Question

What is the designation for an orbital with the following
quantum numbers: *n* = 2 and *l* = 0

How many unpaired electrons are in the ground state electron configuration for chromium? Your answer should be one number.

Answer #1

1) n=2 (principle quantum number)

l = 0 (s orbital)

**designation for an orbital = 2 s**

**2)** chromium configuration = 1s2 2s2 2p6 3s2 3p6
3d5 4s1

number of unpaired electrons = 5 from d -orbital + 1 from s orbital

**= 6**

Question 3
Part B:How many values of ml are possible for an
electron with orbital quantum number l = 1?
Express your answer as an integer.
Part C
The quantum state of a particle can be specified by giving a
complete set of quantum numbers (n,l,
ml,ms). How many different
quantum states are possible if the principal quantum number is
n = 2?
To find the total number of allowed states, first write down the
allowed orbital quantum numbers l,...

For the 3d state (orbital) of the hydrogen atom, the principal
quantum number n=3. The orbital quantum number l = 2. For an
electron with these quantum numbers, what is the smallest angle (in
degrees) that an electron's spin axis (angular momentum axis) can
make with respect to an applied magnetic field?

1) A quantum harmonic oscillator with frequency
Ď‰contains 41 electrons. What is the energy of the
highest-energy electron? Assume that the electrons are in the
lowest states possible.
2 a) An atom has a total of 18 electrons. What is the principal quantum number of the
outermost shell?
2 b) How many electrons
does the outermost shell shell contain?
3) Which of the following represents the possible range of
integer values for the magnetic quantum number?
a) 1 to l...

Each of the following sets of quantum numbers is supposed to
specify an orbital. Choose the one set of quantum numbers that's
does NOT contain an error
A. n = 2, l = 2, m = -1
B. n = 4, l = 4, m = 2
C. n = 2, l = 2, m = 0
D. n= 4, l = 2, m = -2
E. n = 3, l = 2, m = 3

The quantum state of a particle can be specified by giving a
complete set of quantum numbers (n,l,
ml,ms). How many different
quantum states are possible if the principal quantum number is
n = 2?
To find the total number of allowed states, first write down the
allowed orbital quantum numbers l, and then write down the
number of allowed values of ml for each orbital quantum
number. Sum these quantities, and then multiply by 2 to account for
the...

What are the possible values of n and ml for an electron in a 3d
orbital?
A) n = 1, 2, or 3 and ml = 2
B) n = 1, 2, or 3 and ml = -2, -1, 0, +1, or +2
C) n = 3 and ml = 2
D) n = 4 and ml = -2, -1, 0, +1, +2
Each of the following sets of quantum numbers is supposed to
specify an orbital. Choose the one...

Part C
The quantum state of a particle can be specified by giving a
complete set of quantum numbers (n,l,
ml,ms). How many different
quantum states are possible if the principal quantum number is
n = 2?
To find the total number of allowed states, first write down the
allowed orbital quantum numbers l, and then write down the
number of allowed values of ml for each orbital quantum
number. Sum these quantities, and then multiply by 2 to account...

Part C
The quantum state of a particle can be specified by giving a
complete set of quantum numbers (n,l, ml,ms). How many different
quantum states are possible if the principal quantum number is n =
4?
To find the total number of allowed states, first write down the
allowed orbital quantum numbers l, and then write down the number
of allowed values of ml for each orbital quantum number. Sum these
quantities, and then multiply by 2 to account...

1. How many electrons could occupy a subshell with the following
quantum numbers?
a. n=2, l=1
b. n=2, l=0, ml=0
2. How many orbitals are described by each of the below
combinations of quantum numbers?
a. n=3, l=3
b. n=4, l=2, ml=2
3. How many milliliters of 0.100 M HNO3 are needed to neutralize
the following solutions?
a. 34.7 mL of 0.775 M NaOH
b. 58.5 mL of 0.0100 M Al(OH)3
4. How many milliliters of 0.100 M NaOH are...

For the following atoms, write the ground-state orbital
diagrams, the electron configurations, and the
condensed electron configurations. Finally, state the number of
unpaired electrons.
(a) Nitrogen
(b) Sodium
(c) Argon
(d) Titanium
(e) Zinc

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