Mock Final Exam ANSWERS S2008

Mock Final Exam ANSWERS S2008 - Final Exam Review Answers...

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Final Exam Review Answers By: Rima Patel Spring 2008 Electron Configurations and Quantum Numbers: 1. What is the electron configuration for the ground state 24 Cr? a. [Ar] 4s 2 4d 4 b.[Ar] 4s 2 3d 4 c. [Ar] 4s 1 3d 5 d.[Ar] 4s 1 4d 5 You would expect [Ar] 4s 2 3d 5 . However, if you draw this out you will see that the 3d shell is quite unstable as the d-orbital is missing one electron since it only has 4. According to Hund’s Rule, every orbital in a subshell is singly occupied with one electron before any orbital is doubly occupied. Though this has been satisfied with this model, it is NOT the correct configuration. The atom desires stability, which it achieves when an electron “jumps” from the 4s shell to the 3d shell. 2. An atom has a valence shell electron configuration of ns 2 , which group of elements does it belong to? a.Alkaline earth metals b.Transition metals c. Halogens d.Alkali metals Review: Group Special Name Designation 1A Alkaline Metals ns 1 2A Alkaline Earth Metals ns 2 3A None np 1 4A None np 2 5A None np 3 6A None np 4 7A Halogens np 5 8A Noble Gases np 6 3. The electronic structure 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 4 refers to the ground state of a. Zn b.Ga - c. Ge - d. Br + e. Kr 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 4 has 34 electrons total
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Zn: 30 electrons Incorrect Ga - : 31 + 1 = 32 electrons Incorrect Ge - : 32 + 1 = 33 electrons Incorrect Br + : 35 – 1 = 34 electrons Correct Kr: 36 electrons Incorrect 4. Which electron configuration is impossible? a. 1s 2 2s 2 2p 6 3s 2 b.1s 2 2s 2 2p 6 3s 2 3p 6 c. 1s 2 2s 2 2p 3 2d 2 d.1s 2 2s 2 2p 5 3s 1 e. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 5 1s 2 2s 2 2p 6 3s 2 : Mg Possible 1s 2 2s 2 2p 6 3s 2 3p 6 : Ar Possible 1s 2 2s 2 2p 3 2d 2 : 2d shell does not exist Impossible 1s 2 2s 2 2p 5 3s 1 : Excited state of Ne Possible 1s 2 2s 2 2p 6 3s 2 3p 6 4s 1 3d 5 : Cr Possible 5. Which one of these quantum number sets is not possible? a. n=4, l =3, m l =0 b.n=4, l =3, m l =-2 c. n=3, l =2, m l =0 d. n=2, l =1, m l =-2 e. n=2, l =0, m l =0 Quantum Numbers: n = denotes energy: 1=s-orbital, 2=p-oribtal, 3=d-orbital, etc l = denotes angular momentum: 0…n-1 m l = denotes orientation: -l…+l s = denotes spin: +1/2, -1/2 n=4, l =3, m l =0: Possible n = 4 l = 0 to 3 m l = -3 to +3 n=4, l =3, m l =-2: Possible n = 4 l = 0 to 3 m l = -3 to +3 n=3, l =2, m l =0: Possible n = 3 l = 0 to 2 m l = -2 to +2
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n=2, l =1, m l =-2: Not Possible n = 2 l = 0 to 1 m l = -1 to +1 n=2, l =0, m l =0: Possible n = 2 l = 0 to 1 m l = -1 to +1
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6. Which of the following set of quantum numbers is not possible? a. n=1, l =0 m l =0 b.n=4, l =3 m l =-2 c. n=3, l =2 m l =0 d.n=2, l =0 m l =0 e. n=2, l =1 m l =-2 Quantum Numbers: n = denotes energy: 1=s-orbital, 2=p-oribtal, 3=d-orbital, etc l = denotes angular momentum: 0…n-1 m l = denotes orientation: -l…+l s = denotes spin: +1/2, -1/2 n=1, l =0 m l =0: Possible n = 1 l = 0 m l = 0 n=4, l =3 m l =-2: Possible n = 4 l = 0 to 3 m l = -3 to +3 n=3, l =2 m l =0: Possible
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Mock Final Exam ANSWERS S2008 - Final Exam Review Answers...

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