Question

in your textbook, read about the particle nature of light. circle the letter of the choice that best completes the statement or answers the question. 12. a(n) __ is the minimum amount of energy that can be lost or gained by an atom. a. valence electron b. electron c. quantum d. plancks constant 13. according to plancks theory, for a given frequency, v, matter can emit or absorb energy only in a. units of hertz. b. whole - number multiples of hv. c. entire wavelengths. d. multiples of 1/2 hv, 1/4 hv, and so on. 14. the __ is the phenomenon in which electrons are emitted from a metals surface when light of a certain frequency shines on it. a. quantum b. planck concept c. photon effect d. photoelectric effect 15. which equation would you use to calculate the energy of a photon? a. e_photon = hv × plancks constant b. e_photon = hv c. e_photon = 1/2 hv d. c = λv in your textbook, read about atomic emission spectra. for each statement below, write true or false. 16. like the visible spectrum, an atomic emission spectrum is a continuous range of colors. 17. each element has a unique atomic emission spectrum. 18. a flame test can be used to identify the presence of certain elements in a compound. 19. the fact that only certain colors appear in an elements atomic emission spectrum indicates that only certain frequencies of light are emitted. 20. atomic emission spectra can be explained by the wave model of light. 21. the neon atoms in a neon sign emit their characteristic color of light when they absorb energy. 22. when an atom emits light, photons having certain energies are being emitted.

Explanation:

1. A quantum is the minimum amount of energy that can be lost or gained by an atom.
2. According to Planck's theory, matter can emit or absorb energy only in whole - number multiples of $h

u$.

1. The photoelectric effect is the phenomenon where electrons are emitted from a metal's surface when light of a certain frequency shines on it.
2. The energy of a photon is calculated by $E_{photon}=h

u$.

1. An atomic emission spectrum is not a continuous range of colors like the visible spectrum, it is a line spectrum.
2. Each element has a unique atomic emission spectrum due to its distinct electron - energy levels.
3. A flame test can identify elements in a compound as different elements emit characteristic colors.
4. Only certain colors in an element's atomic emission spectrum indicate only certain frequencies of light are emitted as electrons transition between specific energy levels.
5. Atomic emission spectra are explained by the quantum model of the atom, not the wave model.
6. Neon atoms in a neon sign emit their characteristic color when they absorb energy and electrons transition to higher energy levels and then return to lower levels, emitting photons.
7. When an atom emits light, photons with certain energies are emitted corresponding to the energy differences between electron energy levels.

Answer:

1. c. quantum
2. b. whole - number multiples of $h

u$

1. d. photoelectric effect
2. b. $E_{photon}=h

u$

1. false
2. true
3. true
4. true
5. false
6. true
7. true