kT

278
Q

(ch 11) gay-lussac’s law represents the direct relationshjip betrween a gas’s … and its … in kelvins:

A

pressure; temperature

P=kT

279
Q

(ch 11) the combined gas law combines boyle’s, charles’s, and gay-lussac’s law into this epression:

A

PV/ T=k

280
Q

(ch 11) gay-lussac’s law of combining volumes states that the volumes of recting gases and their products at the same temperature and pressure can be expressed as

A

ratios of whole numbers

281
Q

(ch 11) avogadro’s law states that equal volumes of gases at the same temperature and pressure contain

A

equal numbers of molecules

282
Q

(ch 11) the volume occupied by one mole of an ideal gas at STP is called the …, which …

A

standard molar volume; 22.414 L

283
Q

(ch 11) charles’s law, Boyle’s law, and Avogadro’s law can be bombined to create the ideal gas law:

A

PV=nRT

284
Q

(ch 11) gases diffuse, or become morespread out, due to their

A

constant random molecular motion

285
Q

(ch 11) graham’s law of effusion states that the relative rates of effusion of gases at the same temperature and pressurea re inversely proportional to the

A

square roots of their molar masses

286
Q

(ch 11) pressure is defined as the force per

A

unit area on a surface

287
Q

(ch 11) newton: force that will increase the speed of a 1 kilogram mass by one meter per second each second that the

A

force is applied

288
Q

(ch 11) millimeters of mercury: common unit of

A

pressure

289
Q

(ch 11) atmosphere of pressure: exactly equivalent to

A

760 mm Hg

290
Q

(ch 11) pascal: the pressure exerted by a force of one … acting on an area of one

A

newton; square meter

291
Q

(ch 11) partial pressure: pressure of each

A

gas in a mixture

292
Q

(ch 11) absolute zero: teh temperature …, given a value of … in the kelvin scale

A

-273.15 C; zero

293
Q

(ch 11) ideal gas constant: the constant …, with balues of … atm and …. kPa

A

R; .082 atm; 8.314 kPa

294
Q

( ch 12) solutions are

A

homogenous mixtures

295
Q

( ch 12) mixtures are classified as:

A

solutions
suspensions
colloids

296
Q

( ch 12) the way mixtures are classified depends on the … of the solute particles in the mixture

A

size

297
Q

( ch 12) the dissolved substance is the

A

solute

298
Q

( ch 12) solutions that have water as a solvent are

A

aqueous solutions

299
Q

( ch 12) solutions can consist of solutes and solvents that are

A

solids, liquids, or gases

300
Q

( ch 12) suspensions settle out upon

A

standing

301
Q

( ch 12) colloids do not settle out, and they scatter

A

light that’s shined through them

302
Q

( ch 12) most ionic solutes and some molecular solutes form aqueous solutions that conduct an electric current:

A

electrolytes

303
Q

( ch 12) nonelectrolytes are solutes that dissolve in water to form

A

solutions that do not conduct

304
Q

( ch 12) a solute dissolves at a rate that depends on the … of the solute, how vigorously the solution is.., and the … of the solvent

A

surface area; mixed; temperature

305
Q

( ch 12) the solubility of a substance indicates how much of that substance will dissolve in a specified amount of solvent under

A

certain conditions

306
Q

( ch 12) the solubility of a substance depends on the

A

temeprature

307
Q

( ch 12) the solubilityof gases in liquids increases with icreases in

A

pressure

308
Q

( ch 12) the solubility of gases in liquids decreases wtih

A

increases in temperature

309
Q

( ch 12) the overall energy absorbed as heat by the system when a specified amount osf solute dissolved during solution formation is caleld the

A

enthalpy of solution

310
Q

( ch 12) two useful expressions of concentration are

A

molarity and molality

311
Q

( ch 12) the molar concentration of a solution represents the ratio fo moles of solute to

A

liters of solutio

312
Q

n( ch 12) the molal concentration of a solution represents the ratio fo moles of solute to

A

kilograms of solvent

313
Q

( ch 12) soluble: capable of being

A

dissolved

314
Q

( ch 12) solvent: dissolving

A

medium

315
Q

( ch 12) solution equilibrium: physical state in which the opposing processes of … and … of a solute occur at equal rates

A

dissolution; crystallization

316
Q

( ch 12) saturated solution: a solution that contains the maximum amount of

A

dissolved solute

317
Q

( ch 12) unsaturated solution: solution that contains less solute than a

A

saturated solution under same conditions

318
Q

( ch 12) supersaturated solution: contains more dissolved solute that a saturated solution contains under the

A

same conditions

319
Q

( ch 12) hydration: solution process with water as the

A

solvent

320
Q

( ch 12) immiscible: liquids that are nto

A

soluble in each other

321
Q

( ch 12) miscible: liquids that dissolve freely in one another in any

A

proportion

322
Q

( ch 12) henry’s law: solubilityof a gas in al iquid is directly proportional to the partial pressure of that gas on the

A

surface of the liquid

323
Q

( ch 12) effervescence: rapid escape of a gas from a liquid in which it is

A

dissovled

324
Q

( ch 12) solvated: solute particle that is surrounded by

A

solvent molecules

325
Q

( ch 12) enthalpy of solution: the net amount of energy absorbed as heat by the solution when a specific amount of

A

solute dissolves in a solvent

326
Q

( ch 12) concentration: measure fo the amount of solute in a given amount of

A

solvent or solution

327
Q

In general, the atomic radii of the main-group elements… down a group

A

increase

328
Q

In general, ionization energies of the main-group elements … across each period.

A

increase

329
Q

Among the main-group elements, ionization energies generally… down the groups;

A

decrease

330
Q

Ionic radii: cationic radii …across a period

A

decrease

331
Q

anionic radii ….across each period

A

decrease

332
Q

there is a gradual …of ionic radii down a group

A

increase

333
Q

electronegativities tend to …across each period, although there are exceptions;

A

increase

334
Q

electronegativities tend to either …down a group or remain about the same

A

decrease

Chem (54 decks)

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