Font size
WorksheetsQuantum, Orbitals, & Electron Configuration Practice
Total questions: 35
Worksheet time: 53mins
We know that sublevels in the principle energy levels (according to our notes) have different shapes. How many positions or shapes does the "f" suborbital have?
1 shape and it is spherical
3 shapes or positions and it looks like a peanut or figure eight.
5 shapes
7 shapes
We know that sublevels in the principle energy levels (according to our notes) have different shapes. How many positions or shapes does the "d" suborbital have?
1 shape and it is spherical
3 shapes or positions and it looks like a peanut or figure eight.
5 shapes
7 shapes
Which suborbital has three different shapes or orientations?
s
p
d
f
If n=2, then what is the largest suborbital in this energy level? HINT: Check your notes for the two orbitals at this energy level.
s
p
d
f
If n=2, what suborbital(s) are present? Hint: Total number of electrons for n=2 is 8 electrons.
s
p
d
s and p
p and d
Which quantum number tells me the shape of the suborbital?
n, also known as the principal #
l (lower case L), also known as the angular momentum quantum #
ml or (m, sub L), also known as the the magnetic quantum #
ms or (m, sub s), also known as the spin quantum #
None of the above
Which magnetic quantum number is a "code" for the orbital, d?
0
-1, 0, 1
-2, -1, 0, 1, 2
-3, -2, -1, 0, 1, 2, 3
If n=3, the spin, ms or (m, sub s) for an electron is ___.
3
0, 1, 2
-3, -2, -1, 0, 1, 2, 3
+1/2 or -1/2
none of the above
An atom has 10 protons and 10 electrons therefore it is the element Ne. It has an n=2 energy level. what is the third quantum number, or "magnetic quantum number", ml or (m, sub L)?
2
0 and 1
-1, 0, 1
-1/2 or +1/2
None of the above
Which set of four quantum numbers is NOT correct?
n=1,
l=0,
m(l) =0,
m(s) =+1/2
n=2,
l=1,
m(l) =-1,0,1
m(s) =+1/2
n=3,
l=2,
m(l) =-2,-1,0,1,2
m(s) =+1/2
n=1
l=1
m(l)=-1,0,1
m(s)=+1/2
Which of the following is a definition for the Pauli Exclusion Principle?
The electrons in an atom must fill the lowest energy suborbital FIRST before moving to the next energy suborbital
No two electrons can have the SAME 4 quantum numbers
When electrons are filling more than one suborbital in an energy level, they must do so "one at a time", before going back and completing the pair.
Which of the following is a definition for Aufbau Principle?
The electrons in an atom must fill the lowest energy suborbital FIRST before moving to the next energy suborbital.
No two electrons can have the SAME 4 quantum numbers
When electrons are filling more than one suborbital in an energy level, they must do so "one at a time", before going back and completing the pair.
Which of the following is a good definition for Hund's Rule?
The electrons in an atom must fill the lowest energy suborbital FIRST before filling the next energy suborbital.
No two electrons can have the same 4 quantum numbers.
When electrons are filling more than one suborbital in an energy level, they must do so "one at a time", before going back and completing the pair
Which of the following electron configurations is for the element "S" or sulfur?
1s2, 2s2, 2p6, 3s2
1s2, 2s2, 2p6
1s2, 2s2, 2p4
1s2, 2s2, 2p6, 3s2, 3p6
1s2, 2s2, 2p6, 3s2, 3p4
If n = 3, what is the maximum number of electrons that can fit in this shell?
2
8
18
32
What orbital is shown in the picture?
s
p
d
f
What orbital is shown in the picture?
s
p
d
f
What orbital shape is in the image?
s
p
d
f
When atoms _____________ energy, their electrons move to higher energy levels. These electrons _____________ energy by emitting light when they return to lower energy levels.
lose, absorb
absorb, lose
lose, lose
absorb, absorb
What electron configuration matches an oxygen atom?
1s22s22p63s2, 3p64s23d104p5
1s22s22p4
1s22s22p6
1s22s22p63s23p64s23d1
The electron configuration of an atom is 1s22s22p6. The number of electrons in the atom is
3
6
8
10
Which electron configuration belongs to Chlorine (Cl)?
1s2 2s2 2p6 3s2 3p5
1s2 2s2 2p6 3s2 3p6
1s2 2s2 2p6 3s2 3p7
How many electrons can the d-sublevel hold?
3
5
7
10
How many electrons can the s-sublevel hold?
1
2
6
10
What atom matches this electron configuration? 1s22s22p63s23p64s23d10
Zine
Copper
Nickel
Germanium
What element is pictured?
Neon
Magnesium
Fluorine
Argon
What is incorrect about the orbital diagram?
Both arrows in the first 2p box should be pointing down
There is nothing incorrect with this diagram
In the 2p box there should only be 1 up arrow in the first box, 1 up arrow in the 2nd box, & 1 up arrow in the 3rd box
All the arrows should be pointing up for all boxes
Which pair of orbital has the same shape?
2s and 2p
2s and 3s
3p and 3d
More than one is correct.
An ion is an element that loses or gains _____.
Protons
Neutrons
Electrons
Atomic #
Mass #
Which is the electron configuration for the ion, Ca+2
1s2, 2s2, 2p6, 3s2, 3p6
1s2, 2s2, 2p6
1s2, 2s2, 2p6, 3s2
1s2, 2s2, 2p6, 3s2, 3p6, 4s2
The electron configuration, 1s2, 2s2, 2p6, 3s2, 3p6, is for which ion?
Mg+2
Al+3
N-3
S-2
Which element would use the Noble Gas, [Kr] as a `short cut' for the electron configuration?
K, Potassium
Ag, Silver
Cu, Copper
Cl, Chlorine
Complete the following electron configuration for As, Arsenic:
[Ar], 4s2, 3d10, (a) .
