Question 1

Which statement below about an electron shell in a hydrogen-like atom is FALSE?

Accepted Answer

A) Higher shells are at a higher energy. 
B) All electrons in the same shell occupy regions in space that have the same shape. 
C) The principal quantum number, n, is used to specify a shell. 
D) The size of the shell increases as n increases. 
E) A shell can contain no more than N2 orbitals. 
A) Higher shells are at a higher energy. 
B) All electrons in the same shell occupy regions in space that have the same shape. 
C) The principal quantum number, n, is used to specify a shell. 
D) The size of the shell increases as n increases. 
E) A shell can contain no more than N2 orbitals.

Question 2

Orbitals within a given subshell have the same _______.

Accepted Answer

A) principal and angular momentum quantum numbers. 
B) principal quantum numbers. 
C) angular momentum quantum numbers. 
D) angular momentum and magnetic quantum numbers. 
E) angular momentum and spin quantum numbers. 
A) principal and angular momentum quantum numbers. 
B) principal quantum numbers. 
C) angular momentum quantum numbers. 
D) angular momentum and magnetic quantum numbers. 
E) angular momentum and spin quantum numbers.

Question 3

The Fraunhofer lines are evidence that _______.

Accepted Answer

A) atoms contain nuclei. 
B) atoms contain charged particles. 
C) mass is equivalent to energy. 
D) atoms absorb light. 
E) atoms emit light. 
A) atoms contain nuclei. 
B) atoms contain charged particles. 
C) mass is equivalent to energy. 
D) atoms absorb light. 
E) atoms emit light.

Question 4

Which of the following has the largest atomic radius?

Accepted Answer

A) Cs 
B) Rb 
C) Kr 
D) Xe 
E) I 
A) Cs 
B) Rb 
C) Kr 
D) Xe 
E) I

Question 5

Which row 2 element probably has the following successive ionization energies:

Accepted Answer

A) Be 
B) B 
C) N 
D) O 
E) Ne 
A) Be 
B) B 
C) N 
D) O 
E) Ne

Question 6

Astronomers have detected hydrogen atoms in interstellar space in the n = 732 energy level.Suppose an atom in this excited state emits a photon and undergoes a transition from n = 732 to n = 632.How much energy does the atom lose as a result of this transition? What is the frequency of this radiation? In which spectral region does this radiation lie?

Accepted Answer

1.39 *10^-24 J of en

Question 7

Fraunhofer lines are due to _______.

Accepted Answer

A) the emission of radiation by atoms. 
B) the absorption of radiation by atoms. 
C) the photoelectric effect. 
D) chemical reactions in the sun. 
E) nuclear reactions in the sun. 
A) the emission of radiation by atoms. 
B) the absorption of radiation by atoms. 
C) the photoelectric effect. 
D) chemical reactions in the sun. 
E) nuclear reactions in the sun.

Question 8

Which of the following statements about electron spin and the spin quantum number, ms, is NOT true?

Accepted Answer

A) The idea of electron spin was introduced to explain pairs of lines in atomic emission spectra. 
B) The electron creates a magnetic field because it is a charged particle moving through space. 
C) The spin of an electron is quantized. 
D) Electrons in the same orbital can have the same spin. 
E) The spin quantum number can only have one of two values, +1/2 and -1/2 . 
A) The idea of electron spin was introduced to explain pairs of lines in atomic emission spectra. 
B) The electron creates a magnetic field because it is a charged particle moving through space. 
C) The spin of an electron is quantized. 
D) Electrons in the same orbital can have the same spin. 
E) The spin quantum number can only have one of two values, +1/2 and -1/2 .

Question 9

Which one of the following sources produces the highest energy photons?

Accepted Answer

A) a doctor's x-ray source 
B) a heat lamp in a restaurant 
C) a microwave oven 
D) gamma rays from a star 
E) radio waves from a local station 
A) a doctor's x-ray source 
B) a heat lamp in a restaurant 
C) a microwave oven 
D) gamma rays from a star 
E) radio waves from a local station

Question 10

When the principal quantum number = 3, what values are possible for the other quantum numbers $ l $ and ml ?

Accepted Answer

@#LAT-DLM& can equal 0, 1, and 2.
For @#LAT-DLM& =

Question 11

What is the velocity of an O2 molecule if its de Broglie wavelength is 26 pm? 
(1 amu = 1.66054 *10-27 kg.)

Accepted Answer

A) 46 m/s 
B) 960 m/s 
C) 790 m/s 
D) 390 m/s 
E) 480 m/s 
A) 46 m/s 
B) 960 m/s 
C) 790 m/s 
D) 390 m/s 
E) 480 m/s

Question 12

What are the principal and angular momentum quantum numbers for a 4$ f $ orbital?

Accepted Answer

A) n = 4, $ l $ = 2 
B) n = 3, $ l $= 4 
C) n = 4, $ l $ = 3 
D) n = 4, $ l $ = 4 
E) n = 4, $ l $ = 1 
A) n = 4, $ l $ = 2 
B) n = 3, $ l $= 4 
C) n = 4, $ l $ = 3 
D) n = 4, $ l $ = 4 
E) n = 4, $ l $ = 1

Question 13

Which of the following elements would you expect to have the lowest first ionization energy?

Accepted Answer

A) N 
B) As 
C) P 
D) Bi 
E) Sb 
A) N 
B) As 
C) P 
D) Bi 
E) Sb

Question 14

Mercury lamps emit blue light with $\lambda$= 436 nm.What is the energy of these photons in joules?

Accepted Answer

A) 4.56 * 10-19 J 
B) 4.56 * 10-28J 
C) 1.97 * 1044 J 
D) 2.19 * 1018 J 
E) 2.19 * 10-18 J 
A) 4.56 * 10-19 J 
B) 4.56 * 10-28J 
C) 1.97 * 1044 J 
D) 2.19 * 1018 J 
E) 2.19 * 10-18 J

Question 15

Copper commonly forms a cation with a charge of 1+; however, the element to the right of it in the periodic table Zn) typically only forms a cation with a 2+charge.Use your knowledge of electron configurations to explain this observation.

Accepted Answer

Copper has the electronic conf

Question 16

What is the wavelength ($\lambda$, in meters) of a radio station operating at a frequency of 99.6 MHz?

Accepted Answer

A) 3.01*106 m 
B) 3.01 m 
C) 3.32 *10-7 m 
D) 0.332 m 
E) 3.32 m 
A) 3.01*106 m 
B) 3.01 m 
C) 3.32 *10-7 m 
D) 0.332 m 
E) 3.32 m

Question 17

Which of the following is the correct electron configuration for silicon?

Accepted Answer

A)  $  1 s^{2} 2 s^{2} 1 p^{6} 3 s^{2} 2 p^{2} $ 
B)  $  1 s^{2} 2 s^{2} 2 p^{6} 3 s^{4} $ 
C)  $ 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2} $ 
D)  $ 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1} 3 p^{3} $ 
E)  $ 1 s^{2} 2 s^{2} 2 p^{6} 2 d^{4} $ 
A)  $  1 s^{2} 2 s^{2} 1 p^{6} 3 s^{2} 2 p^{2} $ 
B)  $  1 s^{2} 2 s^{2} 2 p^{6} 3 s^{4} $ 
C)  $ 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{2} 3 p^{2} $ 
D)  $ 1 s^{2} 2 s^{2} 2 p^{6} 3 s^{1} 3 p^{3} $ 
E)  $ 1 s^{2} 2 s^{2} 2 p^{6} 2 d^{4} $

Question 18

Which of the following lasers emits photons with the lowest energy?

Accepted Answer

A) a Nd:YAG laser with $\lambda$ = 1064 nm 
B) an Ar+ laser with $\lambda$ = 514.5 nm 
C) a Kr+ laser with $\lambda$ = 647 nm 
D) an ArF laser with $\lambda$= 193 nm 
E) a HeNe laser with $\lambda$= 633 nm 
A) a Nd:YAG laser with $\lambda$ = 1064 nm 
B) an Ar+ laser with $\lambda$ = 514.5 nm 
C) a Kr+ laser with $\lambda$ = 647 nm 
D) an ArF laser with $\lambda$= 193 nm 
E) a HeNe laser with $\lambda$= 633 nm

Question 19

How many unpaired electrons does nickel have?

Accepted Answer

A) 0 
B) 2 
C) 3 
D) 4 
E) 8 
A) 0 
B) 2 
C) 3 
D) 4 
E) 8

Question 20

Which of the following shows the correct expression for the ionization energy indicated?

Accepted Answer

A)  $ \mathrm{IE}_{3}: \mathrm{Al}(g) \rightarrow \mathrm{Al}^{3+}(g)+3 \mathrm{e}^{-} $ 
B)  $ \mathrm{IE}_{1}: \mathrm{Cl}(g) \rightarrow \mathrm{Cl}^{+}(g)+\mathrm{e}^{-} $ 
C)  $ \mathrm{IE}_{2}: \mathrm{Mg}(g) \rightarrow \mathrm{Mg}^{2+}(g)+2 \mathrm{e}^{-} $ 
D)  $ \mathrm{IE}_{1}: \mathrm{Na}(s) \rightarrow \mathrm{Na}^{+}(g)+\mathrm{e}^{-} $ 
E)  $ \mathrm{IE}_{3}: \mathrm{O}_{2}(g) \rightarrow \mathrm{O}_{2}^{+}(g)+\mathrm{e}^{-} $ 
A)  $ \mathrm{IE}_{3}: \mathrm{Al}(g) \rightarrow \mathrm{Al}^{3+}(g)+3 \mathrm{e}^{-} $ 
B)  $ \mathrm{IE}_{1}: \mathrm{Cl}(g) \rightarrow \mathrm{Cl}^{+}(g)+\mathrm{e}^{-} $ 
C)  $ \mathrm{IE}_{2}: \mathrm{Mg}(g) \rightarrow \mathrm{Mg}^{2+}(g)+2 \mathrm{e}^{-} $ 
D)  $ \mathrm{IE}_{1}: \mathrm{Na}(s) \rightarrow \mathrm{Na}^{+}(g)+\mathrm{e}^{-} $ 
E)  $ \mathrm{IE}_{3}: \mathrm{O}_{2}(g) \rightarrow \mathrm{O}_{2}^{+}(g)+\mathrm{e}^{-} $

Exam 3: Atomic Structure Explaining the Properties of Elements

Which statement below about an electron shell in a hydrogen-like atom is FALSE?

Orbitals within a given subshell have the same _______.

The Fraunhofer lines are evidence that _______.

Which of the following has the largest atomic radius?

Which row 2 element probably has the following successive ionization energies:

Fraunhofer lines are due to _______.

Which of the following statements about electron spin and the spin quantum number, ms, is NOT true?

Which one of the following sources produces the highest energy photons?

When the principal quantum number = 3, what values are possible for the other quantum numbers l l l and ml ?

What is the velocity of an O2 molecule if its de Broglie wavelength is 26 pm? (1 amu = 1.66054 *10-27 kg.)

What are the principal and angular momentum quantum numbers for a 4 f f f orbital?

Which of the following elements would you expect to have the lowest first ionization energy?

Mercury lamps emit blue light with λ\lambdaλ = 436 nm.What is the energy of these photons in joules?

Copper commonly forms a cation with a charge of 1+; however, the element to the right of it in the periodic table Zn) typically only forms a cation with a 2+charge.Use your knowledge of electron configurations to explain this observation.

What is the wavelength ( λ\lambdaλ , in meters) of a radio station operating at a frequency of 99.6 MHz?

Which of the following is the correct electron configuration for silicon?

Which of the following lasers emits photons with the lowest energy?

How many unpaired electrons does nickel have?

Which of the following shows the correct expression for the ionization energy indicated?

Matter and Energy an Atomic Perspective

Atoms, Ions, and Molecules the Building Blocks of Matter

Chemical Bonding Understanding Climate Change

Bonding Theories Explaining Molecular Geometry

Intermolecular Forces Attractions Between Particles

Stoichiometry Mass Relationships and Chemical Reactions

Aqueous Solutions Chemistry of the Hydrosphere

Thermochemistry Energy Changes in Chemical Reactions

Properties of Gases the Air We Breathe

Properties of Solutions Their Concentrations and Colligative Properties

Thermodynamics Why Chemical Reactions Happen

Chemical Kinetics Clearing the Air

Chemical Equilibrium Equal but Opposite Reaction Rates

Acid-Base Equilibria Proton Transfer in Biological Systems

Additional Aqueous Equilibria Chemistry and the Oceans

Electrochemistry the Quest for Clean Energy

The Solid State a Particulate View

Organic Chemistry Fuels, Pharmaceuticals, and Modern Materials

Biochemistry the Compounds of Life

Nuclear Chemistry the Risks and Benefits

The Main Group Elements Life and the Periodic Table

Transition Metals Biological and Medical Applications

Filters

Which of the following statements about electron spin and the spin quantum number, m_s, is NOT true?

When the principal quantum number = 3, what values are possible for the other quantum numbers $l$ and m_l ?

What is the velocity of an O₂ molecule if its de Broglie wavelength is 26 pm? (1 amu = 1.66054 *10^-27 kg.)

What are the principal and angular momentum quantum numbers for a 4 $f$ orbital?

Mercury lamps emit blue light with $\lambda$ = 436 nm.What is the energy of these photons in joules?

What is the wavelength ( $\lambda$ , in meters) of a radio station operating at a frequency of 99.6 MHz?