Pharmaceutical Inorganic Chemistry Quiz
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Questions and Answers

What happens in a double displacement reaction?

  • One reactant is oxidized while the other is reduced.
  • Two reactants combine to form one compound.
  • One reactant decomposes into two products.
  • Two reactants exchange ions to form two new compounds. (correct)

    • Which of the following is a correct product of the reaction HCl (aq) + AgNO3 (aq)?

  • AgCl (s) + HNO3 (aq) (correct)
  • AgCl (s) + HCl (aq)
  • AgNO3 (s) + HCl (aq)
  • AgCl (aq) + HNO3 (aq)

    • What are the three components needed to ignite a combustion reaction?

  • Fuel, Oxygen, and Spark (correct)
  • Hydrocarbon, Water, and Heat
  • Oxygen, Spark, and Carbon Dioxide
  • Fuel, Nitrogen, and Heat

    • What are the typical products of combustion when hydrocarbons burn?

    <p>Water and Carbon Dioxide</p> Signup and view all the answers

    Which of the following represents a double displacement reaction?

    <p>NaCl + AgNO3 → NaNO3 + AgCl</p> Signup and view all the answers

    What is the general equation for a decomposition reaction?

    <p>AB → A + B</p> Signup and view all the answers

    Which of the following describes a single displacement reaction?

    <p>A + BC → AC + B</p> Signup and view all the answers

    What does the roman numeral in the name 'Iron (III) chloride' indicate?

    <p>The oxidation state of iron</p> Signup and view all the answers

    Which of the following is an example of a synthesis reaction?

    <p>2Na + Cl2 → 2NaCl</p> Signup and view all the answers

    Which reaction represents a combustion reaction?

    <p>C + O2 → CO2</p> Signup and view all the answers

    What is the formula for Aluminum sulfate?

    <p>Al2(SO4)3</p> Signup and view all the answers

    How do metals with multiple oxidation states differ in their naming?

    <p>They use roman numerals to express the oxidation state.</p> Signup and view all the answers

    What is produced when magnesium reacts with fluorine in a synthesis reaction?

    <p>MgF2</p> Signup and view all the answers

    What is the mass of one mole of carbon dioxide (CO2)?

    <p>44g</p> Signup and view all the answers

    Which formula represents the correct molecular weight calculation for water (H2O)?

    <p>(2 × 1.008) + (1 × 15.999)</p> Signup and view all the answers

    How is the molecular weight of a compound determined?

    <p>By summing the products of the number of each atom and their atomic masses.</p> Signup and view all the answers

    What is the resulting formula for barium chloride?

    <p>BaCl2</p> Signup and view all the answers

    Which one of the following represents a polyatomic ion in the compound ammonium carbonate?

    <p>NH4+</p> Signup and view all the answers

    How many grams are in one mole of methane (CH4)?

    <p>16g</p> Signup and view all the answers

    When writing the chemical formula for a salt, which order do you write the ions in?

    <p>Cation-Anion</p> Signup and view all the answers

    What is the combined formula of ammonium carbonate after balancing the charges?

    <p>(NH4)2CO3</p> Signup and view all the answers

    What type of bond forms molecular compounds?

    <p>Covalent bonds</p> Signup and view all the answers

    Which of the following statements is true about ionic compounds?

    <p>They are formed by cations and anions.</p> Signup and view all the answers

    What is the empirical formula for butene (C4H8)?

    <p>CH2</p> Signup and view all the answers

    What is the significance of Avogadro’s number?

    <p>It is the number of atoms in one mole of an element.</p> Signup and view all the answers

    How is a molecular formula represented?

    <p>With elements followed by the number of atoms in subscript.</p> Signup and view all the answers

    What characterizes molecular compounds compared to ionic compounds?

    <p>They are easily volatilized.</p> Signup and view all the answers

    What is the atomic mass unit of the carbon-12 isotope?

    <p>12 g</p> Signup and view all the answers

    One mole of sodium has a mass of approximately how many grams?

    <p>23 gm</p> Signup and view all the answers

    Study Notes

    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.

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    Related Documents

    Pharmaceutical Inorganic & Physical Chemistry Lecture Notes PDF

    Description

    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.

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