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Chemistry - S1 > Atomic structure > Flashcards

Atomic structure Flashcards

1
Q

What was the plum pudding model, who suggested it and when?

A

J.J. Thomson, 1904, suggested that the atom consisted of a sphere of positive charge with negative electrons embedded in it. This became known as the Plum Pudding Model.

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2
Q

What is the size of an atom?

A

0.1 nanometres (nm) or 1 X 10 to the power of minus ten

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2
Q

What did Ernest Rutherford do?

A

Ernest Rutherford challenged this idea in 1911 when he carried out the gold foil experiment and suggested that the atom had a positive nucleus at the centre and that the electrons orbited this nucleus.

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3
Q

Who discovered the neutron and when?

A

James Chadwick, 1932, discovered the neutron

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4
Q

How do you calculate the Relative Atomic Mass

A

Relative Atomic Mass = (mass number 1 x abundance) + (mass number 2 x abundance) / total abundance

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5
Q

What is the definition of relative atomic mass?

A

The relative atomic mass is the mass of the atom compared with that of the carbon-12 isotope, which has a mass of exactly 12

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6
Q

What is a cation

A

A cation is a positive ion.

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7
Q

What is ionic bonding and what is the type of structure it forms called?

A

Ionic – electrostatic force of attraction between oppositely charged ions

Compound of a metal and a non-metal and electrons are transferred from the metal to the non-metal

The structure it forms is a giant ionic lattice

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7
Q

What is an anion

A

A anion is a negative ion.

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8
Q

Why do ionic structures conduct electricity when molten?

A

The electrons are free to move and carry a charge

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8
Q

What are the properties of ionic bonding?

A

High melting and boiling point

conducts electricity when molten

soluble in water

brittle

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9
Q

Why do ionic structures have high melting and boiling points?

A

Ionic bonds are strong and require a lot of heat energy to break

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10
Q

What is covalent bonding and what is the type of structure it forms called?

A

When 2 non-metals share electrons to obtain a stable electron structure

Molecular covalent structure is for covalent bonding of molecules and molecules not bonding together

Giant covalent Structure is for bonding of atoms

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11
Q

What is an Ion?

A

An ION is an atom that has lost or gained electron(s) to get a full outer shell. An ion is a charged particle.

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12
Q

What is a diatomic molecule

A

A diatomic molecule is when 2 of the same type of atom are covalently bonded together.

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13
Q

What is a molecule?

A

A Molecule is when 2 atoms are covalently bonded together.

14
Q

What atoms form multiple bonds?

A

Oxygen and Carbon dioxide form double covalent bonds and Nitrogen forms Triple covalent bonds

15
Q

What are the properties of covalent bonding?

A

Low melting and Boiling points

soft and brittle

does not conduct electricity

low solubility in water

strong covalent bonds within the molecules but weak attractive forces called Van Deer Waals between the molecules

16
Q

What is an allotrope?

A

Allotropes are different forms of the same element, in the same physical state.

16
Q

Why does covalent bonding have low melting and boiling points

A

As the weak Van Deer Waal forces require little heat energy to break

17
Q

What is the structure of Diamond

A

The carbon atoms are arranged so that each atom forms a single covalent bond with 4 other carbon atoms in a tetrahedral 3-dimensional structure.

18
Q

What are the properties of Diamond

A

Very hard – the carbon atoms are linked by very strong covalent bonds.

Very high melting point – Large amount of energy is needed to break the strong covalent bonds between the carbon atoms.

Does not conduct electricity – it has no free electrons to carry charge.

19
Q

What is a use of Diamond

A

Diamonds are used in cutting tools because of their extreme hardness or as jewellery.

20
Q

What is the structure of Graphite

A

The carbon atoms are arranged into layers, so that each atom forms a single covalent bond with 3 other carbon atoms. The fourth electron of each carbon is free to move between the layers.
Three - dimensional

21
Q

What are the properties of Graphite

A

Slippery– the layers can slide over each other due to the weak Van der Waals forces between the layers.

Very high melting point – a lot of heat energy is needed to break the strong covalent bonds within the layers.

Conducts electricity – it has free electrons to move and carry charge.

22
Q

What is a use of Graphite

A
  • Used in pencil leads
  • Used as a lubricant in machinery
23
Q

What is the structure of Graphene

A

Graphene is a single atom thick layer of graphite
with strong covalent bonds between each carbon
atom. The atoms are arranged in hexagons. Two- Dimensional

24
Q

What are the properties of Graphene

A

High melting point and boiling point – A large amount of energy is needed to break the strong covalent bonds between each carbon.

Electrical conductivity – Able to conduct electricity as each carbon atom has an unbonded electron. These delocalised electrons can move and carry a charge.

Very strong – due to the strong covalent bonds between the carbon atoms.

25
Q

What are the properties of Metallic Bonding?

A

High melting points – because a lot of heat energy is needed to break apart the strong metallic bonds.

Electrical conductivity – Metals are good conductors as they have free electrons which can move and carry charge.

Malleable (can be beaten into shape) and ductile (can be stretched into wires) - the layers of positive metal ions can slide over one another when a force is applied, without disrupting the metallic bonding.

25
Q

What is a use of Graphene

A
  • Used in solar cells and batteries – as it is light, strong and relatively cheap electrical conductor.
26
Q

What is metallic bonding and what is the type of structure it forms called?

A

The electrostatic attraction between the positive metal ions and the sea of delocalised electrons -Metallic Lattice

Metals only

27
Q

Why is an alloy stronger than a regular metal?

A

An alloy contains different sized atoms which disrupt the regular arrangement of atoms in a metal. This makes it harder for the layers of atoms to slide over each other and the resulting alloy is harder and stronger than the metal.

27
Q

What is an alloy?

A

An alloy is a mixture of two or more elements, at least one of which is a metal and the resulting mixture has metallic properties

28
Q

How do you find the percentage of gold?

A

Number of Carats/24 X 100

29
Q

What is the Method for carrying out the flame test?

A
  1. Dip nichrome wire into concentrated hydrochloric acid
  2. Dip the wire into the test solid
  3. Place nichrome wire in the Blue Bunsen flame
  4. Note the colour of the flame
30
Q

What colour does the flame test turn in each metal?
Lithium
Sodium
Potassium
Calcium
Copper (II)

A

Crimson Red
Orange
Lilac
Brick Red
Green-blue

Chemistry - S1 (6 decks)

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