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Introduction to Chemistry > Chapter 2 review > Flashcards

Chapter 2 review Flashcards

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1
Q

what is the quantum mechanical model?

A

explains how electrons exist and behave in atoms

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2
Q

what is electromagnetic radiation?

A

light that travels by waves

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3
Q

what is wavelength

A

measure of the distance covered by a wave

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4
Q

what is amplitude?

A

the height of the wave

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5
Q

what is the symbol for wavelength

A

lambda

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6
Q

what is color?

A

when all the wavelengths of light are not absorbed

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7
Q

what is frequency?

A

number of waves passing a given point per unit of time is the frequency

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8
Q

what relationship does frequency and wavelength have?

A

frequency and wavelength have an inverse relationship

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9
Q

what is total energy proportional to?

A

the amplitude and frequency of the waves

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10
Q

if there is a large amplitude what happens to the force?

A

the force increases

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11
Q

what is the speed of light(c)

A

constant speed that all electromagnetic waves move through

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12
Q

what is the equation for c=

A

c = (wavelength)(frequency)

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13
Q

what does c equal

A

3.00 x10^8

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14
Q

what is the electromagnetic spectrum?

A

all wavelengths of electromagnetic radiation

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15
Q

what are the colors of the spectrum

A

ROYGBV and it is in increasing order of frequency / decreasing length of wave

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16
Q

who was max planck?

A

discovered that energy of matter was not continuous

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17
Q

what is quanta?

A

discrete packets of light

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18
Q

what is quantized energy?

A

energy that can be lost or gained

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19
Q

what is the equation for quantized energy?

A

E = nhv

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20
Q

what does h equal (planck’s constant)

A

6.626x10-34

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21
Q

what did albert einstein do?

A

proposed that radiation was quantized by particles called photons

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22
Q

what are the 2 equations for photons?

A

Ephoton = Hv

E photon = Hc/ wavelength

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23
Q

what does a short wavelength mean?

A

high frequency and high energy

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24
Q

what is threshold frequency?

A

the minimum frequency required before electrons would emit intensity

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25
Q

what is the KEelectron equation

A

1/2mv^2=hv-hV0

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26
Q

what did louis de brogile theorized

A

if light can have material properties matter should exhibit wave properties
-predicted that the wavelength of inversely proportional to its momentum

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27
Q

what does wavelength =

A

lambda = h/mv

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28
Q

what is interference

A

the interacton between waves

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29
Q

what is constructive interference

A

when waves interact so that they add to make a larger wave

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30
Q

what is destructive interference?

A

when waves interact so they cancel each other it is

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31
Q

what is diffraction?

A

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

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32
Q

what are complimentary properties?

A

only one aspect of wave or particle can be obserbed

both can never be observed at the same time

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33
Q

what is a spectrum?

A

common radiation source that contains many different wavelength components

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34
Q

what is a continuous spectrum?

A

when light is produced through a prism

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35
Q

what is a line spectrum

A

discrete wavelengths is observed

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36
Q

what is atomic emission?

A

different gases emit light of different characterisitc colors upon excitation by electrical discharge

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37
Q

what is a flame test?

A

used to identify the presence of certain elements, primarily group 1 metal ions

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38
Q

who created the bohr model

A

niels bohr

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39
Q

what does the bohr model explain

A

where the electrons are and how the atom changes when it undergoes energy transitions

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40
Q

what are stationary states?

A

electrons travel in orbits that are fixed distance from the nucleus

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41
Q

what happens when attraction goes up?

A

the energies are more negative

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42
Q

what happens when n goes up

A

attraction goes down

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43
Q

how do we calculate the energy level of n

A

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

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44
Q

what is the formula to find the change in electron?

A

change in energy level = -2.18x10^-18J(1/nf)^2-(1/(ni)^2

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45
Q

what is the uncertainty principle?

A

heisenburg stated that the product of the uncertainties in both the position and speed was inversely proportional to its mass

46
Q

what is the change in mass and velocity

A

uncertainty in momentum

47
Q

what is the change in x

A

uncertainty in position

48
Q

what is classical physics?

A

a particles velocity , positon, and forces acting on it are known

49
Q

what is quantum mechanics?

A

a particles position or its velocity can be known but not both

50
Q

is classical physics determinacy or interminacy?

A

determinacy

51
Q

what is determinacy?

A

definite or a predictable future

52
Q

indeterminacy?

A

indefinite future

53
Q

who was erwin schrodinger and what did he do?

A

Australian physicist proposed an equation that incorporated both the wave-like and particle-like behavior of electrons

54
Q

what does the square of wave function do?

A

gives a probability density map

55
Q

what are orbitals?

A

wave functions

56
Q

what does n stand for?

A

principal quantum number

57
Q

what does l stand form?

A

angular momentum

58
Q

what does ml stand for?

A

magnetic quantum number

59
Q

what does ms stand for?

A

spin quantum number

60
Q

what is the principal quantum number

A

describes the energy level on which the orbital resides

61
Q

what are the values of n?

A

they are less than 1

62
Q

what is the angular momentum quantum number

A

defines the shape of the orbital

63
Q

what are the allowed values of l

A 
0 to n-1
l = 0
l=1(p)
l=2(d)
l=3(f)
64
Q

what is the magnetic quantum number?

A

describes the 2 d orientation of the orbital

65
Q

what are the allowed values of the magnetic quantum number

A

-1 to 1 or +- l(everything in between)

66
Q

what are the numbers on the given orbital?

A

1s, 3p, 5d, 7f

67
Q

what is the value of l for s orbitals

A

0

68
Q

what is the shape of an s orbital

A

speherical

69
Q

what happens to the radius when n increases (s orbital)

A

the radius of the sphere increases because it’s more distance away from the nucleus

70
Q

what node does the s orbital possess?

A

n-1 nodes

71
Q

what is the value of l for the p orbital?

A

1

72
Q

what is the shape of a p orbital

A

have two lobes with ai node between them. they look like a dumbell

73
Q

what is the value of l for the d orbital?

A

2

74
Q

how many lobes does d have

A

4 lobes

75
Q

what is the shape of the d orbital

A

the other resembles a p orbital with a doughnut

76
Q

what is the l value for an f orbital?

A

3

77
Q

what is a spin quantum number?

A

describes its magnetic field, which affects its energy

78
Q

what is the same thing electrons have regarding spin?

A

they all have the same spin

79
Q

what was discoverd in the 1920s about spin

A

two electrons in the same orbital do not have the same energy

80
Q

what orientation can the spin be in?

A

only in one direction or it’s opposite

spin can be up or down

81
Q

what is the fourth quantum number?

A

spin quantum or ms

82
Q

what are the two quantum numbers spin has

A

+1/2 and -1/2

83
Q

who developed the periodic table?

A

dmitiri mendeleev and lothar meyer came to the conclusion that elements needed to be organized by increasing atomic weight

84
Q

what is periodicity?

A

repeating chemical and physical properties

85
Q

what was meyers approach to the table?

A

he believed that the trends were reflective of the internal structure of the elements

86
Q

what was mendeleev’s approach to the table

A

belived in the trend of the table ( perodicity

87
Q

what did mendeleev discover?

A

germanium, gallium, scandium and he belived that elements were primordial matter

88
Q

what was mendeleev’s prediction?

A

discoveries of gallium and germanium

89
Q

who was henry moseley and what did he do?

A

developed the concept of atomic numbers

90
Q

how did mosely arrange the elements?

A

in order of increasing frequencies

91
Q

what are the main group elements

A

tend to be predictable based on their position in the PT (s and p blocks)

92
Q

are transition element properties more or less predictable

A

less predictable

93
Q

what is the f block called?

A

inner transition metals

94
Q

what is the top row of the f block called?

A

lanthanides

95
Q

what is the bottom of the f block called

A

actinides

96
Q

why is the f blck similar to the d block

A

they are both unpredictable

97
Q

what are some characteristics of metals?

A

shiny luster, solids are malleable and ductile,, good conductors of heat and electricity, most metal oxides are ionic solids that are basic

98
Q

do metals form cations or anions?

A

cations

99
Q

what is a cation?

A

ion that will lose an electron (1st group )

100
Q

what is an anion

A

ion that will gain an electron (7th group)+

101
Q

what are characteristics of nonmetals

A

do not have shiny luster, , solids are usually brittle, poor conductors of heat, tend to form anios

102
Q

what are metalloids

A

have characteristics of meals and nonmetals

103
Q

what are some characteristics of metalloids

A
  • semiconductors

- used in electrical chip

104
Q

what are some metalloids

A

boron, silicon, germanium, arsenic, antimony, tellurium, astatine

105
Q

what are the components of electron configurations?

A

number, (n) letter, (l) superscript

106
Q

what is an orbital diagram

A

another way to represent electron configuration

107
Q

what do the half arrows represent in an orbital diagram

A

electrons

108
Q

what does the direction of the arrow represent

A

the relative spin of the electron

109
Q

what does the pauli exclusion principle state?

A

no two electrons in the same atom have the same energy

  • no orbital may have more than 2 electrons and they must have opposite spins
110
Q

what do they say about one electron hydrogen ataom

A

orbitals on the same principle energy level have the same energy and they degenerate

Introduction to Chemistry (12 decks)

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