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WorksheetsChemisty OR Unit 1
Total questions: 79
Worksheet time: 55mins
Which of the following has the longest wavelength
Gamma Rays
Radio Waves
Mircowaves
UV rays
What do you turn wavelengths into?
kg
cm
meters
picometers
If a photon’s wavelength is 663 nm, what is its energy?
1. 4.40 x 10-37 J
2. 3.00 x 10-22 J
3. 4.40 x 10-40 J
4. 3.00 x 10-19 J
What is the correct order of increasing energy?
1. Microwaves, visible light, UV light, x-rays, gamma rays
2. Microwaves, x-rays, gamma rays, visible light, UV light
3. Microwaves, UV light, visible light, x-rays, gamma rays
4. X-rays, gamma rays, microwaves, visible light, UV light
5. UV light, visible light microwaves, x-rays, gamma rays
= 300 to 800 nm
(a)
300 to 10 nm
(a)
800 nm to 1 μm
(a)
.01 to 10 nm
(a)
Spin nucleus
UV
radio
IF
Gamma
Excited spin of
electrons.
Microwave
visible
UV
gamma
Causes vibrations
in molecules.
microwave
radio
IF
UV
Causes excited
value of e-’s to
higher energy
level.
Radio
Visible
UV
Gamma
Excites
valence
electron.
UV
visible
radio
IF
Excites core e-
’s in atoms.
UV
gamma
x-ray
IF
Associated with
decay of atom
nucleus.
x-ray
Gamma
visible
microwaves
When a given molecule absorbs a photon of infrared (IR) radiation
1. It begins to vibrate.
2. It promotes electrons into delocalized bonding orbitals.
3. It bring to rotate
4. Its electrons are excited to higher energy levels.
5. It leads to hemolytic cleavage.
Radiofrency radiation has what kind of impact on matter?
1. It makes electrons spin.
2. It makes the molecule rotate.
3. It makes the nucleus split.
4. It makes the nuclei spin.
Metals with low ionization energy
(a)
Electrically charged particles are released from or within a material when it absorbs electromagnetic radiation. The effect is often defined as the ejection of electrons from a metal plate when light falls on it.
(a)
Which of the following statement(s) is/are true about the photoelectric effect?
I) The sum of the work function and kinetic energy of an ejected electron is proportional to the frequency of incident light.
II) Given light of high enough intensity, electrons can be ejected from any surface.
III) Einstein employed the concept that photons have quantized amounts of energy to explain the effect.
1. I, II
2. I, II, III
3. I only
4. II, III
5. I, III
Photons above threshold cause electrons
to be ejected with...
(a)
Lights is a ______ and _________
(a)
Wave phenomena includes:
diffraction
reflection
polarization
interference
transfusion
Downfall of classical mechanics:
Blackbody radiators
H emission spectra
photoelectric effect can’t be explained by classical mechanics
electron magnification effect
Diffraction of light
Light as a particle E= hv =
(a)
The famous electron diffraction pattern is proof of what concept?
1. Particles can exhibit wave-like properties
2. The location and trajectory of electrons can be found.
3. Electromagnetic radiation can exhibit wave-like properties.
4. Electrons can spin when hit by microwave radiation.
True or False
Matter is a wave and a particle
True
False
Matter behaves according to...
(a)
But as matter gets smaller
it does not behave like particle
Can’t assign trajectories to electrons
loses energy
no longer acts like a wave
postulated that matter also acts as a wave
Hudi
Einstein
deBroglie
Audolfo
The larger the ____________, the smaller the ______________ (de Broglie)
(a)
True or False
large particles that you can see have undetectably small wavelengths
True
False
According to de Broglie, which of the following objects has the smallest wavelength?
1. electrons
2. neutrons
3. protons
4. molecules
ties experiment and theory to explain the behavior of
electrons in an H atom
Bohrs Theory
Audolfs Theory
de Broglie equation
Rydberg equation
Fall to UV n = 1
(Paschen series)
(Lyman series)
(Balmer series)
Fall to visible n = 2
(Paschen series)
(Lyman series)
(Balmer series)
Fall to IR n = 3
(Paschen series)
(Lyman series)
(Balmer series)
For a Bohr atom, which of the following transitions
emits the highest energy photon?
1. From n = 10 n = 8
2. From n = 4 to n = 3.
3. From n = 6 to n = 5
4. From n = 2 to n = 1
The change in energy decreases between
energy levels as they get closer together and move
away from the nucleus, so the two energy levels with
the largest difference in energy will be the two (a)
energy levels in the list.
Which of the following emission lines corresponds to part of the
Balmer series of lines in the spectrum of a hydrogen atom?
I) n = 2 -> n = 1
II) n = 4 -> n = 2
III) n = 4 -> n = 1
IV) n = 3 -> n = 2
V) n = 4 -> n = 3
1. II and III only
2. II and IV only
3. V only
4. I and III only
5. II, III, and IV only
The Balmer series is produced by electronic transitions
which either begin (_______ spectra) or end (________ spectra) at the energy level n = 2. These correspond mostly to the visible region.
(a)
Schrodinger developed quantum mechanics:
Wave behavior of electrons
Cannot know exact location but can know most probable location
Not all locations are possible
There are rules for where electrons are found
There are quantum rules
n = energy level, distance from nucleus,
n = 1, 2, 3
n = 0, 1, 2
n = 1, 2, 3 ,4
n = 0, 1, 2, 3, 4
l =
shape of energy level
energy level
distance from nucleus
shell
ml=
orientation of shape
shape of energy level
distance from nucleus
energy level
has 1 orientation: 0
(a)
has 3 orientations:
(a)
has five orientations:
(a)
ms=
orientation of shape
electron spin
energy level
distance from nucleus
The size of an atomic orbital is determined by which quantum number?
1. m1
2. l
3. ms
4. n
Whos equation is this?
(a)
What shape is this?
(a)
What shape is this?
S
P
D
F
What shape is this?
(a)
What shape is this?
(a)
How many electrons in n = 1 shell?
1
2
3
4
How many electrons in n = 1 though 3 are p?
10
24
12
2
In an atom, what would be the maximum number of
electrons having the quantum numbers n = 6 and l = 2?
1. 72
2. 6
3. 5
4. 10
5. 8
True or False
if n=1 then l must =1
True
False
Which set of quantum numbers does NOT provide a
satisfactory solution to the wave equation?
1. n = 2, l = 0, ml = -1
2. n = 1, l = 0, ml = 0
3. n = 4, l = 2, ml = +2
4. n = 5, l = 3, ml = -3
5. n = 3, l = 2, ml = -1
Electrons fill from the lowest to
the highest.
Aufbau
Hund
Pauli
Spread out electrons when
they have the same energy
levels in p and d orbitals
Aufbau
Hund
Pauli
No 2 electrons have the same
set of quantum numbers.
This translates as ”no more
than 2 e- per orbital”
Aufbau
Hund
Pauli
Conversion of nm to m
10-9
10-8
10-12
10-36
100 ym 100 cm
(a)
< 0.01 nm
(a)
1 mm to 100s m
(a)
Is used for MRI's
Radio waves
Microwaves
IF
x-rays
y= 1/x^2
Inverse square
linear
squared
proportional
y= 1/x
linear
inverse squared
inverse
proportional
y=2^x
exponential
linear
inverse
proportional
y= x^2 or y= kx^x
squared
parabolic (quadratic)
linear
proportional
E = hv
(a)
v =c/wavelength
(a)
E = hc/wavelength
(a)
(a) is slightly longer than wavelength
Night Vision
IF
Micro
Gamma
UV
Inner electrons
X-rays
Radio
Gamma
UV
What was the wavelength of Dr. Laude when he weighed 100 kg and being quite the athlete could run 10 m/s effortlessly (okay, so I'm rounding up)? What is the wavelength of an electron that weighs 1x10-30 kg with a velocity of 6 x 106 m/s?
The e Broglie equation is below with Planck's constant of 6 x 10-34 Js.
6 x 10^-37 & 0.1nm
7 x 10^-37 & 0.1nm
6 x 10^-36 & 0.1nm
5 x 10^-30 & 0.1nm
