[Ar] a b c d e f g h i ( a,b,c,d,e,f are all filled g,h are half filled and i is

Question

[Ar]                   

          a                  b        c         d       e         f                   g       h        i

( a,b,c,d,e,f are all filled g,h are half filled and i is empty)

(A) Refer to orbital a.

(1) Specify a set of quantum numbers that can be used to represent one of the electrons in orbital a.

(2) Will the set of quantum numbers that represents the second electron in orbital a be different? Explain.

(3) What is the maximum number of electrons that can occupy the principal energy level that contains orbital a?

(B) Refer to orbitals b,c,d,e,and f.

(1) What is the number of sublevels in the principal energy level that includes orbital d?

(2) What is the range of signs and values for the mlquantum numbers for electrons in orbitals b,c,d,e,and f

(C) What is the range of signs and values for the l quantum numbers in orbitals g,h,andi?

(D) From which orbitals will electrons be removed when the Germanium atom is converted to the Ge+4 ion?

Consider the distribution of electrons in the orbitals of a ground-state germanium atom as shown below ( a,b,c,d,e,f are all filled g,h are half filled and i is empty) Refer to orbital a. Specify a set of quantum numbers that can be used to represent one of the electrons in orbital a. Will the set of quantum numbers that represents the second electron in orbital a be different? Explain. What is the maximum number of electrons that can occupy the principal energy level that contains orbital a? Refer to orbitals b,c,d,e,and f. What is the number of sublevels in the principal energy level that includes orbital d? What is the range of signs and values for the ml quantum numbers for electrons in orbitals b,c,d,e,and f What is the range of signs and values for the l quantum numbers in orbitals g,h,andi? From which orbitals will electrons be removed when the Germanium atom is converted to the Ge+4 ion?

Explanation / Answer

Electron configuration of Ge = 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p2 5s0

A)

1)   1,0,0,+1/2 or 1,0,0,-1/2

2) Yes. Spin quantum number will be different for either of the electrons.

3) 2. Its 1st orbit and it contains only one orbital S. so maximum 2 electrons.

B)

1) orbital d is 3s2.
Principal energy level = 3

hence number of subleverls = 3 (s,p,d)

2) b,c,d,e,f all have range of azimuthal quantum numbers, 0,1

range of ml wud be -l <= ml <= l

hence range here is {-1,0,1}

C) g,h,i

range of l wud be s,d,p orbitals..

so range is {0,1,2}

D)

When an element ionizes to form a cation, the electrons are lost from the orbitals with the highest energy.

Ge (ground state) --> [Ar] 3d10, 4s2 4p2
Ge (+4 ion) ----------> [Ar] 3d10

The four electrons are lost from the orbitals with the highest energy, the 4s and 4p.
hence f and h.

Hope ths helps :)

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