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GCSE chemistry > C3 > Flashcards

C3 Flashcards

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1
Q

What are ions

A

Charged particles

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2
Q

Why do atoms want to lose or gain electrons to form ions?

A

To form a full outer shell and become stable

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3
Q

What are positive ions called

A

Cations

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4
Q

What are negative ions called

A

Anions

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5
Q

What is ionic bonding

A

Transfering of electrons

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6
Q

What happens when a metal and non metal react togehter

A

Metal atoms loses electrons to form a positively charged ion and the non metal gains these electrons forming a negativelt chwrged ion. These oppositely charged ions are strongly attrachted to one another by electrostatic forces. This attraction is called ionic bond

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7
Q

How do to show how ionic compounds are formed ?

A

Dot and cross diagram (pg113)

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8
Q

What structure do ionic compounds have

A

Gaint ionic lattice. The ions form a closely packed regular lattice arrangment and there are very strong electrostatic forces of attraction between oppositely charged ions

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9
Q

What are the properties of ionic compounds?

A

They all have high melting points, many strong bonds between ions, takes alot of energy to overcome attraction. When they are solid, can’t conduct electricity and when they melt they are free to move and they carry electrical charge.

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10
Q

How do you work out the empirical formula of an ionic compound?

A

Look at diagram to work out what ions are in the compound. Then work out the charges in which the ions will form. Then balance the charges (bottom pg114)

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11
Q

When are covalent bonds created

A

When non metal atoms bond together sharing pair electrons to make covalent bonds

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12
Q

What makes covalent bonds very 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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13
Q

What does each single covalent bond provide

A

1 extra shared electron for each atom

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14
Q

Why is O2 a gass at room temperature

A

Because most molecular substances are gases or liquid at room temperature because very little energy is required to overcome these forces

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15
Q

Why does methane have a higher boiling point than hydrogen

A

Because the more intermolecular forces, the more energy is needed to break them down therefore the melting and boiling point increases

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16
Q

Why does nitogen not conduct electricity

A

Because molcular compounds do not conduct electricity because they arn’t charged so there are no free electrons or ions

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17
Q

What is a polymer

A

large molecule made up of repeating subunits known as monomers

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18
Q

How are all atoms in a polymer joined

A

Strong covalent bonds

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19
Q

Why do intermolcular forces have lower boiling points than ionic or covalent bonds

A

Intermolecular forces are weaker than ionic and covalent bonds

20
Q

How are giant covalent bonded to eachother

A

Strong covalent bonds

21
Q

Do giant covalent points have a higher or lower melting point

A

High because alot of energy is required to break them diwn

22
Q

Do giant covalent structure conduct electricity and if so why

A

No because they have no charged particles

23
Q

What are allotropes

A

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

24
Q

What structure does diamond have

A

Giant covalent structure

25
Q

In graphite, how many covalent bonds are formed

A

3

26
Q

In diamond, how many covalent bonds are formed

A

4

27
Q

Why does graphite have a high melting point

A

Covalent bonds need alot of energy to break down

28
Q

Are there covalent bonds between layers in a graphite and what does this mean

A

No covalent bonds between layers and held together weakly meaning they are free to move over eachother. Making the graphite soft and slippery - ideal as a lubricating metal

29
Q

What is the name of 1 graphite

A

Graphene

30
Q

What does graphene contain and what does this mean

A

Delocalised electrons meaning graphene can conduct electricity

31
Q

What is a fullerene

A

Molecules of carbon shaped like closed tubes or hollow balls

32
Q

What was the first fullerene to be discovered

A

Buckminsterfullerene c60- hollow sphere

33
Q

3 thing fullerenes can be used to do

A

1) cage other molecules - fullerene structure forms around an atom or molecule so this could be used to deliver a drug in the body
2) huge surface area so help make industrial catalysts
3) greats at making lubricants

34
Q

What are electrons in the outermost shell of metals and what does this mean

A

Delocalised meaning they are free to move around the shell. Strong forces of electrostatic attraction between positive metal ions and negative electrons

35
Q

What is metallic bonding

A

force of attraction between these free-moving (delocalised) electrons and positive metal ions

36
Q

What produces the properties of metals

A

Delocalised electrons

37
Q

Why are most metals a solid at room temp

A

Because electrostatic forces between metal atoms and the delocalised electrons are very strong and need alot of energy to be broken down

38
Q

Why are metals good conductors of electricity and heat?

A

Delocalised electrons carry charged and thermal energy meaning they are good conductors of heat and electricity

39
Q

What makes the metals malleable and what does this mean

A

Most metals can slide over eachother making the metals malleable meaning they can be bent, hammered, rolled

40
Q

What are alloys

A

Mixture of 2 or more metals

41
Q

Why are pure metals no right for certain jobs

A

Because pure metals are not strong enough so they are mixed with other metals so they are stronger called alloys

42
Q

Limitations of the particle model:

A

It assumes that psrticles are made up of solid spheres with no forces between them, however the particles that make up substances are atoms, molecules or ions.

43
Q

Ionic solid features:

A

-Ions are fixed in position in a giant lattice
-they vibrate but can’t move
-it doesnt conduct electricity

44
Q

Molten ionic compound features:

A

-high temperature which provides energy to overcome strong forces of attraction
-ions are free to move
-it does conduct electricity

45
Q

Ionic compound in solution:

A

-Water molecules seperate ions from the lattice
-ions are free to move around within the solution
-it does conduct electricity

46
Q

Properties of polymers

A

The intermolecular forces between polymer molecules are larger than between simple covalent molecules, so more energy’s needed to break down. This means most polymers are solid at room temperature.
The intermolecular forces are still weaker than ionic/covalent bonds, so have lower boiling points than ionic/giant molecular compounds

47
Q

Structure of silicon dioxide

A

GCSE chemistry (10 decks)

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