C1 - Atomic Structure Flashcards
1
Q
The history of the periodic table
True or false: Dalton was the earliest contributor to the periodic table and published a list of elements
A
True
2
Q
The history of the periodic table
What were Dobereiners triads?
A
Elements with similar chemical properties that were in groups of three
For example: lithium sodium and potassium due to similar reactions with water
3
Q
The history of the periodic table
How did Newlands arrange the periodic table?
A
Arranged elements in and sort every eighth element reacts in a similar way
4
Q
The history of the periodic table
What did Newlands call the fact that every eighth element in his table reacted the same way?
A
Law of Octaves
5
Q
The history of the periodic table
True or false, both Newlands and Dobereiners collected, lithium, sodium, and potassium together
A
True
6
Q
The history of the periodic table
What was the problem with the law of octaves?
A
 Some elements were grouped which had completely different properties (this was because they were ordered only increasing atomic weight)
7
Q
The history of the periodic table
How did Dmitri Mendeleyev order the periodic table?
Give three things that he did correctly
A
He switched the order of elements to fit patterns of chemical properties already in the table.
He arranged elements in increasing atomic weight.
He also left gaps in the periodic table.
8
Q
The history of the periodic table
Why did Dmitri Mendeleyev leave gaps in his periodic table?
A
He predicted the properties of elements in the gaps through their position on the table. This was good as these elements were later discovered to be correct by modern scientists. This is the main reason why his table is accepted today.
9
Q
The history of the periodic table
What were the two problems with Dmitri Mendeleev’s periodic table
A
Protons had not been discovered yet, so he ordered elements by atomic weight, which meant due to the presence of isotopes he put some elements in the wrong order
he didn’t have noble gases.
10
Q
The history of the periodic table
How do we arrange the periodic table now?
give three details
A
We arrange periodic table by increasing number of protons (atomic number).
We have groups.
We have periods.
11
Q
Atoms
What is an atom?
A
The simplest form of matter in chemistry
12
Q
Atoms
What three subatomic particles in an atom made of, and what are their charges masses and place in the atom
A
Proton neutron electron
+1, 0, -1
One, one, zero
Nucleus, nucleus, electron shells
13
Q
Atoms
In what order are electron shells filled and how many electrons fill each shell?
A
Lowest to highest energy state
2, 8, 8
14
Q
Atoms
What is a compound
A
A substance of two or more different elements, chemically bonded
15
Q
Atoms
What is an element?
A
A pure substance made from one type of atom
16
Q
Atoms
What does the group number represent in the periodic table?
A
The number of electrons in the outer shell
17
Q
Atoms
Which way do groups go from top to bottom?
A
Up down
18
Q
Atoms
What does the period number represent in the periodic table?
A
The number of electron shells
19
Q
Atoms
True or false elements in the same period have similar chemical properties
A
True
20
Q
Atoms
as you increase period number, what also increases
A
Reactivity
21
Q
Atoms
Are periods, rows or columns
A
Rows
22
Q
Atoms
What is the mass number represent in the periodic table
A
Protons, plus neutrons
23
Q
Atoms
What is the atomic number represent in the periodic table?
A
Number of protons, all the number of electrons
24
Q
Atoms
How many elements are there?
A
110
25
Atoms
Elements are arranged in increasing _____
Atomic number
26
Atoms
Do elements have an overall charge
No
27
Atoms
What is a mixture?
Two or more different substances not chemically bonded together that can be separated by physical process
28
History of the atomic model
Who is the author of the plum pudding model?
Thompson (1897)
29
History of the atomic model
What does the plum pudding model Describe?
A cloud of positive charge with negative electrons in embedded within
The negative electrons, the plums in the positive pudding
30
History of the atomic model
Did Thomsons model include the electron?
Yes
31
History of the atomic model
Did Thomsons model predict that the atom was solid?
No
32
History of the atomic model
Who was the author of the nuclear model?
Rutherford
33
History of the atomic model
What was Rutherford’s experiment in 1909?
He fired alpha particles at a very thin (a few atoms thick) piece of gold foil suspended in a vacuum
Some particles were deflected by large angles and some went straight through the foil and some were deflected 180 degrees
Deflection showed positive nucleus
Most straight through = mostly empty space
Small number coming straight back = centre of mass (nucleus) is in nucleus and the nucleus is very small!
34
History of the atomic model
What did Niels Bohr contribute to the model of the atom?
In 1915 he describes the fact that electrons orbit the nucleus at specific distances - in electron shells
35
History of the atomic model
Who discovered the modern nuclear model?
Chadwick in the 1920s
36
History of the atomic model
What did James Chadwick prove?
The existence of neutrons
37
History of the atomic model
What was the earliest of the atom and who authored it?
The bowling ball model, which proposed that the atom was a solid indivisible sphere
Dalton 1803
38
Isotopes
What is an isotope?
Atoms of the same element, but a different number of neutrons
39
Isotopes
What are the similarities and differences between two isotopes?
Proton/electron number/atomic number is the same
Number of neutrons is different
Remember in an exam always to give the number of neutrons in an isotope and name it using the full symbol (periodic symbol + mass number + atomic number)
40
Isotopes
What is relative atomic mass?
The average value that takes account of the abundance of isotopes of an element
41
Isotopes
How do you calculate relative atomic mass?
The sum of isotope abundances times isotopes mass number divided by the sum of the isotope abundances
Abundance is given as a percentage or ratio
42
Separating methods
What is distillation used for
Separating a mixture of two or more different liquids which have two or more different boiling points (fractional)
Of separating a liquid from a solution with a solid solute in it
43
Separating methods
What is the difference between fractional distillation and simple distillation?
Fractional distillation separates multiple (more than or equal to 2) different liquids with multiple (more than or equal to 2) different boiling points
Whereas simple distillation separate a solvent from a solute in a solution
44
Separating methods
Briefly describe the process of distillation
Heat, a mixture of solvents.
One will evaporate off into a Liebig condenser leaving behind the other solvent
This condenser cools the solvent and it drips into the conical flask
45
Separating methods
What is crystallisation?
The separation of a solute from a solvent to form crystals
46
Separating methods
Briefly describe the process of crystallisation
Evaporate the solution into a smaller volume and let it cool
As the solution cools crystals will form which can be obtained by filtration
47
Separating methods
What does filtration separate?
An insoluble solid from a liquid
48
Separating methods
Briefly describe the process of filtration
A mixture of solid and liquid or poured into the filter funnel and liquid drips through the filter paper, but solid particles are caught by the paper and separated
49
Separating methods
What does chromatography separate?
Mixtures of coloured compounds
Usually pen ink or food colouring agents
50
Separating methods
Briefly describe the process of chromatography
Spots of ink are placed on a pencil line. Paper is lowered into water below the pencil line and dye spreads up the paper.
Ink is separated into its colours forming a chromatogram.
51
Separating methods
What is a paper with separated chromatography inks called?
A chromatogram
52
Separating methods
The further up the paper a colour travels the more soluble/insoluble it is
Soluble
53
Separating methods
How could you increase the accuracy of a chromatography experiment?
 Put a lid on the beaker, prevent the liquid evaporating off
If it did not have a lid this would give the wrong RF value as the solvent wouldn’t travel high up enough the page
54
Separating methods
What is an RF value and how is it calculated?
It’s called the retardation factor
It is calculated by the distance, moved by the compound divided by the distance moved by the solvent
In this case, it’s the distance moved by the colour divided by the distance moved by water
55
Separating mixtures
What is a solution?
When is solute is dissolved in a solvent
56
Separating mixtures
What is a solvent?
A liquid substance, which may be mixed with a solute to make a solution
57
Separating mixtures
What does insoluble mean?
The solute can’t be dissolved in a solvent
58
Separating mixtures
What is a solute?
A solid substance which may be dissolved into the solvent to form a solution
59
Separating mixtures
What does soluble mean?
A solute that can dissolve with a solvent
60
Separating mixtures
What is a mixture?
Different substances, not chemically joined 
61
Why did Rutherford do his experiment in a vacuum?
So that any deflections were due to the gold foil and nothing else
62
Why was gold used by Rutherford in his experiments on the atom?
It was the only metal that could be rolled out very thin without cracking
63
Give all the diatomic elements and a way to remember them
Hydrogen
Nitrogen
Fluorine
Oxygen
Iodine
Chlorine
Bromine
Have no fear of ice cold beer!
64
True or false: elements in a compound are in fixed proportions
True
65
What is the chemical formula for magnesium oxide?
MgO
66
What is the chemical formula of sodium chloride
NaCl
67
What is the chemical formula of potassium bromide?
KBr
68
What is the formula for magnesium iodide?
MgI2
69
What is the formula for carbon monoxide?
CO
70
What is the Cornu,a for sulfur trioxide?
SO3
71
What is the formula for ammonia?
NH3
72
What is the formula for methane>
CH4
73
What is an ion?
A charged particle formed when an atom loses or gains electrons
74
What is the formula of a sodium ion?
Na+
75
What is the formula of a magnesium ion?
Mg2+
76
What is the formula of a chloride ion?
Cl-
Remember it is CHLORIDE when an ion and only chlorine as a normal element diatomic
77
What is the formula of an oxygen ion?
O2-
78
What is the formula of sodium oxide?
NaO2
79
What is the formula of magnesium chloride?
MgCl2
80
What does the state symbol (aq) mean?
Aqueous solution
81
What is the law of the conservation of mass?
No atoms are lost or made during a chemical reaction
(Total mass of products = total mass of reactants)
82
What is an element?
A substance made up of one atom only
83
What is a molecule?
A collection of two or more atoms held together by chemical bonds
84
Bitesize
What is filtration used to separate?
Separates an insoluble solid from a liquid
85
Bitesize
Give two examples where filtration is useful
Mix of sand and water
Excess reactant from mixture
86
Bitesize
How does filtration paper work?
It has tiny pores which let small molecules through but not larger in dissolved particles
87
Bitesize
Give 3 pieces of equipment needed for filtration
Filter paper
Filter funnel
Beakers
88
Bitesize
What does crystallisation produce?
Solid crystals from a solution
89
Bitesize
Give an example of what crystallisation is used for:
Getting copper sulfate crystals from a copper sulfate solution
90
Bitesize
Give 3 bits of equipment needed for crystallisation
Evaporating basin
Bunsen burner
Tripod
91
Bitesize
Describe the process of crystallisation:
Heat evaporates most of solvent
Leave the rest to evaporate over time leaving larger crystals
92
Bitesize
How do you make big crystals?
Heat over a boiling water bath instead of
93
Bitesize
What is simple distillation?
Separation of a solvent from a solution
94
Bitesize
Give an example of something simple distillation is useful for
Producing pure water from seawater
95
Bitesize
How does simple distillation work?
The dissolved solute has a much higher boiling point than the solvent
So when heated only the solvent vaporises off and can be moved away
96
Bitesize
Give 4 pieces of equipment needed for simple distillation
Leibig condenser/condensing tube
Beaker
Bunsen burner
Conical flask with bung
97
Bitesize
What is fractional distillation?
Separated different liquids from a mixture of liquids
98
Bitesize g
Give 2 examples of uses of fractional distillation
Separating ethanol from ethanol and water mixture
Separating fractions from crude oil
99
Bitesize
Describe the process of fractional distillation:
Gas rises through a column which has a temperature gradient (cooler at top, hotter at bottom)
Gas condenses when reaches boiling point
Liquids led away from the column
100
Bitesize
Why does fractional distillation work - in what circumstances would it not work?
Liquids have different boiling points
If they had the same/very very similar boiling points
101
Bitesize
What is the column with the temperature gradient used in fractional distillation also called?
Fractionating column
102
Bitesize
What is paper chromatography used to separate?
Mixtures of soluble substances
103
Bitesize
Give 4 pieces of equipment for chromatography:
Pencil, inks, water, beaker
104
Bitesize
What are the two phases of chromatography?
Stationary phase and mobile phase
Stationary phase = the uniform, absorbent paper
Mobile phase = solvent that moves through paper (usually water) carry substances
105
Bitesize
Why do different substances move at different speeds through the paper?
They are more/less soluble
Or they are more/less attracted to the stationary/mobile phase
(Latter is unnecessary likely)
106
Bitesize
What is a chromatogram?
The results of separating mixtures by chromatography
107
Bitesize
How do you spot the difference between a pure and impure substance on a chromatogram?
A pure substance has 1 spot on chromatogram
A mixture/impure produces 2 or more
108
Bitesize
Give 3 ways of checking if two substances are the same:
They travel same distance up paper (same Rf value)
They have same number of spots
Their spots are the same colour
109
Bitesize
When did Dalton say his thing and what did he say?
1803 - he said matter was made up of tiny indivisible spheres called atoms
110
Bitesize
Who came up with the plum pudding model of the atom?
What did he discover which led him to it?
JJ Thompson
The electron
111
Bitesize
Give 3 conclusions Rutherford made from his experiment:
Mass of atom in nucleus
Nucleus has positive charge
Mostly empty space
112
Bitesize
Give the name of Rutherford’s model
The nuclear model
113
Bitesize
Give the order in which these things were discovered:
Proton
Electron
Neutron
Nucleus
Electron shells
Electron
Nucleus
Electron shells
Proton
Neutron
114
Bitesize
What is the radius of an atom?
1 x 10 to the power -10 m
115
Bitesize
What is the radius of a nucleus compared to the radius of an atom?
More than 10 000 times smaller
116
Bitesize
What is the radius of a nucleus?
1 x 10 to the power -14 m
117
Bitesize
What property is unique across every element - and will always tell you the type of element you have
Number of protons
118
Bitesize
An element has equal numbers of what?
Protons and electrons
(Sometimes they say an atom does too? I would stick with element)
119
Bitesize
Give the 3 isotopes of hydrogen and state which is most common
H1 H2 and H3
H1
120
Bitesize
Number of what determines chemical properties:
Electrons
121
Bitesize
What are chemical properties?
How a substance reacts with another
Substance
(Flammability, pH etc)
122
Bitesize
What is relative atomic mass?
The average of all the masses of isotopes of an element (taking their abundance into account )
123
Bitesize
True or false mass number = relative atomic mass
Which one is found on the periodic table?
False
Relative atomic mass
(Mass number is always a whole number, but relative atomic mass is usually rounded)
124
Bitesize
Which atom is relative atomic mass based off?
1/12th of the mass of a carbon 12 atom
125
Bitesize
What is relative atomic mass?
Mean relative mass of the different isotopes of an element
Number of times heavier an atom is compared to 1/12th of the mass of a carbon atom
126
Bitesize
What measure did early scientists use to order the periodic table?
Atomic weight (relative atomic mass)
127
Bitesize
Give 2 issues with early periodic tables:
They were incomplete and some elements were placed in the wrong groups (with elements not similar to them)
128
Bitesize
Why did Mendeleev leave gaps in his table?
He knew an element should be in the gap but it hadn’t been discovered yet
129
Bitesize
What did leaving gaps allow Mendeleev to do? Give an example:
Predict the properties of the missing elements
He predicted ‘eka-silicon’ would go below silicon - and later germanium was discovered to fit the position!
130
Bitesize
What did Mendeleev do with his periodic table to make it better? Give en example
He swapped elements to make them fit with other elements with similar chemical properties even if their atomic weight put them somewhere else in the table
Eg he swapped iodine and tellurium to make iodine linked with chlorine and bromine
131
Bitesize
The existence of what explains pair reversals
Isotopes (basically atomic weight/relative atomic mass is the wrong way to order your periodic table)
132
Bitesize
What is electronic structure
The way electrons are arranged
133
Bitesize
What type of ions do metals become when reacted?
Positive ions
134
Bitesize
What happens when magnesium burns in air?
It loses 2 electrons becoming an Mg2+ ion
135
Bitesize
True or false: most metal oxides are basic?
True
136
Bitesize
True or false: most non-metal oxides are acidic
True
137
Bitesize
Which of the two tends to have high boiling points?
Non metals
Metals
Metals (obvs)
138
Bitesize
Give 8 properties of a metal when solid:
Brittle
Ductile
Malleable
Sonorous
Good conductor of electricity
Good conductor of heat
Shiny
High density
139
Bitesize
Give 6 properties of a typical non-metal
Dull
Brittle
Poor conductor (of heat + electricity)
Low density
140
Bitesize
Elements in group 1 + 2 are….
Metals
141
Bitesize
How many electrons do elements in group 2 have in their outer shell?
2
142
Bitesize
Give the 3 group numbers of non metals
6,7,0
143
Bitesize
Give the name for group 0
Noble gases
144
Bitesize
What do noble gases exist as?
Single atoms
145
Bitesize
Are the boiling points of noble gases high or low?
Low
146
Bitesize
What element has the lowest overall boiling point?
Helium
147
Bitesize
What is the trend in boiling points going down group 0? Why?
Increase
Larger atoms
More intermolecular force between atoms/becomes stronger
More energy is needed to overcome these forces
148
Bitesize
What word describes how Unreactive group 0 are?
Inert
149
Bitesize
The noble gases have complete outer..
Shells
150
Bitesize
Give the name of group 1
The alkali metals
151
Bitesize
Give 3 properties of metals in group 1
Soft (can be cut with knife)
Low melting point
Low density
152
Bitesize
How does melting point change down group 1?
Melting point decreases down group 1
153
Bitesize
True or false:ions have a stable electron arrangement
True
154
Bitesize
When alkali metals react with water what do they produce?
A metal hydroxide and hydrogen
155
Bitesize
What is an alkali?
A base that is soluble in water (dissolves in water to form an alkaline solution)
156
Bitesize
What is a base
A substance that reacts with an acid to neutralise it and produce a salt
157
Bitesize
What happens to the reactivity of metals down group 1?
It increases
158
Bitesize
What do group 1 elements make when exposed to air
Metal oxides
159
Bitesize
What is the colour of the surface which is made when oxygen reacts with a metal?
White
160
Bitesize
Reaction with chlorine t make a metal chloride gets more or less vigorous down group 1
More
161
Bitesize
Why does reactivity increase down group 1?
Atom is larger
Outer electron further from nucleus
Force of attraction between nucleus and outer electron decreases
Outer electron lost more easily
162
Bitesize
What are group 7 elements called?
Halogens
163
Bitesize
Halogens exist as simple ___
Molecules
164
Bitesize
What type of bond are halogens joined by?
Single covalent bond
165
Bitesize
Down group 7 _____ increases
Relative molecular mass
166
Bitesize
Further down group 7 the ___ point increases/decreases
Increases
(As larger atoms
stronger intermolecular forces
More energy needed to overcome them)
167
Bitesize
When halogens react with metals what do they produce?
Salts
168
Bitesize
The reactivity in group 7 increases/decreases down the group
Decreases
(As harder to gain as less attractive force to nucleus as further away from nucleus)
169
Bitesize
When a halogen reacts with non metals what is formed?
Hydrogen halide
Hydrogen + chlorine -> hydrogen chloride
170
Bitesize
Hydrogen halides are ___ at room temperature
Gases
171
Bitesize
What do hydrogen halides dissolve in water to produce?
Acidic solutions
172
Bitesize
Give an example of a hydrogen halide dissolving in water to form an acid
HCl dissolves to form Hydrochloric acid
173
Bitesize
A more reactive halogen will ___ a less reactive halogen from solutions
Displace
174
Bitesize
If iodine solution forms the reaction mixture turns darker or lighter?
Darker
175
Bitesize
Explain why reactivity decreases down group 7
Atoms become larger
Outer shell further from the nucleus
Force of attraction between nucleus and outer shell decreases
Outer electron gained less easily
Halogen becomes less reactive
176
Bitesize
Give 4 ways in which transition metals are different from other metals
High melt points
Higher density
Greater strength
Greater hardness
177
Bitesize
Give 6 elements that are typical transition metals
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
178
Bitesize
True or false: transition metals aren’t very reactive with oxygen at room temperature
True
179
Bitesize
Do transition metals react very vigorously with water at room temperature? Give an example of an element that does
No
Iron - to form hydrated iron oxide (rust)_
180
Bitesize
True or false: transition metals always have one specific ionic charge
False - they will often make different charges such as copper which can be Cu 1 2 or 3
181
Bitesize
True or false: transition metals form white compounds
False: they form coloured compounds
182
Bitesize
Iron is the catalyst in what process which makes ammonia
Haber process
(Reacts nitrogen and oxygen)
183
Bitesize
Describe how copper chloride crystals could be made from copper carbonate and dilute Hydrochloric acid
Add excess copper carbonate to dilute Hydrochloric acid
Filter
Heat filtrate to evaporate some water leave to cool
N
