Electron Affinity
When an element undergoes a chemical reaction, it either gains energy or loses energy. This gain or loss of energy is due to the phenomena that occur at atomic level. During reaction, atoms either gain electrons from other atoms or lose electrons to other atoms, and in that process, energy is produced.
P-Block Elements
Elements which are present on the right side of the periodic table are called p-block elements. In addition to the noble gases, they include the families of boron, mercury, nitrogen, oxygen and fluorine. These elements have diverse real-life implementations that we regularly experience around us.
Metals and Non-metals
The periodic table is composed of metals, semi-metals and nonmetal elements. The physical and chemical properties of metals and nonmetals differ from each other. The study of metals and nonmetals will help one to understand the appropriate application of the particular element.
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Give a description of the kinds of ions that are expected to form by group : 1A, 2A, 6A, 7A elements.
According to the long form of periodic table:
Group 1 A metals are alkali metals which have general electronic configuration ns1. They loose one electron to attain the electronic configuration of noble gas and form unipositive ion. This ion reacts with non metals to form ionic compounds. E.g. Lithium, sodium, potassium, rubidium and Caesium are group 1A elements.
Group 2 A metals are alkaline earth metals which have general electronic configuration ns2. They loose two electrons to attain the electronic configuration of noble gas and form dipositive ion. This ion reacts with non metals to form ionic compounds. E.g. beryllium, magnesium, calcium, strontium and barium are group 2A elements.
Group 6A are chalcogens (ore forming) which have general electronic configuration ns2np4. They gain two electrons to attain the electronic configuration of the noble gas and form a doubly charged negative ion. The doubly charged negative ion reacts with positive metal ion forming ionic compound. E.g. oxygen, sulfur, selenium, tellurium, polonium are group 6A elements.
Group 7A are halogens (salt forming) which have general electronic configuration ns2np5. They gain one electron to attain the electronic configuration of the noble gas and form a singly charged negative ion. The singly charged negative ion reacts with positive metal ion forming ionic compound. E.g. fluorine, chlorine, bromine, iodine and astatine are group 7A elements.
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