Question 1

If a hydrogen atom and a helium atom are traveling at the same speed,

Accepted Answer

A)  the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom. 
B)  the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium. 
C)  the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom. 
D)  the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom. 
E)  the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom. 
A)  the wavelength of the hydrogen atom will be about 4 times longer than the wavelength of the helium atom. 
B)  the wavelength of the hydrogen atom will be about 2 times longer than the wavelength of the helium. 
C)  the wavelength of the hydrogen atom will be roughly equal to the wavelength of the helium atom. 
D)  the wavelength of the helium atom will be about 2 times longer than the wavelength of the hydrogen atom. 
E)  the wavelength of the helium atom will be about 4 times longer than the wavelength of the hydrogen atom.

Question 2

Which of the following, if any, is the correct ground state electron configuration for Cr

Accepted Answer

A)  [Ar] 4s23d4 or 1s22s22p63s23p64s23d4 
B)  [Ar] 4s13d6 or 1s22s22p63s23p64s13d6 
C)  [Ar] 4s13d5 or 1s22s22p63s23p64s13d5 
D)  [Ne] 4s13d5 or 1s22s22p63s23p64s13d5 
E)  None of the above 
A)  [Ar] 4s23d4 or 1s22s22p63s23p64s23d4 
B)  [Ar] 4s13d6 or 1s22s22p63s23p64s13d6 
C)  [Ar] 4s13d5 or 1s22s22p63s23p64s13d5 
D)  [Ne] 4s13d5 or 1s22s22p63s23p64s13d5 
E)  None of the above

Question 3

A ground-state atom of iron has ___ unpaired electrons and is _____.

Accepted Answer

A)  0, diamagnetic 
B)  6, diamagnetic 
C)  3, paramagnetic 
D)  5, paramagnetic 
E)  4, paramagnetic 
A)  0, diamagnetic 
B)  6, diamagnetic 
C)  3, paramagnetic 
D)  5, paramagnetic 
E)  4, paramagnetic

Question 4

When photons with a wavelength of 310. nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 * 105 m/s. Calculate the binding energy of electrons to the magnesium surface.

Accepted Answer

A)  32.7 kJ/mol 
B)  321 kJ/mol 
C)  353 kJ/mol 
D)  386 kJ/mol 
E)  419 kJ/mol 
A)  32.7 kJ/mol 
B)  321 kJ/mol 
C)  353 kJ/mol 
D)  386 kJ/mol 
E)  419 kJ/mol

Question 5

The electron in a hydrogen atom falls from an excited energy level to the ground state in two steps, causing the emission of photons with wavelengths of 1870 nm and 102.5 nm, respectively. What is the principal quantum number or shell of the initial excited energy level from which the electron falls

Accepted Answer

A)  2 
B)  3 
C)  4 
D)  6 
E)  8 
A)  2 
B)  3 
C)  4 
D)  6 
E)  8

Question 6

Which of the following wavelengths of electromagnetic radiation has the highest energy

Accepted Answer

A)  450. nm 
B)  225 nm 
C)  3.50 x 10-9 m 
D)  8.40 x 10-7 m 
E)  2.50 x 10-5 m 
A)  450. nm 
B)  225 nm 
C)  3.50 x 10-9 m 
D)  8.40 x 10-7 m 
E)  2.50 x 10-5 m

Question 7

Which one of the following sets of quantum numbers is not possible $\begin{array}{lrrr}
~~~~~\text { n } & \text { l } & \mathrm{m}_{l} & \mathrm{~m}_{\mathrm{s}} \
\text { A. } 4 & 3 & -2 & +1 / 2 \
\text { B. } 3 & 0 & 1 & -1 / 2 \
\text { C. } 3 & 0 & 0 & +1 / 2 \
\text { D. } 2 & 1 & 1 & -1 / 2 \
\text { E. } 2 & 0 & 0 & +1 / 2
\end{array}$

Accepted Answer

The answer of Which one of the following sets of...

Question 8

Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = -2.18 * 10-18 J(1/n2).

Accepted Answer

A)  6.8 * 10-18 nm 
B)  0.612 nm 
C)  82.6 nm 
D)  97.2 nm 
E)  365 nm 
A)  6.8 * 10-18 nm 
B)  0.612 nm 
C)  82.6 nm 
D)  97.2 nm 
E)  365 nm

Question 9

Electrons in an orbital with l = 3 are in a/an

Accepted Answer

A)  d orbital. 
B)  f orbital. 
C)  g orbital. 
D)  p orbital. 
E)  s orbital. 
A)  d orbital. 
B)  f orbital. 
C)  g orbital. 
D)  p orbital. 
E)  s orbital.

Question 10

If we take away two electrons from the outer shell of calcium, it would have the same electron configuration as what element

Accepted Answer

A)  Argon 
B)  Titanium 
C)  Stronium 
D)  Magnesium 
E)  None of the above 
A)  Argon 
B)  Titanium 
C)  Stronium 
D)  Magnesium 
E)  None of the above

Question 11

Using the figure below, categorize electromagnetic radiation with an energy of 6.7 x 10-18 J/photon.

Accepted Answer

A)  Gamma rays 
B)  X rays 
C)  Ultraviolet 
D)  Infrared 
E)  Microwave 
A)  Gamma rays 
B)  X rays 
C)  Ultraviolet 
D)  Infrared 
E)  Microwave

Question 12

The frequency of the emitted light from a cesium atom is an intensive property.

Accepted Answer

A) True 
 B)False

Question 13

Calculate the frequency of visible light having a wavelength of 686 nm.

Accepted Answer

A)  4.37 * 1014 /s 
B)  4.37 * 105 /s 
C)  6.17 * 1014 /s 
D)  2.29 * 10-15 /s 
E)  2.29 * 10-6 /s 
A)  4.37 * 1014 /s 
B)  4.37 * 105 /s 
C)  6.17 * 1014 /s 
D)  2.29 * 10-15 /s 
E)  2.29 * 10-6 /s

Question 14

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen En = -2.18 * 10-18 J(1/n2).

Accepted Answer

A)  1.82 * 10-19 /s 
B)  9.13 * 1013 /s 
C)  2.74 * 1014/s 
D)  3.65 * 1014 /s 
E)  1.64 * 1015 /s 
A)  1.82 * 10-19 /s 
B)  9.13 * 1013 /s 
C)  2.74 * 1014/s 
D)  3.65 * 1014 /s 
E)  1.64 * 1015 /s

Question 15

The quantum numbers, n = 4, l = 3, ml = 2, ms = +1/2, represent an electron in a ___ subshell

Accepted Answer

A)  4f 
B)  4d 
C)  4p 
D)  4s 
E)  None of the above 
A)  4f 
B)  4d 
C)  4p 
D)  4s 
E)  None of the above

Question 16

Which element has the following ground-state electron configuration
[Kr]5s14d5

Accepted Answer

A)  Mn 
B)  Mo 
C)  Nb 
D)  Re 
E)  Tc 
A)  Mn 
B)  Mo 
C)  Nb 
D)  Re 
E)  Tc

Question 17

How many orbitals are allowed in a subshell if l = 3

Accepted Answer

A)  1 
B)  3 
C)  5 
D)  7 
E)  9 
A)  1 
B)  3 
C)  5 
D)  7 
E)  9

Question 18

The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of these colors, ______ has the shortest wavelength.

Accepted Answer

A)  Red 
B)  Yellow 
C)  Green 
D)  Indigo 
E)  Violet 
A)  Red 
B)  Yellow 
C)  Green 
D)  Indigo 
E)  Violet

Question 19

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm

Accepted Answer

A)  6.46 * 10-25 J 
B)  6.46 * 10-16 J 
C)  2.46 * 10-4 J 
D)  12.4 kJ 
E)  246 kJ 
A)  6.46 * 10-25 J 
B)  6.46 * 10-16 J 
C)  2.46 * 10-4 J 
D)  12.4 kJ 
E)  246 kJ

Question 20

What is the maximum number of electrons in an atom that can have the following set of quantum numbers
N = 3 $~~$l = 2 $~~$ml = -2

Accepted Answer

A)  18 
B)  10 
C)  5 
D)  2 
E)  1 
A)  18 
B)  10 
C)  5 
D)  2 
E)  1

Exam 7: Quantum Theory and the Electronic Structure of Atoms

If a hydrogen atom and a helium atom are traveling at the same speed,

Which of the following, if any, is the correct ground state electron configuration for Cr

A ground-state atom of iron has ___ unpaired electrons and is _____.

When photons with a wavelength of 310. nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 * 105 m/s. Calculate the binding energy of electrons to the magnesium surface.

Which of the following wavelengths of electromagnetic radiation has the highest energy

Which one of the following sets of quantum numbers is not possible \nobreakspace\nobreakspace\nobreakspace\nobreakspace\nobreakspace n l A. 4 3 -2 +1/2 B. 3 0 1 -1/2 C. 3 0 0 +1/2 D. 2 1 1 -1/2 E. 2 0 0 +1/2

Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen En = -2.18 * 10-18 J(1/n2).

Electrons in an orbital with l = 3 are in a/an

If we take away two electrons from the outer shell of calcium, it would have the same electron configuration as what element

Using the figure below, categorize electromagnetic radiation with an energy of 6.7 x 10-18 J/photon.

The frequency of the emitted light from a cesium atom is an intensive property.

Calculate the frequency of visible light having a wavelength of 686 nm.

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen En = -2.18 * 10-18 J(1/n2).

The quantum numbers, n = 4, l = 3, ml = 2, ms = +1/2, represent an electron in a ___ subshell

Which element has the following ground-state electron configuration [Kr]5s14d5

How many orbitals are allowed in a subshell if l = 3

The colors of the visible spectrum are blue, green, orange, red, violet, and yellow. Of these colors, ______ has the shortest wavelength.

What is the energy in joules of a mole of photons associated with visible light of wavelength 486 nm

What is the maximum number of electrons in an atom that can have the following set of quantum numbers N = 3 ~~ l = 2 ~~ ml = -2

Chemistry: The Study of Change

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Mass Relationships in Chemical Reactions

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Chemical Bonding I: Basic Concepts

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Entropy Free Energy and Equilibrium

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A ground-state atom of iron has _ unpaired electrons and is ___.

When photons with a wavelength of 310. nm strike a magnesium plate, the maximum velocity of the ejected electrons is 3.45 * 10⁵ m/s. Calculate the binding energy of electrons to the magnesium surface.

Calculate the wavelength of the light emitted by a hydrogen atom during a transition of its electron from the n = 4 to the n = 1 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²).

Using the figure below, categorize electromagnetic radiation with an energy of 6.7 x 10^-18 J/photon.

Calculate the frequency of the light emitted by a hydrogen atom during a transition of its electron from the n = 6 to the n = 3 principal energy level. Recall that for hydrogen E_n = -2.18 * 10^-18 J(1/n²).

The quantum numbers, n = 4, l = 3, m_l = 2, m_s = +1/2, represent an electron in a ___ subshell

Which element has the following ground-state electron configuration [Kr]5s¹4d⁵

What is the maximum number of electrons in an atom that can have the following set of quantum numbers N = 3 $$ l = 2 $$ m_l = -2