Quantum Leaps: The Atomic Transitions Spectra Quiz

If an electron absorbs a photon, then it gains that photon's energy. If the energy of the electron increases, then it must move to a shell further from the nucleus that corresponds to a higher energy state. Therefore, the electron transitions to an excited state.

If an electron is in an excited state, it is unstable. If the electron drops to a lower, more stable energy level, then it must release its excess energy. If that energy is released as light, then a bright line appears in the emission spectrum. Therefore, the statement is true.

If an element has a specific number of protons, then the electrical pull on its electrons is unique. If the electrical pull is unique, then the spacing between its energy levels is unique. If the energy levels are unique, then the photons emitted during transitions will have unique energies/colors. Therefore, spectral lines act as an atomic "fingerprint."

If a hydrogen electron falls from a higher level (n>2) down to the second energy level (n=2), then the energy released corresponds to visible light. If this specific group of transitions was named after its discoverer, Johann Balmer, then it is known as the Balmer series. Therefore, the answer is Balmer.

If the energy of a photon is defined by the equation E=hf, then E (energy) is directly proportional to f (frequency). If the frequency of the light wave becomes higher, then the energy of the individual photon must also become higher. Therefore, high-frequency light like X-rays has more energy than low-frequency radio waves.

If a gas is cool, its electrons are in the ground state. If light passes through, the electrons will "pick" only the photons that match the gaps between their energy levels. If those photons are removed from the light beam, then dark gaps (absorption lines) appear in the resulting spectrum. Therefore, A, B, and D are correct.

If energy levels in an atom are "quantized," then electrons can only exist at specific energy values, never in between. If an incoming photon does not have the exact amount of energy to move an electron to an existing higher level, then the electron cannot accept it. Therefore, the photon passes through without being absorbed.

If the gap between n=4 and n=1 is physically and energetically larger than the gap between n=2 and n=1, then an electron dropping from n=4 must release more energy. If more energy is released, the resulting photon will have a higher frequency. Therefore, the 4→1 transition is a higher energy emission.

If an electron is in the orbital closest to the nucleus (n=1), then it has the minimum amount of potential energy possible. If this state is the baseline for the atom, then it is called the ground state. Therefore, the answer is ground.

If an atom is heavy (many protons), the innermost electrons are very tightly bound. If an electron is knocked out and a transition occurs to fill this deep inner shell, then a very large amount of energy is released. If X-rays represent very high-energy photons, then they are the result of these deep transitions. Therefore, X-rays are the correct answer.

If the speed of light is constant, then f=c/λ. If energy is E=hf, then substituting gives E=hc/λ. If λ (wavelength) is in the denominator, then as wavelength gets smaller, energy gets larger. Therefore, shorter wavelengths have higher energy.

If color is determined by the frequency/wavelength of light, and frequency is determined by the energy of the photon (E=hf), then the color is directly tied to the energy. If that energy came from an electron jump, then it must match the gap between the levels. Therefore, the gap size determines the color.

If a photon provides energy that exceeds the highest energy level (the binding energy), then the electron is no longer held by the nucleus. If the atom loses an electron, it becomes a charged ion. Therefore, the process is called ionization.

If we categorize how light is spread out, we see solid rainbows (continuous), bright lines on black (emission), or dark lines on a rainbow (absorption). If reflection and refraction are behaviors of light rather than types of spectra themselves, then only A, B, and C are valid spectral types.

If a source of waves moves away from an observer, then the waves are "stretched" to longer wavelengths (Doppler Effect). If red light has a longer wavelength than blue light, then stretching the light moves the lines toward the red. Therefore, this is known as a Redshift.

If electrons interact with electromagnetic radiation, then they absorb or emit "packets" of light. If "photons" are the particles of light and "protons" are positive particles in the nucleus, then the electron is interacting with photons. Therefore, the statement is false because it identifies the wrong particle.

If the jump down to n=1 is the largest possible jump in a hydrogen atom, then it releases the most energy. If Ultraviolet (UV) light is more energetic than visible light, then these high-energy transitions fall into the UV range. Therefore, the Lyman series is Ultraviolet.

If light needs to be analyzed by color, then it must be physically separated. If a device is designed to "see" (scope) the "spectrum," then it is a spectroscope. Therefore, the answer is spectroscope.

If an electron can only transition if it absorbs the exact energy difference between levels, and it absorbed 10.2 eV, then a gap of exactly 10.2 eV must exist. If the gap were any different, the photon would not have been absorbed. Therefore, A is the only logical conclusion.

If "transition" refers to both absorption and emission, then we must look at both directions. If absorption involves moving away from the nucleus and emission involves moving toward it, then high-energy light can cause either (depending on the direction of the jump). Therefore, the "always" makes the statement false.