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Fall 2017 > Chem 105 Test 1 (Ch. E-2) > Flashcards

Chem 105 Test 1 (Ch. E-2) Flashcards

1
Q

qualitative observations

A

descriptive in nature (e.g., changes in color/physical shape)

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2
Q

quantitative observations

A

measurements, counted values

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3
Q

measurements are a numerical value with a ? and ? unit

A

scalar and dimensional

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4
Q

systematic or determinate error

A

error is in the same direction (either higher or lower than should be)

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5
Q

random/indeterminate error

A

equal probability of measurement being lower or higher than it should be; difficult to correct/find source

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6
Q

SI unit for length, mass, time, temp, amount of a substance, electric current, and luminous intensity

A

meter (m), kilogram (kg), second (s), Kelvin (K), mole (mol), ampere (A), candela (cd)

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7
Q

mega- (M)

A

base x 10^4

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8
Q

kilo- (k)

A

base x 10^3

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9
Q

deci- (d)

A

base x 10^-1

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10
Q

centi- (c)

A

base x 10^-2

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11
Q

milli- (m)

A

base x 10^-3

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12
Q

micro- (mc or µ)

A

base x 10^-6

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13
Q

nano- (n)

A

base x 10^-9

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14
Q

pico- (p)

A

base x 10^-12

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15
Q

water boils at

A

212 F, 100 C, 373 K

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16
Q

water freezes at

A

32 F, 0 C, 273 K

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17
Q

absolute zero

A

-459 F, -273 C, 0 K

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18
Q

how to convert degrees Celsius to degrees Fahrenheit

A

F = 1.8(C) + 32

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19
Q

how to convert degrees Celsius to Kelvin

A

T(K) = t(*C) + 273.15

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20
Q

precision

A

repeat-ability

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21
Q

accuracy

A

actual closeness to value

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22
Q

significant figures rules

A

leading zeroes are not significant, trailing zeroes after a nonzero digit are not significant unless there is a decimal point

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23
Q

multiplication and division with significant figures

A

the least precise value determines the number of significant figures

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24
Q

addition and subtraction with significant figures

A

the value with the smallest decimal measurement determines the number of significant figures

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25
Q

density

A

mass / volume; an intensive physical property

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26
Q

physical or chemical changes in matter result in matter either gaining or releasing energy, which is ?

A

the capacity to do work

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27
Q

work

A

the action of a force applied across a distance

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28
Q

force

A

a pull or push on an object

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29
Q

electrostatic force

A

the push or pull on objects that have an electrical charge

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30
Q

first law of thermodynamics

A

energy of the universe is conserved

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31
Q

system

A

the area or location under study

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32
Q

universe

A

the system and its surroundings

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33
Q

endothermic reaction

A

heat transfers from surroundings to the system; the energy of the system increases, the energy and temperature of the surroundings decreases

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34
Q

exothermic reaction

A

heat transfers from the system to the surroundings; the energy of the system decreases, the energy and temperature of the surroundings increase

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35
Q

Calorie (cal)

A

the amount of heat needed to raise the temperature of 1g H2O by 1*C (1 cal = 4.184 J)

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36
Q

Kilocalorie (kcal)

A

1 kcal = 1000 cal = 4184 J

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37
Q

Joule (J)

A

the amount of heat that will change the temperature of 1g H2O by 1*C (4.184 J = 1 cal)

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38
Q

Kilojoule (kJ)

A

1 kJ = 1000 J

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39
Q

Diet Calorie (Cal or C)

A

1 diet calorie = 1 kcal = 1000 calories

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40
Q

kilowatt-hour (kWh)

A

1 kWh = 3.60 x 10^6 J

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41
Q

matter

A

anything that has mass and occupies space

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42
Q

atoms

A

basic submicroscopic particles that constitute the fundamental building blocks of ordinary matter

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43
Q

molecules

A

substances formed when two or more atoms come together (bond) in specific geometric arrangements

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44
Q

matter can be classified according to ? and ? (and define)

A

its state (its physical form - S, L, G - based on what properties it exhibits) and its composition (the types of particles - elements, compounds, mixtures)

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45
Q

matter can be broken down into two categories based on whether it is one type of particle or not

A

yes > pure substance

no > mixture

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46
Q

pure substances can be broken down into two categories based on whether it is separable into simpler substances

A

no > element

yes > compound

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47
Q

mixtures can be broken down into two categories based upon whether they are uniform throughout

A

no > heterogeneous (e.g. wet sand)

yes > homogeneous (e.g. tea with sugar)

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48
Q

element

A

a substance that cannot be chemically broken down into simpler substances; basic building block of matter; composed of a single type of atom

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49
Q

compound

A

a substance composed of 2+ elements in fixed, definite proportions

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50
Q

scientific method steps

A

observations, formulation of hypothesis, experimentation, formulation of laws and theories

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51
Q

law

A

what, empirical; a brief statement that summarizes past observations and predicts future ones

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52
Q

theory

A

why; a well-established hypothesis or set of hypotheses form the basis for a scientific theory; can be validated by experimental results, but can never be conclusively proven

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53
Q

observation

A

describes characteristics/behavior of nature

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54
Q

hypothesis

A

a tentative interpretation or explanation of the observations

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55
Q

a good hypothesis is ?

A

falsifiable (able to be proven wrong)

56
Q

? and ? were the first to propose that matter was composed of small, indestructible particles

A

Leucippus and Democritus

57
Q

Dalton’s atomic theory

A
  1. each element is composed of tiny, indestructible particles called atoms
  2. all atoms of a given element have the same mass and other properties that distinguish them from the atoms of other elements
  3. atoms combine in simple, whole-number ratios to form compounds
  4. atoms of one element cannot change into atoms of another element; in a chemical reaction, atoms change only the way that they are bound together with other atoms
58
Q

the law of conservation of mass

A

in a chemical reaction, matter is neither created nor destroyed

59
Q

Proust’s law of definite proportions

A

all samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements

60
Q

Dalton’s law of multiple proportions

A

when two elements (call them A and B) form two different compounds, the masses of element B that combine with one gram of element A can be expressed as a ratio of small whole numers

61
Q

JJ Thompson’s cathode ray experiments

A

discovered the electron

62
Q

Millikan’s oil drop experiement

A

determined the charge of an electron (-1.60x10^-19 C/e-)

63
Q

JJ Thompson’s plum pudding model

A

negatively charged electrons were small particles held within a positively charged sphere

64
Q

Rutherford’s gold foil experiment results and conclusion

A

a majority of the particles did not pass directly through the foil, but some were deflected while some even bounced back; matter must not be as uniform as it appears - it must contain large regions of empty space dotted with small regions of very dense matter

65
Q

nuclear theory of the atom

A
  1. most of the atom’s mass and all of its charge are contained in a small core called a nucleus
  2. most of the volume of the atom is empty space, throughout which tiny, negatively charged electrons are dispersed
  3. there are as many negatively charged electrons outside the nucleus as there are positively charged particles (protons) within the nucleus, so that the atom is electrically neutral
66
Q

later work by Rutherford and his student James Chadwick demonstrated that ?

A

the previously unaccounted for mass was due to neutrons - the neutral particles within the nucleus

67
Q

the mass of the ? and ? are most similar

A

proton and neutron

68
Q

the charge of the ? and ? are equal in magnitude but opposite in sign

A

proton and electron

69
Q

charge of an electron

A

-1.60218x10^-19 C

70
Q

mass of an electron

A

0.00091x10^-27 kg

71
Q

the number of ? defines the element; it is its atomic number (Z)

A

protons

72
Q

isotopes

A

all atoms of a given element have the same number of protons, but not necessarily the same number of neutrons

73
Q

mass number (A) represents

A

the sum of the number of neutrons and protons in an atom

74
Q

format for representing isotopes (2 options)

A

1) the chemical symbol with the mass number to the top left and the atomic number to the bottom left of it
2) chemical symbol/name - mass number (X-A)

75
Q

natural abundance of isotopes

A

the percentage value of the relative amount of each different isotope in a naturally occurring sample of a given element

76
Q

ions

A

the number of electrons in a neutral atom is equal to the number of protons in its nucleus, but, in chemical changes, atoms can lose or gain electrons and become charged particles called ions

77
Q

positively charged ions

A

cations (formed from metal elements)

78
Q

negatively charged ions

A

anions (formed from nonmetal elements)

79
Q

atomic mass

A

the average mass of the isotopes that compose that element, weighted based on the element’s natural abundance of each isotope

80
Q

how to calculate atomic mass

A

the sum of the (fraction of isotope n) x (mass of isotope n)

81
Q

mass spectometry

A

measures the masses of atoms and the % abundance of isotopes of an element by separating particles according to their mass

82
Q

Avogadro’s number (1 mole = ?)

A

6.022x10^23

83
Q

subatomic particles of matter

A

electrons, protons, neutrons

84
Q

natural duality of subatomic particles

A

appear to exist in two conditions; wave-matter duality concept

85
Q

the quantum mechanical model tells us (3 things) about an atom’s electrons

A
  1. it explains the manner in which electrons exist and behave in an atom
  2. it forms the foundation of chemistry by explaining the periodic table and its trends, the behavior of elements in chemical bonding, and the colors of the atoms/their size
  3. it predicts the atomic properties that are directly related to the behavior of the electrons
86
Q

light

A

a form of electromagnetic radiation; composed of perpendicular oscillating waves (one for the electric field and one for the magnetic field)

87
Q

speed of light

A

3.00 x 10^8 m/s

88
Q

frequency (v or nu)

A

the number of waves that pass a point in a given period of time; units are Hertz (Hz) or cycles/s (s^-1) (1 Hz = 1 s^-1)

89
Q

total energy (E)

A

proportional to the amplitude of the waves and their frequency

90
Q

frequency equation

A

v = c / λ

91
Q

visible light

A

400 to 700 nm (red to violet)

92
Q

? light has the lowest frequency

A

radio-wave

93
Q

? light has the highest frequency

A

gamma-ray

94
Q

constructive interference

A

waves that interact so that they add to make a larger wave are said to be in phase

95
Q

destructive interference

A

waves that interact so that they cancel each other are said to be out of phase

96
Q

diffraction

A

when traveling waves encounter an obstacle or opening in a barrier that is about the same size as the wavelength, they bend around it

97
Q

interference pattern

A

a characteristic of all light waves; the diffracted of light through two slits separated by a distance comparable to the wavelength results in an interference pattern of the diffracted waves

98
Q

photoelectric effect

A

when light is shined on a metal surface, electrons are produced from the surface

99
Q

experimental observations of the photoelectric effect

A

a minimum frequency was needed before electrons would be emitted regardless of the intensity, called the threshold frequency; high-frequency light from a dim source caused electron emission without any lag time

100
Q

Energy equation

A

E = hv = h (c / λ)

101
Q

Planck’s Constant (h)

A

6.626x10^-34 J*s

102
Q

kinetic energy of the ejected electron

A

Ephoton - Ebinding (hv - Φ)

103
Q

emission spectrum

A

when the light emitted when atoms or molecules absorb energy passes through a prism, a pattern of particular wavelengths of light is seen that is unique to that type of atom or molecule

104
Q

? can be used to identify the elements present in a material as each element has its own unique spectrum

A

line spectra

105
Q

Bohr developed a model of the atom to explain

A

how the structure of an atom changes when it undergoes energy transitions

106
Q

Bohr model of the atom

A

electrons travel in orbits that are at a fixed distance from the nucleus; electrons emit radiation when they “jump” from an orbit with higher energy down to an orbit with lower energy

107
Q

De Broglie proposed that particles could have wave-like character and predicted that the wavelength of a particle was inversely proportional to its momentum; relation:

A

λ = h / (mass * velocity)

108
Q

1 J = 1 ?

A

kg * m^2 / s^2

109
Q

electrons behavior characteristics

A

from particulate perspective (e.g. matter, mass) particle nature = position
from energy perspective (e.g. wavelength, frequency) wave nature = interference pattern

110
Q

the wave and particle nature of the electron are ? properties, meaning ?

A

complementary - the more you know about one, the less you know about the other

111
Q

Heisenberg’s Uncertainty Principle

A

Heisenberg states that the product of the uncertainties in both the position and speed of a particle was inversely proportional to its mass (Δx * mΔv > h/4pi)

112
Q

determinacy

A

definite, predictable future

113
Q

indeterminacy

A

indefinite future, can only predict probability

114
Q

why can’t we predict an electron’s path?

A

according to classical physics, particles move in a path determined by the particle’s velocity, position, and forces acting on it, but we cannot know both the position and velocity of an electron - the best we can do is to describe the probability an electron will be found in a particular region using statistical functions

115
Q

Schrodinger’s Equation

A

Hψ = Eψ; allows us to calculate the probability of finding an electron with a particular amount of energy at a particular location in the atom; solutions may produce wave functions, ψ

116
Q

a plot of distance versus ψ^2 represents ?

A

an orbital, a probability distribution map of a region where the electron is likely to be found

117
Q

4 quantum numbers

A

principal quantum number (n - energy), angular momentum quantum number (l - orbital type), magnetic quantum number (m sub l - position of orbital in an x-y-z plot), and the spin quantum number (m sub s - orientation of the spin of the electron)

118
Q

principal quantum number, n, the energy level - values

A

n ≥ 1

119
Q

angular momentum quantum number, l, orbital type - values

A

0 to n-1

120
Q

magnetic quantum number, m sub l, position - values

A

-l to +l, including zero

121
Q

Energy of n =

A

-2.18x10^-18 J (1 / n^2)

122
Q

spin quantum number, m sub s - values

A

-1/2 for spin down or +1/2 for spin up

123
Q

the number of sublevels within a level

A

n

124
Q

the number of orbitals within a sublevel

A

2l+1

125
Q

the number of orbitals in a level

A

n^2

126
Q

ΔEelectron

A

Efinal state = Einitial state

ΔE = -2.18x10^-18 J [(1 / (nf)^2) - (1 / (ni)^2)]

127
Q

ψ^2 the probability density

A

the probability of finding an electron at a particular point in space - decreases as you move away from the nucleus

128
Q

probability distribution function

A

represents the total probability at a certain distance from the nucleus

129
Q

the maximum value of the probability distribution function

A

is the most probable radius

130
Q

nodes in the probability distribution function

A

are where the probability drops to zero

131
Q

l=0

A

s orbital; each principle energy level has one s orbital; spherical shaped; number of nodes = (n-1)

132
Q

l=1

A

p orbitals; each principle energy state above n=1 has 3 p orbitals; two-lobed; one node at the nucleus - total of n nodes

133
Q

l=2

A

d orbitals; each principle energy state above n=2 has 5 d orbitals; mainly four-lobed “shaped” orbitals; planar nodes - higher principle levels also have spherical nodes

134
Q

l=3

A

f orbitals; each principle state above n=3 has 7 f orbitals; mainly 8-lobed; planar nodes - higher principle levels also have spherical nodes

135
Q

the phase of an orbital

A

orbitals are determined from mathematical wave functions, which can have positive or negative values as wells as nodes where the wave function = 0; the sign of the wave function is called its phase

Fall 2017 (24 decks)

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