Question 1

How many orbitals are there in the fourth shell?

Accepted Answer

A) 3 
B) 4 
C) 6 
D) 16 
A) 3 
B) 4 
C) 6 
D) 16

Question 2

Give an example of a p orbital.

Accepted Answer

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

Question 3

Describe the shape of an s orbital.

Accepted Answer

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

Question 4

Choose the valence orbital diagram that represents the ground state of Se2⁻.

Accepted Answer

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

Question 5

How many photons are contained in a burst of yellow light (589 nm)from a sodium lamp that contains 609 kJ of energy?

Accepted Answer

A) 3.37 × 1019 photons 
B) 3.06 × 1030 photons 
C) 1.80 × 1024 photons 
D) 4.03 × 1028 photons 
E) 2.48 × 1025 photons 
A) 3.37 × 1019 photons 
B) 3.06 × 1030 photons 
C) 1.80 × 1024 photons 
D) 4.03 × 1028 photons 
E) 2.48 × 1025 photons

Question 6

Calculate the velocity of a pickup truck with a de Broglie wavelength of 1.27 × 10-38 m and a mass of 2347 kg.

Accepted Answer

A) 88 km h-1 
B) 62.1 km h-1 
C) 94 km h-1 
D) 79.9 km h-1 
E) 106 km h-1 
A) 88 km h-1 
B) 62.1 km h-1 
C) 94 km h-1 
D) 79.9 km h-1 
E) 106 km h-1

Question 7

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. Whe

Question 8

Only two electrons, with opposing spins, are allowed in each orbital. 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 9

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 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) The emission spectrum of a particular element is always the same and can be used to identify the element. 
B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. 
C) The uncertainty principle states that we can never know both the exact location and speed of an electron. 
D) An orbital is the volume in which we are most likely to find an electron. 
E) All of the above are true. 
A) The emission spectrum of a particular element is always the same and can be used to identify the element. 
B) Part of the Bohr model proposed that electrons in the hydrogen atom are located in "stationary states" or particular orbits around the nucleus. 
C) The uncertainty principle states that we can never know both the exact location and speed of an electron. 
D) An orbital is the volume in which we are most likely to find an electron. 
E) All of the above are true.

Question 12

In which orbital below would an electron (on average)be farthest from the nucleus?

Accepted Answer

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

Question 13

Calculate the energy change associated with the transition from n = 4 to n = 1 in the hydrogen atom.

Accepted Answer

A) +4.89 × 10-18 J 
B) +1.64 × 10-18 J 
C) -6.12 × 10-18 J 
D) +3.55 × 10-18 J 
E) -2.04 × 10-18 J 
A) +4.89 × 10-18 J 
B) +1.64 × 10-18 J 
C) -6.12 × 10-18 J 
D) +3.55 × 10-18 J 
E) -2.04 × 10-18 J

Question 14

Determine the energy change associated with the transition from n = 3 to n = 2 in the hydrogen atom.

Accepted Answer

A) +3.03 × 10-19 J 
B) -1.82 × 10-19 J 
C) +5.51 × 10-19 J 
D) -3.03 × 10-19 J 
E) +2.69 × 10-19 J 
A) +3.03 × 10-19 J 
B) -1.82 × 10-19 J 
C) +5.51 × 10-19 J 
D) -3.03 × 10-19 J 
E) +2.69 × 10-19 J

Question 15

In which orbital below would an electron (on average)be closest to the nucleus?

Accepted Answer

A) 2p 
B) 4s 
C) 2s 
D) 5d 
E) 3p 
A) 2p 
B) 4s 
C) 2s 
D) 5d 
E) 3p

Question 16

Give the number of core electrons for Mg2+.

Accepted Answer

Question 17

Sketch one of the 3p orbitals below. How are they different from the 2p orbitals?

Accepted Answer

They are larger in s

Question 18

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 19

How many different values of ml are possible in the 3d sublevel?

Accepted Answer

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

Question 20

How many orbitals are contained in the n = 2 level? Give the l and ml values of each of them.

Accepted Answer

Four. The 2s and three 2p orbi

Exam 7: The Quantum-Mechanical Model of the Atom

How many orbitals are there in the fourth shell?

Give an example of a p orbital.

Describe the shape of an s orbital.

Choose the valence orbital diagram that represents the ground state of Se2⁻.

How many photons are contained in a burst of yellow light (589 nm)from a sodium lamp that contains 609 kJ of energy?

Calculate the velocity of a pickup truck with a de Broglie wavelength of 1.27 × 10-38 m and a mass of 2347 kg.

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

Only two electrons, with opposing spins, are allowed in each orbital. What is this known as?

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

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

Which of the following statements is TRUE?

In which orbital below would an electron (on average)be farthest from the nucleus?

Calculate the energy change associated with the transition from n = 4 to n = 1 in the hydrogen atom.

Determine the energy change associated with the transition from n = 3 to n = 2 in the hydrogen atom.

In which orbital below would an electron (on average)be closest to the nucleus?

Give the number of core electrons for Mg2+.

Sketch one of the 3p orbitals below. How are they different from the 2p orbitals?

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

How many different values of ml are possible in the 3d sublevel?

How many orbitals are contained in the n = 2 level? Give the l and ml values of each of them.

Units of Measurement for Physical and Chemical Change

Atoms and Elements

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Chemical Bonding I: Lewis Theory

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Filters

Choose the valence orbital diagram that represents the ground state of Se²⁻.

Calculate the velocity of a pickup truck with a de Broglie wavelength of 1.27 × 10^-38 m and a mass of 2347 kg.

Give the number of core electrons for Mg²⁺.

Choose the valence orbital diagram that represents the ground state of Sr^2⁺.

How many different values of m_l are possible in the 3d sublevel?

How many orbitals are contained in the n = 2 level? Give thel and m_l values of each of them.