1. Ground vs. Excited State
Ground State – electrons are in positions of lowest energy possible (normal)
Excited State – electron is in a temporary position of higher energy than ground state
Very unstable; the electron quickly returns to the ground state

2. Compared to a sodium atom in the ground state, a sodium atom in the excited state must have
iRespond Question
Multiple Choice F
There is not change in the number of electrons, just their location
A.) a greater number of electrons
B.) a smaller number of electrons
C.) an electron with greater energy
D.) an electron with less energy
E.)

3. Changes in Electron Energy
Electrons must gain energy to transition to the excited state
Electrons release energy transitioning back to the ground state
Ground  Excited
e- gains energy
Excited  Ground
e- releases energy Be

4. Which electron transition represents a gain of energy?
iRespond Question
Multiple Choice F
The farther from the nucleus the greater the energy
A.) from 2nd to 3rd shell
B.) from 2nd to 1st shell
C.) from 3rd to 2nd shell
D.) from 3rd to 1st shell
E.)

5. Emission of Energy 1
All elements have a unique energy level system (due to differences in nuclear charge)
The amount of energy released when returning from excited state to ground state is different for each element
Multiple transitions are possible
Some of the energy released has wavelengths within the visible light range

6. Atomic Spectra 1
If the light emitted by an electron is passed through a prism it produces an atomic emission spectrum
The results are lines of light at specific energy levels
The atomic spectra of a given element is unique and can be used to identify an element

7. Na K Ca Cu Ba

8. High to low releases energy
The characteristic bright-line spectrum of an element occurs when electrons
iRespond Question F
Multiple Choice
A.) move from lower to higher energy levels
B.) move from higher to lower energy levels
C.) are lost by a neutral atom
D.) are gained by a neutral atom
High to low releases energy
E.)

9. The characteristic spectral lines of elements are caused when electrons in an excited atom move from
iRespond Question F
Multiple Choice
A.) lower to higher energy levels, releasing energy
B.) lower to higher energy levels, absorbing energy
C.) higher to lower energy levels, releasing energy
D.) higher to lower energy levels, absorbing energy
E.)

10. Electron X can change to a higher energy level or a lower energy level
Electron X can change to a higher energy level or a lower energy level. Which statement is true of electron X?
iRespond Question F
Multiple Choice
A.) Electron X emits energy when it changes to a higher energy level.
B.) Electron X absorbs energy when it changes to a higher energy level.
C.) Electron X absorbs energy when it changes to a lower energy level.
D.) Electron X neither emits nor absorbs energy when it changes energy level.
E.)

11. Which of the following quantum leaps would be associated with the greatest energy of emitted light?
iRespond Question F
Multiple Choice
A.) n = 5 to n = 1
B.) n = 4 to n = 5
C.) n = 2 to n = 5
D.) n = 5 to n = 4
E.)

12. The atomic emission spectra of a sodium atom on Earth and of a sodium atom in the sun would be
iRespond Question F
Multiple Choice
A.) the same
B.) different from each other
C.) the same as those of several other elements
D.) the same as each other only in the ultraviolet range
Each element has a unique spectra that is unchanged based on locations
E.)

13. Which two elements are present in the unknown spectra below?
iRespond Question F
Multiple Choice
A.) Li & H
B.) Li & Na
C.) H & He
D.) Li & He
E.)

14. Electron Cumulative Quiz
Valence Electrons
Lewis Dot Diagrams
Ground Vs. Excited State
Bright Line Spectra