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GCSE Chemistry > Paper 1/ 2: Section 1- Key Concepts of Chemistry > Flashcards

Paper 1/ 2: Section 1- Key Concepts of Chemistry Flashcards

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1
Q

A chemical _______ are shown through word or symbol equations. ______ equations need to be balanced- having the same number of _____ of each _______ on both sides of the equation.

A
  1. equations
  2. Symbol
  3. atoms
  4. element
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2
Q

What are the four state symbol and what do they tell you?

A

State symbols show the state of a substance in an equation:
(s)- solid
(l)- liquids
(g)- gas
(aq)- aqueous

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3
Q

List the eight common hazard symbols:

A

. Oxidising
. Toxic
. Harmful
. Corrosive
. Environmental
. Flamable

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4
Q

At the start of the 19th century, how did John Dalton describe an atom?

A

Described an atom as solid spheres. Suggesting that different spheres made up the different elements.

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5
Q

Describe the theory and backstory behind the ‘Plum Pudding Modlel’.

A

In 1897, J J Thomson concluded from his experiments that atoms weren’t solid spheres. His measurements of charge/ mass showed the presence of small, negatively charged particles- electrons. Then creating knew theory of the ‘Plum Pudding Modlel’.

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6
Q

How did Rutherfords gold foil experiment disprove the ‘Plum Pudding Model’?

A

In 1909, Rutherford conducte an experiment where they fired positively charged alpha particles at a thin sheet of gold. While most passed through the foil, more than expected were deflected (some even backwards). This ment the ‘Plum Pudding Model’ couldn’t be right.

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7
Q

What theory did Rutherford use to explain his new evidence?

A

The theory of the nuclear atom- a tiny positively charged nucleus, surrounded by a ‘cloud’ of electrons.

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8
Q

What theory is the closest to the version of the atom we see today? What did it suggest?

A

The Bohr Model:
. Suggested all electrons were contained in the shells or only existed in fixed orbits.
. Proposed the idea that each shell has a fixed energy.

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9
Q

List the relative mass and charge of the three subatomic particles that make up the atom:

A

PARTICLE MASS CHARGE
Proton: 1 +1
Neutron: 1 0
Electron: 1/ 1865 -1

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10
Q

Where is most of the mass of an atom concentrated?

A

The nucleus

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11
Q

Why does every atom have no overall charge?

A

They contain equal numbers of positive protons and negative electrons. These opposite charges cancel each other out making the atom neutral.

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12
Q

What is the atomic number and where can you find this on the nuclear symbol?

A

The number of protons an atom has, which determines an elements place in the periodic table.
. Its the higher number on the nuclear symbol

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13
Q

What is the mass number and where can you find this on the nuclear symbol?

A

The total number of protons and neutrons in a nucleus.
. Its the lower number on the nuclear symbol.

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14
Q

Isotopes are different forms of the same _______ that contain equal numbers of _______ but different numbers of ________ in their nuclei.

A
  1. element
  2. protons
  3. neutrons
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15
Q

What is the relative atomic mass and where can you find this on the nuclear symbol?

A

The ratio of the average mass of one atom of an element to one twelfth of the mass of an atom of carbon-12.
. Its the higher number on the nuclear symbol.

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16
Q

How do you calculate the relative atomic mass (Ar)?

A

Ar= total mass of atoms x total number of atoms/ 100

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17
Q

How can you work out the Ar from isotopic abundances?

A

. Multiply each relative isotopic mass by its different quantities (isotopic abundances), and add up the results.
. Divide by the sum of the abundances.

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18
Q

How do you calculate isotopes?

A

Isotopes= the atomic mass- atomic number

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19
Q

How does the existence of isotopes result in the relative atomic mass of some elements not being whole numbers?

A

The relative atomic mass is the average mass of different isotopes of the element, therefore it is not always a whole number.

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20
Q

Who made the first periodic table and how was it arranged?

A

In 1869, Dmitri Mendeleev created the first proper periodic table. He sorted the elements based on their properties, and in order of atomic mass.

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21
Q

What are the three electron shell rules?

A
  1. Electrons always occupy shells (also known as energy levels)
  2. The lowest energy levels are always filled first.
  3. 1st shell has 2 electrons only, the 2nd only 8 shells and the 3rd only 8 shells too.
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22
Q

How can you work out the electronic configuration?

A
  1. The atomic number tells you the amount of protons, and protons= electrons.
  2. Then follow the electronic configuration rules.
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23
Q

What are ions and when do they form?

A

Ions are charged particles (in groups or as single atoms)- when atoms lose or gain electrons.

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24
Q

What is an anion?

A

Negative ions that form when atoms GAIN electrons.

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25
Q

What is a cation?

A

Positive ions that form when atoms LOSE electrons.

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26
Q

The ______ of electrons lost or gained is the same as the ______ on the ion.

A
  1. number
  2. charge
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27
Q

What is an ion?

A

An atom or group of atoms with a positive or negative charge.

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28
Q

Metal atoms ____ electrons to form positively charged ions. Whereas, non-metal atoms ____ electrons to form _________ charged ions

A
  1. lose
  2. gain
  3. negatively
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29
Q

Why are group 1, 2, 6 and 7 most likely to form ions?

A

or elements in groups 1 and 2 the number of electrons lost is the same as the group number.
Simlarly, for groups 6 and 7, the number of electrons gained is equal to (8 - group number).

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30
Q

What do the endings -ide and -ate mean?

A

-ide means the compound contains 2 elements (one is the nonmetal -ve ion)
-ate means the compound contains at least 3 elements, one of which is oxygen

31
Q

How do you work out the formula of an ionic compound?

A
  1. Write the symbol and charge of the cation (metal) first and the anion (nonmetal) second.
  2. Use a multiplier to make the total charge of the cations and anions equal to each other.
  3. Use the multipliers as subscript for each ion.
  4. Write the final formula. Leave out all charges and all subscripts that are 1.
32
Q

What is the definition of an ionic bond?

A

The electrostatic attraction between oppositely charged ions.

33
Q

How can electron transfer during the formation of an ionic compound be represented?

A

By a dot and cross diagram or the ball model.

34
Q

What is the structure of an ionic compound as a lattice structure?

A

. A giant structure of ions = ionic compound
. Held together by strong electrostatic forces of attraction- High melting points and boiling points
. The forces act in all directions in the lattice, and this is called ionic bonding.
. The lattice has a regular arrangement of ions

35
Q

What are the limitations of the models that show structures?

A
36
Q

What is the definition of a covalent bond?

A

A shared pair of electrons. Covalent bonding results in the formation of molecules or giant structures.

37
Q

Dot and cross

A
38
Q

What are the properties of simple molecular substances?

A

. Low melting and boiling points – this is because little energy is needed to break the weak intermolecular forces.
. Do not conduct electricity – this is because they do not have any free electrons or an overall electric charge in any state of matter.

39
Q

What are polymers made up of and when are they formed?

A
40
Q

What are the properties of most giant covalent structures?

A
41
Q

How many covalent bonds are diamonds formed from?

A

4

42
Q

Do diamonds have a high or low melting point? Why?

A

High melting points because it takes a lot of energy to break the bonds.

43
Q

Why are diamonds really hard?

A

The rigid network of carbon atoms, held together by strong covalent bonds. and 3D arrangment.

44
Q

Do diamonds conduct electricity? Why?

A

No, there are no free electrons.

45
Q

How many covalent bonds are graphite formed from?

A

3

46
Q

What makes graphite soft and slippery?

A

There are layers of carbon atoms bonded by weak covalent bonds.

47
Q

Does graphite have a high or low melting point? Why?

A

High because they have strong bonds.

48
Q

Does graphite conduct electricity? Why?

A

Yes, graphene has free delocalised electrons.

49
Q

How many layers of graphite is graphene?

A

1

50
Q

Graphene is a sheet of carbon joined together in what shape?

A

A hexagoonal design.

51
Q

How many atoms thick is graphene?

A

1

52
Q

Graphene is a ___ dimensional structure and shape?

A

two

53
Q

Fullerenes

A
54
Q

Fullerenes

A
55
Q

Fullerenes

A
56
Q

Fullerenes

A
57
Q

What is shown as metallic bonding?

A
58
Q

What are most metals physical properties?

A
59
Q

What are most non-metals physical properties?

A
60
Q

What are most non-metals physical properties?

A
61
Q

What are most non-metals physical properties?

A
62
Q

What are most non-metals physical properties?

A
63
Q

Describe the conservation of mass.

A
64
Q

How can we know thee is a gas involved in some experiments?

A
65
Q

What is the definition of relative formula mass (Mr)?

A
66
Q

What is the empirical formula and how do you calculate it?

A
67
Q

What is Avodrogados constant?

A
68
Q

What is a mole and how is it calculated?

A
69
Q

What is the definition of concentration?

A
70
Q

How do you calculate the concentration from the mass of solute?

A
71
Q

The amount of product formed is ______…. (limited reactant)

A
72
Q

How do you calculate the product of a limiting reactant?

A
73
Q

How do you balance equations?

A

GCSE Chemistry (18 decks)

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