Quantum Leaps
It's the Principles of the Matter
sO pLEASE dON'T fUSS
EZ ECs
I've seen the lights!
100
Name the 4 quantum numbers and what they each represent.
What is the n (energy level), l (angular/shape), m (magnetic/orientation), and ms (spin)
100
The principle that states that electrons must fill lower energy orbitals before filling higher energy orbitals.
What is Aufbau's Rule?
100
Name the orbital shapes in order from lowest to highest energy and list the maximum number of electrons that can occupy each subshell.
What are s, p, d, and f? 2, 6, 10, 14.
100
Name that element:
[Ar]4s2 3d3
What is V for Vanadium
100
Give the name of the man who can help you remember the order of the colors of the rainbow from lowest to highest energy.
Who is ROY G. BIV?
200
If an element is in the f block, give the l value and the possible m values.
What are l = 3 and m = -3, -2, -1, 0, 1, 2, 3?
200
The principle that states that an electron's position and velocity cannot be simultaneously known.
What is Heisenberg's Principle?

200
Give the l value for the d-block, the number of orientations that d-orbitals can have, and what special consideration must be made for its n-values.
l = 2
5 orientations
n = period number - 1
200
The full electron configuration for an ion of Calcium.
What is
1s2 2s2 2p6 3s2 3p6?
200

Explain why the green lights are brighter than the yellow lights in this foggy street?

The photons from the green light have a higher energy and therefore, a higher frequency than the yellow and red lights.
300
Using the following quantum numbers, identify the element:

n= 4
l= 1
m= 0
ms= -1/2

What is Br?
300
In this principle, every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
What is Hund's Rule?
300
Define the term "orbital"
The approximate area that an electron is most likely to occur in an atom at ground state.
300
The noble gas configuration for Seaborgium
What is [Rn]7s2 5f14 6d4?
300
Describe what atomic adsorption and emission are and what is produced as a result.
Adsorption: an electron becomes excited and moves to a higher energy level from ground state.

Emission: an electron releases energy in the form of a photon as it moves from the excited state back to ground state. The emitted photons create a line emission spectrum specific to the electrons' atom.

400
Using the following quantum numbers, identify the element:

n= 5
l= 2
m= 0
ms= +1/2

What is Ta?
400
The principle that states that no two electrons in an atom can have identical quantum numbers.
What is the Pauli Exclusion Principle?
400
How many electrons can fit in n =4?
What is 32?
(2 + 6 + 10 + 14)
400
Which of the following is a correct orbital diagram and which element is indicated?

What is Option B and Oxygen?
400
Describe how line emission spectroscopy is useful for element identification.
Line emissions from unknown elements being excited can be compared with known line emission spectrums.
500
Identify the quantum numbers for the element Cd (Cadmium)
n= 4
l= 2
m= 2
ms= -1/2
500
What did the Photoelectric Effect prove?
Light travels both as a particle and as a wave.
500
What is the correct order for the following subshells: 4s, 4p, 3d, 3s
What is 3s, 4s, 3d, 4p.
500
The electron configuration for Fe2+
What is 1s2 2s2 2p6 3s2 3p6 3d6
500
What are the two types of ions called and generally how can you determine what charge an element will have?
Cations are positive (PAW-sitive!) and Anions are negative. Generally, metals will form positive charges and nonmetals will form negative charges. The charge number is determined by the number of electrons lost or gained to reach a full octet.
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