Chemistry Key Points Part 1 and 2 For Entry Test

Chemistry Key Points for Entry tests are very important for admission to Engineering University. Almost every good and well-known university like UET, NUST, PIEAS, GIKI, etc. conducts entry tests. So you should have the quality which differs between you and the rest of the candidates.

Chemistry Key Points

You should be hard working and your self-confidence should be very high and you should have firm faith Many students think that getting admission to UET is the first and last thing. No doubt, UET has a name in engineering but there are many other options for you. Apply in every university, appear altogether the entry tests, keep your diligence continue and In Sha ALLAH you’ll get what you deserved.

This document contains important points for Chemistry. In the Entry test, you don’t have to solve the question and show the solution as in board exams. The entry test is different. You have to guess the proper option and you’ll get full marks. If you have good concepts then there’ll be no difficulties for you.

Before reading, we will suggest you first study the textbook very carefully. Take a highlighter and study the idea of the chapter. Highlight details and if you’ve got any confusion then make it clear. This document will only help you if you have studied the textbook very carefully.

Always remember “PRACTICE MAKES A MAN PERFECT”. So, do the maximum practice of MCQ’s. There are a lot of MCQ books available in the market. ILMI is very good and there are many others also. Buy the one you like.
If you discover any error during this document or if you recognize any trick then send us. We will update this document and add your tricks. Have a good time and my best wishes.

Sample Key Points:

> Pressure of ideal gas is doubled, the volume becomes half at constant temperature.

> Isotherms are parabola like they move away from axis at high temp for a gas,

> At high temperature the graph of p and 1/v becomes closer to pressure axis.

> All gases becomes liquid before reaching -273.16 degree C

> For diffusion collision is essential but not for effusion

> Sudden expansion cause cooling

> If gas maintained at critical temp than it can be liquefied if external Pressure is equal to critical pressure.

> H2 and He can’t liquefy by applying joule Thomson effect because they are neatly ideal

> Actual volume of molecules in gas is 4 times the molar volume.

> Intermolecular forces are attractions among molecules while intermolecular forces of attraction with in molecules.

> Greater the electro negativity difference stronger will be the dipole dipole forces and stronger will the bond.

> NOTE 🙁 Remember some electro negativity values of some well-known or frequently used elements)

> London forces exist both in polar and non-polar molecules but more prominent in non-polar molecules because no other forces exists among

non polar molecules.

> London forces and MP BP depends on size of molecules. Such that greater the size greater will be MP BP and stronger London forces and vice versa

> Dipole dipole forces are 1% more effective than covalent and more operate in liquids dipole induced dipole also called Debye forces.

> London forces are more prominent in non-polar

> Hydrogen bonding is most likely to be formed between H and N,0,F .

> Chloroform and Acetone are soluble in each other due to hydrogen bonding.

> Due to high electro negativity of Nitrogen NH3shows maximum boiling points among hydrides.

> H20, HF and Nh3 show relatively high boiling points due to strong intermolecular hydrogen boiling .

> H bonding is 20 time weaker than simple covalent bond.

> greater strength of H.B greater is viscosity

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