HC ions periodicity electrons

Calculate the frequency of the yellow light emitted by a street light, if its wavelength is 588nm.

c=λν ; c=3.00×10⁸m/s; E=hν; h=6.626×10⁻³⁴J⋅s

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NGSS.HS-PS4-1

Calculate the energy of light that has a wavelength of 220 nm

Note: c=λν ; c=3.00×10⁸m/s; E=hν; h=6.626×10⁻³⁴J⋅s

• 1.4 x 10 ¹⁵ J

• 9.0 x 10 ^-19 J

• 3.1 x 10 ^-19 J

• 1.4 x 10 ^-19 J

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NGSS.HS-PS4-1

Solve this problems using the equation: 
C = λν
If an AM radio station broadcasts at
9.95 x 10⁵ s^-1, what is the wavelength of this radiation?

• 6.59 x 10^-28 m
• 1.01 x 10^-6 m
• 3.32 x 10^-3 m
• 302 m

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NGSS.HS-PS4-1

An argon ion laser emits light at 488 nm. What is the frequency of this radiation? Note: Hz = 1/s and c=λν. and c=3.00×10⁸m/s

• 4.07 x 10^-19 Hz

• 6.15 x 10¹⁴ Hz
• 1.46 x 10² Hz
• 2.05 x 10⁶ Hz

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NGSS.HS-PS4-1

A common infrared laser operates at 1.06 x 10³ nm. What if the energy of a photon with this wavelength?

c=λν ; c=3.00×10⁸m/s; E=hν; h=6.626×10⁻³⁴J⋅s

• 7.02 x 10^-40 J
• 6.25 x 10^-28 J
• 3.54 x 10^-15 J
• 1.87 x 10^-19 J

Tags

NGSS.HS-PS4-1

NGSS.HS-PS4-3

Look carefully at the waves.  Which carries the most energy?

• microwave
• infrared
• ultraviolet
• x-ray

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NGSS.HS-PS4-1

NGSS.HS-PS4-3

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

Which of the following elements make up the unknown sample?

• A and B

• B and C

• C and D

Tags

NGSS.HS-PS1-1

Which of the following electron jumps would be responsible for the MOST energetic light emitted?

• 5th to the 2nd energy level

• 3rd to the 2nd energy level

When an electron moves from a LOWER energy level to a HIGHER energy level:

• Energy is absorbed as it moves to the excited state

• Energy is released as it moves to the excited state

• Energy is absorbed as it moves to the ground state

• Energy is released as it moves to the ground state