Question 1

Light is emitted as an electron transitions from a higher energy state to a lower energy state. How long does it take for the actual transition to take place?
A)several seconds
B)several microseconds
C)several nanoseconds
D)no time at all

Accepted Answer

The actual transition happens instantaneously without any time delay. However, the emission of the light may take a certain amount of time, which depends on the characteristics of the emitter and the medium through which the light travels.

Question 2

The electron configuration of any neutral group 1 element always ends with ________. A)s¹ B)d¹⁰ C)s² D)p¹

Accepted Answer

Group 1 elements, also known as alkali metals, have one electron in their outermost s orbital, so their electron configuration ends with s¹.

Question 3

An electron de-excites from the fourth quantum level to the third and then directly to the first. Two frequencies of light are emitted. How do their combined energies compare to the energy of the single frequency that would be emitted by de-excitation from the fourth level directly to the first level? The combined energies of the two frequencies emitted by the one electrons is ________.
A) greater than the energy of the single frequency
B) less than the energy of the single frequency
C) equal to the energy of the single frequency
D) not predictable because other factors, such as the temperature of the surroundings must also be considered.

Accepted Answer

The energy levels in an atom are quantized, and the energy difference between two levels determines the frequency of the emitted light. The total energy released in a multi-step transition is equal to the energy released in a direct transition between the same initial and final states.

Question 4

The energy level diagram ranks orbitals by their ________.
A)sizes
B)complexity
C)electron capacities
D)average distance from the nucleus

Accepted Answer

The energy level diagram shows the relative energy levels of different orbitals in an atom. The orbitals are ordered by their average distance from the nucleus, with the lower energy levels (closer to the nucleus) being filled first. Therefore, choice D - average distance from the nucleus - is the correct answer. Choices A, B, and C are not accurate ways to rank orbitals in an energy level diagram.

Question 5

Suppose that a certain atom possesses only four distinct energy levels. Assuming that all transitions between levels are possible, how many spectral lines will this atom exhibit? 
A)three
B)four
C)six
D)unlimited

Accepted Answer

The number of spectral lines exhibited by an atom is equal to the number of possible transitions between its energy levels. In this case, there are 4 distinct energy levels, so there are 4C2 = 6 possible transitions (choosing 2 levels at a time to form a transition). Therefore, the atom will exhibit 6 spectral lines.

Question 6

Each atomic orbital can hold ________.
A)1 electron
B)up to 2 electrons
C)up to 3 electrons
D)up to 4 electrons

Accepted Answer

Each atomic orbital can hold up to 2 electrons, according to the Pauli exclusion principle.

Question 7

What property of an electron makes it possible to use electron microscopes?
A)They can be focused using smaller lenses.
B)They have shorter wavelengths than visible light.
C)They are electrically charged.
D)They can be generated with electricity.
E)none of the above

Accepted Answer

Electron microscopes use electrons, which have much shorter wavelengths than visible light, allowing for higher resolution imaging.

Question 8

How can a hydrogen atom, which has only one electron, have so many spectral lines?
A)The electron is able to move at various speeds.
B)The protons in the nucleus are also giving off various light frequencies.
C)Because there is more than one energy level in a hydrogen atom.
D)The atomic radius of the hydrogen atom is relatively large.

Accepted Answer

Hydrogen atoms have more than one energy level, so when the electron transitions between different energy levels, it emits or absorbs electromagnetic radiation, resulting in many different spectral lines.

(A) is incorrect because the electron in a hydrogen atom only has specific energy levels, so it cannot move at just any speed. 
(B) is incorrect because only the electron, not the protons in the nucleus, is responsible for the spectral lines. 
(D) is incorrect because the size of the atomic radius does not affect the number of spectral lines.

Question 9

An atom absorbs or emits only particular frequencies of light. White light bends into a glass prism and separates into a rainbow of colors. In which of these two scenarios does the electromagnetic radiation behave as a wave? As a particle?
A)Absorption of light shows wave behavior while bending of light shows particle behavior.
B)Absorption of light shows particle behavior while bending of light shows wave behavior.
C)Both absorption and bending of light show particle behavior.
D)Both absorption and bending of light show wave behavior.

Accepted Answer

Absorption of light by atoms is best explained by the particle nature of light, where photons are absorbed by electrons to move to higher energy levels. The bending of light, or refraction, as it passes through a prism is explained by the wave nature of light, where different frequencies (colors) of light bend at different angles due to their varying wavelengths.

Question 10

How might you distinguish a sodium-vapor street lamp from a mercury-vapor street lamp?
A)use binoculars to look for printing adjacent to the bulb
B)look at the street lamps through a spectroscope and match their spectral patterns to their respective atomic spectra
C)ask your local utility company to identify these lamps for you
D)The shadows cast from a sodium-vapor street lamp tend to be more diffuse around the edges.

Accepted Answer

The best way to distinguish between a sodium-vapor street lamp and a mercury-vapor street lamp is by looking at their spectral patterns. This can be done using a spectroscope, which will match the patterns to the respective atomic spectra for each type of lamp.

Question 11

What is a probability cloud?
A)It is a three-dimensional map of the likelihood of finding something within a given area.
B)It is a map of the likelihood of finding an electron within the nucleus.
C)It is a map of the likelihood of finding a particular proton within the nucleus.
D)It is a map of the likelihood of a photon ejecting an electron from an atom.
E)none of the above

Accepted Answer

A probability cloud is a three-dimensional representation of the probability of finding a particle at a particular point in space. It is commonly used in quantum mechanics to describe the behavior of electrons in atoms and molecules. The shape of the cloud indicates the probability of finding the particle in a particular region of space.

Question 12

Which color of light comes from the higher energy transition, red or blue?
A)Blue is a higher frequency and therefore corresponds to a lower energy level transition.
B)Blue is a higher frequency and therefore corresponds to a higher energy level transition.
C)Red is a higher frequency and therefore corresponds to a lower energy level transition.
D)Red is a higher frequency and therefore corresponds to a higher energy level transition.

Accepted Answer

Blue is a higher frequency and corresponds to a higher energy level transition. This is because frequency and energy are directly proportional. The higher the frequency, the higher the energy. Therefore, the color of light with the highest energy transition is blue.

Question 13

An atomic orbital ________.
A)is the path of an electron
B)is a region of space
C)can hold up to four electrons
D)is always spherical

Accepted Answer

An atomic orbital is a region of space around the nucleus where there is a high probability of finding an electron. It is not a physical path that the electron follows, and it can hold up to two electrons (for most orbitals). The shape of the orbital depends on its quantum numbers and can be spherical, dumbbell-shaped, or more complex.

Question 14

In some instances electromagnetic radiation behaves like a wave. In other instances electromagnetic radiation behaves more like a particle. Which behavior more accurately describes the true nature of electromagnetic radiation?
A)Particle behavior more accurately describes the true nature of electromagnetic radiation.
B)Electromagnetic radiation behaves both as a wave or as a particle depending on the circumstance.
C)Wave behavior more accurately describes the true nature of electromagnetic radiation.
D)There is no circumstance in which electromagnetic radiation can be described as either portraying particle or wave behavior.

Accepted Answer

Electromagnetic radiation exhibits characteristics of both waves and particles, depending on the circumstances. For example, in the photoelectric effect, electromagnetic radiation behaves like a particle (photon), while in diffraction and interference experiments, it behaves like a wave. This phenomenon is known as wave-particle duality, and it is a fundamental concept in quantum mechanics.

Question 15

Consider the various frequencies of the three photons emitted from the following three individual electron transitions in the figure below: n=3 to n=2; n=2 to n=1; n=3 to n=1. These transitions would produce three spectral lines in a spectroscope. If the energy spacing between the levels were equal, would this affect the number of spectral lines? 
A)Yes, two otherwise separate lines would converge into a single more intense line.
B)No, but the spacing between the spectral lines would change.
C)Yes, two otherwise separate lines would converge into a single less intense line.
D)No, but some would then require a prism in order to be seen.

Accepted Answer

The answer of Consider the various frequencies of the three...

Question 16

What is the relationship between the light emitted by an atom and the energies of the electrons in the atom?
A)The larger the atom, the greater the number of electrons and therefore the greater the frequency of a light.
B)The energies of the electrons of an atom are directly proportional to the wavelength of light emitted and therefore inversely proportional to the frequency of the light emitted.
C)The greater the frequency of a photon of light, the greater the energy packed into that photon.
D)The light emitted by an atom is a function of its nuclear density and its ability to absorb and reflect various wavelengths of light from the electromagnetic spectrum.

Accepted Answer

The energy of the electrons in an atom is directly proportional to the frequency of the light emitted. This means that as the energy level of an electron increases, the frequency of the emitted light also increases. Since the frequency of a photon is directly related to its energy, the greater the frequency of a photon of light, the greater the energy packed into that photon.

Question 17

How does the wave model of electrons orbiting the nucleus account for the fact that the electrons can have only discrete energy values?
A)Electrons are only able to vibrate at particular frequencies.
B)When an electron wave is confined, it is reinforced only at particular frequencies.
C)The energy values of an electron only occur where its wave properties and probability clouds are mutually reinforcing.
D)The wave model accounts for the types of orbitals an electron may occupy, not it's energy levels.

Accepted Answer

According to the wave model, electrons can be thought of as waves. When these waves are confined to the space around the nucleus, they interfere with themselves and form standing waves. These standing waves are reinforced only at certain frequencies, which correspond to the allowed energy levels of the electron. This is why electrons can have only discrete energy values in the wave model.

Question 18

Which of the following might best explain the reason why electrons are restricted to certain energy levels in an atom?
A)They behave like restricted waves and are self-reinforcing.
B)They are travelling at very high speeds.
C)They are interacting with the light around the atom.
D)They are out of phase and self-destruct when outside of distinct energy regions.
E)They behave like chaotic waves of alternating frequency.

Accepted Answer

Electrons are restricted to certain energy levels in an atom because they exhibit wave-like behavior, which allows them to exist only in orbits where they can form standing waves. This self-reinforcing wave pattern restricts them to specific energy levels.

Question 19

How might the spectrum of an atom appear if its electrons were not restricted to particular energy levels?
A)It would appear nearly the same as it does with the energy level restrictions.
B)There would be no frequencies within the visible portion of the electromagnetic spectrum.
C)A broad spectrum of all colors would be observed.
D)The frequency of the spectral lines would change with temperature.

Accepted Answer

When electrons are not restricted to particular energy levels, they can transition to any energy level, not just the predetermined ones. This means that they can emit a broad spectrum of all colors rather than the specific, discrete frequencies seen in the normal emission spectrum of an atom with energy level restrictions.

Question 20

Which of the following statements about electrons is true?
A)Electrons have a negative charge.
B)Electrons are particles.
C)Electrons behave like waves.
D)Electrons in atoms can be excited by light energy.
E)all of the above

Accepted Answer

All of the statements are true. Electrons have a negative charge, they are particles, and they also behave like waves. Electrons in atoms can be excited by light energy, which causes them to move to higher energy levels.

Quiz 4: Subatomic Particles

Light is emitted as an electron transitions from a higher energy state to a lower energy state. How long does it take for the actual transition to take place?

The electron configuration of any neutral group 1 element always ends with ________.

The energy level diagram ranks orbitals by their ________.

Suppose that a certain atom possesses only four distinct energy levels. Assuming that all transitions between levels are possible, how many spectral lines will this atom exhibit?

Each atomic orbital can hold ________.

What property of an electron makes it possible to use electron microscopes?

How can a hydrogen atom, which has only one electron, have so many spectral lines?

An atom absorbs or emits only particular frequencies of light. White light bends into a glass prism and separates into a rainbow of colors. In which of these two scenarios does the electromagnetic radiation behave as a wave? As a particle?

How might you distinguish a sodium-vapor street lamp from a mercury-vapor street lamp?

What is a probability cloud?

Which color of light comes from the higher energy transition, red or blue?

An atomic orbital ________.

In some instances electromagnetic radiation behaves like a wave. In other instances electromagnetic radiation behaves more like a particle. Which behavior more accurately describes the true nature of electromagnetic radiation?

What is the relationship between the light emitted by an atom and the energies of the electrons in the atom?

How does the wave model of electrons orbiting the nucleus account for the fact that the electrons can have only discrete energy values?

Which of the following might best explain the reason why electrons are restricted to certain energy levels in an atom?

How might the spectrum of an atom appear if its electrons were not restricted to particular energy levels?

Which of the following statements about electrons is true?