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SCIENCE-CHEMISTRY GCSE > Chapter 1 - Atomic Structure And The Periodic Table > Flashcards

Chapter 1 - Atomic Structure And The Periodic Table Flashcards

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1
Q

How big is an atom?

A

0.1 nanometres

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2
Q

Describe the nucleus of an atom?

A

It is in the middle of the atom
It contains protons and neutrons
It has a positive charge because of the protons
Almost the whole mass of the atom is concentrated in the nucleus

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3
Q

Describe the electrons of an atom?

A

They move around the nucleus in electron shells
They are negatively charged and very small but they cover a lot of space
The volume of their orbits determine the size of the atom
They have no mass

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4
Q

What is the charge of an electron proton and neutron?

A 
Electron= -1
Proton= +1
Neutron= 0
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5
Q

Why are atoms neutral (no charge)?

A

They have the same number of protons and electrons. The charge of the electrons and protons are the same so they cancel out.

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6
Q

What does the nuclear symbol tell you about an atom?

A

It tells you the atomic (proton) number and the mass number

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7
Q

Where is the atomic number found and what does it tell you about the atom?

A

It is found on the bottom left and tells you the number of protons in an atom.

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8
Q

What does the mass number tell you and where is it found?

A

The mass number tells you the number of protons and neutrons there are in an atom.
It is found in the top left

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9
Q

How do you work out the number of neutrons there are in an atom?

A

You subtract the atomic number by the mass number.

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10
Q

What is an element?

A

An element is a substance made up of atoms that all have the same number of protons in their nucleus. They consist of atoms with the same atomic number.

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11
Q

What are isotopes?

A

Isotopes are different forms of the same element which have the same number of protons but a different number of electrons.

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12
Q

What is relative atomic mass?

A

Relative atomic mass is used instead if mass number when referring to the element as a whole. It is an average mass taking into account the different masses and abundance of all the isotopes that make up the element.

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13
Q

Copper has two stable isotopes. Cu-63 has an abundance of 69.2% a d Cu-65 has an abundance of 30.8%. Calculate the relative atomic mass of copper to 1d.p.

A

(69.2x63)+(30.8x65) / 69.2 + 30.8 = 6361.6 / 100 = 63.616 = 63.6

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14
Q

What is a compound?

A

A compound is when other atoms react together and combine to form a compound

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15
Q

What does making bonds involve?

A

It involves giving atoms away, taking or sharing electrons. Only the electrons are involved as they are in the outer shell of the atom.

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16
Q

What is a compound formed from non metals called?

A

Covalent bonding

Each atom shares an electron with another atom

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17
Q

What are the molecules on the left hand side of an equation called?

A

The reactants

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18
Q

What are the molecules on the right hand side of an equation called?

A

The products

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19
Q

Why must all symbol equations be balanced?

A

Because atoms cannot just disappear

You balance the equation by putting numbers in front of the formulas where needed

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20
Q

How do you balance a symbol equation?

A

1) Find an Element that doesn’t balance and put a number in front to make it balance. This may cause another imbalance.
2) if another imbalance is caused, balance that and see where it takes you
3) carry on doing this until all is balanced

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21
Q

What is the difference between a compound and a mixture?

A

There are no chemical bonds between different parts of a mixture.

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22
Q

How can mixtures be separated?

A 
Filtration 
Crystallisation
Simple distillation
Fractional distillation 
Chromotography
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23
Q

How can chromatography be used?

A

To separate different dyes in an ink

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24
Q

How is chromatography done?

A

1) draw a line near the bottom of the sheet of filter paper in pencil as pencil is insoluble and wont dissolve
2) Add a spot of ink to the line and place the sheet in a beaker making sure the water is a couple of centimetres under the line.
3) place a lid on top of the beaker to stop the solvent evaporating.
4) when the solvent has nearly reached the top of the paper, take the paper out and leave it to dry.
5) the end results are called a chromatogram

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25
Q

What is filtration used for?

A

To separate insoluble solids from liquids

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26
Q

What are the two ways to separate soluble solids from solutions?

A

Evaporation

Crystallisation

27
Q

How do you set up an evaporation experiment?

A

1) pour the solution into an evaporation dish

2) slowly heat the solution. The solution will start to evaporate and you should be left with dry crystals

28
Q

What is simple distillation used for?

A

Separating out a liquid from a solution

Eg, pure water from sea water

29
Q

What is fractional distillation used for?

A

To separate out a mixture of liquids

30
Q

How do you do simple distillation?

A

The solution is heated. The part that has the lowest boiling point evaporates first.

The vapour is then cooled, condenses and collected

The rest of the solution is left behind in the flask

31
Q

How do you do fractional distillation?

A

You put your mixture in a flask and stick a fractional column on top. Then you heat it

The different liquids will have different boiling points they will evaporate at different temperatures

The liquid with the lowest boiling point evaporates first .When the temperature on the thermometer matches the boiling point of this liquid it will reach the top of the column.

Liquids with higher boiling points might also start to evaporate . But the column is cooler towards the top so they only get part of the way up before condensing and running back down the floors

when the first liquid has been collected you raise the temperature until the next one reaches the top

32
Q

What did john dalton describe atoms to be in the early 1800s?

A

He described them as solid spheres and that different spheres made up different elements

33
Q

What did JJ Thompson conclude from his experiments?

A

He concluded that atoms weren’t solid spheres.
His measurements of charge and mass showed that an atom must contain even smaller negatively charged particles-electrons. The solid-state idea of atomic structure have to be changed to new theory was known as the plum pudding model

34
Q

What does the plum pudding model show?

A

It shows a positively charged ball or “pudding” with electrons stuck in it

35
Q

What did Ernest Rutherford and Ernest Marsden discover in 1909?

A

They fired positively charged alpha particles at an extremely thin sheet of gold. From the plum pudding model they were expecting the particles passed straight through the sheet will be slightly deflected at most. This was because the positive charge of each atom was thought to be very spread out through the pudding model. But whilst most of the particles did go straight through the gold sheet some were deflected more than expected, and a small number were deflected backwards so the plum pudding model couldn’t be right.

36
Q

What did Ernest Rutherford come up with in 1909 to explain his evidence?

A

Rutherford came up with the nuclear model of the atom. In this there is a tiny, positively charged nucleus at the centre, where most of the mass is concentrated.
A ‘cloud’ of negative electrons surround this nucleus so 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 file directly at the nucleus they were deflected backwards otherwise they passed through the empty space

37
Q

What did Bohr come up with?

A

Bohr proposed that electrons orbit the nucleus in fixed shells aren’t anywhere in between. Each shell is a fixed distance from the nucleus.

His theory of atomic structure was supported by many experiments and it helped to explain many other scientists observations at the time.

It was called the nuclear model

38
Q

What did further experiments by Rutherford and others show?

A

They showed that the nucleus can be divided into smaller particles which have the same charge as a hydrogen nucleus these particles were named protons

39
Q

What did james Chadwick discover 20 years after the discovery that electrons moved in fixed shells?

A

James Chadwick carried out an experiment which provided evidence for neutral particles in the nucleus which are now called neutrons

40
Q

What are the electron shell rules?

A
  • Electrons always occupy shells
  • The lowest shell (ones closest to the nucleus) is filled first
  • Atoms are much happier when they have full electron shells
  • In most atoms the outer shell is not full and this makes the atom want to react to fill it.
41
Q

What were elements arranged by in the 1800s?

A

Atomic Mass

42
Q

What happened in 1869 in regards to the periodic table?

A

Dmitri Mendeleev took 50 known elements and arranged them into his table of elements, leaving gaps as he predicted new elements.
He put the elements mainly in order of atomic mass.

43
Q

How are elements in the periodic table laid out?

A

They are laid out in increasing atomic (proton) number

44
Q

Where are metals and non-metals found in the periodic table?

A

Metals are found on left and non metals are found on the right

45
Q

What does the group number of an element tell you?

A

It tells you how many electrons there are in the outer shell.

46
Q

What do rows in the periodic table represent? What are they called?

A

They are called periods

They represent another full shell of electrons

47
Q

How does electronic structure affect how atoms will react?

A

Atoms generally react to form a full outer shell

Metals to the left of the periodic table don’t have many electrons to remove and metals towards the bottom of the periodic table have outer electrons which are a long way from the nucleus meaning that they have a weaker attraction. This means that that not much energy is needed to remove the electrons so its feasible for the elements to react to form positive ions with a full outer shell.

Non metals tend to either have lots of electrons to remove to get a full outer shell or where the outer electrons are close to the nucleus so they feel a strong attraction. It is a lot easier for them to either share or gain electrons to get a full outer shell.

48
Q

What are group 1 elements known as?

A

Alkali metals

They are pretty reactive

49
Q

What are the features for group 1 metals?

A
  • soft
  • low density
  • one electron in the outer shell which makes them very reactive
50
Q

What are the trends for the alkali metals as you go down group 1?

A

Increasing reactivity - the outer electron is more easily lost as the attraction between the nucleus and electron decreases because the electron is further away from the nucleus the further down you go

Lower melting and boiling points
Higher relative atomic mass

51
Q

What type of compound do alkali metals form?

A

They form ionic compounds with non metals

They do not need a lot of energy to lose their one outer electron to form a full outer shell

They form 1+ ions

52
Q

What happens when group 1 metals are put in water?

A

They react very vigorously
The lower down the group the alkali metal is, the more violent the reaction
Lithium sodium ams potassium float and move around the surface, fizzing furiously. They produce hydrogen

53
Q

What happens when group 1 metals are heated in chlorine gas?

A

They react vigorously when heated in chlorine gas to form white salts called metal chlorides.

54
Q

What happens when group 1 metals react with oxygen?

A

They form a metal oxide
Lithium reacts to form lithium oxide
Sodium reacts to form a mixture of sodium oxide and sodium peroxide
Potassium reacts to form a mixture of potassium peroxide and potassium superoxide

55
Q

What are group 7 elements known as?

A

Halogens

56
Q

What are the group 7 trends as you go down the group?

A

They become less reactive - harder to gain an extra electron because the outer shell is further from the nucleus

They have higher melting and boiling points

Higher relative atomic mass

57
Q

What type of compound forms when halogens react with non metals?

A

Simple molecular structures

They form via covalent bonding

58
Q

What type of bonds do halogens form with metals?

A

Ionic bonds

The halogens form 1- ions called halides

59
Q

What are group 0 elements known as?

A

Noble gases

They are all colourless gases

60
Q

How many electrons do they have in their outer shell?

A

They all have a full outer shell with 8 electrons apart from helium which has 2.

61
Q

What does it mean if group 0 elements have a full outer shell?

A

This means that they are more or less inert which means they dong react much at all.

62
Q

What colour are noble gases at room temperature?

A

They are colourless

63
Q

What are the patterns and properties of noble gases?

A

They are non flammable
The boiling points increase as you move down the group along with increasing relative atomic mass
The increase in boiling point is due to an increase in the number of electrons in each atom leading to greater intermolecular forces between them which need to be overcome.

64
Q

What is a compound formed from a metal and non metal called?

A

Ionic bonding
The metal loses the electron to for, positive ions and the non metal atoms gain electrons to form a negative ion.
The opposite charges of ions means they are strongly attached to each other.

SCIENCE-CHEMISTRY GCSE (6 decks)

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