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chemistry > ACS Exam > Flashcards

ACS Exam Flashcards

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1
Q

chemistry is a science based on…

A

modeling molecules with matter

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2
Q

weight

A

force on an object due to gravity

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3
Q

mass

A

quantity of matter

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4
Q

hypothesis

A

statement made to try to explain an observable pattern in nature, often based on an unobservable causal entity

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5
Q

relationship between volume and pressure

A

P∝F/A

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6
Q

boyles law

A

V∝1/p

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7
Q

atmospheric pressure

A

standard: 760 mm hg = 760 torr = 1 atm

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8
Q

relationship between volume and temp of gas

A

ast temp increases, volume increases (however not directly proportional)

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9
Q

absolute zero

A

lowest temp possible where molecular motion goes to a minimum (-273C) = 0K

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10
Q

Volume is directly proportional to temp when…

A

temp is in K

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11
Q

combined gas law

A

(P1V1 / T1 )= (P2V2 / T2)

Combination of charles law and boyles law

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12
Q

charles law

A

V/T=K (for temp in K)

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13
Q

precision

A

reproducibility of results

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14
Q

accuracy

A

closeness to correct value

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15
Q

density

A

density= mass/volume

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16
Q

algorithm

A

a step by step procedure that can be applied to solve a problem

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17
Q

true problem

A

a problem for which no algorithm can be applied

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18
Q

matter

A

something that has mass and occupies space

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19
Q

liquid

A

indefinite shape, definite volume

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20
Q

solid

A

definite shape, definite volume

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21
Q

gas

A

variable shape and volume

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22
Q

pure substance

A

one kind of matter, distinct physical and chemical properties

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23
Q

compound

A

a pure substance that can be broken down into 2 or more pure substances

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24
Q

element

A

a pure substance that cannot be decomposed into other pure substances by ordinary chemical means

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25
Q

physical change

A

new form of same substance

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26
Q

physical properties

A

measurable and detectable by the senses

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27
Q

mixture

A

sample of matter composed of 2 or more chemicals

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28
Q

homogeneous/solution

A

uniform appearance and composition throughout

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29
Q

heterogenous

A

visibly different phases and/or different composition in a sample of matter

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30
Q

chemical change

A

old substance destroyed, new substance formed

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31
Q

distillation

A

the process of separating the components of a mixture by heating the liquid and collecting the gaseous components that separate.

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32
Q

conservation of mass

A

total mass of the substances that undergo a chemical transformation is equal to the total mass of the products that change (lavoisiers fruit experiment)

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33
Q

law of definite proportions

A

any individual compound is made of the same invariable ratio of more elementary substances by mass

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34
Q

law of multiple proportions

A

when 2 substances react to form more than one product, the amounts of one that completely reacts with a fixed amount of the other are in a reaction of small whole numbers

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35
Q

law of combining volumes

A

the volume ratio in which gases react are always ratios of small whole numbers

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36
Q

avagadros hypothesis explains the law of combing volumes by proposing..

A

equal volumes of gases contain equal numbers of molecules

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37
Q

atomic mass unit (u)

A

one atom of carbon12 has exactly 12u, 6.02E-23=1g

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38
Q

atomic number

A

number of protons

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39
Q

every atom of a particular element has the ______ number of protons

A

same

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40
Q

mass varies among atoms of the same element because of

A

varying number of neutrons

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41
Q

isotopes

A

atoms of the same element that have different masses, different # of neutrons

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42
Q

mass number

A

the total number of protons and neutrons in the nucleus

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43
Q

atomic mass of an element

A

average mass of all atoms of an element as they occur in nature.

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44
Q

periods of periodic table

A

horizontal rows

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45
Q

groups of periodic table (chemical families)

A

vertical columns consisting of elements with similar properties

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46
Q

diatomic molecules

A

each molecule has 2 atoms (superheros night out, fire can burn ice)

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47
Q

polyatomic molecules

A

each molecule has many atoms

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48
Q

two polyatomic molecules to remember

A

sulfur-sexy 8s, phosphorous- foxy 4s

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49
Q

state symbol

A

follows element symbol and represents state at 25C and 1 bar

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50
Q

2 elements that are liquid under ordinary conditions

A

Hg(mercury) Br(bromine)

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51
Q

binary molecular compounds

A

compounds formed by 2 nonmetals or a metalloid and a nonmetal

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52
Q

amonia

A

NH3

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53
Q

cations

A

positively charged ion

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54
Q

anion

A

negatively charged ion

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55
Q

ion

A

atom that gained or lost an electron

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56
Q

ionic compound

A

metal ion- non metal ion compound

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57
Q

acids

A

a molecular compound that reacts with water to yield a hydrogen ion and an anion

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58
Q

oxoacid

A

an acid that contains hydrogen, a nonmetal, and oxygen

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59
Q

mole

A

one mole is that amount of any substance that contains the same number of units as the number of atoms in exactly 12 grams of carbon12 (6.02E23)

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60
Q

empirical formula

A

shows the simplest ratio of atoms of the elements in a compound

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61
Q

what occurs during a chemical change

A

of atoms stay the same but # and type of molecules changes

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62
Q

signs of chemical change

A

color change, formation of gas/solid, heat, light

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63
Q

aqueous solution

A

dissolves in h20

64
Q

base

A

substance that contains hydroxide ions

65
Q

neutralization reaction

A

acid+base➞water+salt

66
Q

ideal yield

A

calculated, amount of product formed from complete conversion of given amount of reactant to product

67
Q

actual yield

A

amount determined by experiment

68
Q

percent yield

A

actual/ideal x 100

69
Q

daltons law of partial pressures

A

the total pressure exerted by a mixture of gases is the sum of the partial pressures of the gases in the mixture.

70
Q

Ideal gas law

A

PV=nRT

71
Q

volume of gas at standard temp and pressure

A

22.7 L/mol

72
Q

law of conservation of energy

A

in a non-nuclear change, energy is conserved, neither created nor destroyed.

73
Q

energy definition

A

the ability to do work or transfer heat

74
Q

work equation

A

W=FxD

75
Q

one joule

A

force of one newton exerted over one meter

76
Q

heat definition

A

form in which energy is transferred between substances of different temperatures.

77
Q

temperature

A

the measure of the average energy of particles in a substance

78
Q

exothermic reaction

A

chemical change that releases energy to tis surroundings

79
Q

endothermic reaction

A

chemical change that absorbs energy from its surroundings

80
Q

calorie

A

the amount of energy required to raise temperature of 1g of water 1C

81
Q

thermodynamic system vs surroundings

A

the portion of the universe under consideration vs everything outside the system

82
Q

state function

A

a property whose value is determined only by the state of a system at a given moment

83
Q

internal energy

A

energy of a system that results from sources other than the influence of external force

84
Q

1st law of thermodynamics in words

A

the internal energy of a system changes by an amount equal to the sum of the heat that flows into or out of the system and the work done by the system.

85
Q

1st law of thermodynamics in math

A

△E=q+w

86
Q

enthalpy definition

A

the heat content of a system

87
Q

enthalpy of reaction definition

A

heat given off or absorbed in a chemical reaction

88
Q

specific heat

A

the heat flow required to change the temp of 1 gram of a substance by 1C

89
Q

calorimeter

A

isolated segment of the universe, a system that cant transfer heat to or from its surroundings

90
Q

hess’s law

A

if a reaction is carried out in a series of steps, the △H for the total reaction is equal to the sum of the △H for the steps

91
Q

speed of light (c)

A

3.00E8 m/sec

92
Q

wavelength (ƕ)

A

distance between identical parts of a wave

93
Q

frequency (v)

A

of complete waves passing a point in a given period of time

94
Q

white light produces a ______ spectrum

A

continuous

95
Q

elements produce a _____ spectrum

A

line

96
Q

photon

A

energy is released by electrons in the form of a massless pocket of electromagnetic radiation (photon)

97
Q

wave particle duality

A

light acts as a wave and a particle

98
Q

hertz

A

one inverse second

99
Q

velocity

A

c = ƕv

100
Q

plancks constant

A

relates energy of a photon to its frequency

h = 6.02E-34 JxS

101
Q

energy frequency proportionality

A

E = hv

102
Q

photoelectric effect

A

light can cause the ejection of electrons from some metal surfaces

103
Q

Bohr model

A
  • energy possessed by electron and radius of its orbit is quantized
  • quantized energy levels, at any instant the electron may have one of several energy levels but can never be in between
104
Q

quantum leap

A

process by which electrons move between orbits, disappear from one orbit and reappear in another

105
Q

ground state

A

condition in which all electrons in an atom occupy the lowest possible energy levels

106
Q

excited state

A

condition at which one or more electrons in an atom has an energy level above ground state

107
Q

equation for wavelength of a moving particle

A

ƕ = h/mv

108
Q

probability density

A

the probability that a particle is found in a specified 3-d region in space

109
Q

pauli exclusion principle

A

at any instant, an orbital may be

  1. unoccupied
  2. occupied by one electron
  3. occupied by 2 electrons
110
Q

hunds rule

A

the most stable arrangement of electrons in a sublevel is the one that has the max # of unpaired electrons

111
Q

valence electrons

A

total # of s and p electrons in the highest occupied energy level

112
Q

effective nuclear charge

A

the charge experienced by an electron in a many-electron atom (actual charge-shielding constant)

113
Q

atomic radius

A

average distance b/w the nucleus of an atom of the element and the outer limit of its electron cloud

114
Q

ionization energy

A

the energy required to remove one electron from a neutral gaseous atom of an element

115
Q

electron affinity

A

the change in energy that occurs when an electron is added to a gaseous atom or ion (generally increases from left to right)

116
Q

an element is a metal if…

A

it can lose one or more electrons and become a positively charged ion, if not is a nonmetal

117
Q

crystal

A

definite geometric structure of a solid

118
Q

ionic bonds

A

strong electrostatic forces that hold the ions of a crystal in a fixed position

119
Q

ionic compound

A

compounds made up of ions

120
Q

molecular compounds

A

ultimate structural unit is an individual particle known as a molecule

121
Q

covalent bonds

A

atoms in a molecule share electrons

122
Q

what causes the octet rule

A

tendency towards a complete octet of electrons in a bonded atom is due to a systems tendency to move to lowest energy state possible

123
Q

nonpolar bonds

A

a bond in which bonding electrons are shared equally

124
Q

polar bond

A

electrons are shared unequally

125
Q

electronegativity

A

ability of an atom to attract bonding electrons to itself (increases left to right, bottom to top)

126
Q

constitutional isomer

A

made of the same atoms but connected differently

127
Q

resonance structures

A

series of lewis diagrams that show the different possible distributions of valence electrons

128
Q

resonance hybrid

A

single unchanging average, represents actual molecule state

129
Q

Free radicals

A

species with an odd # of electrons

130
Q

bond order

A

(# of shared electron pairs)/(# of links)

131
Q

bond length

A

average distance between the nuclei of 2 atoms in a molecule

132
Q

calculating △H using bonds

A

△H= E of bonds broken- E bonds formed

133
Q

electrolysis

A

movement of ions that make up an electron current in a solution

134
Q

molecular compounds do/dont conduct electricity

A

dont (no ions)

135
Q

strong electrolyte

A

substance whose solution is a strong conductor

136
Q

non-electrolyte

A

substance that does not conduct electricity

137
Q

strong acid

A

almost all the molecules of the original compound are converted to ions (major species are ions, minor species are un-ionized molecules)

138
Q

weak acid

A

only slightly ionized in solution

139
Q

seven common strong acids

A

HNO3, H2SO4, HCl, HClO3, HClO4, HI, HBr

140
Q

Ions are the major species in two types of solutions

A
  1. ionic compounds

2. 7 strong acids

141
Q

allotrope

A

different physical forms in which an element can exist

142
Q

alpha particle

A

produced during alpha decay, fast moving helium nucleus

143
Q

Periodic table groups

A

Alkali Earl Takes Happy Naps

144
Q

Titration

A

careful addition of one solution to another by means of a device that can measure volume accurately

145
Q

liquid properties vs gas properties

A
  1. gases can be compressed, liquids cannot
  2. gases expand to fill their container, liquids do not
  3. gases have low densities, liquids do not
  4. gases can be mixed in a fixed volume, liquids cannot
146
Q

vapor pressure

A

partial pressure exerted by evaporated gaseous particles

147
Q

molar heat of vaporization

A

energy required to change one mole of a liquid to a gas at standard temp and pressure

148
Q

viscosity

A

internal resistance of a liquid to flow

149
Q

surface tension

A

tendency of a liquid to arrange for minimum surface tension

150
Q

dipole forces

A

attraction b/w the positive pole of one molecule and the negative pole of another molecule (requires polar molecules)

151
Q

induced dipole forces

A

attractions b/w substances w/ non polar molecules resulting from shifting electron clouds

152
Q

hydrogen bonds

A

hydrogen bonded to an atom that is small and highly electronegative (nitrogen, oxygen, fluorine)

153
Q

covalent bond

A

bond in which atoms share electrons to form octet, (occurs between a nonmetal and a nonmetal, or a nonmetal and a metalloid)

154
Q

ionic bond

A

bond in which one atom loses an electron and another atom gains it to form an octet (occurs between nonmetal and metal)

155
Q

an ionic bond is _____ than a covalent bond

A

stronger

156
Q

sigma bond

A

type of covalent bond where orbitals overlap end to end

chemistry (4 decks)

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