Question 1

Which orbital has the lowest energy in a multielectron atom? The quantum numbers are given as (n,   , ml).

Accepted Answer

A) (3, 2, 1) 
B) (5, 0, 0) 
C) (4, 1, F1F1F1S1F1F1F101) 
D) (4, 2, 1) 
E) All are at equal energy. 
A) (3, 2, 1) 
B) (5, 0, 0) 
C) (4, 1, F1F1F1S1F1F1F101) 
D) (4, 2, 1) 
E) All are at equal energy. B

Question 2

Which of the following is not a possible set of quantum numbers for an electron?

Accepted Answer

A) n   5,   4, me
    F1F1F1S1F1F1F102 
B) n   3,   0, me     0 
C) n   2,   1, me     F1F1F1S1F1F1F101 
D) n   1,   0, me     1 
E) n   4,   3, me     F1F1F1S1F1F1F103 
A) n   5,   4, me
    F1F1F1S1F1F1F102 
B) n   3,   0, me     0 
C) n   2,   1, me     F1F1F1S1F1F1F101 
D) n   1,   0, me     1 
E) n   4,   3, me     F1F1F1S1F1F1F103 D

Question 3

How many electrons can be in the n F1F1F1S1F1F1F10 3 shell of an atom? (Include all orbitals that have n F1F1F1S1F1F1F10 3.)

Accepted Answer

18

Question 4

Which of the transitions in the hydrogen atom energy-level diagram shown here requires the longest wavelength photon?

Accepted Answer

A) a 
B) b 
C) c 
D) d 
A) a 
B) b 
C) c 
D) d

Question 5

Consider the radial distribution shown below for an electron in an s atomic orbital where r is the distance of the electron from the nucleus.   Identify: (1) where the atomic nucleus is located; (2) a radial node; (3) the most probable distance of the electron from the nucleus; and (4) the principle quantum number for this orbital.

Accepted Answer

(1) The nucleus is located at A; (2) rad

Question 6

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

Accepted Answer

A) C 
B) O 
C) Li 
D) Be 
E) B 
A) C 
B) O 
C) Li 
D) Be 
E) B

Question 7

Which listing has the orbitals in order of increasing energy in a multielectron atom?

Accepted Answer

A) 3s   F1F1F1S1F1F1F103p   F1F1F1S1F1F1F103d   F1F1F1S1F1F1F104s 
B) 5s   F1F1F1S1F1F1F104d   F1F1F1S1F1F1F105p 
C) 5s   F1F1F1S1F1F1F103d   F1F1F1S1F1F1F105p 
D) 2px   F1F1F1S1F1F1F102py   F1F1F1S1F1F1F102pz 
E) 3s   F1F1F1S1F1F1F102p   F1F1F1S1F1F1F104s 
A) 3s   F1F1F1S1F1F1F103p   F1F1F1S1F1F1F103d   F1F1F1S1F1F1F104s 
B) 5s   F1F1F1S1F1F1F104d   F1F1F1S1F1F1F105p 
C) 5s   F1F1F1S1F1F1F103d   F1F1F1S1F1F1F105p 
D) 2px   F1F1F1S1F1F1F102py   F1F1F1S1F1F1F102pz 
E) 3s   F1F1F1S1F1F1F102p   F1F1F1S1F1F1F104s

Question 8

Which of the following sources produces the highest energy photons?

Accepted Answer

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

Question 9

If each of the following metals is exposed to light with a wavelength of 240 nm, which will emit photoelectrons with the greatest kinetic energy?

Accepted Answer

A) iron (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 7.2   F1F1F1S1F1F1F10J) 
B) platinum (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 9.1   F1F1F1S1F1F1F10J) 
C) nickel (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 8.3   F1F1F1S1F1F1F10J) 
D) palladium (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 8.2   F1F1F1S1F1F1F10J) 
E) sodium (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 4.4   F1F1F1S1F1F1F10J) 
A) iron (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 7.2   F1F1F1S1F1F1F10J) 
B) platinum (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 9.1   F1F1F1S1F1F1F10J) 
C) nickel (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 8.3   F1F1F1S1F1F1F10J) 
D) palladium (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 8.2   F1F1F1S1F1F1F10J) 
E) sodium (F1F1F1S1F1F1F10 F1F1F1S1F1F1F10 4.4   F1F1F1S1F1F1F10J)

Question 10

What is the orbital designation for an electron with the quantum numbers n   F1F1F1S1F1F1F103,   2?

Accepted Answer

A) 3s 
B) 3d 
C) 2p 
D) 2f 
E) 3e 
A) 3s 
B) 3d 
C) 2p 
D) 2f 
E) 3e

Question 11

How much energy is required to ionize one mole of hydrogen atoms in their ground state?

Accepted Answer

A) 1,312 kJ 
B) 2.18 kJ 
C) 218 kJ 
D) 2,178 kJ 
E) 131.2 kJ 
A) 1,312 kJ 
B) 2.18 kJ 
C) 218 kJ 
D) 2,178 kJ 
E) 131.2 kJ

Question 12

Which orbital has the highest energy in a multielectron atom? The quantum numbers are given as (n,   , ml).

Accepted Answer

A) (3, 2, 0) 
B) (4, 4, 0) 
C) (3, 0, 0) 
D) (4, 1, 1) 
E) (4, 3, F1F1F1S1F1F1F101) 
A) (3, 2, 0) 
B) (4, 4, 0) 
C) (3, 0, 0) 
D) (4, 1, 1) 
E) (4, 3, F1F1F1S1F1F1F101)

Question 13

A radio station's operating frequency has a wavelength of 2.81 m. What is this frequency?

Accepted Answer

A) 1.068   F1F1F1S1F1F1F10MHz 
B) 106.8 MHz 
C) 100.1 MHz 
D) 94.5 MHz 
E) 9.37   F1F1F1S1F1F1F10MHz 
A) 1.068   F1F1F1S1F1F1F10MHz 
B) 106.8 MHz 
C) 100.1 MHz 
D) 94.5 MHz 
E) 9.37   F1F1F1S1F1F1F10MHz

Question 14

Which statement about the quantum numbers that identify an atomic orbital is not correct?

Accepted Answer

A) The angular momentum quantum number,   , identifies the shape of an orbital. 
B) The value of the angular momentum quantum number can range from 0 to n, where n is the principal quantum number for the orbital. 
C) Orbitals with the same value for the principal quantum number and the angular momentum quantum number are said to be in the same subshell. 
D) Orbitals with the same values for the principal quantum number and the angular momentum quantum number have the same energy. 
E) The value for the angular momentum quantum number also is designated by a letter: s F1F1F1S1F1F1F10 0, p F1F1F1S1F1F1F10 1, d F1F1F1S1F1F1F10 2, f F1F1F1S1F1F1F10 3, and so on. 
A) The angular momentum quantum number,   , identifies the shape of an orbital. 
B) The value of the angular momentum quantum number can range from 0 to n, where n is the principal quantum number for the orbital. 
C) Orbitals with the same value for the principal quantum number and the angular momentum quantum number are said to be in the same subshell. 
D) Orbitals with the same values for the principal quantum number and the angular momentum quantum number have the same energy. 
E) The value for the angular momentum quantum number also is designated by a letter: s F1F1F1S1F1F1F10 0, p F1F1F1S1F1F1F10 1, d F1F1F1S1F1F1F10 2, f F1F1F1S1F1F1F10 3, and so on.

Question 15

Which of the following is a possible set of quantum numbers for a 3d orbital?

Accepted Answer

A) n   F1F1F1S1F1F1F103,   1, me
    F1F1F1S1F1F1F101 
B) n   F1F1F1S1F1F1F103,   0, me   F1F1F1S1F1F1F100 
C) n   F1F1F1S1F1F1F103,   2, me   F1F1F1S1F1F1F103 
D) n   F1F1F1S1F1F1F103,   2, me   F1F1F1S1F1F1F100 
E) n   F1F1F1S1F1F1F103,   1, me   F1F1F1S1F1F1F102 
A) n   F1F1F1S1F1F1F103,   1, me
    F1F1F1S1F1F1F101 
B) n   F1F1F1S1F1F1F103,   0, me   F1F1F1S1F1F1F100 
C) n   F1F1F1S1F1F1F103,   2, me   F1F1F1S1F1F1F103 
D) n   F1F1F1S1F1F1F103,   2, me   F1F1F1S1F1F1F100 
E) n   F1F1F1S1F1F1F103,   1, me   F1F1F1S1F1F1F102

Question 16

Which transition in a hydrogen atom requires the largest change in energy?

Accepted Answer

A) n1   F1F1F1S1F1F1F102 to n2 F1F1F1S1F1F1F10 3 
B) n1   F1F1F1S1F1F1F102 to n2 F1F1F1S1F1F1F10 4 
C) n1   F1F1F1S1F1F1F101 to n2 F1F1F1S1F1F1F10 3 
D) n1   F1F1F1S1F1F1F101 to n2   F1F1F1S1F1F1F102 
E) n1   F1F1F1S1F1F1F109 to n2   F1F1F1S1F1F1F1010 
A) n1   F1F1F1S1F1F1F102 to n2 F1F1F1S1F1F1F10 3 
B) n1   F1F1F1S1F1F1F102 to n2 F1F1F1S1F1F1F10 4 
C) n1   F1F1F1S1F1F1F101 to n2 F1F1F1S1F1F1F10 3 
D) n1   F1F1F1S1F1F1F101 to n2   F1F1F1S1F1F1F102 
E) n1   F1F1F1S1F1F1F109 to n2   F1F1F1S1F1F1F1010

Question 17

Astronomers have detected hydrogen atoms in interstellar space in the n F1F1F1S1F1F1F10 732 energy level. Suppose an atom in this excited state emits a photon and undergoes a transition from n F1F1F1S1F1F1F10 732 to n F1F1F1S1F1F1F10 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 F1F1F1S1F1F1F10 10F1F1F1

Question 18

Which orbital does not fill before a 4s in a multielectron atom?

Accepted Answer

A) 2s 
B) 2p 
C) 3s 
D) 3p 
E) 3d 
A) 2s 
B) 2p 
C) 3s 
D) 3p 
E) 3d

Question 19

How much energy is required to ionize one mole of HeF1F1F1S1F1F1F10 ions in their ground state?

Accepted Answer

A) 5,251 kJ 
B) 2,178 kJ 
C) 3,764 kJ 
D) 1,234 kJ 
E) 757 kJ 
A) 5,251 kJ 
B) 2,178 kJ 
C) 3,764 kJ 
D) 1,234 kJ 
E) 757 kJ

Question 20

Write the electron configuration of Co2F1F1F1S1F1F1F10.

Accepted Answer

Which orbital has the lowest energy in a multielectron atom? The quantum numbers are given as (n, , m_l).

Which of the following is not a possible set of quantum numbers for an electron?

How many electrons can be in the n  3 shell of an atom? (Include all orbitals that have n  3.)

Which of the transitions in the hydrogen atom energy-level diagram shown here requires the longest wavelength photon?

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

Which listing has the orbitals in order of increasing energy in a multielectron atom?

Which of the following sources produces the highest energy photons?

If each of the following metals is exposed to light with a wavelength of 240 nm, which will emit photoelectrons with the greatest kinetic energy?

What is the orbital designation for an electron with the quantum numbers n 3, 2?

How much energy is required to ionize one mole of hydrogen atoms in their ground state?

Which orbital has the highest energy in a multielectron atom? The quantum numbers are given as (n, , m_l).

A radio station's operating frequency has a wavelength of 2.81 m. What is this frequency?

Which statement about the quantum numbers that identify an atomic orbital is not correct?

Which of the following is a possible set of quantum numbers for a 3d orbital?

Which transition in a hydrogen atom requires the largest change in energy?

Which orbital does not fill before a 4s in a multielectron atom?

How much energy is required to ionize one mole of He^ ions in their ground state?

Write the electron configuration of Co²^.

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Exam 7: A Quantum Model of Atoms: Waves and Particles

Which orbital has the lowest energy in a multielectron atom? The quantum numbers are given as (n, , ml).

Which of the following is not a possible set of quantum numbers for an electron?

How many electrons can be in the n  3 shell of an atom? (Include all orbitals that have n  3.)

Which of the transitions in the hydrogen atom energy-level diagram shown here requires the longest wavelength photon?

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

Which listing has the orbitals in order of increasing energy in a multielectron atom?

Which of the following sources produces the highest energy photons?

If each of the following metals is exposed to light with a wavelength of 240 nm, which will emit photoelectrons with the greatest kinetic energy?

What is the orbital designation for an electron with the quantum numbers n 3, 2?

How much energy is required to ionize one mole of hydrogen atoms in their ground state?

Which orbital has the highest energy in a multielectron atom? The quantum numbers are given as (n, , ml).

A radio station's operating frequency has a wavelength of 2.81 m. What is this frequency?

Which statement about the quantum numbers that identify an atomic orbital is not correct?

Which of the following is a possible set of quantum numbers for a 3d orbital?

Which transition in a hydrogen atom requires the largest change in energy?

Which orbital does not fill before a 4s in a multielectron atom?

How much energy is required to ionize one mole of He ions in their ground state?

Write the electron configuration of Co2.

Matter and Energy: The Origin of the Universe

Atoms, Ions, and Molecules: Matter Starts Here

Stoichiometry: Mass, Formulas, and Reactions

Solution Chemistry: The Hydrosphere

Thermochemistry: Energy Changes in Reactions

Properties of Gases: The Air We Breathe

Chemical Bonds: What Makes a Gas a Greenhouse Gas

Molecular Geometry: Shape Determines Function

Intermolecular Forces: The Uniqueness of Water

Solutions: Properties and Behavior

Solids: Crystals, Alloys, and Polymers

Chemical Kinetics: Reactions in the Atmosphere

Chemical Equilibrium: How Much Product Does a Reaction Really Make

Acidbase Equilibria: Proton Transfer in Biological Systems

Additional Aqueous Equilibria: Chemistry and the Oceans

Thermodynamics: Spontaneous and Nonspontaneous Reactions and Processes

Electrochemistry: The Quest for Clean Energy

Nuclear Chemistry: Applications to Energy and Medicine

Organic and Biological Molecules: the Compounds of Life

The Main Group Elements: Life and the Periodic Table

Transition Metals: Biological and Medical Applications

Filters

Which orbital has the lowest energy in a multielectron atom? The quantum numbers are given as (n, , m_l).

Which orbital has the highest energy in a multielectron atom? The quantum numbers are given as (n, , m_l).

How much energy is required to ionize one mole of He^ ions in their ground state?

Write the electron configuration of Co²^.