Describe how the Bohr model explains both of these observations.

The question is incomplete, the complete question is;

Scientists made the following two observations about emission spectra:

Each element has a unique emission spectrum.

Atoms emit energy only at specific wavelengths.

Describe how the Bohr model explains both of these observations.

Bohr model of the atom proposed that electrons in atoms were found in specific orbits known as energy levels. Atomic spectra results from when electrons transit between energy levels.

The Bohr model of the atom incorporated the idea of energy quantization into the atomic theory. The energy levels within the atom, according to this theory, is quantized.

This means that electrons can only have positive integer values of energy.

Since the atoms of each element has a unique arrangement of electrons in their orbits, atoms of various elements must have a unique(signature) emission spectrum generated by electronic transitions within the atoms according to Bohr's theory.

Also, emission or absorption of energy occurs at specific wavelengths because energy levels within the atom are quantized.

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In the Bohr model, electrons can exist only in certain energy levels surrounding the atom.

When electrons jump from a higher energy level to a lower one, they emit light at a wavelength that corresponds to the energy difference between the levels.

The energy levels in each atom are unique.

Explanation:

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the answer is true.

since the atomic number is the number of protons in the nucleus, as we move to the left on the periodic table, the electrostatic pull between the nucleus and the valence electron shell decreases. as we move down a group (vertical column), the valence shell energy level gets further and further from the nucleus.