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Chemistry > Topic 1 - Atomic Structure And The Periodic Table > Flashcards

Topic 1 - Atomic Structure And The Periodic Table Flashcards

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1
Q

What is a compound?

A

When an atom is chemically combined with another atom to make a compound

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2
Q

What are the four key features of a chemical reaction?

A
  • compounds are broken up or formed
  • at least one new substance is formed
  • there is a measurable energy change
  • no atoms are created or destroyed
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3
Q

What are mixtures?

A

2+ substances that haven’t been combined chemically and can be separated

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4
Q

Do the chemical properties change in mixtures?

A

No

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5
Q

What does chromatography separate?

A

Solutions with a number of different solutes (solids) in the solvent (liquid)

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6
Q

What does filtration separate?

A

Mixtures that contain insoluble solids and liquids

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7
Q

What does crystallisation separate?

A

Solutions into their separate parts (dissolved solids and liquids)

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8
Q

What does fractional distillation separate?

A

Lots of liquids with different boiling points

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9
Q

What does simple distillation separate?

A

Two liquids with different boiling points

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10
Q

How does simple distillation work?

A

1) The mixture is heated until the liquid with the lower boiling point starts to boil
2) the vapour released passes through a condenser, where the gas cools back into a liquid

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11
Q

Why is a thermometer used in simple distillation?

A

To make sure the highest boiling point isn’t exceeded otherwise both liquids would boil and the process would not separate them

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12
Q

What did John Dalton describe atoms as?

A

Solid spheres

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13
Q

What did JJ Thompson discover?

A

Electrons and came up with the ‘plum pudding model’ which shows atoms as a ball of positive charge with electrons stuck in it

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14
Q

What experiment did Ernest Rutherford do?

A

The alpha particle scattering experiment - he fired positively charged alpha particles at a thin sheet of gold

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15
Q

What conclusion did Ernest Rutherford reach?

A

The mass of an atom was concentrated in the centre and has positively charged protons

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16
Q

What atomic model did Rutherford come up with?

A

The nuclear model

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17
Q

What did Bohr discover?

A

Electrons orbit the nucleus at fixed distances

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18
Q

Who discovered neutrons?

A

James Chadwick

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19
Q

What is an element’s atomic number?

A

How many protons it has

20
Q

What is an element’s mass number?

A

The total number of protons and neutrons

21
Q

What are isotopes?

A

Atoms of the same element with the same number of protons but a different number of neutrons

22
Q

What is a relative atomic mass?

A

The average mass of all of the isotopes of an element

23
Q

What are elements on the periodic table organised by?

A

In order of their atomic number (how many protons they have). Every time you move an element to the right, the proton number increases by 1

24
Q

Why do elements in the same column/group react in similar ways?

A

They have the same number of electrons on their outer shell

25
Q

How did John Newlands organise the periodic table?

A

It was ordered by the mass of an element but the table was incomplete and some elements were placed in inappropriate groups

26
Q

What did Mendeleev do to the periodic table?

A

He recognised that there may be many undiscovered elements so added gaps to account for them. He also predicted the properties and masses of the undiscovered elements.
- he put elements in order of relative atomic mass

27
Q

Where are metals found on the periodic table?

A

The left because they have few electrons on their outer shell

28
Q

Properties of metals:

A

High melting and boiling point
Solid @ room temperature
Good conductors of heat and electricity

29
Q

Where are non-metals found on the periodic table?

A

The right hand side because they have many electrons on their outer shell

30
Q

Properties of non-metals:

A

Low melting and boiling points
Normally found as gases
Generally do not conduct heat or electricity

31
Q

Where are noble gases found?

A

In group 0

32
Q

Properties of noble gases:

A

Unreactive because they have a full outer shell already
Can be used in light bulbs as don’t react with the hot metal filament
Low boiling point
Low density

33
Q

What does it mean by ‘noble gases are monatomic’

A

Noble gases exist as single atoms instead of forming molecules because they are unreactive

34
Q

What happens to the boiling point of noble gases as you go down the periodic table?

A

The boiling point increases
Due to the number of electrons increasing meaning there are greater intermolecular forces

35
Q

What happens to the density of noble gases as you go down the group?

A

It increases because of the increasing relative atomic mass.
Low density makes them useful for balloons

36
Q

Where are halogens found?

A

Group 7

37
Q

Properties of halogens:

A
  • very reactive because they easily accept an electron into the outer shell
  • form negative ions
  • diatomic molecules
38
Q

What happens to the reactivity of halogens as you move down the periodic table?

A

It decreases because the distance between the outer electron shell and the nucleus increases so the attraction between the nucleus and the electron (to be gained from another element) decreases

39
Q

What can happen to less reactive halogens?

A

They can be displaced by more reactive halogens from compounds

40
Q

What are the elements found in group one referred to as?

A

Alkali metals

41
Q

What happens to the reactivity of alkali metals as you move down the periodic table?

A

It increases because the distance between the outer electron and the nucleus increases meaning there is a weaker force of attraction between them and it’s easier for an electron to be lost

42
Q

How do group one metals react with water?

A

The metal floats on the surface and melts to create a metal hydroxide. The energy released in fed reaction is enough to melt the metal

43
Q

How do group one metals react with chlorine?

A

A metal chloride is formed which dissolves in water to give a colourless solution

44
Q

How do group one metals react with oxygen?

A

The metal rapidly turns from silvery/shiny to dull as a metal oxide is produced

45
Q

Where are transition metals found?

A

In the middle of the periodic table

46
Q

Relative to the alkali metals what are the properties of transition metals:

A
  • higher density
  • greater strength and hardness
  • lower reactivity
  • higher melting points
  • can be used as catalysts

Chemistry (9 decks)

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