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Chemistry Paper 1 > Topic 1 > Flashcards

Topic 1 Flashcards

1
Q

John Daltons Atomic theory 1803

A

Matter is made of atoms which are tiny particles which cannot be created, destroyed or divided
Atoms of the same element are identical, and atoms of different elements different
Different atoms combine together to create new substances

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2
Q

Who discovered the electron

A

JJ Thompson

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3
Q

Discovery of the electron

A

JJ Thompson discovered the electron by using a cathode ray tube which identified th electron as a negatively charged particle hence proving that atoms are divisible

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4
Q

Thompsons model after discovering electron

A

Plum pudding model : negative electrons spread through positively charged material

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5
Q

Who discovered the nucleus

A

Ernest Rutherford

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6
Q

The discovery of the nucleus

A

Gold foil experiment
Rutherford shot a beam of positively charged particles at a thin sheet of gold foil and based on the plum pudding model expected the particles to pass through the foil because the positive charge of the nucleus was thought to be evenly spread out

Some particles scattered however and a few were deflected directly back which led to the idea that most of the atoms mass is centred in the nucleus

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7
Q

The Bohr model

A

Niels Bohr further develop Rutherford concept and suggested that electrons orbit in shells
This model showed why the nucleus does not collapse inwards

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8
Q

Proton relative mass

A

1

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9
Q

Neutron relative mass

A

1

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10
Q

Electron relative mass

A

1/1840

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11
Q

Proton charge

A

+1

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12
Q

Neutron charge

A

0

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13
Q

Electron charge

A

-1

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14
Q

Atomic number

A

The number of protons in the nucleus of the atom

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15
Q

Mass number

A

The sum of the number of protons and neutrons in an atom

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16
Q

Relative atomic mass calculations

A

(%of isotope a x mass of isotope a) + (% of isotope b x mass of isotope b) / 100

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17
Q

Mendeleev arrangement

A

Verticle columns based of their properties of their compounds and arranged them horizontally in order of increasing atomic mass

18
Q

How is the table arranged in modern day

A

Increasing Atomic number
Each element has one proton more than the element preceding it

19
Q

In metals The further down a group and element is

A

The more easily it can react and lose its outer electron
This is because the atomic size is larger so the shells are further away from the nucleus
Weakening their attraction

20
Q

In non - metals the higher up the period the more reactive it is

A

This is because it is easier for them to gain an electron than lose one as they have fuller outer shells

21
Q

Ions

A

Electricity charged particles formed by the loss or gain of electrons

22
Q

Negative ions are called

A

Anions and from when electrons are gained

23
Q

All metals become

A

Cations

24
Q

All non metals become

A

Anions

25
Q

Ionic bonds

A

Strong electrostatic forces of attraction between oppositely charged ions

26
Q

Ionic lattices

A

A regular repeating arrangement of ions
High melting and boiling points due to strong electrostatic forces of attraction between oppositely charged ions

27
Q

Ions with a higher charge have

A

Stronger forces of attraction so higher melting and boiling points

28
Q

IDE ending means

A

Non metal element

29
Q

Ate ending

A

Oxygen is present

30
Q

Clhoride charge

A

Cl-

31
Q

Bromide charge

A

Br -

32
Q

Iodide charge

A

I-

33
Q

Nitrate charge

A

N03 -

34
Q

Sulfate charge

A

S04. 2-

35
Q

Carbonate

A

C03 2-

36
Q

Covalent bonding

A

A shared paint of electrons between atoms

37
Q

Covalent bonds between atoms are

A

Strong

38
Q

Simple covalent bonds do not conduct electricity as

A

They do not contain free electrons

39
Q

Empirical formula

A

Dividing the reacting masses by the relative atomic mass of each element (moles)
Divide each result by the lowest number obtained to give the simplest ratio

40
Q

Concentration equation

A

Mass of solute in grams / volume in dm3

41
Q

Formula triangle for moles

A

Particles

Moles x avogadros constant

42
Q

Converting between moles triangle

A

Mass
Moles x mole mass

Chemistry Paper 1 (5 decks)

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