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Chemistry 1320 > Exam 1 > Flashcards

Exam 1 Flashcards

1
Q

Polyatomic Ion

A

an ion composed of more than one atom

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2
Q

What are the polyatomic ions?

A

OH- Hydroxide
NO3- Nitrate
SO4-2 Sulfate

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3
Q

Examples of Chemistry in everyday life

A

digesting food
synthesizing polymers for clothing, cookware, and credit cards
refining cruel oil into gasoline and other products

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4
Q

The 3 domains of chemistry

A

Macroscopic
microscopic
symbolic

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5
Q

Macroscopic

A

realm of everyday things that are large enough to be sensed directly by human sight or touch

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6
Q

Microscopic

A

almost always visited in the imagination. some aspects are only visible through a microscope

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7
Q

Symbolic

A

the specialized language used to represent components of the macroscopic and microscopic domains

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8
Q

Matter

A

anything that occupies space and has mass

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9
Q

Solid

A

is rigid and possesses a definite shape

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10
Q

liquid

A

flows and takes the shape of its container

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11
Q

Gas

A

takes both the shape and volume of its container

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12
Q

Plasma

A

a gaseous state of matter that contains an appreciable amount of electrically charged particles

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13
Q

Mass

A

a measure of the amount of matter in an object

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14
Q

Weight

A

refers to the force that gravity exerts on an object

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15
Q

Law of Conservation of Matter

A

There is no detectable change in the total quantity of matter present when matter converts from one type to another

True for both chemical and physical changes

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16
Q

Element

A

a type of pure substance that cannot be broken down into simpler substances by chemical changes

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17
Q

Compounds

A

pure substances that can be broken into simpler substances by chemical changes

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18
Q

The two types of mixtures

A

Homogenous
heterogeneous

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19
Q

Homogenous mixture

A

exhibits a uniform composition and appears visually the same throughout

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20
Q

Solution

A

another name for homogenous mixture

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21
Q

Heterogenous mixture

A

has a composition that varies from point to point

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22
Q

Atom

A

the smallest particle of an element that has the properties of that element and can enter into a chemical combination

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23
Q

Molecules

A

consists of two or more atoms connected by strong forces known as chemical bonds

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24
Q

Properties

A

the characteristics that enable us to distinguish one substance from another

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25
Q

Physical property

A

a characteristic of matter that is not associated with a change in its chemical composition

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26
Q

Examples of Physical properties

A

density
color
hardness
melting and boiling points
electrical conductivity

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27
Q

Physical change

A

a change in the state or properties of matter without any accompanying change in its chemical composition

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28
Q

Chemical property

A

the change of one type of matter into another type (or the inability to change)

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29
Q

Examples of a chemical property

A

flammability
toxicity
acidity
reactivity
and heat of combustion

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30
Q

Extensive property

A

depends on the amount of matter present

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31
Q

Examples of an extensive property

A

mass, volume, heat

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32
Q

Intensive property

A

Does not depend on the amount of matter present

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33
Q

Examples of an intensive property

A

density
temperature
boiling point

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34
Q

Measurements provide three kinds of information

A

number- the size or magnitude of the measurement
unit- a standard of comparison for the measurement
indication of the uncertainty of the measurement

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35
Q

Femto f

A

10 to the -15

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36
Q

pico p

A

10 to the -12

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37
Q

nano n

A

10 to the -9

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38
Q

micro m

A

10 to the -6

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39
Q

mili m

A

10 to the -3

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40
Q

centi c

A

10 to the -2

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41
Q

deci d

A

10 to the -1

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42
Q

kilo k

A

10 to the 3

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43
Q

mega M

A

10 to the 6

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44
Q

giga G

A

10 to the 9

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45
Q

tera T

A

10 to the 12

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46
Q

SI unit of length

A

meter (m)

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47
Q

SI unit of mass

A

kilogram (kg)

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48
Q

SI unit of temperature

A

kelvin (K)

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49
Q

SI unit of time

A

second (s)

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50
Q

Volume

A

the measure of the amount of space occupied by an object

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51
Q

SI unit of volume

A

cubic meter (m3)

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52
Q

density

A

the ration of the mass of a sample of the substance to its volume

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53
Q

Density formula

A

mass divided by volume

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54
Q

SI unit for density

A

kilogram per cubic meter (kg/m3)

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55
Q

Exact number

A

result of a counting measurement, the only type of measurement that is free from uncertainty

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56
Q

significant figures

A

all the digits in a measurement, including the uncertain last digit

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57
Q

Are nonzero digits significant figures

A

yes always

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58
Q

are captive zeroes significant figures

A

Yes always

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59
Q

Are trailing zeroes significant figures

A

only when they are to the right of the decimal place or in scientific notation

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60
Q

Are leading zeroes significant figures

A

no

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61
Q

What is the significant figures rule when adding or subtracting numbers

A

round to the same number of decimal places as the number with the least number of decimal places

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62
Q

What is the significant figures rule when multiplying or dividing

A

round to the same number of digits as the number with the least number of significant figures

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63
Q

Less than 5

A

round down

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64
Q

more than 5

A

round up

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65
Q

deciding digit is 5

A

go up or down but make sure it ends up even

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66
Q

A measurement is precise if

A

it yields very similar results when repeated in the same manner

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67
Q

A measurement is accurate if

A

it yields a result that is very close to the true or accepted value

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68
Q

Dimensional analysis

A

the mathematical approach based on the premise that the units of quantities must be subjected to the same mathematical operations as their associated numbers

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69
Q

Conversion factor

A

a ratio of two equivalent quantities expressed with different measurement units

70
Q

Celsius scale
water freezes at

A

0

71
Q

Celsius scale
water boils at

A

100

72
Q

Fahrenheit scale
water freezes at

A

32

73
Q

Fahrenheit scale
water boils at

A

212

74
Q

Kelvin scale
water freezes at

A

273.15

75
Q

Kelvin scale
water boils at

A

373.15

76
Q

Dalton’s Atomic Theory

A
  1. Matter is composed of exceedingly small particles called atoms. An atom is the smallest unit of an element that can participate in a chemical change
  2. An element consists of only one type of atom, which has a mass that is characteristic of the element and is the same for all atoms of that element
  3. Atoms of one element differ in properties from atoms of all other elements
  4. A compound consists of atoms of two or more elements combined in a small, whole-number ratio. In a given compound, the number of atoms of each of its elements are always present in the same ratio
  5. Atoms are neither created nor destroyed during a chemical change, but instead rearrange to yield a different type of matter
77
Q

Law of Conservation of Matter

A

Atoms are neither created nor destroyed during a chemical change, then the total mass present when matter changes from one type to another will remain constant

78
Q

Law of definite proportions

A

all samples of a pure compound contain the same elements in the same proportion by mass

79
Q

Who discovered the electron

A

J.J. Thompson

80
Q

How did J.J. Thompson discover the electron

A

Cathode ray tube
when a high voltage was applied across electrodes, a visible beam called a cathode ray appeared between them. Always deflected towards the positive charge and away from the negative charge
Much lighter than atoms

81
Q

Electron

A

a negatively charged, subatomic particle with a mass more than one thousand times less than that of an atom

82
Q

Robert A Millikan did what experiment

A

Oil drop experiment

83
Q

What did the oil drop experiment find

A

The charge of the oil drops were always a multiple of a specific charge, so Millikan concluded that 1.6 x 10 to the -19 C was the charge of a single electron
Mass of an electron=9.107 x 10 to the -31 kg

84
Q

Thompson thought atoms resembles _______ While Nagaoka proposed that atoms resembled ________

A

Plum pudding
Saturn

85
Q

Who discovered the nucleus

A

Ernest Rutherford

86
Q

What experiment did Ernest Rutherford perform

A

Gold foil scattering experiment

87
Q

What did the Gold foil scattering experiment find

A

The volume occupied by an atom must consist of a large amount of empty space.
A small, relatively heavy, positively charged body, the nucleus must be at the center of each atom
nucleus contained most of the atom’s mass
Negatively charged electrons surround the nucleus
the proton is located in the nucleus

88
Q

Proton

A

a positively charged, subatomic particle located in the nucleus

89
Q

Isotopes

A

Atoms of the same element that differ in mass

90
Q

Neutrons

A

uncharged, subatomic particles with a mass approximately the same as that of protons
also found in the nucleus

91
Q

How are electrons and protons similar

A

charged subatomic particles

92
Q

How are electrons and protons different

A

Different masses
Electron- negatively charged, in the rings around the nucleus
Proton- positively charged, in the nucleus

93
Q

How are protons and neutrons simialar

A

same mass
both in the nucleus

94
Q

How are protons and neutrons different

A

Protons are positive
Neutrons have no charge

95
Q

What contains the majority of an atom’s mass

A

the nucleus

96
Q

What occupy almost all of an atom’s volume

A

Electrons

97
Q

amu

A

Atomic mass unit

98
Q

e

A

fundamental unit of charge

99
Q

Properties of a proton

A

Mass- 1.0073 amu
charge- +1

100
Q

Properties of a neutron

A

Mass- 1.0087 amu
Charge- 0

101
Q

Properties of an electron

A

Mass-0.00055 amu
Charge- -1

102
Q

Atomic Number

A

the number of protons in the nucleus of an atom
the key to identifying atoms

103
Q

Neutral atoms

A

the number of protons equals the number of electrons

104
Q

Mass number

A

the total number of protons and neutrons in an atom

105
Q

How to find the number of neutrons

A

the difference between the mass number and the atomic number

106
Q

Ions

A

when the number of protons and electrons are not equal, the atom is electrically charged

107
Q

equation for charge of an atom

A

number of protons-number of electrons

108
Q

Atoms acquire charge by

A

losing or gaining electrons

109
Q

Anion

A

an atom that gains one or more electrons and exhibits a negative charge

110
Q

cation

A

an atom that loses one or more electrons and exhibits a positive charge

111
Q

Chemical symbol

A

an abbreviation that we use to indicate an element or an atom of an element

112
Q

Isotopes have

A

the same number of protons but the number of neutrons are different

113
Q

Each proton and neutron has a mass of

A

about 1 amu

114
Q

Electrons weigh less/more than a proton or neutron

A

far less

115
Q

Atomic mass of a single atom in amu is approximately equal to its

A

mass number

116
Q

Average mass

A

(fractional abundance x isotopic mass)
Example: Boron
19.9% 10B with a mass of 10.0129 amu
80.1% 11B with a mass of 11.0093
=(0.199 x 10.0129 amu)+(0.801x11.0093 amu)
= 10.81 amu -> what is on the periodic table

117
Q

Mass spectrometry

A

how to find the occurrence and natural absences of isotopes

118
Q

Molecular formula

A

a representation of a molecule or compound which consists of the following
- chemical symbols to indicate the types of atoms
- subscripts after the symbol to indicate the number of each type of atom in the molecule

119
Q

Structural formula

A

shows the same information as a molecular formula but also shows how the atoms are connected

120
Q

Empirical formula

A

indicates the simplest whole-number ratio of the number of atoms (or ions) in the compound

121
Q

molecular formula

A

indicates the actual numbers of atoms of each elements in a molecule of a compound

122
Q

Isomers

A

compounds with the same chemical formula but different molecular structures

123
Q

Structural Isomers

A

Molecules that have the same formula but different structures and therefore different chemical properties

124
Q

Mole

A

is an amount unit
defined as the amount of a substance containing the same number of discrete entities (such as atoms, molecules, or ions)

125
Q

A mole provides

A

a link between the mass of a sample and the number of atoms, molecules, or ions in that sample

126
Q

Avogadro’s Number

A

the number of entities composing a mole
6.02214179 x 10^23

127
Q

molar mass

A

of an element is the mass in grams of 1 mole of that substance, a property expressed in units of grams per mole

128
Q

molar mass of a substance is equivalent to

A

its atomic or formula mass in amu
- a single 12C atom has a mass of 12 amu
-a mole of 12C atoms have a mass of 12 g

129
Q

Particles and waves are connected on a fundamental level called

A

wave-particle duality

130
Q

Wave

A

an oscillation or periodic movement that can transport energy from one point in space to another

131
Q

Speed of light

A

c= 2.998 x 10^8 m/s

132
Q

Wavelength

A

distance between two consecutive peaks or troughs in a wave

133
Q

Frequency

A

Number of successive wavelengths that pass a given point in a unit time

134
Q

Amplitude

A

One-half the distance between the peaks and troughs

135
Q

Waves are characterized by

A

Wavelength
frequency
amplitude

136
Q

hertz (Hz)

A

the unit for frequency

137
Q

common multiples of hertz

A

Megahertz (1 MHz= 1 x 10^6 Hz)
Gigahertz (1 GHz= 1 x 10^9 Hz)

138
Q

The product of a wave’s wavelength and its frequency is

A

the speed of the wave

139
Q

wavelength and frequency are

A

inversely proportional
as the wavelength increases, the frequency decreases and vice versa

140
Q

Electromagnetic spectrum

A

the range of all types of electromagnetic radiation

141
Q

Frequency=

A

speed of light divided by amplitude

142
Q

Interference patterns

A

arise when light passes through narrow slits closely spaced about a wavelength apart

143
Q

Dark regions correspond to regions where the peaks for the wave from one slit happen to coincide with the troughs for the wave from the other slit

A

destructive interference

144
Q

brightest regions correspond to the regions where the peaks for the two waves happen to coincide

A

constructive interference

145
Q

Standing waves

A

remain constrained within some region of space
play an important role in understanding of the electronic structure of atoms and molecules

146
Q

one-dimensional standing wave

A

a vibrating string that is held fixed at its two end points is an example of this

147
Q

quantization

A

only discrete values from a more general set of continuous values are observed
a system with fixed end points restricts the number and type of possible waveforms is an example of this

148
Q

nodes

A

harmonic waves all have one or more points between the two end points that are not in motion
these points are called nodes

149
Q

Continuous spectrum

A

sunlight consists of a range of broadly distributed wavelengths that form

150
Q

Blackbody

A

a convenient, ideal emitter that approximates the behavior of many materials when heated

151
Q

ultraviolet catastrophe

A

theoretical expressions as functions of temperature fit the observed experimental blackbody curves well at larger wavelengths.
but there are significant discrepancies at shorter wavelengths

152
Q

Planck’s constant

A

quantity h
h=6.626 x 10^34 J s
used for the understanding of motions of atoms and subatomic particles, as well as how quantum mechanics and modern electronics operate

153
Q

Photoelectric effect

A

the emission of electrons when electromagnetic radiation, such as light hits a material
does not depend on the brightness of the light but increased with increasing frequency of light

154
Q

Photons

A

A particle representing a quantum of light or other electromagnetic radiation. A photon carries energy proportional to the radiation frequency but has zero rest mass

155
Q

Wave particle duality

A

at deep fundamental level still not fully understood light is both wavelike and particle-like

156
Q

Electrons are ejected when hit by

A

photons having sufficient energy (a frequency greater than the threshold

157
Q

Photons produced in this manner have a range of energies, and thereby produce a

A

continuous spectrum

158
Q

Continuous spectrum

A

an unbroken series of wavelengths

159
Q

Line spectra

A

very narrow line widths interspersed throughout the spectral regions
each element displays its own characteristic set of lines

160
Q

According to classical electromagnetic theory, only ________ should be observed

A

continuous spectra

161
Q

Rydberg constant

A

1.097 x 10^7 m^-1

162
Q

empirical formula that predicted all of hydrogen’s emission lines

A

1/amplitude= Rydberg constant (1/N1^2- 1/N2^2)

163
Q

Bohr’s work convinced scientists to abandon classical physics and spurred the development of modern

A

quantum mechanics

164
Q

Bohr incorporated what into classical mechanics description of the atom

A

Planck’s ideas of quantization
Einstein’s finding that light consists of photons whose energy is proportional to their frequency
assumed that the electron orbiting the nucleus would not normally emit any radiation
rather the electron emits or absorbs a photon if it moved to a different orbit

165
Q

When the electron is in this lowest energy orbit (n=1), the atom is said to be in its

A

ground state

166
Q

If the atom receives energy from an outside source, it is possible for the electron to move to an orbit with a higher n value

A

excited state
which has a higher energy

167
Q

When the atom absorbs energy as a photon, th electron

A

moves from an orbit with a lower n to a higher n

168
Q

when an electron falls from an orbit with a higher n to a lower n, the atom

A

emits energy as a photon

169
Q

limitations of the Bohr model

A

unable to extend his theory to the next atom, He
does not account for electron-electron interactions in atoms with more than one electron

170
Q

quantum numbers

A

integer numbers having only specific allowed values and used to characterize the arrangement of electrons in an atom

171
Q

Wave-particle duality first observed with photons is actually a

A

fundamental behavior intrinsic to all quantum particles

172
Q

Heisenberg Uncertainty Principle

A

it is fundamentally impossible to determine simultaneously and exactly both the momentum and the position of a particle

Chemistry 1320 (2 decks)

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