Chapter 16 Review

Video Review

Key Concept Summary

TA Summary

Vocabulary

Any probability standing wave formed by an electron around a nucleus.

A set of orbitals with similar energies.

Points in the same direction of an electron's magnetic field.

No two electrons can be in the same state (address).

The only orbital with a non-zero probability of the electron being in the nucleus.

An orbital that looks like a dumbbell.

True/False

In the quantum model, the nucleus is very small compared to the region where electrons are likely to be found.

True False

The orbital shape describes the probability of finding an electron at different angles about the nucleus.

True False

Two electrons within the same orbital may have the same spin.

True False

There are four different kinds of p orbitals within a given shell.

True False

In the quantum model of the atom, electrons do not accelerate in their orbits around the nucleus as they do in the Bohr Model.

True False

Orbitals in the higher-numbered shells are smaller than orbitals in the lower-numbered shells.

True False

Electrons in the orbitals in the higher-numbered shells have more energy than electrons in the lower-numbered shells.

True False

The electrons in an atom spin around in the orbitals like a top.

True False

It is possible to predict exactly where an electron will be located once its orbital is determined.

True False

Analysis

Which of the following is experimental evidence that the Bohr model is incorrect? (The quantum model can explain why all of these occur, but the Bohr model doesn't provide an explanation as to why one of these happens.)

Atoms produce discrete emission spectra. Electrons moving in circular paths radiate energy, but electrons around undisturbed atoms do not radiate any energy. Positively charged particles are repelled by the nucleus. Atoms can be broken into charged particles.

Below is a diagram showing the 2s orbital. In this diagram what do the dark areas represent? A depiction of the 2s orbital with a dark area in the center.

A depiction of the 2s orbital with a dark area in the center.

The path a 2s electron follows as it travels around the nucleus. The most probable locations to detect 2s electrons around an atom. An orbit where the 2s electron oscillates up and down an integer number of times as it circles the nucleus. The current location of each electron around the nucleus. More than one of the above.

The picture below is a density diagram showing the 2p orbital. In this diagram what do the dark areas represent? A depiction of the 2p orbital with two dark areas above and below the center.

A depiction of the 2p orbital with two dark areas above and below the center.

The path a 2p electron follows as it travels around the nucleus. The most probable locations to detect 2p electrons around an atom. An orbit where a 2p electron oscillates up and down an integer number of times as it circles the nucleus. The current location of each electron around the nucleus. More than one of the above.

If you draw an energy well for a neutral neon atom, how many electrons does a neon atom have in its 2p orbitals? Refer to the periodic table.

2 4 6 8 10

The Exclusion principle states that

there can only be two electrons in one orbital and the electrons must differ by spin. the better one knows an electron's position, the less one knows about the electron's momentum in an atoms, all electrons must have different spin. the lowest energy orbitals are filled first.

Which of the following orbitals will have the highest energy electrons?

1s 2p 3d 3s

An unexcited atom has its most energetic two electrons in the 3s orbital. How many electrons does it have?

1 (hydrogen) 4 (beryllium) 6 (carbon) 9 (fluorine) 12 (magnesium)

If an electron moves from the 3p to the 2s level in an atom,

a photon will be emitted. a photon must have been absorbed. the electron will be absorbed by the nucleus. the atomic number will go down by one. the atomic number will go up by one.

Which of the following are possible electronic configurations in atoms? (select all correct answers)

(1s³) (1s²)(2s) (1s²)(2s²)(2p⁵) (1s²)(2s²)(2p⁶)(2d²) (1s²)(2s²)(2p⁶)(2s²)(2p⁶)(2d⁸)

Which of the following is the best description of an orbital?

the path the electron travels around the nucleus the volume where there is a 10% chance of finding the electron the volume inside of which there is a 90% chance of detecting the electron an integer number of up and down oscillations that an electron makes around an atom part of an orbit

The Exclusion Principle states that how many electrons may occupy a single orbital?

1 2 3 4

The shape of a "p" orbital most closely resembles that of

a random distribution of dots a wave that goes up and down twice a dumbbell. concentric circles. a cone.

In the modern quantum mechanical model of the atom, which of the following best describes the behavior of electrons?

Electrons are described as standing waves of probability. Electrons orbit around the positive nucleus in a restricted number of fixed energy levels. Electrons are small particles embedded in a positive nucleus. Electrons orbit in elliptical paths according to the electric force law and Newton's laws of motion. Electrons orbit around the nucleus in complicated paths that look like dumbbells and cloverleaves.

Free Response

What problems does the quantum model resolve with the Bohr Model? How does it do so?
According to the quantum model, why are only certain orbitals possible in atoms?
What is the difference between an orbital and an orbit?
What is the probability of finding a p electron inside the nucleus? Why?
Using arrows to represent electrons, complete the electron energy diagrams for the following atoms:
- H (1 electron)
- Li (3 electrons)
- Na (11 electrons)
What similarities do you notice among the patterns of filled orbitals for H, Li, and Na?
Which of the following would you expect to have similar atomic shapes? Why?
- hydrogen (1s) and sodium (1s²2s²2p⁶3s)
- helium (1s²) and boron (1s²2s²2p)
- neon (1s²2s²2p⁶) and argon (1s²2s²2p⁶3s²3p⁶)