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Chemistry > Topic 1-Atomic Structure And The Periodic Table > Flashcards

Topic 1-Atomic Structure And The Periodic Table Flashcards

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1
Q

What is an isotope?

A

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

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2
Q

What is relative atomic mass?

A

An average mass taking into account the different masses and amounts of all the isotopes that make up the element.

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3
Q

What is a compound?

A

Substances formed from two or more elements.

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4
Q

How are compounds held together?

A

They are held together by chemical bonds.

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5
Q

How are bonds made?

A

Giving away, taking or sharing electrons.

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6
Q

What does a compound made of metals and non metals consist of?

A

Ions.

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7
Q

What happens to the metal in the compound?

A

It loses electrons to form positive ions.

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8
Q

What happens to non metals in a compounds?

A

They gain electrons to form negative ions.

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9
Q

What is ionic bonding?

A

The opposite charges of the ions mean they are strongly attracted to each other.

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10
Q

What is covalent bonding?

A

Where each atom shares an electron with another atom.

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11
Q

What is a mixture?

A

Two or more elements or compounds mixed together.

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12
Q

What is different between a mixture and a compound?

A

There is no chemical bond between the different parts of a mixture.

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13
Q

Describe how you separate substances using chromotography?

A

Draw a lime near the bottom of a sheet of filter paper using pencil.
Add a spot of ink to the line and place the sheet in a beaker of solvent.
The solvent depends on what is being tested as some compounds dissolve well in water however sometimes ethanol is needed.
Make sure the ink isnt touching the solvent.
The solvent seeps up the paper carrying the ink with it.
Each different dye will move up the paper at a different rate so the dyes will separate out. Each dye will form a spot in a different place.
If any of the dyes are insoluable in the solvent you used it will stay on the baseline.
When the solvent has reached near the top and take the paper out the beaker and leave it to dry.
The end drued result is a chromatogram.

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14
Q

Whag does filtration do?

A

Separates insoluable solids from a liquid. Also used in purification to get rid of solid impurities in a reaction mixture.

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15
Q

What is used in filtration?

A

Filter paper is folded into the cone shape and the solid is left in the filter paper.

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16
Q

Describe the process of evaporation?

A

Pour the solution into an evaporating dish.
Slowly heat the solution and the solvent will evaporate and the solution will get more concentrated. Crystals will start to form.
Keep heating the dish until you have dry crystals.

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17
Q

What can you only ise evaporation for?

A

Only if the salt doesnt break down when it is being heated.

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18
Q

Desribe the process of crystallisation?

A

Pour the solution into an evaporating dish and gently heat the solution. Some of the solvent will evaporate and the solution will get more concentrated.
When you see the crystals start to form remove the dish from the heat and leave the solution to cool.
The salt should start to form crystals as it becomes insoluable in the cold, highly concentrated solution.
Filter the crystals out the solution and leave them in a warm place to dry.

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19
Q

Desribe the crystallisation and filtration practical to separate rock salt?

A

Grind the mixture to make sure the salt crystals are small so they will dissolve easily.
Put the mixture in the water and stir. The salt will dissolve but the sand wont.
Filter the solution. The grains of sand wont fit through the holes of the filter paper so they collect on the paper instead. The salt passes through the filter paper as it is part of the solution.
Evaporate the water from the salt so it forms dry crystals.

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20
Q

What is rock salt?

A

A mixture of salt and sand.

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21
Q

Why does salt and sands physical properties allow them to be separated?

A

They are both compounds but salt dissolves in water and sand doesnt.

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22
Q

Describe simple distillation?

A

Simple distillation is used to separate a liquid from a solution.
The solution is heated. The part of the solution that has the lowest boiling point evaporates first.
The vapour is then cooled, condensed and is then collected.
The rest of the solution is left in the flask.

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23
Q

What mixture can you use distillation to separate?

A

You can use it to get pure water from seawater.

The water evaporates and condenses and eventually you will be left with just left with salt in the flask.

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24
Q

What is the problem with simple distillation?

A

It can only separate things with very different boiling points.
If the temperature goes higher than the boiling point of the substance and goes to the higher boiling point the mixtures will mix again.

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25
Q

How do you carry out fractional distillation?

A

You put your mixture in a flask and put a fractioning column on top then you heat it.
The different liquids have different boiling points so they will evaporate at different temperatures.
The liquid with the lowest boiling point evaporates first. When the teperature on the thermometer matches the boiling point it will reach the top of the column.
Liquids with higher boiling points might start to evaporate but the column is cooler towards the top so it will only get part way up before condensing and running back down to the flask.
When the first liquid has been collected you raise the temperature until the next one reaches the top.

26
Q

What did John Dalton say about the atom?

A

He described the atom as solid spheres and the different spheres made up the different elements.

27
Q

What did JJ Thompson say about the atom?

A

He concluded from his experiments that atoms werent solid spheres. His measurements of charge and mass showed an atom must contain even smaller negatively charged particles (electrons).

28
Q

Describe the Rutherfords model of the atom?

A

Ernest Rutherford conducted the alpha particle scattering experiments. They fired positively charged alpha particles through a thin sheet of gold.
They were expecting the alpha particles to pass straight through as they thought the positive charge was spread out through the atom. Some were deflected more than normal and a small number was deflected backwards so the plum pudding couldnt be right.
He came up with a nuclear model of the atom. There was a positively charged nucleus in the centre where most mass is concentrated.
Most of the atom is empty space with elcetrons surrounding the nucleus.

29
Q

What was Bohr’s model of the atom?

A

It suggested that electrons were contained in shells.
Electrons orbit the nucleus in fixed shells and arent anywhere inbetween. Each shell is a fixed distance from the nucleus.
It was supported by many experiments and helped explain lots of scientists observations at the time.

30
Q

What was wrong with Rutherfords model of the atom?

A

The cloud of electrons he desribed would be attracted to the nucleus causing them to collapse.

31
Q

What experiment proved the existance of protons?

A

Rutherford and others experimented that the nucleus could be divided up into smaller particles which had the same charge as a hydrogen nucleus.
James Chadwick carried out an experimetn which provided evidence for neutral particles in the nucleus.

32
Q

How did elements used to be catergorised?

A

Their physical and chemical properties.

Relative atomic mass.

33
Q

How did Mendeleev arrange the periodic table?

A

He put them mainly in the order of atomic mass but then changed them if the properties of that element were similar to another groups.
He left gaps in the table to make sure elements with similar properties stayed in the same groups. It also indicated undiscovered elements and allowed mendeleev to predict what the properties might be.

34
Q

What discovery proved mendeleevs order of the periodic table to be correct?

A

The discovery of isotopes confirmed medeleev was correct not to place elements in a strict order of atomic mass but take into account their properties. Isotopes have different masses but the same chemical properties.

35
Q

What is the modern periodic table arranged like?

A

It is in increasing atomic number.

Metals are to the left and non metals are to the right.

36
Q

What are the properties of metals?

A

They are strong and malleable.
They are good conductors of heat and electricity.
They have high boiling points and melting points.

37
Q

What are the properties of non metals?

A 
Dull
Brittle
Low density
Dont conduct electricity well
Arent always solids at room temperature.
38
Q

What is group one of the periodic table?

A

Alkali metals.

39
Q

What are the properties of the alkali metals?

A

Soft
Low density
One electron in their outer shell.

40
Q

What is the trend as you go down geoup 1?

A

Increasing reactivity as the outer electron is more easily lost as the attraction between the electron and the nucleus decreases.
Lower melting and boiling points.
Higher relative atomic mass.

41
Q

What happens to alkali metals when they form into ionic compounds?

A

White solids that dissolve in water to form colourless solutions.

42
Q

What do alkali metals produce when they react with water?

A

They react vigorously to produce hydrogen gas and metal hydroxides (salts that dissolve in water to produce alkaline solutions).

43
Q

What happens to the reaction with water as you go down the group of alkali metals?

A

The more reactive the more violent the reaction.

The energy given out increases as you go down the group.

44
Q

What do alkali metals produce when they react with chlorine?

A

They form white metal chlorides.

45
Q

What happens to the reacrion with water as you go down the group of alkali metals?

A

The reactivity increases so the reaction with chlorine gets more vigorous.

46
Q

What happens to the alkali metals when they react with oxygen?

A

It forms a metal oxide.

47
Q

What does lithium form when it reacts with oxygen?

A

Lithium oxide.

48
Q

What does sodium form when it reacts with oxygen?

A

A mixture or Sodium oxide and sodium peroxide.

49
Q

What does lithium form when it reacts with oxygen?

A

A mixture of potassium peroxide and potassium superoxide.

50
Q

What is group 7 known as?

A

The halogens.

51
Q

What is flourine?

A

It is a reactive, poisonous yellow gas.

52
Q

What is chlorine?

A

A fairly reactive, poisonous dense green gas.

53
Q

What is bromine?

A

A dense, poisonous, red brown volatile liquid.

54
Q

What is iodine?

A

A dark grey crystalline solid or a purple vapour.

55
Q

What are all group 7 molecules like?

A

They are in pairs of atoms.

56
Q

What happens as you go down group 7?

A

They become less reactive as its harder to gain an extra electron because the outer shell is further from the nucleus.
They have higher melting and boiling points.
They have higher relative atomic mass.

57
Q

How csn halogens gain a full outer shell?

A

They share electrons via covalent bonding with other non metals to gain a full outer shell.

58
Q

What happens to halogens when it bonds with metals?

A

It forms negatively charged ions called halides when they bond with metals.

59
Q

What are group 0 elements called?

A

Noble gases.

60
Q

Why are the noble gases unreactive?

A

They have a full outer shell so they dont need to give up or gain electrons to become more stable.

61
Q

What are some properties of noble gases?

A

Unreactive.
Colourless gases at room temperature.
Monatomic gases.
They are non flammable.

62
Q

What happens to the boiling points as you move down group 0?

A

The boiling points increase as there is an increase in the number of electrons leading to greater intermolecular forces that need to be overcome.

Chemistry (10 decks)

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