Question 1

Give the number of core electrons for Mg2+.

Accepted Answer

Question 2

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

Accepted Answer

The energies of atoms are quantized.When

Question 3

How many different values of ml are possible in the 4$f$ sublevel?

Accepted Answer

A) 1 
B) 7 
C) 3 
D) 5 
E) 2 
A) 1 
B) 7 
C) 3 
D) 5 
E) 2

Question 4

Which of the following transitions represent the emission of a photon with the largest energy?

Accepted Answer

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

Question 5

How many subshells are there in the shell with n = 4?

Accepted Answer

A) 3 
B) 4 
C) 6 
D) 18 
A) 3 
B) 4 
C) 6 
D) 18

Question 6

What value of l is represented by a d orbital?

Accepted Answer

A) 1 
B) 2 
C) 0 
D) 3 
A) 1 
B) 2 
C) 0 
D) 3

Question 7

Determine the velocity of a marble (m = 8.66 g)with a wavelength of 
3.46 × 10-33 m.

Accepted Answer

A) 45.2 m s-1 
B) 11.3 m s-1 
C) 22.1 m s-1 
D) 38.8 m s-1 
E) 52.9 m s-1 
A) 45.2 m s-1 
B) 11.3 m s-1 
C) 22.1 m s-1 
D) 38.8 m s-1 
E) 52.9 m s-1

Question 8

Which of the following quantum numbers describes the shape of an orbital?

Accepted Answer

A) principal quantum number 
B) magnetic quantum number 
C) spin quantum number 
D) Schrödinger quantum number 
E) angular momentum quantum number 
A) principal quantum number 
B) magnetic quantum number 
C) spin quantum number 
D) Schrödinger quantum number 
E) angular momentum quantum number

Question 9

An electron initially in the n = 5 orbital of a hydrogen atom emits a photon with a wavelength of 1284 nm.Calculate the final orbital,nf.

Accepted Answer

A) 1 
B) 3 
C) 2 
D) 6 
E) 4 
A) 1 
B) 3 
C) 2 
D) 6 
E) 4

Question 10

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10-2 nm-1.

Accepted Answer

A) 656.3 nm 
B) 486.2 nm 
C) 364.6 nm 
D) 2.057 × 10-3 nm 
A) 656.3 nm 
B) 486.2 nm 
C) 364.6 nm 
D) 2.057 × 10-3 nm

Question 11

How many photons are contained in a flash of green light (525 nm)that contains 189 kJ of energy?

Accepted Answer

A) 5.67 × 1023 photons 
B) 2.01 × 1024 photons 
C) 1.25 × 1031 photons 
D) 4.99 × 1023 photons 
E) 7.99 × 1030 photons 
A) 5.67 × 1023 photons 
B) 2.01 × 1024 photons 
C) 1.25 × 1031 photons 
D) 4.99 × 1023 photons 
E) 7.99 × 1030 photons

Question 12

Choose the ground-state electron configuration for Ti2+.

Accepted Answer

A) [Ar]3d2 
B) [Ar]4s2 
C) [Ar]4s23d2 
D) [Ar]4s23d4 
E) [Ar]3d4 
A) [Ar]3d2 
B) [Ar]4s2 
C) [Ar]4s23d2 
D) [Ar]4s23d4 
E) [Ar]3d4

Question 13

Which of the following quantum numbers describes the orientation of an orbital?

Accepted Answer

A) magnetic quantum number 
B) principal quantum number 
C) angular momentum quantum number 
D) spin quantum number 
E) Schrödinger quantum number 
A) magnetic quantum number 
B) principal quantum number 
C) angular momentum quantum number 
D) spin quantum number 
E) Schrödinger quantum number

Question 14

Calculate the orbital for the hydrogen atom that contains an electron with an energy of -2.42 × 10-19 J.

Accepted Answer

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

Question 15

Identify the set of four quantum numbers that could represent the electron lost to form the K ION from the K atom.

Accepted Answer

A) n = 3,l = 1,ml = 1,ms = - $\frac{1}{2}$ 
B) n = 4,l = 1,ml = 1,ms = + $\frac{1}{2}$ 
C) n = 4,l = 4,ml = 0,ms = - $\frac{1}{2}$ 
D) n = 4,l = 0,ml = 0,ms = + $\frac{1}{2}$ 
E) n = 3,l = 0,ml = 1,ms = + $\frac{1}{2}$ 
A) n = 3,l = 1,ml = 1,ms = - $\frac{1}{2}$ 
B) n = 4,l = 1,ml = 1,ms = + $\frac{1}{2}$ 
C) n = 4,l = 4,ml = 0,ms = - $\frac{1}{2}$ 
D) n = 4,l = 0,ml = 0,ms = + $\frac{1}{2}$ 
E) n = 3,l = 0,ml = 1,ms = + $\frac{1}{2}$

Question 16

Describe the shape of an s 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 17

Give an example of a p orbital.

Accepted Answer

The answer of Give an example of a p orbital....

Question 18

An electron ends in orbital n = 4 after a hydrogen atom emits a photon with a wavelength of 2165 nm.Calculate the initial orbital,ni.

Accepted Answer

A) 6 
B) 7 
C) 1 
D) 3 
E) 2 
A) 6 
B) 7 
C) 1 
D) 3 
E) 2

Question 19

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

Accepted Answer

A) n = 4,l = 3,ml = 3,ms = - $\frac{1}{2}$ 
B) n = 3,l = 2,ml = 2,ms = - $\frac{1}{2}$ 
C) n = 3,l = 1,ml = 1,ms = + $\frac{1}{2}$ 
D) n = 3,l = 3,ml = 2,ms = - $\frac{1}{2}$ 
E) n = 4,l = 2,ml = 0,ms = + $\frac{1}{2}$ 
A) n = 4,l = 3,ml = 3,ms = - $\frac{1}{2}$ 
B) n = 3,l = 2,ml = 2,ms = - $\frac{1}{2}$ 
C) n = 3,l = 1,ml = 1,ms = + $\frac{1}{2}$ 
D) n = 3,l = 3,ml = 2,ms = - $\frac{1}{2}$ 
E) n = 4,l = 2,ml = 0,ms = + $\frac{1}{2}$

Question 20

Define paramagnetic.

Accepted Answer

Paramagnetic is when

Exam 7: The Quantum-Mechanical Model of the Atom

Give the number of core electrons for Mg2+.

Why do atoms only emit certain wavelengths of light when they are excited? (Why do line spectra exist?)

How many different values of ml are possible in the 4 fff sublevel?

Which of the following transitions represent the emission of a photon with the largest energy?

How many subshells are there in the shell with n = 4?

What value of l is represented by a d orbital?

Determine the velocity of a marble (m = 8.66 g)with a wavelength of 3.46 × 10-33 m.

Which of the following quantum numbers describes the shape of an orbital?

An electron initially in the n = 5 orbital of a hydrogen atom emits a photon with a wavelength of 1284 nm.Calculate the final orbital,nf.

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10-2 nm-1.

How many photons are contained in a flash of green light (525 nm)that contains 189 kJ of energy?

Choose the ground-state electron configuration for Ti2+.

Which of the following quantum numbers describes the orientation of an orbital?

Calculate the orbital for the hydrogen atom that contains an electron with an energy of -2.42 × 10-19 J.

Identify the set of four quantum numbers that could represent the electron lost to form the K ION from the K atom.

Describe the shape of an s orbital.

Give an example of a p orbital.

An electron ends in orbital n = 4 after a hydrogen atom emits a photon with a wavelength of 2165 nm.Calculate the initial orbital,ni.

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

Define paramagnetic.

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Filters

Give the number of core electrons for Mg²⁺.

How many different values of m_l are possible in the 4 $f$ sublevel?

Determine the velocity of a marble (m = 8.66 g)with a wavelength of 3.46 × 10^-33 m.

An electron initially in the n = 5 orbital of a hydrogen atom emits a photon with a wavelength of 1284 nm.Calculate the final orbital,n_f.

For hydrogen,what is the wavelength of the photon emitted when an electron drops from a 4d orbital to a 2p orbital in a hydrogen atom? The Rydberg constant is 1.097 × 10^-2 nm^-1.

Choose the ground-state electron configuration for Ti²⁺.

Calculate the orbital for the hydrogen atom that contains an electron with an energy of -2.42 × 10^-19 J.

An electron ends in orbital n = 4 after a hydrogen atom emits a photon with a wavelength of 2165 nm.Calculate the initial orbital,n_i.