Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chem 205 > ch 6 > Flashcards

ch 6 Flashcards

(90 cards)

Start Studying
1
Q

electromagnetic radiation

A

is characterized by wavelenght and frequency

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

highest energy rays

A

gamma rays

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

lowest energy rays

A

radiowaves

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

light acts as

A

waves

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

c stands for

A

speed of light

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

h stands for

A

planks constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what is the value of c

A

2.998x10^8 m/s

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

what does R stand for

A

Rydberg constant

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

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

A

c(m/s)= λ(m) x v(1/s)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

what is the speed of light in km/h?

A

(1.079×109 km/h)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Energy increases from

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

formula for energy

A

E=hc/λ=hv

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

When theres a large wavelenght what happens to energy and speed

A

As wavelenght increases, velocity decreases and energy is low

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

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

A

Energy increases and speed increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What is the wavelength of visible light

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

What is the acronym for visible light

A

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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
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

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
What is diffraction
Scattering of waves by regular array of objects
26
Describe absorption for an atom
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.
27
Describe emission for atoms
Emission (EXCITE): the electron returns to the ground state by releasing the extra energy it absorbed. (from high to low)
28
what is descalation
Excited to ground level
29
When is electromagnetic radiation emitted
If a piece of metal is heated to a high temperature, electromagnetic radiation is emitted with wavelengths that depend on temperature
30
Color at different temperatures
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.
31
Describe the ultraviolet catastrophe
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.
32
What is the explanation for the ultraviolet catastrophe
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
33
Who offered an explanation for the ultraviolet catastrophe
Max Planck (1858–1947), offered an explanation for the ultraviolet catastrophe:
34
What did planck propose?
He proposed that energy is quantized
35
What is quantization
That only certain energies are allowed
36
Examples of electromagnetic radiation
Visible light, microwaves, television and radio signals, x-rays, and other forms of radiation are now called electromagnetic radiation
37
Frequency
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
speed of light formula
c (m/s)= wavelegth(m) x frequency (1/s)
39
speed of light value
2.998x10^8 m/s
40
when is electromagnetic radiation emmitted
If a piece of metal is heated to a high temperature, electromagnetic radiation is emit-ted with wavelengths that depend on temperature
41
colors at different temperatures
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
How is wavelength related to temperature
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
what is the ultraviolet catastrophe
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
what did max planck offer?
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
Equation max planck proposed
Because of this, the emitted radiation could have only certain energies, given by the equation E=nhν
46
what is quantization
Quantization means that only certain energies are allowed
47
What is h
h in the equation is now called Planck’s constant
48
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
∆E=Ehigher n−Elower n=∆nhν
49
What did albert einstein incorporate into what explanation
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
What is ejected in the photoelectric effect
In the photoelectric effect, electrons are ejected when light strikes the surface of a metal (Figure 6.4), but only if the frequency of the light is high enough.
51
How does light affect the electrons ejected?
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
What are photons
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
wave like particle duality
wave–particle duality—that is, the idea that electromag-netic radiation has the properties of both a wave and a particle
54
What is line emission spectrum
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
what does the balmer eq calculate
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
n stands for
energy level
57
l stands for
angular momentum
58
ml stands for
specific orbital
59
what must n be
always a positive interger
60
how to find l
n-1 l is equal to for the following orbitals: s=0 p=1 d=2 f=3
61
how to find ml
-l...l
62
what is s shape
spherical
63
what is p shape
dumbbell. There are 3 p orbitals (x,y,z)
64
what is d shape
clover leaf shape. There are 5 d orbitals
65
what is ms
either +1/2 or -1/2 it indicates the spin
66
as energy size increases
the size of the orbital increases and the number of orbitals
67
As the number of orbitals increases
so does their complexity
68
number of energy level equals
number of sublevel
69
n=1 what sublevels
1s
70
n=2 what sublevels
2s 2p
71
n=3 what sublevels
3s 3p 3d
72
n=4 what sublevels
4s 4p 4d 4f
73
how many electrons can s hold
2
74
how many electrons can p hold
6
75
number of e that d can hold
10
76
number of e that f can hold
14
77
gray colored lobe is the
positive lobe
78
white colored lobe is
negative lobe
79
what info does l the angular momentum give us
the shape of the orbital l= 0,1,2,3 s,p,d,f
80
energy increases in orbital order
s p d f energy increases from left to right
81
He is part of
1s
82
where do transition metals have their valence electrons
in the d subshell, that means the d subshell is either half full or totally full
83
what are degenerate orbitals
energy is equal and the orbitals are at the same height
84
how to you do an orbital diagram
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
number of transitions formula
n(n-1)/2
86
absorption
lower to higher
87
emission
higher to lower
88
of subshells =
n number
89
nodal surfaces =
type of orbital spdf 0123
90

Chem 205 (14 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions