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Module 2 Chemistry > 2.1 > Flashcards

2.1 Flashcards

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1
Q

Democritus

A

1st theory- divide a sample of matter only a certain amount of times, then it wouldn’t spilt any further

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2
Q

Dalton

A

2nd theory- atoms are tiny particles that make up elements and atoms cannot be divided
all atoms of a given element are the same, atoms of 1 element are different to every other element

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3
Q

J J Thomson

A

3rd theory (discovered cathode rays (electrons))
-electrons were negative charge and were a stream of particles
-they could be deflected by magnet and electric fields

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4
Q

J J Thomson’s model

A

Plum pudding and showed negative electrons around a sea of positive charge so overall charge of atom is equal

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5
Q

Rutherford’s Gold foil experiment 1911

A

directed alpha particles at thin gold foil, thought because of plum pudding, no alpha deflected

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6
Q

Results to Gold Fold experiment

A

-most weren’t deflected
-small percentage were
-very small value deflected back towards source

This showed there was a nucleus in centre, positive charge and electrons orbited around nucleus. Overall charge must be balanced

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7
Q

Niels Bohr discovery

A

Found electrons must orbit in certain paths otherwise they would spiral into nucleus

This helped to explain periodic properties such as, the energy of electrons is different distances from the nucleus

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8
Q

1918

A

Proton discovered

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9
Q

1932 James Chadwick

A

Neutron discovered

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10
Q

Protons and neutrons can be broken down into…

A

quarks

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11
Q

isotope

A

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

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12
Q

why don’t diff isotopes of the same element react diff

A

as electrons are involved in chemical reactions not neutrons

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13
Q

relative atomic mass

A

the weighted mean mass of an atom of an element, compared with 1/12th of the mass of the atom of carbon-12

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14
Q

relative molecular mass

A

the weighted mean mass of a molecule, compared with 1/12th of the mass of an atom of carbon-12

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15
Q

relative isotopic mass

A

the mass of one atom of an isotope compared with 1/12th of the mass of an atom of carbon-12

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16
Q

relative formula mass

A

the weighted mean mass of a formula unit of a substance compared with 1/12th of the mass of an atom of carbom-12

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17
Q

metals (group 1-13) do they lose/gain

A

lose electrons — positive ion

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18
Q

non-metals (group 15-17) do they lose/gain

A

gain electrons —- negative ions

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19
Q

Be B Si and C all have what in common

A

none of them can form ion as it would require too much energy to transfer outer shell electrons

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20
Q

ionic formula overall charge

A

zero as +ions and -ions have to be balanced

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21
Q

amount of substance

A

the quantity that has moles as its units, used as a way to calculate atoms

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22
Q

mole

A

the amount of substance containing as many particles as there were carbon atoms in 12g of the carbon-12 isotope

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23
Q

molar mass

A

mass per mole of a substance in gmol-1

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24
Q

avogardo constant defintion

A

the number of atoms per mole of the carbon-12 isotope

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25
empirical formula
simplest way of showing a chemical formula
26
molecular formula
not simplified formula, shows all the atoms that make up a molecule
27
standard concentration
has a known concentration
28
concentrated
large amount of solute per dm3
29
dilute
small amount of solute per dm3
30
percentage yield
actual amount in moles of product divided by theorical amount in moles of product x100
31
atom economy
mr of the desired product divided by the sum of mr of all products x100
32
what reactions have 100% atom economy
addition reactions
33
what reactions have less than 100% atom economy
reactions involving substitution or elimination For us to use these types of reactions we need to find uses for all the products of the reaction
34
acid reacting with water
acid releases H+ ions and rest of atoms in acids make -ion
35
stronger acids
strong acids fully dissociate and easily gives up H+ ions
36
weaker acids
not good at giving up H+ ions and, and only partly dissociate. When they give away H+ ions they are quickly taken back
37
common bases
metal oxides and metal hydroxides
38
base
a proton H+ acceptor so neutralises acids
39
acids
proton donor and releases H+ ions into a water
40
alkalis
release OH- ions when dissolved in water
41
acid and alkali reaction
OH- ions neutralise the protons from acid to form water OH- (aq) + H+ (aq) = H2O (l)
42
how we know if its a weak alkali
only a small proportion of dissolved alkali reacts with water- doesn't release many OH- ions
43
when equilibrum sign used in water and alkali reaction
shows weak alkali as reaction can go either way
44
amphoteric substances
substances that can behave as acids and bases eg. glycine as it contains COOH group (which will donate a proton) and NH2 group (will accept a proton)
45
salt is an ionic compound with...
+ion (metal ion) and -ion (from acid) Formula of salt is same as acid expect it can be any +ion
46
acids reacting with carbonates
produces salt, C02 and H20 see bubbles of CO2 carbonates solid form in reaction
47
acids reacting with metal oxide
salt and water formed metal oxides are solid
48
acids and alkali
both aq salt and water formed
49
acids and metals
metals are aq salt and hydrogen gas formed REDOX REACTION
50
ammonia nitrate solution
found as two ions NH4+ NO3-
51
hydrated solution
the crystalline form containing water
52
Anhydrous
the form containing no water
53
water of crystallisation
refers to water molecules that form an essential part of the crystalline structure of a compound if a compound crystalises in water, it becomes part of the crystalline structure
54
CuSO4 . 5H20 what does the dot show?
dot acts as ratio, showing how many compound molecules to water molecules within a crystalline structure The 5 is used within a formula
55
in titration calculations you may be asked to find the ...
-concentration of solution - molar mass -formula -the number of molecules of water of crystallisation
56
how to carry out a titration experiment
1. using a pipette, add a measured volume of one solution (acid) to a conical flask 2. Add a suitable indicator 3. Place the other solution (alkali) to burette 4. Then slowly add alkali into conical flask flask until the reaction has just been completed This is the end point 5. Measure the volume of alkali added from the burette Now know the volume of one acid that exactly reacts with the volume of one alkali You can have acid in burette as well but less common and results in different colour changes if using phenolphthalein
57
Identify end point in titration using indicator, what colours for methyl orange
Methyl orange - acid- red -alkali (base)- yellow -end point- orange
58
Identify end point in titration using indicator, what colours for Bromothymol blue
acid-yellow alkali- blue end point- green
59
Identify end point in titration using indicator, what colours for phenolphthalein
acid- colourless alkali- pink endpoint- pale pink However if you added the acid by the burette and alkali was in conical flask then the end point would be colourless
60
what are oxidation numbers used for
keep track of how electrons are being used in bonding
61
what is an oxidations numbers
the number of electrons that an atom uses to bond with atoms of another element
62
uncombined elements oxidation number Just made up of one element eg. C or O2
zero as only one element
63
If oxygen is combined with other elements, oxidation number?
-2 Except if a peroxide, eg: H2O2 then Oxygen = -1 Peroxide = any of a class of chemical compounds in which two oxygen atoms are linked together by a single covalent bond
64
If hydrogen is combined with other elements, oxidation number ?
+1 Except if combined with metal hydrides then hydrogen = -1 Metal Hydrides= metals which have been bonded to hydrogen eg. LiH
65
if fluorine is combined with other elements, oxidation number?
-1
66
what happens to the oxidation numbers when fluorine bonds with oxygen
fluorine remains -1 oxygen becomes +2
67
Groups 1,2,3 oxidation numbers if in combined with other elements
+1,+2,+3
68
what is chlorines oxidation number if combined with other elements
-1
69
the sum of oxidation numbers is compounds must equal?
zero
70
the sum of oxidation numbers in molecular ions must equal?
the charge of the ion
71
TRUE/ FALSE transition metals form ions with different oxidation numbers
true
72
FeCl2 oxidation number of Fe
+2
73
FeCl3 oxidation number of Fe
+3
74
Cu2O oxidation number of Cu
+1
75
CuO oxidation number of Cu
+2
76
Oxyanions
negative ions that contain an element as well as oxygen
77
TRUE/FLASE Element forms oxyanions and then has different oxidation numbers?
true
78
NO2- oxidation number of N
+3
79
NO3- oxidation number of N
+5
80
SO3^2- oxidation number of S
+4
81
SO4^-2 oxidation number of S
+6
82
Oxidation and Reduction
OIL RIG
83
oxidation
loss of electrons, gain of oxygen
84
reduction
gain of electrons, loss of oxygen
85
half equations for oxidation
start with element then after arrow have ion and electrons- Mg arrow Mg2+ + 2e-
86
half equations for reduction
start with element and electrons- then after arrow put ions you produced Cl2 + 2e- arrow 2Cl2-
87
metals and non-metals oxidised and reduced
metals tend to be oxidised non-metals tend to be reduced
88
reduction with oxidation number
decreases number
89
oxidation with oxidation number
increase number
90
metal and acid redox reactions which is red and oxd
reduction-hydrogen in acid (this forms H2 gas product) oxidised- metal
91
concentration of solution
amount of solute dissolved in a given amount of solvent
92
in titration fill up to...
meniscus
93
titration flask used...
volumetric flask
94
How to make a standard solution
1. weigh out the solute 2. completely dissolve the solute in solvent in a beaker 3. transfer the solution to a volumetric flask and rinse the beaker using more solvent and add rinsing's to flask 4. add more solvent carefully to bottom of the meniscus. may need to use drop by drop method to get exact measure on meniscus 5. mix solution several times by inverting flask several times

Module 2 Chemistry (1 decks)

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