9th Science NCERT Chapter 3
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– Molecules of Compounds: Atoms of different elements join together in definite proportions to form molecules of compounds. Students should learn the symbols and combining capacity of elements to understand how atoms combine to form compounds.
– Writing Chemical Formulae: Students should understand how to write the chemical formula of a compound, ensuring that the valencies or charges on the ions balance to create a neutral structure. They should also be able to write formulae for simple compounds using the valencies of ions provided in tables【4:0†source】.
– Atomicity and Molecular Mass: Students should grasp the concept of atomicity of elements and understand how to calculate molecular masses by summing the atomic masses of all atoms in a molecule. This knowledge helps in determining the relative mass of a molecule expressed in atomic mass units【4:2†source】.
– Formula Unit Mass: Understanding how to calculate the formula unit mass of substances, particularly for ionic compounds, is important. This involves adding up the atomic masses of all atoms in a formula unit of a compound, similar to calculating molecular mass【4:4†source】.
Define the atomic mass unit.
The atomic mass unit is a unit of mass used to express atomic and molecular weights, equal to one-twelfth of the mass of an atom of carbon-12.
Why is it not possible to see an atom with naked eyes?
Atoms are very small, smaller than anything that can be seen with naked eyes. Even when stacked in millions, they would barely make a layer as thick as a sheet of paper.
What is meant by the term chemical formula?
A chemical formula is a notation used to represent the types and numbers of atoms in a pure substance or molecule. It shows the elements present in the substance and their proportions.
How many atoms are present in a (i) H2S molecule and (ii) PO4^3− ion?
(i) In an H2S molecule, there are 3 atoms: 2 hydrogen atoms and 1 sulfur atom. (ii) In a PO4^3− ion, there are 5 atoms: 1 phosphorus atom and 4 oxygen atoms.
In a reaction, 5.3 g of sodium carbonate reacted with 6 g of acetic acid. The products were 2.2 g of carbon dioxide, 0.9 g water, and 8.2 g of sodium acetate. Show that these observations are in agreement with the law of conservation of mass.
The law of conservation of mass states that in a chemical reaction, the total mass of the reactants is equal to the total mass of the products. By calculating the masses of reactants and products in this reaction, it can be shown that the total mass before the reaction equals the total mass after the reaction, thereby confirming the law of conservation of mass.
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