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The periodic table consists of eight groups, each unique from the other groups. Therefore, to understand the periodic table correctly, you need to learn about the properties of groups. Luckily, you don't need to study all the groups. According to the GCSE syllabus, you must study a few groups, including group 0. This resource is made especially for group 0 and its properties.
What is Group 0?
Group 0 is one of the groups in the periodic table. It is the last group of the periodic table that you can find on the right side. Another name for Group 0 is Group 8. The elements in group 0 are known as noble gases. There are some reasons why group 0 elements are called noble gases, and those reasons are:
- All elements are in gaseous form.
- They are single atoms.
- They are inert.
Due to these reasons, they are called noble gases. Noble gases have their own properties, making them different from other groups; let's look at those properties.
Properties of Noble Gases
Noble gases have a valance shell filled with electrons. This means that noble gases do not participate in the chemical reaction, and since noble gases do not react, noble gases don't form ions. That is why noble gases are inert. You won't see helium reacting with any other chemical.
Noble gases have their valance shells filled, meaning they don't need to donate or accept an electron. Hence, they exist in a monatomic state. A monatomic state means a single atom; for example, oxygen exists in a diatomic state, i.e. O2, because oxygen needs two electrons to complete its valance shell. However, in the case of noble gases, their shells are filled, and they don't need electrons; hence, they exist in a monatomic state. Noble gases are colourless and non-flammable and gases at room temperature.
Electronic Configuration of Noble Gases
Furthermore, the periodic table also tells about electronic configuration. Group zero will always have its shell wholly filled; it is called group 8 because, except helium, all elements in group 8 have eight electrons in the valance shell.
How do we know that? The group number always tells how many electrons are in the valance shell. Usually, you will see group 8, but in case you see group 0, now you know that group 0 is another name, group 8.
One thing is clear: group 0 has its valance shell filled; now, you must find how many shells are required. There are two ways; the first is to make the electronic configuration of the noble gas. For example, neon has a proton number of 10. Start making the electronic configuration. If you don't know how to make an electronic configuration, you can check our previous post, which explained how to do so in detail. You can go there directly by clicking this link.
If you are reading this paragraph, you know how to make electronic configurations, but for better understanding, let's do a quick revision. The first shell requires 2 electrons, and the rest requires 8 electrons. An element has an infinite amount of shells. Start filling electrons according to the shell.
In the case of neon, fill the first shell with two electrons and subtract two from the proton number. Then, fill eight electrons and subtract eight from the proton number. Keep doing the last step until you get the proton number zero.
Neon's proton number = 10
Electronic configuration of Ne = 2 (first shell filled, remaining electrons = 10 - 2 = 8)
Electronic configuration of Ne = 2, 8 (first and second shells filled, remaining electrons = 8 - 8 = 0)
Therefore, the electronic configuration of neon is 2, 8. Did you notice the eight electrons in the valance shell? Coincidence? Nope, all the group 0 has eight electrons in their valance shell; just for discussion, we will make an electronic configuration of argon.
The proton number of argon is 10. Use the above method again to make the electronic configuration of argon.
Argon's proton number = 18
Electronic configuration of Ar = 2 (first shell filled, remaining electrons = 18 - 2 = 16)
Electronic configuration of Ar = 2, 8 (first and second shells filled, remaining electrons = 16 - 8 = 8)
Electronic configuration of Ar = 2, 8, 8 (first, second, and third shells filled, remaining electrons = 8 - 8 = 0)
Hence, the electronic configuration of argon is 2, 8, 8. This proves that every member of group 8 has its valance shell filled. Most elements (except helium) have eight electrons in their valance shell. Helium has two electrons in the first shell, yet it is considered a member of group 8 because its valance shell is complete and has the same properties as other noble gases.
The second method is to count the periods. Several periods tell you the number of shells. For example, neon is in the 2nd period, meaning it has two shells, and since it is a member of group 0, it has all electrons filled in a valance shell. The same goes for every element in group 8. Below is the electronic configuration of all group 0 members.
He = 2
Ne = 2, 8
Ar = 2, 8, 8
Kr = 2, 8, 8, 8
Xe = 2, 8, 8, 8, 8
Uses of Noble Gases
Noble gases are inert, but this doesn't mean they are useless. There are a lot of applications of these gases. Below are the uses of noble gases:
- Argon is widely used to make an inert atmosphere in metallurgical processes.
- Helium is used in nuclear reactors as a cooling gas.
- Neon is widely used in making high-quality, colourful lights.
- Argon is also used as a carrier gas in gas chromatography.
- Radon is used in radioactive research.
- Krypton is used in photographic flashes because of its bright light nature.
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Lithium is used in place of Fluorine
Hi Madan. You’re right to point that out – thanks very much for your comment!
amazing side
It’s very educative,I learnt alot thanks ❤️
Was very educative and help. Gave me a broader understanding of the topic