Question

t/f (correct to true if false)

1. the higher the energy of an em wave, the faster it travels.
2. an electron prefers to be in its ground state.
3. when an electron moves to the ground state from an excited state, it absorbs light energy.
4. when an electron moves to an orbit farther away from the nucleus, it emits light energy.
5. all electron transitions require the gaining or releasing of light energy.
6. a photon is an energy packet with no mass that we call light.
7. an electron can only absorb energy from a wavelength of light with the exact quanta of energy the light has.
8. an electron can exist anywhere in the electron cloud.
9. the wavelength of an em wave is measured from the crest to the trough of the wave.
10. emission spectra of an element is a continuous spectrum.
11. some elements can have the same emission spectrum.
12. each line on an emission spectrum corresponds to a single electron transition.
13. in the bohr model, electrons can only exist at fixed distances from the nucleus.
14. the bohr orbitals closer to the nucleus have lower energy than orbitals farther from the nucleus.

Explanation:

1. All electromagnetic (EM) waves travel at the speed of light (\(c = 3\times10^{8}\space m/s\)) in a vacuum, regardless of energy. So, the statement "The higher the energy of an EM wave, the faster it travels" is False.
2. The ground state is the lowest - energy state of an electron. Electrons tend to occupy the lowest - energy available states. So, "An electron prefers to be in its ground state" is True.
3. When an electron moves from an excited state to the ground state, it emits light energy (a photon). Absorption occurs when an electron moves to a higher - energy state. So, "When an electron moves to the ground state from an excited state, it absorbs light energy" is False.
4. When an electron moves to an orbit farther away from the nucleus (to a higher - energy state), it absorbs light energy. Emission occurs when it moves to a lower - energy state. So, "When an electron moves to an orbit farther away from the nucleus, it emits light energy" is False.
5. Electron transitions involve a change in energy. Energy is either gained (absorption) or released (emission) in the form of light (photons). So, "All electron transitions require the gaining or releasing of light energy" is True.
6. A photon is a quantum (packet) of electromagnetic energy. It has no rest mass. So, "A photon is an energy packet with no mass that we call light" is True.
7. Electrons can only absorb photons (light) with an energy equal to the difference between two energy levels (\(\Delta E=h

u\), where \(h\) is Planck's constant and \(
u\) is the frequency of the light). So, "An electron can only absorb energy from a wavelength of light with the exact quanta of energy the light has" is True.

1. Electrons in an atom are found in regions of space (orbitals) with specific probabilities. They are not "anywhere" in the electron cloud. So, "An electron can exist anywhere in the electron cloud" is False.
2. The wavelength (\(\lambda\)) of an EM wave is measured from crest - to - crest or trough - to - trough. So, "The wavelength of an EM wave is measured from the crest to the trough of the wave" is False.
3. The emission spectra of an element is a line spectrum (discrete lines), not a continuous spectrum. So, "Emission spectra of an element is a continuous spectrum" is False.
4. Each element has a unique emission spectrum (like a fingerprint). So, "Some elements can have the same emission spectrum" is False.
5. Each line in an emission spectrum corresponds to a specific electron transition between two energy levels (\(\Delta E = h

u\)). So, "Each line on an emission spectrum corresponds to a single electron transition" is True.

1. In the Bohr model, electrons are in fixed circular orbits at specific distances (radii) from the nucleus. So, "In the Bohr model, electrons can only exist at fixed distances from the nucleus" is True.
2. In the Bohr model, the energy of an electron in an orbit is given by \(E_n=-\frac{13.6}{n^{2}}\space eV\) (\(n = 1,2,3,\cdots\)). As \(n\) (the principal quantum number, related to the distance from the nucleus) increases, the energy of the electron increases. So, "The Bohr orbitals closer to the nucleus have lower energy than orbitals farther from the nucleus" is True.

Answer:

1. False
2. True
3. False
4. False
5. True
6. True
7. True
8. False
9. False
10. False
11. False
12. True
13. True
14. True