C3

Question 1

what are the states of matter

Answer 1

solid, liquid, gas and plasma

Question 2

what is the structure of solids

Answer 2

molecules are packed together tightly

Question 3

what is the structure of liquids

Answer 3

they are packed close together but can slip and slide over each other

Question 4

what is the structure of gases

Answer 4

have lots of space between them

Question 5

what is it called when a solid turns into a gas

Answer 5

sublimation

Question 6

what is it called when a gas turns into a solid

Answer 6

deposition

Question 7

where does ionic bonding take place

Answer 7

between non-metals and metals

Question 8

what happen when sodium (has 1 electron in it’s outer shell) gives 1 electron to chlorine (has 7 electrons in it’s outer shell)

Answer 8

sodium loses 1 electron and Chlorine gains 1 electron so they both have a full outer shell. sodium becomes a +1 ion and Chlorine becomes a -1 ion. since they are positive and a negative ions they will attract each other forming a strong covalent bond

Question 9

why do molecules ionically bonded together have high melting and boiling points

Answer 9

ionic bonds are really strong so they require a lot of energy to overcome

Question 10

when can ionic compounds conduct electricity

Answer 10

when melted or are dissolved in water due to that causing the particle to move around freely

Question 11

the formula for a hydroxide ion

Answer 11

OH -

Question 12

the formula for a sulfate ion

Answer 12

SO4 2-

Question 13

the formula for a nitrate ion

Answer 13

NO3 -

Question 14

the formula for a carbonate ion

Answer 14

CO3 2-

Question 15

the formula for a ammonium ion

Answer 15

NH4 +

Question 16

the formula for a calcium hydroxide ion

Answer 16

CaOH

Question 17

where does metalic bonding take place

Answer 17

in metals

Question 18

what happens in a metal which causes electrons to be delocalised

Answer 18

the metal atoms give up their outer most electrons turning into ions and are therefore ‘sharing’ the electron which are now delocalised.

Question 19

why can metals conduct electricity

Answer 19

due to the delocalised electrons

Question 20

why does it require a lot of energy to break a metallic bond

Answer 20

the delocalised electrons acts like a glue, sticking the metal together due to the strong electrostatic forces which bond the metal ions together.

Question 21

will ionic compounds conduct electricity

Answer 21

yh, it will

Question 22

what happens in a covalent bond

Answer 22

electrons are shared

Question 23

what are intermolecular forces

Answer 23

forces which hold covalently bonded compounds close to each other

Question 24

how strong are intermolecular forces

Answer 24

easy to break

Question 25

how strong are covalent bonds

Answer 25

they are very strong so they need a lot of energy to break

Question 26

where does covalent bonding happen

Answer 26

in non-metals

Question 27

what are simple molecules

Answer 27

a covalently bonded molecule with a low boiling and melting point which doesn’t have a continuous repetitive chain of molecules.

Question 28

what are some examples of simple molecules

Answer 28

water and methane

Question 29

why do simple molecules have low melting and boiling points

Answer 29

they have very weak intermolecular forces

Question 30

do simple molecules conduct electricity and why

Answer 30

no they don’t as they have no overall charge

Question 31

why do giant covalent structures have high melting and boiling points

Answer 31

because you need to break the covalent bonds themselves and not the intermolecular themselves.

Question 32

how can you tell if something is a giant covalent structure

Answer 32

they have regular repeating lattices

Question 33

do giant covalent structures conduct electricity

Answer 33

no they don’t

Question 34

name me the properties of the allotrope diamond

Answer 34

each carbon atom is covalently bonded to 4 others
the bond in each molecule is very strong
don’t conduct electricity as they don’t have spare electrons
are hard substances

Question 35

name me the properties of graphene

Answer 35

a single layer of graphite
do conduct electricity due to the free electron
one atom thick
low density
excellent conductor of heat and electricity]

Question 36

name me the properties of quartz

Answer 36

strong covalent bonds = high melting and boiling point
are hard substances
don’t conduct electricity due to 1 molecule being bonded with 4 others

Question 37

name the properties of graphite

Answer 37

each carbon atom is bonded to 4 others
strong covalent bonds
there are free electrons so they can conduct electricity
weak forces of attraction between each layer of graphite (graphene) so they can slide over each other

Question 38

name the properties of fullerenes

Answer 38

molecules of carbon atoms with hollow shapes
based on hexagonal rings of carbon
rings may contain 4 or 5 carbon atoms
can be used for drug delivery

Question 39

name me the properties of nanotubes

Answer 39

high tensile strength
high electric conductivity
high thermal conductivity
used for reinforcing materials

Question 40

what is an alloy

Answer 40

a metal with 2 or more types of elements used to make the metal stronger

Question 41

what are the properties of a pure metal

Answer 41

can be bent and shaped because the layer of atoms can slide over each other
delocalised electrons can allow electricity and thermal energy to pass through

Question 42

why is an allow stronger than a pure metal

Answer 42

an alloy has different shaped atoms which means there won’t be straight rows of metal; it’ll be misshaped so layers will find it difficult to slide over each other

Question 43

what are the size of nanoparticles

Answer 43

1nm- 100nm

Question 44

what the surface area : volume ratio of nanoparticles

Answer 44

high

Question 45

what are some uses of nanoparticles

Answer 45

catalysts
medicine
electrical circuits

Question 46

and you are f-

Answer 46

-inally done