Group 0 (noble gases)
Lajoy Tucker
Teacher
Contents
Introduction
The elements in Group 0 of the periodic table are called the noble gases.
They include helium , neon , argon , krypton , xenon and radon .
All are non-metals and exist as single atoms (monatomic gases).
Electron Structure and Stability
Noble gases have full outer electron shells, which makes them very stable and therefore chemically inert (unreactive).
This stability means they do not easily gain, lose or share electrons.
Because of this, they rarely form molecules or compounds.
Element | Electron Structure |
Helium | 2 |
Neon | 2,8 |
Argon | 2,8,8 |
Trends Down the Group
As you go down Group 0 the boiling points increase, this is because the atoms get larger and the intermolecular forces between them become stronger, so more energy is needed to separate them.
Element | Relative Atomic Mass | Boiling Point (°C) | Trend |
Helium | 4 | -269 | Lowest |
Neon | 20 | -246 | |
Argon | 40 | -186 | |
Krypton | 84 | -152 | |
Xenon | 131 | -108 | Highest |
Practice Questions
Question 1
Why is helium unreactive?
Answer
Helium has a full outer shell with 2 electrons, so it is stable and does not need to gain or lose electrons.
Question 2
A noble gas is discovered below xenon in Group 0.
Predict its relative atomic mass, boiling point and reactivity compared to xenon.
Answer
It would have a greater relative atomic mass.
It would have a higher boiling point.
It would still be unreactive, as it would have a full outer electron shell.
Summary
Group 0 elements are unreactive (chemically inert) gases with full outer shells.
Boiling points increase down the group because atomic size and intermolecular forces increase.
You can predict trends down the group using their position in the periodic table.
No answer provided.