C1 - Atomic Structure & the Periodic Table Flashcards
1
Q
What is the definition of an element? Give an example
A
Elements are made from one type of atom (eg. sodium)
2
Q
What is the definition of a compound? Give an example
A
Compounds are two or more different elements chemically bonded (eg. sodium chloride)
3
Q
What is the definition of a mixture? Give an example
A
Mixtures are two or more elements or compounds not chemically bonded (eg. air)
4
Q
Name the 3 subatomic particles
A
Protons, electrons and neutrons
5
Q
Which particles are found in the nucleus?
A
Protons and neutrons
6
Q
Which particle orbits the nucleus on shells?
A
Electrons
7
Q
What is the charge of an electron?
A
-1, negative
8
Q
What is the charge of a neutron?
A
0, neutral
9
Q
What is the charge of a proton?
A
+1, positive
10
Q
What is the overall charge of an atom? Why?
A
Neutral - there are the same number of electrons and protons (they cancel each other out)
11
Q
How do you work out the number of protons in an atom?
A
Use the atomic number
12
Q
How do you work out the number of electrons in an atom?
A
Use the atomic number
13
Q
How do you work out the number of neutrons in an atom?
A
Atomic mass number - atomic number
14
Q
Which subatomic particle decides what the element is?
A
The number of protons
15
Q
What did the plum pudding model suggest the atom was like?
A
A ball of positive charge with negatively charged electrons scattered in it
16
Q
What did Rutherford (nuclear) model think the atom looked like?
A
Positively charged nucleus (small) with electrons surrounding the nucleus
17
Q
What did Bohr discovery about the atom?
A
He discovered that electrons went around in shells
18
Q
State the size of the nucleus
A
1 x 10-14m
19
Q
State the size of the atom
A
1 x 10-10m
20
Q
What is an isotope?
A
An element with the same number of protons and electrons but different numbers of neutrons
21
Q
How are elements organised in the modern periodic table?
A
According to atomic / proton number
22
Q
How were elements ordered in the early periodic table?
A
According to atomic weight
23
Q
What were the main issues with the early periodic table?
A
- It had no gaps for undiscovered elements
- Some elements were placed in groups with elements that had very different properties
24
Q
How are elements in the modern periodic table grouped?
A
They are grouped according to their properties
25
Where are metals found on the periodic table?
Left and bottom
26
What is group 1 called?
Alkali metals
27
What is group 7 called?
Halogens
28
What is group 0/8 called?
Noble gases
29
How many electrons can go on each shell?
1st - 2, 2nd - 8, 3rd - 8, 4th- 18
30
How are group number and outer electrons number related?
Group number = number of electron on outer shell
31
How are period number and shell number related?
Period number = number of shells
32
What are the properties of group 1 metals?
- Conduct electricity, can be cut
- React with water and oxygen
- Low density
33
How does the reactivity of group 1 elements change down the group?
They get more reactive
34
Complete the equation:
| metal + water > ... + ...
Metal + water = metal hydroxide + hydrogen
35
What is the test for hydrogen?
Squeaky pop
36
How do I test that metal hydroxides are alkali?
Add universal indicator - it will turn purple
37
Complete the equation:
| Metal + oxygen > ......
Metal + oxygen > metal oxide
38
What is the formula for chlorine?
Cl2 (diatomic)
39
What is the formula for fluorine?
F2 (diatomic)
40
What is the colour and state of fluorine at room temperature?
Yellow / green gas
41
What is the colour and state of chlorine at room temperature?
Green gas
42
What is the colour and state of bromine at room temperature?
Brown liquid
43
What is the state symbol for a gas, liquid and a solid?
(s), (l), (g)
44
Name some properties of noble gases
Low melting points, unreactive
45
Why are noble gases unreactive?
They have a full outer shell
46
What is the easiest way to identify whether something is a element?
Look in the periodic table
47
What is a molecule?
Two or more atoms chemically bonded
48
What is the mass of a proton?
1
49
What is the mass of a neutron?
1
50
What is the mass of a electron?
0
51
What did Thompson (plum pudding model) suggest the atom was like?
A ball of positive charge with negative electrons scattered in it
52
Rutherford realised that the plum pudding model was wrong.
What was Rutherford's model of the atom like?
What did he call his model of the atom?
Rutherford thought the atom was made of a tiny positively charged nucleus, surrounded by scattered electrons.
He called it 'the nuclear model'
53
How did Bohr improve Rutherford's nuclear model of the atom?
Bohr realised that electrons orbit the nucleus on shells
54
How big is the nucleus of an atom compared to the whole atom?
The nucleus of the atom is 1/10,000 of the size of an atom
55
Where is most of the mass of the atom found?
In the nucleus, because this is where protons and neutrons are found
56
How did Mendeleev organise the elements in his periodic table?
Mainly order of relative atomic mass but he changed the order slightly to put elements with similar properties in the same group
57
What unusual step did Mendeleev take to make this possible?
He left gaps in his periodic table
58
How did the gaps in Mendeleev's periodic table hep to prove his ideas?
Elements were discovered that fitted the gaps and had similar properties to the other elements in the same group
(For example, gallium fitted in a gap in group 3 and it had similar properties to aluminium)
59
What do elements in the same group of the periodic table have in common?
- The same number of electrons in their outer shell (e.g group 1 elements have 1 electron in their outer shell)
- Similar properties (e.g all group 1 elements react with water producing hydrogen and metal hydroxides)
60
Where are nonmetals found in the periodic table?
On the right and towards the top
61
What properties do most metals have in common?
- They are strong
- They can be bent or hammered into shape (Malleable)
- They are good at conducting heat and electricity.
- They have high melting and boiling points
62
What properties do most nonmetals have in common?
- They are brittle
- Dull looking
- Often liquids or gases at room temperature.
- Poor conductors
63
What do we call the metals in the middle of the periodic table?
Transition metals
64
Is hydrogen a metal or nonmetal?
Nonmetal
65
What do we call atoms that have lost or gained electrons and so have a positive or negative charge?
Ions
66
If two elements are in the same group in the periodic table, what does this tell you about them?
- That they have the same number of electrons in their outer shell (e.g all group 1 element have 1 electron in their outer shell).
- That they have similar properties
67
What charge do group 1 ions have (e.g sodium ions)?
+1
68
What happens when group 1 elements react with water?
- They float and move around on the surface fizzing.
- Hydrogen (which may burst into flame) is made.
Metal hydroxides (e.g sodium hydroxide) are made. These dissolve in the water making alkaline solutions.
- sodium + water → sodium hydroxide + hydrogen
- 2Na (s) + 2H2O (l) →2NaOH (aq) + H2 (g)
69
Lithium + oxygen→......
Lithium + oxygen →lithium oxide
70
Sodium + oxygen →......
Sodium + oxygen →sodium oxide (+ sodium peroxide)
71
Sodium + chlorine →......
Sodium + chlorine→sodium chloride
72
Potassium + chlorine →......
Potassium + chlorine→potassium chloride
73
Explain why the group 1 elements (alkali metals) get more reactive as you go down the group.
The outer electron is further from the nucleus
There is a weaker (electrostatic) attraction between the nucleus and outer electron.
It is easier to lose the outer electron
74
Compare the properties of group 1 metals and transition metals
- Group 1 are more reactive
- Alkali metals have much lower boiling points
- Transition metals are more dense, strong and hard
- Transition metals have much higher melting point
75
Fluorine and chlorine are both in group 7 of the periodic table, how many electrons do they have in their outer shell?
7
76
Group 7 elements form diatomic molecules. What are diatomic molecules?
Molecules made from two atoms bonded together
77
How does the reactivity of group 7 elements (halogens) change as you go down the group?
They get less reactive as you go down the group
78
Complete the equation below and explain why this happens:
Chlorine + sodium bromide→......
Chlorine displaces bromine, because it is more reactive than bromine.
Chlorine + sodium bromide →sodium chloride and bromine
79
What is oxidised (loses electrons) and what is reduced (gains electrons) in this reaction.
- Chlorine atoms are reduced (gain electrons) forming chloride ions.
- Bromide ions are oxidised (lose electrons) forming bromine molecules
80
Explain why the group 7 elements (halogens) get less reactive as you go down the group.
- The outer shell is further from the nucleus.
- The (electrostatic) attraction between the nucleus and outer shell/electrons is weaker.
- It's more difficult to attract electrons to the outer shell
81
How many electrons do the group 0 elements (noble gases) have in their outer shell?
8, except helium which has 2 electrons in its outer shell
82
Why are group 0 elements unreactive?
- They have full outer shells of electrons.
| - They have a stable arrangement of electrons so they don't need to gain/lose or borrow electrons from other atoms
83
What is the state and colour of group 0 elements at room temperature?
They are all colourless gases
84
Why does the boiling point of group 1 elements increase as you go down the group?
- The atoms have more electrons.
- There are stronger forces of (electrostatic) attraction between the atoms.
- It takes more energy to break these forces
85
Which elements form diatomic molecules (molecules made from two atoms joined together)?
- Oxygen (O2)
- Hydrogen (H2)
- Nitrogen (N2)
- Group 7 elements:
- Fluorine F2
- Chlorine Cl2
- Bromine Br2
- Iodine I2
86
A nanometer is one ___th of a metre
Billionth
87
What is one nanometer in standard form?
1x10-9m
88
How many different elements are there?
118
89
What is relative atomic mass and why is it used?
Because many elements can exist as different isotopes, RAM is used as a mass number. It is an average, taking into account the different masses and their abundance
90
What formula is used to calculate the RAM of an element?
Sum of all the elements' masses in a compound, mixture etc.
91
Chromatography is used to separate different dyes within an ink. Explain how a chromatography experiment is set up.
1. Draw a line near the bottom of a sheet of filter paper in pencil (since it's insoluble).
2. Add a spot of ink to this line.
3. Place the sheet in a beaker of solvent (e.g. water - depends on what's being tested), making sure the ink doesn't touch the solvent.
4. Put a lid on the container to stop the solvent evaporating
92
Explain what happens during chromatography
- The mobile phase (solvent) seeps up the paper, carrying the ink with it.
- Each dye within the ink moves up the paper at a different rate; the dyes separate out into spots.
If any of the dyes are insoluble, they stay on the stationary phase (pencil line).
- When the solvent has nearly reached the top, the paper is taken out and allowed to dry; the result is a chromatogram
93
What are the mobile and stationary phases in chromatography?
- Mobile phase = solvent (because it moves up the paper).
| - Stationary phase = pencil line (it doesn't move)
94
How would you separate an insoluble solid from a liquid?
Filtration
95
How would you separate a soluble salt from a liquid? Give 2 ways.
- Evaporation: heating the solution, in an evaporating dish, over a bunsen burner. However, this can only be used if the salt doesn't thermally decompose. If it does:
- Crystallisation: gently heating the solution until crystals start to form, then leaving it to cool. More crystals will form, which are filtered out of the solution and left in a warm place to dry
96
How would you separate out rock salt (a mixture of salt and sand)?
- Grind it to make the salt crystals small (so that they dissolve easily).
- Put it in water and heat; salt will dissolve but sand won't.
- Filter out the sand.
- Evaporate the water from the salt, so that it forms dry crystals
97
What is simple distillation used for?
Separating out a liquid from a solution
98
How does simple distillation separate out a liquid from a solution?
- Solution is heated.
- The part of the solution with the lowest boiling point evaporates first.
- The vapour is cooled in a condenser, then collected in a beaker at the end of the condenser.
- The rest of the solution remains in the flask
99
What is the problem with simple distillation?
You can only use it to separate liquids with very different boiling points
100
What is fractional distillation used for?
Separating out liquids, from a mixture, with close boiling points
101
How does fractional distillation work?
1. Heat the mixture in the flask
2. The liquid with the lowest boiling point evaporates first.
3. When the thermometer's temperature reaches the boiling point of this liquid, it reaches the top of the column, condenses, and is collected.
4. Other liquids may start to evaporate, but will condense part of the way up the column (bc it's cooler towards the top).
5. Once the first liquid's collected, the temperature is raised until the next one reaches the top of the column. Etc.
102
What was Dalton's model of the atom?
Atoms were solid, indivisible spheres. Each element was made of a different type of sphere
103
What was Thomson's model of the atom?
He discovered electrons which could be removed from atoms, disproving Dalton's theory of indivisibility.
Thomson suggested atoms were spheres of positive charge, with negative electrons scattered throughout (plum pudding model)
104
What was Rutherford's model of the atom?
Positively charged nucleus, surrounded by a cloud of negative electrons. This was the first nuclear model of the atom
105
What discovery did Bohr make? How was he proven right?
Electrons orbit the nucleus in fixed positions, called energy levels.
His theoretical calculations agreed with experimental data
106
What discovery was made after electron orbits?
Experiments showed that the nucleus' positive charge was subdivided between a group of particles, called protons
107
What discovery did Chadwick make? Why did this make sense?
He proved the existence of neutrons in the nucleus. This explained the imbalance between the atomic and mass numbers
108
Who theorised that atoms were solid, indivisible spheres?
Dalton
109
Who theorised the plum pudding model?
Thompson
110
Whose discoveries led to the nuclear model of the atom?
Rutherford
111
Who calculated that electrons had fixed orbits?
Bohr
112
Who discovered neutrons?
Chadwick
113
How was Rutherford's alpha scattering experiment conducted?
Scientists in Rutherford's lab fired a beam of alpha particles at a thin sheet of gold foil
114
In Rutherford's alpha scattering experiment, what did the scientists expect to happen and why?
From the plum pudding model, they expected particles to pass straight through the gold foil, or only be slightly deflected
115
What were the results of Rutherford's alpha scattering experiment? Why wasn't this as expected?
The majority of the alpha particles went straight through the gold sheet. However, some were deflected more than expected and a few were deflected right back the way they came. The plum pudding model couldn't explain this
116
In Rutherford's alpha scattering experiment, a few alpha particles were deflected back. What did the scientists deduce from this?
They realised that most of the atom's mass was concentrated in a central nucleus, which must also have a positive charge, since it repelled the positive alpha particles
117
In Rutherford's alpha scattering experiment, most of the alpha particles passed straight through. What did the scientists deduce from this?
They realised that most of the atom is just empty space, and that the nucleus is very small relative to this space
118
What was deduced from the results of Rutherford's alpha scattering experiment?
1. Because a few alpha particles were deflected back, they realised that most of the atom's mass was concentrated in a central nucleus, which must also have a positive charge, since it repelled the positive alpha particles.
2. Because most of the alpha particles passed straight through, they realised that most of the atom is just empty space, and that the nucleus is very small relative to this space
119
How were elements organised in the early periodic table, and what was the problem with this?
Elements were organised according to their relative atomic masses.
The table wasn't complete, and some elements were placed in the wrong group because the ordering didn't take into account their properties
120
How was Mendeleev's periodic table different to - and better than - the early versions of the periodic table?
- He organised elements mainly in order of atomic mass, but also taking into account their properties.
- The discovery of isotopes showed he was right to do this.
- He left gaps which predicted the existence of undiscovered elements, allowing him to predict their properties.
- The discovery of certain elements that fit this pattern confirmed his ideas, for example, he left a gap for an element with similar properties to aluminium.
- Gallium was discovered, and it showed these properties
121
Transition metals are found in the middle of the periodic table. Give 7 properties of transition metals
- Good conductors of electricity + heat
- Strong
- Dense
- Shiny
- Can form more than one ion
- Colourful
- Transition metal compounds often make good catalysts
122
What are the trends in properties of alkali metals as you go down the group?
Increasing reactivity
Decreasing melting + boiling points
Increasing relative atomic mass
123
Alkali metals only ever form ionic compounds. What are these compounds usually like?
White solids that dissolve in water to form colourless solutions
124
Explain why sodium is more reactive than lithium
- Sodium is further down group 1 than lithium.
- Group 1 ions lose one electron to become stable.
- Sodium's outer electron is further from the nucleus that lithium's.
- So the electrostatic attraction between the electron and nucleus is weaker
- So the electron is more easily released.
- So sodium is more reactive
125
Compare the reactions of lithium and potassium with water. Describe what would be observed in each reaction and explain the similarities and differences [6 marks]
- A vigorous reaction would be observed with both metals
- The reaction with potassium would be more vigorous as it is more reactive than lithium
- This is because the outer electron of potassium is further from its nucleus and therefore more easily lost
- Both metals would float, as they are less dense than water.
- Both metals will fizz, producing bubbles of hydrogen gas
- The reaction with potassium would produce more hydrogen bubbles, as potassium is more reactive
- The reaction with potassium would release more energy, to the extent that the potassium and hydrogen could ignite
126
Compare the properties of transition and alkali metals
Alkali metals are much more reactive.
Transition metals are stronger, denser and harder.
Alkali metals have much lower boiling points.
127
How do alkali metals react with water?
- They react vigorously to produce hydrogen gas and metal hydroxides
- The violence of reactivity (and energy released from the reaction) increases as you go down the group
128
How do alkali metals react with chlorine?
- When heated in chlorine gas, they form white metal chloride salts
- The reaction gets more vigorous as you go down the group
129
How do alkali metals react with oxygen?
They react with oxygen to form metal oxides (which is why they tarnish in the air), different types of oxide forming depending on the metal:
Lithium → lithium oxide.
Sodium → mixture of sodium oxide and sodium peroxide
Potassium → mixture of potassium peroxide and potassium superoxide
130
What are the trends in properties of the halogens as you go down the group?
- Decreasing reactivity
- Increasing melting + boiling points
- Increasing relative atomic masses
131
Give 3 properties of the halogens
Form diatomic molecules
Bond ionically w/ metals
Bond covalently to form simple molecular compounds
A more reactive halogen will displace a less reactive one from an aqueous solution of its salt
132
What is the colour and state of fluorine at room temperature? Give 2 of its properties
- Very reactive and poisonous
| - Yellow gas
133
What is the colour and state of chlorine at room temperature? Give 3 of its properties
- Green gas.
| - Fairly reactive, poisonous, dense
134
What is the colour and state of bromine at room temperature? Give 3 of its properties
- Red-brown liquid
| - Poisonous, dense, volatile
135
What is the colour and state of iodine at room temperature? What does its gas look like?
- Dark grey, crystalline solid
| - Purple gas
136
A chemist places a glass lid over a beaker containing aqueous iodine. She places an ice cube on top of the lid and then gently heats the solution. Predict and explain her observations
A purple vapour will form over the solution as the iodine evaporates.
Purple/grey crystals will form on the lid as the iodine deposits/crystallises/solidifies
137
Give 4 properties of noble gases
Inert
Non-flammable (bc of above)
Exist as monatomic gases
All colourless gases at room temperature
138
Why are the noble gases inert?
They have full outer shells which are energetically stable. They therefore don't need to react to gain or lose electrons to become stable
139
What are the trends in properties of the noble gases as you go down the group?
- Increasing boiling points (greater no. electrons in each element leads to greater intermolecular forces
- Increasing relative atomic mass
140
If isotopes have different numbers of neutrons how else must they also be different?
They must have different atomic masses.
