Later C3

Question 1

Name the groups and what charge of ions they make from ionic bonding

Answer 1

1: +1
2: +2
3: +3
4: +4, -4
5: -3
6: -2
7: -1
0: ❌

Question 2

What is ionic bonding

Answer 2

Ionic compounds are held together by strong forces of attraction between their oppositely charged ions

Question 3

If you had: Al3+ and O2- what charge would you need for them to become neutral

Answer 3

(Al3+)2, (O2-)3 ( they both equal the same number of opposite charge, 6 is their LCM )

6+ and 6-

Question 4

What would happen in order for potassium ( K ) and oxygen (O) to correctly ionicly bond

Answer 4

Oxyegn needs 2 more electrons for a full outer shell. K has one on outer shell. x2 K to lose 1 electron each ( stable now ) to give to O which now has 8 on outer shell ( stable )

Question 5

Why can sea water conduct electricity

Answer 5

Sea water has salt in it and therefore the ions are free and separated so they are drawn to opposite charge and can carry a charge, therefore they can conduct electricity

Question 6

Why do ionic compounds have high melting points

Answer 6

It takes a lot of energy to break up every bond in the lattice since there are a lot of bonds to break and you have to overcome the electrostatic attraction and therefore you need immense heat to melt them

Question 7

Give the properties of an ionic solid

Answer 7

Ions are in fixed position in a giant lattice. They vibrate but cannot move around. It does not conduct electricty

Question 8

Give properties of molten ionic compound

Answer 8

High temperature provides enough energy to overcome the many strong attractive forces between ions. Ions are free to move around within the molten compound. It does conduct electricty

Question 9

Properties of ionic compound in solution

Answer 9

Water molecules separate ions from the lattice. Ions are free to move around within the solution. It does conduct electricty

Question 10

What are the difference between inter and intra molecular forces

Answer 10

Intermolecular forces: between molecules ( drawn as dotted lines )
Intramolecular forces: within the molecules ( drawn as lines )

Question 11

Describe what would happen if 2 hydrogen atoms covalently bonded

Answer 11

The two molecules would share electrons so that they each have 2 on the outer shell ( full and stable )

Question 12

Describe how a carbon atom would bond with two oxygen atoms

Answer 12

The carbon atom would share two of it’s 4 electrons with each of the oxygen atoms ( 2 each ) each of the oxygen atoms would also share their two electrons with carbon and have 4 spare. This means that each atoms has 8 electrons on the outer shell

Question 13

Which noble gas electron structure do the atoms in a molecule of hydrogen chloride attain?

Answer 13

Hydrogen would have 2 on outer shell: same as helium

Chlorine would be 2,8,8: same as Argon

Question 14

How do the covalent bonds bond the atoms to each other

Answer 14

The electro static attraction between the electrons and the positive nuclei on either side of the pair of electrons holds the atoms together

Question 15

What happens to the INTERmolecular forces when the INTRAmolecular forces are stronger

Answer 15

The intermolecular forces are weaker

Question 16

What happens to the INTERmolecular forces when the INTRAmolecular forces are weaker

Answer 16

The intermolecular forces are stronger

Question 17

What are the melting and boiling points of substances made of simple molcules

Answer 17

Both are lower

Question 18

Why do substances made of simple molecules have lower melting and boiling points

Answer 18

The forces between the molecules ( intermolecular ) are weak so they need little energy to melt or boil

Question 19

Why can’t molecules carry charge?

Answer 19

They have no overall charge so there is no electrostatic attraction so they can’t carry a charge

Question 20

Properties of giant covalent structures

Answer 20

Very high melting points
Insoluble in water
Do nkt conduct electricity

Question 21

What do chemists call different forms of the same element in the same state

Answer 21

Allotropes

Question 22

Why is graphite soft and slippery

Answer 22

It has covalent bonds horizontally although it has no covalent bonds connecting the layers so the layers can slide between one another

Question 23

Why is diamond so rigid

Answer 23

It is a gaint covalent structure making is very strong since the carbon bonded in all directions ( carbon atoms have each made 4 bonds )

Question 24

Why can graphite conduct electricity and thermal electricity

Answer 24

Every carbon has one electrons spare ( called delocalised electrons ) can move between the layers and carry a charge

Question 25

What medical use can fullerene cages provide

Answer 25

Delivering toxic drugs to cancerous cells to only kill off and damage the cancer cell amd not the rest of the cell

Question 26

What are bucky balls made out of

Answer 26

Hexagons of carbon

Question 27

What is graphene

Answer 27

A single layer of graphite and it was found when scientists in 2004 ripped selotape off graphite to get a layer one cell thick ( graphene )

Question 28

What is graphene usefull for

Answer 28

It is incredible strong for what it is

It is an excellent conductor

Question 29

What can graphene be used for in the future

Answer 29

It can be used to make more powerful computer chips and flexible electronic displays. Such as watching a film with a screen on your sleeve

Question 30

What was the first fullerene to be discovered

Answer 30

C60. A fullerene with 60 carbon atoms to make a sphere

Question 31

How did buckminster fullerene gets its name and what can it be abreviated to

Answer 31

A canadian scientist called Buckminster Fuller and can be abreviated to ‘ bucky ball ‘

Question 32

Why does the melting and boiling point and also conductivity of metals go up as the groups progress

Answer 32

Because they give as much delocalised electrons to the sea of delocalised electrons as their group number. E.g. group 3: each metal atom will delocalise 3 electrons.
This means that there is stronger electrostatic forces of attraction between the positive metal ions and the nucleus meaning it will take more energy to break them apart

Question 33

How are the ions arranged in a metallic lattice

Answer 33

In uniform and neatly

Question 34

Why can a metal be bent, shaped and pulled out into wire?

Answer 34

Because the atoms are arrangd regularly and can slide out over each other easily

Question 35

What is it called when a metal can be hammered into shape

Answer 35

Malleable

Question 36

What is it called when a metal can be pulled out into wires?

Answer 36

Ductile

Question 37

Why can alloying a metal make it harder

Answer 37

The different atoms in a metal can distort the uniform arrangement of the original metal so that the atoms cannot slide over one another as easily

Question 38

Why are metals good conductors of heat and electricity

Answer 38

The delocalised electrons can flow through the giant metallic lattice. The electrical charge and thermal energy transferred quickly through metal by the free - moving electrons

Question 39

What is an alloy

Answer 39

A mixture of two or more elements, at least one of which has to be a metal

Question 40

What is nanoscience

Answer 40

The study if small particles between 1 and 10 nanometres in size

Question 41

Why do materials behave differently when they are under 100nm in size?

Answer 41

Nanoparticles have a huge proportion of their molecules at the surface of the particle compared with a grain of sand

Question 42

What is the rule with surface area : volume ratio?

Answer 42

As a cube’s side decreases by 10 the SA : V ratio increases by 10

Question 43

Show how the SA : V rule works

Answer 43

Cube of 100cm sides: 
Surface Area = ( 100 x 100 ) x 6 ( cubes have 6 equal sides where you need to find area
V = (100 x 100x 100)cm3 = 1,000,000 cm3
SA : V ratio = 60,000cm2 : 1,000,000cm3
= 0.06 / cm
WHEREAS 
Cube of 10cm sides 
SA: ( 10 x 10 ) x6 = 600
V = ( 10 x 10 x 10 )cm3 = 1000cm3
SA : V ratio
= 600cm2 : 1000cm3 
= 0.6 / cm

Question 44

What does a high surface area : volume ratio give

Answer 44

They are highly reactive compared to other reactants

Question 45

What is better about using nanoparticles than other materials?

Answer 45

It means that the use of nanoparticles instead of traditional bulk materials should mean that smaller quantities are needed. Their high SA : V ratio means they are much more reactive than materials with normal particles sizes

Question 46

What does the use of nanoparticles mean for the future? 🚀🤷🏻

Answer 46

It will result in a more sustainable approach in industry as less resources are used up

Question 47

What is the length of 1 nanometre in metres

Answer 47

1 x 10^-9 metres or 0.0000000001 ( a billionth of a metre )

Question 48

What are delocalised electrons

Answer 48

Electrons that have not been used in bonding

Question 49

Where are the delocalised electrons in metallic bonding

Answer 49

In the sea of electrons

Question 50

Uses of nanoparticles

Answer 50

Silver nanoparticles to act as anti microbial surfaces for hospitals and keyboards
Titanium nanoparticles on windows to break down dirt through chemical resctions with sunlight

Question 51

Structure of graphite

Answer 51

Carbon atoms are bonded to three other ones. They form hexagons why are arranged in giant layers. There are only weak intermolecular forces attaching these layers vertically.

Question 52

Metallic bonding

Answer 52

Metals are a giant lattice of positively charged ions. The outer electrons can easily move around the giant structure in a sea of ions. Strong electrostatic attraction between the negatively charge electrons and positively charged ions bond the meatals ions together.