Chapter 5

What do the sublevel designations s, p, d, and f specify with respect to the atom’s orbitals?

How are the five orbitals related to an atom’s d sublevel designated?

What is the maximum number of electrons an orbital can contain?

Describe the relative orientations of the orbitals related to an atom’s 2p sublevel.

How many electrons can be contained in all the orbitals related to an argon atom’s third energy level?

How does the quantum mechanical model of the atom describe the paths of an atom’s electrons?

Macroscopic Objects Why do we not notice the wavelengths of moving objects such as automobiles?

Why is it impossible to know precisely the velocity and position of an electron at the same time?

In what sequence do electrons fill the atomic orbitals related to a sublevel?

What are valence electrons? How many of a magnesium atom’s 12 electrons are valence electrons?

Light is said to have a dual wave-particle nature. What does this statement mean?

Describe the difference between a quantum and a photon.

When writing the electron configuration notation for an atom, what three principles or rules should you follow?

Write the electron configuration and draw the orbital notation for atoms of oxygen and sulfur.

List the aufbau sequence of orbitals from 1s to 7p.

Write each element’s orbital notation and complete electron configuration. a. beryllium c. nitrogen b. aluminum d. sodium

Use noble-gas notation to describe the electron configurations of the elements represented by the following symbols. a. Kr c. Zr b. P d. Pb

What element is represented by each electron configuration? a. 1 \(\mathrm{s}^{2} 2 \mathrm{s}^{2} 2 \mathrm{p}^{5}\) b. \([\mathrm{Ar}] 4 \mathrm{s}^{2}\) c. \([\mathrm{Xe}] 6 \mathrm{s}^{2} 4 \mathrm{f}^{4}\) d. \([\mathrm{Kr}] 5 \mathrm{s}^{2} 4 \mathrm{d}^{10} 5 \mathrm{p}^{4}\) e. \([\mathrm{Rn}] 7 \mathrm{s}^{2} 5 \mathrm{f}^{13}\) f. 1 \(\mathrm{s}^{2} 2 \mathrm{s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{s}^{2} 3 \mathrm{p}^{6} 4 \mathrm{s}^{2} 3 \mathrm{d}^{10} 4 \mathrm{p}^{5}\)

Which electron configuration notation describes an atom in an excited state? a. \([\mathrm{Ar}] 4 \mathrm{s}^{2} 3 \mathrm{d}^{10} 4 \mathrm{p}^{2}\) b. \([\mathrm{Ne}] 3 \mathrm{s}^{2} 3 \mathrm{p}^{5}\) c. \([\mathrm{Kr}] 5 s^{2} 4 \mathrm{d}^{1}\) d. \([\mathrm{Ar}] 4 \mathrm{s}^{2} 3 \mathrm{d}^{8} 4 \mathrm{p}^{1}\)

Draw an electron-dot structure for an atom of each element. a. carbon b. arsenic c. polonium d. potassium e. barium

Arsenic An atom of arsenic has how many electroncontaining orbitals? How many of the orbitals are completely filled? How many of the orbitals are associated with the atom’s n = 4 principal energy level?

For an atom of tin in the ground state, write the electron configuration using noble-gas notation, and draw its electron-dot structure.

What is the maximum number of electrons that can be contained in an atom’s orbitals having the following principal quantum numbers? a. 3 c. 6 b. 4 d. 7

What is the wavelength of light with a frequency of \(5.77 \times 10^{14} \mathrm{Hz}\) ?

How many orientations are possible for the orbitals related to each sublevels? a. s c. d b. p d. f

Which elements have only two electrons in their electrondot structures: hydrogen, helium, lithium, aluminum, calcium, cobalt, bromine, krypton, or barium?

In Bohr’s atomic model, what electron-orbit transition produces the blue-green line in hydrogen’s atomic emission spectrum?

Zinc A zinc atom contains a total of 18 electrons in its 3s, 3p, and 3d orbitals. Why does its electron-dot structure show only two dots?

XRay An X-ray photon has an energy of 3.01 \(\times 10^{-18} \mathrm{J}\) . What is its frequency and wavelength?

Which element has the ground-state electron configuration represented by the noble-gas notation \([\mathrm{Rn}] 7 \mathrm{s}^{1} ?\)

How did Bohr explain atomic emission spectra?

Infrared Radiation How many photons of infrared radiation with a fre-quency of \(4.88 \times 10^{13} \mathrm{Hz}\) are required to provide an energy of 1.00 \(\mathrm{J} ?\)

Light travels slower in water than it does in air; however, its frequency remains the same. How does the wavelength of light change as it travels from air to water?

According to the quantum mechanical model of the atom, what happens when an atom absorbs a quantum of energy?

Compare and Contrast Briefly discuss the difference between an orbit in Bohr’s model of the atom and an orbital in the quantum mechanical view of the atom.

Calculate It takes \(8.17 \times 10^{-19} \mathrm{J}\) of energy to remove one electron from a gold surface. What is the maximum wavelength of light capable of causing this effect?

Hydrogen Atom The hydrogen atom's energy is \(-6.05 \times 10^{-20} \mathrm{J}\) when the electron is in the \(n=6\) orbit and \(-2.18 \times 10^{-18} \mathrm{J}\) when the electron is in the \(n=1\) Calculate the wavelength of the photon emitted when the electron drops from the \(n=6\) orbit to the \(n=1\) orbit. Use the following values: \(h=6.626 \times 10^{-34} \mathrm{J} \bullet \mathrm{s}\) and \(c=3.00 \times 10^{8} \mathrm{m} / \mathrm{s}\)

Round 20.56120 \(\mathrm{g}\) to three significant figures. (Chapter 2\()\)

Identify whether each statement describes a chemical property or a physical property. (Chapter 3) a. Mercury is a liquid at room temperature. b. Sucrose is a white, crystalline solid. c. Iron rusts when exposed to moist air. d. Paper burns when ignited.

An atom of gadolinium has an atomic number of 64 and a mass number of 153. How many electrons, protons, and neutrons does it contain? (Chapter 4)

Neon Signs To make neon signs emit different colors, manufacturers often fill the signs with gases other than neon. Write an essay about the use of gases in neon signs and the colors produced by the gases.

Calculate the energies of photons related to the two lines using the relationships expressed in the following equations. \(E_{\text { photon }}=h v ; c=\lambda v ; E=h c / \lambda\)