Question 1

In quantum mechanics, an " l " value of 2 corresponds to a letter designation of:
A) s
B) p
C) d
D) f

Accepted Answer

The "l" value in quantum mechanics corresponds to the angular momentum quantum number, which determines the shape of the orbital. An "l" value of 0 corresponds to an s orbital, 1 to a p orbital, 2 to a d orbital, and 3 to an f orbital. Therefore, an "l" value of 2 corresponds to a d orbital.

Question 2

X-ray fluorescence is an analytical technique that uses high energy x-rays to eject protons from the nucleus of an atom.

Accepted Answer

X-ray fluorescence (XRF) is an analytical technique that involves the excitation of atoms in a sample by bombarding it with high-energy X-rays, leading to the ejection of electrons from the inner shells of the atoms. The vacancies are then filled by electrons from higher energy levels, emitting X-ray fluorescence in the process. It does not involve the ejection of protons from the nucleus.

Question 3

The bending of light as it passes between air and another denser media is referred to as:
A) diffraction
B) refraction
C) retraction
D) an illusion

Accepted Answer

Refraction is the bending of light as it passes from one medium to another of different density, such as from air into water.

Question 4

Atomic absorption spectrometry (AAS) works based on the principle that certain atoms or molecules absorp light in direct proportion to the number of atoms or molecues of that type in the sample.

Accepted Answer

Atomic absorption spectrometry (AAS) is based on the principle that atoms in the ground state can absorb light of specific wavelengths, and the amount of light absorbed is directly proportional to the number of atoms of the element in the sample.

Question 5

Quantum numbers arise from the functions that solve the wave equations for an atom.

Accepted Answer

Quantum numbers are derived from the solutions to the Schrödinger wave equation for an atom, which describe the quantized states of an electron in an atom, including its energy, angular momentum, and magnetic orientation.

Question 6

Infrared light has higher wavelengths than gamma rays.

Accepted Answer

Infrared light has longer wavelengths ranging from about 700 nanometers to 1 millimeter, whereas gamma rays have much shorter wavelengths, less than 10 picometers, making infrared light's wavelengths higher than those of gamma rays.

Question 7

If photon "A" has twice the energy of photon "B" in a given media, then "A" should have  the frequency of "B".

Accepted Answer

The answer of If photon "A" has twice the energy...

Question 8

The Pauli Exclusion Principle states that no two electrons in the same atom may have the same set of four quantum numbers.

Accepted Answer

The Pauli Exclusion Principle, formulated by Wolfgang Pauli in 1925, asserts that no two electrons in an atom can have identical values for all four of their quantum numbers (principal, azimuthal, magnetic, and spin), ensuring each electron in an atom has a unique quantum state.

Question 9

To better characterize the electron in a quantum mechanical model, Erwin Schrödinger introduced the equation: H ψ = E ψ . In this equation ψ represents a(n):
A) neutron redux
B) proton period
C) electron mass
D) wave function

Accepted Answer

In the Schrödinger equation, ψ represents the wave function of a particle, which in this context is related to the probability amplitude of finding an electron at a particular location.

Question 10

The now-characteristic model of the atom relies upon the idea that the electrons reside in stable orbits from which they can not deviate and are found outside of a small, densely packed group of protons. This model was created by:
A) Albert Einstein
B) Julius Saulk
C) Niels Bohr
D) Edward Teller

Accepted Answer

Niels Bohr proposed the model of the atom where electrons orbit the nucleus in stable, quantized orbits, with the nucleus containing protons (and neutrons, though the neutron was not yet discovered at the time of his initial model). This was a significant advancement from previous models and helped explain atomic structure and spectral lines.

Question 11

The characteristic wavelengths of light absorbed by and emitted from an atom is known as the atom's:
A) parcel number
B) atomic spectrum
C) nuclear potential
D) period

Accepted Answer

The atomic spectrum is a unique set of frequencies of electromagnetic radiation emitted or absorbed by an atom, serving as a fingerprint for the element.

Question 12

In the wave model, the amplitude of the wave determines the brightness of the light.

Accepted Answer

In the wave model of light, the amplitude of the wave is directly related to the brightness or intensity of the light; higher amplitudes correspond to brighter light.

Question 13

A museum holds a painting by Renoir and wishes to learn more about the trace composition of the pigments used in the priceless artwork. XRF is superior to AAS for this project because:
A) XRF is a non-destructive techinique
B) XRF is capable of measure multiple elements simultaneously
C) AAS is only used for molecular analysis
D) both a and b

Accepted Answer

XRF (X-ray fluorescence) is superior for this project because it is non-destructive (A), meaning it won't damage the priceless artwork by requiring a sample to be removed. Additionally, XRF can measure multiple elements simultaneously (B), making it more efficient for analyzing the complex mixtures of pigments in a painting. AAS (Atomic Absorption Spectroscopy), on the other hand, typically analyzes one element at a time and often requires sample preparation that could harm the artwork.

Question 14

The "n" value of the quantum number assigned to an atom best describes the orbit's:
A) shape
B) size
C) orientation
D) electron spin

Accepted Answer

The "n" value of the quantum number assigned to an atom best describes the orbit's size.

Question 15

As an electron moves closer to the nucleus, energy is:
A) absorbed
B) released
C) remains unchanged
D) transformed into a proton

Accepted Answer

When an electron moves closer to the nucleus, it moves to a lower energy level, and the energy difference is released, usually in the form of a photon. This process is consistent with the conservation of energy principle.

Question 16

In quantum mechanics, an " l " value of 0 corresponds to a letter designation of:
A) s
B) p
C) d
D) f

Accepted Answer

In quantum mechanics, the azimuthal quantum number (l) defines the shape of an orbital, and an l value of 0 corresponds to an s orbital.

Question 17

As part of the quantization of light, Einstein proposed that light could behave as packets of energy referred to as:
A) photons
B) protons
C) electrons
D) nucleons

Accepted Answer

Einstein proposed the concept of light consisting of discrete packets of energy, which he called photons, to explain phenomena such as the photoelectric effect. This was a key development in the field of quantum mechanics.

Question 18

An excited electron can not remain so indefinitely and must eventually return to its ground state.

Accepted Answer

An excited electron cannot remain in an excited state indefinitely because it is unstable; it will eventually release energy (often in the form of a photon) and return to its ground state, which is its most stable and lowest energy level.

Question 19

The energy of an incoming photon must be greater than the binding energy of the metal's electron in order to have that electron ejected from the metal's surface.

Accepted Answer

For the photoelectric effect to occur, the energy of the incoming photon must be greater than the binding energy of the electron in the metal. This is necessary to overcome the forces holding the electron in the metal and eject it from the surface.

Question 20

Because the speed of light remains constant for a given media frequency and wavelength are inversely proportional.

Accepted Answer

In a given medium, the speed of light is constant, so as the frequency of the light increases, its wavelength decreases, and vice versa, making frequency and wavelength inversely proportional to each other. This relationship is described by the equation $c = \lambda \nu$, where $c$ is the speed of light in the medium, $\lambda$ is the wavelength, and $\nu$ is the frequency.

Quiz 6: The Periodic Table and Atomic Structure

In quantum mechanics, an " l " value of 2 corresponds to a letter designation of:

X-ray fluorescence is an analytical technique that uses high energy x-rays to eject protons from the nucleus of an atom.

The bending of light as it passes between air and another denser media is referred to as:

Atomic absorption spectrometry (AAS) works based on the principle that certain atoms or molecules absorp light in direct proportion to the number of atoms or molecues of that type in the sample.

Quantum numbers arise from the functions that solve the wave equations for an atom.

Infrared light has higher wavelengths than gamma rays.

If photon "A" has twice the energy of photon "B" in a given media, then "A" should have the frequency of "B".

The Pauli Exclusion Principle states that no two electrons in the same atom may have the same set of four quantum numbers.

To better characterize the electron in a quantum mechanical model, Erwin Schrödinger introduced the equation: H ψ = E ψ . In this equation ψ represents a(n) :

The now-characteristic model of the atom relies upon the idea that the electrons reside in stable orbits from which they can not deviate and are found outside of a small, densely packed group of protons. This model was created by:

The characteristic wavelengths of light absorbed by and emitted from an atom is known as the atom's:

In the wave model, the amplitude of the wave determines the brightness of the light.

A museum holds a painting by Renoir and wishes to learn more about the trace composition of the pigments used in the priceless artwork. XRF is superior to AAS for this project because:

The "n" value of the quantum number assigned to an atom best describes the orbit's:

As an electron moves closer to the nucleus, energy is:

In quantum mechanics, an " l " value of 0 corresponds to a letter designation of:

As part of the quantization of light, Einstein proposed that light could behave as packets of energy referred to as:

An excited electron can not remain so indefinitely and must eventually return to its ground state.

The energy of an incoming photon must be greater than the binding energy of the metal's electron in order to have that electron ejected from the metal's surface.

Because the speed of light remains constant for a given media frequency and wavelength are inversely proportional.