Chemistry 111 Study Guide

Core Topics to Master

1. Fundamentals

• Metric System: Understanding the metric system and its importance in scientific measurements.

• SI Units and Prefixes: Familiarity with basic SI units and prefixes, unit conversions.

• Significant Figures: Identify the number of significant figures in a number and apply rules for:

  • Addition and subtraction

  • Multiplication and division

2. The Mole, Chemical Formulas, and Equations

• Relationship between moles, weight, volume, concentration, and number of atoms/molecules.

• Balancing equations by inspection.

• Given a compound's formula:

  • Name the elements in the compound

  • Indicate the number of each type of atom

  • Determine the mass of each element in one mole of the compound

  • Calculate the molecular (formula) weight

• Given a sample and formula:

  • Calculate:

    • Number of moles in the sample

    • Number of moles of an element in the sample

    • Number of molecules (formula units) in the sample

    • Number of atoms of an element in the sample

3. Chemical Stoichiometry

• Given a compound and mass:

  • Find the percent (by weight) of each element.

• Calculate:

  • Moles of products/reactants from given information (molecules, mass, concentration).

  • For a reaction with known reactants/products, deduce:

    • Moles of one product/reactant

    • Mass of any product/reactant

    • Concentration and volume of a solution of a reactant/product.

• Exothermic and Endothermic Reactions: Definitions and their relationship to chemical reactions.

4. Properties of Liquids and Solutions

• Describe molecular behavior during phase changes (solid to liquid, liquid to gas):

  • Arrangement of atoms/molecules

  • Average speed of particles

  • Distance between particles

  • Temperature changes and reasons

• Calculate density and required measurements.

• Practical examples:

  • Preparation of a solution with specific volume and concentration (e.g., 200 mL of 0.1 M NaCl).

  • Calculate moles/mass of solute in specific volumes (e.g., grams of NaCl in 50 mL of a 1.5 M solution).

  • Prepare lower concentration solutions via dilution (e.g., 100 mL of 0.22 M HCl from 2.5 M stock solution).

5. Periodic Chemistry

• Utilize the Periodic Table to identify common valences in specific groups (IA, IIA, IB, etc.).

• Write the formula and charge for major polyatomic ions (e.g., ammonium, sulfate).

• Identify periodic characteristics (atomic radius, ionic radius, electronegativity) and trends.

6. Electronic Structure of Atoms

• Relationships between the speed of light, frequency, and wavelength.

• Determine the number of protons and electrons for a given element or ion using the Periodic Table.

• From isotopes, ascertain protons, neutrons, and electrons.

• Determine electron configurations for elements and ions, identifying valence electrons, and chemical family/group membership.

7. Chemical Bonding and Related Phenomena

• Write Lewis structures for elements and compounds (maximum of three elements).

• Identify molecular shapes and polarity using bond polarity to assess molecular polarity.

• Predict compound types (ionic or covalent) based on properties (e.g., electrical conductivity).

• Use electronegativity values to determine bond types.

Sample Examination Questions

Gas Laws and Stoichiometry

1. Calculate the volume of 1.63 mol carbon dioxide gas at 295 K and 1.14 atm.

2. Calculate the volume occupied by 48.3 g of sulfur dioxide gas at 0°C and 1.00 atm.

3. Determine the molar mass of a gas from a 93 g sample occupying 29.5 L at 27°C and 1.25 atm.

4. Calculate the pressure at which oxygen has a density of 1.44 g/L at 22°C.

5. Determine the liters of oxygen gas prepared by the thermal decomposition of 0.950 g KClO3 using the following equation:
   $2KClO3(s) <br>ightarrow 2KCl(s) + 3O2(g)$

6. Calculate volumes of products in the reaction of ammonium carbonate decomposition:
   $(NH4)2CO3(s) <br>ightarrow 2NH3(g) + CO2(g) + H2O(g)$

Kinetics and Effusion

7. Predict and calculate the root mean square speed (vrms) of nitrogen at 25°C.

8. Calculate effusion rates of helium and oxygen gases.

9. Determine molar mass of NOx based on effusion rates relative to oxygen.

10. Analyze the volume and pressure changes for 1.00 mol of argon gas with the ideal gas equation and the van der Waals equation; explain discrepancies.

Light and Energy Relationships

11. Calculate the wavelength corresponding to a frequency of 7.30 × 10^14 Hz.

12. Identify energy relationships in photon emission in blue light striking strontium. Look for calculations regarding work function and photon energies.

13. Assess electron transitions in hydrogen and calculate resulting photons.

Chemical Properties and Electron Configurations

14. Write full electron configurations for given elements and ions; determine isoelectronic species.

15. Calculate effective nuclear charges, compare ionization energies, identify atomic sizes (Cl vs Cl−).

16. Evaluate lattice energies and predict behavior of elements based on energy stability.

Additional Topics

17. Discuss qualitative characteristics of visible light (wavelength, frequency, energy).

18. Analyze the properties of elements based on subshell configurations (maximum electrons per level).

19. Assess the unpaired electrons in given elements using electron diagrams.

• These notes provide an exhaustive overview of the concepts and areas of focus vital for success in Chemistry 111, as well as practical questions that emulate potential examination queries.