Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry - Edexcel - GCSE > Topic 1 - Bonding and Structure > Flashcards

Topic 1 - Bonding and Structure Flashcards

1
Q

When are atoms most stable?

A

When they have a full outer shell

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

In which two groups are the bible gases?

A

Group 0 and 8

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

Why are the Nobel gases so unreactive?

A

Because they all have a full outer shell of 8 electrons

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

Atoms that do not have a full outer shell will react forming what and why?

A

Chemical bonds with other atoms in order to gain a full outer shell, which is then stable

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

What are the 3 types of bonding?

A
  • Ionic Bonding
  • Covalent Bonding
  • Metallic Bonding
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Ionic bonding forms between what?

A

Metal and non metal atoms

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

What happens to the electrons in ionic bonding?

A

Involves electrons being transferred to gain full outer shells

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

Where is ionic bonding found? Give examples:

A

Found in ionic compounds such as sodium chloride (NaCl) and Aluminium Oxide (Al2O3)

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

What does ionic bonding result in?

A

The oppositely charged ions are attracted together, forming a regular arrangement called a lattice or a giant structure

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

Covalent bonding forms between what?

A

Non metal atoms

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What happens to the electrons in covalent bonding?

A

Involves electrons being shared to gain full outer shells

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

Where is covalent bonding found? Give examples:

A
  • Found in covalent compounds such as carbon dioxide (CO2) and ammonia (NH3)
  • Also found in some non metal elements e.go H2, Cl2, N2, O2
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

What does covalent bonding result in?

A

Simple molecular or giant covalent structures

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

Metallic bonding is formed between what?

A

Metal atoms

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

What happen to electrons in metallic Bonding?

A
  • The outer shell electrons from each atom become delocalised
  • The structure is held together by the strong electrostatic forces between the positive ions and the “sea” of free electrons
  • This means metals have high melting points
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Where is metallic bonding found? Give examples:

A

Found in metals such as potassium (K), copper (Cu), iron (Fe) and aluminium (Al)

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

What does metallic bonding result in?

A

Giant Metallic structures

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

Definition of metallic bonding:

A

Metallic bonding is the strong electrostatic attraction between the positive ions and the delocalised electrons

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

Metals, eg. copper, consist of what kind of arrangement?

A

They consist of a regular arrange to of atoms called a giant structure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

What makes metals malleable?

A

The layers of atoms/ions slide over each other when a force is applied but the structure does not break apart because it is held together by the delocalised electrons. This makes metals malleable

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
21
Q

What does malleable mean?

A

It can be hammered into shape

22
Q

Why can metals conduct electricity and heat?

A

Due to the delocalised electrons being able to move freely throughout the structure

23
Q

What is an alloy?

A

Alloys are less amoebae than pure metals, so cannot easily be pressed into shape

24
Q

Why are alloys less malleable than pure metals?

A
  • In pure metals, the regular structure of atoms is arranged in layers. When a force is applied, the layers of atoms can slide over each other —> malleable
  • In alloys, there are atoms of other element, disrupting the layers. When a force is applied, the layers cannot slide over each other —> not so malleable
25
What type of Bonding do dot and cross diagrams represent?
Ionic and covalent bonding and substances
26
Definition of Ionic Bonding:
Ionic Bonding is the strong electrostatic attraction between the positive ions and the negative ions
27
Examples of Ionic Bonding:
- Magnesium Oxide (MgO), made from magnesium (metal) and oxygen (non-metal), therefore must contain ionic bonding - Aluminium Fluoride (ALF3), made from aluminium (metal) and fluorine (non-metal), therefore must contain ionic bonding
28
What happens in magnesium oxide as it is Bonding?
- Mg has 2 electrons in its outer shell so needs to lose 2 for a full outer shell - O has 6 electrons in its outer shell so needs to gain 2 for a full outer shell ——> 2 electrons from Mg transferred to O ——> - Mg has lost 2 negative charges (electrons) so becomes an ion with a charge of +2 - O has gained 2 negative charges (electrons) from Mg so Beckens an ion with a charge of -2
29
What happens to Aluminium fluoride as it is Bonding?
- Al has 3 electrons in its outer shell so needs to lose 3 for a full outer shell - F has 7 Electrons in its outer shell so needs to gain 2 for a full outer shell. 3 F atoms are needed to accept the 3 electrons from the outer shell of Al ——> - Al has lost 3 negative charges (electrons) so becomes an ion with a charge of +3 - The F atoms have each gained 1 negative charge (electron) from Al so become ions with a charge of -1. 3 F ions are needed to balance the 3+ charge on Al and make the compound neutral
30
When do Ionic compounds conduct electricity?
When they are molten or in a solution
31
Why do Ionic compounds only conduct electricity when they are molten or in solution and not when solid?
- Because the ions are free to move (many Ionic compounds dissolve in water) - Solid ionic compounds do not conduct because the ions are fixed in the lattice
32
What gives Ionic compounds high melting points?
Strong electrostatic forces between oppositely charged ions
33
Definition of Covalent Bonding:
Covalent Bonding is the strong electrostatic attraction between the nuclei and the shared pair of electrons
34
Example of covalent Bonding:
- Water (H2O), made from 2 hydrogen (non-metal) atoms and 1 oxygen (non-metal) atom, therefore must contain covalent bonding - Carbon dioxide (CO2), made from 1 carbon (non-metal) atom and 2 oxygen (non-metal) atoms, therefore must contain covalent bonding - Fluorine (F2) made from 2 fluorine (non-metal) atoms, therefore must contain covalent bonding. Note that several non-metal elements exist naturally as covalent molecules eg. H2, O2, N2, Cl2, Br2, I2
35
What happen to water when it is bonding?
- H has 1 electron in its outer shell so needs to gain 1 for a full outer shell (the 1st shell only holds 2 electrons - O has 6 electrons in its outer shell so needs to gain 2 for a full outer shell ——> pairs of electrons shared ——> - The O atom and both H atoms have gained full outer shells by sharing electron pairs. Each electron pair is a single bond, so the structure can also be drawn as H – O – H. The H2O molecule formed is neutral
36
What happens to carbon dioxide when it is Bonding?
- C has 4 electrons in its outer shell so needs to gain 4 for a full outer shell - O has 6 electrons in its outer shell so needs to gain 2 for a full outer shell ——> pairs of electrons shared ——> - The C atom and both O atoms have gained full outer shells by sharing electron pairs. Each electron pair is a single bond, so the structure can also be drawn as O = C = O. The CO2 molecule formed is neutral
37
What happens to fluorine when it is Bonding?
- F has 7 electrons in its outer shell so needs 1 electron for a full outer shell - This is achieved when the 2 F atoms share 1 pair of electrons to form a single covalent bond
38
How do the vast majority of covalent substances exist?
As simple molecules
39
What holds the atoms in the molecules together in a covalent substance?
Strong covalent bonds
40
What does the weak intermolecular fiefs between the molecules in a covalent substance result in?
It results in the molecules being easy to pull apart so that they have low melting and boiling points
41
What charge are the molecules in a covalent substance?
Neutral - they cannot carry any electrical charge - covalent substances made up of simple molecules do not conduct electricity
42
How many covalent subsides exist as giant covalent structures?
A very small number
43
Give examples of giant covalent structures:
- Silicon dioxide (SiO2) - Graphite - Diamond - Fullerenes ⬆️All different forms of carbon ⬆️
44
Why do covalent structures have high melting and boiling points?
Because all giant covalent structures have strong covalent bonds throughout the structure, they need lots of energy to break these bonds
45
In Diamond, each C atom is attached to how many others?
4 others
46
Why is the structure hard in diamond?
Because there are string covalent bonds throughout the structure
47
How are the C atoms arranged in graphite?
In layers
48
Why can the layers easily slide over one another in graphite?
Because there are strong covalent bonds within the layers but only weak intermolecular forces between layers
49
In graphite, each C atom is attached to how many others?
3, leaving 1 spade electric in the outer shell of each C atom
50
Why can graphite conduct electricity?
- Because in graphite, each C atom is attached to 3 others, leaving 1 spare electron in the outer shell of each C atom - This electron is free to move – it is delocalised enabling graphite to conduct electricity
51
The structure of SiO2 is very similar to which other giant covalent structure, with the same properties?
Diamond

Chemistry - Edexcel - GCSE (1 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions