# Electrons And Energy: Question Preview (ID: 5751)

### Below is a preview of the questions contained within the game titled ELECTRONS AND ENERGY: Calculations With Wavelength, Frequency, And Energy .To play games using this data set, follow the directions below. Good luck and have fun. Enjoy! [print these questions]

To calculate the frequency of an electromagnetic wave, you need to know the speed of the wave and its:
a) wavelength
b) intensity
c) amplitude
d) energy

What is the frequency of a light wave with a wavelength of 680 nm (6.8 e - 7 m)
a) 2.04 e 9 Hz
b) 2.04 s
c) 2.27 e - 15 Hz
d) 4.41 e 14 Hz

An electromagnetic wave in a vacuum has a wavelength of 0.07m. What is its frequency?
a) 3.0 e 8 m/s
b) 4.3 e 9 Hz
c) 3.0 e 9 Hz
d) 4.3 e 8 m/s

Use Plank's constant to solve the following. What is the amount of energy carried by a photon that has a frequency of 5.71 e 14 Hz.
a) 525 nm
b) 3.78 e -19 J
c) 1.16 e -8 J
d) 8.62 e 47 J

Infrared rays have a shorter wavelength than
a) ultraviolet rays
b) gamma rays
c) x rays

A photon is emitted from an atom with an energy of 4.25 e -19 J. What is the wavelength of the photon?
a) 4.69 e -7 m
b) 1.28 e -10 m
c) 2.73 e -4 m
d) 6.42 e 14 m

For an electron in an atom to change from the ground state to an excited state,
a) energy must be released
b) energy must be gained
d) the electron must move from a higher to a lower energy level

A student records the following electron configuration for the element Arsenic: 1s2 2s2 2p6 3s2 3p6 4s2 4d10 4p3. Is this correct? Why or why not?
a) It is a correct electron configuration.
b) It is not correct because there are too many electrons
c) It is not correct because there are not enough electrons
d) It is not correct because the 4d should be 3d

The statement that no two electrons in the same atom can have the same four quantum numbers is a restatement of:
a) Bohr's Law
b) Hund's Rule
c) Aufbau Principle
d) Pauli Exclusion Principle

Oxygen has an electron configuration of 1s2 2s2 2p4, how many unpaired electrons does oxygen have?
a) 1
b) 2
c) 3
d) 4

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