General Chemistry Test 1: Syllabus and Assessment Guidelines

General Chemistry Test 1 Syllabus and Assessment Guidelines

Test Overview

This document outlines the structure, content coverage, and rules for the upcoming General Chemistry Test 1. The test is designed to assess foundational knowledge in chemistry, including atomic structure, periodic trends, and chemical reactions.

• Date and Time: Thursday, October 2, 6:30 pm – 8:15 pm

• Length: 1 hour 45 minutes (105 minutes)

• Format: Multiple Choice (approximately 26 questions)

• Location: As posted in the Term Assessment information folder in D2L

Permitted Materials

• Aid Bubble Sheet

• The formula sheet

• The quantum booklet

• The question booklet and periodic tables

• Calculator: Non-programmable calculator only

• Student ID or government-issued photo ID

Note: You may not use your own periodic table or formula sheet. All formula sheets will be provided in the Term Assessment information folder in D2L.

Content Covered

The test will cover the following chapters and topics:

• Chapter 1: Sections 1.1 to 1.4

  • Common metric prefixes

  • Significant digits in calculations

  • Common derived units (Table 1.3)

• Chapter 2: Sections 2.1 and 2.7

  • Discovery of the electron and nucleus

  • Structure of the atom

  • Note: You are not required to know the relative ionization energies for the main group and main transition elements (pages 34–43).

• Chapter 3: Sections 3.1 and 3.5

  • Polyatomic ions in Table 3.2

  • Writing chemical formulas

  • Balancing oxidation-reduction reactions (pages 121–124)

  • Gas-evolution reactions in Table 4.2

Key Definitions and Concepts

• Metric Prefixes: Standard prefixes used to denote powers of ten in the metric system (e.g., kilo-, centi-, milli-).

• Significant Digits: The digits in a measurement that are known with certainty plus one estimated digit. Used to indicate the precision of a measurement.

• Atomic Structure: Atoms consist of a nucleus (protons and neutrons) and electrons. The discovery of the electron and nucleus was fundamental to modern chemistry.

• Polyatomic Ions: Ions composed of more than one atom (e.g., sulfate SO42−, nitrate NO3−).

• Oxidation-Reduction (Redox) Reactions: Chemical reactions involving the transfer of electrons between species. Balancing these reactions requires accounting for both mass and charge.

• Gas-Evolution Reactions: Reactions that result in the formation of a gas as a product.

Example: Balancing a Redox Reaction

To balance a redox reaction, follow these steps:

1. Write the unbalanced equation.

2. Separate the reaction into half-reactions (oxidation and reduction).

3. Balance all elements except hydrogen and oxygen.

4. Balance oxygen atoms by adding H2O.

5. Balance hydrogen atoms by adding H+.

6. Balance charges by adding electrons.

7. Combine the half-reactions and ensure electrons are canceled out.

Example Equation:

$\ce{MnO4^- + 8H^+ + 5Fe^{2+} -> Mn^{2+} + 5Fe^{3+} + 4H2O}$

Exam Rules and Conduct

• Turn off all electronic devices and place them in bags under the desk.

• Only writing materials are allowed on the desk (no pencil cases).

• Food and drink are not permitted except for medical reasons.

• Conduct the exam in silence and remain in the room until the exam is complete.

• Follow all academic integrity standards.

Health-Related Guidance

• If you feel ill during the exam, notify your invigilator.

• If you are unable to complete the exam due to illness, contact your instructor and physician.

• Documentation may be required for academic consideration requests.

Summary Table: Permitted and Prohibited Materials

Permitted Materials	Prohibited Materials
Non-programmable calculator Aid bubble sheet Formula sheet (provided) Quantum booklet Student ID	Personal periodic table Personal formula sheet Programmable calculator Electronic devices (phones, tablets, etc.) Food and drink (except for medical reasons)