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CHEMISTRY -EVIE💘 > Topic 7- organic chemistry > Flashcards

Topic 7- organic chemistry Flashcards

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1
Q

What are group 7 metals also called?

A

Halogens

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2
Q

Are group seven metals?

A

No

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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

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4
Q

What are alkali metals also known as?

A

Group one

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5
Q

Give some features of alkali metals

A

Soft
Low density
Very reactive

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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

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7
Q

What happens to the alkali metals as you go down the group?

A

They get more reactive

Low melting and boiling points

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8
Q

What group are noble glasses

A

Group 0

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9
Q

Metals have what sort of ion

A

Positive

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10
Q

What do you atoms react to form?

A

A full outer shell of electrons

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11
Q

Give some properties of transition metals?

A

good conductors
Shiny
Strong
Dense

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12
Q

Where about on the table are transition metals

A

Central

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13
Q

Get some properties of metals

A

Strong
malleable
conductors
high boiling and melting points

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14
Q

Name the three parts of an atom and if they’re positive or negative

A

Proton positive
neutron neutral
electron negative

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15
Q

Give the amount of electrons allowed on each shell

A

1,8,8

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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)

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17
Q

What are two parts to a chemical equation

A

Reactants and products

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18
Q

What happens when elements react?

A

Atoms combine with other atoms to form compounds

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19
Q

What is a compound?

A

2 or more elements together Ina substance

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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

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21
Q

What are the alkanes like at the top of the column

A

Alkanes are shorter
less viscous
more volatile

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22
Q

What are the alkanes like at the bottom of the column

A

Alkanes longer
More viscous
Less volatile

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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

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24
Q

What are the hydrocarbons in crude oil called?

A

Alkanes and alkenes

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25
Q

How is crude oil separated?

A

Fractional distillation

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26
Q

Name the two atoms that make a hydrocarbon

A

Hydrogen

Carbon

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27
Q

Are alkanes saturated or unsaturated?

A

Saturated

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28
Q

What is crude oil

A

A mixture of different compounds

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29
Q

Are alkenes saturated

A

No, they’re unsaturated

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30
Q

By cracking hydrocarbons what are made

A

Alkenes and alkanes

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31
Q

What’s the rhyme for alkanes and alkenes

A

Men eat polar bears

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32
Q

What do alkenes have?

A

A double bond

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33
Q

What’s the formula for alkenes

A

CnH2n

^

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34
Q

What’s the polymer displayed formula

A

( h h )
-(-c-c-)-
( h h

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35
Q

How do you show an alkenes reacting with hydrogen?

A

The double bond opens up and lets in the new amount of hydrogen(2)

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36
Q

What does ethene and steam make?

A

Ethanol

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37
Q

What do you do to Ethene when steam (h20) is added

A

Remove the double bond and add an O-H

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38
Q

What happens when hydrocarbon fuels are burned in plenty of air

A

The hydrogen and carbon in the fuel become completely oxidised- complete combustion

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39
Q

The shorter the carbon chain the…

A

Less viscous
More volatile
More flammable

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40
Q

What makes an ester

A

An alcohol and a carboxylic acid

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41
Q

How do you make an ester displayed formular

A

You do the carboxylic acid minus the h

You connect that to the original alkane minus the h

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42
Q

Can alkenes react with halogens

A

Yep!

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43
Q

What’s bromine and ethene?

A

Dibromoethane

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44
Q

Give the equation for incomplete combustion

A

Fuel+ bit of oxygen=> carbon monoxide and water

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45
Q

Why is carbon monoxide produced in incomplete combustion

A

When there isn’t enough oxygen

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46
Q

Give the equation for complete combustion

A

Fuel+bit of oxygen=> carbon dioxide+ water+ heat

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47
Q

What does limewater do and what does it test for

A

Cloudy/milky

carbon dioxide

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48
Q

What is cobalt chloride paper a test for

A

Water vapour

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49
Q

Give the formula for alkanes

A

CnH(2n+2)

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50
Q

What’s the equation for propane

A

C3H8

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51
Q

What does every carbon atom have

A

4 bonds

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52
Q

What’s the end part of a carboxylic acid

A

COOH

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53
Q

Give the four carboxylic acids

A

Methanoic
Ethanoic
Propanoic
Butanoic

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54
Q

Give the letters for esters

A

Cooc

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55
Q

Give the first four esters

A 
Methyl
Ethyl 
Propyl
Butyl
(Methanoate, ethanoate etc)
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56
Q

How do you draw the displayed formula for a carboxylic acid

A

Take 3 Hs from the alkane

Add a double bond oxygen and an O-H

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57
Q

What are polymers made up of

A

Lots of the same molecules joined together in one long chain

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58
Q

What do polymers make

A

Plastic

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59
Q

Lots of small monomers make…

A

Polymers

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60
Q

What’s the reaction called that makes polymers

A

Polymerisation

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61
Q

How can polymers be made with alkenes

A

The double bond can open up and join together to make a polymer

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62
Q

Lots of ethene molecules make,,,

A

Polythene

Poly(ethene)

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63
Q

Give the four alcohols

A

Methanol
Ethanol
Propanol
Butanol

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64
Q

How do do make an alcohol displayed formula

A

Remove one h and add an o-h

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65
Q

What’s a fuel?

A

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

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66
Q

What’s the carbon footprint

A

A measure of the amount of carbon dioxide and other greenhouse gases released over a cycle

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67
Q

How do I reduce the carbon footprint

A

Using renewable energy resources

More efficient processes putting a cap on emissions

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68
Q

What does sulfur dioxide make

A

Acid rain

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69
Q

Name three greenhouse gases

A

Corbin dioxide methane water vapour

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70
Q

What do greenhouse gases act as

A

Insulation layer

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71
Q

Explain the greenhouse effect

A

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

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72
Q

Give some causes of climate change

A

Burning fossil fuels volcanoes erupting sunspot cycle
cutting down trees
transport

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73
Q

Yes some consequences of a climate change

A

Rising sea levels agricultural effects extinction
more natural rain and temperatures disasters
ice caps melting

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74
Q

How has the oxygen increased

A

Algae used energy from the Sun to do photosynthesis releasing oxygen. Algae and bacteria thrive In the sea

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75
Q

How did the carbon dioxide decrease

A

It got locked into rocks and dissolved in the new oceans

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76
Q

How did nitrogen increase

A

By volcanoes producing it

77
Q

Methane and ammonia

A

Oxygen reacted with it

78
Q

Describe the early atmosphere

A 
Hot climate
 volcanic eruptions
 no human life
 no water 
no oxygen
79
Q

How is water collected by

A

Icy comets

hollows which formed oceans

80
Q

How does bromine water work

A

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
Q

What process happens in cracking

A

Thermal de composition

82
Q

What is cracking

A

Splitting up long chain hydrocarbons (paraffin)

83
Q

Which type of chain is useful

A

Short chain

84
Q

Explain cracking

A

Heat long chain hydrocarbons which produce gas

Vapour passed over catalyst

Long chains split apart on the catalyst surface

85
Q

What’s the percentages of chemicals in atmosphere today

A

Oxygen 21% nitrogen 78% carbon dioxide 0.03% other 1%

86
Q

What was the early atmosphere like with chemicals

A

Ammonia carbon dioxide water vapour and nitrogen methane little oxygen

87
Q

What’s evaporation used for?

A

To separate soluble salt from a solution

88
Q

Explain evaporation

A

The solvent evaporated after being heated leaving a more concentrated solution and dry crystals are left over

89
Q

Explain crystallisation

A

the solution in the evaporating dish gently heats up. Some solvent evaporated and solution gets more concentrated. Crystals form in fish

90
Q

What’s paper chromatography used for?

A

Separating dyes in an ink

91
Q

explain chromatography

A

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
Q

What will happen in chromatography if any insolubles are present,

A

They will stay on the baseline

93
Q

Explain filtration

A

filtration paper holds the solids after the liquid has been put through it

94
Q

when is filtration used

A

if your product is an insoluble solid that needs to be separated from a liquid reaction mixture

95
Q

what is special about chemical bonds in mixtures

A

there aren’t any

96
Q

What do mixtures contain

A

elements and compounds

97
Q

what processes can separate mixtures

A 
filtration 
crystallisation 
simple distillation 
fractional distillation 
chromatography
98
Q

What are products

A

The end bit of the equation

99
Q

what are reactants

A

the start but of the equation

100
Q

How are compounds formed

A

when elements react, atoms combine with other atoms to form compounds

101
Q

what’s a compound

A

substances formed from 2 or more elements

102
Q

What are bonds

A

when atoms give away take or share electrons

103
Q

Explain ionic bonding

A

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
Q

Explain covalent bonding

A

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
Q

Which energy levels are always field first

A

The lowest because they’re closest to the nucleus

106
Q

how many electrons are allowed on each shell

A

two on the inner and every other shell eight

107
Q

What happens when the outer shell isn’t full

A

it makes the atom want to react to fill it

108
Q

explain the first thought about the atom

A

John Dalton thought different spheres made up different elements (solid spheres )

109
Q

explain the plum pudding model

A

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
Q

Explain the nuclear model

A

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
Q

what’s an element

A

A substance made up of atoms that all have the same number of protons in the nucleus

112
Q

What does the number of protons decide

A

What type of atom it is example one proton the nucleus equals hydrogen two protons equals helium

113
Q

How many different elements are there around about

A

100

114
Q

What do particular elements have

A

Same number of protons

115
Q

What do different elements have

A

Different number of protons

116
Q

What are isotopes

A

Different forms of the same element which have the same number of protons but different number of neutrons

117
Q

What dogroup 0 elements have

A

Full outer shell

118
Q

Explain noble gas properties

A

Don’t react much Colourless
nonflammable
boiling point increases and so does relative atomic mass as you go down the group

119
Q

What does metallic bonding cause

A

Similar basic physical properties

120
Q

Explain metals properties

A

Strong malleable good conductors of heat and electricity high boiling and melting points

121
Q

Explain the properties of nonmetals

A

dull brittle don’t conduct low-density aren’t always solids

122
Q

what do atoms react to form

A

A full outer shell

123
Q

How do you atoms react to form a full outer shell

A

Via losing gaining or sharing electrons

124
Q

Explain metals on the left of the periodic table

A

they don’t have many electrons to remove

125
Q

explain metals towards the bottom of the periodic table

A

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
Q

What are metals

A

Elements which can form positive ions when they react

127
Q

where are metals on the periodic table

A

towards the bottom and to the left of the periodic table

128
Q

Where are non-metals on the periodic table

A

at the far right and top of the periodic table

129
Q

What don’t nonmetals generally form when they react

A

Positive ions

130
Q

Describe Dimitri Mendeleev’s table

A

He left gaps for predicted new elements

Order of atomic mass but switched order if properties meant it should be changed

131
Q

In the 1800s what did the periodic table look like

A

ordered by Atomic mass physical and chemical properties and their relative atomic mass

132
Q

Why is it hard for non-metals to form positive ions

A

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
Q

Explain the modern periodic table

A

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
Q

What do you elements with similar properties forms

A

columns

135
Q

What a vertical columns called

A

Groups

136
Q

What does the group number describe

A

how many electrons are in the outer shell

137
Q

explain group 1 trends

A

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
Q

What are group on metals also called

A

Alkali metals

139
Q

Explain the alkali metals

A

Don’t need much energy to lose their one outer electron to form a full outer shell

140
Q

what’s more reactive transition metals or alkali metals

A

Alkali metals

141
Q

Give some properties of alkali metals

A

Leston stronger and harder than transition metals have lower points than transition metals

142
Q

explain the reactivity of the halogens

A

reactivity decreases as you go down the group

143
Q

what are rows called

A

periods

144
Q

What does each period

Present

A

Another full shell of electrons

145
Q

Are halogens metals or nonmetals

A

Nonmetals

146
Q

As you go down the group the halogens are

A

Less reactive higher melting and boiling points higher relative atomic mass

147
Q

what type of bonding can halogens uses

A

Covalent bonding and ionic bonding

148
Q

1-ions=?

A

halides

149
Q

What’s distillation used to do

A

separate mixtures which contain liquids

150
Q

explain simple distillation

A

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
Q

how do you draw a covalent drawing

A

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
Q

How do you know if a covalent bond is single or double

A

You look at how many bonds it shared from each shell

153
Q

what structure do ionic compounds have

A

A regular lattice structure a structure called a giant ionic lattice

154
Q

Explain ionic compound structure

A

irons form closely packed regular lattice arrangement and they’re very strong electrostatic forces of attraction between oppositely charged ions in all directions

155
Q

What ionic compounds boiling and melting points like and why

A

High because the strong bonds between the ions

156
Q

explain a solid ionic compound

A

Ions are in place compounds can’t conduct electricity

157
Q

explain ionic compound when it melts

A

ions are free to move and carry electric current

158
Q

Why do ionic compounds dissolve easily

A

because Ions separate all free to move in solution

159
Q

when are ions made

A

when electrons are transferred

160
Q

ions are…

A

charged particles which can be single or in groups

161
Q

if two electrons are lost the charge is…

A

2+

162
Q

three electrons are gained the charge is…

A

3-

163
Q

which groups most readily form ions

A

One and two are metals and lose electrons to form positive irons

164
Q

which other groups most readily form Iions

A

67 a non-metal also gain electrons to form negative ions

165
Q

explain the groups with charges

A

Group 1= 1+
2=2+
6=2-
7=1-

166
Q

what is covalent bonding between

A

nonmetals and nonmetals

167
Q

what happens when elementa bond together in covalent bonding

A

they share pairs of electrons to make covalent bond

168
Q

What makes covalent bonds strong

A

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
Q

what does each single covalent bond provide

A

One extra shared electron for each atom

170
Q

What does having a full outer shell mean for a noble gas

A

the electronic structure of a noble gases very stable

171
Q

what is simple molecular substances made up of

A

molecules containing a few atoms joined together by covalent bonds

172
Q

give the properties of simple molecular substances

A

very strong covalent bonds in the atoms which means by contrast the attraction between his molecules very weak

173
Q

are the melting and boiling points high or low

A

low because the molecules are easily parted from each other

174
Q

what a simple molecular substances like at room temperature

A

gases or liquids

175
Q

The bigger the molecules the strength of the intermolecular forces…

A

increases so r more energy is needed to break them

176
Q

Why don’t simple molecular substances conduct electricity

A

because they aren’t charged so there are no free electrons or irons

177
Q

what are polymers

A

Long chains of repeating units

178
Q

what all the atoms in a polymer joined by

A

strong covalent bonds

179
Q

What type of covalent bonds to giant structures have

A

strong

180
Q

Descry the boiling and melting points of giant covalent structure is

A

very high melting and boiling points as lots of energy is needed to break the covalent bonds between the atoms

181
Q

what don’t giant covalent structures do

A

have charged particles or conduct electricity

182
Q

give two examples of giant covalent structures

A

Diamond graphite

183
Q

Describe the giant covalent bond in diamond

A

each carbon atom forms for covalent bonds in a rigid giant covalent structure

184
Q

describe the giant covalent bond in graphite

A

each carbon atom forms three covalent bonds to create layers of the hexagons

each carbon atom also has one delocalised electrons

185
Q

What are nonmetals and metals attracted by in ionic bonding

A

electrostatic forces

186
Q

what is the metals symbol in a dot and cross diagram

A

.

187
Q

what’s the symbol for a non-metal in a dot and cross atom

A

cross

188
Q

describe metallic bonding

A

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
Q

Describe the changes in state

A

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

CHEMISTRY -EVIE💘 (9 decks)

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