Chemistry Course Overview and Ethics

Course Information

• Course Code: BMD1102
• Course Title: Chemistry
• Instructor: Prof. Dr. Hossieny Ibrahim
• University: Badr University in Assiut
• School: School of Biotechnology
• Email: [email protected]
• Office Number: Bio-326

Lecture Ethics

• Mobile phones should be silenced.
• Questions only permitted with permission.
• Side discussions are prohibited.
• Entrance and exit should be quiet and organized.

Course General Information

• Lectures: Monday 9:00 - 12:00 (Group B), Tuesday 1:00 - 4:00 (Group A)
• Room Numbers: Bus-206 (Group B), Bus-101 (Group A)
• Assessment:
  • Quizzes & Midterm Exam: 60 marks
  • Oral Exam: 40 marks
  • Practical Exam: 100 marks
  • End Term Exam: 200 marks

Textbooks

• Atkins P.W., 2006, Physical Chemistry, 8th ed., Oxford University Press.
• McMurry & Thompson, Fundamentals of Organic Chemistry, Brooks-Cole 2002.

Aim and Objectives

• Understand the foundations of organic chemistry and its importance.
• Relate molecular structure to properties of organic compounds.
• Identify and classify functional groups in organic compounds.
• Learn IUPAC nomenclature and common names of organic compounds.
• Connect functional groups to reactivity patterns in organic compounds.
• Understand fundamental reactions in organic chemistry (substitution, addition, elimination).
• Study aliphatic compounds, including nomenclature, structure, properties, preparation, and reactions.
• Learn about physical properties of solutions, thermodynamics and thermochemistry of chemical and physical changes, metals, alloys, and electrochemistry and corrosion.

Course Content

• Introduction
  • Types of bonds
  • Electronegativity
  • Lewis structures
  • Lewis acid/base
• Hydrocarbons
  • Aliphatic compounds
    • Alkanes
    • Cycloalkanes
    • Alkenes
    • Alkynes
  • Aromatic compounds
• Alcohols and Ethers
• Carbonyl compounds: Aldehydes & Ketones
• Physical properties of solution
• Thermodynamics & thermochemistry of chemical and physical changes
• Electrochemistry & corrosion of metals
• Metals & alloys
• Resonance
• Hybridization
• Isomers
• Functional groups

Introduction to Organic Chemistry

• Early definitions focused on compounds from living things.
• Modern organic chemistry is a major branch dealing with carbon compounds.
• Carbon's bonding capacity is 4.
• Carbon-carbon bonds can be single, double, or triple.
• Carbon atoms are organized into straight chains, branched chains, or rings.
• Other atoms (e.g., oxygen, nitrogen, halogens, sulfur) are commonly found attached to carbon structures.
• Groups can be in different positions on a carbon skeleton.

The Significance of Carbon

• Millions of carbon-containing organic compounds are known.
• Types of carbon compounds in organisms:
  • Carbohydrates: contain C, H, and O, made of monosaccharides.
  • Lipids: contain C, H, and O, made of glycerol and fatty acids.
  • Proteins: contain C, H, O, and N, made from amino acids.
  • Nucleic acids: contain C, H, O, N, and P.

Carbon Compounds Classified as Inorganic

• Certain carbon compounds (e.g., carbon monoxide, carbon dioxide, carbonates, cyanides, carbides) are considered inorganic exceptions.

Atomic Structure and Electronic Configuration

• Atoms are composed of a nucleus (protons, neutrons) and orbiting electrons.
• Atomic number equals the number of protons.
• Atomic weight equals the sum of protons and neutrons.
• Electrons fill orbitals in specific configurations.

Valence Electrons & Lewis Structure

• Valence electrons are those in the outermost shell; they participate in chemical bonding.
• Lewis structures show the atom's symbol and valence electrons (dots) around it.

Formation of Ions & Lewis Model of Bonding

• Atoms tend to gain/lose electrons to achieve a stable octet (eight valence electrons) similar to noble gases.
• Gaining electrons forms anions (negative charge).
• Losing electrons forms cations (positive charge).

Formation of Chemical Bonds

• Ionic bonds form from electrostatic attraction between oppositely charged ions (cations and anions).
• Covalent bonds form by sharing electron pairs between atoms.

Ionic Bonds vs. Covalent Bonds

• Ionic bonds typically form between a metal and a nonmetal.
• Covalent bonds usually occur between nonmetals or metalloids and nonmetals.

Electronegativity and Chemical Bonds

• Electronegativity: an atom's ability to attract electrons in a covalent bond.
• Differences in electronegativity determine the type of bond:
  • Nonpolar covalent bond: small difference
  • Polar covalent bond: moderate difference
  • Ionic bond: large difference

Polar Covalent Bonds

• In polar covalent bonds, shared electrons are not equally distributed.
• Polarity is indicated by an arrow pointed towards the more electronegative atom.

Lewis Structures of Molecules and Ions

• Determine the total number of valence electrons.
• Apply the octet rule (except for hydrogen, which has only two valence).
• Arrange atoms around central atom, forming bonds.
• Fill the octets by adding electrons

Writing Lewis Structures

Steps for drawing Lewis structures

• Calculate the total number of valence electrons.
• Apply the octet rule.
• Determine the central atom.
• Place single bonds between atoms.
• Fill the remaining electrons to complete the octets.
• Calculate formal charges to see which structures are more plausible and better represent the molecule.

A Summary of Common Formal Charges

• Formal charge is a way of evaluating possible Lewis Structures and their relative stability.

Resonance Structures

• Resonance structures are valid Lewis structures representing different arrangements of electrons for one molecule.
• They show how a molecule's delocalized electrons can occupy different regions, thereby stabilizing it.

Resonance Structure Examples

• Examples include ozone, carbonate, sulfur dioxide, nitrate.

Lewis Acids (LA) and Lewis Bases (LB)

• Lewis acids are electron-pair acceptors.
• Lewis bases are electron-pair donors.
• Examples of Lewis acids and bases include those containing H, O, N, along with metal ions and certain metal compounds.

Solved Problems

• Examples of calculating formal charges and writing Lewis structures.