Models of the Atom
Quantum Theory
Quantum Theory
Electron Configuration
Electron Configuration
100

the amount of energy needed to move an electron from one energy level to another energy level

What is a quantum

100

the sublevel that has a shape that consists of two dumbbells

What is d.

100

the spin quantum number says that the number of spins an electron can have is

What is 2

100

the technique of writing electron configurations with arrows is known as

What is orbital notation or orbital diagrams

100
the rule that says two electrons in the same orbital in the same sublevel can not have the same spin state.
What is Pauli's exclusion principle
200

when an electron moves from a higher energy level to a lower energy level, energy is _____________.

What is released (in the form of a photon)

200

the number of electrons that can fill the sublevel 4f

What is 14

200

which of the following locations of an electron is not possible: 3s, 4f, 3d, 1p, 2p, 1s

What is 1p

200
the rule that states electrons will fill separate orbitals in the same energy level first before pairing up in the same orbital
What is Hund's rule
200
the rule that states electrons will fill the lowest energy levels first
What is aufbau's principle
300

the equation that tells us the energy of a photon

What is E = hv

300

The four letters that represent electron locations

What is 1. principle quantum number: tells you the energy level (n=1, n=2,...) 2. Sublevels found in each energy level (s,p,d,f) 3. The number of orbitals found in each sublevel (s=1, p=3, d=5, f=7) 4. The Spin: two electrons per orbital that spin in opposite directions

300

the number of electrons needed to completely fill the 4th energy level

What is 32

300
write the electron configuration (not orbital notation or noble gas notation) for Germanium (Atomic Number 32)
What is 1s(2), 2s(2), 2p(6), 3s(2), 3p (6), 4s(2), 3d(10), 4p (2)
300
Give the noble gas notation for Potassium
What is [Ar] 4s(1)
400

Why is it that we see a certain color of light from certain atoms when their electrons are excited and allowed to relax?

because the energy is quantified into orbitals and the electrons only exist in certain locations because that is the wave function that allows them to exist

400

give the number of orbitals that can be found in the main energy level of 3.

What is 9 (s=1, p=3, d=5)

400

the sublevels that are known to exist in the 6th energy level

What is s, p, d, f

400
using an orbital diagram show how an example that would violate Hund's rule of the orbital diagram of Nitrogen (Atomic Number 7)
What is diagram would have two paired electrons instead of each in its own orbital in the 2p sublevel
400

show an orbital diagram that would violate the Pauli exclusion principle for Mg (Atomic Number 12)

What is 2 arrows in the same orbital that are both up or both down

500

the difference between Bohr's model of the atom and the quantum mechanical model of the atom (the second model you learned about)

What is Bohr: electrons are found in a circular orbit in a fixed location, QMM: the exact location of an electron can not be found but instead the electron cloud can show the orbital where it is most likely to be found

500

the number of electrons in the outermost energy level of an oxygen atom

What is 6

500

if an element has 15 electrons in the third energy level, how many more electrons does it need to fill the third energy level.

What is 3.

500
name the element with the following electron configuration by using the periodic table method: [Xe] 4f (14), 5d (10),6s(2),6p (3)
What is Bi (bismuth)
500

how many electrons does an element have with and electron configuration of [Ar] 3d(4),4s(2)

What is 24.

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