Question

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?

1. does a gas - discharge tube filled with boron emit the same wavelengths of light as a tube filled with hydrogen? use evidence from model 2 to support your answer.
2. “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 interacted 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:

a. Violet light has the shortest wavelength in the visible spectrum and according to the formula $E = h\frac{c}{\lambda}$ (where $E$ is energy, $h$ is Planck's constant, $c$ is the speed of light and $\lambda$ is wavelength), shorter wavelength means higher energy.
b. Red light has the longest wavelength in the visible spectrum and thus the least energy.

1. Different elements have different electron - configurations and energy levels, so 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.
2. Just as human fingerprints are unique, the spectral lines of hydrogen and boron are unique to each element. They are determined by the specific energy levels and electron transitions within the atoms of those elements.
3. Electrons are negatively charged and protons are positively charged, so they attract each other.
4. As an electron gets closer to the nucleus, the attraction to the nucleus gets stronger because of the electrostatic force between the negatively - charged electron and the positively - charged nucleus.
5. For an electron to move from an energy level close to the nucleus to an energy level far from the nucleus, it needs to gain energy as it is moving to a higher energy state.
6. For an electron to move from an energy level far from the nucleus to an energy level close to the nucleus, it needs to lose energy as it is moving to a lower energy state.
7. If the electron is moving from a higher energy level (outer levels) to a lower energy level (inner levels), energy is released. This is because when electrons transition to lower energy states, they emit photons of light with energy equal to the difference in energy between the two levels.

Answer:

a. Violet
b. Red

1. No, different elements have unique spectral lines due to different electron - configurations and energy levels.
2. Each element has a unique set of spectral lines determined by its electron transitions and energy levels, like unique fingerprints.
3. attract
4. attraction, stronger
5. gain
6. lose
7. If the electron is moving from a higher to a lower energy level, energy is released as photons are emitted.