What element is represented by each electron

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 1 0 -7 m. What is the frequency of the light?

X rays can penetrate body tissues and are widely used to diagnose and treat disorders of internal body structures. What is the frequency of an X ray with a wavelength of 1.15 1 0 -10 m?

After careful analysis, an electromagnetic wave is found to have a frequency of 7.8 1 0 6 Hz. What is the speed of the wave?

Challenge While an FM radio station broadcasts at a frequency of 94.7 MHz, an AM station broadcasts at a frequency of 820 kHz. What are the wavelengths of the two broadcasts? Which of the drawings below corresponds to the FM station? To the AM station? a b

Calculate the energy possessed by a single photon of each of the following types of electromagnetic radiation. a. 6.32 1 0 20 s 1 b. 9.50 1 0 13 Hz c. 1.05 1 0 16 s 1

The blue color in some fireworks occurs when copper(I) chloride is heated to approximately 1500 K and emits blue light of wavelength 4.50 1 0 2 nm. How much energy does one photon of this light carry?

Challenge The microwaves used to heat food have a wavelength of 0.125 m. What is the energy 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 of light.

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 Plancks quantum concept to explain the photoelectric effect.

Calculate Heating 235 g of water from 22.6C to 94.4C in a microwave oven requires 7.06 1 0 4 J of energy. If the microwave frequency is 2.88 1 0 10 s -1 , how many quanta are required to supply the 7.06 1 0 4 J?

Interpret Scientific Illustrations Use Figure 5.5 and your knowledge of electromagnetic radiation to match the numbered items with the lettered items. The numbered items may be used more than once or not at all. a. longest wavelength 1. gamma ray b. highest frequency 2. infrared wave c. greatest energy 3. radio waves

Explain the reason, according to Bohrs atomic model, why atomic emission spectra contain only certain frequencies of light

Differentiate between the wavelength of visible light and the wavelength of a moving soccer ball.

Enumerate the sublevels contained in the hydrogen atoms first four energy levels. 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 the Heisenberg uncertainty principle and de Broglies wave-particle duality. How is the location of electrons in atoms defined?

Calculate Use the information in Table 5.1 to calculate how many times larger the hydrogen atoms seventh Bohr radius is than its first Bohr radius.

Compare and contrast Bohrs model and the quantum mechanical model of 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 the atoms third energy level. How many of the seven electrons occupy p orbitals? How many of the 17 electrons in a chlorine atom occupy p orbitals?

When a sulfur atom reacts with other atoms, electrons in orbitals related to the atoms third energy level are involved. How many such electrons does a sulfur atom have?

An element has the ground-state electron configuration [Kr]5 s 24 d 105 p 1. It is part of some semiconductors and used in various alloys. What element is it?

Challenge In its ground state, an atom of an element has two electrons in all orbitals related to the atoms highest energy 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 b. thallium c. xenon

An atom of an element has a total of 13 electrons. What is the element, and how many electrons are shown in its electron-dot structure?

Challenge An element exists in the gaseous state at room temperature and normal atmospheric pressure and is known to be one of the following: hydrogen, helium, nitrogen, oxygen, fluorine, chlorine, or neon. Identify the element based on the electrondot structure at right

Apply the Pauli exclusion principle, the aufbau principle, and Hunds rule to write out the electron configuration and draw the orbital diagram for each of the following elements. a. silicon b. fluorine c. calcium d. krypton

Define valence electron.

Illustrate and describe the sequence in which ten electrons occupy the five orbitals related to an atoms d sublevel.

Extend the aufbau sequence through an element that has not yet been identified, but whose atoms would completely fill 7p orbitals. How many electrons such an atom would have? Write its electron configuration using noble-gas notation for the previous noble gas, radon.

Interpret Scientific Illustrations Which is the correct electron-dot structure for an atom of selenium? Explain. a. b. c. Se Se Se d. S

Define the following terms. a. frequency c. quantum b. wavelength d. ground state

Arrange the following types of electromagnetic radiation in order of increasing wavelength. a. ultraviolet light c. radio waves b. microwaves d. X rays

A gamma ray has a frequency of 2.88 1 0 21 Hz. What does this mean?

What is the photoelectric effect?

Neon Sign How does light emitted from a neon sign differ from sunlight?

Explain Plancks quantum concept as it relates to energy lost 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 a heated, glowing object as its temperature increases?

What are three deficiencies of the wave model of light related 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 following types of radiation. a. radiation with a frequency of 8.6 1 0 11 s -1 b. radiation with a wavelength of 4.2 nm c. radiation with a frequency of 5.6 MHz d. radiation that travels at a speed of 3.00 1 0 8 m/s

What is the wavelength of electromagnetic radiation with a frequency of 5.00 1 0 12 Hz? What kind of electromagnetic radiation is this?

What is the frequency of electromagnetic radiation with a wavelength of 3.33 1 0 -8 m? What type of electromagnetic radiation is this?

What is the speed of an electromagnetic wave with a frequency of 1.33 1 0 17 Hz and a wavelength of 2.25 nm?

What is the energy of a photon of red light that has a frequency of 4.48 1 0 14 Hz? Hg (nm) 400 450 500 550 600 650 700 Figure 5.21

Mercury Mercurys atomic emission spectrum is shown in Figure 5.21. Estimate the wavelength of the orange line. What is its frequency? What is the energy of a photon corresponding to the orange line emitted by the mercury atom?

What is the energy of an ultraviolet photon that has a wavelength of 1.18 1 0 -8 m?

A photon has an energy of 2.93 1 0 -25 J. What is its frequency? What type of electromagnetic radiation is the photon?

A photon has an energy of 1.10 1 0 -13 J. What is the photons wavelength? What type of electromagnetic radiation is it?

Spacecraft How long does it take a radio signal from the Voyager spacecraft to reach Earth if the distance between Voyager and Earth is 2.72 1 0 9 km?

Radio Waves If your favorite FM radio station broadcasts at a frequency of 104.5 MHz, what is the wavelength of the stations signal in meters? What is the energy of a photon of the stations electromagnetic signal?

Platinum What minimum frequency of light is needed to eject a photoelectron from atoms of platinum, which require at least 9.08 1 0 -19 J/photon?

Eye Surgery The argon fluoride (ArF) laser used in some refractive eye surgeries emits electromagnetic radiation of 193.3 nm wavelength. What is the frequency of the ArF lasers radiation? What is the energy of a single quantum of the radiation? (nm) 400 434 nm 486 nm 656 nm 410 nm 450 500 550 Hydrogens Atomic Emission Spectrum 600 650 700 750 Figure 5.22

Hydrogen One line in hydrogens emission spectrum has a wavelength of 486 nm. Examine Figure 5.22 to determine the lines color. What is the lines frequency?

According to the Bohr model, how do electrons move in atoms?

What does n designate in Bohrs atomic model?

What is the difference between an atoms ground state and 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? Ultraviolet series (Lyman) Visible series (Balmer) Infrared series (Paschen) n = 4 n = 5 n = 6 n = 7 n = 3 n = 1 + n = 2 Figure 5.23

Electron Transition According to the Bohr model shown in Figure 5.23, what type of electron-orbit transitions produce the ultraviolet lines in hydrogens Lyman series?

How many energy sublevels are contained in each of the hydrogen atoms first three energy levels?

What atomic orbitals are related to a d sublevel?

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

How are the five orbitals related to an atoms d sublevel designated?

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

Describe the relative orientations of the orbitals related to an atoms 2p sublevel.

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

How does the quantum mechanical model of the atom describe the paths of an atoms 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? 3d 5d 6d 4d 5f 4f 2p 4p 3p 6p 7p 5p 4s 3s 6s 7s 5s 2s Orbital filling sequence Increasing energy 1s Figure 5.24

Rubidium Using Figure 5.24, explain why one electron in a rubidium atom occupies a 5s orbital rather than a 4d or 4f orbital

What are valence electrons? How many of a magnesium atoms 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

How many electrons are shown in each elements electron-dot structure? a. carbon c. calcium b. iodine d. gallium

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 elements 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 s 2 2 s 2 2 p 5 b. [Ar]4 s 2 c. [Xe]6 s 2 4 f 4 d. [Kr]5 s 2 4 d 10 5 p 4 e. [Rn]7 s 2 5 f 13 f. 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 5

Which electron configuration notation describes an atom in an excited state? a. [Ar]4 s 2 3 d 10 4 p 2 b. [Ne]3 s 2 3 p 5 c. [Kr]5 s 2 4 d 1 d. [Ar]4 s 2 3 d 8 4 p 1 3s 3p 4s 3d 3d 3s 3p 4s 3d 3s 3p 4s 3d 3s 3p 4s Figure 5.25

Which orbital diagram in Figure 5.25 is incorrect for an atom in its ground state?

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 atoms n = 4 principal energy level? X Figure 5.26

Which element could have the ground-state electron-dot notation shown in Figure 5.26? a. manganese c. calcium b. antimony d. samarium

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 atoms 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 10 14 Hz? 1. 3. 2. 4. Figure 5.27

Waves Using the waves shown in Figure 5.27, identify the wave or waves with the following characteristics. a. longest wavelength b. greatest frequency c. largest amplitude d. shortest wavelength

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 Bohrs atomic model, what electron-orbit transition produces the blue-green line in hydrogens 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?

X Ray An X-ray photon has an energy of 3.01 1 0 -18 J. What is its frequency and wavelength?

Which element has the ground-state electron configuration represented by the noble-gas notation [Rn]7 s 1 ?

How did Bohr explain atomic emission spectra?

Infrared Radiation How many photons of infrared radiation with a fre-quency of 4.88 1 0 13 Hz are required to provide an energy of 1.00 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 Bohrs model of the atom and an orbital in the quantum mechanical view of the atom.

Calculate It takes 8.17 1 0 -19 J of energy to remove one electron from a gold surface. What is the maximum wavelength of light capable of causing this effect? z x y 1s orbital py p orbital z x y z x y dxz d orbital Figure 5.28

Describe the shapes of the atomic orbitals shown in Figure 5.28. Specify their orientations and relate each orbital to a particular type of energy sublevel.

Infer Suppose that you live in a universe in which the Pauli exclusion principle states that a maximum of three, rather than two, electrons can occupy a single atomic orbital. Evaluate and explain the new chemical properties of the elements lithium and phosphorus.

Hydrogen Atom The hydrogen atoms energy is -6.05 1 0 20 J when the electron is in the n = 6 orbit and -2.18 1 0 18 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 1 0 34 Js and c = 3.00 1 0 8 m/s

Round 20.56120 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.

Rutherfords Model Imagine that you are a scientist in the early twentieth century, and you have just learned the details of a new, nuclear model of the atom proposed by the prominent English physicist Ernest Rutherford. After analyzing the model, you discern what you believe to be important limitations. Write a letter to Rutherford in which you express your concerns regarding his model. Use diagrams and examples of specific elements to help you make your point.

Differentiate between the two spectra shown above.

Sodiums two bright lines have wavelengths of 588.9590 nm and 589.9524 nm. What is the groundstate electron configuration notation for sodium, and how does sodiums electron configuration relate to the lines?

Calculate the energies of photons related to the two lines using the relationships expressed in the following equations. Ephoton = hv; c = v; E = hc/