Emission Spectra

Emission of light from an atom occurs when an electron

• drops from a higher to a lower energy level.
•    jumps from a lower to a higher energy level.   
•    moves within its atomic orbital.
• falls into the nucleus.

Line emission spectrum shown below happens when

• Electron transition from lower to higher energy level.
• Electron transition from higher to lower energy level.
• Electron exist in fixed energy states
• Electron transition between different energy levels.

The unknown emissions spectra belongs to the element

• Hydrogen

• Mercury

• Neon

• Sodium

If an electron moves from n=4 to n=2 it ____

• absorbs energy

• releases energy

Which elements are in the unknown sample?

• A and B
• B and C
• A and D
• B and D

The parallel lines represents...

• energy levels of the atom
• energy levels of the electrons
• energy levels of the photons
• energy levels of the nucleus

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

• Ground State

• Excited State

Which element(s) is/are found in the star's spectra below?

• Hydrogen only

• Hydrogen & Helium

• Calcium only

• Hydrogen & Calcium

The color of emitted light with the SHORTEST wavelength is

• violet

• green

• red

• indigo

The color of emitted light with the LONGEST wavelength is

• violet

• green

• red

• indigo