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chemistry > bonding, structure and properties of matter > Flashcards

bonding, structure and properties of matter Flashcards

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
when two non metal atoms bond together what happens
covalent bonding
26
covalent bonding is what
2 non metal atoms bonding together
27
diff between dot and cross diagram and energy level diagram and stick diagram
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
28
what is a covalent bond
a shared pair of electrons
29
all covalent molecules are big/small?
small
30
properties of small covalent molecules
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
intermolucular forces are always what and therefore wjat
weak and therefor do not require much energy to break
32
why small covalent molcules have low melting and boiling points for liquid
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
as alkains (which are also small covalent molcules) get larger, their boiling point increases...why?
because the intermolecular forces increase and requir more energy to break
34
another property with small covalent molecules
they do not conduct electricity because the molecules do not have an overall electric charge
35
giant covalent molecules key fact abt room temp
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
what element is diamond formed from
carbon
37
in diamond, each carbon atom forms how many covalent bonds to .... other covalent atms
4 4
38
why does diamond have a very high melting and boiling point
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
does diamond conduct electricity and why
no because there are no free electrons to carry electrical charge
40
silicone dioxide key facts
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
is graphite a form of carbon
yes
42
three keys facts about graphite
high melting and boiling point is soft and slippery is an excellent conductor of electricity and of heat
43
in graphite, each carbon atom forms how many covalent bonds
three
44
in graphite, the carbon atoms form what kind of rings
hexagonal
45
why has graphite got a high melting and boiling point
because graphite has many strong covalent bonds and so it takes much energy to break these , that's why
46
why is graphite slippery
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
why is graphite not a metal
because it's based on the element carbon
48
why is graphite similar to metal (tho it's not metal)
because both graphite and metal are good conductors of heat and electricity because they both have delocalised electrons that can move
49
what is graphene and what does this mean
it is a single layer of graphite, meaning that it is one atom thick
50
why is graphene an excellent conductor of electricity
because it has delocalised electrons
51
graphene is very strong, making it useful for what
new materials
52
what are fluerrens
molecules of carbon atoms with hollow shapes
53
usually, what do fullerenes have however what can they also have
hexagonal rings of carbon atoms however they can also have rings with five or seven atoms
54
what is the first fullerene molecule discovered
buckminsterfullerene
55
what is buckminsterfullerene
the first fulerene molecule discovered
56
uses of fuleerens
pharmaceuutical delivery lubricants catalysts
57
what are carbon nanotubes
fullerenes shapes into long cyllinders
58
useful properties of carbon nanotubes
they have high tensile strength (can be stretched without breaking) excellent conductors of heat and electricity
59
one use of carbon nanotubes
to reinforce materials eg in tennis rackets
60
what are polymers
very large molecules
61
what are polymers made by
by joining together thousands of small, identical molecules (monomers)
62
what are monomers often
alkene molecules eg ethene
63
monomers have what kind of carbon bond vs polymer kind of cabron bond
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
polymer facts
they are solids at room temp because the intermolecular forces of attraction between polymer molecules are relatively strong
65
why polymers have high melting point
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
how do atoms become stable
by gaining a full outer energy level
67
metals consist of a ............ ........ of atoms arranged how?
giant structure arranged in regular layers
68
in a metal, the electrons in the outer energy level of each atom are what?
delocalised

chemistry (11 decks)

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