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chemistry > bonding, structure and properties of matter > Flashcards

bonding, structure and properties of matter Flashcards

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1
Q

features of solids

A

hard to compress
because packed together in a regular pattern with almost no spaces between the particles

fixed shape and cannot flow from place to place
they can vibrate tho

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2
Q

features of liquids

A

hard to compress
since particles are close together with not many spaces between them

take the shape of their container and flow from place to place
this is because the particles in a liquid can move

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3
Q

features of gases

A

very easy to compress
since particles are widely spaced

they spread out and fill the space of their container
because particles move quickly and random;y

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4
Q

how can we change the state of a substance

A

by putting in or taking out energy

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5
Q

a solid changing state to a liquid is?

and do u have to put energy in or take it out and why

A

melting

have to put energy in
because the particles in a liquid have more kinetic energy than the particles in a solid
(since they move more around).
This energy is needed to break the particles in a solid.

(this happens at melting point)

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6
Q

The stronger the forces of attraction between the particles, the ………… energy that we have to put in to break them and the …… the melting point

A

more

higher

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7
Q

liquid to a solid is

A

freezing

takes place at same temp as melting, aka at the melting point

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8
Q

liquid to gas is

A

boiling

takes place at boiling point

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9
Q

gas to liquid is

A

condensing

takes place at same temp as boiling, aka at boiling point

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10
Q

in ionic bonding, why do elements react and what do they achieve by doing this

A

to achieve a full outer energy level

by doing this, they achieve the electronic structure of a noble gas (full outer energy level)

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11
Q

when does ionic bonding occur

A

when a metal reacts with a non metal

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12
Q

what is an ion

A

an atom with an overall charge (happens after ionic bonding)

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13
Q

in ionic bonding, what happens to group1 metals

A

they lose one electron forming a plus 1 ion

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14
Q

in ionic bonding, what happens to group 7 non metals

A

gain one electron forming a 1 minus ion

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15
Q

ionic compounds form giant structures called what

A

called giant ionic lattices

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16
Q

are giant lattices 3 dimensional

A

yes

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17
Q

ionic compounds form giant structures where every positive ion is surrounded by ….. ions and vias versa

A

negative

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18
Q

in giant lattice structures, there are very strong forces between positive and negative ions, what do scientists call these?

A

electrostatic forces

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19
Q

what do electrostatic forces do

A

hold negative and positive ions in place

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20
Q

what do we call electrostatic forces that hold negative and positive ions in place

A

ionic bonds and they act in all directions

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21
Q

properties of ionic compounds

A

they have very high melting and boiling points

because ….

the strong electrostatic forces require a great deal of heat energy to break

they cannot conduct electricity when they are solid

because

the ions cannot move they are locked in place by strong electrostatic forces of attraction

however

they can conduct eelctricity when they are melted or dissolved in water

because

the ions can now move and carry the charge

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22
Q

when ionic compounds conduct electricity, what moves?

A

the ANODES (NOT THE ELECTRONS!!!)

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23
Q

in ionic bonding, the outer energy level is transferred from the …. atom to the …… atom

A

metal

non metal

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24
Q

ionic bonding produces ions which have electronic structure of what

A

a noble gas, in other words, a full outer energy level

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25
Q

when two non metal atoms bond together what happens

A

covalent bonding

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26
Q

covalent bonding is what

A

2 non metal atoms bonding together

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27
Q

diff between dot and cross diagram and energy level diagram and stick diagram

A

dot n cross only dot n cross whereas energy level includes a circle dots n crosses on / in circle,
stick diagram is like this

h-h the stick represents the single covalent bond, aka the shared pari of electrons

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28
Q

what is a covalent bond

A

a shared pair of electrons

29
Q

all covalent molecules are big/small?

A

small

30
Q

properties of small covalent molecules

A

low melting and boiling points

so

they are usually gases or liquid at room temp

because they all boil at temperatures below room temperature

the weak intermolecular forces between the molecules do not require a lot of energy to break

31
Q

intermolucular forces are always what and therefore wjat

A

weak and therefor do not require much energy to break

32
Q

why small covalent molcules have low melting and boiling points for liquid

A

becaue

molucules vibrate. …

Firstly, the atoms in each molecule are held together by strong covalent bonda

Secondly, there are weak intermolecular forces between one molecule and another aka between molecules

as we increase the temp, the vibration of the molecules increases, at a certain point this vibration is strong enough to break the weak intermolecular forces holding the molecules to each other, at this point, the molecules change state , in other words they boil and turn to a gas.
Because they have weak intermolecular forces it does not take much energy to turn small covalent molecules from liquid to gas

33
Q

as alkains (which are also small covalent molcules) get larger, their boiling point increases…why?

A

because the intermolecular forces increase and requir more energy to break

34
Q

another property with small covalent molecules

A

they do not conduct electricity

because

the molecules do not have an overall electric charge

35
Q

giant covalent molecules key fact abt room temp

A

they are always solids at room temp

because

they have millions of strong covalent bonds

meaning

they always have high melting and boiling points

36
Q

what element is diamond formed from

A

carbon

37
Q

in diamond, each carbon atom forms how many covalent bonds to …. other covalent atms

A

4

4

38
Q

why does diamond have a very high melting and boiling point

A

because each carbon atom forms four strong covalent bonds so diamonds have a huge number of covalent bonds and these have to be broken when diamond is melted so this requires a great deal of energy

39
Q

does diamond conduct electricity and why

A

no because there are no free electrons to carry electrical charge

40
Q

silicone dioxide key facts

A

high melting and boiling points

because

a huge number of strong covalent bonds must be broken and this takes a great deal of energy

41
Q

is graphite a form of carbon

A

yes

42
Q

three keys facts about graphite

A

high melting and boiling point

is soft and slippery

is an excellent conductor of electricity and of heat

43
Q

in graphite, each carbon atom forms how many covalent bonds

A

three

44
Q

in graphite, the carbon atoms form what kind of rings

A

hexagonal

45
Q

why has graphite got a high melting and boiling point

A

because graphite has many strong covalent bonds and so it takes much energy to break these , that’s why

46
Q

why is graphite slippery

A

because the hexagonal rings are arranged in layers. There are no covalent bonds between these layers so they can slide, which makes graphite slippery

47
Q

why is graphite not a metal

A

because it’s based on the element carbon

48
Q

why is graphite similar to metal (tho it’s not metal)

A

because both graphite and metal are good conductors of heat and electricity

because

they both have delocalised electrons that can move

49
Q

what is graphene and what does this mean

A

it is a single layer of graphite, meaning that it is one atom thick

50
Q

why is graphene an excellent conductor of electricity

A

because it has delocalised electrons

51
Q

graphene is very strong, making it useful for what

A

new materials

52
Q

what are fluerrens

A

molecules of carbon atoms with hollow shapes

53
Q

usually, what do fullerenes have however what can they also have

A

hexagonal rings of carbon atoms however they can also have rings with five or seven atoms

54
Q

what is the first fullerene molecule discovered

A

buckminsterfullerene

55
Q

what is buckminsterfullerene

A

the first fulerene molecule discovered

56
Q

uses of fuleerens

A

pharmaceuutical delivery

lubricants

catalysts

57
Q

what are carbon nanotubes

A

fullerenes shapes into long cyllinders

58
Q

useful properties of carbon nanotubes

A

they have high tensile strength (can be stretched without breaking)

excellent conductors of heat and electricity

59
Q

one use of carbon nanotubes

A

to reinforce materials

eg in tennis rackets

60
Q

what are polymers

A

very large molecules

61
Q

what are polymers made by

A

by joining together thousands of small, identical molecules (monomers)

62
Q

what are monomers often

A

alkene molecules eg ethene

63
Q

monomers have what kind of carbon bond

vs

polymer kind of cabron bond

A

a double, carbon to carbon covalnet bond

a single carbon to carbon covalent bond

(remember that because these bonds are covalent they are extremely strong)

64
Q

polymer facts

A

they are solids at room temp

because

the intermolecular forces of attraction between polymer molecules are relatively strong

65
Q

why polymers have high melting point

A

because there are many intermolecular forces of attraction acting between polymer molecules and they are strong so it takes a lot of energy to break these forces

66
Q

how do atoms become stable

A

by gaining a full outer energy level

67
Q

metals consist of a ………… …….. of atoms arranged how?

A

giant structure

arranged in regular layers

68
Q

in a metal, the electrons in the outer energy level of each atom are what?

A

delocalised

chemistry (11 decks)

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