General Chemistry Core Competencies and Study Guide

General Chemistry Core Competencies

1. Chemical Math and Measurement

Accurate numeric measurements and calculations are essential for solving chemical problems. This includes understanding scientific notation, significant figures, and unit conversions.

• Perform numeric measurements: Use correct units and significant figures in calculations.

• Scientific notation: Express large and small numbers efficiently.

• Unit conversions: Convert between metric and English units.

• Dimensional analysis: Use conversion factors to solve problems.

• Example: Convert 0.025 kg to grams: $0.025 \text{ kg} \times \frac{1000 \text{ g}}{1 \text{ kg}} = 25 \text{ g}$

2. Structure of Matter

Matter is composed of atoms and molecules, which can be classified as elements, compounds, or mixtures. Understanding their structure is fundamental to chemistry.

• Atoms: The basic unit of matter, consisting of protons, neutrons, and electrons.

• Molecules: Groups of atoms bonded together.

• Elements vs. Compounds vs. Mixtures: Elements are pure substances; compounds are chemically bonded elements; mixtures are physical combinations.

• Example: Water ($H_2O$) is a compound; air is a mixture.

3. Types of Chemical Reactions

Chemical reactions involve the transformation of substances through breaking and forming chemical bonds. Understanding reaction types and equations is crucial.

• Synthesis, decomposition, single replacement, double replacement, combustion: Main types of reactions.

• Chemical equations: Represent reactants and products.

• Balancing equations: Ensure conservation of mass.

• Example: $2H_2 + O_2 \rightarrow 2H_2O$

4. Properties of Gases, Liquids, and Solids

Matter exists in different states, each with unique properties. Understanding these properties helps explain physical and chemical behavior.

• Gases: Compressible, fill containers, described by gas laws.

• Liquids: Definite volume, take shape of container.

• Solids: Definite shape and volume.

• Intermolecular forces: Affect boiling/melting points.

• Example: Boyle's Law: $P_1V_1 = P_2V_2$

5. Chemical Quantities and Calculations

Stoichiometry involves calculating the amounts of reactants and products in chemical reactions using the mole concept.

• Mole concept: $1 \text{ mole} = 6.022 \times 10^{23}$ particles.

• Stoichiometric calculations: Use balanced equations to relate quantities.

• Percent yield: $\text{Percent yield} = \frac{\text{actual yield}}{\text{theoretical yield}} \times 100\%$

• Example: Calculate moles of $H_2O$ produced from 4 moles of $O_2$.

6. Acids, Bases, and Buffers

Acids and bases are important classes of compounds with distinct properties. Buffers help maintain pH stability.

• Acids: Donate protons ($H^+$); pH < 7.

• Bases: Accept protons; pH > 7.

• Buffers: Resist changes in pH.

• Example: $HCl$ is a strong acid; $NaOH$ is a strong base.

7. Organic Compounds and Nomenclature

Organic chemistry focuses on carbon-containing compounds, their structures, and naming conventions.

• Hydrocarbons: Alkanes, alkenes, alkynes.

• Naming: Use IUPAC rules for systematic names.

• Functional groups: Alcohols, carboxylic acids, amines, etc.

• Example: Methane ($CH_4$) is the simplest alkane.

8. Nuclear Chemistry

Nuclear chemistry studies changes in atomic nuclei, including radioactive decay and nuclear reactions.

• Types of radiation: Alpha, beta, gamma.

• Half-life: Time for half of a radioactive sample to decay.

• Nuclear equations: Represent changes in nuclei.

• Example: $^{14}C \rightarrow ^{14}N + \beta^-$

9. Laboratory Skills and Scientific Investigation

Laboratory work is essential for understanding chemical principles and developing scientific skills.

• Scientific method: Systematic investigation.

• Experimental procedures: Good laboratory practices (GLP).

• Measurement: Use of standard laboratory equipment.

• Data analysis: Interpret and communicate results.

• Example: Measuring density using a balance and graduated cylinder.

Additional info:

This study guide is based on a syllabus outlining core competencies and measurable objectives for a General Chemistry college course. It covers all major topics listed in the provided chapter titles and expands on each with definitions, examples, and key equations.