Topic 7- organic chemistry Flashcards
1
Q
What are group 7 metals also called?
A
Halogens
2
Q
Are group seven metals?
A
No
3
Q
What happens to the halogens as you go down the group
A
The get less reactive
They have higher melting and boiling points
4
Q
What are alkali metals also known as?
A
Group one
5
Q
Give some features of alkali metals
A
Soft
Low density
Very reactive
6
Q
Why are alkali metals so reactive
A
The outer electrons are a long way from the nucleus and have a weaker attraction
Easy to lose the one element
7
Q
What happens to the alkali metals as you go down the group?
A
They get more reactive
Low melting and boiling points
8
Q
What group are noble glasses
A
Group 0
9
Q
Metals have what sort of ion
A
Positive
10
Q
What do you atoms react to form?
A
A full outer shell of electrons
11
Q
Give some properties of transition metals?
A
good conductors
Shiny
Strong
Dense
12
Q
Where about on the table are transition metals
A
Central
13
Q
Get some properties of metals
A
Strong
malleable
conductors
high boiling and melting points
14
Q
Name the three parts of an atom and if they’re positive or negative
A
Proton positive
neutron neutral
electron negative
15
Q
Give the amount of electrons allowed on each shell
A
1,8,8
16
Q
How do you work out the amount of neutrons by looking at the amount of protons electrons and neutrons
A
Relative atomic mass= p+n
Atomic number= both electrons and protons
So…. relative atomic mass-atomic number= neutrons
(Electrons-little)
(Protons- little)
(Neutrons big take little)
17
Q
What are two parts to a chemical equation
A
Reactants and products
18
Q
What happens when elements react?
A
Atoms combine with other atoms to form compounds
19
Q
What is a compound?
A
2 or more elements together Ina substance
20
Q
Explain how fractional distillation works
A
Oil is heated until it’s a gas and the enters a fractionating column
The column is coolest at the top and hottest at the bottom
The long hydrocarbons have high boiling points they condense back to liquids and leave the column early on at the bottom
The shorter hydrocarbon length means it’s got a lower point and they leave to column later, once they’ve condensed at the top
21
Q
What are the alkanes like at the top of the column
A
Alkanes are shorter
less viscous
more volatile
22
Q
What are the alkanes like at the bottom of the column
A
Alkanes longer
More viscous
Less volatile
23
Q
How are hydrocarbons made
A
The plankton dies and gets covered with mud. Pressure and heat builds up and then the newly made hydrocarbons get dug up
24
Q
What are the hydrocarbons in crude oil called?
A
Alkanes and alkenes
25
How is crude oil separated?
Fractional distillation
26
Name the two atoms that make a hydrocarbon
Hydrogen
| Carbon
27
Are alkanes saturated or unsaturated?
Saturated
28
What is crude oil
A mixture of different compounds
29
Are alkenes saturated
No, they're unsaturated
30
By cracking hydrocarbons what are made
Alkenes and alkanes
31
What's the rhyme for alkanes and alkenes
Men eat polar bears
32
What do alkenes have?
A double bond
33
What's the formula for alkenes
CnH2n
| ^
34
What's the polymer displayed formula
( h h )
-(-c-c-)-
( h h
35
How do you show an alkenes reacting with hydrogen?
The double bond opens up and lets in the new amount of hydrogen(2)
36
What does ethene and steam make?
Ethanol
37
What do you do to Ethene when steam (h20) is added
Remove the double bond and add an O-H
38
What happens when hydrocarbon fuels are burned in plenty of air
The hydrogen and carbon in the fuel become completely oxidised- complete combustion
39
The shorter the carbon chain the...
Less viscous
More volatile
More flammable
40
What makes an ester
An alcohol and a carboxylic acid
41
How do you make an ester displayed formular
You do the carboxylic acid minus the h
You connect that to the original alkane minus the h
42
Can alkenes react with halogens
Yep!
43
What's bromine and ethene?
Dibromoethane
44
Give the equation for incomplete combustion
Fuel+ bit of oxygen=> carbon monoxide and water
45
Why is carbon monoxide produced in incomplete combustion
When there isn't enough oxygen
46
Give the equation for complete combustion
Fuel+bit of oxygen=> carbon dioxide+ water+ heat
47
What does limewater do and what does it test for
Cloudy/milky
| carbon dioxide
48
What is cobalt chloride paper a test for
Water vapour
49
Give the formula for alkanes
CnH(2n+2)
50
What's the equation for propane
C3H8
51
What does every carbon atom have
4 bonds
52
What's the end part of a carboxylic acid
COOH
53
Give the four carboxylic acids
Methanoic
Ethanoic
Propanoic
Butanoic
54
Give the letters for esters
Cooc
55
Give the first four esters
```
Methyl
Ethyl
Propyl
Butyl
(Methanoate, ethanoate etc)
```
56
How do you draw the displayed formula for a carboxylic acid
Take 3 Hs from the alkane
Add a double bond oxygen and an O-H
57
What are polymers made up of
Lots of the same molecules joined together in one long chain
58
What do polymers make
Plastic
59
Lots of small monomers make...
Polymers
60
What's the reaction called that makes polymers
Polymerisation
61
How can polymers be made with alkenes
The double bond can open up and join together to make a polymer
62
Lots of ethene molecules make,,,
Polythene
| Poly(ethene)
63
Give the four alcohols
Methanol
Ethanol
Propanol
Butanol
64
How do do make an alcohol displayed formula
Remove one h and add an o-h
65
What's a fuel?
A source that releases energy from a store whilst using oxygen from the atmosphere when a fuel is burned, energy is made, carbon dioxide and smoke is released
66
What's the carbon footprint
A measure of the amount of carbon dioxide and other greenhouse gases released over a cycle
67
How do I reduce the carbon footprint
Using renewable energy resources
| More efficient processes putting a cap on emissions
68
What does sulfur dioxide make
Acid rain
69
Name three greenhouse gases
Corbin dioxide methane water vapour
70
What do greenhouse gases act as
Insulation layer
71
Explain the greenhouse effect
Greenhouse gases absorb long wavelength radiation they then reradiate in all directions including back towards earth longwave radiation is thermal radiation which makes the warming of the Earth happen
72
Give some causes of climate change
Burning fossil fuels volcanoes erupting sunspot cycle
cutting down trees
transport
73
Yes some consequences of a climate change
Rising sea levels agricultural effects extinction
more natural rain and temperatures disasters
ice caps melting
74
How has the oxygen increased
Algae used energy from the Sun to do photosynthesis releasing oxygen. Algae and bacteria thrive In the sea
75
How did the carbon dioxide decrease
It got locked into rocks and dissolved in the new oceans
76
How did nitrogen increase
By volcanoes producing it
77
Methane and ammonia
Oxygen reacted with it
78
Describe the early atmosphere
```
Hot climate
volcanic eruptions
no human life
no water
no oxygen
```
79
How is water collected by
Icy comets
| hollows which formed oceans
80
How does bromine water work
When orange bromine water is added to saturated compounds, (alkanes) it will stay bright orange but when added to an alkene the bromine water it will go colourless
81
What process happens in cracking
Thermal de composition
82
What is cracking
Splitting up long chain hydrocarbons (paraffin)
83
Which type of chain is useful
Short chain
84
Explain cracking
Heat long chain hydrocarbons which produce gas
Vapour passed over catalyst
Long chains split apart on the catalyst surface
85
What's the percentages of chemicals in atmosphere today
Oxygen 21% nitrogen 78% carbon dioxide 0.03% other 1%
86
What was the early atmosphere like with chemicals
Ammonia carbon dioxide water vapour and nitrogen methane little oxygen
87
What’s evaporation used for?
To separate soluble salt from a solution
88
Explain evaporation
The solvent evaporated after being heated leaving a more concentrated solution and dry crystals are left over
89
Explain crystallisation
the solution in the evaporating dish gently heats up. Some solvent evaporated and solution gets more concentrated. Crystals form in fish
90
What’s paper chromatography used for?
Separating dyes in an ink
91
explain chromatography
Each different dye in an ink will move up the paper at different rates so the dyes separate out and form spots at different points
92
What will happen in chromatography if any insolubles are present,
They will stay on the baseline
93
Explain filtration
filtration paper holds the solids after the liquid has been put through it
94
when is filtration used
if your product is an insoluble solid that needs to be separated from a liquid reaction mixture
95
what is special about chemical bonds in mixtures
there aren’t any
96
What do mixtures contain
elements and compounds
97
what processes can separate mixtures
```
filtration
crystallisation
simple distillation
fractional distillation
chromatography
```
98
What are products
The end bit of the equation
99
what are reactants
the start but of the equation
100
How are compounds formed
when elements react, atoms combine with other atoms to form compounds
101
what’s a compound
substances formed from 2 or more elements
102
What are bonds
when atoms give away take or share electrons
103
Explain ionic bonding
When metals and non-metals react together to form an outer shell
Metal atoms lose electrons and become positive ions
nonmetals gain electrons and become negative ions
104
Explain covalent bonding
Between nonmetals and nonmetals
each atom shares an electron with another atom to form a full outer shell
example hydrogen chloride carbon monoxide water
105
Which energy levels are always field first
The lowest because they’re closest to the nucleus
106
how many electrons are allowed on each shell
two on the inner and every other shell eight
107
What happens when the outer shell isn’t full
it makes the atom want to react to fill it
108
explain the first thought about the atom
John Dalton thought different spheres made up different elements (solid spheres )
109
explain the plum pudding model
JJ Thomson concluded that it atoms weren’t solid spheres
his measurements of charge and mass showed that atom must contain even smaller negatively charged particles called electrons
the plum pudding model shows the atom as a ball
/cloud of positive charge with electrons to cut it
110
Explain the nuclear model
Ernest Rutherford invented it
he fired positively charged alpha particles at an extremely thin sheet of gold
they expected the particles passed straight through the sheet or be slightly defective at most because the positive charge for each atom was thought to be very spread out through the pudding
but whilst most the particles did go straight through the gold sheet some were deflected more than expected
small numbers deflected backwards so the plum pudding couldn’t be right
Rutherford came up with the nuclear model in this there is a tiny positively charged nucleus at the centre where the most of the atom is empty space
when alpha particles came near the concentrated positive charge of the nucleus they were deflected
if they were fired directly at the nucleus they reflected back otherwise they pass through empty space
111
what’s an element
A substance made up of atoms that all have the same number of protons in the nucleus
112
What does the number of protons decide
What type of atom it is example one proton the nucleus equals hydrogen two protons equals helium
113
How many different elements are there around about
100
114
What do particular elements have
Same number of protons
115
What do different elements have
Different number of protons
116
What are isotopes
Different forms of the same element which have the same number of protons but different number of neutrons
117
What dogroup 0 elements have
Full outer shell
118
Explain noble gas properties
Don’t react much Colourless
nonflammable
boiling point increases and so does relative atomic mass as you go down the group
119
What does metallic bonding cause
Similar basic physical properties
120
Explain metals properties
Strong malleable good conductors of heat and electricity high boiling and melting points
121
Explain the properties of nonmetals
dull brittle don’t conduct low-density aren’t always solids
122
what do atoms react to form
A full outer shell
123
How do you atoms react to form a full outer shell
Via losing gaining or sharing electrons
124
Explain metals on the left of the periodic table
they don’t have many electrons to remove
125
explain metals towards the bottom of the periodic table
Have outer electrons which are a long way from the nucleus so have a weaker attraction not much energy is needed to remove electrons therefore reactive and it’s feasible To react to form positive irons with a full outer shell
126
What are metals
Elements which can form positive ions when they react
127
where are metals on the periodic table
towards the bottom and to the left of the periodic table
128
Where are non-metals on the periodic table
at the far right and top of the periodic table
129
What don’t nonmetals generally form when they react
Positive ions
130
Describe Dimitri Mendeleev’s table
He left gaps for predicted new elements
Order of atomic mass but switched order if properties meant it should be changed
131
In the 1800s what did the periodic table look like
ordered by Atomic mass physical and chemical properties and their relative atomic mass
132
Why is it hard for non-metals to form positive ions
Because that either to the right of the periodic table where they have lots of electrons to move to gain full outer shell
or towards the top where the outer electrons are close to the nucleus so feel strong attraction therefore they either share or gain electrons
133
Explain the modern periodic table
100-ish elements
order of increasing atomic number
repeating patterns in properties of elements handy for working out which elements are metals and which are non-metals
metals are on the left nonmetals are on the right
134
What do you elements with similar properties forms
columns
135
What a vertical columns called
Groups
136
What does the group number describe
how many electrons are in the outer shell
137
explain group 1 trends
elements react more vigourously as you go down the group because the electron is further away from the nucleus lower melting and boiling points as you go down the group
138
What are group on metals also called
Alkali metals
139
Explain the alkali metals
Don’t need much energy to lose their one outer electron to form a full outer shell
140
what’s more reactive transition metals or alkali metals
Alkali metals
141
Give some properties of alkali metals
Leston stronger and harder than transition metals have lower points than transition metals
142
explain the reactivity of the halogens
reactivity decreases as you go down the group
143
what are rows called
periods
144
What does each period
Present
Another full shell of electrons
145
Are halogens metals or nonmetals
Nonmetals
146
As you go down the group the halogens are
Less reactive higher melting and boiling points higher relative atomic mass
147
what type of bonding can halogens uses
Covalent bonding and ionic bonding
148
1-ions=?
halides
149
What’s distillation used to do
separate mixtures which contain liquids
150
explain simple distillation
solution is heated
the lowest boiling point evaporates first
vapour is cooled and condenses and turns back into liquid by the water the outer tube
the rest of the solution is left in the flask
151
how do you draw a covalent drawing
you see how many electrons has its outer shell then subtract that number away from 8 to find out how many covalent bonds it needs
152
How do you know if a covalent bond is single or double
You look at how many bonds it shared from each shell
153
what structure do ionic compounds have
A regular lattice structure a structure called a giant ionic lattice
154
Explain ionic compound structure
irons form closely packed regular lattice arrangement and they’re very strong electrostatic forces of attraction between oppositely charged ions in all directions
155
What ionic compounds boiling and melting points like and why
High because the strong bonds between the ions
156
explain a solid ionic compound
Ions are in place compounds can’t conduct electricity
157
explain ionic compound when it melts
ions are free to move and carry electric current
158
Why do ionic compounds dissolve easily
because Ions separate all free to move in solution
159
when are ions made
when electrons are transferred
160
ions are...
charged particles which can be single or in groups
161
if two electrons are lost the charge is...
2+
162
three electrons are gained the charge is...
3-
163
which groups most readily form ions
One and two are metals and lose electrons to form positive irons
164
which other groups most readily form Iions
67 a non-metal also gain electrons to form negative ions
165
explain the groups with charges
Group 1= 1+
2=2+
6=2-
7=1-
166
what is covalent bonding between
nonmetals and nonmetals
167
what happens when elementa bond together in covalent bonding
they share pairs of electrons to make covalent bond
168
What makes covalent bonds strong
positively charged nucleus of the bonded atoms are attracted to the shared pair of electrons by electrostatic forces making covalent bond is very strong
169
what does each single covalent bond provide
One extra shared electron for each atom
170
What does having a full outer shell mean for a noble gas
the electronic structure of a noble gases very stable
171
what is simple molecular substances made up of
molecules containing a few atoms joined together by covalent bonds
172
give the properties of simple molecular substances
very strong covalent bonds in the atoms which means by contrast the attraction between his molecules very weak
173
are the melting and boiling points high or low
low because the molecules are easily parted from each other
174
what a simple molecular substances like at room temperature
gases or liquids
175
The bigger the molecules the strength of the intermolecular forces...
increases so r more energy is needed to break them
176
Why don’t simple molecular substances conduct electricity
because they aren’t charged so there are no free electrons or irons
177
what are polymers
Long chains of repeating units
178
what all the atoms in a polymer joined by
strong covalent bonds
179
What type of covalent bonds to giant structures have
strong
180
Descry the boiling and melting points of giant covalent structure is
very high melting and boiling points as lots of energy is needed to break the covalent bonds between the atoms
181
what don’t giant covalent structures do
have charged particles or conduct electricity
182
give two examples of giant covalent structures
Diamond graphite
183
Describe the giant covalent bond in diamond
each carbon atom forms for covalent bonds in a rigid giant covalent structure
184
describe the giant covalent bond in graphite
each carbon atom forms three covalent bonds to create layers of the hexagons
each carbon atom also has one delocalised electrons
185
What are nonmetals and metals attracted by in ionic bonding
electrostatic forces
186
what is the metals symbol in a dot and cross diagram
.
187
what’s the symbol for a non-metal in a dot and cross atom
cross
188
describe metallic bonding
There are strong forces of electrostatic attraction between the positive irons and the shared negative electrons
these forces of attraction hold the atoms together in a regular structure the electrostatic forces are stronger need lots of energy to be broken
the electrons on the outer shell are de localised and carry an electric current
malleable because layers of atoms slide over each other
189
Describe the changes in state
In a solid the particles are packed closely together and can move in fixed positions
when the surroundings get hotter the particles gain heat energy therefore they begin to move more this is a solid turning into liquid
when this has happened the particles are touching and still moving around each other
the particles now gain energy faster and therefore move faster and eventually boil into a gas where the particles move very fast
