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Chemistry GCSE > Topic 2 - Bonding, Structure and Properties of Matter > Flashcards

Topic 2 - Bonding, Structure and Properties of Matter Flashcards

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1
Q

What is a compound?

A

A substance in which 2+ elements are chemically bound

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2
Q

List 3 types of strong chemical bonds.

A

Ionic
Covalent
Metallic

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3
Q

Which kind of elements form ionic bonds in a compound?

A

Metal and non-metal

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4
Q

Which kind of elements form covalent bonds in a compound (or element)?

A

Non-metals

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5
Q

Which kind of elements form metallic bonds?

A

Metals

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6
Q

What happens to electrons in ionic bonds?

A

The metals lose electrons to the non-metals, so both gain a full outer shell

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7
Q

What are the charges of the elements forming ionic bonds?

A

Metals lose electrons and form positively charged ions

Non-metals gain electrons and form negatively charged ions

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8
Q

Which forces attract oppositely charged ions?

A

Electrostatic forces

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9
Q

Which groups are most likely to form ions?

A

Groups 1, 2, 6 and 7

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10
Q

Group 1 and 2 are - and make - charged ions called - when they - electrons.

A

Group 1 and 2 are METALS and make POSITIVELY charged ions called CATIONS when they LOSE electrons.

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11
Q

Group 6 and 7 are - and make - charged ions called - when they - electrons.

A

Group 6 and 7 are NON-METALS and make NEGATIVELY charged ions called ANIONS when they GAIN electrons.

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12
Q

What is the structure of ionic compounds?

A

A giant ionic lattice - it is a regular structure and has strong electrostatic forces of attraction between oppositely charged ions in all directions in the lattice

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13
Q

What are the properties of ionic compounds?

A

High melting and boiling points
Can carry electric currents when melted or dissolved
Cannot conduct electricity when solid

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14
Q

Why do ionic compounds have high boiling points?

A

It takes a lot of energy to overcome the many strong bonds between the ions

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15
Q

Why can ionic compounds conduct electricity when liquid or dissolved in a liquid?

A

The ions can freely move around so can carry electric current

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16
Q

Why can’t ionic compounds conduct electricity when solid?

A

The ions can’t move so the compound can’t conduct electricity

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17
Q

What is an ion?

A

A charged particle

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18
Q

What is a covalent bond?

A

A shared pair of electrons

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19
Q

Why are covalent bonds strong?

A

The positively charged nuclei of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces

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20
Q

Which electrons do atoms share?

A

Only those in the outer shell/highest energy level

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21
Q

How many electrons are shared per covalent bond?

A

One from each atom (two)

22
Q

List three ways of drawing covalent bonds and draw water using each.

A

Dot and cross diagrams
Displayed formula
3D model

23
Q

What are the pros and cons of dot and cross diagrams?

A

Pros: show which atoms the electrons come from
Cons: don’t show relative sizes of atoms, don’t show how atoms are arranged in space

24
Q

What are the pros and cons of displayed formula?

A

Pros: show how atoms are connected in large molecules
Cons: don’t show 3D structure of molecule, nor which atoms the electrons in covalent bond have come from

25
Q

What are the pros and cons of 3D models?

A

Pros: show the atoms, the covalent bonds and their arrangement
Cons: get confusing for large molecules, don’t show where electrons in bonds come from

26
Q

What are the properties of simple molecular structures? (Covalent bonds)

A

Weak intermolecular forces -> low melting and boiling points -> smaller structures are gas or liquid at room temp. (bigger molecules -> stronger intermolecular forces -> higher b.p.)
Not charged -> don’t conduct electricity

27
Q

What are polymers?

A

Large covalently bonded molecules

28
Q

What are the boiling points of polymers?

A

Higher than of simple molecular structures so solid at room temp. (Larger particles -> stronger intermolecular bonds)
Lower than of ionic or giant molecular compounds

29
Q

What are macromolecules?

A

Giant covalent structures - all atoms bonded to each other by strong covalent bonds

30
Q

What are the properties of giant covalent structures and why?

A

High b.p. - lots of energy needed to break covalent bonds

Most don’t conduct electricity (even when molten) - don’t contain charged particles

31
Q

List three examples of giant molecular structures.

A

Diamond
Graphite
Silicon dioxide (sand)

32
Q

What are allotropes?

A

Different structural forms of the same element in the same physical state

33
Q

List allotropes of carbon.

A

Diamond
Graphite
Graphene
Fullerenes - buckminsterfullerene (C60), nanotubes

34
Q

What are the properties of diamond? Why?

A

Hard - each C atom has four covalent bonds
High melting point - strong covalent bonds take lots of energy to break
Doesn’t conduct electricity - no free electrons/ions

35
Q

What are the properties of graphite? Why?

A

Soft and slippery (good lubricating material) - no covalent bonds between layers so can move over each other
High melting point - strong covalent bonds
Conducts electricity and thermal energy - each C atom only makes 3 bonds, so one electron is delocalised

36
Q

What is graphene?

A

A sheet of carbon atoms joined in hexagons one atom thick

37
Q

What are the properties of graphene? Why?

A

Strong - covalent bonds
Light - can be added to composite material and improve strength with little weight inc.
Conducts electricity - each C atom has a delocalised electron

38
Q

What can fullerenes be used for?

A

To deliver drugs - they can “cage” other molecules (buckminsterfullerene)
As catalysts - high surface area
As lubricants

39
Q

What are the properties of nanotubes?

A

Conduct electricity and thermal energy

Have high tensile strength (don’t break when stretched)

40
Q

What can nanotubes be used in?

A

Nanotechnology - in electronics, to strengthen material without adding weight

41
Q

What does metallic bonding consist of?

A

Positive metal ions and delocalised electrons in a regular structure

42
Q

What are the properties of metals? Why?

A

High b.p. - strong electrostatic bonds between metal ions ans delocalised sea of electrons
Good conductors of electricity and thermal energy - delocalised electrons can carry electrical current and energy
Malleable - layers of atoms can slide over each other

43
Q

Why are alloys harder than pure metals?

A

The layers of pure metals can slide over each other
Different metals have differently sized atoms
The new metal distorts the layers of metal atoms, so they can’t slide over each other as easily

44
Q

What does the boiling point of a substance depend on?

A

The strength if the intermolecular binds - the stronger they are, the more energy is necessary ro break them so the higher the boiling point.

45
Q

Name the three states of matter.

A

Solid
Liquid
Gas

46
Q

What is the name of the temperature at which a liquid becomes a gas?

A

Boiling point

47
Q

What is nanoscience?

A

Using nanoparticles

48
Q

What are nanoparticles?

A

Particles with a diameter of 110^-9m to 110^-7m

49
Q

What is the equation for surface area to volume ratio?

A

Surface area to volume ratio = surface area/volume

50
Q

What is the surface area to volume ratio for nanoparticles?

A

High

51
Q

What are some uses for nanoparticles?

A 
Catalysts
Nano-medicine
As electric circuits in computer chips
Cosmetics
(Silver nanoparticles have antibacterial properties) added to polymer fibres used in surgical masks, wound dressing
52
Q

What afe the effects of nanoparticles on the body?

A

Unknown, leading to some people believing products containing nanoparticles should be clearly labelled as such

Chemistry GCSE (2 decks)

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