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Chemistry Chapters 7, 8, and 9 practice problems
Terms in this set (18)
What are the principle quantum number n?
What does the principle quantum number determine?
n=1,2,3....and so on
it determines the overall size and energy of an orbital
List all the orbitals in each principle level. Specify the three quantum numbers for each orbital.
a. n=1; l=0; ml=0
b. n=2; l=0; ml=0
n=2; l=1; ml=-1, 0, 1
c. n=3, l=0; ml=0
n=3; l=1; ml=-1,0,1
n=3; l=2; ml=-2,-1,0,1,2
d. n=4; l=0; ml=0
n=4; l=1; ml=-1,0,1
n=4; l=2; ml=-2,-1,0,1,2
n=4; l=3; ml=-3,-2,-1,0,1,2,3
List these types of electromagnetic radiation in order of (i) increasing wavelength and (ii) increasing energy per photon
a. radio waves
d. ultraviolet radiation
ultraviolet radiation, infrared radiation, microwaves, radio waves
radio waves, microwaves, infrared radiation, ultraviolet radiation
List these types of electromagnetic radiation in order of (i) increasing frequency and (ii) decreasing energy per photon.
a. gamma rays
b. radio waves
d. visible light
radio waves, microwaves, visible light, gamma rays
gamma rays, visible light, microwaves, radio waves
Calculate the frequency of each wavelength of electromagnetic radiation:
a. 632.8 nm
c. 0.052 nm
a. 4.74×10¹⁴ Hz
b. 5.96×10¹⁴ Hz
c. 5.8×10¹⁸ Hz
Calculate the energy of a photon of electromagnetic radiation at each of the wavelengths:
a. 632.8 nm
c. 0.052 nm
a. 3.14×10⁻¹⁹ J
b. 3.95×10⁻¹⁹ J
c. 3.8×10⁻¹⁵ J
A laser pulse with λ 532 nm contains 3.85 mJ of energy. How many photons are in the laser pulse?
Determine the energy of 1 mol of photons for each kind of light (3 sig figs)
a. infrared radiation (1500 nm)
b. visible light (500 nm)
c. ultraviolet radiation (150 nm)
a. 79.8 kJ/mol
b. 239 kJ/mol
c. 798 kJ/mol
Which electron is on average closer to the nucleus: an electron in a 2s orbital or an electron in a 3s orbital
Which electron is, on average, further from the nucleus: an electron in a 3p orbital or an electron in a 4p orbital
what are the possible values of l for each value of n?
b. l=0 and 1
c. l=0, 1, and 2
d. l=0,1,2,and 3
What are the possible ml values for each value of l?
Which set of quantum number cannot occur together to specify an orbital?
a. n=2; l=1; ml=-1
b. n=3; l=2; ml=0
c. n=3; l=3; ml=2
d. n=4; l=3; ml=0
Which combinations of n and l orbitals represent real orbitals and which do not exist?
d. doesn't exist
An electron in a hydrogen atom is excited with electrical energy to an excited state with n=2. The atom then emits a photon. What is the value of n for the electron following the emission.
According to the quantum-mechanical model for the hydrogen atom, which electron transitions would produce light with the longer wavelength: 2p ->1s or 3p -> 1s
2p -> 1s
Calculate the λ of the light emitted when an electron in a hydrogen atom makes each transition and indicate the region of the electromagnetic spectrum where the light is found.
a. n=2 -> n=1
b. n=3 -> n=1
c. n=4 -> n=2
d. n=5 -> n=2
a. 122 nm, UV
b. 103 nm, UV
c. 486 nm, visible
d. 434 nm, visible
An electron in the n=7 level of the hydrogen atom relaxes to a lower energy level, emitting light of 397 nm. What is the value of n for the level to which the electron relaxed.