The Electron Configuration: Quantum Numbers

How many p electrons does Se (atomic number 34) possess? 1. 6 2. 10 3. 12 4. 4 5. 0 6. 34 7. 16 

Give the set of four quantum numbers that could represent the electron last added to the configuration for nitrogen. A) n = 2, ℓ = 1, m ℓ = 1, m s = -1/2 B) n =1, ℓ = 1, m ℓ = 1, m s = +1/2 C) n = 3, ℓ = 4, m ℓ = 0, m s = -1/2 D) n = 2, ℓ = 1, m ℓ = 0, m s = +1/2 

Give the set of three quantum numbers that could represent the last electron added to the Sr atom. A. n = 5, l = 0, ml = 0 B. n = 4, l = 1, ml = 1 C. n = 5, l = 1, ml = 0 D. n = 4, l = 1, ml = -1 E. n = 5, l = 2, ml =1

What is the set of correct quantum numbers (n, ℓ, m ℓ) for the last electron P –? 1. 3, 1, –1 2. 2, 0, 1 3. 3, 1, -2 4. 3, 2, 1 5. 2, 0, 0 6. 3, 0, 0 7. 2, 1, 1 8. 3, 2, 0

Consider an atom of Zirconium (Zr) where the electrons are in the ground state. How many electrons would be in orbitals that are spherical in shape?                                 A. 2                B. 10                C. 17               D. 20                 E. 25

Give the set of four quantum numbers that represent the indicated electron in each of the following elements:  Al (11th electron)            n =                     , l =                  ,    m l =             ,  m s =      

Give the set of four quantum numbers that represent the indicated electron in each of the following elements:  Se (32nd electron)          n =                     , l =                  ,    m l =             ,  m s =            

Give the set of four quantum numbers that represent the indicated electron in each of the following elements:  Cr (23rd electron)            n =                     , l =                  ,    m l =             ,  m s =     

Which set of quantum numbers,  n, ℓ, m ℓ , could correspond to one of the highest energy electrons in Zr? 1. 4, 2, +3 2. 3, 2, -2 3. 4, 3, -2  4. 4, 2, -2

What are the correct quantum numbers ( n, ℓ, m ℓ ) for the seventh electron of Cl? 1. 3, 1, 0 2. 2, 1, 1 3. 3, 0, 0 4. 3, 1, 1 5. 2, 0, 1 6. 2, 1, 2 7. 2, 2, 1 8. 3, 2, 1

How many p electrons does Se (atomic number 34) possess? 1. 6 2. 10 3. 12 4. 4 5. 0 6. 34 7. 16

How many electrons are in the third principal level ( n = 3 ) of a chromium (Cr) atom? 1. 8 2. 4 3. 24 4. 2 5. 13 6. 6 7. 12  

Which of the following statements is true? A. The 2s and 2p orbitals for the hydrogen atom have the same energy.B. The energy of electromagnetic radiation increases as its frequency decreases.C. An electron in the n=1 state in the hydrogen atom can go to the n=3 state by emitting electromagnetic radiation at the appropriate frequency.D. The exact position and velocity of an electron can be measured simultaneously from accurate experiments.E. In the usual order of filling, the 3 d orbital is filled before the 3s orbital for transition metal elements.

The four quantum numbers (n, ℓ, mℓ , ms) for the last two electrons added to complete the electron configuration if Si are:a. (2,1,-1,½) and (2,1,0,½)b. (3,1,-1,½) and (3,1,0,½)c. (3,0,-1,½) and (3,1,0,½)d. (3,2,-2,½) and (3,2,-1,-½)e. (2,0,0,½) and (2,0,0,-½) 

Which statement about atomic orbitals and quantum numbers is correct?A. The maximum number of orbitals with the quantum number n = 3 is 18.B. There are five 2d orbitals.C. The angular momentum quantum number is related to the shape of the orbital.D. A 4f orbital is not possible.E. None of the above are true.

Fluorine can gain an electron to become fluoride (F−). What is the quantum number (following the numbering conventions) that describes the electron that was gained by fluorine.(a) n = 2,  ℓ  = 0, m ℓ  = 1, ms = -1⁄2(b) n = 2, ℓ = 1,  m ℓ  = 0, ms = -1⁄2(c) n = 3, ℓ = 1, m ℓ = 1, ms = +1⁄2(d) n = 2, ℓ = 1,  m ℓ  = 1, ms = -1⁄2(e) n = 2, ℓ = 1,  m ℓ  = -1, ms = -1⁄2

Which of the following sets of the four quantum numbers n, l, m  l, and ms decribes one of the outermost electrons in a ground-state barium atom?a) 6, 1, 1, ½b) 6, 0, 1, -½c) 6, 0, 0, -½d) 6, 1, 0, ½e) 6, 2, 1, -½

Which electron configuration represents a violation of the  Pauli Exclusion Principle? 

Give the set of four quantum numbers that represent the indicated electron in each of the following elements: Br – (30th electron)          n =                     , l =                  ,    m l =             ,  m s =          

Which of the following represents a set of quantum number for valence electron of Chlorine?A. (3,1,0,-1)B. (3, 2, 0, -1/2)C. (3,0,2, 1/2)D. (3,1,-1, -1/2)E. (3,1,0,0)

According to the Aufbau principle, what are the values of principal quantum number ( n ) and angular momentum quantum number ( l ) for the sub-level that is filled  AFTER the 4s orbital?A. n = 3, l = 2B. n = 4, l = 2C. n = 4, l = 1D. n = 3, l = 1E. n = 5, l = 0 

Which of the following statements is true?A. We can determine the exact location of an electron if we know its energy.B. An electron in a 2s orbital can have the same n, l, and ml quantum numbers as an electron in a 3s orbital.C. Ni has two unpaired electrons in its 3d orbitals.D. In the building up of atoms, electrons occupy the 4f orbitals before the 6s orbitals.E. Only three quantum numbers are needed to uniquely describe an electron.

Each set is ordered(n,l,ml,ms). Identify the sets of quantum numbers that describe all the electrons in the ground state of a neutral beryllium atom, Be. Each set is ordered(n,l,ml,ms). Choose the appropriate items to their respective bins.

a. How many electrons does a Co atom have in its 3d subshell?b. How many of those electrons are unpaired? 

How many electrons in a Cl atom have an angular momentum quantum number of 0?a. 2b. 4c. 6d. 8e. 10

Which of the following combinations could give the quantum numbers (n, l, ml, ms) for the single valence electron of the copper atom in its ground state?a. 4, 0, 0, 3/2b. 4, 1, 0, 1/2c. 4, 0, 0, - 1/2d. 4, 1, 2, 1/2e. 4, 2, 1, 1/2

Write out the four possible quantum numbers for each of the electrons in the diagram below. Give them in the order of: n, l, ml, and ms.HINT: There are 6 electrons therefore you should give 6 answers.

a. How many electrons does a Mn atom have in its 3d subshell? b. How many of those electrons are unpaired?