Electronic Structure and ionisation energy

Question 1

How many orbitals in the a subshell ?

Answer 1

1

Question 2

How many orbitals in the p subshell ?

Answer 2

3

Question 3

How many orbitals in the d subshell ?

Answer 3

5

Question 4

How many orbitals in the f subshell ?

Answer 4

7

Question 5

Electrons fill up the what energy sublevels first

Answer 5

Lowest

Question 6

What’s special about 3D and 4s ?

Answer 6

4s has lower energy level so it is filled up first

Question 7

In orbitals describe the motion of the electrons

Answer 7

The electrons spin in opposite directions

Question 8

How do electrons full orbitals ?

Answer 8

Singly before they start sharing

Question 9

What is the electron configuration for chromium ?

Answer 9

3d^5, 4s^1

Question 10

What is the electron configuration for copper ?

Answer 10

3d^10 4s^1

Question 11

Why do copper and chromium donate one of their 4s electrons to the 3D sub shell ?

Answer 11

They’re happier with a more stable full or half full d sub shell

Question 12

What else is special about transition metals ?

Answer 12

They loose their 4s electrons beige their 3D electrons even though the 4s electron she’ll is filled first

Question 13

What is ionisation energy ?

Answer 13

The enthalpy change needed to remove 1 mole of electrons from 1 mole of gaseous atoms

Question 14

What is the equation for the first ionisation energy ?

Answer 14

X(g) –> X+(g) +e-

Question 15

What are the 3 factors affecting ionisation energy ?

Answer 15

Nuclear charge , distance from the nucleus and shielding

Question 16

How does nuclear charge effect ionisation energy ?

Answer 16

The more protons there are in the nucleus the more positively charged the nucleus is and the stronger the attraction for the electrons.

Question 17

How does distance from nucleus effect the ionisation energy ?

Answer 17

The closer the electron is to the nucleus the more strongly it will be attracted to the nucleus

Question 18

How does shielding effect ionisation energy ?

Answer 18

As the number of electrons between the outer electrons and the nucleus increases the outer electrons feel less attraction towards the nuclear charge. This lessens the pull of the nucleus

Question 19

What does successive ionisation energy involve ?

Answer 19

Removing additional electrons

Question 20

What is the definition of second ionisation energy ?

Answer 20

The enthalpy change required to removed 1 mole of electrons from 1 mole of gaseous ions to for 2+ ions

Question 21

Why within each she’ll do successive ionisation energies increase ?

Answer 21

As the electrons are being removed from and increasingly positive ion with less repulsion amongst the remaining electrons so they are held strongly by the nucleus

Question 22

Why are there big jumps when new shells are broken into ?

Answer 22

An electron is being removed from a shell that is closer to the nucleus

Question 23

What is the trend in first ionisation energy as you go down a group ?

Answer 23

The first ionisation energy decreases

Question 24

What is the trend in first ionisation energy as you go across a period ?

Answer 24

Increases

Question 25

What do graphs showing first ionisation energy energy down a group provide evidence for ?

Answer 25

That electron shells exist

Question 26

Why is it that ionisation energy decreases as you go down group 2 ?

Answer 26

Bea she there is shielding from the inner shells which shields the outer electrons from the attraction of the nucleus Also the extra shells mean that the outer electrons are further away from the nucleus do the nucleus' attraction will be greatly reduced.

Question 27

Why is it that as you go across the period the ionisation energy increases ?

Answer 27

This is due to change of the nucleus increasing as number of protons increases so there is a stronger nuclear attraction. All the extra electrons are at roughly the same energy level ( similar shielding )

Question 28

Why is there a small drop from magnesium to aluminium in ionisation energy as you go across period 3 ?

Answer 28

Because aluminium a outer electron is in a 3p orbital rather than 3s. 3p orbital has a slightly higher energy than 3s orbital. So the electron is on avenger further from the nucleus Also the 3p orbital has the additional shielding from the 3s^2 electrons

Question 29

In period 3 why is there a drop between group 5 and group 6 ( phosphorus and sulfur) ?

Answer 29

This is due to electron repulsion Shielding is identical Phosphorus soured electron is removed from a singly occupied orbital whereas in sulphur the electron is being removed from an orbital containing 2 electrons. More repulsion - easier to remove

Question 30

What is 1 mole ?

Answer 30

6.02 X 10^23

Question 31

What is the equation to find out mass , moles and mr?

Answer 31

Mass = mrx mole

Question 32

What is the equation for concentration ?

Answer 32

Concentration = moles/volume

Question 33

In the concentration calculation what is volume measures in ?

Answer 33

Dm ^3

Question 34

What is the units for concentration ?

Answer 34

Mol dm ^-3

Question 35

How do u convert cm^3 into dm^3 ?

Answer 35

Divide by 1000

Question 36

What is the ideal has equation ?

Answer 36

pV =nRT

Question 37

What is the unites for pressure ?

Answer 37

Pa

Question 38

What is the units for volume in the idea has equation ?

Answer 38

M^3

Question 39

What is the units for temperature in the ideal gas equation ?

Answer 39

K

Question 40

How do u convert degrees Celsius into k ?

Answer 40

+ 273

Question 41

What's the maximum number of electrons can orbitals hold ?

Answer 41

2