CHEMY.4M2.5PERIODIC CLASSIFICATION

PERIODIC CLASSIFICATION

PERIODIC TABLE

Is the chart  table which shows the arrangement of elements in order of increasing atomic numbers in such a way that elements with similar properties fall in the same vertical column.

PERIODIC LAW

States that “The properties of elements are periodic function of their atomic number in the periodic table”.

Periodicity –

These are regular periodic changes of elements due to their atomic number

In the periodic table; elements are arranged in groups and periods.

1.    PERIODS –

Are the horizontal row of elements in the periodic table.

2.    GROUPS –

 Are the vertical columns of elements in the periodic table.

GROUPS:

There are eight groups in the periodic table.Groups are usually indicated by roman number eg. I, II,III,IV, V, VI, VII, VIII.

Its important to note that the group number signifies the number of electrons in the outer most shell. The group are numbered from left to right.

NOTE:

Lanthanide series are part of period 6 ,Actinides series are part of period 7.

PERIODS:

These are seven horizontal rows in the periodic table. Periods are usually indicated in normal numbers eg , 1,2,3,4,5,6,7,. It is important to note that elements with the same number of shells belong to the same group.

                    Properties of element within a group

Group 1 elements (Alkali metals)

                     i.        They are known as Alkali metals , they include Li, Na, k

                    ii.        They are called alkali metals because they all react with water to form alkali.

                   iii.        They have one electron in their outer most shell.

Group 2 elements (Alkaline earth metals)

     i.        They are called alkaline earth metals because their oxides are alkaline in nature and exist in earth eg, Be, Mg, Ca ,they have 2 electrons in their out most shell.

    ii.        They are called alkaline earth metals because their oxides are alkaline in nature and exist in earth eg, Be, Mg, Ca ,they have 2 electrons in their out most shell.

Group 7 elements (Halogens)

     i.        Are called halogens because they react with metals to form salt.

    ii.        They have seven electrons in outer most shells eg chlorine, fluorine

Group 8 element (Noble gases)

     i.        These elements are very stable. Their outer most shells are full of electrons.

    ii.        They have 8 electrons in their outer most shell.

General periodic trends

The trends observed include variations in:

                      i.        Melting point - This is the temperature at which a solid melts to form liquid.

                    ii.        Boiling point - This is a temperature at which a liquid boils form a gas.

                   iii.        Density - This is mass per unit volume of a substance.

                  iv.         Electronegativity -Ability of an atom to attract an electron.

                   v.        Ionization energy - This is the energy required to remove electron from an atom or ion.

                  vi.        Atomic radius - This is the distance between the nucleus of an atom and the outer most stable energy level.

Trends across periods

1). The atomic radius of element in a period decrease from left to right

2). Elements to the left of the periodic table show metallic properties while elements to the right show non-metallic properties.

3). Electronegativity increases from left to right

4). The number of electrons and protons increase from left to right

5). The physical states of elements at room temperature 20°c move from solid to gas

General group trends

1). Atomic radius increases down the group as successive energy levels are filled.

2). Densities increase down the group.

3). Melting point decreases down the group as the element becomes less metallic in nature.

4). Electronegativity and ionization energy decrease down the group.

TRANSITION METALS

Properties;

1. They are denser metals.

2. They are strong high melting point.

3. They form colored compound.

35. Electronegativity increases from left to right

4). The number of electrons and protons increase from left to right

5). The physical states of elements at room temperature 20°c move from solid to gas.

General group trends

1). Atomic radius increases down the group as successive energy levels are filled.

2). Densities increase down the group.

3). Melting point decreases down the group as the element becomes less metallic in nature.

4). Electronegativity and ionization energy decrease down the group.

TRANSITION METALS

Properties;

1. They are denser metals.

2. They are strong high melting point.

 3. They form colored compound.

4. They form insoluble oxide hydroxide.

5. They can show the number of valency state (oxidation state) (have variable valency).