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Eleanor Rowe Chemistry GCSE > Atomic Structure and the Periodic Table > Flashcards

Atomic Structure and the Periodic Table Flashcards

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1
Q

Facts about the nucleus:

A

In the middle of an atom.
Contains protons and neutrons.
Positive charge because of the protons.
Almost whole mass of atom is found in the nucleus.

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2
Q

Facts about electrons:

A

Move around the nucleus in electron shells.
Negatively charged.
Have virtually no mass.

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3
Q

What charge are atoms and why?

A

Neutral, they have the same number of protons as electrons.

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4
Q

What does the atomic number tell you?

A

How many protons there are.

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5
Q

What does the mass number tell you?

A

How many protons and neutrons there are.

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6
Q

How do you get the number of neutrons?

A

Subtract the atomic number from the mass number.

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7
Q

What is an element?

A

A substance made up of atoms that all have the same number of protons in their nucleus. e/g Nitrogen will have a different number of protons in its nucleus compared to Oxygen.

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8
Q

How many different types of elements are there?

A

100

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9
Q

What is an isotope?

A

A different form of the same element, which have the same number of protons but a different number of neutrons.

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10
Q

What is the relative atomic mass?

A

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

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11
Q

What is a compound?

A

When two or more elements are combined together and are held by chemical bonds.

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12
Q

How are two elements bonded together?

A

Usually involves atoms giving away, taking or sharing electrons. The nucleus of an atom is never affected.

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13
Q

What is an ion?

A
  • Ions are positively or negatively charged particles formed when atoms loose or gain electrons.
  • They have the same stable electronic structures as noble gasses.
  • The metal atoms lose electrons to form positive ions and the non-metal atoms gain electrons to form negative ions.
  • The opposite charges are attracted to each other.
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14
Q

What is covalent bonding?

A
  • A compound formed from non-metals consists of molecules.
  • Each atom shares an electron with another atom.
    e/g Hydrogen Chloride
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15
Q

What is a mixture?

A

When two or more elements or compounds are mixed together.

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16
Q

How can a mixture be separated?

A
  • Filtration
  • Crystallisation
  • Simple Distillation
  • Fractional Distillation
  • Chromatography
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17
Q

Are the chemical properties of a substance affected by it being part of a mixture?

A

No

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18
Q

How do you do Paper Chromatography?

A
  1. Draw a line near the bottom of the sheet of filter paper in pencil.
  2. Add a spot of ink to the line and placed the sheet in a beaker of solvent, e.g water.
  3. Make sure the ink isn’t touching the solvent.
  4. Place a lid on top of the container to stop the solvent evaporating.
  5. The solvent seeps up the paper, carrying the ink with it.
  6. Each different dye in the ink will move up the paper at a different rate so the dyes will separate out. Each day I will form a spot in a different place.
  7. The end result is a pattern of spots called a chromatogram.
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19
Q

How does Filtration work?

A

Filtration can be used if your product is an insoluble solid that needs to be separated from a mixture. It is done by using filter paper over a beaker to separate the solid from the liquid.

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20
Q

How does evaporation work?

A
  1. Pour the solution into an evaporating dish.
  2. Slowly heat the solution. The solvent will evaporate and the solution will get more concentrated. Crystals will start to form.
  3. Keep hearing the evaporating dish until all you have left if crystals.
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21
Q

How does crystallisation work?

A
  1. Pour the solution into an evaporating dish and heat it. Some of the solvent will evaporate and the solution will be more concentrated.
  2. When you see crystals start to form, remove from heat and leave to cool.
  3. The salt should start to form crystals as it becomes insoluble.
  4. Filter the crystals out of the solution and leave them in warmth to dry.
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22
Q

How does simple Distillation work?

A
  1. Used for separating out a liquid from a solution.
  2. The solution is heated. The part of the solution that has the lowest boiling point evaporated first.
  3. The vapour is then cooled, condensed (in a condenser) and is collected (in a beaker).
  4. The rest of the solution is left behind in the flask.
  • The problem with this is that you can only use it to separate things with different boiling points, otherwise they will mix again.
23
Q

How does fractional distillation work?

A
  1. Put your mixture in a flask and put a fractionating column on top. Heat it up.
  2. They will evaporate at different temperatures due to their various boiling points.
  3. The liquid with the lowest boiling point evaporates first, it will rise up the fractioning column filled with glass rods to the top.
  4. Liquids with higher boiling points may start to evaporate, however the column is cooler at the top so they will only get part way up before condensing and going back down the flask.
  5. The liquid will go from the top of the fractionating column to the condenser where is it condensed and then the different fractions are collected.
24
Q

Brief timeline of the atom:

A 
John Dalton
J J Thompson
Rutherford
Bohr
Chadwick
25
Q

What did John Dalton do?

A

Atoms are solid spheres

26
Q

What did J J Thompson do?

A

Plum pudding model

Atoms contain electrons

27
Q

What did Rutherford do?

A

Gold foil experiment

Positive nucleus
Electrons surround nucleus
Empty space

28
Q

What did Bohr do?

A

Electrons are in shells

Electrons orbit the nucleus

29
Q

Electron Shell rules:

A

The first shell can only ever have 2 electrons
After that they can have 8
An atom is stable when it has a full outer shell of electrons
If the outer shell isn’t full it will want to react with another atom to fill it

30
Q

Who created the periodic table?

A

Mendeleev

31
Q

How did Mendeleev create the periodic table?

A

He put the elements in order of atomic mass.

He left gaps for places where he thought elements that haven’t been discovered yet should go

32
Q

How is the periodic table laid out?

A

In order of increasing atomic (proton) number.
Metals on the left
Non metals on the right
Elements with similar properties in columns

33
Q

What are the vertical columns of the periodic table called?

A

Groups

34
Q

What does the group number of an element tell you?

A

How many electrons are in the outer shell

Group 0 is an exception to this

35
Q

What is a row called in the periodic table

A

Periods

36
Q

What does the period of an element tell you

A

Another full shell of electrons

37
Q

Do metals form positive or negative ions?

A

Positive

38
Q

Why is not much energy needed to react a metal at the bottom of the periodic table?

A

It has more shells of electrons which are further away from the nucleus

39
Q

Why is it hard to form ions with non metals?

A

They are at the right of the periodic table so have lots of electrons to remove to get a full outer shell of electrons

Or

The outer shell is closer to the nucleus so it requires more energy to react and form an ion

40
Q

What are the physical properties of metals?

A

Strong
Conduct heat and electricity
High boiling and melting points

41
Q

Properties of non metals

A 
Dull looking 
Brittle
Aren’t always solids
Don’t conduct electricity 
Lower density
42
Q

Properties of transition metals

A

Found in the centre of the periodic table
Normal metal properties; strong, conductors, shiny, dense…
Can have more than one ion

43
Q

Alkali metals (group 1) properties

A 
Soft
Low density
One electron on outer shell
Very reactive 
Similar properties 
Don’t require much energy to loose outer electron to form full outer shell 
Form 1+ ions
44
Q

Trends for alkali/group 1 metals as you go down the group:

A

Increasing reactivity
Lower melting and boiling points
Higher relative atomic mass

45
Q

When a group 1/alkali metal is reacted with water, what happens?

A

React vigorously

Produce hydrogen gas and metal hydroxides

46
Q

When group 1/alkali metals react with chlorine, what happens?

A

React vigorously

Form white chloride salt

47
Q

When group 1/alkali metals are reacted with oxygen, what happens?

A

Tarnish in air

Form the oxide of what element it was

48
Q

How are group 1 metals different to transition metals?

A

More reactive
Less dense, strong and hard
Lower melting points.

49
Q

Trends of halogens/group 7 going down the group

A

Less reactive
Higher melting and boiling points
Higher relative atomic masses

50
Q

What happens with a halogen/group 7 element forms an ion

A

It has a 1- charge

51
Q

What is a displacement reaction?

A

When a more reactive halogen displaces a less reactive one.

E/g Brad,angelina + Jen -> brad,jen +angelina

52
Q

Group 0 elements properties:

A

Full outer shells
Colourless gasses
Non flammable

53
Q

Trends in noble gasses going down

A

Boiling points increase

Eleanor Rowe Chemistry GCSE (9 decks)

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