Chemistry of the Elements Flashcards
1
Q
The rows of the periodic table are called …. The properties of elements … as you go along a period
A
The rows of the periodic table are called periods. The properties of elements change as you go along a period
2
Q
The columns of the periodic table are called …
A
The columns of the periodic table are called groups
3
Q
What do elements in the same group have in common? Why? What changes?
A
elements in the same group have similar chemical properties
this is because they have the same number of electrons on their outer shell
the proprties of elements (such as reactivity) often gradually change as you go down a group (i.e. as the atomic number increases)
4
Q
Do you metals conduct electricity? Why?
A
(they are the green)
metals conduct electricity because they allow charge to pass through them easily
5
Q
Metal oxides are basic. What does this mean?
A
(they are the green)
this means they wil neautralise acids
metal oxides which dissolve will form solutions of a pH of more than 7
6
Q
Do non-metals conduct electricity?
A
(they are the blue)
non-metals are poor conductors of electricity
7
Q
Non-metals are acidic. What does this mean?
A
(they are the blue)
this means they dissolve in water to form solutions with a pH of less than 7
8
Q
What state of matter do metals tend to be?
A
solids
e.g. mercury is an exception - it is a liquid
9
Q
What are the differences in melting and boiling points between metals and non-metals?
A
metals tend to have high melting and boiling points
non-metals tend to have low metling and boiling points (carbon and silicon are obvious exceptions)
10
Q
Do metals tend to have relatively low or relatively high densities?
A
metals tend to have relatively high densities
11
Q
Metals are … when they are polished (known as metallic …), and tend to be easily …
A
Metals are shiny when they are polished (known as metallic lustre), and tend to be easily workable
12
Q
Non-metals tend to … as solids and, even if they are crystalline, they don’t have the same sort of … a metals
A
Non-metals tend to brittle as solids and, even if they are crystalline, they don’t have the same sort of shinea metals
13
Q
What is the difference in conducting electricity and heat in metals and non-metals?
A
metals are good conductors of electricity and heat
non-metals usually don’t conduct electricity - carbon (in the form of graphite) and silicon are exception
non-metals are poor conductors of heat
14
Q
Metals form … ions in their compounds. Non-metals form … ions and … compounds
A
Metals form positive ions in their compounds. Non-metals form negative ions and covalent compounds
15
Q
What is Group 0? Which elements are in it?
A
the noble gases
(in order):
helium
neon
argon
krypton
xenon
radon
16
Q
Noble gases are coloured/colourless gases
A
Noble gases are colourless gases
17
Q
What percentage of the air is made up of Argon?
A
nearly 1%
18
Q
Helium has the … density of any gas
A
Helium has the second lowest density of any gas (after hydrogen)
19
Q
All noble gases are monatomic/diatomic. What does this mean?
A
All noble gases are monatomic
This means that their molecules consist of single atoms
20
Q
The density and boiling point of noble gases increases/decreases as you down the Group
Why is this?
A
The density and boiling point of noble gases increases as you down the Group
this is because the attractions between one molecules and its neighbour get stronger as the atoms get bigger
more energy is needed to break the stronger attractions
21
Q
Noble gases do/don’t form stable ions, and so do/don’t produce ionic compounds
A
Noble gases don’t form stable ions, and so don’t produce ionic compounds
22
Q
Noble gases are/aren’t inert. What does this mean? Why?
A
Noble gases are inert
this means they don’t react with much at all
this is because they have a full outer shell of electrons
23
Q
What is Group 1 of the periodic table? What elements are in it?
A
the alkali metals
(in order):
lithium
sodium
potassium
rubidium
caesium
francium
24
Q
The alkali metals have low/high melting and poling points (for metals), and get lower/higher as you go down the group
Their densities tend to … as you go down the group
A
The alkali metals have low melting and poling points (for metals), and get lower as you go down the group
Their densities tend to increase as you go down the group
25
Which alkali metals float on water? Why?
lithium, sodium and potassium are less dense than water, so they will float
26
The alkali metals are very **soft/hard** and get **softer/harder** as you go down the group
They are **...** but **...** within seconds of exposure to air
The alkali metals are very **soft** and get **softer** as you go down the group
They are **shiny** but **tarnish** within seconds of exposure to air
27
How must the alkali metals be stored?
they have to be stored out of contact with air or water, so they are stored under oil
28
When lithium, sodium and potassium are put in water, how do they react?
they react vigorously
29
What does the reaction of an alkali metal with water produce? Is this alkaline or acidic?
a metal hydroxide and hydrogen
this solution is alkaline
30
What does aqueous (aq) mean?
dissolved in water
31
What is the word and symbol equation for the reaction of sodium with **cold** water?
sodium + **cold** water → sodium hydroxide + hydrogen
2Na (s) + 2H2O (l) → 2NaOh (aq) + H2 (g)
32
Alkali metals have mainly **... (a colour)** compounds which dissolve to produce **coloured/colourless** solutions
Alkali metals have mainly **whit** compounds which dissolve to produce **colourless** solutions
33
As you go down Group 1, the elements become **less/more** reactive as the atomic number **increases/decreases**
As you go down Group 1, the elements become **more** reactive as the atomic number **increases**
34
What is observed in the reaction of lithium with water? What colour does the universal indicator turn?
the lithium moves slwowly around rge surface, fizzing, until it disappears
the indicator turns from neutral to purple because the water has become alkaline
35
What is observed in the reaction of sodium with water? What colour does the universal indicator turn?
sodium fizzed rapidly and moves quickly around the surface, it may ignite
it reacts faster than lithium
the indicator turns from neutral to purple because the water has become alkaline
36
What is observed in the reaction of potassium with water? What colour does the universal indicator turn?
potassium reacts vigorously, burns with a lilac flame - and sometimes explodes
potassium reacts faster than lithium and sodium
the indicator turns from neutral to purple because the water has become alkaline
37
Group 1 metals have **...** electron on their outer shell
As you go down Group 1, the outermost electron is in a shell that is **closer/further** from the nucleus. What does this mean?
What charge are their ions?
Group 1 metals have **one**electron on their outer shell
As you go down Group 1, the outermost electron is in a shell that is **further** from the nucleus
This means that as the atom gets bigger as you go down the group, the attraction between the outermost electron and the nucleus becomes loess and the outer electron is lost more easily, and the metals are move reactive
Their ions are +1 charged
38
What is Group 7? What elements are in it?
halogens
(in order):
fluorine
chlorine
bromine
iodine
astatine
39
The halogens are **monatomic/diatomic**
The halogens are **diatomic**
40
What state of matter and colour is flourine?
gas
yellow
41
What state of matter and colour is chlorine?
gas
green
42
What state of matter and colour is bromine?
liquid
dark red liquid - red/brown vapour
43
What state of matter and colour is iodine?
solid
dark grey solid - purple vapour
44
The halogens are **good/poor** conductors of heat and electricity
When they are solid, their crystals **will/will not** be brittle
The halogens are **poor** conductors of heat and electricity
When they are solid, their crystals **will** be brittle
45
As the atomic number of the halogens increased, the elements have a **lighter/darker** colour and a **lower/higher** boiling point
As the atomic number of the halogens increased, the elements have a **darker** colour and a **higher** boiling point
46
As you go up Group 7, the reactivity **increases/decreases**. Why?
As you go up Group 7, the reactivity **increases**
**this is because the shell with the missing electron is nearer to the nucleus, so the attraction to to positive nucleus is greater**
47
What do the halogens react with hydrogen to form?
hydrogen halides
48
What three things are hydrogen halides? How are they bonded?
steamy, acidic, poisonous gases
they are bonded covalently
49
Are hydrogen halides soluble in water? What do they react with water to produce?
hydrogen halides are very soluble in water
they react with water to produce solutions of acids, such as HCl (a solution of hydrogen chloride in water)
50
What state of matter is HCl at room temperature?
gas
51
What does hydrogen chloride do in water? Is this an alkaline or acidic solution? Why?
hydrogen chloride dissociates in water
the Hcl molecules split into H+ ions and Cl- ions - this process is called dissociation
this is an acidic solution because it contains H+
52
When hydrochloric acid solution in water is tested with blue litmus paper, what colour does the paper turn?
blue to pink
53
What does hydrogen chloride do in methy;benzene? Is this an acidic solution? Why?
HCl doesn't dissociate into H+ and Cl- ions when disolved in organic solvents like methylbenzene
this means there are no H+ ions so produced so it is not acidic
54
When hydrogen chloride solution in methylbenzene is tested with blue litmus paper, what colour does the paper turn? What happens if there is any moisture on the paper or in the bottle
the blue litmus paper stays blue
but if there is any moisture on the paper or in the bottle then the HCl can dissociate and it will behave like an acid again
55
What do halogens form with metals?
ionic salts
56
What do halogens form with non-metals?
covalent compounds
57
Halogens are **oxidising/reducing** agents with **oxidising/reducing** ability decreasing down the Group
Halogens are **oxidising** agents with **oxidising** ability decreasing down the Group
58
What are two uses of halogens in general? What is a use of chlorine? What is a use of iodine?
toothpaste
non-stick coating on drying pans
chlrine kills bacteria - used in bleach and swimming pools
iodine is used as an antiseptic to prevent cuts from being infected
59
Transition metals are typically **metallic/non-metallic** elements
They are **good/poor** conductors of heat and electricity
They are **workable/not workable**, **strong/weak**, and mostly with **high/low** densities
With the exception of liquid mercury, Hg, they have **high/low** melting points
(they are the orange)
Transition metals are typically **metallic** elements
They are **good** conductors of heat and electricity
They are **workable,** **strong**, and mostly with **high** densities
With the exception of liquid mercury, Hg, they have **high** melting points
60
Transition metals are much **more/less** reactive than the metals in Group 1 and 2, so they **do/don't** react as rapidly with air or water
(they are the orange)
Transition metals are much **less** reactive than the metals in Group 1 and 2, so they **don't** react as rapidly with air or water
61
Transition metals form **coloured/colourless** compounds
Transition metals form **coloured** compounds
62
What are the uses of transition metals?
they are often useful catalsysts:
iron in the manufacture of ammonia (Haber process)
vanadium (V) oxide in the manufacture of sulphuric acid (Contact process)
63
More reactitve halogens **...** less reactive halogens - they take part in **...** reaction
More reactitve halogens **displacement** less reactive halogens - they take part in **displacement** reaction
64
What happens in the reaction of chlorine water, Cl2 (aq) , with potassium chloride solution, KCl (aq)? Why?
no reaction
chloride cannot displace chlorine
65
What happens in the reaction of chlorine water, Cl2 (aq) , with potassium bromide solution, KBr (aq)? Why?
orange solution (Br2) is formed
the chlorine displaced the bromide because it is more reactive than bromide
66
What happens in the reaction of chlorine water, Cl2 (aq) , with potassium bromide solution, KI (aq)? Why?
brown solution (I2) is formed
chlorine displaces the iodide because it is more reactive than iodide
67
What happens in the reaction of chlorine water, Br2 (aq) , with potassium bromide solution, KCl (aq)? Why?
no reaction
bromine cannot displace chloride because chloride is more reactive than bromine
68
What happens in the reaction of chlorine water, Br2 (aq) , with potassium bromide solution, KBr (aq)? Why?
no reaction
bromine cannot displace bromide
69
What happens in the reaction of chlorine water, Br2 (aq) , with potassium bromide solution, KI (aq)? Why?
brown solution (I2) is formed
bromine displaces the iodide because it is more reactive than iodide
70
What happens in the reaction of iodine water, I2 (aq) , with potassium chloride solution, potassium bromide solution and potassium iodide?
no reaction
chloride and bromide are more reactive than iodine so the iodine cannot displace them
iodine cannot displace iodide
71
What is the equation for the reaction of chlorine water with potassium iodide solution? What type of reaction is this? What is happening to the electrons in this reaction?
this is a displacement reaction:
Cl2 (aq) + 2Kl (aq) → I2 (aq) + 2KCl (aq)
the electrons are passed from the iodine to the chlorine
each chlorine atom in the Cl2 molecule gains an electron from two negative Cl- ions
Two iodide ions lose an electron each and them form a neutral I2 molecule
chlorine is reduced and iodine is oxidised
72
What is the equation for a the reaction of a metal with **dilute**?
The more reactive the metal, the **faster/slower** the reaction will go - very reactive metals (e.g. sodium) react **...**
What is the speed of reaction indicated by?
metal + **dilute** acid → salt + hydrogen
The more reactive the metal, the **faster** the reaction will go - very reactive metals (e.g. sodium) react **explosively**
the speed of reaction is indicated by the rate at which the bubbles of hydrogen are given off
73
How does magnesium react with **cold dilute** acids?
magnesium reacts vigorously with cold dilute acids and produces loads of bubbles
74
How does aluminium react with **cold dilute** acids? Why? How does aluminium react with **warm dilute** acids?
aluminium doesn't react much with cold dilute acids because it has a protective aluminium oxide layer
but, it reacts vigorously with warm dilute acids and produces a lot of bubbles
75
How do sinz and iron react with cold dilute acids? What happens if you heat them up?
both zinc and iron react slowly with dilute acids but more strongly if you heat them up
76
What is the equation of a metal reacting with steam?
metal + steam → metal oxide + hydrogen
77
As you go down the reactivity series, the reactions with water become **more/less** vigorous
As you go down the reactivity series, the reactions with water become **less** vigorous
78
Hydrochloric acid will always produce **...** salts
Sulphuric acid will always produce **...** salts
Hydrochloric acid will always produce **chloride** salts (e.g. magnesium chloride)
Sulphuric acid will always produce **sulphate** salts (e.g. magnesium sulphate)
79
What is the equation for the reaction of a metal reacting with water?
metal + water → metal hydroxide + hydrogen
80
Very reactive metals, like potassium, sodium, lithium and calcium, will react vigorously with **...**
Less reactive metals, like magnesium, zinc and iron, won't react much with **...** but they will react with **...**
Copper won't react with either **...** or **...**
Very reactive metals, like potassium, sodium, lithium and calcium, will react vigorously with **water**
Less reactive metals, like magnesium, zinc and iron, won't react much with **water** but they will react with **steam**
Copper won't react with either **water** or **steam**
81
What is the order of the reactivity series?
82
More reactive metals will **...** a less reactve metal from its oxide. Why?
More reactive metals will **displace** a less reactve metal from its oxide
this is because it will bond more strongly to the oxygen
83
What is the word and symbol equation for the reaction of iron oxide with aluminium?
iron oxide + aluminium → aluminium oxide + iron
Fe2O3 + 2Al → Al2O3 + 2Fe
84
More reactive metals will **...** less reactive metals in a metal salt (such as sopper sulphate, zinc chloride and sodium chloride)
More reactive metals will **displace** less reactive metals in a metal salt (such as sopper sulphate, zinc chloride and sodium chloride)
85
What is the word and symbol equation for reaction of copper sulphate with iron?
copper sulphate + iron → iron sulphate + copper
CuSO4 + Fe → FeSO4 + Cu
86
What happens if a piece of silver metal is put into a solution of copper sulphate? Why?
nothing happens
this is because the more reactive metal (copper) is already in the salt
87
What are three uses of iron and what property does this depend on?
iron is a strong metal
it is used for building construction, car manufacture and wrought iton garden furniture
88
How is iron galvanised?
a coating of zin is sprayed onto the object
89
How do you prevent rusting on ship's hulls or underground iron pipes?
sacrificial protection: big blocks of zinc can be bolted to the iron
90
How do you prevent rusting on bike chains?
barrier method: oiling/greasing
this is used when moving parts are involved
91
How do you prevent rusting on big and small structures alike?
barrier method: painting/coating with plastic
can be decorative too
92
What is the atmosphere made up of (percentages)?
78% nitrogen
21% oxygen
nearly 1% argon
0.04% carbon dioxide
there can also be a lot of water vapour too
93
What two ways can you investigate the proportion of oxygen in the atmosphere?
using copper
using iron or phosphorus
94
How do you investigate the proportion of oxygen in the atmosphere by using copper? What is the chemical equation for this reaction?
1. when it's heated, copper reacts with oxygen in the air to make coppe (II) oxide - so the reaction uses up oxygen
2. if you heat an excess of copper in a tube and pass air over it using two syringes, you can use the markers on the syringe to tell how much oxygen has been used up
3. if you start with 100cm3 of air, you'll end up with 80cm3 when the reaction is finished and the air has cooled. If 20cm3 air has gone then around 20% of the air must be oxyegn
you need to make sure the system is sealed so no extra air can get in and out
**chemical equation:**
2Cu + O2 → 2CuO
95
How do you investigate the proportion of oxygen in the atmosphere by using iron or phosphorus?
1. Iron reacts with oxygen in the air to form rust - so iron will remove oxygen from the air
2. To do this experiment, first soak some iron wool in acetic acid (the acid will catalyse the reaction). Then push the wool into a test tube, put your thumb over the end and ivert the tube into a beaker of water
3. Over time, the level of the water in the test tube will rise - this is because iron reacts with oxygen in the air to make iron oxide. The water rises to fill the space the oxygen took up
4. To work out the percentage of air that is oxygen you need to mark the starting and finishing position of the water
5. Then, fill the tube up to each mark with water and pour the contents into a measuring cylinder to find out the volume of air at the start and the end
6. Using the difference between the start and end volumes to work out the percentage of the starting volume that has been used up - it should be about 20%
7. You can do a similar experiment with white phosphorus. White phosphorus smoulders in air to produce phosphorus oxide. Calculate the amount of oxygen in the air in the same was as for iron
96
How do you make oxygen, O2, in the lab?
1. It is made using hydrogen peroxide (H2O2)
2. The hydrogen peroxide will decompose into water and oxygen:
2H2O2 (aq) → 2H2O (l) + O2 (g)
3. this decomposition is really slwo but the rate of reaction can be increased with maganese (IV) oxide catalyst - this speeds up the reaction without being used up itself
4. you can collect the oxygen that's produced over water or by using a gas syringe
97
When making oxygen, O2, in the lab, how do you collect the oxygen over water?
you can use a delivery tube to bubble the gas into an upsdie down measuring cylinder or gas jar filled with water
98
When making oxygen, O2, in the lab, how do you collect the oxygen by using a gas syringe?
you can use a gas syringe to collect pretty much any gas, including oxygen
99
Oxides can have either **...** or **...** character
Oxides can have either **acidic** or **basic** character
100
Magnesium burns with a **...** flame in air and **...** that is formed is magnesium oxide
The equation for this is: **...**
Magnesium oxide is slightly **...** when it's dissolved in water
Magnesium burns with a **bright white** flame in air and **white powder** that is formed is magnesium oxide
The equation for this is: **2Mg (s) + O2 (g) → 2MgO (s)**
Magnesium oxide is slightly **alkaline** when it's dissolved in water
101
Carbon will burn in air if it's **...**
It has an **...** flame and it produces **...**
The equation for this is: **...**
Carbon dioxide is slightly **...** when it's dissolved in water
Carbon will burn in air if it's **very strongly heated**
It has an **orangey/yellowy** flame and it produces **carbon dioxide**
The equation for this is: **C (s) + O2 (g)** → **CO2 (g)**
Carbon dioxide is slightly **acidic** when it's dissolved in water
102
Sulphur burns in air or oxygen with a **...** flame and produces **...**
The equation for this is: **...**
Sulphur dioxide is **...** when it's dissolved in water
Sulphur burns in air or oxygen with a **pale blue** flame and produces **sulphur dioxide**
The equation for this is: **S (s) + O2 (g)** → **SO2 (g)**
Sulphur dioxide is **acidic** when it's dissolved in water
103
How can you collect gases in a test tube?
upward/ downward delivery
1. the delivery tube is fed directly into a test tube either upwards of downwards
2. use upward delivery to collect 'lighter than air' gases (e.g. H2)
3. use downward delivery to collect 'heavier than air' gases (e.g. CO2, Cl2)
104
What two ways can you produce carbon dioxide?
reacting dilute hydrochloric acid with calcium carbonate
thermal decomposition of metal carbonates
105
How do you produce carbon dioxide by reacting dilute hydrochloric acid with calcium carbonate?
1. the calcium carbonate (marble chips) is put in the bottom of a sflask and dilute hydrochloric acid is added
2. dilute HCl reacts with the calcium carbonate to produce calcium chloride, water and carbon dioxide gas:
hydrochloric acid + calcium carbonate → calcium chloride + water + carbon dioxide
2HCl (aq) + CaCO3 (s) → CaCl2 (aq) + H2O (l) + CO2 (g)
3. the carbon dioxide gas is collected in a gas syringe or using downward delivery
106
How do you produce carbon dioxide by the thermal decomposition of metal carbonates?
1. heat a metal carbonate (thermal decomposition)
2. copper (II) carbonate is a green powder that will easily decompose to form carbon dioxide and copper (II) ocide when you heat it:
copper (II) carbonate → copper oxide + carbon dioxide
CuCO3 (s) → CuO (s) + CO2 (g)
5. to do this experiment, heat copper (II) carbonate then collect the gas that's given off using the downward delivery method
107
What is thermal decomposition?
when a substance breaks down into simpler substances when heates
108
What are two uses of carbon dioxide?
fizzy drinks
fire extinguishers
109
Expalin the role of carbon dioxide in fizzy drinks
CO2 is used in carbonated drinks to make them fiz
CO2 is slightly soluble in water and dissolves into the drinks when under pressure - this produces a slightly acidic solution due to the formation of carbonic acid:
carbon dioxide + water → carbonic acid
CO2 (g) + H2O (l) → H2CO3 (aq)
when you open the bottle the bubb;es are the CO2 excaping - if you leave the drink out long enough it will go flat because all the CO2 escapes
110
Expalin the role of carbon dioxide in fire extinguishers
carbon dioixide is used in fire extinguishers
CO2 is more dense than air - so its sinks onto the flame sand stops the oxygen the fire needs getting to it
carbon dioxide fire extinguishers are used when water extinguishers aren't safe, for example when putting out electrical fires
111
The temperature of the Earth is a balance between **...** and **...**
The temperature of the Earth is a balance between **the heat it gets from the sun** and **the heat it radiates back out into space**
112
Gases in the atmosphere such as **(name three)** **...** naturally act like **...**
They are often called '**...**'
What do they do?
Gases in the atmosphere like **carbon dioxide, methane and water vapour** naturally act like **an insulating layer**
They are often called '**greenhouse gases**'
They absorb most of the heat that would normallly be radiated out into space, and re-radiate it in all directions - inclusing back towards the earth
113
**...** activity affects the amount of carbon dioxide in the atmosphere - examples include:
1. **...**
2. **...**
**human** activity affects the amount of carbon dioxide in the atmosphere - examples include:
1. **deforestation:** **fewer tress means less CO2 is removed from the atmosphere via photosynthesis**
2. **burning fossil fuels: carbon that was 'locked up' in these fuels is being released as CO2**
114
The concentration of carbon dioxide over the last 200 years has **increased/decreased**. Why?
The concentration of carbon dioxide over the last 200 years has **increased**
CO2 is being released into the air faster than it's being removed
115
What is the increase in carbon dioxide linked to?
climate change which causes:
the average temperature of the Earth is increasing (global warming)
changing rainfall patterns
severe flooding due to the polar ice caps melting and sea level rise
