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Chemistry paper 1 > Key Concepts > Flashcards

Key Concepts Flashcards

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1
Q

Which 5 scientists contributed to the atomic structure in order

A

Dalton
Thompson
Rutherford
Bohr
Chadwick

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2
Q

What did Dalton say about atoms

A

Hard speeds that are indivisible

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3
Q

What did Thompson discover and what was his model

A

Electron - plum pudding model

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4
Q

What did Rutherford discover and what was the name of his experiment

A

Positive nucleus - gold foil experiment

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5
Q

What did Bohr discover

A

Shells and energy levels

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6
Q

What did Chadwick discover

A

Neutron

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7
Q

What is the relative mass of an electron

A

Negligible or 1/1836

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8
Q

What 2 values are shown next to the name of an atom on the periodic tabke

A

Mass number
Atomic number

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9
Q

What is theass number

A

Protons + neutrons

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10
Q

What is the atomic number

A

The number of protons/electrons

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11
Q

What is an isotope

A

Atoms of an element that have the same number of protons but a different number of neutrons

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12
Q

Who made the modern periodic table

A

Mendeleev

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13
Q

What 3 steps did Mendeleev take to make the periodic table

A
  1. Put all the elements in order of relative atomic mass
  2. He checked the properties of elements and swapped some elements around so that elements with similar properties lined up
  3. He left gaps where he thought there were other elements and predicted their properties
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14
Q

What do you call the vertical columns on the periodic table

A

Groups

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15
Q

What do you call the horizontal rows on the periodic table

A

Periods

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16
Q

What does the group of an element show

A

The number of electrons on its outer shell

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17
Q

What does the period of an element show

A

The number of shells

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18
Q

Which side of the periodic tables are metals

A

Left side

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19
Q

What is the electronic configuration of oxygen

A

2.8.6

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20
Q

What is an ion

A

An atoms that has gained or lost electrons to make an atom with a charge

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21
Q

Do metals form anions or cations

A

Cations

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22
Q

What diagram can be used to show ions being formed

A

Dot and cross model

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23
Q

What is the name of a fluorine ion

A

Flouride

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24
Q

What is the charge of a nitrate

A

-1

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25
Q

What is the charge of a carbonate

A

2-

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26
Q

What is the charge of a sulfate

A

-2

27
Q

What is the charge of a hydroxide ion

A

-1

28
Q

What are ionic bonds and where are they formed

A

Strong electrostatic forces of attraction between 2 oppositely charged ions

29
Q

What is the name of the arrangement given to an ionic compound

A

Lattice

30
Q

What are the melting/boiling point of ionic compounds and why

A

They have high boiling/melting points as they have many strong ionic bonds and each bond needs a large amount of energy to be transferred to the lattice structure to break these bonds

31
Q

Are ionic compounds soluble

A

Yes

32
Q

Explain conductivity for ionic compounds

A

Yes but only when liquid as the charged ions need to be free to move around so that they can carry the electrical charge from place to place

33
Q

When is a covalent bond formed

A

When electrons are shared between stoms

34
Q

What are some properties of covalent bonds

A

Are strong
Form between non metals

35
Q

What type of bonds do diatomic molecules have

A

Covalent

36
Q

What diagram can be used to show covalent bonding

A

Dot and cross

37
Q

How many covalent bonds can carbon form

A

4

38
Q

What is a simple molecular substance

A

Consists of just a few atoms joined together by strong covalent bonds

39
Q

Give some examples of simple covalent substances

A

H2O
Oxygen

40
Q

What are the boiling points of simple molecular substances like and why

A

Low melting and boiling point as even though they have strong covalent bonds there are only weak intermolecular forces between molecules which do not require much energy to be overcome

41
Q

Why can’t simple molecular substances conduct electricity

A

They are not charged and do contain electrons that are free to move around and carry the current

42
Q

What are giant molecular substances

A

Consist of many atoms that are bonded together by strong covalent bonds and arranged in a regular lattice

43
Q

What are the boiling/melting points like in giant molecular substances and why

A

High melting/ boiling point as a lot of energy must be transferred to break the many strong covalent bonds

44
Q

What model can be used to model giant molecules

A

Ball and stick models

45
Q

What are 2 giant molecular allotropes of carbon

A

Graphite
Diamond

46
Q

What are some properties of diamond

A

Each carbon atom is bonded to 4 others
Strong covalent bonds between each atom

47
Q

What are some properties of graphite

A

Each atoms is bonded to 3 others
Weak intermolecular forces between layers
Delocalised electrons

48
Q

What is graphene

A

A giant molecular substance that is a single layer of graphite

49
Q

What are some properties of graphene that make it extremely useful and why it has those features

A

Graphene conducts electricity
Very strong
Transparent

50
Q

What is a fullerene

A

A layer of graphene that is in a rolled form of graphene

51
Q

What are 2 examples of fullerene

A

Hollow balls
Nanotubes

52
Q

What is bucky ball

A

A fullerene with 60 carbon atoms. It is in a speed form made out of hexagons

53
Q

What is nanotube

A

A fullerene that are long hollow tubes

54
Q

What are some properties of fullerenes

A

Conduct electricity
Are soft when in sold state as they have weak intermolecular forces

55
Q

What are some properties of nanotubes

A

Conduct electricity
Very strong as they have lots of covalent bonds

56
Q

What are 4 properties of metals

A

Shiny
Good conductors
High density
High melting points

57
Q

What is the metallic structure and bonding

A

Consists of a giant lattice of positively charged metal ions. Surrounded by a sea of delocalised electrons

58
Q

Why are metallic bonds strong

A

Have strong electrostatic forces of attraction between metal ions and delocalised electrons

59
Q

Why are metals malleable

A

Layers of positive ions slide over each other so they can change shape

60
Q

What does ductile mean

A

It can be thinned into wires without breaking

61
Q

How to cover from cm3 to dm3

A

Divide by a thousand

62
Q

What is the formula for concentration that uses grams

A

Conc = mass / volume

63
Q

What is the formula for conc that uses moles

A

Conc = mol / vol

Chemistry paper 1 (9 decks)

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