Test Review Sheet

Sample Problems:

1. The types of electromagnetic radiation listed below are in order of increasing energy.

Type of radiation (in order of increasing energy)

long radio waves

FM radio waves

microwaves

infrared light

visible light

X-rays

Frequency

Wavelength

Complete the table by matching the frequencies and wavelengths from the list below with the appropriate type of radiation. You should not need a diagram of the electromagnetic spectrum to do this.

Frequencies: 1010 s-1 1013 s-1 108 s-1 101 s-1 1018 s-1 1015 s-1

Wavelengths: 10-7 m 10-10 m 108 m 101 m 10-4 m 10-2 m

2. Violet light has a wavelength of about 410 nm. What is its frequency?

What is the energy of one photon of this light?

What is the energy of one mole of violet light photons?

3. Use the following table to answer the question below.

Ultraviolet

10 nm – 400 nm

Blue-green light

400 nm – 550 nm

Red-orange light

550 nm – 700 nm

Short wave Infrared

700 nm – 2000 nm

The reaction of hydrogen gas with chlorine gas to form hydrogen chloride can be initiated with electromagnetic radiation. The radiation must have a minimum energy of 9.91x10-19 J/photon in order to initiate the reaction. A student suggests shining a blue-green laser through the gases as a method to initiate the reaction. Do you agree or disagree? Justify your response.

4. How many subshells (types of orbitals) exist in the n=5 principal energy level?

5. How many f orbitals are there in the n=4 principal energy level?

6. Use correct orbital box notation to write the electron configuration for phosphorus.

7. Use spdf (unabbreviated) notation to write the electron configuration for Silver.

8. Use noble gas (abbreviated) notation to write the electron configuration for tungsten.

9. The rare earth elements (lanthanides) usually attain a 3+ charge. Write an electron configuration for the Ce+3 ion. The electron configuration for a Ce atom has been provided below.

Ce: [Xe]4f15d16p2

10. Rank the following in order of increasing atomic size: Rb and Sr. Explain your choice.

11. Rank the following in order of increasing ionization energy: Br and Cl. Explain your choice.

12. Rank the following in order of increasing size: Cl, Cl- and O. Explain your choice.

13. Which atom has the highest affinity for electons: Se, Cl or Br? Why?

14. What is larger: an argon atom or a chloride ion (Cl-)? How do you know?

Conceptual Questions:

1. Why is the radius of Li+ so much smaller than that of Li? Why is the radius of F- so much larger than that of F?

2. Discuss the first, second and third ionization energies that would be expected for Indium in terms of where the largest increase in ionization would be expected and why.

3. Why do the elements with the highest ionization energy also have the most negative electron affinity?

4. When electricity is passed through a glass tube containing Neon gas, a bright orange glow is observed.

a. Explain this phenomenon on an atomic scale.

b. What does this indicate about the electronic structure of an atom?

5. The four electron transitions shown below release electromagnetic radiation within the visible spectrum. Rank the light released from highest to lowest frequency.

6. Draw where the peaks might appear in the photoelectron spectrum of Sulfur on the graph below. A peak for the 1s electrons has been added to help you get started.

7. The photoelectron spectra to the

right shows the energy required to remove

a 1s electron from a nitrogen atom and

from an oxygen atom. Explain why the peak

in nitrogen’s spectrum is to the right of the

peak in oxygen’s spectrum?

(Hint: think about the “arsenal”)

8. What does mass spectrometry tell us about atoms and how their structure differs?

9. The graph to the right is part of the mass spectrum for a sample of Copper atoms. What does it reveal about Copper’s two commonly occurring isotopes; Cu-63 and Cu-65?

10. Bohr’s shell model of the atom requires the electrons to be moving in quantized circular orbits around the nucleus. The distance of an electron from the nucleus determines its energy level in this model. However, Heisenberg’s uncertainty principle limits the accuracy with which the momentum and position of an electron can be known, suggesting that fixed orbits are not a good description of electron behavior.

Which of the following statements best describes the current understanding of electron behavior in an atom?

11. The first ionization energy (IE) of carbon (C) is 1086 kJ/mol. What can be predicted about the IE values for nitrogen (N) and silicon (Si) compared with that of carbon, based on differences in the effective nuclear charge (Zeff) and/or the radius of each type of atom?

12. The table below shows the first ionization energies (IE’s) for the first 10 elements in the periodic table.

Which of the following statements describes the aspect of these data that cannot be explained using atomic number and radius?

13. Bohr’s model of the atom was refined by adding subshells within the primary shells. The graph on the right shows a simulated photoelectron spectroscopy (PES) spectrum for boron (B). Ionization energy (IE) is the energy required to overcome an electron’s binding energy.

The table below the graph provides the IEs required to remove successive electrons from a boron atom:

14. A simulated photoelectron spectroscopy (PES) spectrum for an unknown element is shown below. Ionization energy (IE) is the energy required to overcome an electron’s binding energy.

Which statement about the peaks in the PES spectrum and the resulting electron configuration for the element is consistent with the data?

15. A scientist inserted a sample of the element lead (Pb) into a mass spectrometer. The instrument vaporized and ionized the sample, accelerated the ions with an electric field, and then deflected the ions into a detector, using a magnetic field. The information below includes the mass spectrum for this sample of Pb and the four postulates of Dalton’s model of the atom.

Dalton’s Model of the Atom

1. All matter is made of tiny, indivisible particles called atoms.

2. All atoms of an element are alike, but are different from atoms of any other element.

3. Compounds are formed when atoms of different elements combine in fixed proportions.

4. A chemical reaction involves a rearrangement of atoms, not a change in the atoms themselves.

How does the mass spectrum for this sample of Pb support or refute Dalton’s model of the atom?

Test Review Sheet

Sample Problems

:

1.

The types of electromagnetic radiation listed below are in order

of

increasing energy.

Type of radiation

(in order of

increasing energy)

long radio

waves

FM radio

waves

microwaves

infrared light

visible light

X

-

rays

Frequency

Wavelength

Complete the table by matching the frequencies and wavelengths from the list below with the appropriate type of

radiation

. You should not need a diagram of the electromagnetic spectrum to do this.

Frequencies:

10

10

s

-

1

10

13

s

-

1

10

8

s

-

1

10

1

s

-

1

10

18

s

-

1

10

15

s

-

1

Wavelengths:

10

-

7

m

10

-

10

m

10

8

m

10

1

m

10

-

4

m

10

-

2

m

2. Violet light has a wavelength of about 410 nm. What is its frequency?

What is the energy of one photon of this light?

What is the energy of one mole of violet light photons?

3. Use the following table to answer

the question below.

Ultraviolet

10 nm

–

400 nm

Blue

-

green light

400 nm

–

550 nm

Red

-

orange light

550 nm

–

700 nm

Short wave

Infrared

700 nm

–

2000 nm

The reaction of hydrogen gas with chlorine gas to form hydrogen chlor

ide can be initiated with

electromagnetic

radiation. The radiation must have a minimum energy of 9.91x10

-

19

J/photon in order to initiate the reaction. A student

suggests shining a blue

-

green laser through the gases as a method to initiate the reaction. Do you agree or disagree?

Justify your response.

4

. How many subshells

(

types of orbitals

)

exist in the n=5 principal energy level?

5

. How many f orbitals are there in the n=4 principal energy level?

6

. Use correct orbital box notation to write the electron configuration for

phosphorus.

Test Review Sheet

Sample Problems:

1. The types of electromagnetic radiation listed below are in order of increasing energy.

Type of radiation

(in order of

increasing energy)

long radio

waves

FM radio

waves

microwaves infrared light visible light X-rays

Frequency

Wavelength

Complete the table by matching the frequencies and wavelengths from the list below with the appropriate type of

radiation. You should not need a diagram of the electromagnetic spectrum to do this.

Frequencies: 10

10

s

-1

10

13

s

-1

10

8

s

-1

10

1

s

-1

10

18

s

-1

10

15

s

-1

Wavelengths: 10

-7

m 10

-10

m 10

8

m 10

1

m 10

-4

m 10

-2

m

2. Violet light has a wavelength of about 410 nm. What is its frequency?

What is the energy of one photon of this light?

What is the energy of one mole of violet light photons?

3. Use the following table to answer the question below.

Ultraviolet 10 nm – 400 nm

Blue-green light 400 nm – 550 nm

Red-orange light 550 nm – 700 nm

Short wave Infrared 700 nm – 2000 nm

The reaction of hydrogen gas with chlorine gas to form hydrogen chloride can be initiated with electromagnetic

radiation. The radiation must have a minimum energy of 9.91x10

-19

J/photon in order to initiate the reaction. A student

suggests shining a blue-green laser through the gases as a method to initiate the reaction. Do you agree or disagree?

Justify your response.

4. How many subshells (types of orbitals) exist in the n=5 principal energy level?

5. How many f orbitals are there in the n=4 principal energy level?

6. Use correct orbital box notation to write the electron configuration for phosphorus.