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Chem 205 > ch 6 > Flashcards

ch 6 Flashcards

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1
Q

electromagnetic radiation

A

is characterized by wavelenght and frequency

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2
Q

highest energy rays

A

gamma rays

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3
Q

lowest energy rays

A

radiowaves

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4
Q

light acts as

A

waves

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5
Q

c stands for

A

speed of light

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6
Q

h stands for

A

planks constant

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7
Q

what is the value of c

A

2.998x10^8 m/s

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8
Q

what does R stand for

A

Rydberg constant

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9
Q

Broglies equation

A

λ = h/mv, where λ is wavelength, h is Planck’s constant, m is the mass of a particle, moving at a velocity

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10
Q

What is a wavelenght and how is it measured?

A

is defined as the distance between a given point on a wave and the corresponding point in the next cycle of the wave; it is often measured as the distance between successive crests or high points of a wave

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11
Q

Frequency symbol and what is it

A

Frequency, symbolized by the Greek letter (ν), refers to the number of waves that pass a given point in some unit of time, usually per second.

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12
Q

What is the unit for frequency

A

The unit for frequency, written either as s−1 or 1/s and standing for 1 oscillation per second, is called a hertz

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13
Q

equation to relate c (speed of light) to wavelenght to v (frequency)

A

c(m/s)= λ(m) x v(1/s)

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14
Q

what is the speed of light in km/h?

A

(1.079×109 km/h)

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15
Q

Order of electromagnetic rays from highest to lowest

A

Electromagnetic radiation has a wide spectrum, including gamma y-rays, X-rays, UV rays, visible light, IR radiation, microwaves, and radio waves (FM and AM) and long radio waves.

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16
Q

Energy increases from

A

microwaves (lowest energy) to y rays. With y rays having the highest energy.

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17
Q

formula for energy

A

E=hc/λ=hv

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18
Q

Formula for wavelenght (debroglies)

A

λ=h/mv
m is mass in kg
v is velocity in m/s
h is plancks constant
wavelenght is in meters

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19
Q

When theres a large wavelenght what happens to energy and speed

A

As wavelenght increases, velocity decreases and energy is low

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20
Q

What happens to energy and velocity when wavelength becomes smaller and smaller

A

Energy increases and speed increases

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21
Q

What is the wavelength of visible light

A

From 380 nm for violet end to 750 nm to red end

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22
Q

What is the acronym for visible light

A

ROYGBIV
RED HIGHEST WAVELENGTH
ORANGE
YELLOW
GREEN
BLUE
INDIGO
VIOLET LOWEST WAVELENGTH

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23
Q

How is a photon of light created?

A

When an electron changes from one atomic orbital to another, the electron’s energy changes. When the electron changes from an orbital with high energy to a lower energy state, a ​photon of light is created.

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24
Q

Rydberg equation to find spectral lines of h

A

Change in E (nm)= -Rhc (1/nf^2 - 1/ni^2)
λ is the wavelength of the photon
R = Rydberg’s constant
c=speed of light
h=plancks constant
ni and nf are integers where nf > ni

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25
Q

What is diffraction

A

Scattering of waves by regular array of objects

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26
Q

Describe absorption for an atom

A

An atom changes from a ground state to an excited state by taking on energy from its surroundings in a process called absorption (RELAX). The electron absorbs the energy and jumps to a higher energy level.

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27
Q

Describe emission for atoms

A

Emission (EXCITE): the electron returns to the ground state by releasing the extra energy it absorbed. (from high to low)

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28
Q

what is descalation

A

Excited to ground level

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29
Q

When is electromagnetic radiation emitted

A

If a piece of metal is heated to a high temperature, electromagnetic radiation is emitted with wavelengths that depend on temperature

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30
Q

Color at different temperatures

A

At lower temperatures, the color is a dull red. As the temperature increases, the red color brightens, and at even higher temperatures a brilliant white light is emitted.

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31
Q

Describe the ultraviolet catastrophe

A

Theories available at the time predicted that, as a solid is heated, the intensity should increase continuously with decreasing wavelength, instead of reaching a maximum and then declining as is actually observed. This perplexing situation became known as the ultraviolet catastrophe because predictions failed in the ultraviolet region.

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32
Q

What is the explanation for the ultraviolet catastrophe

A

The emitted electromagnetic radiation originated in vibrating atoms (called oscillators) in the heated object. Max proposed that each oscillator had a fundamental frequency (ν) of oscillation and that these oscillators could only oscillate at either this frequency or whole-number multiples of it (nν). Because of this, the emitted radiation could have only certain energies, given by the equationE=nhν

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33
Q

Who offered an explanation for the ultraviolet catastrophe

A

Max Planck (1858–1947), offered an explanation for the ultraviolet catastrophe:

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34
Q

What did planck propose?

A

He proposed that energy is quantized

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35
Q

What is quantization

A

That only certain energies are allowed

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36
Q

Examples of electromagnetic radiation

A

Visible light, microwaves, television and radio signals, x-rays, and other forms of radiation are now called electromagnetic radiation

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37
Q

Frequency

A

Frequency, symbolized by the Greek letter (ν), refers to the number of waves that pass a given point in some unit of time, usually per second. The unit for frequency, written either as s−1 or 1/s and standing for 1 oscillation per second, is called a hertz

38
Q

speed of light formula

A

c (m/s)= wavelegth(m) x frequency (1/s)

39
Q

speed of light value

A

2.998x10^8 m/s

40
Q

when is electromagnetic radiation emmitted

A

If a piece of metal is heated to a high temperature, electromagnetic radiation is emit-ted with wavelengths that depend on temperature

41
Q

colors at different temperatures

A

At lower temperatures, the color is a dull red. As the temperature increases, the red color brightens, and at even higher temperatures a brilliant white light is emitted.

42
Q

How is wavelength related to temperature

A

The wavelength of the most intense radiation is related to temperature: As the temperature of the metal is raised, the maximum intensity shifts toward shorter wavelengths, that is, toward the ultraviolet

43
Q

what is the ultraviolet catastrophe

A

Theories available at the time predicted that, as a solid is heated, the intensity should increase continuously with decreasing wavelength, instead of reaching a maximum and then declining as is actually ob-served. This perplexing situation became known as the ultraviolet ca-tastrophe because predictions failed in the ultraviolet region.

44
Q

what did max planck offer?

A

Max Planck (1858–1947), offered an explanation for the ultraviolet catastrophe: The emitted electro-magnetic radiation originated in vibrating atoms (called oscillators) in the heated object. He proposed that each oscillator had a fundamen-tal frequency (ν) of oscillation and that these oscillators could only oscillate at either this frequency or whole-number multiples of it (nν).

45
Q

Equation max planck proposed

A

Because of this, the emitted radiation could have only certain energies, given by the equation E=nhν

46
Q

what is quantization

A

Quantization means that only certain energies are allowed

47
Q

What is h

A

h in the equation is now called Planck’s constant

48
Q

If an oscillator changes from a higher energy to a lower one, energy is emitted as electromagnetic radiation, where the difference in energy between the higher and lower energy states is

A

∆E=Ehigher n−Elower n=∆nhν

49
Q

What did albert einstein incorporate into what explanation

A

A few years after Planck’s work, Albert Einstein (1879–1955) incorporated Planck’s ideas into an explanation of the photoelectric effect and in doing so changed the description of electromagnetic radiation.

50
Q

What is ejected in the photoelectric effect

A

In the photoelectric effect, electrons are ejected when light strikes the surface of a metal (Figure6.4), but only if the frequency of the light is high enough.

51
Q

How does light affect the electrons ejected?

A

If light with a lower frequency is used, no electrons are ejected, regardless of the light’s intensity (its brightness). If the frequency is at or above a minimum, critical frequency, increasing the light intensity causes more electrons to be ejected.

52
Q

What are photons

A

That light has particle like properties. Einstein characterized these massless particles, now called photons, as packets of energy, and stated that the energy of each photon is proportional to the frequency of the radiation as defined by Planck’s equation.

53
Q

wave like particle duality

A

wave–particle duality—that is, the idea that electromag-netic radiation has the properties of both a wave and a particle

54
Q

What is line emission spectrum

A

The spectrum obtained in this manner is A line emission spectrum is caused when energy is added to an atom. This added energy causes the electrons in the atom to jump up energy levels. When this happens, the atom is in an excited state.

55
Q

what does the balmer eq calculate

A

the Balmer equation was found that could be used to calculate the wavelength of the red, green, and blue lines in the visible emission spectrum of hydrogen

56
Q

n stands for

A

energy level

57
Q

l stands for

A

angular momentum

58
Q

ml stands for

A

specific orbital

59
Q

what must n be

A

always a positive interger

60
Q

how to find l

A

n-1
l is equal to for the following orbitals:
s=0
p=1
d=2
f=3

61
Q

how to find ml

A

-l…l

62
Q

what is s shape

A

spherical

63
Q

what is p shape

A

dumbbell. There are 3 p orbitals (x,y,z)

64
Q

what is d shape

A

clover leaf shape. There are 5 d orbitals

65
Q

what is ms

A

either +1/2 or -1/2
it indicates the spin

66
Q

as energy size increases

A

the size of the orbital increases and the number of orbitals

67
Q

As the number of orbitals increases

A

so does their complexity

68
Q

number of energy level equals

A

number of sublevel

69
Q

n=1
what sublevels

A

1s

70
Q

n=2
what sublevels

A

2s 2p

71
Q

n=3
what sublevels

A

3s 3p 3d

72
Q

n=4
what sublevels

A

4s 4p 4d 4f

73
Q

how many electrons can s hold

A

2

74
Q

how many electrons can p hold

A

6

75
Q

number of e that d can hold

A

10

76
Q

number of e that f can hold

A

14

77
Q

gray colored lobe is the

A

positive lobe

78
Q

white colored lobe is

A

negative lobe

79
Q

what info does l the angular momentum give us

A

the shape of the orbital
l= 0,1,2,3
s,p,d,f

80
Q

energy increases in orbital order

A

s p d f
energy increases from left to right

81
Q

He is part of

A

1s

82
Q

where do transition metals have their valence electrons

A

in the d subshell, that means the d subshell is either half full or totally full

83
Q

what are degenerate orbitals

A

energy is equal and the orbitals are at the same height

84
Q

how to you do an orbital diagram

A

1 electron configuration
2 arrows in

the arrows are filled from lowest to highest aufbau

fill out degenerate orbitals one at a time hunds rule

85
Q

number of transitions formula

A

n(n-1)/2

86
Q

absorption

A

lower to higher

87
Q

emission

A

higher to lower

88
Q

of subshells =

A

n number

89
Q

nodal surfaces =

A

type of orbital
spdf
0123

90
Q
A

Chem 205 (14 decks)

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