Question

11 consider the hydrogen spectrum in model 2.
a which color of light has the most energy?
b which color of light has the least energy?
12 does a gas - discharge tube filled with boron emit the same wavelengths of light as a tube filled with hydrogen? use evidence from model 3 to support your answer.
13 “the spectral lines for atoms are like fingerprints for humans.” how do the spectral lines for hydrogen and boron support this statement?
circle the appropriate word to complete each statement in questions 14 - 17.

1. electrons and protons (attract/repel) each other.
2. as an electron gets closer to the nucleus the (attraction/repulsion) to the nucleus gets (stronger/weaker).
3. for an electron to move from an energy level close to the nucleus to an energy level far from the nucleus it would need to (gain/lose) energy.
4. for an electron to move from an energy level far from the nucleus to an energy level close to the nucleus it would need to (gain/lose) energy.

read this!
niels bohr modified rutherfords nuclear atom model to explain how light interacts with the electrons in an atom to produce spectral lines. his model included electrons orbiting the nucleus at specific energy levels. electrons absorb energy from various sources (electricity) when they move from lower energy levels (ground state) to higher energy levels (excited states). energy is released as electrons return to their lower energy levels.

1. is energy absorbed or released for the electron transition shown in the diagram to the right? explain.

Explanation:

Step1: Recall the relationship between color, wavelength and energy of light

The energy of a photon of light is given by $E = h
u=\frac{hc}{\lambda}$, where $h$ is Planck's constant, $
u$ is the frequency, $c$ is the speed of light and $\lambda$ is the wavelength. Shorter wavelengths correspond to higher frequencies and higher energies. Violet light has a shorter wavelength than red light, so violet has more energy and red has less energy.

Step2: Understand atomic spectra

Each element has a unique set of electron energy levels. When electrons transition between these levels, they emit or absorb light of specific wavelengths. Since hydrogen and boron have different electron configurations and energy - level structures, their spectral lines are different.

Step3: Explain the uniqueness of spectral lines

The energy - level transitions in an atom are quantized and unique to each element. The pattern of spectral lines produced by these transitions is like a fingerprint for the element, allowing for element identification.

Step4: Recall electric charge interactions

Electrons are negatively charged and protons are positively charged. Opposite charges attract, so electrons and protons attract each other.

Step5: Analyze electron - nucleus attraction

As an electron gets closer to the nucleus, the electrostatic attraction between the negatively - charged electron and the positively - charged nucleus increases.

Step6: Consider electron energy level transitions

To move to a higher energy level (farther from the nucleus), an electron needs to gain energy from an external source.

Step7: Consider reverse electron energy level transitions

To move to a lower energy level (closer to the nucleus), an electron releases energy.

Step8: Analyze electron transitions and energy

Based on the Bohr model, if an electron moves to a higher energy level, it must absorb energy to overcome the electrostatic pull and move to a more distant orbital. If it moves to a lower energy level, it releases energy.

Answer:

11.
a. Violet light has the most energy.
b. Red light has the least energy.

1. No, a gas - discharge tube filled with boron will not emit the same wavelengths of light as a tube filled with hydrogen. Each element has a unique set of spectral lines because the energy levels of electrons in different atoms are different. Hydrogen and boron have different electron - configurations and thus different energy level transitions, resulting in different spectral lines.
2. The spectral lines for hydrogen and boron are unique to each element. Just as human fingerprints are unique to each individual, the pattern of spectral lines for each element is characteristic and can be used to identify the element. Each element has a specific set of electron - energy level transitions that produce a distinct set of spectral lines.
3. Attract
4. Attraction; stronger
5. Gain
6. Lose
7. If the electron is moving from a lower energy level to a higher energy level (e.g., from n = 1 to n = 2 in the diagram), energy is absorbed. This is because electrons need to gain energy to move to a higher - energy orbital. If it is moving from a higher energy level to a lower energy level, energy is released.