Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry Module 2 > Electron Structure > Flashcards

Electron Structure Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What is the maximum amount of electrons that can go into each main shell and what are their energy levels?

A

1- 2 electrons lowest energy
2- 8 electrons
3- 18 electrons
4- 32 electrons highest energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What are shells made up from?

A

Orbitals

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

How many electrons can 1 orbital hold?

A

2 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are the 3 different types of orbitals what shape do they have, how many are there in each sub-shell and what is the max amount of electrons they hold?

A

s orbital- spherical shape
Each sub-level has 1 s orbital
Each s orbital holds 2 electrons

p orbital- dumbbell shape
Each sub-level after level 1 has 3 p orbitals
Each p orbital holds 2 electrons so in each subshell (3x2) holds 6 electrons

d orbital
Each sub-level after 3 has 5 d orbitals
Each d orbital holds 2 electrons so in each subshell (5x2) holds 10 electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

For each main shell name the type and number of each orbitals, the max number of electrons from each type of orbital and the max number of electrons in that shell:

A

1- 1s which holds 2 electrons therefore max number is 2

2- 1s 3p (2+6) so max number is 8

3- 1p 3p 5d (2+6+10) so max number is 18

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is spin and how is it represented?

A

The property of electrons due to them repelling as they have a negative charge
Up and down arrows represent spin

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

What is an orbital?

A

The space around the nucleus that can hold up to 2 electrons of opposite spin

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How is electron configuration written?

A

E.g 3p^6

3 (large number) represents the number of the main shell
p (the letter) represents type of orbital
^6 (the power) represents how many electrons in the sub-shell

Written in order of energy level

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Why is 4s written before 3d?

A

4s has a lower energy level than 3d so is filled 1st

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What are the rules for filling shells and sub-shells?

A
  1. Electrons added 1 at a time
  2. Lowest available energy level fills 1st
  3. Each main shell (usually) is full before the next one starts to fill
  4. In p+d orbitals each orbital fills singly before pairing
  5. Electrons in each orbital have opposite spin
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What are the 2 exceptions to these rules and why?

A

Chromium and copper-
Half-filled and full subshells are more stable so 1 of the electrons from 4s is moved to 3d leaving -
Cr- 4s^1 3d^5
Cu- 4s^1 3d^10

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

In the periodic table what does the block of an element represent?

A

The highest energy sub-shell occupied by an electron

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What is the periodic trend in electron configuration across a period?

A

Each period starts with an electron in the newest highest energy main shell
Across the period the s+p sub shell are filled the same way (repeating pattern)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What is the periodic trend in electron configuration down a group?

A

Elements in the same group have the same number of electrons in outer shell and same number of electrons in each outer sub-shell

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

How are positive cations formed and how does the electron configuration change from atom to ion?

A

Formed when electrons are removed (from highest energy sub-shell 1st)
Electron configuration is shortened as electrons are removed

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

How are negative anions formed and how does this effect the configuration?

A

Formed when electrons move into the lowest unoccupied energy level
Configuration is increased

17
Q

Is the 3d orbital or 4s orbital electrons removed from 1st and why?

A

4s orbitals are empties before 3d as in an ion 4s has a higher energy level than 3d

18
Q

What is atomic radii and what factors effect it?

A

The distance between the centre of the nucleus and the outermost electron.
Factors:
1. Strength of attraction between positive nucleus and negative electron
2. Strength of repulsion between outermost electrons and inner shell electrons (amount of shielding)

19
Q

What is the trend of atomic radii across a group and why?

A

Atomic radii decreases:

  1. Same amount of shielding as electrons added to same outer shell
  2. Increasing attraction between nucleus and electrons as there is an increasing number of protons
20
Q

What is the trend in atomic radii down a group and why?

A

Radii increases:

  1. More shielding as more full inner shells repelling
  2. Decreasing attraction between nucleus and outer electron as outer electron is further away from nucleus due to more inner shells
21
Q

What is ionisation energy?

A

Energy to remove an electron from the highest energy subshell to form positive ions

22
Q

What is the 1st ionisation energy?

A

The energy required to remove 1 electron from each atom in 1 mole of gaseous atoms to form 1 mole of gaseous 1+ ions

23
Q

What factors effect the ionisation energy?

A
  1. Attraction between nucleus and electron

2. Amount of shielding

24
Q

What does the strength of attraction depend on?

A
  1. Atomic radii
  2. Nuclear charge (atomic number)
  3. Electron shielding
25
Q

What are the trends in 1st ionisation energy across a period and why?

A

Ionisation energy increases
1. Same shielding (electron removed from same shell)
2. Stronger attraction (more protons)
So more energy is required to overcome the attraction

26
Q

What is the trend of ionisation energy down a group and why?

A

Ionisation energy decreases

  1. More shielding (more full inner shells repelling)
  2. Decreasing attraction (outer electron is further from the nucleus- larger radii)
27
Q

What are the exceptions for the general trend of 1st ionisation energies across group 2 and why?

A

Al is lower than Mg
Even though Al has more protons
The 3p^1 electron is removed more easily than 3s^2 in Mg as it is in a higher energy level

S has a lower energy than P
Even though S has more protons the 3p^4 electron is removed more easily than the 3p^3 electron in P due to spin.
Less energy is required as the 2 electrons that have been forced in a pair repel which raises the energy

28
Q

What is the 2nd Ionisation energy?

A

The energy required to remove the 2nd electron from 1 mole of gaseous 1+ ions to form 1 mole of gaseous 2+ ions

29
Q

What is the trend of successive ionisation energies and why?

A

The more electrons you remove the harder it becomes to remove the next (ionisation energy increases)
This is because when each electron is removed the shell is drawn closer to the nucleus and as the distance decreases the attraction increases

30
Q

In a successive ionisation graph what does a big jump represent?

A

The big significant increase in ionisation energy shows a jump from 1 subshell to the other

Chemistry Module 2 (10 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions