what is the relationship between behaviour of gases,atomic structure and chemical bonding?

Answer 1

Your question is a touch vague.

Almost all compounds and elements can exist as gasses, providing that the correct temperature and pressures exist.

Atomic structure is a function of the atomic number and atomic mass.

Chemical bonding is a function of the electronic configuration of the atom. The probability shell of an atom or ion is a function of the atomic number of the atom and the ionization state of the atom.

Also all three are investigated by physical and theoretical chemists.

Ken

Answer 2

I'm not sure what do you mean by the behaviour of gases... but..

The atomic structure of an element decides the chemical property of an element. Basically the elements follow the following electronic structure trend: 1s 2s 2p 3s 3p 3d 4s 4p 4d 4f......

the number is the electron shell number, while the s, p, d, f are the orbitals. Electrons will fill up the orbitals, each orbital can contain 2 electrons of opposite spin. The number of the outer shell electrons decide its chemical property. In the case of Oxygen, it would be 1s2 2s2 2p4. Therefore, oxygen has 6 outer shell electrons.
S orbital can takes in 1X2=2 electrons
P orbital: 3X2=6
D orbital : 5X2=10
F orbital : 7X2=14

Elements with 4 or more outer shell electrons (valence electrons) tend to form bonds by gaining electrons. This is because they have to gain the stable octet electronic structure of noble gases (which have 8 outer shell electrons), they do not lose the electrons because less energy is needed to gain the electrons.

While elements with less valence electrons tend to lose the electrons to gain the noble gas' electronic structure, because there is less energy change with losing electrons.

Ionic bondings are formed when, say, Na and Cl. form bonds. The Na tends to lose the 1 valence electrons while Cl will gain that electron.

Covalent bonds are formed between non-metals because the atoms, having more valence electrons, will have their electron orbital overlapped, thus achieving the noble gas structure by sharing their electrons. Cl2, O2... are such examples.

Some gases are more volatile (if you mean boiling point melting point... etc.) because the intermolecular force between them is weak, thus less energy is required to separate them further. Some gases are polar and other are non-polar. The polar gases needs more energy to boil because there is stronger intermolecular forces.

The boiling points of non-polar molecules depend on the size of electron cloud. Generally the larger the electron cloud the larger the intermolecular force.

Answer 3

Physics

Answer 4

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Answer 5

your question.