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

Topic 1 - Atomic Structure And Periodic Table Flashcards

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1
Q

What are all substances made from?

A

Atoms

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2
Q

What is an atom?

A

The smallest part of an element that can exist

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3
Q

How many elements are there?

A

About 100

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4
Q

Where are elements shown?

A

Periodic table

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5
Q

How are compounds formed?

A

chemical reactions of elements

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6
Q

What is a chemical reaction?

A

The formation of 1 or more new substances - often involving a detectable energy change

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7
Q

What are compounds?

A

Contain two or more elements chemically combined in fixed proportions

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8
Q

How do you separate compounds into elements?

A

Chemical reactions

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9
Q

What is a mixture?

A

Two or more elements or compounds NOT chemically combined together

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10
Q

Why are mixtures different from compounds?

A

Chemical properties of each substance in the mixture are unchanged

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11
Q

What are the 5 ways that mixtures can be separated?

A 
Filtration
Crystallisation 
Simple Distillation 
Fractional distillation 
Chromatography
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12
Q

How do physical changes differ from chemical changes?

A

Do not involve chemical reactions

No new substances are made

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13
Q

What is the nucleus?

A

Middle of atom which contains protons and neutrons so has a positive charge

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14
Q

What are electrons?

A

Negatively charged particles that orbit the nucleus in shells

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15
Q

What is the mass of protons, neutrons and electrons?

A

Proton 1
Neutron 1
Electron 1/1830

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16
Q

What is the charge of protons, neutrons and electrons?

A

Proton +1
Neutron 0
Electron -1

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17
Q

What is the atomic number?

A

Number of protons/electrons

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18
Q

What is the mass number?

A

Number of protons + neutrons

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19
Q

What are isotopes?

A

Different forms of the same element which have the same number of protons but a different number of neutrons

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20
Q

What can new experimental evidence leads to?

A

Models being changed or replaced

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21
Q

Before the discovery of the electron, what were atoms thought to be?

A

Tiny spheres that couldn’t be divided

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22
Q

What did the discovery of the electron lead to?

A

The plum pudding model of the atom - suggesting that the atom was a ball of positive charge with negative electrons embedded in it

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23
Q

What did alpha particle scattering experiments lead to?

A

The conclusion that the mass of an atom was concentrated at the centre and was charged (nucleus) - this nuclear model replaced the plum pudding model

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24
Q

How did Neil’s Bohr adapt the nuclear model?

A

He suggested that electrons orbit the nucleus at specific distances - the theory agreed with experimental observations

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25
Q

What happened after Niels Bohr adapted the nuclear model?

A

Experiments led to the idea that positive charge of the nucleus can be subdivided into a number of smaller particles each with the same amount (protons)

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26
Q

What did the experimental work of James Chadwick lead to?

A

Evidence to show the existence of neutrons in the nucleus

27
Q

Do atoms has an overall charge?

A

No

28
Q

How large are atoms?

A

0.1 nm

29
Q

How large is the radius of a nucleus?

A

1/10000

30
Q

What is the relative atomic mass of an element?

A

Average value that takes account of the abundance of the element

31
Q

How are elements in the periodic table arranged?

A

In order of atomic number so elements with similar properties lie in the same group

32
Q

What do elements in the same group of the periodic table share?

A

Have they same number of electrons in their outermost shell giving the similar chemical properties

33
Q

How did scientists classify elements before the discovery of protons, neutrons and electrons?

A

Arranging them into order of their atomic weights

34
Q

Why were the early periodic tables bad?

A

Incomplete

Elements placed in inappropriate groups if order of atomic weights was followed

35
Q

How did Mendeleev solve the problems with the early periodic table?

A

Left gaps for undiscovered elements

Changed some orders

36
Q

How was the periodic table completed?

A

Elements with properties predicted by Mendeleev were discovered and filled the gaps

37
Q

What did the knowledge of isotopes show?

A

Why the order based on atomic weights was not always correct

38
Q

What is a metal?

A

Elements that react to form positive ions

39
Q

What are nonmetals?

A

Elements that do not form positive ions

40
Q

How are metals bonded?

A

Metallic bonding

41
Q

What are the features of a metal?

A

Strong but malleable
Good Heat and electrical conductors
Night melting and boiling points

42
Q

What are the features of a non-metal?

A 
Dull looking 
Brittle 
Not always solids at room temperature 
Lower density 
Can’t conduct electricity generally
43
Q

What group of the periodic table are transition metals found in?

A

Between 2 and 3

44
Q

What are the properties of transition metals?

A 
Can have more than one ion 
Often coloured 
Good catalysts 
Dense 
Strong 
Good conductors
45
Q

What is group 0 also known as?

A

The noble gases

46
Q

What are the properties of noble gases?

A

Unreactive because the atoms have stable arrangements of electrons and a full outer shell

47
Q

How does the boiling point of noble gases change as they go down the table?

A

Increases

48
Q

What our group 1 of the periodic table also known as?

A

Alkali metals

49
Q

How many electrons do group 1 elements have in their outer shell?

A

1

50
Q

What are the properties of alkali metals?

A

Soft
Low density
Increasing reactivity (down the table)
Lower melting and boiling points (down the table)

51
Q

Describe the reaction between water and alkali metals?

A

Produce hydrogen and metal hydroxides
Vigorous reaction
Amount of energy released increases as you go down the group

52
Q

Describe the reaction between Chlorine and Alkali metals?

A

Vigorous (increases as you go down the table)

Heated to Form white metal chloride salts

53
Q

Describe the reaction between oxygen and alkali metals?

A

Form metal oxide

54
Q

How are group one properties different from the properties of transition metals?

A

Group one are more reactive
Group one are less strong, dense and hard
Group one have lower melting points

55
Q

What is group 7 in the periodic table also known as?

A

The halogens

56
Q

Why do all group 7 elements have similar reactions?

A

Because they all have seven electrons in their outer shell

57
Q

What are the halogens?

A

Non-metals that consist of molecules made up of pairs of atoms

58
Q

What happens to the properties of group 7 elements as you go down the table?

A

Reactivity decreases

Higher melting and boiling points

59
Q

What are the properties of fluorine?

A

Very reactive
Poisonous
Yellow gas

60
Q

What are the properties of chlorine?

A

Fairly reactive
Poisonous
Dense
Green gas

61
Q

What are the properties of bromine?

A

Dense
Poisonous
Red-brown volatile liquid

62
Q

What are the properties of iodine?

A

Dark grey Crystalline solid or purple vapour

63
Q

What is a displacement reaction between halogens?

A

A more reactive halogen can displace the salt of a less reactive halogen

Chemistry (11 decks)

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