Atomic And Molecular Orbitals

Question 1

What can an electron be described as

Answer 1

Question 2

What can a wave function tell you about an electron

Answer 2

Can tell you where an electron is

Question 3

What can a radial electron distribution graph tell you about an electron

Answer 3

Question 4

What does the square of the wave function tell you

Answer 4

Electron density

Question 5

What shape are s orbitals

Answer 5

Sphere

Question 6

What is the equation for calculating electrostatic potential energy (coulombs law) and what does each component of the equation mean

Answer 6

Question 7

What does it mean if q1 is negative and q2 is positive (coulombs law)

Answer 7

Question 8

What does it mean if q1 and q2 are both negative

Answer 8

Question 9

What is the diagram for a 2p orbital

Answer 9

Question 10

What is aufbaus principle

Answer 10

Question 11

What is the Pauli exclusion principle

Answer 11

2 electrons per orbital, spins paired
Electrons have to have opposite spins

Question 12

What is hunds rule

Answer 12

Due to repulsion between electrons
So electrons wouldn’t hate an orbital if there are empty orbitals of the same energy

Question 13

Why is the electron in the 1s orbital most favourable

Answer 13

Closest to nucleus → low energy → high attraction
As energy increases → less favourable (so electron would be lost more easily)

Question 14

As nuclear charge increases, why does the energy become more favourable

Answer 14

Question 15

Why is the outermost electrons in groups 1 and 2 lost easily

Answer 15

That electron is in a high energy orbital
(Has a lower attraction to the nucleus)

Question 16

What would a wave function diagram look like for 2 molecular orbitals which are both positive (and are moving up and down in synchrony)

Answer 16

Question 17

What would a wave function diagram for 2 molecular orbitals (which have combined), where one orbital is positive and the other is negative (so they are out of synchrony), look like? Show where the chance of an electron bring present would be zero

Answer 17

Question 18

Why would 2 orbitals with wave functions that are out of synchrony not form a bond. What is this called

Answer 18

The elections are repelling and only interacting with one nuclei
The wave functions are interacting but no bond is formed this is called antibonding

Question 19

In a molecular orbital, where would an electron most likely be found

Answer 19

Question 20

What is one property of molecular orbitals

Answer 20

They are cylindrically symmetrical so if you flip them head still be the same shape

Question 21

What happens if the antibording orbital has a greater number or same amount of electrons as the bonding orbital

Answer 21

The molecule wont form because in order for the bond to form the number of electrons in the bonding orbital has to be greater than the number of electrons in the antibonding orbital

Question 22

Draw the energy level diagram for diatomic hydrogen molecule

Answer 22

Question 23

What is the condition for two atoms to share a pair of electrons

Answer 23

Question 24

What forms when 2 atomic orbitals overlap

Answer 24

Question 25

What is a molecular orbital

Answer 25

Question 26

How many electrons can a molecular and atomic orbital hold

Answer 26

2

Question 27

What does electrons in a bonding orbital do?
What does electrons in an antibonding orbital do?

Answer 27

Question 28

What condition must be met for a covalent bond to form

Answer 28

Question 29

What is a non bonding orbital

Answer 29

Question 30

What are the two types of molecular orbital

Answer 30

Sigma and pi

Question 31

What are the 4 types of atomic orbital

Answer 31

Spdf

Question 32

What does * mean Ontop of a peak on a radial electron distribution graph

Answer 32

Most likely position of an electron (in angstroms e.g * at 2 angstrom= position of electron is two angstroms)