Group 1,7,0 Topic Test (Periodic Table) Flashcards
1
Q
What are group 1 metas also known as
A
Alkali metals
2
Q
Propoerties of group 1
A
- all have one electron in outer shell so they’re very reactive and gives them similar roperties
- all soft and have low density
3
Q
Trends as you go DOWN group 1
A
- increasing reactivity: the outer electron is more easily lost as the attraction between between the nucleus and electron decrease, because the electron is further away from the nucleus the further down the group you go
- lower melting and boiling points
- higher relative atomic mass
4
Q
How do alkali metals react
A
- they don’t need much energy to lose their one outer electron to form a full outer shell
- its so easy for them to lose their outer electron that they only ever react to form ionic compounds
- these compounds are generally white solids that dissolve in water to form colourless solutions
5
Q
Group 1 reaction with oxygen
A
- react with oxygen to form a metal oxide
- lithium reacts to form Li2O
- sodium reacts to form a mixture of sodium (Na2O) and sodium peroxide (Na2O2)
- potassium reacts to form a mixture of potassium (K2O2) and potassium superoxide (KO2)
6
Q
Group 1 reaction with chlorine
A
- react vigorously when heated in chlorine gas to form white salts called metal chlorides
- as you go down the group, reactivity series increases so the reaction with chlorine gets more vigorous
7
Q
Why do group 1 metals tarnish in the air
A
The metals react with oxygen in the air to form a dull metal oxide layer
8
Q
Group 1 reaction with water
A
- when they’re put in water, they react vigorously
- the more reactive an alkali metal is, the more violent the reaction
- lithium sodium and potassium float and move around the surface, fizzing furiously
- they produce hydrogen. The amount of energy given out when they react increases down the group. For potassium and below in the group, theres enough energy to ignite hydrogen
- they also form hydroxides that dissolve in water to give alkaline solutions
9
Q
Fluorine
A
Very reactive, poisonous yellow gas
10
Q
Chlorine
A
Fairly reactive poisonous dense green gas
11
Q
Bromine
A
Dense, poisonous red-brown volatile liquid
12
Q
Iodine
A
Dark grey crystalline solid or purple vapour
13
Q
What are group 7 elements known as
A
Halogens
14
Q
Trend as you go DOWN group 7
A
- become less reactive - it’s harder to gain an extra electron because the outer shell is further from the nucleus
- have higher melting and boiling points
- had higher relative atomic masses
15
Q
Halogens as molecular compounds
A
- halogen atoms can share electrons via covalent bonding with other non-metas so as to achieve a full outer shell
- for example HCl, PCl5,HF and CCl4 contain covalent bonds
- the compounds that form when halogens react with non metals all have simple molecular structures
16
Q
Halogens reacting with metals
A
- the halogens form 1- ions called halides when they bond with metals
- the compounds that form have ionic structures
17
Q
More reactive halogens will displace less reactive ones
A
- a displacement reaction can occur between a more reactive halogen and the salt of a les reactive one
18
Q
What are group 0 elements known as
A
Noble gases
19
Q
Proeoprties of group 0
A
- they all have full outer shells
- as their outer shell is energetically stable they don’t need to give up or gain electrons to become more stable. This means they are more or less inert (they don’t react with much at all)
- all exist as monatomic gases - single atoms not bonded to each other
- all are colourless gases at room temperature
- all non-flammable
20
Q
What is inert
A
Don’t react
21
Q
Patterns in properties of noble gases
A
- boiling points of the noble gases INCREASE as you go down the group
- the increase in boiling point is due to an increase in the number of electrons in each atom leading to greater intermolecular forces between them which need to be overcome
22
Q
Lithium reaction with oxygen
A
Burns with a strongly red-tinged flame and produces a white solid
23
Q
Sodium reaction with water
A
Strong orange flame and produces white solid
24
Q
Potassium reaction with oxygen
A
Large pieces produce lilac flame, smaller ones make a solid immediately
25
Lithium reaction with water
Fizzes steadily, gradually disappears
26
Sodium reaction with water
Fizzes rapidly, melts into a ball and disappears quickly
27
Potassium reaction with water
Ignites with sparks and a lilac flame, disappears very quickly
28
Lithium reaction with chlorine
White powder is produced and settles on the sides of the container
29
Sodium reaction with chlorine
Burns with a bright yellow flame, clouds of white powder are produced and settles on on the sides of the container
30
Potassium reaction with chlorine
Reaction is even more vigorous than with sodium
31
Chlorine reaction with potassium bromide
Pale green to orange
32
Chlorine reaction with potassium iodide
Pale green to brown
33
Bromine reaction with potassium iodide
Orange to brown
34
Fluorine use
Used in toothpaste to prevent decay
35
Bromine use
Used in some types of fire extinguishers that don’t use water
36
Iodine use
Used in photographic chemicals to produce a visible image
37
Chlorine use
Used as a disinfectant added to drinking water
38
Helium use
- A gas for inflating balloons and airships because it’s less dense than air and inflammable
- a component of breathing gas for deep sea divers because it is unreactive, insoluble and prevents divers getting ‘the bends’
- a super coolant for high performance magnets eg. In body scanners because it has a very low boiling point
39
Argon use
- In normal lights, because it’s unreactive and prevents the tungsten filament from burning
- in energy efficient fluorescent light bulbs
- as a gas blanket for arc welding because it is unreactive and prevents the hot welding metal from oxidising
40
Neon use
- in certain types of lasers
- As a cryogenic refrigerant
- in neon advertising signs because it glows red when an electric current is passed through it
- In Tvtubes
