Brainscape's Knowledge GenomeTM

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


See full index

Chemistry > Bonding, structures and properties of matter > Flashcards

Bonding, structures and properties of matter Flashcards

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

How do substances melt

A

Energy transfer to the particles causes the attractive forces between the particles to weaken

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

How do substances evaporate

A

Chemical bonds in the substances are overcome

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

Difference between boiling and evaporation

A

In evaporation particles only leave the substance from the surface
In boling bubbles of gas form throughout the liquid and rise to the surface

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

A higher attractive force means

A

Higher melting and boiling point
because more energy is needed to overcome them

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

Describe particles in a solid

A

Regular lattice/ pattern
Vibrate around a fixed point
Low amount of kinetic energy
Particles cannot be compressed
Do not fill a container

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

Describe particles in a liquid

A

Irregular pattern
Move around
More kinetic energy than solid
Particles cannot be compressed
Particles fill a container from the bottom

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

Describe particles in gas

A

Randomly arranged
Particles moves fast and in any direction
Highest amount of kinetic energy
Completely fill a container
Particles can be compressed

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

Why is the model used to show particles in a solid liquid gas limited

A

Particles are represented as solid spheres
Particles aren’t always sphereical
Particles like atoms are mostly empty space

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

Metal ions charge

A

Positive

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

In metallic bonding positive metal ions are surrounded by

A

A sea of negative electrons

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

What holds metallic bonding together

A

Electrostatic force between metal ions and electrons

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

How do alloys make metals harder

A

The mixture of different metal atoms distorts the regular lattice layers and prevents them from sliding over each other making alloys harder to bend

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

Ionic bonding is between

A

Metal and non-metal

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

What holds ionic bonds together

A

Electrostatic attraction between oppositely charged ions

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

Ionic compounds form structures called

A

Giant lattices

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

Properties of ionic compounds

A

High melting point, energy needed to overcome electrostatic bonds
High boiling point
Can’t conduct electricity as ions cannot move around the substance
However can conduct electricity as liquid or solution

17
Q

Simple covalent properties

A

Low melting/ boiling points
Weak intermolecular forces
Do not conduct electricity

18
Q

Describe the diamond giant covalent structure

A

Each carbon bonded to 4 other carbons
Very strong
Alot of energy needed to break bonds
High melting/boiling point
Does not conduct electricity has no free floating electrons

19
Q

Describe the silicon dioxide giant covalent structure

A

Similar to diamond but not bonded to as many particles

20
Q

Describe the graphite giant covalent structure

A

Each carbon bonded to 3 other carbons
Arranged hexagonally
Each carbon has 1 delocalised electron that can carry electricity through the substance
Millions of layers on top of each other
Layers are held together by the weak intermolecular forces
Layers can slide over each other because of no covalent bond between the layers
High melting point as there is alot of energy required to break the 3 bonded carbons

21
Q

Describe the graphene giant covalent structure

A

Strong due to 3 covalent bonds for every carbon
Conduct electricity due to delocalised electrons

22
Q

2 Uses of graphene

A

Added to other materials to make them stronger
Used in electrics and composites

23
Q

What type of particles have a large SA:V ratio

A

Nanoparticles

24
Q

What size is nanoparticles

A

1-100nm

24
Q

What size is fine particles

A

100-2500nm

25
Q

What size is course particles

A

2500-10000nm

26
Q

What are polymers made of

A

Monomers

26
Q

What are polymers held together by

A

Covalent bonds

27
Q

Which type of polymers have stronger forces of attraction

A

Long ones

28
Q

Buckminister fullerijne formula

A

C60

29
Q

Usesof Fullerene

A

Deliver drugs into the body

30
Q

Uses of carbon nanotube

A

Electronics, nanotechnology, strengthening materials

31
Q

Risks of nanoparticles

A

Easily be inhaled (so)
Initiate harmful reactions
Toxic substances bind to them because of SA:V ratio

32
Q

Nanoparticle application

A

Medicine, cosmetic, sun cream, deodrants, catalysts

33
Q

Risk of nanoparticles being a modern technology

A

Difficult for scientists to know the risks for them

Chemistry (10 decks)

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