The number of sublevels within each energy level of an atom is equal to the value of the

angular momentum quantum number.

All of the following describe the Schrödinger wave equation except

C. it is similar to Bohr's theory.

A. it helped lay the foundation for the modern quantum theory.

B. it is an equation that treats electrons in atoms as waves.

D. only waves of specific energies and frequencies provide solutions to the equation.

If electromagnetic radiation A has a lower frequency than electromagnetic radiation B, then compared to B, the wavelength of A is

exactly half the length of B's wavelength.

The Aufbau principle states that an electron

occupies the lowest available energy level.

must be paired with another electron.

The quantum number that indicates the position of an orbital about the three axes in space is the

angular momentum quantum number.

The angular momentum quantum number indicates the

A. main energy level of an orbital.

C. orientation of an orbital around the nucleus.

D. direction of the spin of the electron in its orbital.

According to the particle model of light, certain kinds of light cannot eject electrons from metals because

the energy of the light is too low.

the frequency of the light is too high.

the wavelength of the light is too short.

the mass of the light is too low.

For an electron in an atom to change from the ground state to an excited state,

the electron must make a transition from a higher to a lower energy level.

All of the following describe the Heisenberg uncertainty principle except

A) it helps to locate an electron in an atom.

B) it states that it is impossible to determine simultaneously both the position and velocity of an electron or any other particle.

C) it helped lay the foundation for the modern quantum theory.

D) it is one of the fundamental principles of our present understanding of light and matter.

The product of the frequency and the wavelength of a wave equals the

time for one full wave to pass.

number of waves passing a point in a second.

A line spectrum is produced when an electron moves from one energy level

to another position in the same sublevel.

Bohr's theory helped explain why

excited hydrogen gas gives off certain colors of light.

electrons have negative charge.

atoms combine to form molecules.

most of the mass of the atom is in the nucleus.

Because excited hydrogen atoms always produce the same line-emission spectrum, scientists concluded that hydrogen:

A) released photons of only certain energies.

D) could only exist in the ground state.

A spherical electron cloud surrounding an atomic nucleus would best represent:

a combination of an s and a p_x orbital.

a combination of p_x and p_y orbitals.

Both the Heisenberg uncertainty principle and the Schrödinger wave equation

led to locating an electron in an atom.

led to the concept of atomic orbitals.

The French scientist Louis de Broglie theorized that

electrons could have a dual wave-particle nature.

light waves did not have a dual wave-particle nature.

Bohr's model of the hydrogen atom was completely correct.

the natures of light and quantized electron orbits were not similar.

The spin quantum number of an electron can be thought of as describing

the direction of electron spin.

whether the electron's charge is positive or negative.

the electron's exact location in orbit.

the number of revolutions the electron makes about the nucleus per second.

How many electrons can occupy the s orbitals at each energy level?

two, if they have opposite spins

two, if they have the same spin

Electron Configuration Review Quiz

56 questions

Show all answers

1.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The element with electron configuration 1s² 2s² 2p⁶ 3s² 3p² is:

Si (Z = 14)

Mg (Z = 12)

C (Z = 6)

S (Z = 16)

Tags

NGSS.HS-PS1-1

2.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The specific wavelengths of light seen through a prism that are made when high-voltage current is passed through a tube of hydrogen gas at low pressure is a:

electron configuration.

continuous electromagnetic spectrum.

photoelectric effect.

line-emission spectrum.

3.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

The energy of a photon is related to its

frequency.

speed.

size.

mass.

Tags

NGSS.HS-PS4-1

4.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

For the f sublevel, the number of orbitals is

A. 5.

B. 18.

C. 9.

D. 7.

5.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the wavelength of microwaves of 3.0 × 10^9 Hz frequency?

0.050 m

0.060 m

0.20 m

0.10 m

Tags

NGSS.HS-PS4-1

6.

DRAG AND DROP QUESTION

30 sec • 1 pt

An electron for which n = 4 has more (a) than an electron for which n = 2.

particle nature

wave nature

spin

energy

7.

MULTIPLE CHOICE QUESTION

30 sec • 1 pt

What is the frequency of a photon with an energy of 1.99 × 10^-19 J? (h = 6.63 × 10^-34 J·s)

4.00 × 10^14 Hz

1.00 × 10^14 Hz

3.00 × 10^14 Hz

2.00 × 10^14 Hz

Tags

NGSS.HS-PS4-1

NGSS.HS-PS4-3

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Electron Configuration Review

The element with electron configuration 1s² 2s² 2p⁶ 3s² 3p² is:

The specific wavelengths of light seen through a prism that are made when high-voltage current is passed through a tube of hydrogen gas at low pressure is a:

The energy of a photon is related to its

For the f sublevel, the number of orbitals is

What is the wavelength of microwaves of 3.0 × 10^9 Hz frequency?

An electron for which n = 4 has more (a) than an electron for which n = 2.

What is the frequency of a photon with an energy of 1.99 × 10^-19 J? (h = 6.63 × 10^-34 J·s)

The number of sublevels within each energy level of an atom is equal to the value of the

What is the frequency of infrared light of 1.0 × 10⁻⁴ m wavelength?

The main energy levels of an atom are indicated by the

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