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Chemistry > C1-5 Revision > Flashcards

C1-5 Revision Flashcards

1
Q

Aquaeous solution

A

Mixture made by adding a soluble substance to water

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2
Q

Atom

A

the smallest part of an element that can still be recognised as that element

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3
Q

Atomic number

A

the number of protons (which equals the number of electrons) in an atom. It is sometimes called the proton number

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4
Q

Balanced symbol equation

A

a symbol equation in which there are equal numbers of each type of atom on either side of the equation

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5
Q

Biofuel

A

Fuel made from animal or plant products

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6
Q

Chromatography

A

the process whereby small amounts of dissolved substances are separated by running a solvent
along a material such as absorbent paper

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7
Q

Compound

A

substance made when two or more elements are chemically bonded together

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8
Q

Electron

A

tiny particle with a negative charge. Electrons orbit the nucleus of atoms or ions in shells

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9
Q

Electronic structure

A

set of numbers to show the arrangement of electrons in their shells (or energy levels)

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10
Q

Element

A

substance made up of only one type of atom. An element cannot be broken down chemically into any
simpler substance

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11
Q

Group

A

All the elements in the columns (labelled 1 to 7 and 0) in the periodic table

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12
Q

Ion

A

a charged particle produced by the loss or gain of electrons

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13
Q

Isotope

A

atoms that have the same number of protons but different number of neutrons, i.e., they have the same atomic
number but different mass numbers

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14
Q

Law of conservation of mass

A

the total mass of the products formed in a reaction is equal to the total mass of the reactants

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15
Q

Mass number

A

the number of protons plus neutrons in the nucleus of an atom

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16
Q

Neutron

A

A dense particle found in the nucleus of an atom. It is electrically neutral, carrying no charge

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17
Q

Noble gases

A

the very unreactive gases found in Group 0 of the periodic table. Their atoms have very stable electronic structures

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18
Q

Nucleus (of an atom)

A

the very unreactive gases found in Group 0 of the periodic table. Their atoms have very stable electronic structures, radius of nucleus 1/10,000 that of an atom

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19
Q

Periodic table

A

an arrangement of elements in the order of their atomic numbers, forming groups and periods

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20
Q

Product

A

A substance made as a result of a chemical reaction

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21
Q

Proton

A

A tiny positive particle found inside the nucleus of an atom

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22
Q

Reactant

A

a substance we start with before a chemical reaction takes place

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23
Q

Shell

A

an area in an atom, around its nucleus, where electrons are found

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24
Q

State symbol

A

the abbreviations used in balanced symbol equations to show if reactants and products are solid (s), liquid (l), gas
(g) or dissolved in water (aq)

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25
Symbol equation
an equation that helps you see how much of each substance is involved in a chemical reaction by showing the chemical symbols and formulae of all the reactants and products involved
26
Word equation
way of describing what happens in a chemical reaction by showing the names of all reactants and the products they form
27
Alkali metal
elements in Group 1 of the periodic table
28
Halogens
The elements found in Group 7 of the periodic table
29
Universal indicator
mixture of indicators that can change through a range of colours to show how strongly acidic or alkaline liquids and solutions are
30
Alloy
a mixture of two or more elements, at least one of which is a metal
31
Covalent bond
the bond between two atoms that share one or more pairs of electrons
32
Covalent bonding
the attraction between two atoms that share one or more pairs of electrons (non-metals)
33
Delocalised electron
bonding electron that is no longer associated with any one particular atom
34
Dot and cross diagram
a drawing to show only the arrangement of outer shell electrons of the atoms or ions in a substance
35
Fullerene
form of the element carbon that can exist as large cage-like structures, based on hexagonal rings of carbon atoms
36
Gases
substances that have no fixed shape or volume and can be compressed easily
37
Giant covalent structure
A huge 3D network of covalently bonded atoms
38
Giant lattice
a huge 3D network of atoms or ions
39
Giant structure
A huge 3D network of atoms or ions
40
Intermolecular force
the attraction between the individual molecules in a covalently bonded substance
41
Ionic bond
the electrostatic force of attraction between positively and negatively charged ions
42
Liquids
substances that have a fixed volume, but they can flow and change their shape
43
Particle theory
a theory that explains the properties of solids, liquids and gases based on the fact that all matter is made from tiny particles. It describes the movement of particles and the distance between them
44
Polymer
A substance made from very large molecules made up of many repeating units
45
Solids
substances that have a fixed shape and volume that cannot be compressed
46
States of matter
the forms in which matter can exist. A substance can be solid, liquid or gas
47
Avogadro constant
the number of atoms, molecules, or ions in a mole of any substance (i.e., 6.02 × 10 -23 per mol)
48
Concentration
the amount of a substance dissolved in a given volume of liquid
49
Limiting reactant
the reactant in a chemical reaction that when used up causes the reaction to stop
50
Mole
the amount of substance in the relative atomic or formula mass of a substance in grams
51
relative atomic mass Ar
the average mass of the atoms of an element compared with carbon-12 (which is given a mass of exactly 12). The average mass must take into account the proportions of the naturally occurring isotopes of the element
52
Relative formula mass Mr
the total of the relative atomic masses, added up in the ratio shown in the chemical formula, of a substance
53
Acid
when dissolved in water, its solution has a pH value less than 7. Acids are proton (H + ion) donors
54
Alkali
its solution has a pH value more than 7
55
Base
the oxide, hydroxide, or carbonate of a metal that will react with an acid, forming a salt as one of the products. (If a base dissolves in water it is called an alkali). Bases are proton (H+ ion) acceptors Accepts hydrogen ions when dissolved in water Bases: Metal oxide Metal carbonate Metal hyroxide=alkalis-dissolve in water All alkalis are bases but not all bases are alkalis Ammonia=alkalis-dissolve in water
56
Displacement reaction
a reaction in which a more reactive element takes the place of a less reactive element in one of its compounds or in solution
57
Electrolysis
the breakdown of a substance containing ions by electricity
58
Equilibrium
the point in a reversible reaction at which the forward and backward rates of reaction are the same. Therefore, the amounts of substances present in the reacting mixture remain constant
59
Half equation
an equation that describes reduction (gain of electrons) or oxidation (loss of electrons)
60
Ionic equation
an equation that shows only those ions or atoms that change in a chemical reaction
61
Metal ore
a rock that contains enough of a metal or metal compound that it is worth extracting the metal
62
Neutral
a solution with a pH value of 7 which is neither acidic nor alkaline. Alternatively, something that carries no overall electrical charge
63
Neutralisation
the chemical reaction of an acid with a base in which a salt and water are formed. If the base is a carbonate or hydrogen carbonate, carbon dioxide is also produced in the reaction
64
Ore
rock which contains enough metal to make it economically worthwhile to extract the metal
65
Oxidation/oxidised
a reaction where oxygen is added to a substance / or when electrons are lost from a substance
66
pH/pH scale
a number which shows how strongly acidic or alkaline a solution is
67
Reactivity series
a list of elements in order of their reactivity
68
Reduction/redused
A reaction in which oxygen is removed or electrons are gained
69
Salt
a compound formed when some or all of the hydrogen in an acid is replaced by a metal
70
Strong acids
these acids completely ionise in aqueous solutions
71
Weak acids
acids that do not ionise completely in aqueous solutions
72
Molecules
Small groups of atoms that are covalently bonded
73
Noble gases=unreactive coz
Do not easily form molecules coz atoms stable arrangements of electrons
74
Polyatomic elements
Consisting multiple atoms chemically bonded e.g. sulphur and phosphorus
75
Diatomic elements
Consisting of 2 atoms chemically bonded
76
Monoatomic elements
Noble gases (single atoms)
77
Ionic bonding
Electrostatic attraction between oppositely charged ions (metal+non-metal)
78
Current
Flow of charges
79
Charges
Ions or electrons
80
Do ionic solids conduct electricity
No because ions are not free to flow and are held in rigid lattice only in water or when melted
81
Can metals conduct electricity
Yes because delocalised electrons are free to flow in metal
82
Dative covalent bond
Only one of the atom contributes all of the electrons
83
Metallic bond
Electrostatic attraction between delocalised electrons and positive nucleus within a pure metal
84
Molecular formula
Show actual amount of atoms in a molecule
85
Empirical formula
Shows the simplest ratio of atoms which make up a molecule
86
Moles
Mass/relative formula mass AND concentration (mol/dm3)*volume(cm3/ml/dm3)
87
Concentration(g/dm3)
Mass(g)/volume(dm3) AND amount of solute(g)/volume of solution(dm3)
88
Idm3
1000cm3 and 1000ml
89
Percentage yield
Real yield ------------ *100 Theoretical
90
Ionic properties
High melting and boiling point, doesn't conduct as a solid, conducts in a liquid, solution doesn't conduct
91
Simple molecular properties
Low melting and boiling point, doesn't conduct electricity and solution insoluble
92
Giant covalent bond properties
Very high melting and boiling point, doesn't conduct and isn't soluble
93
Metallic properties
High melting and boiling point, conducts in a states and insolubsle
94
Concentrated=
Large amount of dissolved, high concentration hydrogen ions
95
Dilute acids=
Small amount dissolved, low concentration hydrogen ions
96
Weak acids=
Only partially ionise/dissociate
97
Strong acids
Fully ionise/dissociate
98
Difference between bases and alkalis
All alkalis are bases but not all bases are alkalis Alkalis:metal hydroxide, ammonia NH3 Bases:metal carbonate, metal oxide
99
Why percentage yield is not 100%
Errors or spills Incomplete reaction Un desirable side effects
100
Metal+acid->
Salt+hydrogen
101
Metal oxide+acid->
Salt+water
102
Metal hydroxide+acid->
Salt+water
103
Metal carbonate+acid
Salt+water+carbon dioxide
104
Acid+base->
Water+salt (apart from ammonia which just =a salt)
105
``` Common acids HCI(aq)-> H2SO4(aq)-> HNO3(aq)-> H3PO4(aq)-> CH3COOH(aq)-> ```
``` Dissociate (split up) [H]+[Cl]- chloride 2[H]+[SO4]2- Sulphate [H]+[NO3]- Nitrate 3[H]+[PO]3- Phosphate [H]+[CH3COO]- Ethanoate Acids release hydrogen ions (proton) when dissolved The 'ate' is in the acid with oxygen ```
106
Electrons:OILRIG
Oxidation Is Loss Reduction Is Gain

Chemistry (7 decks)

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