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GCSE - Chemistry > Topic 1 > Flashcards

Topic 1 Flashcards

1
Q

What do atoms contain?

A

Protons, Neutrons and electrons.

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2
Q

What is the radius of an atom?

A

0.1 nanometres

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3
Q

What does the nucleus of the atom contain?

A

Protons and neutrons

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4
Q

What is the charge of the nucleus and why?

A

It has a positive charge because of the protons

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5
Q

What is the relative mass and charge of a proton?

A

relative mass = 1
charge = +1

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6
Q

What is the relative mass and charge of a neutron?

A

Relative mass = 1
Charge = 0

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7
Q

What is the relative mass and charge of an electron?

A

Relative mass = very small or 0
Charge = -1

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8
Q

What does the number of protons equal in an atom?

A

The number of electrons

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9
Q

What is the overall charge of an atom and why?

A

No charge / neutral because they have the same number of protons and electrons

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10
Q

Do ions have an overall charge and why?

A

In an ion the number of protons doesn’t equal the number of electrons. This means it has an overall charge.

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11
Q

Where is the atomic number and what does it tell us?

A

Its the bottom number and it tells us the number of protons.

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12
Q

Where is the mass number and what does it tell us?

A

It’s the top number and it tells us the total number of protons and neutrons.

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13
Q

What is an element?

A

a substance made up of atoms that all have the same number of protons in their nucleus.

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14
Q

What are isotopes?

A

Isotopes are different forms of the same element, which have the same number of protons but different number of neutrons.
(Isotopes have the same atomic number but different mass numbers)

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15
Q

What is the formula to work out the relative atomic mass?

A

Relative atomic mass (Ar)=

Sum of(isotope abundance x isotope mass number)
__________________________________
Sum of abundance of all isotopes

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16
Q

What happens when elements react?

A

Atoms combine with other atoms to form compounds

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17
Q

How do compounds form?

A

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

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18
Q

What are compounds?

A

substances formed from two or more elements, held together by chemical bonds.

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19
Q

How do elements make bonds?

A

giving away, taking or sharing electrons (the nuclei of the atoms aren’t affected at all when a bond is made).

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20
Q

What is needed to separate the original elements of a compound out again?

A

A chemical reaction.

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21
Q

What is ionic bonding?

A

ionic bonding is when a compound which is formed from a metal and non-metal. The metal atoms lose electrons to form positive ions and the non-metal atoms gain electrons to form negative ions. The opposite charges of the ions mean that they’re strongly attracted to each other.

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22
Q

How are covalant bonds made?

A

When non-metals atoms bond together, they share pairs of electrons to make covalent bonds.

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23
Q

Are the properties of a compound the same as the properties of the original elements.

A

The properties of a compound are usually totally different from the properties of the original elements.
For example, if iron (a lustrous magnetic metal) and sulfur (a nice yellow powder) react the compound formed (iron sulfide) is a dull grey solid lump and doesn’t behave anything like either iron or sulfur.

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24
Q

What is the formula for carbon dioxide?

A

CO2

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25
What is the formula for Ammonia?
NH3
26
What is the formula for Water?
H O 2
27
What is the formula for Sodium Chloride?
NaCl
28
What is the formula for Carbon monoxide?
CO
29
What is the formula for Hydrochloric acid?
HCl
30
What is the formula for Calcium chloride?
CaCl2
31
What is the formula for Sodium carbonate?
Na2CO3
32
What is the formula for Sulfuric acid?
H SO 2 4
33
Can mixtures be separated?
Unlike compounds mixtures are easily separated.
34
What are some examples of separating techniques?
1)Filtration 2)Crystallisation 3)Simple distillation 4)Fractional distillation 5)Chromatography
35
What experiments did Ernest Rutherford and his student Ernest Marsden carry out?
Ernest Rutherford and his student Ernest Marsden carry out the alpha particle scattering experiments where they fired positively charged alpha particles at an extremely thin sheet of gold.
36
How did John Dalton describe the atom and when?
At the start of the 19th century John Dalton described atoms as solid spheres and said that different spheres made up the different elements,
37
What did the plum pudding model show the atom as?
It showed the atom as a ball of positive charge with electrons stuck in it.
38
What did J J Thompson conclude about the atom and when?
In 1897 J J Thompson concluded from his experiments that atoms where not solid spheres. His measures of charge and mass showed that an atom must contain even smaller, negatively charged particles - electrons. The new theory was known as the 'plum pudding model'.
39
What did Ernest Rutherford and his student Ernest Marsden expect to happen from there experiments and what actually happened?
In 1909 From the plum pudding model, they were expecting the particles to pass straight through the sheet or be slightly deflected at most. This was because the positive charge of each atom was thought to be very spread out. 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.
40
How did Rutherford explain his evidence from the alpha particle scatter experiment?
Rutherford explained his experiment with the nuclear model of the atom. In this, there's 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, positively charge of the nucleus, they were deflected. If they were fired directly at the nucleus, they were deflected backwards. Otherwise, they passed through the empty space.
41
What did Scientists realise about the electrons in 'clouds' as Rutherford described?
Scientists realised that the electrons would be attracted to the nucleus, causing the atom to collapse.
42
What did Niels Bohr propose?
Bohr proposed that electrons orbit the nucleus in fixed shells and aren't anywhere in between. Each shell is at a fixed distance from the nucleus.
43
What did further experiments carried out by Rutherford and others show?
That the nucleus can be divided into smaller particles, which each have the same charge as a hydrogen nucleus. These particles were named protons.
44
What did James Chadwick discover?
About 20 years after scientists had accepted that atoms have nuclei James Chadwick carried out an experiment which provided evidence for neutral particles in the nucleus which are called neutrons.
45
Why do atoms react?
To get a full outer shell
46
How many electrons are allowed in the outer shells?
1st shell = 2 2nd shell = 8 3rd shell = 8
47
What ways were elements categorised in the past? and why?
-physical and chemical properties -their atomic weight Scientists had no idea about electrons protons and neutrons so their was no such thing as atomic number to them.
48
What did Dmitri Mendeleev do?
In 1869 Mendeleev took 50 known elements and arranging them mainly in order of atomic weight but did switch that order if properties meant it should be changed.
49
Why did Mendeleev leave gaps in his periodic table?
Gaps were left in the table to make sure that elements with similar properties stayed in the same group. some gaps indicate the existence of
50
What confirmed that Mendeleev was correct?
The discovery of isotopes in the early 20th century.
51
What are metals?
Metals are elements that can form positive ions when they react.
52
Where are metals and non-metals located in the periodic table?
metals - towards the left and to the bottom non-metals - towards the right and to the top
53
Why is it much harder for non-meals to form positive ions?
This is as they are either to the right of the periodic table where they have lots of electrons to remove to get a full outer shell or towards the top where the outer electrons are close to the nucleus so feel a strong attraction
54
Where does metallic bonding bonding happen?
In metals
55
What are the similar physical properties of metals?
-They're strong (hard to break), but can be bent or hammered -They're great at conducting heat and electricity -They have high boiling and melting points
56
Why don't non-metals exhibit the same properties as metals?
They don't have metallic bonding
57
What are the properties of non-metals at room temperature?
-dull looking -more brittle -aren't always solids at room temperature -don't generally conduct electricity -often have a lower density
58
What are the properties of the transition metals? What are some that are specific to transition metals?
They tend to have the properties of 'proper' metals -good conductors of heat and electricity -very dense -strong -shiny -transition metals can form coloured compounds -transition metal compounds are good catalysts -transition metals can have more than 1 ion
59
What are group 1 elements also known as?
alkali metals
60
How many electrons do group 1elements have in their outer shell?
1
61
What are the properties of the group 1 elements?
-soft -low density
62
What are the trends as you go down group 1 elements?
-increase in reactivity -lower melting and boiling points -higher relative atomic mass
63
What do alkali metals form with non-metals?
ionic compounds. These compounds are generally white solids that dissolve in water to form colourless solutions.
64
How do group 1 metals react in water?
They react vigorously to produce hydrogen gas and metal hydroxides - compounds that dissolve in water to produce alkaline solutions the lower down in the group an alkali metal is the more violent the reaction - the energy given out increases
65
How do group 1 metals react in chlorine?
They react vigorously when heated in chlorine gas to form white metal chloride salts
66
What do group 1 metals form when it reacts with oxygen?
The group 1 metals can react with oxygen to form a metal oxide.
67
Compare group 1 metals with transition metals.
Group 1 metals are much more reactive than transition metals, they react more vigorously with water, oxygen or group 7 elements. Transition metals and have much lower melting points, stronger and harder.
68
What are group 7 elements also known as?
Halogens - non metals with coloured vapours
69
Describe fluorine.
very reactive, poisonous yellow gas
70
Describe Chlorine.
Fairly reactive, poisonous dense green gas
71
Describe Bromine.
dense, poisonous red-brown volatile liquid
72
Describe Iodine.
dark grey crystalline solid or a purple vapour
73
What are the trends as you go down group 7?
-less reactive -higher melting and boiling points -higher relative atomic mass
74
What do group 7 form with metals?
Ionic bonds
75
What are group 0 elements called?
Noble gases
76
How many electrons are there in the outer shell of the group 0 elements?
8 giving them a full outer shell
77
What do group 0 elements live as?
Monatomic gases - single atoms not bonded to each other
78
Describe the group 0 elements at room temperature.
Colourless gasses
79
What are the trends as you go down the group 0 elements?
-increased boiling points -increased relative atomic mass

GCSE - Chemistry (10 decks)

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