The Nature of matter, atomic structure and the periodic table

Solid (s) particles are strongly attracted to one another and are arranged in a lattice form. Thus, they keep their own shape.

Solid particles can easily move around within the solid.

A solid cannot be compressed.

The attractive forces between liquid particles is more easily broken since the particles have more kinetic energy. This means they are more mobile than solid particles - liquids can flow, but still take the shape of their container.

Particles at the surface of a liquid can break away and escape - a liquid can evaporate.

There is a vast space between the particles in a liquid, so they can easily be compressed.

Gas particles have even more kinetic energy than liquid particles and there is very little attraction between them. The particles move at very high speeds and independently of one another, so they fill any available space.

Gas particles collide with the surface of their container and exert pressure (force per unit area)

Gases do not mix readily with other gases, because of the particle's rapid motion.

As matter is heated, the particles gain kinetic energy, transferred from heat energy, and so are able to move faster.

As a solid is heated, the vibrations of its particles decrease, until eventually the particles are able to break away from each other into a sparse collection.

The temperature at which all solid becomes liquid is the solid's melting point.

Similarly, the particles in a liquid move faster as they are heated, until the particles break free of the liquid to become a gas. This temperature is called the liquid's boiling point.

The electrons are found only in distinct energy levels.

The energy levels are located at fixed distances from the nucleus.

They have counseling.

There is the same amount of neutrons, protons and electrons in the atom.

Each energy level only has up to a certain amount of electrons. These can not be empty, nor can they have any more electrons than they allow.

Level 1 = Max. 2

Level 2= Mass. 8

Level 3= Mass 16

Level 3= Mass 8

Level 4= Mass 32

Level 4= Mass 2

A characteristic property of metals is their ability to lose electrons to form positive ions with a stable octet of electrons.

For metals with only one valence electron, the atom requires only a small amount of energy of remove the electron from the attraction of the nucleus.

For metals with two or three valence electrons, it requires more energy to remove the valence electrons.

Group 1 - Alkaline metals
These elements have one valence electron. This is easily removed, so the elements are not very reactive.
Their atoms undergo reactions where they lose the valence electron to from positive ions with a +1 charge

Group 2- Alkaline earth metals
These elements have two valence electrons. Removing these requires more energy, because there is greater attraction to the nucleus.
Their atoms undergo reactions where they lose the two outer electrons to form positive ions with a +2 charge

Group 17- The Halogens
These elements have 7 valence electrons, just 1 short of a stable 'octet'. Their atoms readily undergo reactions where they gain an electron to form negative ions with a -1 charge.

(2,4,6,5)

(2,8,7)

(8,2,7)

(2,8,8)