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From Flashcardlet > Chemistry > Flashcards

Chemistry Flashcards

0
Q

the principal quantum number

A

specifies size

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1
Q

the magnetic quantum number

A

specifies orientation

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2
Q

the distance between identical points on successive waves

A

wavelength

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3
Q

particles of light

A

photons

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4
Q

there are three quantum numbers necessary to describe

A

atomic orbital

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5
Q

states that it is impossible to know simultaneously both the momentum and the position of a particle with certainty

A

heisenberg uncertainty principle

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6
Q

states that electrons are added to the lowest energy orbitals first before moving to higher energy orbitals

A

aufbau principle

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7
Q

the angular moment quantum number

A

specifies shape

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8
Q

energy is the smallest quantity of energy that can be emitted (or absorbed)

A

quantum

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9
Q

the probability of finding an electron in a certain area of space is proportional to w2

A

electron density

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10
Q

reasoned that if light can behave like a stream of particles (photons) then electrons could exhibit wavelike properties

A

Louis de Broglie

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11
Q

is used to specify an electron’s spin

A

electron spin quantum number

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12
Q

are the emission of light only at specific wavelengths

A

line spectra

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13
Q

describes the shape of the orbital

A

angular quantum number

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14
Q

the number of waves that pass through a particular point in 1 second

A

frequency

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15
Q

each energy state in which n>1

A

excited state

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16
Q

designates the size of the orbital

A

principal quantum number

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17
Q

are spherical in shape but different in size

A

s orbitals

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18
Q

the lowest state

A

ground state

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19
Q

visible light is only a small component of the continum of radiant energy known as the

A

electromagnetic spectrum

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20
Q

no two electrons can have the same four quantum numbers

A

pauli exclusion principle

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21
Q

collection of orbitals with the same value of n is frequently

A

shell

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22
Q

are required to describe the distribution of electron density in an atom

A

quantum numbers

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23
Q

derived a complex mathematical formula to incorporate the wave and particle characteristics of electrons

A

erwin schrodinger

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24
Q

collection of orbitals with the same value of n and i is referred to as a

A

subshell

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25
Q

has both an electric field component and a magnetic component

A

electromagnetic wave

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26
Q

the most stable arrangement of electrons is the one in which the number of electrons with the same spin is maximized

A

hund’s rule

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27
Q

the vertical distance from the midline of a wave to the top of the peak or the bottom of the trough

A

amplitude

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28
Q

the amplitude of the wave is zero

A

node

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29
Q

describes how the electrons are distributed in the various atomic orbitals

A

electron configuration

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30
Q

when a solid is heated, it emits electromagnetic radiation

A

blackbody radiation

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31
Q

a substance can be seen by energizing a sample of material with some form of energy

A

emission spectrum

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32
Q

states that electrons are added to the lowest energy orbitals first moving to higher energy orbitals

A

aufbau principle

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33
Q

absorption of heat

A

endothermic

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34
Q

sum of the kinetic and potential energies of all the “particles” of a system

A

internal energy

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35
Q

the energy of the universe is constant

A

first law

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36
Q

everything else in the universe

A

surroundings

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37
Q

energy of object due to its motion (mass and velocity)

A

kinetic energy

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38
Q

the capacity to do work or to produce heat

A

energy

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39
Q

force acting over a distance

A

work

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40
Q

evolution of heat

A

exothermic

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41
Q

part of the universe on which we wish to focus our attention

A

system

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42
Q

the manner in which energy transfer is divided between transfer is divided between work and heat
-ex: ball rolling down hill

A

pathway

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43
Q

property of a system that depends only on its present state

A

state functions

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44
Q

energy due to position or compositions

A

potential energy

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45
Q

involves the transfer of energy between two objects due to difference in temperature

A

heat

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46
Q
  • kinetic energy- molecular motion

- potential energy- attractive/ repulsive interactions

A

internal energy (U)

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47
Q

the change in enthalpy that occurs when reactants are converted to products is the same whether the reaction occurs in one step or a series of steps

A

Hess’s Law

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48
Q

energy resulting from the interaction of charged particles

A

electrostatic energy

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49
Q

energy of motion

A

kinetic energy

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50
Q

exchange of mass and energy

A

open

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51
Q

are the rest of the universe
-ex: when heat is given off from the reaction of NaOH and HCL, the energy is transferred from the system to the surroundings

A

surroundings

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52
Q

is a state function defined as

A

enthalpy (H)

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53
Q

is the SI unit for energy

A

Joule (J)

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54
Q

equations that represent both mass and enthalpy changes

A

thermochemical equations

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55
Q

the transfer of heat from the surroundings of the system

A

endothermic

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56
Q

the measurement of heat changes

A

calorimetry

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57
Q

depend only on initial and final states of the system and not on how the change was carried out

A

state functions

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58
Q

the amount of heat required to raise the temp of 1 g of a substance by 1cC

  • units J/g C
  • relation to amount of heat (q)
A

specific heat (s)

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59
Q

is stored within structural units of chemical substances

A

chemical energy

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60
Q

the capacity to do work or transfer heat

A

energy

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61
Q

the amount of heat required to raise the temp of an object by 1 C

  • units J/C
  • relation to amount of heat (q)
A

heat capacity (c)

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62
Q

no exchange

A

isolated

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63
Q

exchange of energy

A

closed

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64
Q

energy of position

A

potential energy

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65
Q

-the study if the transfer of heat (thermal energy) in chemical reactions

A

thermochemistry

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66
Q

is the part of the universe of intrest

-ex: the reactants NaOH and HCL

A

system

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67
Q

transfer of heat from the system to the surroundings

A

exothermic

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68
Q

commonly used on food labels

A

calorie (cal)

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69
Q

two ionizable hydrogens

A

diprotic

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70
Q

used to signal the endpoint

A

indicator

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71
Q

shows only the reacting species in the chemical equation

-eliminates spectator ions

A

net ionic equation

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72
Q

the component that does the dissolving

A

solvent

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73
Q

two OH- groups

A

dibasic

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74
Q

higher ratio of solute to solvent

A

concentrated

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75
Q

proton acceptor

A

bronsted base

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76
Q

produces OH- in solution

A

Arrhenius base

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77
Q

smaller ratio of solute to solvent

A

dilute

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78
Q

process by which water molecules remove and surround individual ions from the solid

A

hydration

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79
Q

where the titration is stopped

A

endpoint

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80
Q
  • mass analysis

- ex: precipitation reaction

A

gravimetric analysis

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81
Q

three ionixable hydrogens

A

triprotic

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82
Q

shows all compounds represented by their chemical formulas

A

molecular equation

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83
Q

shows all strong electrolytes as ions and all other substances (non-electrolytes, weak electrolytes, gases) by their chemical formulas

A

ionic equation

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84
Q
  • partially ionized in solution
  • exist mostly as the molecular form in solution
  • weak acids and weak bases
A

weak electrolyte

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85
Q

one ionizable hydrogen

A

monoprotic

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86
Q

reactions

-one element undergoes both oxidation and reduction

A

disproportionation

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87
Q

is the ratio of moles solute per liter of solution

A

molarity

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88
Q

is the maximum amount of a solid that can dissolve in a given amount of solvent at a specified temperature
-prediction based on solubility rules

A

solubility

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89
Q

addition of a solution of known concentration (standard solution) to another solution of unknown concentration

A

titration

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90
Q

the component that is dissolved

A

solute

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91
Q
  • volume analysis

- ex:titration

A

volumetric analysis

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92
Q

a homogeneous mixture

A

solution

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93
Q

100% dissociation

-al water soluble ionic compounds, strong acids and strong bases

A

strong electrolyte

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94
Q

reactions

-common example, hydrocarbon fuel reacts with oxygen to produce carbon dioxide and water

A

combustion

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95
Q

is the amount of solute dissolved in a given amount of solvent

A

concentration

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96
Q

substance that dissolved in water produces a solution that does not conduct electricity

A

nonelectrolyte

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97
Q

substance that dissolved in water produces a solution that conducts electricity
-contains ions

A

electrolyte

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98
Q

produces H+ in solution

A

arrhenius acid

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99
Q

reaction between an acid and a base

A

neutralization

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100
Q

represents completion of the reaction

A

equivalence point

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101
Q

(formation of a solid from two aqueous solutions) occurs when product is insoluble

  • produce insoluble ionic compounds
  • double replacement (or metathesis reaction)
A

precipitation

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102
Q

the determination of the exact concentration of a solution

A

standardization

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103
Q

process of preparing a less concentrated solution from a more concentrated one

A

dilution

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104
Q

proton donor

A

bronsted acid

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105
Q

generic term meaning more than one ionizable hydrogen

A

polyprotic

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106
Q

ionic compounds separate into constituent ions when dissolved in solution

A

dissociation

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107
Q

formation of ions by molecular compounds when dissolved

A

ionization

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108
Q

one OH- group

A

monobasic

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109
Q

to maintain constant P and T, as V increases n must increase

A

avogadros’ law

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110
Q

empirical relationships among gas parameters

A

gas laws

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111
Q

gas molecules do not attract or repel one another, so one gas is unaffected by the other and the total pressure is a simple sum

A

dalton’s law

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112
Q

the pressure exerted by each gas in a gaseous mixture

A

partial pressure

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113
Q

an instrument used to measure atmospheric pressure

A

barometer

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114
Q

62.36

A

Ltorr/K*mol

115
Q

the volume of a gas sample is directly proportional to the number of moles in the sample at constant pressure and temperature

A

avogadro’s law

116
Q

8.314

A

m3Pa/Kmol or J/K*mol

117
Q

pressure-volume relationship at constant temperature

A

boyle’s law

118
Q

the mixing of gases as a results of random motion and collisions

A

diffusion

119
Q

a device used to measure pressures other than atmospheric pressure

A

manometer

120
Q

force per unit area

A

pressure

121
Q

0.08314

A

Lbar/Kmol

122
Q

unti of pressure

A

pascal

123
Q

1.987

A

cal/K*mol

124
Q

combing the historic gas laws yields

A

the ideal gas law

125
Q

0.08206

A

Latm/Kmol

126
Q

temperature-volume relationship at constant pressure

A

charles’ and guy-lussac’s law

127
Q

the escape of a gas from a container to a region of vacuum

A

effusion

128
Q

unit of force

A

newton

129
Q

the ratio of the number of moles of one component to the total number of moles in a mixture

A

mole fraction

130
Q

to maintain constant P, as V increases T must increase; fewer collisions require harder collisions

A

charles’ law

131
Q

the maximum amount of product predicted by stoichiometry

A

theoretical yield

132
Q

using balanced equations to find amounts

A

stoichiometry

133
Q

any species to the right of the arrow (formed)

A

product

134
Q

any species to the left of the arrow (consumed)

A

reactant

135
Q

the mass in amus of an ionic compound

A

formula mass (formula weight)

136
Q

the amount produced in a laboratory setting

A

actual yield

137
Q
  • (s) solid
  • (l) liquid
  • (g) gas
  • (aq) water solution
A

state symbols

138
Q

the reactant that is used up first in a reaction (limits the amount of product produced)

A

limiting reactant

139
Q

one product is formed

A

combination

140
Q

simplest whole-number ratio of atoms in a formula

A

empirical

141
Q

one reactant produces more than one product

A

decomposition

142
Q

the one that is left over

A

excess reactant

143
Q

same number and kind of atoms on each side of the equation

A

balanced

144
Q

the mass of one mole of a substance in grams

A

molar mass

145
Q

-the mass in amus of the individual molecule

A

molecular mass (molecular weight)

146
Q

a ratio of actual to theoretical(tells efficency of reaction)

A

percent yield

147
Q

analysis of organic compounds (C, H and sometimes O) are carried using an apparatus

A

combustion analysis

148
Q

a hydrocarbon reacts with oxygen to produce carbon dioxide and water

A

combustion

149
Q

the “true” ratio of atoms in a formula; often a whole-number multiple of the empirical formula

A

molecular

150
Q

nitrate

A

NO3-

151
Q

good conductors of heat and electricity (majority of elements on the table, located to the left of the stair step)

A

metals

152
Q
  • 5thh century B.C.
  • greek
  • “atomos”
  • which is to say “indivisible”
  • no substantial visual model
  • determine properties
A

Democritus

153
Q

reveal the elements present and in what whole-number ratio they are combined

A

empirical formula

154
Q

is the mass of the atom in atomic mass units (amu)

A

atomic number

155
Q
  • vertical columns

- elements in the same family have similar chemical and physical properties

A

families

156
Q

determines chemical properties

A

functional group

157
Q

hypochlorite

A

ClO-

158
Q

in between metals and nonmetals (those that lie along the separation line)

A

metalloids

159
Q

simplest examples of hydrocarbons

A

alkanes

160
Q

bicarbonate

A

HCO3-

161
Q

ions that are a combination of two or more atoms

A

polyatomic ions

162
Q
  • english..1808
  • billard ball model
  • solid sphere
  • determined composition
  • workable atomic theory
  • revived greek thoughts
A

Dalton

163
Q

chromate

A

Cr2O7-2

164
Q

hydrogen phosphate

A

HPO4-2

165
Q
  • suggested name “radioactivity”
  • rays were highly energetic and not deflected by a magnet
  • however, rays arose spontaneously unlike the rays discovered by roentgen
A

marie curie

166
Q

total num,ber of neutrons and protons present in the nucleus

A

mass number (A)

167
Q

is defined as a mass exactly equal to one-twelth the mass of one carbon- 12 atom

A

atomic mass unit

168
Q

carbonate

A

CO3-2

169
Q

nitrite

A

NO2-

170
Q

shows exact number of atoms of each element in a molecule

A

molecules

171
Q

hexa

A

6

172
Q

hydroxide

A

OH-

173
Q
  • 1910
  • gold foil experiment
  • nuclear model
  • what a surprise
A

Rutherford

174
Q

contain carbon and hydrogen (sometimes with oxygen, nitrogen, sulfur and the halogens)

A

organic compounds

175
Q

tetra

A

4

176
Q

Mercury(I)

A

Hg2+2

177
Q

chlorite

A

ClO2-

178
Q

determined the charge on an electron

A

milikan

179
Q

penta

A

5

180
Q

di

A

2

181
Q

peroxide

A

O2-2

182
Q

positively charged particles

A

alpha (a)

183
Q

combination of at least two atoms in a specific arrangement held together by chemical bonds

A

molecule

184
Q

one atom with a positive or negative charge

A

monatomic ion

185
Q

octa

A

8

186
Q

accidentally discovered that uranium darkened photographic film

A

antonine becquerel

187
Q

an atom or group of atoms that has a net positive or negative charge

A

ion

188
Q

ion with a net negative charge due to the gain of one or more electrons

A

anion

189
Q

ion with a net positive charge due to the loss of one or more electrons

A

cation

190
Q

Chlorate

A

ClO3-

191
Q
  • noticed that cathode rays caused glass and metal to emit another type of ray
  • he named the rays “X rays” because of their mysterious nature
  • caused fluoresence
  • were not defined by a magnet
A

wilhelm roentgen

192
Q

compounds that have a specific number of water molecules within their solid structure

A

hydrates

193
Q

mono

A

1

194
Q

dichromate

A

Cr2O7-2

195
Q

-discovered the ratio of the electric charge to the mass of an individual electron using the cathode ray tube

A

J.J. Thomson

196
Q

bisulfate

A

HSO4-

197
Q

shows the general arrangement of atoms within the molecule

H-O-H

A

structural formula

198
Q

cyanide

A

CN-

199
Q

horizontal rows

A

periods

200
Q

one of the two or more distinct forms of an element

-ex: oxygen, ozone, diamond and graphite

A

allotrope

201
Q

states that if two elements can combine to form more than one compound with each other, the masses of the one element that combine with a fixed mass of the other element are in ratios of small whole numbers

A

law of multiple proportions

202
Q

sulfate

A

SO4-2

203
Q

2 different atoms

A

heteronuclear- diatomic molecules

204
Q

tri

A

3

205
Q

azide

A

N3-

206
Q

perchlorate

A

ClO4-

207
Q

deca

A

10

208
Q

2 of the same atoms

A

homonuclear- diatomic molecules

209
Q

sulfite

A

SO3-2

210
Q

describes a substance that spontaneously emits radiation

A

radioactive

211
Q

contain only carbon and hydrogen

A

hydrocarbons

212
Q

electrons

A

beta (B)

213
Q

thiocyanate

A

SCN-

214
Q
  • contain more than 2 atoms
  • most molecules
  • may contain more than one element
  • ex: ozone, o3; white phosphorus, p4; water, h2o, and methane CH4
A

polyatomic molecules

215
Q

states that different samples of a given compound always contain the same elements in the same mass ratio

A

law of definite proportions

216
Q

no charge and are unaffected by external electric or magnetic fields

A

gamma (y)

217
Q

a substance that produces hydrogen ions (H+) when dissolved in water

A

acid

218
Q
  • all atoms are not identical (as proposed by Dalton)

- same atomic number (Z) but different mass numbers (A)

A

isotopes

219
Q

nonconductors (located in upper right-hand corner)

A

nonmetals

220
Q
  • early 1900’s
  • discovered e’s
  • plum-pudding model
  • but blueberry muffin model is better
A

JJ Thomson

221
Q

phosphate

A

PO4-3

222
Q

ammonium

A

NH4+

223
Q

dihydrogen phosphate

A

H2PO4-

224
Q

oxalate

A

C2O4-2

225
Q

number of protons in the nucleus of each atom of an element

A

atomic number (Z)

226
Q
  • many contributors
  • schroedinger a key player
  • probability model with electron cloud
  • 1920’s
A

Quantum-Mechanical

227
Q

phosphite

A

PO3-3

228
Q

hydronium

A

H3O+

229
Q

nona

A

9

230
Q

permanganate

A

MnO4-

231
Q

hepta

A

7

232
Q
  • 1913
  • planetary model
  • energy levels
  • defined orbits
  • not bad for the time
A

Bohr

233
Q

deci (d)

A

1 x 10^-1

234
Q

does not depend on amount

-ex: density, temperature, color

A

intensive property

235
Q

temperature

A

kelvin (K)

236
Q
  • particles close together but not held rigidly in position
  • particles are free to move past one another
  • a liquid sample conforms to the shape of the part of the container it fills
A

liquid

237
Q

a problem solving method employing conversion factors to change one measure to another often called the “factor-label method”

A

dimensional analysis

238
Q
  • celsius
  • represented by C
  • based on freezing point of water as 0C and boiling point of water as 100C
A

temperature

239
Q
  • composition of the mixture is uniform throughout

- ex: sugar dissolved in water

A

homogeneous

240
Q

how closely measurements of the same thing are to one another

A

precision

241
Q

-a fraction in which the same quantity is expressed one way in the numerator and another way in the denominator

A

conversion factor

242
Q

can be observed and measured without changing the substance

-ex: color, melting point, states of matter

A

physical properties

243
Q

the identity of the substance stays the same

-ex: changes of state (melting, freezing)

A

physical changes

244
Q

expressed using numbers

A

quantitative

245
Q

aluminum foil

A

substance, element

246
Q

the study of matter and the changes that matter undergoes

A

chemistry

247
Q

baking soda

A

substance, compound

248
Q

centi (c)

A

1 x 10^-2

249
Q

electric current

A

ampere (A)

250
Q

used to express the uncertainty of inexact numbers obtained by measurement

A

significant figures

251
Q

numbers with defined values

-ex: counting numbers, conversation factors based on definitions

A

exact numbers

252
Q

depends on amount of matter

-ex: mass, length

A

extensive property

253
Q

milli (m)

A

1 x 10^-3

254
Q

time

A

second (s)

255
Q

pico (p)

A

1 x 10^-12

256
Q
  • can be either an element or a compound
  • has a definite (constant) composition and distinct properties
  • examples: Sodium chloride, water, oxygen
A

substance

257
Q

must be determined by the chemical changes that are observed
-ex: flammability, acidity, corrosiveness, reactivity

A

chemical properties

258
Q

anything that has mass and occupies space

A

matter

259
Q

mega (M)

A

1 x 10^6

260
Q
  • particles close together in orderly fashion
  • little freedom of motion
  • a solid sample does not conform to the shape of the container it fills
A

solid

261
Q

how close a measurement is to the true or accepted value

A

accuracy

262
Q
  • physical combination of two or more substances
  • substances retain distinct identities
  • no universal constant composition
  • can be separated by physical means
  • ex: sugar/iron; sugar/water
A

mixture

263
Q

tera (T)

A

1 x10^12

264
Q

ratio of mass to volume

A

density

265
Q
  • represented by K (no degree sign)
  • the absolute scale
  • units of Celsius and Kelvin are equal in magnitude
  • fahrenheit(the English system) (F)
A

Kelvin

266
Q

kilo (k)

A

1 x 10^3

267
Q

cannot be separated into simpler substances by chemical means
-examples: iron, mercury, oxygen, and hydrogen

A

element

268
Q

copper wire

A

substance, element

269
Q

nano (n)

A

1 x 10^-9

270
Q

milk

A

mixture, homogeneous

271
Q

air

A

mixture, homogeneous

272
Q
  • two or more elements chemically combined in define ratios
  • cannot be separated by physical means
  • examples: salt, water, and carbon dioxide
A

compounds

273
Q

length

A

meter (M)

274
Q

expressed using properties

A

qualitative

275
Q

giga (G)

A

1 x 10^9

276
Q

after a chemical change, the original substance no longer exists
-ex: combustion, digestion

A

chemical changes

277
Q

numbers obtained by any method other than counting

-ex: measured values in the laboratory

A

inexact numbers

278
Q

micro (1u)

A

1 x 10^-6

279
Q
  • particles randomly spread apart
  • particles have complete freedom of movement
  • assumes both shape and volume of a container
A

gas

280
Q
  • measure of the amount of matter

- weight refers to gravitational pull

A

mass

281
Q

amount of substance

A

mole (mol)

282
Q
  • composition is not uniform throughout

- ex: sugar mixed with iron fillings

A

heterogeneous

283
Q

mass

A

kilogram (kg)

284
Q

The study of matter and the changes that matter undergoes

A

Chemistry

From Flashcardlet (2 decks)

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