Which of the following statements about quantum theory is incorrect?
A.
The energy and position of an electron cannot be determined simultaneously.
B.
Lower energy orbitals are filled with electrons before higher energy orbitals.
C.
When filling orbitals of equal energy, two electrons will occupy the same orbital before filling a new orbital.
D.
No two electrons can have the same four quantum numbers.
E.
All of these are correct.
2.
Which of the following statements is true?
A.
The exact location of an electron can be determined 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 2 unpaired electrons in its 3d orbitals.
D.
In the buildup of atoms, electrons occupy the 4f orbitals before the 6s orbitals.
E.
Only three quantum numbers are needed to uniquely describe an electron.
3.
Which of the following statements is false?
A.
An orbital can accommodate at most two electrons.
B.
The electron density at a point is proportional to psi2 at that point.
C.
The spin quantum number of an electron must be either +1/2 or –1/2.
D.
A 2p orbital is more penetrating than a 2s; i.e., it has a higher electron density near the nucleus and inside the charge cloud of a 1s orbital.
E.
In the usual order of filling, the 6s orbital is filled before the 4f orbital.
4.
How many f orbitals have the value n = 3?
A.
0
B.
3
C.
5
D.
7
E.
1
5.
How many electrons in an atom can have the quantum numbers n = 3,
l = 2?
A.
2
B.
5
C.
10
D.
18
E.
6
6.
How many electrons can be described by the quantum numbers n = 3,
l = 3, ml= 1?
A.
0
B.
2
C.
6
D.
10
E.
14
7.
Which of the following is incorrect?
A.
The continuous spectrum of hydrogen contains only four discrete colors.
B.
Diffraction produces both constructive and destructive interference.
C.
All matter displays both particle and wavelike characteristics.
D.
Niels Bohr developed a quantum model for the hydrogen atom.
E.
The lowest possible energy state of a molecule or atom is called its ground state.
8.
How many d orbitals have n = 3?
A.
2
B.
5
C.
10
D.
7
E.
18
9.
How many electrons in an atom can have the quantum numbers n = 4,
l = 2?
A.
14
B.
12
C.
5
D.
10
E.
6
10.
Which of the following is an incorrect designation for an atomic orbital?
A.
1s
B.
3d
C.
1p
D.
4f
E.
6s
11.
Which of the following combinations of quantum numbers do not represent permissible solutions of the Schroedinger equation for the electron in the hydrogen atom (i.e., which combination of quantum numbers is not allowed)?
n
l
ml
s (or ms)
A.
9
8
–4
1/2
B.
8
2
2
1/2
C.
6
–5
–1
1/2
D.
6
5
–5
1/2
E.
All are allowed.
12.
Which of the following atoms or ions has 3 unpaired electrons?
A.
N
B.
O
C.
Al
D.
S2–
E.
Zn2+
13.
The electron configuration for the barium atom is:
A.
1s22s22p63s23p63d104s2
B.
[Xe] 6s2
C.
1s22s22p63s23p64s1
D.
1s22s22p63s23p64s2
E.
none of these
14.
The electron configuration for the carbon atom is:
A.
1s22s22p2
B.
[He] 2s4
C.
[Ne] 2s22p2
D.
1s22p4
E.
none of these
15.
The electron configuration of indium is
A.
1s22s22p63s23p63d104s24p64d105s25p15d10
B.
1s22s22p63s23p63d104s24d104p1
C.
1s23s22p63s23p64s24p64d105s25d105p1
D.
1s22s22p63s23p63d104s24p64d105s25p1
E.
none of these
16.
If
l= 3, how many electrons can be contained in all the possible orbitals?
A.
7
B.
6
C.
14
D.
10
E.
5
17.
Which of the following combinations of quantum numbers is not allowed?
n
l
ml
ms
A.
1
1
0
1/2
B.
3
0
0
–1/2
C.
2
1
–1
1/2
D.
4
3
–2
–1/2
E.
4
2
0
1/2
18.
The electron configuration for Cr2+ is
A.
[Ar]4s23d4
B.
[Ar]4s13d5
C.
[Ar]3d4
D.
[Ar]4s23d2
E.
none of these
19.
The electron configuration of Ti2+ is
A.
[Ar]4s2
B.
[Ar]4s13d1
C.
[Ar]3d2
D.
[Ar]4s23d2
E.
none of these
20.
Consider the following sets of quantum numbers. Which set(s) represent(s) impossible combinations?
n
l
ml
ms
Set a
1
0
1
+1/2
Set b
3
3
0
+1/2
Set c
2
1
1
–1/2
Set d
3
2
–2
–1/2
Set e
3
1
–2
–1/2
Set f
2
0
0
–1/2
Answer:
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