C4.1
Predicting chemical reactions of the noble gases
Summary
Models of
how substances react and the different types of chemical reactions that can
occur enable us to predict the likelihood and outcome of a chemical reaction.
The current periodic table was developed based on observations of the
similarities and differences in the properties of elements. The way that the
periodic table is arranged into groups and periods reveals the trends and
patterns in the behavior of the elements. The model of atomic structure
provides an explanation for trends and patterns in the properties of elements.
The arrangement of elements in groups and periods reveals the relationship between
observable properties and how electrons are arranged in the atoms of each
element.
Common
misconceptions
Learners
consider the properties of particles of elements to be the same as
the bulk
properties of that element. They tend to rely on the continuous matter model
rather than the particle model. Learners confuse state changes and dissolving
with chemical changes. Also, since the atmosphere is invisible to the eye and
learners rely on concrete, visible information, this means they therefore often
avoid the role of oxygen in their explanations for open system reactions. Even
if the role of oxygen is appreciated, learners do not realize that solid
products of an oxidation reaction have more mass than the starting solid.
Underlying
knowledge and understanding
Learners
should be familiar with the principles underpinning the Mendeleev periodic
table; the periodic table: periods and groups; metals and non-metals; the
varying physical and chemical properties of different elements; the chemical
properties of metals and non-metals; the chemical properties of metal and
non-metal oxides with respect to acidity and how patterns in reactions can be
predicted with reference to the periodic table.
C4.1a-b
To recall the simple properties of Group 0, both physical and chemical
properties.
To be able to explain how observed simple properties of Group 0 depend on
the outer shell of electrons of the atoms and predict properties from given
trends down the groups including the ease of electron gain or loss.
Group 0 elements are the noble gases.
Structure
You can see that all noble gases are monomolecular. Unlike halogens, which are all bimolecular,
Noble gas atoms do not bond to each other covalently.
Noble gas atoms exist independently from one another.
Bonding
Each atom bonds weakly to others via an induced dipole or London force.
The movement of electrons in the atom gives rise to an imbalance of
electrons and a temporary or flickering dipole.
The more electrons in the Noble gas atom then the stronger is this
temporary dipole.
What’s more this dipole can then induce a dipole in another atom.
Melting and
boiling points
As a result of this increase in the number of electrons per atom, the interatomic
induced dipole forces increase down the group and therefore there is more
energy required to separate these atoms and so the melting and boiling points
increase going down the group.
Inertness
Most courses suggest you think about the inertness or the un-reactivity of
the noble gases.
You can see from the table that all the noble gases have full outer
electron shells.
The noble gas atoms it seems can neither share electrons to fill their
outer shells nor lose or gain electrons in order to form ions and bond
electrostatically with another element.
This is true for Helium, Neon and Argon.
But Krypton with four electron shells and Xenon with five etc. are able to
accommodate more than eight electrons in their outer shells leading to the
formation of compounds with the very electronegative non–metals like fluorine
and oxygen.
For example XeF4 Xenon tetrafluoride the first noble gas
compound to be made. The video below is from the Chem study program and discusses the formation of inert gas compounds. It shows samples of XeF4 and the properties of XeO3. You can tell of course that the video clip is from 1963!!.
As this video clip shows there are more than eight electrons in the Xenon
outer shell.
Density
Noble gas densities provide substance (!) to the proverbial lead balloon
since Xenon is over eight times denser than air. Density of air is 1.275 g/dm3 and
Xenon has a density of 9.97 g/dm3
As this video shows Xenon sinks in air!!
The increased density going down the group is further evidence of stronger
inter–atomic forces down the group.
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