Periodic Table

Runs horizontally from left to right

Numbered from 1-7

Number of electron shells is the same as period number

Elements changes from Metals to Non-Metals Across the Period

METALS

Transition Metals (E.g. Cr, Mn, Fe, Cu)

Found between Group II and III

Properties

Transition Metals have high melting and boiling points and high densities

Transition Metals have variable oxidation states

Transition Metals form coloured compounds

Colours of the compounds of a transition metal are different at different oxidation state

Colour of hydrated compounds may differ from anhydrous compound

Compounds of transition metals are used in dyes, pigments and paints to produce different colours

Transition metals and their compounds are good catalysts

Iron - Haber process for the manufacture of ammonia

Nickel - Manufacture of margarine from vegetable oil

Group I Metals - Alkali Metals (E.g. Li, Na, K, Rb)

Properties

Physical Properties

Soft, easily cut

Shiny and Slivery when freshly cut

Good conductors of heat and electricity

Low melting and boiling points

Low densities

Trends in physical properties

Melting and boiling points decrease down the group

Densities increase down the group

Chemical Properties

Alkali metals are very reactive

Sodium tarnishes easily in air to form an oxide

Stored in oil to prevent reaction with air and moisture

Reacts with cold water to form alkali and hydrogen gas

Reactivity increases down the group

Alkali Metals are good reducing agents

Each alkali metal loses its valence electron easily to attain a noble gas structure

Group I Elements

React with water to form alkalis

Also known as alkali metals

Contain one electron each in their valence shells

NON-METALS

Group VII (Halogens)

Physical Properties

Low melting and boiling points

Coloured

Melting and boiling points increases down the group

colour intensity increases down the group

Chemical Properties

Have 7 electrons in their valence shell

Reactive with a high tendency to attract one more electron

To attain stable octet configuration

Exist as covalent, diatomic molecules

Halogens react with most metals to form halides

Halogens are powerful oxidising agents

Each halogen atom only needs to gain 1 addictional electron to attain a noble gas structure, forming a negative ion

Halogens undergo displacement reactions

Chlorine, the most reactive halogen displaces bromine from sodium bromide solution

As it goes down group VII, reactivity and oxidising power decreases

About Group VII Elements

Non-metals

React with metals to form salts

Known as Halogens

Have 7 electrons each in their valence shells

Group 0

Physical Properties

Colourless and Odourless at Room Temperature

Very low melting and boiling points

Insoluble in water

Chemical Properties

Chemically unreactive

do not gain, lose or share electrons

do not form compounds

exists as monatomic gases

About

Non-metals

Form 1% of the Earth's Atmosphere

Also known as noble or inert gases

Run vertically from top to bottom

Numbered from I to VII and O

Number of valence electrons is the same as group number

Charge of ion is related to group number