Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > 2. Bonding, structure, and the properties of matter > Flashcards

2. Bonding, structure, and the properties of matter Flashcards

1
Q

Three types of chemical bonds

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

Buckministerfullerene

A
  • Consists of 60 carbon atoms
  • Each atom bonded to 3 other carbon atoms
  • Arranged in rings of 5-6 atoms (pentagons & hexagons)
  • Weak intermolecular forces between the molecules of buckministerfullerene, so it is slippery
  • Because it is slippery and spherical, it is useful for lubricants
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Where are the electrostatic forces of attraction in ionic bonds?

A

Strong electrostatic forces of attraction between the oppositely charged ions

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

Where are the electrostatic forces of attraction in covalent bonds?

A

Nuclei of two atoms and a shared pair of electrons

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

Where are the electrostatic forces of attraction in metallic bonds?

A

Nuclei of atoms and delocalised electrons

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

What is an ion?

A

An atom with a positive or negative charge that has gained or lost electrons to obtain a full outer shell

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

Explain Ionic Bonding in terms of metals and non metals

A
  • When a metal atom reacts with a non-metal atom, electrons in the outer shell of the metal atom are transferred.
  • Metal atoms lose electrons to become positively charged ions. Non-metal atoms gain electrons to become negatively charged ions.
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Dot and Cross Diagram

& Limitations

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

Ionic Compounds & Properties

A
  • Form Giant regular structures known as a giant ionic lattice
  • Strong electrostatic forces of attraction in all directions between oppositely charged ions
  • High melting & boiling points because lots of energy is needed to break down the strong bonds
  • Can only conduct electricity in molten or liquid form because the ions are free to move so charge can flow
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Ball and Stick Diagram

& Limitations

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

2D + 3D Diagrams

& Limitations

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

What is Covalent Bonding?

A

The sharing of pairs of electrons between non-metal atoms

Note: A molecule is a group of two or more atoms joined together by covalent bonds

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

Which type of bond are molecules?

A

Covalent bonds

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

Properties of Covalent Bonds

& small molecules

A
  • Covalent Bonds are strong bonds
  • Covalent Bonds have weak intermolecular forces
  • Small molecules are usually gases or liquids that have low melting or boiling points because the weak intermolecular forces are easily overcome
  • The larger the molecules are, the stronger the intermolecular forces, so the melting and boiling points increase
  • They cannot conduct electricity because the molecules have no overall charge
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

Giant Covalent Structures & Properties

A

They are many atoms joined together by covalent bonds in a giant lattice structure
- High melting and boiling points as there are a large number of bonds to be broken in a giant covalent structure, and all the bonds are linked by strong covalent bonds

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

Examples of Giant Covalent Structures

A

Diamond, Graphite ( + graphene ), and silicon dioxide

17
Q

Diamond & Properties

A
  • A giant covalent structure
  • Each carbon atom is bonded with 4 other carbon atoms
  • Does not conduct electricity
  • Rigid network held together by stong covalent bonds, so:
    • It is hard enough to resist forces that could distort the structure
    • It has a very high melting and boiling point
18
Q

Graphite & Properties

A
  • A giant covalent structure
  • Has hexagonal rings in layers
  • There are weak intermolecular forces between the layers which means that the layers can slide past each other - making graphite soft and slippery
  • Each carbon atom is bonded with 3 other carbon atoms
  • Carbon has 4 electrons - 3 are bonded - so there is one delocalised electron for each carbon atom in graphite
  • Delocalised electrons mean that they are free to move so they can conduct electricity and heat
19
Q

Graphene & Properties

A

A single layer of graphite so it is transparent and flexible

• Strong covalent bonds which means:

  • High melting point
  • Very strong - useful for making composites

• Has delocalised electrons so it conducts electricity - useful in electronics

20
Q

Fullerenes

& Examples

A

Molecules of carbon atoms with hollow shapes ( such as tubes, balls and cages )

• Fullerenes have a structure of hexagonal rings with 5, 6 or 7 carbon atoms

Examples: Buckministerfullerene (C60), Carbon Nanotubes

21
Q

Carbon Nanotubes

A
  • Cylindrical fullerenes
  • Very high length to diameter ratios - ( Very long compared to their width )
  • This makes them useful for nanotechnology, electronics and materials (they conduct electricity)
22
Q

Polymers

A
  • Polymers have very large molecules
  • They are linked to other atoms by strong covalent bonds
  • The intermolecular forces between polymer molecules are relatively strong and so these substances are solids at room temperature.
23
Q

What is metallic bonding?

  • How are they organised?
  • Talk about their attraction
A

Metallic bonding is the bonding of metal atoms

  • It consists of a giant structure of metal atoms - which are positive ions - and a sea of delocalised electrons which are free to move through the structure
  • The sharing of delocalised electrons results in strong metallic bonds.
24
Q

Properties of metals

A
  • High melting and boiling points as lots of energy required to break a number of strong metallic bonds
  • Metals are good conductors of electricity because the delocalised electrons in the metal carry electrical charge through the metal.
  • Metals are good conductors of thermal energy because energy is transferred by the delocalised electrons.
  • Particles in pure metals have a regular arrangement and size, so the layers are able to slide over each other, resulting in them being malleable (bent) and ductile (pulled/shaped)
25
Q

Alloys

  • What is it?
  • Why is it used?
  • An example
A
  • An alloy is a mixture of two or more elements
  • Pure metals are too soft for many uses due to their regular arrangement and size
  • They are mixed with other metals to make alloys, which are harder because the different-sized atoms distort the layers to slide over each other
  • Steel is an alloy made of iron and small amounts of carbon
26
Q

Nanoscience & Nanoparticles

A
  • Nanoscience is the study of structures that are between 1 and 100 nanometres (nm) in size.
  • Nanoparticles are only a few hundred atoms in size
  • They have a high surface area to volume ratio
27
Q

Nanoparticle Uses

Advantages & Disadvantages

A
  • Electronics - They have high length to diameter ratio
  • Sun Creams - They are small in size so are invisible to skin. However, it is difficult to see where it has been applied as it is invisible to skin
  • Deodorants - Nano particles are antibacterial (kill bacteria that gives bad smells)
  • Catalysts - High surface area to volume ratio
28
Q

Where does ionic bonding occur?

A

Occurs in compounds formed of metals combining with non-metals

29
Q

Where does covalent bonding occur?

A

Occurs in compounds of non metals

30
Q

Where does metallic bonding occur?

A

Occurs in metallic elements and alloys

Chemistry (10 decks)

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