Free download SAT Chemistry Subject Test Crash Course by Adrian Dingle 

Authors of:  SAT Chemistry Subject Test Crash Course by Adrian Dingle

Zarrin Khan

Karabi Ghosh

Table of Contents in SAT Chemistry Subject Test Crash Course by Adrian Dingle

About This Book

About Our Author

Acknowledgments

PART I Introduction

Chapter 1 Keys to Success on the SAT Chemistry Subject Test

PART II Structure of Matter

Chapter 2 Atomic Structure: Experimental Evidence for

Atomic Structure

Chapter 3 Quantum Numbers and Energy Levels (Orbitals)

Quantum numbers are essential for understanding the behavior of electrons in atoms. They describe the properties of atomic orbitals and the electrons within them, providing a framework for understanding the arrangement of electrons in an atom.

There are four primary quantum numbers:

1. Principal Quantum Number (n): This number defines the energy level or shell in which an electron resides. It can have positive integer values (n = 1, 2, 3, …). The larger the value of \(n\), the higher the energy level and the farther the electron is from the nucleus. As \(n\) increases, the electron’s energy and the size of the orbital also increase.

2. Azimuthal Quantum Number (l): Also called the angular momentum quantum number, \(l\) determines the shape of the orbital. It has integer values from 0 to \(n-1\). Each value of \(l\) corresponds to a specific type of orbital:

   – \(l = 0\) (s orbital, spherical)

   – \(l = 1\) (p orbital, dumbbell-shaped)

   – \(l = 2\) (d orbital, cloverleaf-shaped)

   – \(l = 3\) (f orbital, complex shape)

3. Magnetic Quantum Number (m\(_l\)): This number specifies the orientation of the orbital in space. It can have integer values ranging from \(-l\) to \(+l\). For instance, if \(l = 1\), \(m\(_l\)\) can be -1, 0, or 1, indicating three possible orientations for a p orbital.

4. Spin Quantum Number (m\(_s\)): The spin quantum number refers to the direction of the electron’s spin, which can either be +½ or -½. This is crucial for the Pauli Exclusion Principle, which states that no two electrons in an atom can have the same set of quantum numbers.

These quantum numbers collectively determine the energy, position, and behavior of electrons, crucial for understanding chemical bonding and atomic structure.

Chapter 4 Electron Configurations

Chapter 5 Periodic Trends

Chapter 6 Molecular Structure: Lewis Structures, ThreeDimensional Shapes, and Polarity

Chapter 7 Bonding: Ionic, Covalent, and Metallic Bonds

Chapter 8 Relationships between the Bonding and Structure

of Solids and Their Properties

Chapter 9 Intermolecular Forces: Hydrogen Bonding,

Dipole–Dipole Forces, and London Dispersion

Forces

PART III States of Matter

Chapter 10 Gases: The Kinetic Molecular Theory

Chapter 11 Gases: Gas Law Relationships

Chapter 12 Molar Volume, Density, and Stoichiometry of

Gases

Chapter 13 Phase Changes and Phase Diagrams

Chapter 14 Solutions: Molarity and Percent by Mass

Concentrations

Chapter 15 Solution Preparation and Solution Stoichiometry

Chapter 16 Factors Affecting Solubility of Solids, Liquids, and

Gases

Chapter 17 Qualitative and Quantitative Aspects of Colligative

Properties

PART IV Reaction Types

Chapter 18 Acids and Bases: Brønsted-Lowry Theory and

other Definitions of Acids and Bases

Chapter 19 Strong and Weak Acids and Bases, pH, and

Buffers

Chapter 20 Titrations and Indicators

Chapter 21 Oxidation Numbers and REDOX

Chapter 22 REDOX Reactions, the Activity Series and

Electrochemistry

Chapter 23 Precipitation Including Basic Solubility Rules

PART V Stoichiometry

Chapter 24 Mole Concept, Avogadro’s Number, and Molar

Mass

Chapter 25 Empirical and Molecular Formula

Chapter 26 Chemical Equations and Balancing Chemical

Equations

Chapter 27 Stoichiometry Calculations

Chapter 28 Percent Yield and Limiting Reactants

PART VI Equilibrium and Reaction Rates

Chapter 29 Equilibrium and Equilibrium Constants

Chapter 30 Le Chatelier’s Principle

Chapter 31 Rates of Reaction (Chemical Kinetics)

PART VII Thermochemistry

Chapter 32 Calorimetry and Specific Heat

Chapter 33 Enthalpy Changes and Hess’s Law

Chapter 34 Heating and Cooling Curves

Chapter 35 Entropy

PART VIII Descriptive Chemistry

Chapter 36 Inorganic Descriptive Chemistry

Chapter 37 Organic Chemistry

Chapter 38 Environmental Chemistry and Nuclear Chemistry

PART IX Laboratory

Chapter 39 Knowing Your Way Around the Laboratory

Index   

File Size: 4.73 MB. Pages: 280 Please read Disclaimer.

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