Some Basic Concepts of Chemistry

This is a mind map on Some Basic Concepts of Chemistry Made by Aditya Singh. I hope this will help you in your studies.

Edited at 2021-06-15 03:35:52

Aditya Singh

Some Basic Concepts of Chemistry

Aditya Singh

Recommended to you
Outline

Basic Concepts of Chemistry

Mole Facts

1 Mole = Atomic/Molecular weight of element/compound (in grams)

1 Mole of atoms

Gram Atomic Mass

6.022×1023

1 Mole of Molecules

Gram Molecular Mass

22.4L at S.T.P.

6.02×1023 Molecules

Mole-related Formlae

Number of entities/Avogadro's number = Moles(n) = Mass of substance/ Molar Mass

No. of entities = Moles X Avogadro's Number

Molar Mass (M) = Sum of the atomic masses of the elements present in a molecule.

Avogadro's No.(NA) = 6.022×1023 Definition:No. of atoms/ molecules present in one moleof an element/ compound.

Atomic mass (A) = Mass of 1 mole of atom

Mole of atoms/molecules/ ions/electrons = (No. of atoms/molecules/ions/ electrons)/Avogadro's No.

Percentage Composition (mass %) = No. of parts by mass of the element or contituents/ Molecular mass of the compound x 100

Empirical Formula vs Molecular Formula

Molecular Formula = n x Empirical Formula

Mass/Volume = Density

Mole Concept in Solutions

Mass percent (%) = (mass/given mass of solute)/mass of given solution x 100

Mole fraction (x) = No. of moles of the component/ total no. of moles of the component

Mole fraction of the solute = (Xa) - nA/nA+nB

Molarity (M) = No. of the moles of the solute(n)/Volume of the solution in litres (V), where n-w(given mass) / (molar mass)

If the solution of molarity M1 & volume V1 is diluted to volume V2 and its new molarity M2, no. of moles of the solute does not change. Hence, M1V1 = M2V2

Molality (m) - no.of moles of the solute (n)/mass of solvent in kg, where n-w(given mass)/(molar mass)

Parts per million (ppm) = mass of the component/mass of solution x 106