Calculate the wavelength of light emitted when each of the following transitions occur in the hydrogen atom.
(a) n = 4> n = 3
nm
(b) n = 3> n = 1
nm
(c) n = 5> n = 2
nm
The ionization energy of gold is 890.1 kJ/mol. Is light with a wavelength of 240. nm capable of ionizing a gold atom (removing an electron) in the gas phase?
Yes
No
maximum wavelength that can ionize a gold atom in nano meters?
An excited hydrogen atom emits light with a frequency of 1.141 1014 Hz to reach the energy level for which n = 4. In what principal quantum level did the electron begin?
Calculate the maximum wavelength of light capable of removing an electron for a hydrogen atom from the energy state characterized by the followingn in nano meters
n = 5
n = 7
Which of the following orbital designations are incorrect?
1s correct
incorrect
1p correct
incorrect
7d correct
incorrect
9s correct
incorrect
3f correct
incorrect
4f correct
incorrect
2d correct
incorrect
Which of the following sets of quantum numbers are not allowed in the hydrogen atom? For the sets of quantum numbers that are incorrect, indicate what is wrong in each set.
(a) n = 3, = 2, m = 2
allowed
not allowed, n is not valid
not allowed, is not valid
not allowed, m is not valid
(b) n = 4, = 3, m = 4
allowed
not allowed, n is not valid
not allowed, is not valid
not allowed, m is not valid
(c) n = 0, = 0, m = 0
allowed
not allowed, n is not valid
not allowed, is not valid
not allowed, m is not valid
(d) n = 2, = -1, m = 1
allowed
not allowed, n is not valid
not allowed, is not valid
not allowed, m is not valid
How many orbitals in an atom can have the following designation?
5p
3dz2
4d
n = 5
n = 4
Give the maximum number of electrons in an atom that can have these quantum numbers.
(a) n = 4
(b) n = 3
(c) n = 2, = 1, m = -1, ms = -1/2
(d) n = 1, = 0, m = 0
(e) n = 2, = 2
Write the expected electron configurations for each of the following atoms. (Type your answer in noble gas notation using the format [Ar] 4s2 3d10 4p2 for [Ar]4s23d104p2.)
Tc
Ta
W
Am
Sr
As
A certain oxygen atom has the electron configuration 1s22s22px22py2. How many unpaired electrons are present?
Is this an excited state of oxygen?
Yes
No
In going from this state to the ground state would energy be released or absorbed?
Energy would be released.
Neither, the oxygen atom is in the ground state.
Energy would be absorbed.
Which of the following electron configurations correspond to an excited state? Identify the atoms and write the ground-state electron configuration where appropriate. (For 'element' enter the name or symbol of the element that corresponds to the given electron configuration. For 'electron configuration' either enter the words 'ground state', if the configuration given is a ground state configuration; or enter the proper ground state configuration for the element, if the configuration given represents an excited state. Type your answer using the format [Ar] 4s2 3d10 4p2 for [Ar]4s23d104p2.)
(a) 1s22s23p1
element (Enter the element name or symbol.)
electron configuration (Enter the words 'ground state' or the correct ground state configuration -- see instructions.)
(b) 1s22s22p6
element
electron configuration
(c) 1s22s22p43s1
element
electron configuration
(d) [Ar]4s23d54p1
element
electron configuration
How many unpaired electrons are present in each of these excited species and their ground state configurations?
(a) 1s22s23p1
ground-state
(b) 1s22s22p6
ground-state
(c) 1s22s22p43s 1
ground-state
(d) [Ar]4s23d54p1
ground-state
(a) Na, Rb, Be
---Select--- Rb Na Be < ---Select--- Rb Na Be < ---Select--- Rb Na Be
(b) Ne, Sr, Se
---Select--- Sr Se Ne < ---Select--- Sr Se Ne < ---Select--- Sr Se Ne
(c) P, Fe, O
---Select--- Fe P O < ---Select--- Fe P O < ---Select--- Fe P O
In each of the following sets, which atom or ion has the smallest ionization energy?
(a) Cs, Ba, La
Cs
La
Ba
(b) Zn, Ga, Ge
Zn
Ge
Ga
(c) In, P, Ar
In
P
Ar
(d) Tl, Sn, As
Tl
Sn
As
(e) O, O-, O2-
O-
O2-
O
For each of the given pairs of elements, pick the atom with the following characteristics.
(Mg and K)
(a) more favorable (exothermic) electron affinity
K
Mg
(b) higher ionization energy
K
Mg
(c) larger size
K
Mg
(F and Cl)
(a) more favorable (exothermic) electron affinity
Cl
F
(b) higher ionization energy
Cl
F
(c) larger size
Cl
F
For each of the given pairs of elements, pick the atom with the following characteristics.
(Mg and K)
(a) more favorable (exothermic) electron affinity
K
Mg
(b) higher ionization energy
K
Mg
(c) larger size
K
Mg
(F and Cl)
(a) more favorable (exothermic) electr
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