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GCSE Chemistry Paper 1 v2 > Atomic Structure > Flashcards

Atomic Structure Flashcards

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1
Q

What is an atom?

A

The smallest particle of a chemical element that can exist.

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2
Q

Where is the main mass of the atom located?

A

The nucleus

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3
Q

What is the nucleus made up of?

A

Protons and neutrons

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4
Q

What is the radius of a nucleus compared to the full atom?

A

1/10,000 of the full atoms radius

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5
Q

What charge is the nucleus?

A

Positive

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6
Q

What are electrons?

A

Negatively charged sub-atomic particles

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7
Q

Where are electrons located in an atom?

A

In energy shells that orbit the atom’s nucleus

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8
Q

What is the charge of protons, electrons and neutrons?

A 
Proton = +1
Electron = +1
Neutron = 0
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9
Q

What is the overall charge of an atom?

A

0, atoms are normally stable so are neutral

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10
Q

What is the purpose of an atomic number?

A

It communicates the number of protons in the element and defines what element you are looking at.

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11
Q

What defines an element?

A

Every element has a different atomic number, atoms can have a different number of neutrons and electron, but they change to a whole different element if their number of protons change. They include only one type of atom.

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12
Q

What does the relative atomic mass of an atom tell you?

A

The total number of protons and neutrons and the mass of the atom relative to the other atoms.

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13
Q

How do you work out the number of Neutrons in an element?

A

Subtract the number of protons (atomic number) from the number of protons + neutrons (atomic mass).
[atomic mass-atomic number]

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14
Q

What are isotopes?

A

Isotopes are atoms with a different number of neutrons to the average atom, this means that the relative mass of the atom is different, but the atomic number is the same.

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15
Q

How do you calculate the relative atomic mass of an element?

A 
          Sum of abundance of all the isotopes
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16
Q

What is an element?

A

One type of atom

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17
Q

What is a compound?

A

Substances formed with two or more elements that chemically bond together, the new substance will have different properties to the elements

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18
Q

How are bonds created and what sub-atomic particle is involved in the creation of bonds?

A

Bonds are created from the sharing, loss or gain of electrons, only electrons are involved in bonding?

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19
Q

How do you calculate the relative formula mass of a compound?

A 
Add all the relative formula masses of the elements, multiplied by the number of that element:
CO2
C = 12
O = 16 > O2 = 32
CO2 relative atomic mass = 44
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20
Q

What is the formula for Carbon Dioxide?

A

CO2

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21
Q

What is the formula of Ammonia?

A

NH3

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22
Q

What is the formula of water?

A

H2O

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23
Q

What is the formula of Sodium Chloride?

A

NaCl

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24
Q

What is the formula of Carbon Monoxide?

A

CO

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25
Q

What is the formula of Hydrochloric acid?

A

HCl

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26
Q

What is the formula of Calcium Chloride?

A

CaCl2

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27
Q

What is the formula of Sodium Carbonate?

A

Na2CO3

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28
Q

What is the formula of Sulfuric acid?

A

H2SO4

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29
Q

What is a mixture?

A

A combination of multiple elements that are not chemically bound but just mixed together.

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30
Q

What are the separation techniques?

A
  • Chromatography
  • Simple Distillation
  • Fractional Distillation
  • Crystallisation
  • Filtration
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31
Q

What is chromatography?

A

A method used to separate a mixture by dissolving it in a solvent that moves up a special chromatography paper.

32
Q

What is the method to Chromatography?

A
  • Draw a base line at the bottom of the chromatography paper, this should be draw in pencil,
  • Add a dot of ink (the mixture you wish to separate) onto the paper, this is on the base line,
  • clip the chromatography paper onto a wood splint so it can hang from the lid of the container and not fall into the solvent,
  • Put the chromatography paper into a solvent in a container, the solvents volume should not reach the base line,
  • Place a lid on top of the container,
  • The mixture should dissolve in the solvent and move up the paper, the experiment stops when the mixture stops moving up the paper.
  • This shows the different colours of ink and how soluble they are, more soluble inks move further up the paper.
33
Q

How does filtration work?

A

A liquid with an insoluble substance inside is filtered to separate the liquid from the insoluble substance:

  • The mixture is poured through a filter paper that is above a beaker,
  • The liquid will soak through the paper and into the beaker,
  • The insoluble substance will get caught in the filter paper
34
Q

What is filtration used for?

A

Most commonly used to separate impurities from a substance, this is also known as PURIFICATION.

35
Q

How does crystallisation work?

A

It is used to separate a mixture with a solvent and a dissolved solute:

  • First pour the mixture into an evaporation dish,
  • Place this over a Bunsen burner and begin to heat the mixture,
  • When the solvent has evaporated, all that is left should be the solute crystals,
  • However, if you wanted to keep the solvent use distillation.
36
Q

How do you separate Rock Salt?

A

Filtration and Crystallisation can be used to extract the salt and sand:

  • First grind the rock salt into tiny granules,
  • Add all the rock salt into water so that the salt can dissolve,
  • Stir
  • Then pour the mixture into a beaker through filter paper.
  • The sand should be collected in the filter paper, the salt solution should have passed through into the beaker,
  • Then use crystallisation to separate and collect the salt crystals from the solution.
  • After this, heat up the sand to evaporate any trapped water and have only fry sand left.
37
Q

How does distillation work?

A

A mixture of two liquids or a solute and solvent can be separated whilst all products are kept:
- The solution is kept in a closed flask with a bung on top
- Through the bung is a thermometer,
The solution is heated and the solvent with the lowest boiling point evaporates,
- The vapour then goes up the flask and through a condenser to a conical flask,
- In the condenser, the solvent condenses and flows down into the conical flask,
- Both liquids / liquid and solute and now separate and stored.

38
Q

Wow does fractional distillation work?

A

Uses distillation to separate a mixture with multiple fractions, each fraction is collected and stored separately by using a condenser and having multiple collection tubes (measuring cylinders).

39
Q

What is fractional distillation mainly used for and how is it used?

A

Separating crude oil.
The boiling points of each hydrocarbon in the mixture of crude oil are manipulated. The lower the boiling point of the hydrocarbon (the shorter the chain), the higher it liquid rises in vapour form, it will then condense when it rises to a point high enough on the chamber where it is cooler than its boiling point and condense. The separated hydrocarbon now flows down a tube into a storage container that stores each hydrocarbon individually.

40
Q

How did John Dalton describe the atom?

A

He said the atom was a solid sphere, different spheres made up different elements.

41
Q

What model did J J Thomson invent?

A

The plum pudding model,

a cloudy positive charge with tiny negatively charged particles inside (electrons)

42
Q

How did Ernest Rutherford disprove Thomson’s theory?

A

He shot alpha particles (a helium nucleus), at a an extremely thin sheet of gold,

Rutherford expected them all to pass straight through because there was thought to be no central mass in the middle of an atom and it was neutrally charged,
However, some alpha particles were deflected and some were deflected directly back to the alpha particle radiator.

This means that there must be a positively charged nucleus or mass in the middle of an atom because some alpha particles (which are positively charged) repelled of to the side. Those that were some directly to the nucleus deflected straight back by repulsion, this means the centre of the atom must hold a great deal of mass.

But most the alpha particles went straight through so atoms are mainly empty space.

43
Q

What was Rutherford’s model called?

A

The nuclear model

44
Q

What was Neils Borh’s theory of the atom?

A

He disproved that a cloud of electrons existed because they would attract to the positive nucleus and collapse the atom, therefore, he suggested that electrons were kept in energy shells.

45
Q

Who discovered the neutron?

A

James Chadwick

46
Q

Who are the scientists involved in the history of the atom? (in order)

A 
John Dalton - atoms are spheres
J J Thomson - plum pudding
Ernest Rutherford - gold foil + alpha particles = nucleus
Neils Bohr - electron sheels
James Chadwick - neutrons
47
Q

How many electrons in the first, second and third shell?

A

2,8,8

48
Q

What were the two ways to sort the periodic table in the 1800s?

A
  • atomic mass

- atomic properties

49
Q

Who created the first periodic table?

A

Dmitri Mendeleev

50
Q

What did Mendeleev do to change the ordering of the periodic table?

A
  • He left gaps for undiscovered elements

- The properties of the elements are more important in the ordering of the elements than the atomic mass.

51
Q

How is the modern period table sorted?

A

By atomic number (protons number)

52
Q

Why are elements sorted into groups?

A
  • All elements in the same group have similar chemical qualities,
  • All elements in the same group have the same number of electrons on the outershell
53
Q

Why are elements sorted in periods?

A

Groups represent the number of electron shells, e.g. group 3 has 3 outer shells

54
Q

What side of the periodic table are the metals?

A

The left and middle

55
Q

What side of the periodic table are the non-metals?

A

The right side

56
Q

What ions do metals form?

A

+ions (cation)

57
Q

What ions do non-metals form?

A

-ion (anion)

58
Q

What are the properties of metals?

A
  • They are strong
  • They are malleable
  • Are very good conductors of heat and electricity
  • high boiling and melting points
59
Q

What are the properties of non-metal?

A
  • They are dull
  • Brittle
  • Aren’t always solid at room temperature
  • Poor conductors of electricity and electricity
  • Often have a low density
60
Q

What are the properties of transitional metals?

A
  • They can have more than one ion, e.g. Cu(I) and Cu(II)
  • They can be used as catalysts
  • Make coloured compounds
61
Q

What are the trends going down group 1 (Alkali metals)?

A
  • Increasing reactivity
  • Decreased melting and boiling point
  • higher relative atomic mass
62
Q

What do alkali metals make when they react with water?

A

Metal Hydroxide + Hydrogen

63
Q

What do alkali metals make when they react with Cl, I or Br

A
  • Metal Chloride
  • Metal Iodide
  • Metal Bromide
64
Q

What are differences between group 1 metals and transitional metals?

A
  • Transitional metals are stronger
  • Transitional metals have higher melting points and boiling points
  • Group 1 metals are much more reactive
65
Q

What are the trends going down group 7 (halogens)?

A
  • Decreasing reactivity
  • Higher melting and boiling points
  • Higher relative atomic mass
66
Q

What is fluorine?

A

A very reactive, poisonous, yellow vapour

67
Q

What is chlorine?

A

A fairly reactive, poisonous dense green gas

68
Q

What is bromine?

A

Is a dense, poisonous, red-brown volatile liquid

69
Q

What is iodine?

A

A dark grey crystalline solid or purple vapour

70
Q

What does diatomic mean?

A

When particles come in pairs of atoms,

- all group 7 elements are diatomic molecules

71
Q

What are the two ways that group 7 molecules can bond?

A
  • Covalent bonding with other non-metals

- Ionic bonding with metals

72
Q

What happens in a reaction if two group 7 elements are involved?

A

The more reactive element displaces the less reactive elements

73
Q

What are the trends going down group 0/8 (noble gases)?

A

Boiling point increases because there are more electrons, this means more energy is needed to break the stronger inter-molecular forced

74
Q

Why are the noble gases not reactive?

A

they have a full outer shell so they do not need to gain or lose electrons to get a full outer shell.

75
Q

What are the properties of the noble gases?

A
  • They are colourless gases,
  • Very low boiling and melting point
  • They are monotonic gases (single atoms, not diatomic)
  • Non-flammable
  • full outer shell

GCSE Chemistry Paper 1 v2 (5 decks)

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