Question 1

The (principal quantum number) n = ____ shell is the lowest that may contain s-orbitals.

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  4 
E)  5 
A)  1 
B)  2 
C)  3 
D)  4 
E)  5

Question 2

Which type of experiment demonstrates that an electron has the properties of a wave?

Accepted Answer

A)  nuclear fission 
B)  electron diffraction 
C)  light emission from atomic gases 
D)  mass spectroscopy 
E)  photoelectric effect 
A)  nuclear fission 
B)  electron diffraction 
C)  light emission from atomic gases 
D)  mass spectroscopy 
E)  photoelectric effect

Question 3

Which of the following properties of orbital is associated with the value of the principal quantum number?

Accepted Answer

A)  Number of electrons in an orbital 
B)  Size of an orbital 
C)  Orientation in space of an orbital 
D)  Energy of an orbital 
E)  Shape of an orbital 
A)  Number of electrons in an orbital 
B)  Size of an orbital 
C)  Orientation in space of an orbital 
D)  Energy of an orbital 
E)  Shape of an orbital

Question 4

How many orbitals have the following set of quantum numbers: n = 5, $\ell$ = 3, $m _ { \ell }$ = -1?

Accepted Answer

A)  0 
B)  1 
C)  3 
D)  6 
E)  7 
A)  0 
B)  1 
C)  3 
D)  6 
E)  7

Question 5

Which of the following orbital can be represented by n = 4, $\ell$ = 3, and $m _ { \ell }$ = -2?

Accepted Answer

A)  4s 
B)  4p 
C)  4d 
D)  4f 
E)  None of these 
A)  4s 
B)  4p 
C)  4d 
D)  4f 
E)  None of these

Question 6

What is the total number of orbitals having n = 3 and $\ell$ = 2?

Accepted Answer

A)  1 
B)  3 
C)  5 
D)  7 
E)  10 
A)  1 
B)  3 
C)  5 
D)  7 
E)  10

Question 7

Which of the following sets of quantum numbers refers to a 4d orbital?

Accepted Answer

A)  n = 2, $\ell$ = 1, $m _ { \ell }$ = -1 
B)  n = 2, $\ell$ = 4, $m _ { \ell }$ = -1 
C)  n = 4, $\ell$ = 2, $m _ { \ell }$ = -1 
D)  n = 4, $\ell$ = 3, $m _ { \ell }$ = 0 
E)  n = 4, $\ell$ = 3, $m _ { \ell }$ = +2 
A)  n = 2, $\ell$ = 1, $m _ { \ell }$ = -1 
B)  n = 2, $\ell$ = 4, $m _ { \ell }$ = -1 
C)  n = 4, $\ell$ = 2, $m _ { \ell }$ = -1 
D)  n = 4, $\ell$ = 3, $m _ { \ell }$ = 0 
E)  n = 4, $\ell$ = 3, $m _ { \ell }$ = +2

Question 8

A light emitting diode (L.E.D.) emits photons with an energy of 
$5.315 \times 10 ^ { - 19 }$
J. What is the energy per mole of photons emitted? ?

Accepted Answer

A)  $3.201 \times 10 ^ { 5 }$ J/mol 
B)  $8.826 \times 10 ^ { 0 }$ J/mol 
C)  $3.201 \times 10 ^ { 8 }$ J/mol 
D)  $5.315 \times 10 ^ { - 19 }$ J/mol 
E)  $8.826 \times 10 ^ { 6 }$ J/mol 
A)  $3.201 \times 10 ^ { 5 }$ J/mol 
B)  $8.826 \times 10 ^ { 0 }$ J/mol 
C)  $3.201 \times 10 ^ { 8 }$ J/mol 
D)  $5.315 \times 10 ^ { - 19 }$ J/mol 
E)  $8.826 \times 10 ^ { 6 }$ J/mol

Question 9

Which of the following sets of quantum numbers is not allowed?

Accepted Answer

A)  n = 4, $\ell$ = 2, and $m _ { \ell }$ = -2 
B)  n = 6, $\ell$ = 1, and $m _ { \ell }$ = 1 
C)  n = 5, $\ell$ = 4, and $m _ { \ell }$ = -4 
D)  n = 2, $\ell$ = 1, and $m _ { \ell }$ = -3 
E)  n = 6, $\ell$ = 3, and $m _ { \ell }$ = -2 
A)  n = 4, $\ell$ = 2, and $m _ { \ell }$ = -2 
B)  n = 6, $\ell$ = 1, and $m _ { \ell }$ = 1 
C)  n = 5, $\ell$ = 4, and $m _ { \ell }$ = -4 
D)  n = 2, $\ell$ = 1, and $m _ { \ell }$ = -3 
E)  n = 6, $\ell$ = 3, and $m _ { \ell }$ = -2

Question 10

The size of an electron orbital is often chosen to be the distance within which 90% of the electron density is found. Why is the orbital radius not chosen to be the distance within which 100% of the electron density is found?

Accepted Answer

The probability of finding an electron d

Question 11

A 4d orbital has ?

Accepted Answer

A)  3 planar nodes and 3 spherical nodes. 
B)  1 planar node and 1 spherical node. 
C)  2 planar nodes and 1 spherical node. 
D)  2 planar nodes and 4 spherical nodes. 
E)  4 planar nodes and 2 spherical nodes. 
A)  3 planar nodes and 3 spherical nodes. 
B)  1 planar node and 1 spherical node. 
C)  2 planar nodes and 1 spherical node. 
D)  2 planar nodes and 4 spherical nodes. 
E)  4 planar nodes and 2 spherical nodes.

Question 12

If a cordless phone operates at a frequency of 9.00 × 108 s-1, what is the wavelength of this radiation?

Accepted Answer

A)  0.333 m 
B)  1.99 m 
C)  3.33 × 10-9 m 
D)  3.71 × 10-18 m 
E)  2.70 × 1017 m 
A)  0.333 m 
B)  1.99 m 
C)  3.33 × 10-9 m 
D)  3.71 × 10-18 m 
E)  2.70 × 1017 m

Question 13

Which of the following is the correct series of lines that have energies in visible region of the hydrogen spectrum?

Accepted Answer

A)  Balmer series 
B)  Lyman series 
C)  Brackett series 
D)  Pfund series 
E)  Humphreys series 
A)  Balmer series 
B)  Lyman series 
C)  Brackett series 
D)  Pfund series 
E)  Humphreys series

Question 14

The contribution for which de Broglie is best remembered in modern science is

Accepted Answer

A)  his statement that no electron can have identical values for all four quantum numbers. 
B)  his proposal that particles of matter should be associated with wavelike behavior. 
C)  his statement that an electron can exist in an atom only in discrete energy levels. 
D)  his statement that elements show periodic repetition of properties. 
E)  his statement that electrons occupy all the orbitals of a given sublevel singly before pairing begins. 
A)  his statement that no electron can have identical values for all four quantum numbers. 
B)  his proposal that particles of matter should be associated with wavelike behavior. 
C)  his statement that an electron can exist in an atom only in discrete energy levels. 
D)  his statement that elements show periodic repetition of properties. 
E)  his statement that electrons occupy all the orbitals of a given sublevel singly before pairing begins.

Question 15

For which of the following electron transitions would a hydrogen atom emit a photon of the longest wavelength?

Accepted Answer

A)    
B)    
C)    
D)    
A)    
B)    
C)    
D)

Question 16

What is the energy per mole of photons of light with a wavelength of 690.8 nm?

Accepted Answer

A)  2.88 × 10-19 kJ/mol 
B)  4.16 × 1014 kJ/mol 
C)  2.61 × 1035 kJ/mol 
D)  4.34 × 1014 kJ/mol 
E)  1.73 × 102 kJ/mol 
A)  2.88 × 10-19 kJ/mol 
B)  4.16 × 1014 kJ/mol 
C)  2.61 × 1035 kJ/mol 
D)  4.34 × 1014 kJ/mol 
E)  1.73 × 102 kJ/mol

Question 17

Occupied states or energy levels in the hydrogen atom with n > 1 are called _____ states.

Accepted Answer

The answer of Occupied states or energy levels in the...

Question 18

A device operates at a frequency of $7.7 \times 10 ^ { 14 }$ Hz. What is the wavelength of this radiation?

Accepted Answer

A)  ?390 nm 
B)  $2.57 \times 10 ^ { 31 }$ nm 
C)  $2.58 \times 10 ^ { - 31 }$ nm 
D)  0.153 nm 
E)  $5.11 \times 10 ^ { - 10 }$ nm 
A)  ?390 nm 
B)  $2.57 \times 10 ^ { 31 }$ nm 
C)  $2.58 \times 10 ^ { - 31 }$ nm 
D)  0.153 nm 
E)  $5.11 \times 10 ^ { - 10 }$ nm

Question 19

Which type of orbital is designated n = 2 and $\ell$ = 1?

Accepted Answer

A)  2p 
B)  3s 
C)  4d 
D)  1f 
E)  2d 
A)  2p 
B)  3s 
C)  4d 
D)  1f 
E)  2d

Question 20

​A device emits light at 219.4 nm. What is the frequency of this radiation?

Accepted Answer

A)  ​1.37 × 10-3 Hz 
B)  3.31 × 1026 Hz 
C)  1.37 × 1015 Hz 
D)  9.07 × 10-37 Hz 
E)  9.07 × 10-19 Hz 
A)  ​1.37 × 10-3 Hz 
B)  3.31 × 1026 Hz 
C)  1.37 × 1015 Hz 
D)  9.07 × 10-37 Hz 
E)  9.07 × 10-19 Hz

Exam 7: The Structure of Atoms

The (principal quantum number) n = ____ shell is the lowest that may contain s-orbitals.

Which type of experiment demonstrates that an electron has the properties of a wave?

Which of the following properties of orbital is associated with the value of the principal quantum number?

How many orbitals have the following set of quantum numbers: n = 5, ℓ\ellℓ = 3, mℓm _ { \ell }mℓ​ = -1?

Which of the following orbital can be represented by n = 4, ℓ\ellℓ = 3, and mℓm _ { \ell }mℓ​ = -2?

What is the total number of orbitals having n = 3 and ℓ\ellℓ = 2?

Which of the following sets of quantum numbers refers to a 4d orbital?

A light emitting diode (L.E.D.) emits photons with an energy of 5.315×10−195.315 \times 10 ^ { - 19 }5.315×10−19 J. What is the energy per mole of photons emitted? ?

Which of the following sets of quantum numbers is not allowed?

The size of an electron orbital is often chosen to be the distance within which 90% of the electron density is found. Why is the orbital radius not chosen to be the distance within which 100% of the electron density is found?

A 4d orbital has ?

If a cordless phone operates at a frequency of 9.00 × 108 s-1, what is the wavelength of this radiation?

Which of the following is the correct series of lines that have energies in visible region of the hydrogen spectrum?

The contribution for which de Broglie is best remembered in modern science is

For which of the following electron transitions would a hydrogen atom emit a photon of the longest wavelength?

What is the energy per mole of photons of light with a wavelength of 690.8 nm?

Occupied states or energy levels in the hydrogen atom with n > 1 are called _____ states.

A device operates at a frequency of 7.7×10147.7 \times 10 ^ { 14 }7.7×1014 Hz. What is the wavelength of this radiation?

Which type of orbital is designated n = 2 and ℓ\ellℓ = 1?

​A device emits light at 219.4 nm. What is the frequency of this radiation?

Basic Concepts of Chemistry

Lets Review: the Tools of Quantitative Chemistry

Atoms, Molecules, and Ions

Chemical Reactions

Stoichiometry: Quantitative Information About Chemical Reactions

Principles of Chemical Reactivity: Energy and Chemical Reactions

The Structure of Atoms and Periodic Trends

Bonding and Molecular Structure

Bonding and Molecular Structure Orbital Hybridization and Molecular Orbitals

Gases and Their Properties

Intermolecular Forces and Liquids

The Solid State

Solutions and Their Behavior

Chemical Kinetics: the Rates of Chemical Reactions

Principles of Chemical Reactivity: Equilibria

Principles of Chemical Reactivity: the Chemistry of Acids and Bases

Principles of Chemical Reactivity: Other Aspects of Aqueous Equilibria

Principles of Chemical Reactivity: Entropy and Free Energy

Principles of Chemical Reactivity: Electron Transfer Reactions

Environmental Chemistry: Earths Environment, Energy, and Sustainability

The Chemistry of the Main Group Elements

The Chemistry of the Transition Elements

Carbon: Not Just Another Element

Biochemistry

Nuclear Chemistry

Filters

How many orbitals have the following set of quantum numbers: n = 5, $\ell$ = 3, $m _ { \ell }$ = -1?

Which of the following orbital can be represented by n = 4, $\ell$ = 3, and $m _ { \ell }$ = -2?

What is the total number of orbitals having n = 3 and $\ell$ = 2?

A light emitting diode (L.E.D.) emits photons with an energy of $5.315 \times 10 ^ { - 19 }$ J. What is the energy per mole of photons emitted? ?

If a cordless phone operates at a frequency of 9.00 × 10⁸ s^-1, what is the wavelength of this radiation?

A device operates at a frequency of $7.7 \times 10 ^ { 14 }$ Hz. What is the wavelength of this radiation?

Which type of orbital is designated n = 2 and $\ell$ = 1?

A device emits light at 219.4 nm. What is the frequency of this radiation?