Brainscape's Knowledge GenomeTM


Top Flashcards (Certified)
All Flashcards

Chemistry Unit 1 > 1.2 and 1.3 Bonding And Structure > Flashcards

1.2 and 1.3 Bonding And Structure Flashcards

1
Q

What is a cation?

A

A positively charged ion which forms when an atom loses electrons

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

What is an anion ?

A

A negatively charged ion which forms when an atom gains electrons

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

What is ionic bonding typical of ?

A

It is typical of metal compounds e.g sodium chloride

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

What is ionic bonding ?

A

Ionic bonding is the strong electrostatic force of attraction between oppositely charged ions

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

What is a molecular ion ?

A

A charged particle containing 2 or more atoms covalently bonded together e.g. NH⁴, SO⁴2+

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

What is the structures of an ionic compound described as ?

A

Giant ionic lattice

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

What are the properties of ionic bonding?

A
  • High melting and boiling point - substantial energy is required to break the string ionic bonds in the giant ionic lattice
  • Soluble in water
  • Do not conduct electricity when solid - because in the solid state the ions are in fixed positions meaning they are not free to move and carry charge
  • Good conductors of electricity when molten or dissolved in water - ?When molten or in solution the ions are free to move and carry charge
  • Hard - Substantial energy is required to break the strong ionic bonds in the giant ionic lattice
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

What is covalent bonding ?

A

Covalent bonding is the sharing of electron pairs between non-metal atoms in a molecule

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

What is covalent bonding typical of ?

A

Covalent bonding is typical of non- metallic elements and compounds

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

What is a molecule ?

A

A molecule is two or more atoms covalently bonded together

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

What is meant by the term diatomic ?

A

Two of the same atoms covalently bonded together in a molecule

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

What is a compound ?

A

A compound is substance formed when two or more different types of elements are chemically combined e.g. carbon dioxide

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

What is an element ?

A

An element is made up of only one type of atom

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

What structure does a substance containing covalent bonds have ?

A

They can have either a Molecular Covalent structure or a Giant Covalent Structure

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

What do molecular covalent structure exist as ?

A

Substances with a molecular covalent structure exist as individual molecules e.g. water

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

What is an example of a molecular covalent substance existing as an element?

A

Iodine (I²) is an element which consists of two non-metal atoms covalently bonded together i.e it has a molecular covalent structure

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

What are the properties of molecular covalent substances and their explanations ?

A
  • They have low melting and boiling points = The van der Waals forces between the molecules are weak and require little energy to break
  • Cannot conduct electricity - They do not contain charged particles to move and carry the charge
  • Most are insoluble in water
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

What are the intermolecular forces between covelent molecules called ?

A

The intermolecular forces between covelent molecules are weak van der Waals forces

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

What are the three giant covalent structures ?

A
  • Graphite
  • Graphene
  • Diamond
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

Are covalent bonds strong?

A

Covalent bonds are very strong meaning that a lot of energy is required to break them, however substances with a molecular covalent structure generally have a low melting and boiling point since only a small amount of energy is required to break the weak van der Waals forces between the molecules

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

What are allotropes ?

A

Allotropes are different forms of the same element in the same physical state

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
22
Q

Describe the structure of diamond ?

A

In Diamond each carbon atom is covalently bonded to 4 other carbon atoms in a tetrahedral arrangement

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
23
Q

What are the 4 physical properties of diamond and their explanations?

A

1) High melting and boiling point - This is because substantial energy is required to break the many strong covalent bonds between the carbon atoms in the giant covalent structure
2) Hard - This is because there are many strong covalent bonds throughout the rigid three dimensional giant covalent structure
3) Doesn’t conduct electricity - Does not contain free ions or electrons to move and carry charge
4) Insoluble in water

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
24
Q

What is diamond used for and why ?

A

Diamond is used in cutting tools such as drill tips for drilling through rock as it is the hardest naturally known substance because there are many strong covalent bonds throughout the rigid three dimensional, giant covalent structure

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
25
Why are ionic substances good conductors when molten ?
Because when they are molten or in solution the ions are free to move and carry charge
26
Why are ionic substances not good conductors when solid?
Because in the solid state the ions are in fixed positions meaning they are not free to move and carry charge
27
Why do ionic substances have high melting and boiling points ?
This is because substantial energy is required to break the strong ionic bonds in the giant ionic lattice
28
Why are ionic substances hard ?
Substantial energy is required to break the strong ionic bonds in the giant ionic lattice
29
Why are ionic substances brittle ?
This is because when struck, ions of the same charge align and repel each other, causing the crystal structure to shatter
30
What does covalent bonding involve?
Covalent bonding involves the sharing of electron pairs
31
What type of atoms do covalent bonds form between?
Covalent bonds form between non-metal atoms
32
How are covalent bonds represented ?
The covalent bonds are represented by a line connecting the non-metal atoms
33
What are the bonds and forces in molecular covalent structures ?
The bonds between the atoms in the molecule are strong covalent bonds, whereas the forces between the molecules are weak van der Waals forces
34
Why do molecular covalent substances have low melting and boiling points ?
This is because only a small amount of energy is required to break the weak van der Waals forces between the molecules
35
Why are molecular covalent substances poor conductors of electricity?
Molecular covalent substances do not contain charged particles to move and carry charge
36
What is the structure of diamond?
Diamond has a rigid, 3 dimensional, giant covalent structure in which each carbon atom covalently bonds with four other carbon atoms in a tetrahedral arrangement
37
Why is diamond hard and therefore good for use in drill tips and saws ?
There are many strong covalent bonds throughout the rigid three dimensional, giant covalent structure
38
Why does diamond not conduct electricity ?
Diamond doesn't conduct electricity as there are no charged delocalised electrons free to move and carry charge
39
Why does diamond have a high boiling point?
Substantial energy is required to break the many strong covalent bonds between the carbon atoms in the giant covalent structure
40
What is the structure of graphite ?
- Graphite has a giant covalent structure where each carbon atom forms strong covalent bonds with 3 other carbon atoms in hexagonal rings, which are arranged in layers. - Consequently, each carbon atom contains a non-bonded electron which becomes delocalised in the layers, making graphite a conductor of electricity since the delocalised electrons in the layers are free to move and carry charge - Weak van der Waals forces exist between the layers of carbon atoms, as result the layers can slide over each other
41
In graphite how many carbon atoms does each carbon atom form bonds with ?
Each carbon atom forms strong covalent bonds with 3 other carbon atoms in hexagonal rings, which are arranged in layers
42
What forces of attraction exist between the layers of carbon atoms in diamond?
Weak forces of attraction called van der Waals forces exist between the layers of carbon atoms and as a result the layers can slide over each other
43
Describe the structure of graphite ?
Graphite has a giant covalent structure where each carbon atom forms strong covalent bonds with 3 other carbon atoms in hexagonal rings, which are arranged in layers. - Consequently, each carbon atom contains a non-bonded electron which becomes delocalised in the layers and makes graphite a conductor of electricity since the delocalised electrons in the layers are free to move and carry charge - Graphite has weak forces of attraction called van der Waals forces which exist between the layers of carbon atoms and as a result the layers can slide over each other
44
What are properties of Graphite and there explanations ?
- High Melting point - Substantial energy is needed to break the many strong covalent bonds between the carbon atoms in the giant covelent structure - Conductor of electricity - The delocalised electrons in the structure are free to move and carry charge through the layers - Insoluble in water - Does not dissolve in water - Soft and slippery - This is because weak van der Waals forces between the layers of carbon atoms and as a result, the layers can slide over each other
45
What are 2 uses of graphite and what property allows this and why ?
- Pencil lead - Because graphite is soft and slippery because weak van der waals forces exist between the layers of carbon atoms and as a result the layers can slide over each other and leave a mark on paper - Lubricant - Because graphite is soft and slippery because weak van der waals forces exist between the layers of carbon atoms and as a result the layers can slide over each other
46
Why is graphite used as a lubricant?
Because graphite is soft and slippery because weak van der waals forces exist between the layers of carbon atoms and as a result the layers can slide over each other
47
Why is graphite used in pencils ?
Because graphite is soft and slippery because weak van der waals forces exist between the layers of carbon atoms and as a result the layers can slide over each other
48
What is the structure of graphene ?
- Graphene is made up a single layer of graphite which is one carbon atom thick - Each carbon atom forms strong covalent bonds with 3 other carbon atoms in hexagonal rings in a single layer - Consequently, each carbon atom contains a non-bonded electron which becomes delocalised in the layer
49
What are the properties of graphene and their explanations?
- Strong - Because substantial energy is needed to break the strong covalent bonds between the carbon atoms in the rigid structure of heaxagons - Low density - Graphene is made up of a single layer of graphite one carbon atom thick - Flexible - The flat layer of carbon atoms can bend without breaking the covalent bonds - Excellent conductor of electricity - Each carbon atom is covalently bonded to 3 others, meaning there is a non-bonded electron which becomes delocalised. These delocalised electrons in the layer are free to move and carry charge. Graphene is a better conductor than any metal - Transparent - The single layer of carbon atoms is very thin, resulting in Graphene being transparent
50
What are the properties of graphene and their explanations?
- Strong - Because substantial energy is needed to break the strong covalent bonds between the carbon atoms in the rigid structure of heaxagons - Low density - Graphene is made up of a single layer of graphite one carbon atom thick - Flexible - The flat layer of carbon atoms can bend without breaking the covalent bonds - Excellent conductor of electricity - Each carbon atom is covalently bonded to 3 others, meaning there is a non-bonded electron which becomes delocalised. These delocalised electrons in the layer are free to move and carry charge. Graphene is a better conductor than any metal - Transparent - The single layer of carbon atoms is very thin, resulting in Graphene being transparent
51
Why is Graphene strong?
Substantial energy is needed to break the strong covalent bonds between the carbon atoms in the rigid structure of hexagons
52
Why does Graphene have a low density ?
Graphene has a low density because Graphene is made up of a single layer of graphite one carbon atom thick
53
Why is Graphene flexible?
The flat single layer of carbon atoms can bend without breaking the covalent bonds
54
Why is Graphene excellent conductor of electricity?
- This is because each carbon atom is covalently bonded to 3 others meaning that there is a non - bonded electron which becomes delocalised in the layer. These delocalised electrons in the layer are free to move and carry charge
55
Why is Graphene transparent ?
Graphene is transparent because the single layer of carbon atoms is very thin, resulting in Graphene being transparent
56
What are 2 uses of Graphene?
- Battery - Solar cell
57
Why is Graphene used in batteries?
- It's an excellent conductor of electricity because the delocalised electrons in the layer are free to move and carry charge - Low density - Graphene is made up of a single layer of graphite (one carbon atom thick) making Graphene batteries smaller, lighter and therefore faster to recharge
58
Why is Graphene used in solar cells ?
- Transparent - Because the single layer of carbon atoms is very thin, resulting in Graphene being transparent - Excellent conductor of electricity - The delocalised electrons in the layer of graphene are free to move and carry charge - Low density - Graphene is made up of a single layer of graphite (one carbon atom thick)
59
What is metallic bonding?
Metallic bonding is the attraction between positive metal ions in a regular lattice and negativly charged delocalised electrons.
60
When drawing metallic bonding what must be made sure ?
The positive metal ions MUST be drawn in a regular arrangement and there must be a greater number of negativly charged delocalised electrons scattered throughout the structure
61
What are the 4 properties of metals and their explanations?
- High melting point - Substantial energy is required to break the strong metallic bonds between the positive metal ions and delocalised electrons - Conductor of electricity - The delocalised electrons are free to move and carry charge through the metal - Malleable - can be hammered into shape because the layers of ions can slide over each other without disrupting the metallic bonding - Ductile - can be drawn out into wires because the layers of ions can slide over each other without disrupting the metallic bonding
62
Why are metals good conductors of electricity?
The delocalised electrons are free to move and carry charge through the metal
63
Why do metals have a high melting point ?
Substantial energy is required to break the strong metallic bonds between the positive metal ions and delocalised electrons
64
What is meant by malleable ?
Can be hammered/ bent into shape
65
What is meant by ductile?
Can be drawn out into wires

Chemistry Unit 1 (6 decks)

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