atoms to molecules
Determine the frequencies that hydrogen atoms emit in transitions from n = 6 and n = 5 levels to the n = 3 level. For the H atom, En = –2.18x10–18 J/n2.
What is the frequency (in Hz) of light emitted in the transition from n = 6 to n = 3 level in hydrogen?
Hz
The number of significant digits is set to 3; the tolerance is +/-1%
What is the frequency (in Hz) of light emitted in the transition from n = 5 to n = 3 level in hydrogen?
Hz
The number of significant digits is set to 3; the tolerance is +/-1%
In what region of the electromagnetic spectrum do these photons lie? The answer consists of only one word. Do not abbreviate the name of the spectral region.
Microwave ovens use radiation whose wavelength is 12.5 cm.
What is the frequency (Hz) of this radiation?
Hz
The number of significant digits is set to 3; the tolerance is +/-2%
What is the energy (kJ·mol–1) of this radiation?
kJ·mol–1
The number of significant digits is set to 3; the tolerance is +/-2%
If you know an electron has ml = –2, which of the following is true? (Select all that apply):
A. n ≥ l +1
B. l
C. n ≤ l
D. l ≥ 2
What is the orbital designation corresponding to the following sets of n and l?
n = 4, l = 0
n = 3, l = 2
n = 2, l = 1
n = 5, l = 3
1. 2p
2. 4s
3. 3d
4. 5f
The energy of the n=2 He+ ion is the same as the energy of the n=1 orbital of the hydrogen atom. Select all that is true to answer this question.
A. orbital energy is independent of n
B. orbital energy is independent of Z
C. both n and Z are equal to 2 for the He+ ion
D. both n and Z are equal to 1 for the hydrogen atom
Which of the following sets of quantum numbers are acceptable?
A. n = 3, l = 2, ml = –3
B. n = 3, l = 1, ml = 0
C. n = 3, l = –1, ml = 1
D. n = 3, l = 1, ml = 2
E. n = 3, l = 2, ml = –1
In which chemical species would you expect the strongest bond: C2+ ; F2+; O2+?
A. C2+
B. O2+
C. F2+
Select the electronic molecular orbital configuration for that species.
A. (ss)2 (ss*)2 (sp)2 (px)2 (py)2 (px*)1
B. (ss)2 (ss*)2 (px)2 (py)2 (sp)2 (px*)1
C. (ss)2 (ss*)2 (px)2 (py)2 (sp)2 (px*)0
Calculate the bond order for that species.
1,2,3,1.5,3.5,0.5,2.5
Select the electron configuration for O2–.
(ss)2 (ss*)2 (sp)2 (px)2 (py)2 (px*)2 (py*)1
(ss)2 (ss*)2 (sp)2 (px)2 (py)2 (px*)1
(ss)2 (ss*)2 (px)2 (py)2 (sp)2 (px*)2 (px*)2 (py*)1
The bond order is
and the number of unpaired electrons for O2– is