WorksheetsLight and Electron Energy Quiz
Total questions: 35
Worksheet time: 32mins
Explain how spectral lines of elements are like fingerprints of human beings:
What happens to white light when it passes through a prism?
It splits into the colors it's comprised of
It becomes brighter
It becomes dimmer
It disappears
Why are the color labels in the table in Model 1 plural?
Because there are different shades of each color
Because there are multiple colors mixed together
Because the colors change as light travels
Because it's a grammatical error
Which color corresponds to the longest wavelengths?
Reds
Blues
Violets
Greens
Do all colors of light have the same energy?
Yes
No, violets have the most energy and reds have the least energy
No, reds have the most energy and violets have the least energy
No, all colors have different energy levels
Which color of light corresponds to the shortest wavelength?
Red
Blue
Violet
Green
Which color of light has the most energy?
Red
Blue
Violet
Green
Which color of light has the least energy?
Red
Blue
Violet
Green
Is energy absorbed or released for the electron transition shown in the diagram?
Absorbed
Released
Neither absorbed nor released
Cannot be determined
Is energy absorbed or released for the electron transition shown in the diagram?
Absorbed
Released
Neither absorbed nor released
Cannot be determined
Which element(s) are in the Unknown mixture?
Li
H
He
Na
Which electron transition leads to the highest energy released:
n6 to n2
n5 to n2
n4 to n2
n3 to n2
Which electron transition leads to the lowest energy released:
n6 to n2
n5 to n2
n4 to n2
n3 to n2
Identify an unknown element with a brilliant yellow flame:
lithium
strontium
sodium
copper
potassium
Identify the unknown element using the spectral lines:
beryllium
copper
manganese
strontium
titanium
Violet waves have (a) wavelengths and (b) frequency.
Red waves have (a) wavelengths and (b) frequency.
Radio waves have (a) wavelengths and (b) frequency.
Gamma waves have (a) wavelengths and (b) frequency.
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 (a) energy.
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 (a) energy.
Are these electrons in the ground state or excited state?
Ground
Excited
Are these electrons in the ground state or excited state?
Ground
Excited
Are these electrons in the ground state or excited state?
Ground
Excited
Are these electrons in the ground state or excited state?
Ground
Excited
Are these electrons in the ground state or excited state?
Ground
Excited
Explain why this atom contains an electron in the excited state:
How many electrons can the first energy level hold?
(a)
How many electrons can the second energy level hold?
(a)
Which energy transition would emit the highest frequency wave:
Which energy transition would emit the lowest frequency wave:
Which energy transition would emit the longest wavelength of light:
Which energy transition would emit the shortest wavelength of light:
Match the following electron transition to the color of light it will produce:
Violet light
Blue-violet light
Blue-green light
Red light
Match the following electron transition to the wavelength of light it will produce:
410 nm
434 nm
486 nm
656 nm
