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Misc.
Quantum Theory
Quantum Theory
Electron Configuration
Electron Configuration
100

Explain the difference between paramagnetic and diamagnetic 

Paramagnetic: wants a pair/ is looking for electrons, AND is attracted to a magnet

Diamagnetic-all e are paired. Full orbitals 

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

Identify the subshell in which electrons with the following quantum numbers are found:

  1. n = 2, l = 1
  2. n = 4, l = 2
  3. n = 6, l = 0

1. 2p

2.4d

3.6s

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

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

released (in the form of a photon) 

300
the 4 quantum numbers and what they mean
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

How many moles are present in 34 grams of Cu(OH)2?

0.35 moles 

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

Valid or Invalid? 

n= 2 l=0 ml=0 ms=-1/2 

n=3 l=1 ml=1. ms=1/2

n=2 l=2  ml=-2 ms=-1/2

1. valid 

2. valid 

3. invalid 

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

Convert 95.0 °C into F

203

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.