Chapter Questions
Objects get their colors from reflecting only certain wavelengths when hit with white light.Light reflected from a green leaf is found to have a wavelength of $4.90 \times 10^{-7} \mathrm{m} .$What is the frequency of the light?
$X$ rays can penetrate body tissues and are widely used to diagnose and treat disordersof internal body structures. What is the frequency of an $X$ ray with a wavelength of$1.15 \times 10^{-10} \mathrm{m}^{2}$
After careful analysis, an electromagnetic wave is found to have a frequency of$7.8 \times 10^{6} \mathrm{H} \mathrm{z}$ What is the speed of the wave?
While an FM radio station broadcasts at a frequency of $94.7 \mathrm{MH} \mathrm{z},$ anAM station broadcasts at a frequency of 820 $\mathrm{kHz}$ . What are the wavelengths of thetwo brodcasts? Which of the drawings below corresponds to the FM station?To the AM station?
Calculate the energy possessed by a single photon of each of the following types ofelectromagnetic radiation.$$6.32 \times 10^{20} \mathrm{s}^{-1} \quad \text { b. } 9.50 \times 10^{13} \mathrm{Hz} \quad \text { c. } 1.05 \times 10^{16} \mathrm{s}^{-1}$$
The blue color in some fireworks occurs when copper(l) chloride is heated toapproximately 1500 $\mathrm{K}$ and emits blue light of wavelength $4.50 \times 10^{2} \mathrm{nm}$ . How muchenergy does one photon of this light carry?
The microwaves used to heat food have a wavelength of 0.125 $\mathrm{m.}$ What is theenergy of one photon of the microwave radiation?
Compare the dual nature of light.
Describe the phenomena that can be explained only by the particle model oflight.
Compare and contrast continuous spectrum and emission spectrum.
Assess Employ quantum theory to assess the amount of energy that matter gains and loses.
Discuss the way in which Einstein utilized Planck's quantum concept to explainthe photoelectric effect.
Heating 235 g of water from $22.6^{\circ} \mathrm{C}$ to $94.4^{\circ} \mathrm{C}$ in a microwave ovenrequires $7.06 \times 10^{4} \mathrm{J}$ of energy. If the microwave frequency is $2.88 \times 10^{10} \mathrm{s}^{-1}$ ,how many quanta are required to supply the $7.06 \times 10^{4} \mathrm{J} ?$
Interpret Scientific Illustrations Use Figure 5.5 and your knowledge ofelectromagnetic radiation to match the numbered items with the lettered items.The numbered items may be used more than once or not at all.$$\begin{array}{ll}{\text { a. longest wavelength }} & {\text { 1. gamma ray }} \\ {\text { b. highest frequency }} & {\text { 2. infrared wave }} \\ {\text { c. greatest energy }} & {\text { 3. radio waves }}\end{array}$$
Explain the reason, according to Bohr's atomic model, why atomic emission spectra contain only certain frequencies of light.
Differentiate between the wavelength of visible light and the wavelengthof a moving soccer ball.
Enumerate the sublevels contained in the hydrogen atom's first four energylevels. What orbitals are related to each s sublevel and each p sublevel?
Explain why the location of an electron in an atom is uncertain using theHeisenberg uncertainty principle and de Broglie's wave-particle duality. How isthe location of electrons in atoms defined?
Calculate Use the information in Table 5.1 to calculate how many times largerthe hydrogen atom's seventh Bohr radius is than its first Bohr radius.
Compare and contrast Bohr's model and the quantum mechanical modelof the atom.
Write ground-state electron configurations for the following elements.a. bromine (Br) C. antimony (Sb) e. terbium (Tb)b. strontium (Sr) d. rhenium (Re) f. titanium (Ti)
A chlorine atom in its ground state has a total of seven electrons in orbitals related to theatom's third energy level. How many of the seven electrons occupy p orbitals? How manyof the 17 electrons in a chlorine atom occupy p orbitals?
When a sulfur atom reacts with other atoms, electrons in orbitals related to the atom'sthird energy level are involved. How many such electrons does a sulfur atom have?
An element has the ground-state electron configuration $[\mathrm{Kr}] 5 \mathrm{s}^{2} 4 \mathrm{d}^{10} 5 \mathrm{p}^{1} .$ It is part of som
Challenge In its ground state, an atom of an element has two electrons in all orbitalsrelated to the atom's highest level for which $n=6 .$ Using noble-gas notation,write the electron configuration for this element, and identify the element.
Draw electron-dot structures for atoms of the following elements.a. magnesium $\quad$ b. thallium $\quad$ c. xenon
An atom of an element has a total of 13 electrons. What is the element, and how manyelectrons are shown in its electron-dot structure?
Challenge An element exists in the gaseous state at room temperature and normalatmospheric pressure and is known to be one of the following: hydrogen, helium,nitrogen, oxygen, fluorine, chlorine, or neon. Identify the element based on the electron dot structure at right.
Apply the Pauli exclusion principle, the aufbau principle, andHund's rule to write out the electron configuration and draw the orbital diagramfor each of the following elements.a. silicon $\quad$ b. fluorine $\quad$ c. calcium $\quad$ d. krypton
Define valence electron.
Illustrate and describe the sequence in which ten electrons occupy the five orbitals related to an atom's d sublevel.
Extend the aufbau sequence through an element that has not yet been identified, but whose atoms would completely fill 7 p orbitals. How many electrons suchan atom would have? Write its electron configuration using noble-gas notationfor the previous noble gas, radon.
Interpret Scientific Illustrations Which is the correct electron-dot structure for an atom of selenium? Explain.
Define the following terms.$$\begin{array}{ll}{\text { a. frequency }} & {\text { c. quantum }} \\ {\text { b. wavelength }} & {\text { d. ground state }}\end{array}$$
Arrange the following types of electromagnetic radiationin order of increasing wavelength.$$\begin{array}{ll}{\text { a. ultraviolet light }} & {\text { c. radio waves }} \\ {\text { b. microwaves }} & {\text { d. } X \text { rays }}\end{array}$$
A gamma ray has a frequency of $2.88 \times 10^{21} \mathrm{Hz}$ . Whatdoes this mean?
What is the photoelectric effect?
Neon Sign How does light emitted from a neon sign differ from sunlight?
Explain Planck's quantum concept as it relates to energylost or gained by matter.
How did Einstein explain the photoelectric effect?
Rainbow What are two differences between the red and green electromagnetic waves in a rainbow?
Temperature What happens to the light emitted by aheated, glowing object as its temperature increases?
What are three deficiencies of the wave model of lightrelated to lights interaction with matter?
How are radio waves and ultraviolet waves similar? How are they different?
Radiation Use Figure 5.20 to determine the followingtypes of radiation.$$\begin{array}{l}{\text { a. radiation with a frequency of } 8.6 \times 10^{11} \mathrm{s}^{-1}} \\ {\text { b. radiation with a wavelength of } 4.2 \mathrm{nm}} \\ {\text { c. radiation with a frequency of } 5.6 \mathrm{MHz}} \\ {\text { d. radiation that travels at a speed of } 3.00 \times 10^{8} \mathrm{m} / \mathrm{s}}\end{array}$$
What is the wavelength of electromagnetic radiation with a frequency of $5.00 \times 10^{12} \mathrm{Hz}$ ? What kind of electromagnetic radiation is this?
What is the frequency of electromagnetic radiationwith a wavelength of $3.33 \times 10^{-8} \mathrm{m}$ ? What type ofelectromagnetic radiation is this?
What is the speed of an electromagnetic wave with afrequency of $1.33 \times 10^{17}$ Hz and a wavelength of 2.25 $\mathrm{nm}$ ?
What is the energy of a photon of red light that has afrequency of $4.48 \times 10^{14} \mathrm{Hz}$ ?
Mercury Mercury's atomic emission spectrum is shownin Figure $5.21 .$ Estimate the wavelength of the orangeline. What is its frequency? What is the energy of a photon corresponding to the orange line emitted by themercury atom?
What is the energy of an ultraviolet photon that has awavelength of $1.18 \times 10^{-8} \mathrm{m} ?$
A photon has an energy of $2.93 \times 10^{-25} \mathrm{J} .$ What is its frequency? What type of electromagnetic radiation isthe photon?
A photon has an energy of $1.10 \times 10^{-13} \mathrm{J.}$ What is thephoton's wavelength? What type of electromagneticradiation is it?
Spacecraft How long does it take a radio signal fromthe Voyager spacecraft to reach Earth if the distancebetween Voyager and Earth is $2.72 \times 10^{9} \mathrm{km}$ ?
Radio Waves If your favorite FM radio stationbroadcasts at a frequency of 104.5 $\mathrm{MHz}$ , what is thewavelength of the station's signal in meters? What isthe energy of a photon of the station's electromagneticsignal?
Platinum What minimum frequency of light is neededto eject a photoelectron from atoms of platinum, whichrequire at least $9.08 \times 10^{-19} \mathrm{J} /$ photon?
Eye Surgery The argon fluoride (ArF) laser used insome refractive eye surgeries emits electromagneticradiation of 193.3 nm wavelength. What is the frequencyof the ArF laser's radiation? What is the energy of a sin-gle quantum of the radiation?
Hydrogen One line in hydrogen's emission spectrumhas a wavelength of 486 $\mathrm{nm}$ . Examine Figure 5.22 todetermine the line's color. What is the line's frequency?
According to the Bohr model, how do electrons movein atoms?
What does $n$ designate in Bohr's atomic model?
What is the difference between an atom's ground stateand an excited state?
What is the name of the atomic model in which electrons are treated as waves? Who first wrote the electron wave equations that led to this model?
What is an atomic orbital?
What does $n$ represent in the quantum mechanical model of the atom?
Electron Transition According to the Bohr model shown in Figure 5.23, what type of electron-orbittransitions produce the ultraviolet lines in hydrogen's Lyman series?
How many energy sublevels are contained in each of the hydrogen atom's first three energy levels?
What atomic orbitals are related to a d sublevel?
What do the sublevel designations s, p, d, and f specifywith respect to the atoms orbitals?
How are the five orbitals related to an atom's d subleveldesignated?
What is the maximum number of electrons an orbital can contain?
What is the maximum number of electrons an orbitalcan contain?
How many electrons can be contained in all the orbitalsrelated to an argon atom's third energy level?
How does the quantum mechanical model of the atomdescribe the paths of an atom's electrons?
Macroscopic Objects Why do we not notice the wave-lengths of moving objects such as auto mobiles?
Why is it impossible to know precisely the velocity andposition of an electron at the same time?
In what sequence do electrons fill the atomic orbitalsrelated to a sublevel?
Rubidium Using Figure 5.24 explain why one electronin a rubidium atom occupies a 5 s orbital rather than a4d or 4f orbital.
What are valence electrons? How many of a magnesiumatom's 12 electrons are valence electrons?
Light is said to have a dual wave-particle nature. Whatdoes this statement mean?
Describe the difference between a quantum anda photon.
How many electrons are shown in each element's electron-dot structure?$$\begin{array}{ll}{\text { a. carbon }} & {\text { c. calcium }} \\ {\text { b. iodine }} & {\text { d. gallium }}\end{array}$$
When writing the electron configuration notation for anatom, 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.$$\begin{array}{ll}{\text { a. beryllium }} & {\text { c. nitrogen }} \\ {\text { b. aluminum }} & {\text { d. sodium }}\end{array}$$
Use noble-gas notation to describe the electron configurations of the elements represented by thefollowing symbols.$$\begin{array}{ll}{\text { a. } \mathrm{Kr}} & {\text { c. Zr }} \\ {\text { b. } \mathrm{P}} & {\text { d. Pb }}\end{array}$$
What element is represented by each electron configuration?$$\begin{array}{l}{\text { a. } 1 \mathrm{s}^{2} 2 \mathrm{s}^{2} 2 \mathrm{p}^{5}} \\ {\text { b. }[\mathrm{Ar}] 4 \mathrm{s}^{2}} \\ {\text { c. }[\mathrm{Xe}] 6 \mathrm{s}^{2} \mathrm{4f}^{4}} \\ {\text { d. }[\mathrm{Kr}] 5 \mathrm{s}^{2} 4 \mathrm{d}^{10} \mathrm{5p}^{4}} \\ {\text { e. }[\mathrm{Rn}] 7 \mathrm{s}^{2} 5 \mathrm{f}^{13}} \\ {\text { f. } 1 \mathrm{s}^{2} 2 \mathrm{s}^{2} 2 \mathrm{p}^{6} 3 \mathrm{s}^{2} 3 \mathrm{p}^{6} 4 \mathrm{s}^{2} 3 \mathrm{d}^{10} 4 \mathrm{p}^{5}}\end{array}$$
Which electron configuration notation describes anatom in an excited state?$$\begin{array}{l}{\text { a. }[\mathrm{Ar}] 4 \mathrm{s}^{2} 3 \mathrm{d}^{10} \mathrm{4p}^{2}} \\ {\text { b. }[\mathrm{Ne}] 3 \mathrm{s}^{2} 3 \mathrm{p}^{5}} \\ {\text { c. }[\mathrm{Kr}] 5 \mathrm{s}^{2} 4 \mathrm{d}^{1}} \\ {\text { d. }[\mathrm{Ar}] 4 \mathrm{s}^{2} 3 \mathrm{d}^{8} 4 \mathrm{p}^{1}}\end{array}$$
Which orbital diagram in Figure 5.25 is correct for an atom in its ground state?
Draw an electron-dot structure for an atom of each element.$$\begin{array}{l}{\text { a. carbon }} \\ {\text { b. arsenic }} \\ {\text { c. polonium }} \\ {\text { d. potassium }} \\ {\text { e. barium }}\end{array}$$
Arsenic An atom of arsenic has how many electron containing orbitals? How many of the orbitals are completely filled? How many of the orbitals are associatedwith the atom's $n=4$ principal energy level?
Which element could have the ground-stateelectron-dot notation shown in Figure 5.26$?$$$\begin{array}{ll}{\text { a. manganese }} & {\text { c. calcium }} \\ {\text { b. antimony }} & {\text { d. samarium }}\end{array}$$
For an atom of tin in the ground state, write the electronconfiguration using noble-gas notation, and draw itselectron-dot structure.
What is the maximum number of electrons that can becontained in an atom's orbitals having the followingprincipal quantum numbers?$$\begin{array}{ll}{\text { a. } 3} & {\text { c. } 6} \\ {\text { b. } 4} & {\text { d. } 7}\end{array}$$
What is the wavelength of light with a frequency of$5.77 \times 10^{14} \mathrm{Hz} ?$
Waves Using the waves shown in Figure $5.27,$ identifythe wave or waves with the following characteristics.$$\begin{array}{l}{\text { a. longest wavelength }} \\ {\text { b. greatest frequency }} \\ {\text { c. largest amplitude }} \\ {\text { d. shortest wavelength }}\end{array}$$
How many orientations are possible for the orbitalsrelated to each sublevels?$$\begin{array}{ll}{\text { a. } \mathrm{s}} & {\text { c. d }} \\ {\text { b. } \mathrm{p}} & {\text { d. } \mathrm{f}}\end{array}$$
Which elements have only two electrons in their electron-dot structures: hydrogen, helium, lithium, aluminum,calcium, cobalt, bromine, krypton, or barium?
In Bohr's atomic model, what electron-orbit transitionproduces the blue-green line in hydrogen's atomic emission spectrum?
Zinc A zinc atom contains a total of 18 electrons in its$3 \mathrm{s}, 3 \mathrm{p},$ and 3 $\mathrm{d}$ orbitals. Why does its electron-dot structure show only two dots?
X Ray An X-ray photon has an energy of $3.01 \times 10^{-18} \mathrm{J} .$What is its freguency 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 infraredradiation with a fre-quency of $4.88 \times 10^{13}$ Hz arerequired 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 wave-length of light change as it travels from air to water?
According to the quantum mechanical model of theatom, what happens when an atom absorbs a quantumof energy?
Compare and Contrast Briefly discuss the differencebetween an orbit in Bohr's model of the atom and anorbital in the quantum mechanical view of the atom.
Calculate It takes $8.17 \times 10^{-19} \mathrm{J}$ of energy to removeone electron from a gold surface. What is the maximumwavelength of light capable of causing this effect?
Infer Suppose that you live in a universe in whichthe Pauli exclusion principle states that a maximumof three, rather than two, electrons can occupy a singleatomic orbital. Evaluate and explain the new chemicalproperties of the elements lithium and phosphorus.
Hydrogen Atom The hydrogen atom's energy is$-6.05 \times 10^{-20} \mathrm{J}$ when the electron is in the $n=6$ orbitand $-2.18 \times 10^{-18} \mathrm{J}$ when the electron is in the $n=1$Calculate the wavelength of the photon emitted whenthe electron drops from the $n=6$ orbit to the $n=1$orbit. Use the following values: $h=6.626 \times 10^{-34} \mathrm{Jes}$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 chemicalproperty 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 anda mass number of $153 .$ How many electrons, protons,and neutrons does it contain? (Chapter 4$)$
Neon Signs To make neon signs emit different col-ors, manufacturers often fill the signs with gases otherthan neon. Write an essay about the use of gases inneon signs and the colors produced by the gases.
Rutherford's Model Imagine that you are a scientistin the early twentieth century, and you have justlearned the details of a new, nuclear model of the atomproposed by the prominent English physicist ErnestRutherford. After analyzing the model, you discernwhat you believe to be important limitations. Write aletter to Rutherford in which you express your concerns regarding his model. Use diagrams and examplesof specific elements to help you make your point.
Differentiate between the two spectra shown above.
Sodium's two bright lines have wavelengths of588.9590 $\mathrm{nm}$ and 589.9524 $\mathrm{nm} .$ What is the ground-state electron configuration notation for sodium, andhow does sodium's electron configuration relate tothe lines?
Calculate the energies of photons related to thetwo lines using the relationships expressed in thefollowing equations.$$E_{\mathrm{photon}}=h v ; c=\lambda v ; E=h c / \lambda$$