Question 1

The maximum number of electrons that can occupy an energy level described by the principal quantum number, n, is

Accepted Answer

A) n 
B) n + 1 
C) 2n 
D) 2n2 
E) n2 
A) n 
B) n + 1 
C) 2n 
D) 2n2 
E) n2 D

Question 2

Rank the following types of electromagnetic radiation from lowest energy to highest energy: infrared, microwave, radio waves, gamma rays, visible, and ultraviolet.

Accepted Answer

radio waves < microwaves < infrared < visible < ultraviolet < gamma rays

Question 3

"No two electrons in an atom can have the same four quantum numbers" is a statement of

Accepted Answer

A) the Pauli exclusion principle. 
B) Bohr's equation. 
C) Hund's rule. 
D) de Broglie's relation. 
E) Dalton's atomic theory. 
A) the Pauli exclusion principle. 
B) Bohr's equation. 
C) Hund's rule. 
D) de Broglie's relation. 
E) Dalton's atomic theory. A

Question 4

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

Accepted Answer

The answer of The colors of the visible spectrum are...

Question 5

Which ground-state atom has an electron configuration described by the following orbital diagram?

Accepted Answer

A) phosphorus 
B) germanium 
C) selenium 
D) tellurium 
E) none of these 
A) phosphorus 
B) germanium 
C) selenium 
D) tellurium 
E) none of these

Question 6

Which ground-state atom has an electron configuration described by the following orbital diagram?

Accepted Answer

A) antimony 
B) germanium 
C) indium 
D) lead 
E) tin 
A) antimony 
B) germanium 
C) indium 
D) lead 
E) tin

Question 7

Which of the following ground-state atoms is diamagnetic?

Accepted Answer

A) Ca 
B) As 
C) Cu 
D) Fe 
E) none of these 
A) Ca 
B) As 
C) Cu 
D) Fe 
E) none of these

Question 8

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

Question 9

Transition metal elements have atoms or ions with partially filled

Accepted Answer

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

Question 10

A photon is roughly 1800 times more massive than an electron.If a proton and an electron have the same kinetic energy,

Accepted Answer

A) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. 
B) the wavelength of the photon will be about   times longer than the wavelength of the electron. 
C) the wavelength of the photon will be roughly equal to the wavelength of the electron. 
D) the wavelength of the electron will be about   times longer than the wavelength of the photon. 
E) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon. 
A) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. 
B) the wavelength of the photon will be about   times longer than the wavelength of the electron. 
C) the wavelength of the photon will be roughly equal to the wavelength of the electron. 
D) the wavelength of the electron will be about   times longer than the wavelength of the photon. 
E) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon.

Question 11

For all atoms of the same element, the 2s orbital is larger than the 1s orbital.

Accepted Answer

A) True 
 B)False

Question 12

If one electron is added to the outer shell of chlorine, it would have the same electron configuration as what element?

Accepted Answer

The answer of If one electron is added to the...

Question 13

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by En = -2.18 * 10-18 J(1/n2)

Accepted Answer

A) 4.45 * 10-20 nm 
B) 2.16 * 10-6 nm 
C) 9.18 * 10-20 nm 
D) 1.38 * 1014 nm 
E) 2.16 * 103 nm 
A) 4.45 * 10-20 nm 
B) 2.16 * 10-6 nm 
C) 9.18 * 10-20 nm 
D) 1.38 * 1014 nm 
E) 2.16 * 103 nm

Question 14

A photovoltaic cell converts light into electrical energy. Suppose a certain photovoltaic cell is only 63.5% efficient, in other words, that 63.5% of the light energy is ultimately recovered. If the energy output of this cell is used to heat water, how many 520 nm photons must be absorbed by the photovoltaic cell in order to heat 10.0 g of water from 20.0°C to 30.0°?

Accepted Answer

1.72 * 10<

Question 15

A possible set of quantum numbers for the last electron added to complete an atom of germanium (Ge)in its ground state is

Accepted Answer

The answer of A possible set of quantum numbers for...

Question 16

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by En = -2.18 * 10-18 J(1/n2)

Accepted Answer

A) 2.07 * 10-29 J 
B) 2.19 * 105 J 
C) 2.04 *10-18 J 
D) 3.27 * 10-17 J 
E) 2.25 * 10-18 J 
A) 2.07 * 10-29 J 
B) 2.19 * 105 J 
C) 2.04 *10-18 J 
D) 3.27 * 10-17 J 
E) 2.25 * 10-18 J

Question 17

Which ground-state atom has an electron configuration described by the following orbital diagram?

Accepted Answer

A) phosphorus 
B) nitrogen 
C) arsenic 
D) vanadium 
E) none of these 
A) phosphorus 
B) nitrogen 
C) arsenic 
D) vanadium 
E) none of these

Question 18

The orbital diagram for a ground-state oxygen atom is

Accepted Answer

The answer of The orbital diagram for a ground-state oxygen...

Question 19

How many electrons in a ground-state cadmium atom are in orbitals labeled by ml = -1?

Accepted Answer

A) 2 
B) 10 
C) 12 
D) 18 
E) 36 
A) 2 
B) 10 
C) 12 
D) 18 
E) 36

Question 20

A proton is roughly 1800 times more massive than an electron.If a proton and an electron are traveling at the same speed,

Accepted Answer

A) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. 
B) the wavelength of the photon will be about   times longer than the wavelength of the electron. 
C) the wavelength of the photon will be roughly equal to the wavelength of the electron. 
D) the wavelength of the electron will be about   times longer than the wavelength of the photon. 
E) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon. 
A) the wavelength of the photon will be about 1800 times longer than the wavelength of the electron. 
B) the wavelength of the photon will be about   times longer than the wavelength of the electron. 
C) the wavelength of the photon will be roughly equal to the wavelength of the electron. 
D) the wavelength of the electron will be about   times longer than the wavelength of the photon. 
E) the wavelength of the electron will be about 1800 times longer than the wavelength of the photon.

Exam 7: Quantum Theory and the Electronic Structure of Atoms

The maximum number of electrons that can occupy an energy level described by the principal quantum number, n, is

Rank the following types of electromagnetic radiation from lowest energy to highest energy: infrared, microwave, radio waves, gamma rays, visible, and ultraviolet.

"No two electrons in an atom can have the same four quantum numbers" is a statement of

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

Which ground-state atom has an electron configuration described by the following orbital diagram?

Which ground-state atom has an electron configuration described by the following orbital diagram?

Which of the following ground-state atoms is diamagnetic?

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.

Transition metal elements have atoms or ions with partially filled

A photon is roughly 1800 times more massive than an electron.If a proton and an electron have the same kinetic energy,

For all atoms of the same element, the 2s orbital is larger than the 1s orbital.

If one electron is added to the outer shell of chlorine, it would have the same electron configuration as what element?

Calculate the wavelength, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by En = -2.18 * 10-18 J(1/n2)

A possible set of quantum numbers for the last electron added to complete an atom of germanium (Ge)in its ground state is

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by En = -2.18 * 10-18 J(1/n2)

Which ground-state atom has an electron configuration described by the following orbital diagram?

The orbital diagram for a ground-state oxygen atom is

How many electrons in a ground-state cadmium atom are in orbitals labeled by ml = -1?

A proton is roughly 1800 times more massive than an electron.If a proton and an electron are traveling at the same speed,

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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, in nanometers, of the light emitted by a hydrogen atom when its electron falls from the n = 7 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by E_n = -2.18 * 10^-18 J(1/n²)

Calculate the energy, in joules, required to excite a hydrogen atom by causing an electronic transition from the n = 1 to the n = 4 principal energy level. Recall that the energy levels of the H atom are given by E_n = -2.18 * 10^-18 J(1/n²)

How many electrons in a ground-state cadmium atom are in orbitals labeled by m_l= -1?