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Chemistry Easter Test > Easter Test > Flashcards

Easter Test Flashcards

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1
Q

Saturated

A

A hydrocarbon with only single bonds between its atoms. This means that it contains as many hydrogen atoms as possible in each molecule eg an alkane

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2
Q

Unsaturated

A

A hydrocarbon whose molecules contain at least one carbon-atom double bond eg. An alkene

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3
Q

Alkane

A

Saturated hydrocarbon with the formula of CnH2n+2

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4
Q

Alkene

A

An unsaturated hydrocarbon which contains a carbon-carbon double bond. It generally formula is CnH2n

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5
Q

Hydrocarbon

A

A compound containing only hydrogen and carbon

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6
Q

Molecular formula

A

The total number of atoms of each element in a molecule

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7
Q

Structural formula

A

Shows the arrangement of atoms in a molecule

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8
Q

Displayed formula

A

Shows how the atoms and bonds in a molecule are arranged

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9
Q

Homologous series

A

A group of chemicals (eg alkanes) which have similar chemical properties and can be represented as general formula

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10
Q

Explain the process of fractional distillation

A

The crude oil is heated until vaporised, these vapours move up the fractioning column the further up the column the cooler it becomes. As the gasses move up the fractioning column they cool down, as each fraction condenses at a different temperature they are collected at different points, each fraction contains hydrocarbons with a similar number of carbon atoms. The refinery gasses have very low boiling points and do not condense and pass out the top of the fractioning column, longer chained hydrocarbons such as bitumen have higher boiling points and collected towards the bottom of the column whereas shorter chained hydrocarbons like petrol are collected near the top.

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11
Q

Wh do long chained hydrocarbons have high boiling points

A

The intermolecular forces between large molecules are stronger than the intermolecular forces between small molecules. More energy is needed to break the forces between the large molecules, and so the boiling point is higher.

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12
Q

First four Alkenes

A

Methane,ethane,propane,butane

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13
Q

What are the 2 conditions for cracking

A

High temperature, a catalyst

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14
Q

Describe the process for cracking

A

The paraffin is heated until vapourised/ evaporated, the broken porcelain or aluminium oxide acts as a catalyst. The paraffin is cracked into smaller chained hydrocarbons and an alkane and an alkene are produced

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15
Q

What is the test for alkane/ alkenes

A

Bromine water
Alkane + bromine water=no reaction & solution stays orange
Alkene + bromine water=reaction & solution turns colourless

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16
Q

Equation for complete combustion

A

Hydrocarbons + oxygen —> carbon dioxide+ water

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17
Q

Equation for incomplete combustion

A

Hydrocarbon + oxygen —> carbon monoxide + carbon + water

18
Q

Equation for incomplete combustion when there is not enough oxygen to produce monoxide

A

Hydrocarbon + oxygen —> carbon + water

19
Q

What is mass number

A

The mass number of an atom is its total number of protons and neutrons and is always the bigger number

20
Q

How do u find out how many neutrons there are

A

Number of neutrons = mass number- atomic number

21
Q

What is atomic number

A

Number of protons / electrons ( smaller number )

22
Q

What does the aq state symbol mean

A

aqueous (dissolved in water)

23
Q

Where is proton found and what is its relative charge and mass

A

Found in the nucleus
Relative mass = 1
Relative charge = +1

24
Q

where is neutron found and what is its relative charge and mass

A

Found in nucleus
Relative mass = 1
Relative charge = 0

25
Q

Where is electron found and what is its relative mass and charge

A

Found in shells
Relative mass = 0
Relative charge = -1

26
Q

What are ions

A

Electrically charged particles formed when atoms lose or gain electrons

27
Q

What happens to non metals in chemical reactions

A

Gain electrons and become negative

28
Q

What happens to metals during chemical reactions

A

Lose electrons and become positive

29
Q

What is an ionic bond

A

The metal atoms become positive ions and the non-metal atoms become negative ions. There is a strong electrostatic force of attraction between these oppositely charged ions – this is called an ionic bond, it is between a metal and non metal.

30
Q

What is covalent bonding

A

When 2 or more atoms bond by sharing electrons normally occurring between non metal atoms.the atoms in the molecule are held together strongly but there are weak forces between individual molecules, so have low melting and boiling points and are usually liquids or gasses

31
Q

What is metallic bonding

A

Metallic bonding is the electrostatic attraction between positive metal ions and delocalised electrons. The organisation of the metal ions and the free-moving electrons give metals certain properties, such as malleability and ability to conduct heat and electricity, between 2 metals.

32
Q

Why does metal conduct electricity

A

There are delocalised electrons which carry charge through the structure

33
Q

How are metals arranged

A

In a lattice pattern of positive metal ions in a sea of negative delocalised electrons

34
Q

Reactivity series

A

Please - potassium
Stop - sodium
Calling - calcium
Me - magnesium
A - aluminium
Careless - carbon
Zebra - zinc
Instead -iron
Try - tin
Learning - lead
How - hydrogen
Copper
Saved - silver
Gold

35
Q

General equation for reaction between metals and oxygen

A

Metal + oxygen —> metal oxide

36
Q

What is a displacement reaction

A

A more reactive element displaces (kick out) the less reactive element from the compound after the reaction the less reactive element is now left pure and uncombined
Eg. Cucl2 + mg = mgcl2 + cu

37
Q

What is oxidation

A

The addition of oxygen Or the removal of electrons.

38
Q

What is reduction

A

Removal of oxygen or the addition of electrons

39
Q

What is a metal ore

A

A rock that contains enough of a metal or metal compound to make it worth extracting the metal

40
Q

How do you extract metals

A

If a metal is less reactive than carbon, it can be extracted from its oxide by heating with carbon. The carbon displaces the metal from the compound, and removes the oxygen from the oxide. This leaves the metal.

However if the metal is more reactive we use electrolysis,electrolysis involves using electricity to break down electrolytes to form elements

Chemistry Easter Test (1 decks)

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