Electron and Orbitals

Question 1

What is the Bohr Model?

Answer 1

• A theoretical model for the hydrogen atom
• Based on the planetary model

Question 2

Which energy level/shell (n) has the lowest energy?

Answer 2

The n=1 shell

Question 3

What is a Shell?

Answer 3

• “n” value
• Distance from the nucleus

Question 4

What does a Subshell do?

Answer 4

• determines the orbital shape
• labelled as s, p, d, f
• each subshell is found in a specific section on the periodic table

Question 5

What is the Orbital/Boundary Diagram used for?

Answer 5

The probability of finding an electron

Question 6

What is the maximum amount of electrons in an orbital

Answer 6

A maximum of two electrons per orbital

Question 7

What waves do we treat electrons as?

Answer 7

A standing wave

Question 8

What does the Schrodinger Equation describe?

Answer 8

It describes the wave-particle duality of electrons

Question 9

What is the Heisenberg Uncertainty Principle?

Answer 9

It is impossible to know exactly both the position and momentum of an object (can only know one, not both)

Question 10

What is a Standing Wave?

Answer 10

Waves that are fixed at each end

Question 11

What is the probability of finding an electron in Nodes?

Answer 11

0% probability of finding an electron

Question 11

What are Nodes?

Answer 11

Areas of destructive interference

Question 12

What kind of nodes do “s” orbitals have?

Answer 12

Spherical Nodes

Question 13

What kind of nodes do “p” orbitals have?

Answer 13

Planar Nodes

Question 14

What kind of nodes do “d” orbitals have?

Answer 14

Planar Nodes

Question 15

Which energy level (n) can you find each type of orbital?

Answer 15

• ”s” orbitals can be found in n=1 and onward
• “p” orbitals can be found in n=2 and onward
• “d” orbitals can be found in n=3 and onward

Question 16

What is the “s” orbital shape?

Answer 16

Spherical

Question 17

The 3 “p” orbitals are similar in?

Answer 17

Shape/size and energy

Question 18

The 3 “p” orbitals differ in?

Answer 18

Orientation

Question 19

“p” and “d” orbitals are names based on the?

Answer 19

Named based on the x, y, z orientation

Question 20

The “d” orbital lobes are located in?

Answer 20

The planes

Question 21

How many “d” orbital shapes are there?

Answer 21

There are 5 “d” orbital shapes

Question 22

What should you include in Electron Configuration?

Answer 22

Indicate shell (n), subshell, and # of electrons in the subshell
(e.g. 1s¹)

Question 23

What is an Orbital Box Diagram?

Answer 23

Indicate shell, subshell, then in a box show spin for electrons

Question 24

What is an Energy Diagram?

Answer 24

Indicates increasing energy in shells for everything but H (3 “d” is higher energy than 4 “s” orbital), shell, subshell, and spin for electrons

Question 25

What is Aufbau’s Principle?

Answer 25

Fill from lower to higher energy orbitals (1s, 2s, 2p)

Question 26

What is the Pauli Exclusion Principle?

Answer 26

No two electrons can have the same spin in the same orbital

Question 27

What is Hund’s Rule

Answer 27

Unpaired electrons in the same energy level must have parallel spins, put one in each orbital first before pairing

Question 28

What does degenerate mean?

Answer 28

The same amount of energy

Question 29

How to write a shorthand electron configuration?

Answer 29

Write the closest noble gas to the atom, then write the remaining (valence electrons) shell, subshell, and electrons
(e.g. [Ar] 4s¹ for K)

Question 30

What are valence electrons?

Answer 30

Valence electrons are the electrons located on the outermost shell

Question 31

Which atoms typically lose electrons?

Answer 31

Cation (positive charge) loses electrons and groups 1, 2, and 13

Question 32

Which atoms typically gain electrons?

Answer 32

Anions (negative charge) gain electrons and groups 15, 16, 17.

Question 33

What does it mean to be isoelectronic?

Answer 33

When two or more molecular entities have the same amount of electrons and/or electronic configuration despite having different elements or charges.