General Chemistry Exam Study Guide: Chapters 1–3, Nomenclature, and Key Concepts

General Chemistry Exam Overview

Exam Logistics and Policies

This section outlines the rules, procedures, and expectations for the upcoming General Chemistry exam covering Chapters 1, 2, and 3. Students must adhere strictly to exam protocols to ensure fairness and academic integrity.

• Exam Date & Time: Friday, 09/26/2025, 4:00–5:30 pm. Arrive 20 minutes early.

• Coverage: Chapters 1, 2, and 3.

• Allowed Materials: Bring a scantron, pencils, and your university ID card.

• Prohibited Items: No calculators, cell phones, smart devices, or notes. All such items must be turned off and stored in your backpack or purse.

• Seating: Students will be seated in rows, 2 seats apart from each other.

• Leaving the Room: You may not leave the exam room except for emergencies and only with permission.

• Watches: Only non-smart watches are allowed.

Exam Format

• 25 multiple-choice questions (3 points each; 75 points total)

• 5 nomenclature questions (names and formulas; 5 points each; 25 points total)

• Exam total: 100 points

• Extra credit: Up to 5 points for scantron completion

• Free response questions may be included for additional points

Topics and Concepts to Study

Chapter 1: Introduction to Chemistry

This chapter introduces the scientific approach, basic chemical concepts, and foundational terminology.

• Scientific Method: Hypothesis, theory, scientific law

• Classification of Matter: Elements, compounds, mixtures

• Physical vs. Chemical Properties: Definitions and examples

• Physical vs. Chemical Changes: How to distinguish between them

• Units and Measurements: SI units, metric prefixes (kilo, deci, centi, milli, micro, nano, pico)

• Significant Figures: Rules for determining and using significant figures in calculations

• Density: Definition and calculation

  • $\text{Density} = \frac{\text{mass (g)}}{\text{volume (mL)}}$

• Temperature Conversions:

  • $^\circ\text{C} = \frac{5}{9}(^\circ\text{F} - 32)$

  • $^\circ\text{F} = \frac{9}{5}^\circ\text{C} + 32$

• Length Conversions:

  • $1\text{ in} = 2.54\text{ cm}$

  • $1\text{ L} = 1.06\text{ quart}$

Chapter 2: Atomic Theory and Structure

This chapter covers the structure of atoms, the periodic table, and the classification of elements.

• Modern Atomic Theory: Laws of conservation of mass, law of definite proportions

• Atomic Structure: Nucleus, protons, neutrons, electrons, electron cloud

• Periodic Table: Organization by groups (columns) and periods (rows); metals, nonmetals, metalloids

• Groups and Families: Alkali metals, alkaline earth metals, chalcogens, halogens, noble gases, transition metals

• Atomic Number and Mass Number: Definitions and how to find them

• Isotopes: Atoms of the same element with different numbers of neutrons

• Average Atomic Mass: Calculation using isotopic abundance

  • $\text{Average atomic mass} = \sum (\text{isotope mass} \times \text{fractional abundance})$

• Spectroscopy: Used to determine atomic masses

• Important Metals with Roman Numerals: Know which transition metals use Roman numerals for charge (e.g., Fe, Cu, Hg, Sn, Pb)

Chapter 3: Chemical Quantities and Equations

This chapter focuses on chemical equations, mole concept, and stoichiometry.

• Law of Conservation of Mass: Balancing chemical equations

• Types of Bonds: Ionic and covalent

• Mole Concept: Avogadro's number ($6.022 \times 10^{23}$ particles per mole)

• Conversions: Mass, moles, number of particles

  • $1\text{ mol} = 6.022 \times 10^{23}$ particles$

  • $1\text{ mol Na} = 6.022 \times 10^{23}$ Na atoms$

  • $1\text{ mol MgCl}_2 = 6.022 \times 10^{23}$ MgCl$_2$ molecules$

• Empirical and Molecular Formulas: Determining formulas from percent composition

• Combustion Analysis: Calculating empirical formulas from combustion data

• Percent Composition: Calculation and interpretation

• Balancing Equations: Steps and examplesD

Nomenclature and Memorization Requirements

Names and Symbols of Elements

Students must memorize the names and symbols of elements as indicated on the periodic table provided in lecture.

Common Monatomic Ions

Know the charges and names of common monatomic ions, especially those from Groups 1A, 2A, 6A, 7A, and key transition metals.

• Group 1A ions: +1

• Group 2A ions: +2

• Aluminum: +3

• Silver: +1

• Zinc: +2

• Hydrogen: +1 in binary compounds with nonmetals, -1 in binary compounds with metals

• Group 5A, 6A, 7A elements as anions: -3, -2, -1 respectively

Common Polyatomic Ions

Memorize the names and formulas of common polyatomic ions. These ions are frequently encountered in chemical nomenclature and reactions.

Name	Formula	Name	Formula
Mercury(I)	Hg$_2^{2+}$	Permanganate	MnO$_4^-$
Ammonium	NH$_4^+$	Nitrate	NO$_3^-$
Cyanide	CN$^-$	Nitrite	NO$_2^-$
Carbonate	CO$_3^{2-}$	Hydroxide	OH$^-$
Bicarbonate (or hydrogen carbonate)	HCO$_3^-$	Peroxide	O$_2^{2-}$
Acetate	CH$_3$COO$^-$ or C$_2$H$_3$O$_2^-$	Phosphate	PO$_4^{3-}$
Perchlorate	ClO$_4^-$	Hydrogen phosphate	HPO$_4^{2-}$
Chlorate	ClO$_3^-$	Sulfate	SO$_4^{2-}$
Chlorite	ClO$_2^-$	Sulfite	SO$_3^{2-}$
Hypochlorite	ClO$^-$

Greek Prefixes and Roman Numerals

Be familiar with Greek prefixes (mono-, di-, tri-, tetra-, penta-, hexa-, hepta-, octa-, nona-, deca-) for naming covalent compounds, and Roman numerals (I, II, III, IV, V, VI) for indicating oxidation states of transition metals.

Additional Key Points and Examples

• Significant Figures: Used in all measurements and calculations. Example: 0.00450 has 3 significant figures.

• Empirical vs. Molecular Formula: Empirical formula is the simplest whole-number ratio; molecular formula is the actual number of atoms in a molecule.

• Example Calculation: To convert grams to moles: $\text{moles} = \frac{\text{mass (g)}}{\text{molar mass (g/mol)}}$

• Example of Polyatomic Ion Use: Sodium sulfate: Na$_2$SO$_4$ (contains SO$_4^{2-}$)

Summary Table: Key Conversion Factors

Conversion	Factor
Density	$\text{Density} = \frac{\text{mass (g)}}{\text{volume (mL)}}$
Temperature (C to F)	$^\circ\text{F} = \frac{9}{5}^\circ\text{C} + 32$
Temperature (F to C)	$^\circ\text{C} = \frac{5}{9}(^\circ\text{F} - 32)$
Length	$1\text{ in} = 2.54\text{ cm}$
Volume	$1\text{ L} = 1.06\text{ quart}$
Mole	$1\text{ mol} = 6.022 \times 10^{23}$ particles$

Recommended Study Strategies

• Review lecture notes, textbook material, and worked examples.

• Practice nomenclature and memorize required ions and prefixes.

• Complete end-of-chapter exercises and quizzes.

• Use flashcards for element symbols, polyatomic ions, and conversion factors.

Additional info: Some content inferred for completeness, such as the structure of the exam and clarification of nomenclature requirements.