Brainscape's Knowledge GenomeTM

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


See full index

AS chemistry AQA > Electronic Structure > Flashcards

Electronic Structure Flashcards

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

What happens in the currently accepted model of the atom?

A
  • electrons have fixed energies
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What do electrons do?

A
  • they move around the nucleus in certain regions of the atom called shells or energy levels
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What is each shell given?

A
  • a principle quantum number
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

The further the shell is from the nucleus………

A
  • the higher its energy and the larger its principle quantum number
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What’s the principle quantum number for the 1st electron shell and describe its energy?

A

1
- this shell has the lowest energy

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

What is the principle quantum number of the 2nd electron shell?

A

2

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

What is the principle quantum number of the 3rd electron shell and describe its energy?

A

3
- this shell has the highest energy

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

What do experiments show?

A
  • that not all the electrons in a shell have exactly the same energy
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What does the atomic model explain?

A
  • shells are divided into subshells
  • different shells have different numbers of subshells, which each have a different energy
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What can the sub shells be?

A
  • s subshells
  • p subshells
  • d subshells
  • f subshells
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What does the first shell contain?

A
  • one subshell 1s
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What does the second shell contain?

A

Two subshells 2s and 2p

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

What does the third shell contain?

A
  • 3 subshells 3s 3p 3d
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What does the fourth shell contain?

A
  • 4 subshells 4s 4p 4d 4f
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What do the subshells have?

A
  • different numbers of orbitals which can each hold upto 2 electrons
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

How many orbitals are there in the s subshell?

A

1

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How many orbitals are there in the p subshell?

A

3

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

How many orbitals are there in the d subshell?

A

5

19
Q

How many orbitals are there in the f subshell?

A

7

20
Q

What is the maximum number of electrons in the s subshell?

A

2

21
Q

What is the maximum number of electrons in the p subshell?

A

6

22
Q

What is the maximum number of electrons in the d subshell?

A

10

23
Q

What is the maximum number of electrons in the f subshell?

A

14

24
Q

What is the total number of electrons in the 1st shell?

A

2

25
Q

What is the maximum number of electrons in the 2nd shell?

A

8

26
Q

What is the maximum number of electrons in the 3rd shell?

A

18

27
Q

What is the maximum number of electrons in the 4th shell?

A

32

28
Q

What is electron configuration?

A
  • the number of electrons that an ion or atom has, and how they are arranged
29
Q

What are the different ways that electron configuration can be shown?

A
  • subshell notation
  • arrows in boxes
  • energy level diagrams
30
Q

Describe the arrows in boxes method of electronic structure

A
  • each of the boxes represents one orbital
  • each of the arrows represents one electron
  • the up and down arrows represent the electrons spinning in opposite directions
  • two electrons can only occupy the same orbital if they have opposite spin
31
Q

Describe the energy level diagrams for electronic configuration

A
  • these show the energy of the electrons in different orbitals as well as the number of electrons and their arrangement
32
Q

What are the steps in showing the electron configuration?

A
  • start with the principle quantum number
  • then the subshell letter (lower case)
  • then the number of electrons occupying the subshell (superscript)
33
Q

Name the three rules for working out the electron configurations

A
  • Aufbau principle
  • Hund’s rule
  • ions rule
34
Q

Describe the aufbau principle

A
  • as part of his work on electron configuration, Niels Bohr developed the aufbau principle, which states how electrons occupy sublevels
  • the aufbau principle states that the lowest energy sublevels are occupied first
  • this means the 1s sub level is filled first, followed by 2s 2p 3s 3p
  • however the 4s sublevel is lower in energy than the 3d, so it will fill first
35
Q

Describe Hund’s rule

A
  • electrons prefer to occupy orbitals on their own, and only pair up when no orbitals of the same energy are available
36
Q

Describe the ions rule

A
  • for the configuration of ions from the s and p blocks of the periodic table, just add or remove the electrons to or from the highest energy occupied subshell
  • for negative ions add electrons, for positive ions remove electrons
  • count the number of electrons
  • add or remove the electrons due to charge
  • fill sublevels as for uncharged atoms
37
Q

What is used as shorthand in electron configurations?

A
  • noble gas symbols in square brackets
38
Q

Describe the electron configuration of transition metals

A
  • although the 3d sublevel is in a lower principle energy level than the 4s sub level, it is actually higher in energy
  • this means that the 4s sublevel is filled before the 3d sub level
  • when transition metals form ions, it is the 4s electrons that are removed before the 3d electrons
  • count number of electrons in atom
  • fill sublevels, remembering 4s is filled before 3d
  • count number of electrons to be removed
  • remove electrons starting with 4s
39
Q

What decides the chemical properties of an element?

A
  • the number of outer shell electrons
40
Q

Describe the electronic structure of the s block elements

A
  • groups 1 or 2 have 1 or 2 outer shell electrons, these are easily lost to form positive ions with an inert gas configuration
41
Q

Describe the electron configuration of the p block elements

A
  • group 5, 6 and 7 can gain 1,2 or 3 electrons to form negative ions with an inert gas configuration
  • groups 4 to 7 can also share electrons when they form covalent bonds
42
Q

Describe the electronic structure of group 0 elements

A
  • have completely filled s and p subshells and don’t need to gain, lose or share electrons, their full subshells make them inert
43
Q

Describe the pauli exclusion principle and spin

A
  • the pauli exclusion principle states that each orbital may contain no more than two electrons
  • it also introduces a property of electrons called spin, which has two states, up and down, the spins of electrons in the same orbital must be opposite
  • a spin diagram shows how the orbitals are filled, orbitals are represented by squares and electrons by arrows pointing up and down
  • when two electrons occupy a sublevel, they could either completely fill the same orbital or half fill two different orbitals
  • if two electrons enter the same orbital, there is repulsion between them due to their negative charges
  • the most stable configuration is with single electrons in different orbitals

AS chemistry AQA (9 decks)

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