Pharmaceutical Inorganic Chemistry Quiz

Pharmaceutical Inorganic & Physical Chemistry

• Course taught by Dr. Mahmoud Mohamed Abbas
• Presented at Galala University, Faculty of Pharmacy
• Supported by Arizona State University

Compounds

• Compounds are formed when atoms bond together
• Bonding can be covalent (molecular compounds) or ionic (ionic compounds or salts)
• The molecule is the smallest unit of a compound, holding its chemical properties
• A compound is made of different elements in definite proportions

Types of Compounds

• Ionic Compounds
  • Produced from reactions between acids and bases
  • Known as salts
  • Formed from cations and anions
  • Have a crystal structure with cations and anions in ratios
  • High melting and boiling points, low vapor pressure
  • Good electrical conductivity in solution
• Molecular Compounds
  • Include diatomic elements (H, N, O, halogens) and non-metallic compounds (e.g., H₂O, NH₃, CH₄, C₂H₅OH)
  • Lower melting and boiling points
  • Exist in gas, liquid, and solid phases
  • Easy to volatilize

Molecule Representation

• Molecular Formula: Shows each element and its count in a molecule (e.g., H₂O, CO₂, C₄H₈)
• Empirical Formula: The simplest ratio of atoms in a compound(e.g., in butene C₄H₈, the empirical formula is CH₂)
• Structural Formula: Shows how atoms are connected through bonds

Atomic Weight Scale and Mole

• 12C atom has 12 atomic mass units
• 12 grams of 12C represents 1 mole
• 1 mole of 12C contains 6.022 × 10²³ atoms (Avogadro's number)
• One mole of an element has a mass in grams equivalent to its atomic mass
• Example: 1 mole of sodium = 22.989 g ≈ 23 g
• One mole of any element contains Avogadro's number of atoms.
• Mole of a compound (includes diatomic elements):
  • One mole has a mass in grams equivalent to the sum of the atomic masses of its atoms
  • Example: Molecular weight or relative molecular mass (M,)

Molecular Weight Calculations

• Write the chemical formula
• Get the atomic mass for each element from the periodic table
• Multiply each element's mass by its atomic count in the molecule
• Add together the resulting products
• Express the result in grams (molecular weight)

Mole Calculations

• Calculate moles for CO₂, CH₄, and CH₃OH (using atomic masses C=12, H=1, O=16)
• Provide resulting grams for each

Writing Salts Chemical Formulae

• Arrange cation and anion in correct order (e.g., Ba²⁺, Cl⁻)
• Write charges below each ion.
• Combine cation and anion symbols, adjusting for numbers by reducing to lowest common ratio ( e.g., BaCl₂ ). This should also be done for polyatomic anions (within brackets).

Stocks System

• Used for metals with multiple oxidation numbers (like Iron: Fe²⁺/Fe³⁺)
• A Roman numeral indicates the oxidation number after the metal name (e.g., FeCl₂, iron (II) chloride)

Reactions and Reaction Types

• Key types of reactions: synthesis, decomposition, single displacement, double displacement, combustion

Types of Reactions

• Synthesis: When two compounds react to form a new compound.
• Decomposition: When a compound breaks down into two or more smaller compounds
• Single Displacement: One element replaces another element in a compound.
• Double Displacement: Two compounds exchange ions to form new compounds.
• Combustion: A rapid chemical reaction that forms heat and light, typically involving oxygen

Synthesis Reactions

• Examples of synthesis reactions
  • 3 H₂ + N₂ → 2 NH₃
  • MgO + CO₂ → MgCO₃
  • 2 CO + O₂ → 2 CO₂
• Practice: Predict the products and balance the equations

Decomposition Reactions

• General Equation: AB → A + B
• Examples of decomposition reactions
• 2 Fe(OH)₃ → Fe₂O₃ + 3 H₂O
• 2 H₂O → 2 H₂ + O₂
• Use decomposition reactions to predict products and balance equations

Single Displacement Reactions

• General Equation: A + BC → AC + B
• Example Reaction: Zn + CuCl₂ → ZnCl₂ + Cu
• Reaction involves more active metal replacing less active metal within an ionic compound

Double Displacement Reactions

• General Equation: AB + CD → AD + CB
• Examples:
  • Na₂SO₄ + SrCl₂ → 2 NaCl + SrSO₄
  • HCl + NaOH → NaCl + H₂O
  • Na₂S + 2 HCl → 2 NaCl + H₂S

Combustion Reactions

• Reaction with oxygen that gives off heat and light
• Products depend on reactants:
  • Metals react to form oxides
  • Hydrocarbons react to form CO₂ and H₂O
• Three components for combustion: fuel, oxygen, ignition source

Practice Questions

• Provide example equations to practice writing and balancing single and double displacement reactions
• Provide example equations for combustion reactions to practice writing and balancing.

Test your knowledge on the fundamentals of pharmaceutical inorganic and physical chemistry. This quiz covers concepts such as types of compounds, their properties, and the bonding processes involved. Suitable for students in pharmacy courses and related fields.