Question 1

Identify the correct values for a 4f sublevel.

Accepted Answer

A) n = 3,l = 1,ml = 0 
B) n = 2,l = 1,ml = -2 
C) n = 1,l = 0,ml = 0 
D) n = 2,l = 0,ml = 0 
E) n = 4,l = 3,ml = -2 
A) n = 3,l = 1,ml = 0 
B) n = 2,l = 1,ml = -2 
C) n = 1,l = 0,ml = 0 
D) n = 2,l = 0,ml = 0 
E) n = 4,l = 3,ml = -2

Question 2

Choose the valence orbital diagram that represents the ground state of Zn.

Accepted Answer

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

Question 3

Describe the shape of a p orbital.

Accepted Answer

A) a ball 
B) two dumbbells 
C) three dumbbells 
D) four dumbbells 
E) eight dumbbells 
A) a ball 
B) two dumbbells 
C) three dumbbells 
D) four dumbbells 
E) eight dumbbells

Question 4

An electron ends in orbital n = 3 after a hydrogen atom emits a photon with a wavelength of 1093 nm.Calculate the initial orbital,ni.

Accepted Answer

A) 1 
B) 5 
C) 2 
D) 3 
E) 6 
A) 1 
B) 5 
C) 2 
D) 3 
E) 6

Question 5

What total energy (in kJ)is contained in 1.0 mol of photons,all with a frequency of 2.75 × 1014 Hz?

Accepted Answer

A) 182 kJ 
B) 219 kJ 
C) 457 kJ 
D) 326 kJ 
E) 110 kJ 
A) 182 kJ 
B) 219 kJ 
C) 457 kJ 
D) 326 kJ 
E) 110 kJ

Question 6

How many sublevels are contained in the second shell (n = 2)of a given atom?

Accepted Answer

A) 1 
B) 2 
C) 9 
D) 4 
E) 3 
A) 1 
B) 2 
C) 9 
D) 4 
E) 3

Question 7

Give the value of l for a 3p sublevel.

Accepted Answer

A) 1 
B) 0 
C) -1 
D) 2 
E) -2 
A) 1 
B) 0 
C) -1 
D) 2 
E) -2

Question 8

Choose the paramagnetic species from below.

Accepted Answer

A) Ti4+ 
B) O 
C) Ar 
D) All of the above are paramagnetic. 
E) None of the above is paramagnetic. 
A) Ti4+ 
B) O 
C) Ar 
D) All of the above are paramagnetic. 
E) None of the above is paramagnetic.

Question 9

Calculate the energy of the orange light emitted,per photon,by a neon sign with a frequency of 4.89 × 1014 Hz.

Accepted Answer

A) 3.09 × 10-19 J 
B) 6.14 × 10-19 J 
C) 3.24 × 10-19 J 
D) 1.63 × 10-19 J 
E) 5.11 × 10-19 J 
A) 3.09 × 10-19 J 
B) 6.14 × 10-19 J 
C) 3.24 × 10-19 J 
D) 1.63 × 10-19 J 
E) 5.11 × 10-19 J

Question 10

No two electrons can have the same four quantum numbers.What is this known as?

Accepted Answer

A) Pauli exclusion principle 
B) Hund's rule 
C) aufbau principle 
D) Heisenberg uncertainty principle 
A) Pauli exclusion principle 
B) Hund's rule 
C) aufbau principle 
D) Heisenberg uncertainty principle

Question 11

Which of the following statements is TRUE?

Accepted Answer

A) We can sometimes know the exact location and speed of an electron at the same time. 
B) All orbitals in a given atom are roughly the same size. 
C) Since electrons have mass,we must always consider them to have particle properties and never wavelike properties. 
D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped,they take on a spherical shape. 
A) We can sometimes know the exact location and speed of an electron at the same time. 
B) All orbitals in a given atom are roughly the same size. 
C) Since electrons have mass,we must always consider them to have particle properties and never wavelike properties. 
D) Atoms are roughly spherical because when all of the different shaped orbitals are overlapped,they take on a spherical shape.

Question 12

What are the possible values of l if n = 6?

Accepted Answer

A) 6 
B) 0,1,2,3,4,or 5 
C) -4,-3,-2,-1,0,+1,+2,+3,or +4 
D) -5,-4,-3,-2,-1,0,+1,+2,+3,+4,or +5 
A) 6 
B) 0,1,2,3,4,or 5 
C) -4,-3,-2,-1,0,+1,+2,+3,or +4 
D) -5,-4,-3,-2,-1,0,+1,+2,+3,+4,or +5

Question 13

Which of the following transitions (in a hydrogen atom)represent absorption of the smallest frequency photon?

Accepted Answer

A) n = 5 to n = 6 
B) n = 5 to n = 4 
C) n = 4 to n = 1 
D) n = 1 to n = 3 
E) n = 1 to n = 2 
A) n = 5 to n = 6 
B) n = 5 to n = 4 
C) n = 4 to n = 1 
D) n = 1 to n = 3 
E) n = 1 to n = 2

Question 14

Determine the shortest frequency of light required to remove an electron from a sample of Ti metal if the binding energy of titanium is 3.14 × 103 kJ mol-1.

Accepted Answer

A) 7.87 × 1015 Hz 
B) 4.74 × 1015 Hz 
C) 2.11 × 1015 Hz 
D) 1.27 × 1015 Hz 
E) 6.19 × 1015 Hz 
A) 7.87 × 1015 Hz 
B) 4.74 × 1015 Hz 
C) 2.11 × 1015 Hz 
D) 1.27 × 1015 Hz 
E) 6.19 × 1015 Hz

Question 15

Calculate the wavelength of an electron (m = 9.11 × 10-28 g)moving at 3.66 × 106 m s-1.

Accepted Answer

A) 1.99 × 10-10 m 
B) 5.03 × 10-10 m 
C) 1.81 × 10-10 m 
D) 5.52 × 10-9 m 
E) 2.76 × 10-9 m 
A) 1.99 × 10-10 m 
B) 5.03 × 10-10 m 
C) 1.81 × 10-10 m 
D) 5.52 × 10-9 m 
E) 2.76 × 10-9 m

Question 16

Give the number of valence electrons for Mg2+.

Accepted Answer

Question 17

Identify the set of four quantum numbers that could represent the last electron added (using the aufbau principle)to form the Ne atom.

Accepted Answer

A) n = 3,l = 1,ml = 1,ms = + $\frac{1}{2}$ 
B) n = 3,l = 0,ml = 1,ms = - $\frac{1}{2}$ 
C) n = 3,l = 2,ml =1 ,ms = + $\frac{1}{2}$ 
D) n = 2,l = 1,ml = 1,ms = - $\frac{1}{2}$ 
E) n = 3,l =2 ,ml = 1,ms = - $\frac{1}{2}$ 
A) n = 3,l = 1,ml = 1,ms = + $\frac{1}{2}$ 
B) n = 3,l = 0,ml = 1,ms = - $\frac{1}{2}$ 
C) n = 3,l = 2,ml =1 ,ms = + $\frac{1}{2}$ 
D) n = 2,l = 1,ml = 1,ms = - $\frac{1}{2}$ 
E) n = 3,l =2 ,ml = 1,ms = - $\frac{1}{2}$

Question 18

Calculate the wavelength of light emitted from a hydrogen atom when an electron undergoes an n = 8 to n = 4 transmission.

Accepted Answer

A) 1940 nm 
B) 2620 nm 
C) 1.245 × 103 nm 
D) 3.178 × 103 nm 
E) 714.8 nm 
A) 1940 nm 
B) 2620 nm 
C) 1.245 × 103 nm 
D) 3.178 × 103 nm 
E) 714.8 nm

Question 19

Choose the valence orbital diagram that represents the ground state of Sr2+.

Accepted Answer

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

Question 20

Which of the following visible colours of light has the longest wavelength?

Accepted Answer

A) blue 
B) green 
C) yellow 
D) red 
E) violet 
A) blue 
B) green 
C) yellow 
D) red 
E) violet

Exam 7: The Quantum-Mechanical Model of the Atom

Identify the correct values for a 4f sublevel.

Choose the valence orbital diagram that represents the ground state of Zn.

Describe the shape of a p orbital.

An electron ends in orbital n = 3 after a hydrogen atom emits a photon with a wavelength of 1093 nm.Calculate the initial orbital,ni.

What total energy (in kJ)is contained in 1.0 mol of photons,all with a frequency of 2.75 × 1014 Hz?

How many sublevels are contained in the second shell (n = 2)of a given atom?

Give the value of l for a 3p sublevel.

Choose the paramagnetic species from below.

Calculate the energy of the orange light emitted,per photon,by a neon sign with a frequency of 4.89 × 1014 Hz.

No two electrons can have the same four quantum numbers.What is this known as?

Which of the following statements is TRUE?

What are the possible values of l if n = 6?

Which of the following transitions (in a hydrogen atom)represent absorption of the smallest frequency photon?

Determine the shortest frequency of light required to remove an electron from a sample of Ti metal if the binding energy of titanium is 3.14 × 103 kJ mol-1.

Calculate the wavelength of an electron (m = 9.11 × 10-28 g)moving at 3.66 × 106 m s-1.

Give the number of valence electrons for Mg2+.

Identify the set of four quantum numbers that could represent the last electron added (using the aufbau principle)to form the Ne atom.

Calculate the wavelength of light emitted from a hydrogen atom when an electron undergoes an n = 8 to n = 4 transmission.

Choose the valence orbital diagram that represents the ground state of Sr2+.

Which of the following visible colours of light has the longest wavelength?

Units of Measurement for Physical and Chemical Change

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Molecules,compounds,and Nomenclature

Chemical Reactions and Stoichiometry

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Chemical Bonding I: Lewis Theory

Chemical Bonding II: Molecular Shapes, valence Bond Theory, and Molecular Orbital Theory

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Organic Chemistry I: Structures

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Filters

An electron ends in orbital n = 3 after a hydrogen atom emits a photon with a wavelength of 1093 nm.Calculate the initial orbital,n_i.

What total energy (in kJ)is contained in 1.0 mol of photons,all with a frequency of 2.75 × 10¹⁴ Hz?

Calculate the energy of the orange light emitted,per photon,by a neon sign with a frequency of 4.89 × 10¹⁴ Hz.

Determine the shortest frequency of light required to remove an electron from a sample of Ti metal if the binding energy of titanium is 3.14 × 10³ kJ mol^-1.

Calculate the wavelength of an electron (m = 9.11 × 10^-28 g)moving at 3.66 × 10⁶ m s^-1.

Give the number of valence electrons for Mg²⁺.

Choose the valence orbital diagram that represents the ground state of Sr²⁺.