Things to note for (N03) The Periodic Table:
1. General points about the Periodic Table
2. Group I elements (Alkali metals)
Example: When sodium reacts with water, the reaction should be:
sodium + water → sodium oxide + hydrogen
BUT because sodium oxide is soluble in water, the reaction will then be:
sodium + water → sodium hydroxide + hydrogen
1. General points about the Periodic Table
- The elements in the Periodic Table are arranged in increasing order of proton number.
- The Group number indicates the number of valence electrons of an atom of the element.
- The Period number indicates the number of occupied shells of an atom of the element.
- Elements are placed in different groups because of the number of valence electrons they possess.
- Elements in the same group will have the same chemical properties due to the same number of valence electrons they posses. Hence they react in the same way.
- No. of valence electrons = No. of electrons in the outermost shell
- Valency of an element = No. of electrons involve in a reaction regardless whether the electrons are gained or lost
- Charge is written as, for example '3+', '2-', with the quantity first, followed by the +/- sign.
- Reactivity of an element is related to how readily it forms an ion. Higher the tendency to form a stable ion, more reactive will be the element. The reaction of reactive elements will also appear to be more vigorous or violent.
- Tendency to form a stable ion, depends on the distance between the nucleus and the valence electron, which will in turn affect the forces of attraction between the nucleus and the valence electrons.
- (By convention) When naming or writing the chemical formula the compounds consisting of a metal and non-metal, the name of the metal will come first, followed by the non-metal. The name of the metal remains the same, while that of the non-metal will change.
2. Group I elements (Alkali metals)
- The elements consist of only 1 valence electron.
- Melting and boiling point decreases down the group.
- Density increases down the group.
- In order to form a stable ion, the elements tend to lose 1 electron to form a positively charged ion. Therefore, valency will be 1.
- Reactivity increases down the group. (Fr is the most reactive metal.)
- Group I metal reacts chlorine to produce metal halide.
- Group I metal reacts with water to produce metal hydroxide and hydrogen.
Example: When sodium reacts with water, the reaction should be:
sodium + water → sodium oxide + hydrogen
BUT because sodium oxide is soluble in water, the reaction will then be:
sodium + water → sodium hydroxide + hydrogen
- Most Group I metal compounds are white solids and when dissolved in water they form colourless solution. THERE IS NO WHITE SOLUTION.
3. Group VII elements (Halogens)
4. Group 0 elements (Noble gases)
credit:
some of the above points came from questions or comments contributed by students, from 3E4 and 3E5, who came for consultation on Saturday (27 March '10).
- The elements consist of only 7 valence electrons.
- They exist as diatomic molecules, 2 atoms per molecule.
- Melting and boiling point increases down the group.
- Density increases down the group.
- Colour of the element darkens down the group.
- In order to form a stable ion, the elements tend to gain 1 electron to form a negatively charged ion. Therefore, valency will be 1.
- Reactivity decreases down the group. (F is the most reactive non-metal.)
- Group VII elements can undergo displacement reactions, whereby the more reactive element displaces the less reactive element from its salt solution.
4. Group 0 elements (Noble gases)
- The elements consist of a stable electronic configuration also known noble gas configuration.
- They exist as monoatomic atoms, individual.
- Melting and boiling point increases down the group.
- They are unreactive due to their stable electronic configuration.
credit:
some of the above points came from questions or comments contributed by students, from 3E4 and 3E5, who came for consultation on Saturday (27 March '10).
------------------------------ Part 1: Elements and their reactions --------------------------------
Video 1: (Group I elements) Alkali metals and their reactions with water
Video 2: Alkali metals and their reaction with water (with Universal Indicator).
Video 3: (Group VII elements) Halogens and their reactions
* For more videos related to reactions of the elements in the Periodic Table:
http://www.periodicvideos.com/ (by the University of Norttingham)
Video 1: (Group I elements) Alkali metals and their reactions with water
Video 2: Alkali metals and their reaction with water (with Universal Indicator).
Video 3: (Group VII elements) Halogens and their reactions
* For more videos related to reactions of the elements in the Periodic Table:
http://www.periodicvideos.com/ (by the University of Norttingham)
In the presence of Universal Indicator, water will appear to be green in colour as it is neutral. However, when a Group I metal is placed in it, the Group I metal hydroxide will be produced. Thus, changing the colour from green to blue/purple. This is because the metal hydroxide which is formed is alkaline in nature.
For Universal Indicator:
pH 1 (Acidic): Red
pH 7 (Neutral): Green
pH 14 (Alkaline): Purple