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Transition Elements and Their Property

1. Transition metal is a block of metallic elements in between Groups 2 and 13 in the Periodic Table.
2. They are much less reactive than the alkali metals.
3. They do not react as quickly with water or oxygen as alkali metal.

General Physical Characteristics

All transition elements are metals. Therefore they have the all the physical properties of metal such as:

1. high melting point and boiling point
2. hard,
3. high density,
4. high electrical conductivity,
5. high tensile strength ,
6. shinny surfaces,
7. ductile
8. malleable ,

High Melting Point and Boiling Point

1. The bond between atoms of metal is called metallic bond and usually it is a very strong bond.
2. Thus all the transition metals have high melting points and boiling points.
3. For example: iron melts at 1535°C and boils at 2750°C.
4. Mercury is a transition metal, but with unusual low melting point ( − 39°C).

Special Properties of Transition Elements
Form Coloured Compounds and Ions in Solute

1. Transition elements tend toform coloured compounds either in solid form or dissolved in a solvent.
2. Table below shows the colours of some aqueous solutions of ions of transition elements.

Catalytic Properties

1. Transition elements or their compounds have catalytic properties.
2. A catalyst is a substance that speeds up a reaction but it itself does not change chemically after a reaction.
3. Many transition metals are used directly as catalysts in industrial chemical processes.

Variable Oxidation State

1.  transition metal can have a variable oxidation state, which means it can form more than one ion.
2. For example, iron(II), Fe2+ and iron(III) Fe3+; copper(I), Cu+ and copper (II) Cu2+.

Forming Complex Ions

1. Transition elements can form complex ions.
2. A complex ion is a polyatomic ions (positive or negative) consisting of a central metal ion with other groups bonded to it.

Chemical Properties Change Across a Period

1. There is gradual chemical change across a period.
2. The acidity (or basicity) of the oxide of element changes across a period.
3. The metallic properties, the electronegativity of element also change across a period.

Acidic Oxide or Basic Oxide

From left to right across a period the oxides change from alkaline/basic (with metals e.g. Na₂O) to acidic (with non-metals e.g. SO₂).

Metal, Metalloid and Non-metal

1. As we go across a period from left to right, the elements change from metals to non-metals.
2. There are about 7 elements in the periodic table are classified as semi-metals.
3. The metals in the periodic table are mainly found in the left hand columns (Groups 1 and 2) and in the central blocks of the transition elements.
4. On the right hand side of the periodic table, there are 7 semi-metals form a staircase like pattern, act as a divider between metal and non-metal.
5. The semi-metals are also called the metalloid.

Uses of Metalloids

1. The most widely used semi-metals are silicon and germanium.
2. It is used to make diodes and transistors in electronic industry.

Electronegativity

1. Electronegativity is a measure of the potential of atoms to attract electrons to form negative ions.
2. Metals have low electronegativities.
3. Non-metals have high electronegativities.
4. Electronegativities of the elements increase across a period with increasing proton number. This is because
1. as the proton number increases, the positive charge of the nucleus will increase accordingly.
2. this will increase the ability of the atom to attract electrons from the surrounding and thus increase the electronegativity of the atom.

The Periods

1. Period is the horizontal rows of elements in the Periodic Table.
2. The modern periodic table has 7 periods.
3. The period number indicates the number of electron shell.
4. Elements in the same period have same number of electron shells.
5. The proton number of elements increases from left to right crossing the period.
6. The number of electrons is also increases from left to right crossing the period.

Lanthanide and Actinide Series

1. The sixth period has 32 elements. Due to short of space, 14 elements in the transition metal group are removed from the same horizontal row and is placed below the main table, These elements are called the Lanthanide Series.
2. The seven period also has 32 elements. With the same reason, 14 elements are removed from the same horizontal row and is placed below the main table, These elements are called the Actinide Series.

Explaining the Reactivity Trend of the Halogens

1. The reactiveness of halogens decreases down the group.
2. This can be explained as below:
1. When a halogen atom reacts, it gains an electron to form a singly negative charged ion.
2. As we go down the group from F => Cl => Br => I, the size of the atom increases due to an extra filled electron shell.
3. The valence electrons are further and further from the nucleus, the attraction force between the electrons and the nucleus become weaker and weaker.
4. Therefore the ability of the atom to attract electron to fill the outermost shell reduces., which means the reactiveness of the atom reduces.