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GCSE Chemistry Revision > C1 - Atomic Structure > Flashcards

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

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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

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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

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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

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5
Q

The history of the periodic table
True or false, both Newlands and Dobereiners collected, lithium, sodium, and potassium together

A

True

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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)

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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.

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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.

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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.

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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.

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11
Q

Atoms
What is an atom?

A

The simplest form of matter in chemistry

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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

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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

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14
Q

Atoms
What is a compound

A

A substance of two or more different elements, chemically bonded

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15
Q

Atoms
What is an element?

A

A pure substance made from one type of atom

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16
Q

Atoms
What does the group number represent in the periodic table?

A

The number of electrons in the outer shell

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17
Q

Atoms
Which way do groups go from top to bottom?

A

Up down

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18
Q

Atoms
What does the period number represent in the periodic table?

A

The number of electron shells

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19
Q

Atoms
True or false elements in the same period have similar chemical properties

A

True

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20
Q

Atoms
as you increase period number, what also increases

A

Reactivity

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21
Q

Atoms
Are periods, rows or columns

A

Rows

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22
Q

Atoms
What is the mass number represent in the periodic table

A

Protons, plus neutrons

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23
Q

Atoms
What is the atomic number represent in the periodic table?

A

Number of protons, all the number of electrons

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24
Q

Atoms
How many elements are there?

A

110

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25
Q

Atoms
Elements are arranged in increasing _____

A

Atomic number

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26
Q

Atoms
Do elements have an overall charge

A

No

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27
Q

Atoms
What is a mixture?

A

Two or more different substances not chemically bonded together that can be separated by physical process

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28
Q

History of the atomic model
Who is the author of the plum pudding model?

A

Thompson (1897)

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29
Q

History of the atomic model
What does the plum pudding model Describe?

A

A cloud of positive charge with negative electrons in embedded within
The negative electrons, the plums in the positive pudding

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30
Q

History of the atomic model
Did Thomsons model include the electron?

A

Yes

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31
Q

History of the atomic model
Did Thomsons model predict that the atom was solid?

A

No

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32
Q

History of the atomic model
Who was the author of the nuclear model?

A

Rutherford

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33
Q

History of the atomic model
What was Rutherford’s experiment in 1909?

A

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!

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34
Q

History of the atomic model
What did Niels Bohr contribute to the model of the atom?

A

In 1915 he describes the fact that electrons orbit the nucleus at specific distances - in electron shells

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35
Q

History of the atomic model
Who discovered the modern nuclear model?

A

Chadwick in the 1920s

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36
Q

History of the atomic model
What did James Chadwick prove?

A

The existence of neutrons

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37
Q

History of the atomic model
What was the earliest of the atom and who authored it?

A

The bowling ball model, which proposed that the atom was a solid indivisible sphere
Dalton 1803

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38
Q

Isotopes
What is an isotope?

A

Atoms of the same element, but a different number of neutrons

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39
Q

Isotopes
What are the similarities and differences between two isotopes?

A

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)

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40
Q

Isotopes
What is relative atomic mass?

A

The average value that takes account of the abundance of isotopes of an element

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41
Q

Isotopes
How do you calculate relative atomic mass?

A

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

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42
Q

Separating methods
What is distillation used for

A

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

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43
Q

Separating methods
What is the difference between fractional distillation and simple distillation?

A

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

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44
Q

Separating methods
Briefly describe the process of distillation

A

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

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45
Q

Separating methods
What is crystallisation?

A

The separation of a solute from a solvent to form crystals

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46
Q

Separating methods
Briefly describe the process of crystallisation

A

Evaporate the solution into a smaller volume and let it cool
As the solution cools crystals will form which can be obtained by filtration

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47
Q

Separating methods
What does filtration separate?

A

An insoluble solid from a liquid

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48
Q

Separating methods
Briefly describe the process of filtration

A

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

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49
Q

Separating methods
What does chromatography separate?

A

Mixtures of coloured compounds
Usually pen ink or food colouring agents

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50
Q

Separating methods
Briefly describe the process of chromatography

A

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.

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51
Q

Separating methods
What is a paper with separated chromatography inks called?

A

A chromatogram

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52
Q

Separating methods
The further up the paper a colour travels the more soluble/insoluble it is

A

Soluble

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53
Q

Separating methods
How could you increase the accuracy of a chromatography experiment?

A

 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

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54
Q

Separating methods
What is an RF value and how is it calculated?

A

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

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55
Q

Separating mixtures
What is a solution?

A

When is solute is dissolved in a solvent

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56
Q

Separating mixtures
What is a solvent?

A

A liquid substance, which may be mixed with a solute to make a solution

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57
Q

Separating mixtures
What does insoluble mean?

A

The solute can’t be dissolved in a solvent

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58
Q

Separating mixtures
What is a solute?

A

A solid substance which may be dissolved into the solvent to form a solution

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59
Q

Separating mixtures
What does soluble mean?

A

A solute that can dissolve with a solvent

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60
Q

Separating mixtures
What is a mixture?

A

Different substances, not chemically joined 

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61
Q

Why did Rutherford do his experiment in a vacuum?

A

So that any deflections were due to the gold foil and nothing else

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62
Q

Why was gold used by Rutherford in his experiments on the atom?

A

It was the only metal that could be rolled out very thin without cracking

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63
Q

Give all the diatomic elements and a way to remember them

A

Hydrogen
Nitrogen
Fluorine
Oxygen
Iodine
Chlorine
Bromine
Have no fear of ice cold beer!

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64
Q

True or false: elements in a compound are in fixed proportions

A

True

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65
Q

What is the chemical formula for magnesium oxide?

A

MgO

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66
Q

What is the chemical formula of sodium chloride

A

NaCl

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67
Q

What is the chemical formula of potassium bromide?

A

KBr

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68
Q

What is the formula for magnesium iodide?

A

MgI2

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69
Q

What is the formula for carbon monoxide?

A

CO

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70
Q

What is the Cornu,a for sulfur trioxide?

A

SO3

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71
Q

What is the formula for ammonia?

A

NH3

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72
Q

What is the formula for methane>

A

CH4

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73
Q

What is an ion?

A

A charged particle formed when an atom loses or gains electrons

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74
Q

What is the formula of a sodium ion?

75
Q

What is the formula of a magnesium ion?

76
Q

What is the formula of a chloride ion?

A

Cl-
Remember it is CHLORIDE when an ion and only chlorine as a normal element diatomic

77
Q

What is the formula of an oxygen ion?

78
Q

What is the formula of sodium oxide?

79
Q

What is the formula of magnesium chloride?

80
Q

What does the state symbol (aq) mean?

A

Aqueous solution

81
Q

What is the law of the conservation of mass?

A

No atoms are lost or made during a chemical reaction

(Total mass of products = total mass of reactants)

82
Q

What is an element?

A

A substance made up of one atom only

83
Q

What is a molecule?

A

A collection of two or more atoms held together by chemical bonds

84
Q

Bitesize
What is filtration used to separate?

A

Separates an insoluble solid from a liquid

85
Q

Bitesize
Give two examples where filtration is useful

A

Mix of sand and water
Excess reactant from mixture

86
Q

Bitesize
How does filtration paper work?

A

It has tiny pores which let small molecules through but not larger in dissolved particles

87
Q

Bitesize
Give 3 pieces of equipment needed for filtration

A

Filter paper
Filter funnel
Beakers

88
Q

Bitesize
What does crystallisation produce?

A

Solid crystals from a solution

89
Q

Bitesize
Give an example of what crystallisation is used for:

A

Getting copper sulfate crystals from a copper sulfate solution

90
Q

Bitesize
Give 3 bits of equipment needed for crystallisation

A

Evaporating basin
Bunsen burner
Tripod

91
Q

Bitesize
Describe the process of crystallisation:

A

Heat evaporates most of solvent
Leave the rest to evaporate over time leaving larger crystals

92
Q

Bitesize
How do you make big crystals?

A

Heat over a boiling water bath instead of

93
Q

Bitesize
What is simple distillation?

A

Separation of a solvent from a solution

94
Q

Bitesize
Give an example of something simple distillation is useful for

A

Producing pure water from seawater

95
Q

Bitesize
How does simple distillation work?

A

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
Q

Bitesize
Give 4 pieces of equipment needed for simple distillation

A

Leibig condenser/condensing tube
Beaker
Bunsen burner
Conical flask with bung

97
Q

Bitesize
What is fractional distillation?

A

Separated different liquids from a mixture of liquids

98
Q

Bitesize g
Give 2 examples of uses of fractional distillation

A

Separating ethanol from ethanol and water mixture

Separating fractions from crude oil

99
Q

Bitesize
Describe the process of fractional distillation:

A

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
Q

Bitesize
Why does fractional distillation work - in what circumstances would it not work?

A

Liquids have different boiling points

If they had the same/very very similar boiling points

101
Q

Bitesize
What is the column with the temperature gradient used in fractional distillation also called?

A

Fractionating column

102
Q

Bitesize
What is paper chromatography used to separate?

A

Mixtures of soluble substances

103
Q

Bitesize
Give 4 pieces of equipment for chromatography:

A

Pencil, inks, water, beaker

104
Q

Bitesize
What are the two phases of chromatography?

A

Stationary phase and mobile phase
Stationary phase = the uniform, absorbent paper
Mobile phase = solvent that moves through paper (usually water) carry substances

105
Q

Bitesize
Why do different substances move at different speeds through the paper?

A

They are more/less soluble

Or they are more/less attracted to the stationary/mobile phase

(Latter is unnecessary likely)

106
Q

Bitesize
What is a chromatogram?

A

The results of separating mixtures by chromatography

107
Q

Bitesize
How do you spot the difference between a pure and impure substance on a chromatogram?

A

A pure substance has 1 spot on chromatogram

A mixture/impure produces 2 or more

108
Q

Bitesize
Give 3 ways of checking if two substances are the same:

A

They travel same distance up paper (same Rf value)
They have same number of spots
Their spots are the same colour

109
Q

Bitesize
When did Dalton say his thing and what did he say?

A

1803 - he said matter was made up of tiny indivisible spheres called atoms

110
Q

Bitesize
Who came up with the plum pudding model of the atom?
What did he discover which led him to it?

A

JJ Thompson
The electron

111
Q

Bitesize
Give 3 conclusions Rutherford made from his experiment:

A

Mass of atom in nucleus
Nucleus has positive charge
Mostly empty space

112
Q

Bitesize
Give the name of Rutherford’s model

A

The nuclear model

113
Q

Bitesize
Give the order in which these things were discovered:
Proton
Electron
Neutron
Nucleus
Electron shells

A

Electron
Nucleus
Electron shells
Proton
Neutron

114
Q

Bitesize
What is the radius of an atom?

A

1 x 10 to the power -10 m

115
Q

Bitesize
What is the radius of a nucleus compared to the radius of an atom?

A

More than 10 000 times smaller

116
Q

Bitesize
What is the radius of a nucleus?

A

1 x 10 to the power -14 m

117
Q

Bitesize
What property is unique across every element - and will always tell you the type of element you have

A

Number of protons

118
Q

Bitesize
An element has equal numbers of what?

A

Protons and electrons

(Sometimes they say an atom does too? I would stick with element)

119
Q

Bitesize
Give the 3 isotopes of hydrogen and state which is most common

A

H1 H2 and H3
H1

120
Q

Bitesize
Number of what determines chemical properties:

121
Q

Bitesize
What are chemical properties?

A

How a substance reacts with another
Substance
(Flammability, pH etc)

122
Q

Bitesize
What is relative atomic mass?

A

The average of all the masses of isotopes of an element (taking their abundance into account )

123
Q

Bitesize
True or false mass number = relative atomic mass
Which one is found on the periodic table?

A

False
Relative atomic mass

(Mass number is always a whole number, but relative atomic mass is usually rounded)

124
Q

Bitesize
Which atom is relative atomic mass based off?

A

1/12th of the mass of a carbon 12 atom

125
Q

Bitesize
What is relative atomic mass?

A

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
Q

Bitesize
What measure did early scientists use to order the periodic table?

A

Atomic weight (relative atomic mass)

127
Q

Bitesize
Give 2 issues with early periodic tables:

A

They were incomplete and some elements were placed in the wrong groups (with elements not similar to them)

128
Q

Bitesize
Why did Mendeleev leave gaps in his table?

A

He knew an element should be in the gap but it hadn’t been discovered yet

129
Q

Bitesize
What did leaving gaps allow Mendeleev to do? Give an example:

A

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
Q

Bitesize
What did Mendeleev do with his periodic table to make it better? Give en example

A

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
Q

Bitesize
The existence of what explains pair reversals

A

Isotopes (basically atomic weight/relative atomic mass is the wrong way to order your periodic table)

132
Q

Bitesize
What is electronic structure

A

The way electrons are arranged

133
Q

Bitesize
What type of ions do metals become when reacted?

A

Positive ions

134
Q

Bitesize
What happens when magnesium burns in air?

A

It loses 2 electrons becoming an Mg2+ ion

135
Q

Bitesize
True or false: most metal oxides are basic?

136
Q

Bitesize
True or false: most non-metal oxides are acidic

137
Q

Bitesize
Which of the two tends to have high boiling points?
Non metals
Metals

A

Metals (obvs)

138
Q

Bitesize
Give 8 properties of a metal when solid:

A

Brittle
Ductile
Malleable
Sonorous
Good conductor of electricity
Good conductor of heat
Shiny
High density

139
Q

Bitesize
Give 6 properties of a typical non-metal

A

Dull
Brittle
Poor conductor (of heat + electricity)
Low density

140
Q

Bitesize
Elements in group 1 + 2 are….

141
Q

Bitesize
How many electrons do elements in group 2 have in their outer shell?

142
Q

Bitesize
Give the 3 group numbers of non metals

143
Q

Bitesize
Give the name for group 0

A

Noble gases

144
Q

Bitesize
What do noble gases exist as?

A

Single atoms

145
Q

Bitesize
Are the boiling points of noble gases high or low?

146
Q

Bitesize
What element has the lowest overall boiling point?

147
Q

Bitesize
What is the trend in boiling points going down group 0? Why?

A

Increase

Larger atoms
More intermolecular force between atoms/becomes stronger
More energy is needed to overcome these forces

148
Q

Bitesize
What word describes how Unreactive group 0 are?

149
Q

Bitesize
The noble gases have complete outer..

150
Q

Bitesize
Give the name of group 1

A

The alkali metals

151
Q

Bitesize
Give 3 properties of metals in group 1

A

Soft (can be cut with knife)
Low melting point
Low density

152
Q

Bitesize
How does melting point change down group 1?

A

Melting point decreases down group 1

153
Q

Bitesize
True or false:ions have a stable electron arrangement

154
Q

Bitesize
When alkali metals react with water what do they produce?

A

A metal hydroxide and hydrogen

155
Q

Bitesize
What is an alkali?

A

A base that is soluble in water (dissolves in water to form an alkaline solution)

156
Q

Bitesize
What is a base

A

A substance that reacts with an acid to neutralise it and produce a salt

157
Q

Bitesize
What happens to the reactivity of metals down group 1?

A

It increases

158
Q

Bitesize
What do group 1 elements make when exposed to air

A

Metal oxides

159
Q

Bitesize
What is the colour of the surface which is made when oxygen reacts with a metal?

160
Q

Bitesize
Reaction with chlorine t make a metal chloride gets more or less vigorous down group 1

161
Q

Bitesize
Why does reactivity increase down group 1?

A

Atom is larger
Outer electron further from nucleus
Force of attraction between nucleus and outer electron decreases
Outer electron lost more easily

162
Q

Bitesize
What are group 7 elements called?

163
Q

Bitesize
Halogens exist as simple ___

164
Q

Bitesize
What type of bond are halogens joined by?

A

Single covalent bond

165
Q

Bitesize
Down group 7 _____ increases

A

Relative molecular mass

166
Q

Bitesize
Further down group 7 the ___ point increases/decreases

A

Increases
(As larger atoms
stronger intermolecular forces
More energy needed to overcome them)

167
Q

Bitesize
When halogens react with metals what do they produce?

168
Q

Bitesize
The reactivity in group 7 increases/decreases down the group

A

Decreases
(As harder to gain as less attractive force to nucleus as further away from nucleus)

169
Q

Bitesize
When a halogen reacts with non metals what is formed?

A

Hydrogen halide

Hydrogen + chlorine -> hydrogen chloride

170
Q

Bitesize
Hydrogen halides are ___ at room temperature

171
Q

Bitesize
What do hydrogen halides dissolve in water to produce?

A

Acidic solutions

172
Q

Bitesize
Give an example of a hydrogen halide dissolving in water to form an acid

A

HCl dissolves to form Hydrochloric acid

173
Q

Bitesize
A more reactive halogen will ___ a less reactive halogen from solutions

174
Q

Bitesize
If iodine solution forms the reaction mixture turns darker or lighter?

175
Q

Bitesize
Explain why reactivity decreases down group 7

A

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
Q

Bitesize
Give 4 ways in which transition metals are different from other metals

A

High melt points
Higher density
Greater strength
Greater hardness

177
Q

Bitesize
Give 6 elements that are typical transition metals

A

Chromium
Manganese
Iron
Cobalt
Nickel
Copper

178
Q

Bitesize
True or false: transition metals aren’t very reactive with oxygen at room temperature

179
Q

Bitesize
Do transition metals react very vigorously with water at room temperature? Give an example of an element that does

A

No
Iron - to form hydrated iron oxide (rust)_

180
Q

Bitesize
True or false: transition metals always have one specific ionic charge

A

False - they will often make different charges such as copper which can be Cu 1 2 or 3

181
Q

Bitesize
True or false: transition metals form white compounds

A

False: they form coloured compounds

182
Q

Bitesize
Iron is the catalyst in what process which makes ammonia

A

Haber process
(Reacts nitrogen and oxygen)

183
Q

Bitesize
Describe how copper chloride crystals could be made from copper carbonate and dilute Hydrochloric acid

A

Add excess copper carbonate to dilute Hydrochloric acid
Filter
Heat filtrate to evaporate some water leave to cool

N

GCSE Chemistry Revision (13 decks)

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