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GCSE Chemistry > Half term 1 > Flashcards

Half term 1 Flashcards

1
Q

What are group one elements also called?

A

alkali metals

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2
Q

What are the main properties of group 1 elements?

A

soft
low densities
low melting and boiling points
very reactive

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3
Q

What group are alkali metals in?

A

group 1

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4
Q

What are the trends as you move down group 1?

A

Increasing reactivity
decreasing mpt and bpt
higher relative atomic masses

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5
Q

Why does the reactivity increase as you move down group 1?

A

outer electron more easily lost
attraction between the nucleus and the electron decreases because the electron id further away from the nucleus due to there being more shells

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6
Q

What ions do alkali metals make?

A

1+

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7
Q

Why is it so easy for alkali metals to form ions?

A

They only need to lose one electron to get a full outer shell and that does not take much energy

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8
Q

What are the ionic compounds formed by alkali metals usually like?

A

white solids
dissolve in water to form colourless solutions

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9
Q

Why do alkali metals only ever react to form ionic compounds>

A

It is so easy for them to lose their outer electron.

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10
Q

How do alkali metals react with water?

A

They react vigorously to form products hydrogen gas and metal hydroxide:
compounds that can dissolve in water to produce alkaline solutions.

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11
Q

More reactive metals result in a more ….. reaction?

A

violent/ vigorous
the amount of energy given off will also increase

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12
Q

How do alkali metals react with chlorine?

A

react vigorously when heated with chlorine gas to produce white metal chloride salts

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13
Q

How do alkali metals react with oxygen?

A

forms a metal oxide (the type of oxide depends on the alkali metal reacted)

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14
Q

Why do transition metals tarnish in the air?

A

They react with oxygen in the air which causes a dull metal oxide layer to form

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15
Q

Lithium reacts with oxygen to form ….

A

lithium oxide

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16
Q

Sodium reacts with oxygen to form….

A

a mixture of sodium oxide and sodium peroxide

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17
Q

Potassium reacts with oxygen to form….

A

a mixture of potassium peroxide and potassium superoxide

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18
Q

How are alkali metals different to transition metals?

A

alkali metals are much more reactive, less dense, less strong, less hard and have lower melting points.

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19
Q

How are the particles in solids arranged?

A

strong forces of attraction between particles- holds them close together in a regular lattice arrangement
particles vibrate around a fixed point
keep a definite shape and volume
expand slightly when heated - the particles vibrate more

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20
Q

How are the particles in liquids arranged?

A

Weak forces of attraction between particles
randomly arranged and free to move past each other- tend to stick closely together.
definite volume
no definite shape- flow to fill the bottom of a container
particles constantly move in a random motion
expand slightly when heated - the particles move around more

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21
Q

How are the particles in gases arranged?

A

very weak forces of attraction between particles
free to move and are apart - particle in gases travel in straight lines
no definite shape or volume - fills the container
particles move constantly in a random motion
particles move faster when heated - gas either expands or has an increase in pressure

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22
Q

What factor controls that state a substance is at a certain temperature?

A

how strong the forces of attraction are between the particles

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23
Q

The strength of the forces of attraction between particles depends on three things?

A

temperature
pressure
the material

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24
Q

What are the drawbacks of particle theory?

A

particles aren’t solid, inelastic or spheres - they are atoms ions or molecules
model doesn’t show forces between the particle - no way of knowing how strong they are

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25
Q

What does a change of state change about the particles?

A

their arrangement or energy

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26
Q

solid to liquid?

A

melting

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27
Q

Liquid to solid?

A

freezing / solidifying

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28
Q

Liquid to gas?

A

evaporating

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29
Q

gas to liquid?

A

condensing

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30
Q

gas to solid?

A

deposition

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31
Q

solid to gas?

A

sublimation

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32
Q

The boiling point is where…

A

a liquid changes to a gas

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33
Q

the melting point is where…

A

the solid changes to a liquid

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34
Q

What are the 3 types of bonding?

A

Covalent
Ionic
Metallic

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35
Q

Covalent bonding is where…

A

atoms share electrons so they have full outer shells

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36
Q

Each single covalent bond provides…

A

one electron for each atom

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37
Q

Covalent bonding happens in both…

A

compound (H20) and elements (Cl2)

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38
Q

What three ways can you draw covalent bonds?

A

Dot and cross diagrams
structural formulae (displayed formula)
Three dimensional structures

39
Q

Does ionic bonding happen between metals or non metals?

A

metal - non-metal

40
Q

What happens in ionic bonding?

A

transfer of electrons
metal atom loses electrons to form positively charged ion
non metal gains these electrons to form a negative ion
They are strongly attracted to one another by electrostatic forces, this is an ionic bond

41
Q

What is the name of the forces holding ionic compounds together?

A

electrostatic forces

42
Q

What is metallic bonding?

A

where a sea of delocalised electrons hold together positive ions

43
Q

Is metallic bonding strong?

A

It is very strong

44
Q

What are some key properties of metals?

A

solid at room temperature
conduct electricity and heat
most are malleable

45
Q

What are alloys?

A

Metals that are mixed with other metals (or sometime non-metals) to make them stronger, better suited for a job
the different sized atoms distort the layers and make it difficult for the atoms to slide over each other- making the metal harder

46
Q

Physical properties of metals:

A

strong(hard to break)
malleable
great conductors of heat and electricity
high mpts and bpts
lustrous (shiny)
sonorous (ringing sound when hit)

47
Q

Physical properties of non metals

A

dull looking
more brittle
low mpts and bpts generally
often lower densities
mostly don’t conduct

48
Q

Why can non metals have a range of different chemical properties?

A

They can form a variety of different structures

49
Q

What are elements made up of?

A

atoms with the same atomic number

50
Q

What subatomic particle determines the type of atom?

A

proton

51
Q

What are isotopes?

A

different forms of the same element
same number of protons
different number of neutrons

52
Q

What is a molecule?

A

two or more atoms held together by chemical bonds (can have different atoms)

53
Q

What is a compound?

A

two or more different elements held together by chemical bonds

54
Q

What is a mixture?

A

two or more substances that are not chemically combined

55
Q

What are 3 conclusions drawn from the alpha scattering experiments?

A
  1. Most of the atom was empty space.
    2.There is a concentrated area of positive charge in the atom.
    3.Atoms contain a very small, heavy mass.
56
Q

Who discovered the electron?

A

J. J Thompson

57
Q

Who discovered the proton?

A

Ernest Rutherford

58
Q

Who discovered the neutron?

A

James Chadwick

59
Q

When was the proton discovered?

A

1917

60
Q

When was the electron discovered?

A

1897

61
Q

When was the neutron discovered?

A

1932

62
Q

Where does the word ‘atom’ come from?

A

The Greek word ‘atomos’ meaning indivisible

63
Q

Who described atoms as solid spheres?

A

John Dalton

64
Q

Who created the plum pudding model?

A

J.J.Thompson

65
Q

Who created the first nuclear model?

A

Ernest Rutherford

66
Q

Who conducted the alpha particle scattering experiments?

A

Ernest Rutherford
Hans Geiger
Ernest Marsden

67
Q

What was different about Niels Bohr’s nuclear model?

A

He had the electrons on shells orbiting the nucleus at fixed distances from it.
if there was a cloud of electrons they would all be attracted to the nucleus and the atom would collapse

68
Q

What is the structure of a ionic compound like?

A

a giant ionic lattice
closely packed regular lattice arrangement

69
Q

What are the forces like in ionic compounds?

A

very strong electrostatic forces of attraction between oppositely charged ions in all directions of the lattice.

70
Q

What are the properties of ionic compounds?

A

High melting and boiling points
Conduct electricity when they are molten or dissolved - the ions are free to move and carry electrical charge

71
Q

Atoms are stable when they…

A

have full outer shells

72
Q

How do you work out the number of neutrons in an atom?

A

mass number - atomic number

73
Q

Proton relative mass?

A

1

74
Q

Proton relative charge?

A

+1

75
Q

Neutron relative mass?

A

1

76
Q

Neutron relative charge?

A

0

77
Q

Electron relative mass?

A

0 (negligible)

78
Q

Electron relative charge?

A

-1

79
Q

What is the overall charge of an atom?

A

no overall charge

80
Q

Group 0 elements are also known as…

A

noble gases

81
Q

Properties of the noble gases?

A

Exist as monatomic gases-single atoms not bonded to each other
practically inert (unreactive)
non-flammable
colourless at room temp

82
Q

As you move down the noble gases they:

A

increasing atomic mass
increasing boiling point - caused by greater intermolecular forces which need to be overcome.

83
Q

What used to be the two clear ways to categorize elements?

A

Their physical and chemical properties
their atomic weight

84
Q

How were elements originally organised?

A

by their atomic weight
they didn’t take into account the properties

85
Q

When did Dmitri Mendeleev publish his periodic table?

A

1869

86
Q

What was different about Mendeleev’s periodic table?

A

He left gaps for unknown elements
showed elements with the same chemical properties lined up in groups

87
Q

Group 7 elements are also called …

A

Halogens

88
Q

As you move down the halogens they:

A

become less reactive
have higher melting and boiling points
have higher relative atomic masses

89
Q

What is the order of the reactivity series?

A

potassium
sodium
lithium
calcium
Magnesium
carnon
zinc
iron
tin
hydrogen
copper

90
Q

What is an example of a group 1 element reacting with chlorine?

A

sodium + chlorine -> sodium chloride

91
Q

What is a macromolecule?

A

A giant covalent structures
bonds arranged in giant lattices or networks

92
Q

small molecules contain …

A

a fixed number of atoms joined by covalent molecules

93
Q

giant covalent structures contain …

A

many atoms joined by covalent bonds

94
Q
A

Potassium
sodium
calcium

GCSE Chemistry (5 decks)

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