schm000

• UNIVERSITY OF LIMPOPO FACULTY OF SCIENCES AND AGRICULTURE SCHOOL OF PHYSICAL AND MINERAL SCIENCES DEPARTMENT OF CHEMISTRY
• Introduction to General Chemistry 1A Study Guide for SCHM000 First semester Number of credits 24 Dr E Makhado and Dr TC Maponya Content evaluated by Prof MJ Hato, University of Limpopo
• Table of Contents Module information Guidance on how to use the study guide Overview of module Purpose and learning outcomes Content assumptions Structure Assessment criteria Prescribed textbooks References Suggested further readings
• Chemistry


  The study of the composition, structure, properties and behavior of matter
• Experiment


  • Systematic procedure carried out to test a hypothesis or answer a question
  • Involves observation and measurement
• States of Matter


  • Solid
  • Liquid
  • Gas

  
• Substance


  A pure chemical element or compound
• Mixture


  A combination of two or more substances that are not chemically combined
• Accuracy


  The closeness of a measurement to the true value
• Significant Figures


  The meaningful digits in a measurement, including the first uncertain digit
• Rounding


  1. Reducing the number of significant figures in a measurement

  2. Following specific rules to determine the appropriate number of significant figures
• Temperature


  A measure of the average kinetic energy of the particles in a substance
• Conversion Factor


  A ratio that relates two different units of measurement
• Dalton's Atomic Theory


  • Matter is composed of tiny, indivisible particles called atoms
  • All atoms of the same element are identical
  • Atoms of different elements have different properties
  • Atoms cannot be created, divided, or destroyed in chemical reactions

  
• Discovery of the Electron
• Discovery of the Nucleus
• Atomic Mass Unit


  A unit of mass used to express the masses of atoms and molecules
• Chemical Formula


  A symbolic representation of the composition of a chemical compound
• Polymer


  A large molecule composed of repeating structural units
• Ionic Bond


  A chemical bond formed by the transfer of electrons from a metal to a nonmetal
• Organic Compound


  A compound containing carbon and hydrogen, and often other elements such as oxygen, nitrogen, sulfur, and halogens
• Polyatomic Ion


  An ion composed of more than one atom
• Acids and Corresponding Anions

  • Hydrochloric acid (HCl) and chloride ion (Cl-)
  • Sulfuric acid (H2SO4) and sulfate ion (SO4^2-)
  • Nitric acid (HNO3) and nitrate ion (NO3-)
• Hydrate


  A compound that contains water molecules incorporated into the crystalline structure
• Chemical Equation


  A symbolic representation of a chemical reaction, showing the reactants and products
• Molecular Mass


  The sum of the atomic masses of the atoms in a molecule
• Mole


  The SI unit for the amount of a substance, equal to the number of particles (atoms, molecules, or ions) in 12 grams of carbon-12
• Percentage Composition


  The percentage by mass of each element in a compound
• Empirical Formula

  The simplest whole number ratio of the atoms of the elements present in a compound
• Molecular Formula


  The actual number and type of atoms present in a molecule of a compound
• Stoichiometry


  The calculation of the quantities of reactants and products in a chemical reaction
• Limiting Reactant


  The reactant that is completely consumed in a chemical reaction, limiting the amount of products that can be formed
• Theoretical Yield


  The maximum amount of product that can be formed in a chemical reaction based on the limiting reactant
• Gas Pressure


  The force exerted by gas molecules per unit area of the container
• Boyle's Law


  • The pressure of a gas is inversely proportional to its volume at constant temperature and amount of gas
• Charles's Law


  • The volume of a gas is directly proportional to its absolute temperature at constant pressure and amount of gas
• Combined Gas Law


  • Combines Boyle's Law and Charles's Law to relate the pressure, volume, and absolute temperature of a gas
• Avogadro's Law


  • Equal volumes of gases at the same temperature and pressure contain equal numbers of particles (atoms or molecules)
• Ideal Gas Law


  Relates the pressure, volume, amount, and absolute temperature of a gas
• Dalton's Law of Partial Pressures

  The total pressure of a gas mixture is the sum of the partial pressures of the individual gases