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Chemistry > All of year 9 > Flashcards

All of year 9 Flashcards

(95 cards)

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1
Q

What are the 3 states of matter

A

liquid
solid
gas

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2
Q

what does each sate of matter depend on

A

how strong the forces of attraction are between the particles of the material

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3
Q

descirbe the arrangement in solids and why

A

very regular because of the strong forces of attraction holding them together

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4
Q

describe the movement of solid particles

A

they don’t move but do vibrate about a fixed point whilst keeping a definite shape and volume

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5
Q

what happens when materials are heated

A

the particles vibrate/move more gaining energy causing the material to expand

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6
Q

describe the arrangement and movement of liquids

A

weak forces of attraction cuase the particles to be random and free to move over each other and fill the bottom of the container

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7
Q

desribe the arrangement of gas particles

A

very weak forces allow the particles to be free to move and be far apart filling any container

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8
Q

What happens when gases are heated

A

they either expand or the pressure is increased

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9
Q

what is the process where a solid becomes liquid

A

melting

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10
Q

what is the process where a liquid becomes a solid

A

freezing

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11
Q

what is the process where a liquid becomes a gas

A

evaporating

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12
Q

what is the process where a gas becomes a liquid

A

condensing

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13
Q

what is the process where a solid becomes a gas

A

subliming

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14
Q

what is diffusion

A

the gradual movement of gas or liquid particles from places where there are lots to places where there are fewer

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15
Q

In a diffusion experiment with ammonia and hyrogen chloride why is the ring of ammonium chloride not in the center

A

becuase the hydrogen chloride particles are denser than the ammonium particles - they take longer to move

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16
Q

what is a solution

A

a mixture of solvent and solute that does not seperate out

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17
Q

what is a solute

A

the substance being dissolved

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18
Q

what is a solvent

A

the liquid the solute dissolves into

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19
Q

what is a saturated solution

A

a solution where the maximum amount of solute has been dissolved

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20
Q

what is solubility

A

the measure of how much solute will dissolve in 100g of solvent

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21
Q

how do you calculate solubility

A

(mass of solid / mass of water removed) x 100

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22
Q

How can you investigate how temperture affects solubility

A
  • weigh empty evaporating basin
  • pour some solution in basin
  • re-weigh basin
  • heat with bunsen burner
  • re-weigh pure substance once water evaportated
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23
Q

define isotope

A

isotopes are different atomic forms of the same element, which have the same number of protons but a different number of neutrons

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24
Q

what does the atomic number of an element tell you

A

how many protons

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25
how can you find out the group number of an element
the number of electrons on the outer shell
26
how can you find out the period of an element
the number of occupied shells
27
what is an element
an element consists of only one atom
28
what is a compound
compounds are chemically boned elements (two or more)
29
what is a mixture
mixtures are easily seperated: there is no chemical bond
30
how can you tell if something is a pure substance
because it will have a speecific, sharp melting and boiling point
31
What is filtration used for
to seperate an insoluable solid from a liquid
32
what is crystallisation used for
to seperate a soluable solid from a solution
33
what do you need to perform filtration
beaker funnel filter paper
34
what is the mixture that stays in the filter paper call
the residue
35
how does crystallisation work
- pour mixture into evapourating dish - heat solution ~ water will evapourate - once water evaporated leave dish to cool and dry
36
why does chromatography work when seperating mixtures
becuase dyes in the mixture move up the paper at different rates
37
how do you preform chromotagraphy
- draw base line wiht pencil - add spots of ink to baseline - loosely roll paper and put in beaker with some water (ensure the baseline is above water level) - once dyes have spread take out to dry
38
how do you calculate the Rf value
distance travelled by solute / distance traveled by solvent
39
when is simple distillation used
to seperate out solutions
40
when is fractional distillation used
to seperate out a mixture of liquids (with similar boiling points)
41
how does simple distillation work
- solution is heated - part of solution with lowest BP evapourates - vapour is cooled and condenses and collected in beaker - rest of solution is left in falsk
42
What do you need to conduct distillation
flask bung thermometer beaker liebig condenser with water jacket bunsun buner tripod
43
what is the relative charge of a proton
+1
44
what is the relative charge of a neutron
0
45
what is the relative charge of an electron
-1
46
What is the relative mass of a proton
1
47
What is the relative mass of a neutron
1
48
What is the relative mass of an electron
0.0005
49
what does the mass number of an element tell you
how many protons and neutrons there are
50
how do you calculate the relative atomic mass of isotopes
((mass number x percentage) + (mass number x percentage)) / 100
51
Why are the elements lower down in the group most reactive
becuase the outermost electron is further from the nucleus so the attraction is less
52
What is a negative ion called
an anion
53
what is a positive ion called
a cation
54
what is an ion
an atom with a charge
55
describe ionic bonding
- metal + non-metal react to get complete outer shell - metal loses electron(s) forming a cation - non-metal gains the electron(s) forming an anion - oppositely charged ions are strongly attracted by ellectrostatic forces causing the bond
56
define ionic bonding
the electrostatic forces of attraction between two oppositely charged ions
57
why do ionic compounds have high MP and BP
becuase the a lot of energy is needed to overcome the strong attraction
58
can ionic compounds conduct electricity
yes but only when molton or dissolved becuase the ions have to be free to maove and carry the charge
59
How are metals held together
by metallic bonding
60
describe a metallic bond
a giant structure of positive metal ions surrounded by a sea of delocalised electrons
61
what does this diagram show
metallic bonding
62
define metallic bonding
the strong electrostatic forces of attraction between metal ions and delocalised electrons
63
why can metals conduct electricity
because the delocalised electrons can move to carry a charge
64
why are metals malleable and ductile
becuase the layers of metal ions can slide as the atoms are all the same size
65
what is the state symbol for solid
(s)
66
what is the state symbol for liquid
(l)
67
what is the state symbol for gas
(g)
68
what is the state symbol for dissolved in water (aqueous)
(aq)
69
what are metal ores
reactive metals found in the earths crust that have enough metal to be extracted from their ore
70
what is the reactivity series
Potassium Sodium Calcium Magnesium Aluminium Carbon Zinc Iron Tin Lead Hydrogen Copper Silver Gold
71
how are metals more reactive than carbon extracted
using electrolysis
72
what is the word equation for rusting
iron + oxygen + water --> hydrated iron(III) oxide
73
What are the the two methods to prevent rusting
barrier methods sacrificial methods
74
What are barrier methods to pevent rusting
painting oiling
75
what are sacrificial methods to prevent rusting
galvanising
76
what is galvanising
when a coating of zinc is sprayed onto an object so that the whole object will not rust
77
define covalent bonding
the electrostatic forces of attraction between the shared pair of electrons and the nuclei of the bonding atoms
78
describe covalent bonding
- non-metals react together to get full outer shell - they share electrons
79
what are intermolecular forces
simple covalent substances have intermoleccular forces, these are the forces between the covalent molecules themselves
80
if a covalent molecule has a high melting point what are the intermolecular forces like
strong
81
if a covalent molecule has a low melting point what are the intermolecular forces like
weak
82
do covalent molecules conduct electricity
no becuase there are no free moving charged particles
83
what are the three most important giant covalent structures
diamond graphite sand
84
what is diamond made up of
carbon
85
what is graphite made up of
carbon
86
what is sand made up of
silicon and oxygen
87
describe graphites intermolecular forces
weak but still present
88
why can you write with graphite
becuase the weak intermolecular forces between the layers
89
Why does graphite have a slippery feel
because weak intermolecular forces hold the layers of carbon atoms together, therefore making the layers able to slide and graphite has delocalised electrons as well so it can conduct
90
why do giant molecular structures have high boiling and melting points
because they require a lot of energy to overcome the strong covalent bonds
91
What is the structure of diamond like
tetrahedral
92
what is the structure of graphite like
hexagonal layers
93
Why is diamond hard
because the tetrahedral stucture allow external forces to be spread throughout the lattice and the forces of attraction are stong so they require a lot of energy to overcome
94
why is graphite soft
because weak forces between layers allow to slide easily
95
why does graphite conduct electricity
there are delocalised electrons between the layers

Chemistry (25 decks)

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