Brainscape's Knowledge GenomeTM

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


See full index

Chemistry Paper 1 > C3 Structure and bonding > Flashcards

C3 Structure and bonding 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 are the three states of matter?

A

Solids, liquids and gases

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

Solids

A
  • Fixed shape and volume
  • Cannot be compressed
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Liquids

A
  • Fixed volume
  • Can flow and change their shape
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

Gases

A
  • No fixed shape or volume
  • Can be compressed easily
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Particle theory - solids

A
  • Each particle in a solid is touching its nearest neighbour and they remain in this fixed arrangement
  • They cannot move around but they do vibrate constantly
  • High density
  • Low energy
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

Particle theory - liquids

A
  • The particles in a liquid are also very close together but they can move past each other
  • This results in a constantly changing, random arrangement of particles
  • Medium density
  • Greater energy than in solids
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

Particle theory - gases

A
  • The particles in a gas have on average, much more space between them
  • They can move around at high speeds in any direction
  • This means the particles have a random arrangement
  • The hotter the gas, the faster the particles move
  • The pressure of a gas is caused by the particles colliding with the sides of the container
  • The more frequent and energetic the collisions are, the higher the pressure of the gas (in a sealed container the pressure of gas increases with temperature)
  • Low density
  • Highest energy
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

Limitations of the particle model

A

The atoms, molecules, and ions that make up all substances are not solid spheres with no forces operating between them

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

Energy transfers during change of state

A
  • In melting and boiling, energy is transferred from the surroundings to the substance (endothermic)
  • In freezing and condensing, energy is transferred from the substance to the surroundings (exothermic)
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Compound

A

Contains two or more elements, which are chemically combined

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

Covalent bonding

A

Non-metal atoms share electrons between each other

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

Ionic bonding

A
  • Metals and non-metals react by transferring electrons
  • The atoms involved are oppositely charged particles (known as ions) in which electron transfer occurs
  • The ions formed are held next to each other by very strong electrostatic forces of attraction between the oppositely charged ions
  • The ionic bonds between the charge particles result in an arrangement of ions called a giant structure or giant lattice
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Ions and the periodic table

A
  • Group 1 form 1+ ions
  • Group 2 form 2+ ions
  • Group 3 form 3+ ions, when they form ions as opposed to sharing electrons
  • Group 4 do not form ions (apart from tin (Sn), lead (Pb), at the bottom of the group)
  • Group 5 form 3- ions, when they form ions as opposed to sharing electrons
  • Group 6 form 2- ions, when they form ions as opposed to sharing electrons
  • Group 7 form 1- ions, when they form ions as opposed to sharing electrons
  • Group 0 never form ions in compounds
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Metallic bonding

A
  • Metal ions are arranged in regular layers, on top of each other
  • Positively charged metal ions, which are held together by electrons from the outermost shell of each metal atom
  • Strong electrostatic attraction between the negatively charged electrons and the positively charged ions bond the metal ions to each other
  • These delocalised electrons are free to move throughout the giant metallic lattice
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

General properties of giant covalent structures

A
  • Very high melting and boiling points
  • Insoluble in water
  • Apart from graphite, they are hard and do not conduct electricity
How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Bonding in graphite

A
  • Carbon atoms are only bonded to three other carbon atoms
  • Carbon atoms have four electrons in their outer shell available for bonding. This leaves one spare outer electron on each carbon atom in graphite
  • They form hexagons, which are arranged in giant layers
  • There are no covalent bonds between the layers, only weak intermolecular forces, so the layers can slide over each other. This makes graphite soft and slippery
  • Graphite can conduct electricity and thermal energy because of the delocalised electrons that can move along its layers
17
Q

What is an alloy?

A

A mixture of two or more elements, at least one of which is a metal

18
Q

Carbon nanotubes properties

A
  • High tensile strength, leading to their use in reinforcing composite materials, such as those used in making tennis rackets
  • High electrical conductivity and high thermal conductivity, because their bonding is like the bonding in graphite, giving them delocalised electrons, resulting in their use in the electronics industry
19
Q

Fullerenes

A
  • Carbon atoms join together to make large hollow cages
  • The structures are based on hexagonal rings of carbon atoms but they may also contain rings with five or seven carbon atoms
20
Q

What is graphene?

A

A single layer of graphite

21
Q

Properties of graphene

A
  • Excellent conductor of electricity and thermal energy
  • Very low density
  • Very strong
22
Q

Explain how a covalent bond holds two atoms together

A

Electrostatic force of attraction between shared pair of negatively charged electrons and the positively charged nuclei.

23
Q

What shape is a Buckminsterfullerene molecule?

A

Spherical

24
Q

What are the uses of a fullerene?

A
  • Drug delivery around the body
  • Catalysts
  • Lubricants
25
Q

Explain why graphite is a good electrical conductor and is soft and slippery

A
  • Graphite contains covalent bonds and is a macromolecular structure
  • There are three covalent bonds per carbon atom so one electron per carbon atom is delocalised
  • These delocalised electrons can move through the structure and carry electrical charge, so graphite conducts electricity
  • The layered structure of interlocking hexagonal rings has no covalent bonds between layers so the layers can slide over each other, so graphite is soft and slippery
26
Q

Explain why sodium oxide has a high melting point

A
  • It is a giant structure
  • With strong electrostatic forces of attraction between ions
  • So large amounts of energy are needed to break the bonds
27
Q

Explain why alloys are harder than pure metals

A
  • In an alloy the atoms are different sizes
  • So the layers are distorted
  • The layers slide over each other less easily

Chemistry Paper 1 (9 decks)

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