NMDCAT revised CHEMISTRY syllabus online topic wise-fusionstories

 Here is nmdcat revised CHEMISTRY syllabus online topic wise is prepared following PMC guidelines. All included topics and subtopics are mentioned here.  We’ve also mentioned a few of removed topics from revised nmdcat syllabus. Here are also topics which are new addition and also UHS syllabus topics included.

 One thing to remind that there is not any official ndmcat syllabus but all topics and questions will be from Fsc. text books. The topics that are common in Sindh, Punjab, KPK, Baluchistan and Gilgit Baltistan textbooks are added. We recommend you to prepare your syllabus for MCQS, short questions thoroughly. This nmdcat Chemistry ONLINE syllabus will help you to define your preparation guidelines.

CHEMISTRY

 

Table of contents

1. Introduction to fundamental concepts of chemistry

2. Atomic Structure

3. Gases

4. Liquids

5. Solids

6. Chemical Equilibrium

7. Reaction Kinetics

8. Thermochemistry and Energetics of Chemical Reactions

9. Electrochemistry

10. Chemical Bonding

11. s and p Block Elements

12. Transition Elements

13. Fundamental Principles of Organic Chemistry

14. Chemistry of Hydrocarbons

15. Alkyl Halides

16. Alcohols and Phenols

17. Aldehydes and Ketones

18. Carboxylic Acids

19. Macromolecules13

 

Introduction to fundamental concepts of chemistry

⮚ Atomic mass

⮚ Empirical formula

⮚ Molecular formula

⮚ Concept of mole

⮚ Construction of mole ratios as conversion factors in stoichiometry calculations

⮚ Avogadro’s number

⮚ Important assumptions of stoichiometric calculations

⮚ Stoichiometry

⮚ Limiting reactant

⮚ Percentage yield

 

Learning Outcomes

⮚ Construct mole ratios from balanced equations for use as conversion factors in

stoichiometric problems.

⮚ Perform stoichiometric calculations with balanced equations using moles, representative

particles, masses and volumes of gases (at STP).

⮚ Knowing the limiting reagent in a reaction, calculate the maximum amount of product(s)

produced and the amount of any unreacted excess reagent.

⮚ Given information from which any two of the following may be determined, calculate the

third: theoretical yield, actual yield, percentage yield.

⮚ Calculate the theoretical yield and the percent yield when given the balanced equation,

the amounts of reactants and the actual yield.

 

Atomic Structure

⮚ Concept of orbitals

⮚ Electronic configuration

⮚ Discovery and properties of proton (positive Rays)

⮚ Quantum numbers

⮚ Shapes of orbitals

Learning Outcomes

⮚ Describe discovery and properties of proton (positive rays)

⮚ Define photon as a unit of radiation energy.

⮚ Describe the concept of orbitals.

⮚ Distinguish among principal energy levels, energy sub-levels, and atomic orbitals.

⮚ Describe the general shapes of s, p, and d orbitals.

⮚ Describe the hydrogen atom using the quantum theory.

⮚ Use the Aufbau Principle, the Pauli Exclusion Principle, and Hund’s Rule to write the

electronic configuration of the atoms.

⮚ Write electronic configuration of atoms.

 

Gases

⮚ Properties of gases

⮚ Gas laws

⮚ Boyle’s law14

⮚ Charles’s law

⮚ General gas equation

⮚ Kinetic molecular theory of gases

⮚ Kinetic interpretation of temperature

⮚ Ideal gas equation

Learning Outcomes

⮚ List the postulates of kinetic molecular theory.

⮚ Describe the motion of particles of a gas according to kinetic theory.

⮚ State the values of standard temperature and pressure (STP).

⮚ Describe the effect of change in pressure on the volume of gas.

⮚ Describe the effect of change in temperature on the volume of gas.

⮚ Explain the significance of absolute zero, giving its value in degree Celsius and Kelvin.

⮚ Derive ideal gas equation using Boyle’s, Charles’ and Avogadro’s law.

⮚ Explain the significance and different units of ideal gas constant.

⮚ Distinguish between real and ideal gases.

 

Liquids

⮚ Properties of liquids

⮚ Intermolecular forces

⮚ Dipole-dipole forces

⮚ Dipole-induced dipole forces

⮚ Hydrogen bonding

⮚ Vapor pressure

⮚ Boiling point and external pressure

Learning Outcomes

⮚ Describe simple properties of liquids e.g; diffusion, compression, expansion, motion of

molecules, spaces between them, intermolecular forces and kinetic energy based on

kinetic molecular theory.

⮚ Explain applications of dipole-dipole forces and dipole-induced dipole forces.

⮚ Explain physical properties of liquids such as evaporation, vapor pressure, boiling point.

⮚ Describe the hydrogen bonding in H2O, NH3 and HF molecules.

⮚ Anomalous behavior of water when its density shows maximum at 4 degree centigrade

 

Solids

⮚ Introduction

⮚ Types of solids

⮚ Ionic solids

⮚ Molecular solids

⮚ Crystal lattice

Learning Outcomes

⮚ Describe crystalline solids.

⮚ Name three factors that affect the shape of an ionic crystal.

⮚ Give a brief description of ionic and molecular solids.15

⮚ Describe crystal lattice.

⮚ Define lattice energy.

 

Chemical Equilibrium

⮚ Reversible and irreversible reactions

⮚ State of chemical equilibrium

⮚ Equilibrium constant expression for important reaction

⮚ Applications of equilibrium constant

⮚ Solubility product

⮚ The Le Chatelier’s principle

⮚ Applications of chemical equilibrium in industry

⮚ Synthesis of ammonia by Haber’s Process

⮚ Common ion effect

⮚ Buffer solutions

⮚ Equilibria of slightly soluble ionic compounds (solubility product)

Learning Outcomes

⮚ Define chemical equilibrium in terms of a reversible reaction.

⮚ Write both forward and reverse reactions and describe the macroscopic characteristics

of each.

⮚ State Le Chatelier’s Principle and be able to apply it to systems in equilibrium with changes

in concentration, pressure, temperature, or the addition of catalyst.

⮚ Explain industrial applications of Le Chatelier’s Principle using Haber’s process as an

example.

⮚ Define and explain solubility product.

⮚ Define and explain the common ion effect giving suitable examples.

⮚ Describe buffer solutions and explain types of buffers.

⮚ Explain synthesis of ammonia by Haber’s Process.

Reaction Kinetics

⮚ Rate of reaction

⮚ Determination of the rate of a chemical reaction

⮚ Factors affecting rate of reaction

⮚ Specific rate constant or velocity constant

⮚ Units of rate constant

⮚ Order of reaction and its determination

Learning Outcomes

⮚ Define chemical kinetics.

⮚ Explain the terms rate of reaction, rate equation, order of reaction, rate constant and rate

determining step.

⮚ Explain qualitatively factors affecting rate of reaction.

⮚ Given the order with respect to each reactant, write the rate law for the reaction.

⮚ Explain what is meant by the terms activation energy and activated complex.

⮚ Relate the ideas of activation energy and the activated complex to the rate of a reaction.

⮚ Explain effects of concentration, temperature and surface area on reaction rates.16

⮚ Describe the role of the rate constant in the theoretical determination of reaction rate.

Thermochemistry and Energetics of Chemical Reactions

⮚ System, Surrounding and State function

⮚ Definitions of terms used in thermodynamics

⮚ Standard states and standard enthalpy changes

⮚ Energy in chemical reactions

⮚ First Law of thermodynamics

⮚ Sign of ΔH

⮚ Enthalpy of a reaction

⮚ Born-Haber cycle

⮚ Hess’s law of constant heat summation

Learning Outcomes

⮚ Define thermodynamics.

⮚ Classify reactions as exothermic or endothermic.

⮚ Define the terms system, surrounding, boundary, state function, heat, heat capacity,

internal energy, work done and enthalpy of a substance.

⮚ Name and define the units of thermal energy.

⮚ Explain the first law of thermodynamics for energy conservation.

⮚ Apply Hess’s Law to construct simple energy cycles.

⮚ Describe enthalpy of a reaction.

⮚ Describe Born-Haber cycle.

 

Electrochemistry

⮚ Oxidation number or state

⮚ Explanation of electrolysis

⮚ Electrode potential

⮚ Balancing of redox equations by ion-electron method

⮚ Balancing redox equations by oxidation number change method

Learning Outcomes

⮚ Give the characteristics of a redox reaction.

⮚ Define oxidation and reduction in terms of a change in oxidation number.

⮚ Use the oxidation-number change method to identify atoms being oxidized or reduced in

redox reactions.

⮚ Define cathode, anode, electrode potential and S.H.E. (Standard Hydrogen Electrode).

⮚ Define the standard electrode potential of an electrode.

⮚ Use the ion-electron method/oxidation number method to balance chemical equations.

Chemical Bonding

⮚ Energetics of bond formation

⮚ Atomic sizes

⮚ Atomic radii

⮚ Ionic radii

⮚ Covalent radii

⮚ Ionization energy17

⮚ Electron affinity

⮚ Electronegativity

⮚ Bond energy

⮚ Bond length

⮚ Types of bonds

⮚ Electrovalent or Ionic Bond

⮚ Covalent bond

⮚ Co-ordinate or dative covalent bond

⮚ Ionic character of covalent bond

⮚ Sigma and Pi bond

⮚ Hybridization

⮚ sp3 - Hybridization

⮚ sp2 - Hybridization

⮚ sp-hybridization

⮚ The Valence Shell Electron Pair Repulsion theory

⮚ Postulates of VSEPR theory

⮚ Applications of VSEPR theory

Learning Outcomes

⮚ Use VSEPR theory to describe the shapes of molecules.

⮚ Describe the features of sigma and pi bonds.

⮚ Describe the shapes of simple molecules using orbital hybridization.

⮚ Determine the shapes of some molecules from the number of bonded pairs and lone pairs

of electrons around the central atom.

⮚ Predict the molecular polarity from the shapes of molecules.

⮚ Explain what is meant by the term ionic character of a covalent bond.

⮚ Describe how knowledge of molecular polarity can be used to explain some physical and

chemical properties of molecules.

⮚ Define bond energies and explain how they can be used to compare bond strengths of

different chemical bonds.

⮚ Define and explain the terms atomic radii, ionic radii, covalent radii, ionization energy,

electron affinity, electronegativity, bond energy and bond length.

s and p Block Elements

⮚ Electronic configuration

⮚ Chemical properties of s-block elements

⮚ Group 1 Elements (Alkali Metals)

⮚ Atomic and Physical properties

⮚ Trends in reactivity

⮚ Group 2 Elements (Alkaline earth metals)

⮚ Trends in reactivity

⮚ Physical and chemical properties

⮚ Group trends: atomic radii, ionic radii, electronegativity, ionization potential,

electropositivity or metallic character, melting and boiling points18

Learning Outcomes

⮚ Recognize the demarcation of the periodic table into s block, p block, d block, and f block.

⮚ Describe how physical properties like atomic radius, ionization energy, electronegativity,

electrical conductivity and melting and boiling points of elements change within a group

and within a period in the periodic table.

⮚ Describe reactions of Group I elements with water, oxygen and chlorine.

⮚ Describe reactions of Group II elements with water, oxygen and nitrogen.

⮚ Describe reactions of Group III elements with water, oxygen and chlorine.

Transition Elements

⮚ General characteristics

Learning Outcomes

⮚ Describe electronic structures of elements and ions of d-block elements.

Fundamental Principles of Organic Chemistry

⮚ Classification of organic compound

⮚ Isomerism

Learning Outcomes

⮚ Define organic chemistry and organic compounds.

⮚ Classify organic compounds on structural basis.

⮚ Explain that organic compounds are also synthesized in the laboratory.

⮚ Define functional group.

⮚ Explain isomerism and its types.

Chemistry of Hydrocarbons

⮚ Open chain and closed chain hydrocarbons

⮚ Nomenclature of alkanes, alkenes and alkynes

⮚ Benzene: Properties, structure, modern representation, reactions, resonance method,

electrophilic substitution,

⮚ The molecular orbital treatment of benzene.

Learning Outcomes

⮚ Classify hydrocarbons as aliphatic and aromatic.

⮚ Describe nomenclature of alkanes.

⮚ Define free radical initiation, propagation and termination.

⮚ Describe the mechanism of free radical substitution in alkanes exemplified by methane

and ethane.

⮚ Explain the IUPAC nomenclature of alkenes.

⮚ Explain the shape of ethene molecule in terms of sigma and pi C-C bonds.

⮚ Describe the structure and reactivity of alkenes as exemplified by ethene.

⮚ Define and explain with suitable examples the terms isomerism and structural isomerism.

⮚ Explain dehydration of alcohols and dehydrohalogenation of RX for the preparation of

ethene.

⮚ Describe the chemistry of alkenes by the following reactions of ethene:19

Hydrogenation, hydrohalogenation, hydration, halogenation, halohydration,

polymerization.

⮚ Explain the shape of the benzene molecule (molecular orbital treatment).

⮚ Define resonance, resonance energy and relative stability.

⮚ Compare the reactivity of benzene with alkanes and alkenes.

⮚ Describe addition reactions of benzene and methylbenzene.

⮚ Describe the mechanism of electrophilic substitution in benzene.

⮚ Discuss chemistry of benzene and methyl benzene by nitration, sulphonation,

halogenation, Friedal Craft’s alkylation and acylation.

⮚ Apply the knowledge of positions of substituents in the electrophilic substitution of

benzene.

⮚ Use the IUPAC naming system for alkynes.

⮚ Compare the reactivity of alkynes with alkanes, alkenes and arenes.

⮚ Describe the preparation of alkynes using elimination reactions.

⮚ Describe acidity of alkynes.

⮚ Discuss chemistry of alkynes by hydrogenation, hydrohalogenation, and hydration.

⮚ Describe and differentiate between substitution and addition reactions.

Alkyl Halides

⮚ Classification of alkyl halides

⮚ Nomenclature

⮚ Reactions

⮚ Mechanism of nucleophilic substitution reaction SN1, SN2, E1 and E2 reaction

Learning Outcomes

⮚ Name alkyl halides using IUPAC system.

⮚ Discuss the structure and reactivity of RX.

⮚ Describe the mechanism and types of nucleophilic substitution reactions.

⮚ Describe the mechanism and types of elimination reactions.

Alcohols and Phenols

⮚ Alcohols:

 Classification: Primary, secondary and tertiary alcohols

 Nomenclature

 Reactivity

⮚ Phenols:

 Physical properties

 Nomenclature

 Acidity

 Reactivity

Learning Outcomes

⮚ Explain nomenclature and structure of alcohols.

⮚ Explain the reactivity of alcohols.

⮚ Describe the chemistry of alcohols by preparation of ethers and esters.20

⮚ Explain the nomenclature and structure of phenols.

⮚ Discuss the reactivity of phenol and their chemistry by electrophilic aromatic substitution.

⮚ Differentiate between an alcohol and phenol.

Aldehydes and Ketones

⮚ Nomenclature

⮚ Preparation

⮚ Reactions

Learning Outcomes

⮚ Explain nomenclature and structure of aldehydes and ketones.

⮚ Discuss the preparation of aldehydes and ketones.

⮚ Describe reactivity of aldehydes and ketones and their comparison.

⮚ Describe acid and base catalyzed nucleophilic addition reactions of aldehydes and

ketones.

⮚ Discuss the chemistry of aldehydes and ketones by their reduction to alcohols.

⮚ Describe oxidation reactions of aldehydes and ketones.

Carboxylic Acids

⮚ Nomenclature

⮚ Classification

⮚ Physical properties

⮚ Preparations of carboxylic acids

⮚ Reactivity

Learning Outcomes

⮚ Describe nomenclature, chemistry and preparation of carboxylic acids.

⮚ Discuss reactivity of carboxylic acids.

⮚ Describe the chemistry of carboxylic acids by conversion to carboxylic acid derivatives: acyl

halides, acid anhydrides, esters, amides and reactions involving interconversion of these.

Macromolecules

⮚ Proteins

⮚ Enzymes

Learning Outcomes

⮚ Explain the basis of classification and structure-function ship of proteins.

⮚ Describe the role of various proteins in maintaining body functions and their nutritional

importance.

⮚ Describe the role of enzymes as biocatalysts