N5 Flashcards
(182 cards)
1
Q
How are elements in the periodic table arranged?
A
In order of increasing atomic number
2
Q
What can the periodic table be used to determine
A
Whether an element is a metal or non metal
3
Q
What does a nucleus contain
A
Contains protons neutrons and electrons that orbit the nucleus
4
Q
Protons charge ?
A
1positive
5
Q
Charge if neutrons?
A
Neutral
6
Q
Electron charge?
A
1 negative
7
Q
What has the approximate mass of 1 atomic mass unit
A
Protons and neutrons
8
Q
How do u know the number of protons given from an atom
A
Is given by the atomic number
9
Q
In a neutral atom the number of electrons is eaqual to the…?
A
Number of protons
10
Q
The mass number of an atom is equal to….?
A
The number of protons added to the number of neutrons
11
Q
What are isotopes defined as
A
Atoms with the same atomic number but differnt mass numbers
12
Q
What is nuclide notation used to show?
A
Atomic number
Mass number
Charge of atoms from which the number of protons electrons and neutrons can be determined
13
Q
How many isotopes do elements normally have
A
1 or 2
14
Q
How was the average atomic mass calculated for each element ?
And what are the values known as
A
By using the mass and proportion of each isotope present
These are known as relative atomic masses
15
Q
What forms between non metal atoms
A
Covalent bonds
16
Q
When do covalent bonds form ?
A
When 2 positive nuclei are held together b their common attraction for a shared pair of elements
17
Q
What are the 7 diatomic elements
A
Hydrogen
Nitrogen
Oxygen
Fluorine
Chlorine
Bromine
Iodine
18
Q
What does the shape of covalent molecules depend on
A
Number of bonds and the orientation of these bonds around the central atom
19
Q
What are the 4 shapes of covalent molecules
A
Linear
Angular
Trigonal pyramidal
Tetrahedral
20
Q
What does more than 1 forming between atoms lead to
A
Double or triple covalent bonds
21
Q
What can covalent substances form?
A
Discrete molecular or giant network structures
22
Q
Covalent molecular substances have strong….?
A
Covalent bonds within the molecules and only weak attractions between the molecules
23
Q
Covalent molecular substances have low….?
A
Melting and boiling points as only weak forces of attraction between the molecules are broken when a substance changes state
24
Q
Covalent molecular substances have a network of……?
A
Strong covalent bonds within one giant structure
25
Covalent molecular substances do not conduct…?
Electricity because they do not have charged particles which are free to move
26
Covalent molecular substances which are…?
Insoluble in water may dissolve in other solvents
27
Covalent network structures have a network of…?
Strong covalent bonds within a giant structure
28
Covalent network structures have very high…?
Melting and boiling points because the network of strong covalent bonds is not easily broken
29
Covalent network structures do not….?
Dissolve in general
30
Covalent network substances do not…?
Conduct electricity this is because they do not have charged particles which are free to move
31
When are ions formed
Ions are formed when when atoms lose or gain electrons to the stable electron arrangement of a noble gas
32
In general metal atoms lose……?
electrons forming positive ions and non metal atoms to gain electrons forming negative ions
33
What are ionic bonds .?
Are the electrostatic attraction between positive and negative ions
34
Ionic compounds form…?
Lattice structures of oppositely charged ions with each a positive ion surrounded by negative ions and each negative ion surrounded with each positive ions
35
Ionic compounds have high…?
Melting and boiling points because strong ionic bonds must be broken in order to break up the lattice
36
Many ionic compounds are..?
Soluble in water
37
What happens as ionic compounds dissolve ?
The lattice structure breaks up allowing water molecules to surround the separated ions
38
Ionic compounds can … only when molten or in solution
Conducts electricity
39
How can conduction be explained in ionic compounds ?
By the movements of ions towards oppositely charged electrodes
40
What are compound names derived from
From the names of the elements from which they are formed
41
What does a compound ending ide mean
It contains 2 elements
42
What does compound ending in ite or ate mean
It has oxygen in it
43
What are group ions ?
Ions containing more than one type of atom
44
What is the mass of a mole in grams equal to
To the gram of formula mass can be calculated using relative atomic masses
45
What is formed when a solute is dissolved in a solvent
A solution
46
What is the ph scale an indication of?
Hydrogen ion concentration and runs from 0-14
47
What does a neutral solution have equal of
H+ and OH- ions
48
What ph is water
Neutral
As it dissociates producing equal concentrations of hydrogen and hydroxide ions at any time
49
The symbol of 2 arrows represents what
That the reaction is reversible and occurs in both directions
50
Acidic solutions have a higher….?
Concentration H+ions than OH-and have ph below 7
51
Alkaline solutions have higher…?
Concentration of OH- ions than H+ ions and have a ph above 7
52
Dilution of an acidic solution with water will…?
Decrease the concentration oh H+ and the ph will increase towards 7
53
Dilution of an alkaline solution with water will …?
Decrease the concentration of OH- and the ph will decrease towards to 7
54
Soluble non metal Oxides will….?
Dissolve in water to forming acidic solutions
55
Soluble metal oxides…?
Dissolve in water to form alkaline solution
56
What neutralises acids
Name some ?
Bases
Metal oxides ,metal hydroxides, metal carbonates
57
What is a neutralisation reaction ?
Which a base reacts with an acid to form water
58
What does the name of a salt produced depend on
On the acid and base used
59
What does hydrochloric acid produce
Chlorides
60
What does sulphuric acid produce
Sulphates
61
What does nitric acid produce
Nitrates
62
What are spectator ions
Ions that remain unchanged by the reaction
63
What can an indicator do at the end of an experiment
Be added to show the result
64
What does titration do
Produce a soluble salt
65
What is used to produce soluble salts
Insoluble metal carbonates and insoluble metal oxides
66
What are reactants
The chemicals you start a reaction with
67
How can you speed up a chemical reaction?
Heating them up
Increasing the surface area
Add a catalyst
Increasing concentration
68
Formula for average rate
/\quantity
—————
/\ time
69
What is an element ?
A substance made up of the same type of atom
70
What is an isotope
Atoms of the same element which have differnt mass snumbers but same atomic number
71
How do elements in groups 1-7 become stable like elements in group 8
By sharing electrons
Transferring electrons
72
Where does ionic Bonding occur
Between non metals and metal
73
Some examples of ionic compounds ?
Sodium chloride
Copper sulphate
Sodium hydroxide
74
What state are ionic compounds at room temperature
Solid
75
Mono means ?
1
76
Di means
2
77
Tri means
3
78
Tetra means?
4
79
Penta means?
5
80
Hexa means
6
81
Hepta means?
7
82
SVISS how to produce an ionic formula ?
(S)ymbols down
(V)alency under symbol
(I)nclude charge
(S)wap valency
(S)implify valency if possible
83
Name some common acids
Hydrochloric acid
Sulfuric acid
Nitric acid
84
Formula for hydrochloric acid ?
HCL
(H+Cl-)
85
Formula for sulfuric acid
H2SO4
((H+)2SO2-4)
86
Formula for nitric acid
HNO3
(H+NO3-)
87
Name some common bases
Sodium hydroxide
Potassium hydroxide
Sodium carbonate
88
Formula for sodium hydroxide
NaOH
(Na+OH-)
89
Formula for potassium hydroxide
KOH
(K+OH-)
90
Formula for sodium carbonate
Na2Co3
((Na+)2Co2-3
91
Word equation for how to make a base
Metal oxide +water ->metal hydroxide
92
Word equation for how to make an acid
Non metal oxide + water -> acid
93
What is metallic bonding
Electrostatic attraction between 2 positively charged ions and delocalised electrons
94
Why are metallic elements conductors
They contain delocalised electrons
95
What can metals be used to produce
Soluble salts
96
What is reduction in metals
A gain of electrons in a reactant in any reaction
97
what is oxidation in metals
A loss of electrons by a reactant in any reaction
98
What happens in a redox reaction
Reduction and oxidation takes place at the same time
99
What happens during the extraction of metals
Metal ions are reduced forming metal atoms
100
What are the methods to remove a metal from an ore
Heat alone
Electrolysis
heat + C/CO
101
What is electrolysis
The decomposition of the ionic compound into its elements using electricity
102
What happens to ions in electrolysis
Positive ions gain electrons at the negative electrode and negative ions lose electrons at the positive electrode
103
What are electrolytes
Solutions that conduct electricity containing ions
104
How can a simple cell be made
By placing 2 metals in an electrolyte
105
What does growing plants require
Nutrients
106
What must a fertiliser contain to be effective
Nitrogen
Phosphorus
Potassium
107
What are fertilisers
Substances which restore elements , essential for healthy plant growth
108
What are ammonia and nitric acid important for
To produce soluble nitrogen contains salts (fertilisers)
109
Describe ammonia
Pungent clear colourless gas which dissolves in water
110
What happens if u dissolve ammonia in water
It produces an alkaline solution
111
What is the Haber process
Production of ammonia required for fertiliser production
112
What is the catalyst used in the haber process
Iron
113
What is the starting material for the production of nitric acid
Ammonia
114
What does the Ostwald process use
Ammonia
Oxygen
Water
115
What is the catalyst used in the Ostwald process
Platinum
116
What does radioactive decay involve
Changes in nuclei of atoms
117
How can radioisotopes become more stable
By giving out alpha, beta or gamma radiation
118
Alpha particles consist of?
2 protons and 2 neutrons and carry. A double positive charge
119
What stops alpha radiation
A piece of paper
120
Alpha particles will be attracted towards…..
Negatively charged plates
121
What are beta particles
Electrons ejected from the nucleus of an atom
122
What stops beta rays of radiation
A thin sheet of aluminium
123
Beta particles are attracted to…..
Towards a positively charged plate
124
What are gamma rays
waves emitted from within the nucleus of an atom
125
What can stop gamma rays
Barriers like lead or concrete
126
Gamma rays are not….
Deflected by an electric field
127
What are the 3 radiation types
Gamma alpha beta
128
How can an alpha particle be represented
4
He
2
129
How can a beta particle be represented
0
e
-1
130
How can proton be represented
1
P
1
131
How can a neutron be represented
1
n
0
132
What is a half life
The time for half of the nuclei of a particular isotope to decay
133
The half life of an isoptope is a constant
What does this mean?
It is unaffected by chemical or physical conditions
134
What can be used to date materials
Radioactive isotopes
135
How do you determine a half life of an isotope
For a. Graph showing a decay curve
136
what has a range of uses in medicine and in industry
radioisotopes
137
what are plastics
materials known as polymers
138
what are polymers
a long chain of molecules formed by joining together a large number of small molecules called monomers
139
what does unsaturated mean
that there's a double bond
140
what is the name given to a chemical reaction in which unsaturated monomers are joined, forming a polymer
addition polymerisation
141
what is a reapeating unit
the shortest section of polymer chain which, if repeated, would yield the complete structure of a polymer
142
what is a homologous series
a family of compounds with the same general formula and similar chemical properties
143
the subsequent members of homologous series show a....
general increase in their melting and boiling points
144
what is the pattern attributed to
increasing strength of the intermolecular forces as the molecular size increases
145
what are hydrocarbons
compounds containing only hydrogen and carbon atoms
146
what does saturated mean
compounds containing only single carbon-carbon bonds
147
what does unsaturated mean
compounds contaning at least 1 carbon-carbon double bond
148
how do you disdinguish unsaturated compound from a saturated one
with bromine solution
149
what happens when you add bromine solution to an unsaturated compound
it decolourises it
150
what are isomers
compounds with the same molecular formula but different structural formula
151
isomers may belong to ......
different homologous series
152
isomers usually have different....
physical properties
153
what are alkanes
homologous series of unsaturated hydrocarbons
154
what is a use of alkanes
fuels
155
what happens to an alkane in water
nothing , its insoluble
156
what is the general formula for alkane
CnH2n+2
157
what are cycloalkanes
a homologous series of saturated , cyclic hydrocarbons
158
what are cycloalkane uses
fuels and solvents
159
what is the general formula for cycloalkanes
CnH2n
160
what are alkenes
homologous series of unsaturated hydrocarbons
161
what are the functions of alkenes
made to make polymers and alcohols
162
what is the alkenes functional group
the c=c double bond group
163
what is the general formula for alkenes
CnH2n
164
what are the addition reactions
hydrogen forming alkanes - hydrogenation
halogens forming dihhaloalkanes
water forming alcohols - hydration
165
what are some functions of alcohols
fuels
solvents
perfumes
166
methanol, ethanol and propanol are miscible in water this means .....
the solubility decreases as size increases
167
as alcohols increase in their melting and boiling points increase due to?
increasing strength of the intermolecular forces
168
what is an alcohol
a molecule containing a hydroxyl functional group - OH group
169
what is the general formula for alcohols
CnH2n+1OH
170
how are carboxylic acids used
in the preparation of soaps and preservatives and medicines
171
what is vinegar
and what is its formula
a solution of ethanoic acid with molecular formula - CH3COOH
172
what is vinegar used for and in
in household cleaning products as it is non toxic
173
methanoic , ethanoic and propanoic and butanoic acid are miscible in water this means?
the solubility decreases as size increases
174
a carboxylic acid increase in size their melting and boiling points increase due to?
the increasing strength of the intermolecular forces
175
what functional group are carboxylic acids in
carboxyl group - COOH
176
whta is the general formula for carboxylic acids
CnH2n+1COOH
177
carboxylic acids can form ....
salts
178
exothermic
a process that releases heat energy
179
endothermic
reaction that takes in heat energy
180
what is combustion
when a substance reacts with oxygen releasing energy
181
what does hydrocarbons and alchohauls burning with plentiful oxygen produce
CO2 and water
182
what happens when fuels burn
they release diffrent quantities of energy
