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Quantum/Mechanical Model
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Gravity
Terms in this set (96)
The vertical height of a wave is called
amplitude
The number of cycles that pass through a stationary point is called
frequency
Place the following types of electromagnetic radiation in order of increasing wavelength.
ultraviolet light gamma rays radio wave
gamma rays < ultraviolet light < radio waves
) Place the following types of electromagnetic radiation in order of decreasing energy.
ultraviolet light radio waves microwaves
ultraviolet light > microwaves > radio waves
On the electromagnetic spectrum, visible light is immediately between two other wavelengths. Name them.
infrared and ultraviolet
Identify the color that has a wavelength of 700 nm.
red
Identify the color that has a wavelength of 460 nm.
blue
9) Which of the following visible colors of light has the highest frequency?
red
Which of the following colors of electromagnetic radiation has the shortest wavelength?
violet
Which of the following types of electromagnetic radiation has the lowest frequency?
orange
Calculate the wavelength (in nm) of a the red light emitted by a neon sign with a frequency of 4.74 × 1014 Hz.
633 nm
A sunburn is caused by overexposure to __________ radiation.
ultraviolet
Food can be cooked by __________ radiation.
microwave
When waves of equal amplitude from two sources are out of phase when they interact, it is called __________.
destructive interference
Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.
436 nm
Which of the following occur as the energy of a photon increases?
the wavelength gets shorter.
Which of the following occur as the wavelength of a photon increases?
the frequency decreases
Calculate the frequency of the red light emitted by a neon sign with a wavelength of 659.9 nm.
4.55 × 1014 s-1
Calculate the energy of the green light emitted, per photon, by a mercury lamp with a frequency of 5.49 × 1014 Hz.
3.64 × 10-19 J
Calculate the energy of the orange light emitted, per photon, by a neon sign with a frequency of 4.89 × 1014 Hz.
3.24 × 10-19 J
Calculate the frequency of the green light emitted by a hydrogen atom with a wavelength of 486.1 nm.
6.17 × 1014 s-1
Calculate the energy of the red light emitted by a neon atom with a wavelength of 703.2 nm.
2.83 × 10-19 J
Calculate the energy of the violet light emitted by a hydrogen atom with a wavelength of 410.1 nm.
4.85 × 10-19 J
How many photons are contained in a burst of yellow light (589 nm) from a sodium lamp that contains 609 kJ of energy
1.80 × 1024 photons
How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy?
4.99 × 1023 photons
How much energy (in kJ) do 3.0 moles of photons, all with a wavelength of 655 nm, contain?
548 kJ
Determine the shortest frequency of light required to remove an electron from a sample of Ti metal, if the binding energy of titanium is 3.14 × 103 kJ/mol.
7.87 x 1015 Hz
What total energy (in kJ) is contained in 1.0 mol of photons, all with a frequency of 2.75 × 1014 Hz?
10 kJ
Determine the longest wavelength of light required to remove an electron from a sample of potassium metal, if the binding energy for an electron in K is 1.76 × 103 kJ/mol.
68.0 nm
Identify the color of a flame test for potassium.
violet
Identify the color of a flame test for sodium.
yellow
Which of the following statements is TRUE?
All of the above are true.
Calculate the wavelength of an electron (m = 9.11 × 10-28 g) moving at 3.66 × 106 m/s.
1.99 × 10-10 m
Calculate the wavelength of a baseball (m = 155 g) moving at 32.5 m/s.
1.32 × 10-34 m
Determine the velocity of a marble (m = 8.66 g) with a wavelength of 3.46 × 10-33 m.
22.1 m/s
Determine the velocity of a medicine ball (m = 10.0 kg) with a wavelength of 1.33 × 10-35 m.
4.98 m/s
Determine the mass of a ball with a wavelength of 3.45 x 10-34 m and a velocity of 6.55 m/s.
293 g
Determine the mass of a ball with a velocity of 35.1 m/s and a wavelength of 8.92 x 10-34 m.
21.2 g
It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy for an atom of hydrogen, making the assumption that ionization is the transition from n=1 to n=∞.
+2 .18 × 10-18 J
Which of the following transitions (in a hydrogen atom) represent emission of the longest wavelength photon?
n = 5 to n = 4
Which of the following transitions (in a hydrogen atom) represent absorption of the smallest frequency photon?
n = 5 to n = 6
Choose the transition (in a hydrogen atom) below that represents the absorption of the shortest wavelength photon.
n = 1 to n = 2
Which of the following transitions represent the emission of a photon with the largest energy?
n = 3 to n = 1
For n = 3, what are the possible sublevels?
0, 1, 2
What are the possible orbitals for n = 3?
s, p, d
What value of l is represented by a d orbital?
2
Each of the following sets of quantum numbers is supposed to specify an orbital. Which of the following sets of quantum numbers contains an error?
n = 3, l =3 , ml = -2
Each of the following sets of quantum numbers is supposed to specify an orbital. Choose the one set of quantum numbers that does not contain an error.
n = 4, l = 3, ml =-2
How many orbitals are contained in the third principal level (n=3) of a given atom?
9
How many sublevels are contained in the second shell (n=2) of a given atom?
2
Which of the following statements is TRUE?
Atoms are roughly spherical because when all of the different shaped orbitals are overlapped, they take on a spherical shape
Which of the following quantum numbers describes the shape of an orbital?
angular momentum quantum number
Which of the following quantum numbers describes the orientation of an orbital?
magnetic quantum number
Which of the following quantum numbers describes the size and energy of an orbital?
principal quantum number
How many different values of ml are possible in the 4f sublevel?
7
How many different values of l are possible in the third principal level?
3
How many different values of ml are possible in the 3d sublevel?
5
How many different values of ml are possible in the 2p sublevel?
3
Give all possible values of l for a 3 sublevel.
0, 1, 2
Give the value of l for a 3p sublevel.
1
Identify the correct values for a 1s sublevel.
n = 1, l = 0, ml = 0
Identify the correct values for a 2p sublevel.
n = 2, l = 1, ml = 0
Identify the correct values for a 3p sublevel.
n = 3, l = 1, ml = 0
Identify the correct values for a 4f sublevel.
n = 4, l = 3, ml = -2
If two electrons in the same atom have the same value of "l", they are
in the same sublevel, but not necessarily in the same level.
In which orbital below would an electron (on average) be farthest from the nucleus?
4f
In which orbital below would an electron (on average) be closest to the nucleus?
2s
Determine the energy change associated with the transition from n=2 to n=5 in the hydrogen atom.
+4.58 × 10-19 J
Determine the energy change associated with the transition from n=3 to n=2 in the hydrogen atom.
-3.03 × 10-19 J
Calculate the energy change associated with the transition from n=4 to n=1 in the hydrogen atom.
-2.04 × 10-18 J
Which of the following statements is TRUE?
The magnetic quantum number (ml) describes the orientation of the orbital.
It is possible to determine the ionization energy for hydrogen using the Bohr equation. Calculate the ionization energy (in kJ) for a mole of hydrogen atoms, making the assumption that ionization is the transition from n=1 to n=∞.
1.31 × 103 kJ
Calculate the wavelength of light associated with the transition from n=1 to n=3 in the hydrogen atom
103 nm
Calculate the frequency of light associated with the transition from n = 2 to n = 3 in the hydrogen atom.
4.57 × 1014 s-1
How much energy (in kJ) is required to ionize 2.78 moles of hydrogen atoms?
3.65 × 103 kJ
Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n = 4 and the atom emits a photon of light with a wavelength of 486 nm.
2
Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n = 2 and the atom absorbs a photon of light with a frequency of 4.57 × 1014 Hz.
3
Determine the end (final) value of n in a hydrogen atom transition, if the electron starts in n = 1 and the atom absorbs a photon of light with an energy of 2.044 × 10-18 J.
4
Describe the shape of a p orbital.
two balls
Describe the shape of a s orbital.
a ball
Give the numbers for ml for a d orbital.
-2, -1, 0, 1, 2
What is the maximum number of s orbitals that are possible?
1
What is the maximum number of p orbitals that are possible?
3
What is the maximum number of d orbitals that are possible?
5
What is the maximum number of f orbitals that are possible?
7
Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The frequency of this light is __________ s-1.
5.71 × 1014
An FM radio station broadcasts electromagnetic radiation at a frequency of 100.6 MHz. The wavelength of this radiation is __________ m.
2.982
Electromagnetic radiation with a wavelength of 525 nm appears as green light to the human eye. The energy of one photon of this light is __________ J.
3.79 × 10-19
Electromagnetic radiation with a wavelength of 531 nm appears as green light to the human eye. The energy of one photon of this light is 3.74 × 10-19 J. Thus, a laser that emits 1.3 × 10-2 J of energy in a pulse of light at this wavelength produces __________ photons in each pulse.
3.5 × 1016
The de Broglie wavelength of an electron with a velocity of 6.00 × 106 m/s is __________ m. The mass of the electron is 9.11 × 10-28 g.
1.21 × 10-10
What are the possible values of n and ml for an electron in a 4d orbital?
n = 5 and ml = -2, -1, 0, +1, +2
How many subshells are there in the shell with n = 4?
4
What are the possible values of l if n = 6?
0, 1, 2, 3, 4, or 5
9) How many orbitals are there in the fourth shell?
16
For a hydrogen atom, which electronic transition would result in the emission of a photon with the highest energy?
6p → 4s
For hydrogen, what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10-2 nm-1.
486.2 nm
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