Question 1. 1. The orbital with n = 2 and l = 0 is: (Points : 1) 1s 2s 2p 3s Que

Question

Question 1. 1. The orbital with n = 2 and l = 0 is: (Points : 1)       1s
      2s
      2p
      3s

Question 2. 2. The azimuthal quantum number (l) of a d subshell is: (Points : 1)       0
      1
      3
      2

Question 3. 3. Which of the following values of the magnetic quantum number (m) is not possible for a 3p orbital? (Points : 1)       0
      -1
      2
      1

Question 4. 4. What are the values of the principal quantum number (n) and the azimuthal quantum number (l) of a 4f subshell? (Points : 1)       3, 2
      4, 2
      4, 3
      4, 1

Question 5. 5. Which of the following sets of quantum numbers is not possible? (Points : 1)       n = 1, l = 0, m = 0
      n = 2, l = 1, m =  -1
      n = 2, l = 0, m = 0
      n = 3, l = 3, m = 1

Question 6. 6. What is the value of 'l' for a g subshell? (Points : 1)       3
      4
      2
      1

Question 7. 7. How many electrons in an atom can have the quantum numbers 'n = 3, l = 2' ? (Points : 1)       10
      8
      6
      2

Question 8. 8. Which of the following orbitals is not possible? (Points : 1)       3d
      2s
      5p
      3f
Question 1. 1. The orbital with n = 2 and l = 0 is: (Points : 1)       1s
      2s
      2p
      3s

Explanation / Answer

Q1. 2S

Q2. 2

Q3. 2

Q4. 4,3

Q5. n=3, l=3,m=1

Q6. 4

Q7. 10

Q8. 3f

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