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Yr9 Chemistery > Bonding and nanoparticles and states of matter > Flashcards

Bonding and nanoparticles and states of matter Flashcards

1
Q

What are the three types of bonding?

A

Ionic bonding
Covalent bonding
Metallic bonding

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2
Q

Covalent bonding between…

A

Two non-metals

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3
Q

Ionic bonding between…

A

A metal and non-metal

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4
Q

Metallic bonding…

A

Electrostatic force of attraction within a metal

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5
Q

Ions

A

When an element loses or gains an electron

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6
Q

An ionic compound is a…

A

giant structure

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7
Q

Ionic bonding: High or low melting and boiling point? Why?

A

High because the giant structure
really strong bonds
need a lot of energy to break

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8
Q

Ions are very…

A

closely packed together

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9
Q

Do ions conduct electricity?

A

Yes, when they are in the water or are molten

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10
Q

Why ions conduct electricity when in water or molten

A

Then they can carry a charge because they are free to move

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11
Q

Metals always… an electron and a non-metal

always… an electron

A

lose

gains

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12
Q

… … between ions

A

Strong electrostatic forces

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13
Q

What should we consider before writing a ratio of an ionic bond?

A

The metal goes first

It is supposed to be in its simplest form

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14
Q

What are the limitations in showing ions in 3D?

A

Each of the ions are represented as spheres
Does not show the charges
How the ions were formed

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15
Q

What are the limitations in showing ions in 2D?

A

The diagram is not three dimensional

Does not show the structural arrangement of ions

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16
Q

What are the limitations in showing ions in ball and stick

A

No sticks/gap between the bonds

Does not show charges

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17
Q

Difference between an ion and an atom?

A

Atom when neutral

Ion when there is a charge

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18
Q

After the covalent bond has been formed all elements must have…

A

a full outer shell

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19
Q

Covalent bonding can also be in an element

A

Because gases are diatomic molecules except for the noble gases

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20
Q

How many pairs can you have in a covalent bond

A

Up to 3

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21
Q

In a covalent bond can there be one electron more contributed than the other elemen?

A

No, it should be in pairs

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22
Q

Limitations of covalent bonding in Dot and cross diagrams?

A

Size of the atom

Intermolecular forces

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23
Q

Limitations of covalent bonding in a structure

A

How covalent bonds are formed

Size of the atom

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24
Q

Limitations of covalent bonding in ball and stick method?

A

How covalent bonds are made

That bonds are not sticks

25
Q

Limitations of covalent bonding in space-filling model

A

How covalent bonds are formed

Which elements are present( unless given a color key)

26
Q

Limitations of covalent bonding in 2D

A

Not accurate

27
Q

Limitations of covalent bonding in 3D

A

Difficult to see 3D packing with no spacing

28
Q

Intermolecular forces are…

A

weak and are easy to break

29
Q

Small molecules conduct/ does not conduct electrecity?

30
Q

Intermolecular forces strength increases as…

A

the bigger the molecule

31
Q

Polymers and fullerenes are…

A

large molecules

covalent bonding

32
Q

Name covalent bonding- giant molecules

A

Silicon dioxide
diamonds
graphite
graphene

33
Q

Polymers and fullerenes have a … intermolecular force

34
Q

Giant molecules covalent bond have … intermolecular forces

35
Q

Giant molecules properties

A

Does not conduct electrecity
Usually insoluble in water
no intermolecular forces

36
Q

Allastropes

A

Different forms of same element

37
Q

Allastropes of carbon

A

Diamond
Graphite
Graphene
Fullerenes

38
Q

Properties of diamond

A 
Allastrope of carbon
Carbon in group 4 so can form a maximum of 4 bonds
Hardest natural material
Has a very high melting point
it does not conduct electricity
39
Q

Properties of Graphite

A

Each carbon atom forms 3 covalent bonds
This forms a layer of hexagonal rings
Layers are free to move over each other as there are no covalent bonds between layers
Has high boiling and melting point
It does conduct electricity and thermal energy because there is a delocalize electron free to carry a charge
There is weak forces between layers

40
Q

Properties of graphine

A

one layer of graphite
one atom thick- one layer so if you see it sideway then it is one layer of carbon joined together so thickness of one carbon

41
Q

Properties of fullerenes

A

A molecule of carbon atoms forming a hallow 3D shapes
Based on hexagonal rings of carbon atoms
Rings may contain 5 to 7 carbon atoms
First discovered was fullerene Buckminster, fullerene
Can be used for drug delivery, a lubricant and a catalyst
Drug delevery- hexagonal ring can be used as a cage and put in a certain part

42
Q

Lubricant

A

Something that makes something slippery

43
Q

Why are fullerenes used to make tennis rackets?

A

Hard impact does not break will stretch

44
Q

Properties of fullernes- nanotubes

A 
Nanotubes are cyndrical fullerenes
High tensile strength
High electrical conductivity
High thermal conductivity
Used for reinforcing materials e.g tennis racket and bullet vests
if you stretch it it does not break
45
Q

In metallic bonding can you conduct electrecity

A

Yes because in atom there is a delocalised electron so it can carry charge

46
Q

Metallic bonding malleable?

A

yes, atoms can slide over each other

47
Q

Alloys

A

Mixture of metals

48
Q

What hapeens within a alloy

A

metal becomes stronger and it is difficult for layers to slide over each other because the layers are broken cause atoms are of different sizes

49
Q

States of matter- limitations of a particle model

A

Assumes that paticles are the same in reality from different elements
mass or size
the force of attraction between them
energy

50
Q

Melting point

A

point of temp when it turns from solid to liquid

When you heat a solid the particle svibrate and the force of attraction weakens

51
Q

Boiling point

A

Is when it turns from a liquid to a gas

they vibrate a lot and then the force of attractio breaks

52
Q

Melting and boiling point depends on:

A

The type of bonding and structure
covalent structure
the length of the chain( more links) and forces between particles

53
Q 
What are the state symbols for:
liquid
solid
gas
aqueous
54
Q

When aqueous?

A

When something is dissolved in water
Most acid and alkali solutions are aqueous
All acids have hydrogen
Alkalis will end in OH or O
Every liquid is aqueous unless it is a pure form like pure water
An ionic bond will be a aqueous

55
Q

Size of a nanometer

A

1 billion times smaller than a meter
Are smaller than fine particles( PM (2.5 lowercase))
Smaller than coarse particles( PM (10 in lower case))

56
Q

Because nanoparticles are so small they have a

A

very high surface area to volume ratio( useful in chemical reactions)

57
Q

Uses of nanoparticles: ( at least 4)

A 
Cosmetics
clothing
healthcare
industrial 
biomedical
food
catalyst
paint
58
Q

Why are people concerned about nm?

A

Because they say they can be toxic and can enter the bloodstream and brain.
Before increasing the number of us they should do more research

Yr9 Chemistery (6 decks)

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