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THE ULTIMATE CREDIT-BY-EXAM STUDY GUIDE FOR:

Chemistry

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THE ULTIMATE CREDIT-BY-EXAM STUDY GUIDE FOR: Chemistry 1 st Edition

06/10/2024

Acknowledgements We would like to thank the author for their patience, support, and expertise in contributing to this study guide; and our editors for their invaluable efforts in reading and editing the text. We would also like to thank those at Achieve Test Prep whose hard work and dedication to fulfilling this project did not go unnoticed. Lastly, we would like to thank the Achieve Test Prep students who have contributed to the growth of these materials over the years.

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Contents

Chapter1: Structure of Matter

A. Atomic Structure

2 7 8 9

B. Atomic Representation

C. Isotopes

D. Electron Shells E. Periodic Table

14 15 16 17 17 18 20 21 22 32 37 39 40 42 48 49 51 53 56 59 61 66 72 76 77 78 80 81 82 36 76

F. Element’s Classification in the Periodic Table

G. Alkali Metals

H. Alkaline Earth Metals

I. Transition Metals

J. Metalloids K. Halogens L. Noble Gases

M. Periodic Trends

Quiz

Chapter2: Chemical Bonding

A. Ions

B. Octet Rule

C. Ionic Bonding

D. Covalent Bonding E. Metallic Bonds F. Lewis Dot Structure

G. VSEPR Theory

H. Dipole and Dipole Moment

I. Intermolecular Forces J. Sigma and Pi Bonds

K. Hybridization

L. Quantum Numbers

Quiz

Chapter3: Organic Compound Naming

A. Hydrocarbons

B. Structural Representation

C. Alkane D. Alkenes E. Alkynes F. Alcohols

G. Ethers

83 84 85 86 88 89 90 91 91 93

H. Aldehydes

I. Ketones

J. Carboxylic Acids

K. Amines

L. Biological compounds

M. Lipids

N. Carbohydrates

O. Proteins

Quiz

Chapter4: Radioactivity

A. Radioactive Decay

95 96 97 98

B. Alpha Decay C. Beta Decay D. Gamma Decay

E. Predicting Decay Outcome F. Radioactive Decay Formula

101 102 104 106

G. Application On Nuclear Chemistry

Quiz

Chapter5: Chemical Reactions

110

A. Chemical Reactions: Fundamentals and Applications

111 113 115 122 124 125 127 131 135 140 146 151 159 162 164 168

B. Balancing Chemical Reactions

C. Stoichiometry

D. Molarity

E. Limiting Reactant and Excess Reactant F. Reversible and Irreversible Reactions

G. Dynamic Equilibrium

H. Dissolution Rate

I. Solubility Constant & Solubility Rules

J. Acid and Base

K. Acid-Base Reactions

L. Redox Reactions

M. Electrochemical Cell

N. Electrolytic Cell

O. Spontaneity

Quiz

Chapter6: States of Matter

172

A. Solid, Liquid, and Gas

173

B. Solid

174 176 177 179 181 193 198 202 204 206 210 214 215 217 220 222 224 225 226 228 228 229 232 237 238 240 241 243 244 246 248 251 254 214 236

C. Liquids D.Gases

E. Kinetic Molecular Theory

F.GasLaws

G. Colligative Properties

H. Phase Changes

I. Phase Changes Diagram

J. Heating Curve K. Cooling Curve

Quiz

Chapter7: Thermodynamics

A. Introduction to Thermodynamics in Chemistry

B. Thermodynamics Quantities

C. Enthalpy H D. Entropy S

E. Free Energy G

F. Laws of Thermodynamics

G. Zeroth Law of Thermodynamics H. First Law of Thermodynamics I. Second Law of Thermodynamics J. Third Law of Thermodynamics

K. Ecell, ΔG, and K

Quiz

Chapter8: Dimensional Analysis

A. Ensuring Unit Consistency in Physical Equations

B. SIUnits

C. Conversation of Temperature

D. Significant Figures

E. Rounding

F. Scientific Notation

G. Laboratory

H. Laboratory Techniques

I. Laboratory Safety Procedures

Quiz

Answers

258

Chapter1: Structure of Matter

Overview This chapter delves into the fundamental building blocks of the universe: matter and its atomic constituents. Starting with the atomic structure, we explore the intricate details of protons, neutrons, and electrons and how they come together to form atoms. The concept of isotopes introduces variations in atomic mass, leading to a deeper understanding of atomic representation. As we move through electron shells and their configurations, we lay the groundwork for understanding the periodic table—an invaluable tool in chemistry that organizes elements based on their properties. Classifying elements into groups such as alkali metals, alkaline earth metals, transition metals, metalloids, halogens, and noble gases reveals the periodic trends governing their behavior. These trends, including electronegativity, electron affinity, ionization energy, and atomic size, are pivotal in predicting the properties and reactivity of elements. Through this chapter, we aim to provide a comprehensive overview of the structure of matter, guided by the periodic table, to understand the principles that underpin chemical reactions and material properties. Objectives ● Describe the basic atomic structure, including the roles of protons, neutrons, and electrons. ● Understand and represent isotopes, recognizing how variations in neutron numbers affect atomic mass. ● Identify and explain the significance of electron shells in determining an element’s chemical behavior. ● Navigate the periodic table, understanding its organization and the significance of element groups. ● Classify elements into alkali metals, alkaline earth metals, transition metals, metalloids, halogens, and noble gases, noting their characteristic properties. ● Explain periodic trends and how they affect element properties such as electronegativity, electron affinity, ionization energy, and atomic size. ● Apply knowledge of periodic trends to predict element behavior and reactivity in various chemical contexts. At the end of this chapter, you should be able to:

A. Atomic Structure Historical Models of the Atom

Starting with Democritus’ idea of indivisible particles, the understanding of atomic structure evolved through Dalton’s solid sphere model, Thomson’s plum pudding model, Rutherford’s nuclear model, and Bohr’s planetary model, resulting in the modern quantum model. An impartial overview of key details in the field:

460 Democritus’ Atomic Theory: Democritus, an ancient Greek philosopher, proposed that everything is composed of tiny, indivisible particles called atoms.

1803 John Dalton’s Solid Sphere Model: In Dalton’s solid sphere model, atoms are envisioned as indivisible and solid spheres, each with a unique weight. These solid spheres combine in fixed ratios to create compounds.

1897 J.J Thomson’s Plum Pudding Model: Joseph John Thomson, a prominent physicist, proposed the existence of electrons within a positively charged ‘pudding-like’ substance. He challenged the idea of indivisible atoms and introduced the concept of the plum pudding model.

1912 Ernest Rutherford’s Nuclear Model: Rutherford’s groundbreaking nuclear model, derived from his gold foil experiment, revealed that atoms consist of a tiny, positively charged nucleus at the center, containing most of the mass. Electrons were found to orbit around the nucleus, akin to planets around the sun, dispelling the previous notion of a uniformly distributed positive charge throughout the atom. This model laid the foundation for a more nuanced understanding of atomic structure. 1913 Niels Bohr’s planetary Model: Bohr’s atomic model, a refinement of earlier models, suggested that electrons orbit the nucleus in fixed energy levels or shells. Electrons can jump between these levels by absorbing or emitting discrete amounts of energy, leading to the observation of distinct spectral lines. This idea provided a more precise explanation for the behavior of electrons within the atom and marked a significant advancement in our understanding of atomic structure.

1930 Quantum Atomic Model: The quantum model, developed in the early 20th century, redefines our understanding of atomic structure. By introducing electron orbitals as probability-based regions, it embraces uncertainty and electrons’ dual wave-particle nature. Departing from classical fixed orbits, this foundational framework in modern physics offers a more accurate and nuanced depiction of the atom.

The historical journey through ancient Greek ideas of indivisible particles, Dalton’s atomic theory, Thomson’s discovery of the electron, Rutherford’s nuclear model, and Bohr’s 20th-century model culminates in the transformative quantum model. This progression highlights the dynamic nature of scientific understanding, each phase refining and expanding our comprehension of the intricate world of atoms.

Chapter2: Chemical Bonding

Overview This chapter delves into the fundamental concept of chemical bonding, the force that holds atoms together in molecules and compounds, shaping the structure and properties of matter. Starting from the basics of ions and the octet rule, we explore the different types of chemical bonds: ionic, covalent (polar and nonpolar), and metallic. The chapter also covers the naming conventions for ionic and covalent compounds, offering a guide to understanding chemical nomenclature. Advanced topics such as Lewis dot structures, Valence Shell Electron Pair Repulsion (VSEPR) theory, dipole moments, and intermolecular forces are discussed to provide a deeper insight into how molecules form and interact. Furthermore, the concepts of sigma and pi bonds, hybridization, and quantum numbers are introduced to bridge the understanding of molecular structure with the principles of quantum mechanics. Objectives ● Differentiate between ionic, covalent, and metallic bonds and understand their characteristics. ● Name ionic and covalent compounds correctly using standard chemical nomenclature. ● Draw Lewis dot structures for molecules and ions. ● Use the VSEPR theory to predict the shapes of molecules. ● Understand the concepts of dipole and dipole moment and their significance in molecular interactions. ● Describe intermolecular forces and their impact on the physical properties of substances. ● Identify sigma and pi bonds and explain their role in molecule formation. ● Comprehend hybridization and its application in determining molecular geometry. ● Interpret quantum numbers and their importance in understanding electron configurations and atomic orbitals. At the end of this chapter, you should be able to: ● Explain the concept of ions and how they relate to chemical bonding. ● Apply the octet rule to predict the formation of chemical bonds.

A. Ions

An ion is an atom or molecule that has gained or lost one or more electrons, resulting in a net electrical charge.

Cations: A cation is a positively charged ion formed when an atom loses one or more electrons. This electron loss results in an imbalance between protons and electrons, with the former outnumbering the latter, leading to a net positive charge. Anions: An anion is a negatively charged ion that forms when an atom gains one or more electrons. This gain of electrons creates an excess of negative charge, causing an imbalance with the positively charged protons in the nucleus.

Atom

Ion

The smallest unit of an element that retains its properties.

An ion is either a single charged particle or a collection of particles with a net positive or negative charge. Independence in Solution: In solution, ions are generally independent entities, capable of moving freely. Formation: Ions form through the gain or loss of electrons, often resulting in electrovalent or ionic bonding between oppositely charged ions. Electron-Proton Balance: Ions have an unequal number of electrons and protons, leading to a net positive or negative charge. Stability: Ions can be relatively stable depending on the type of ion formed and its environment, such as stable noble gas configurations for certain ions.

Independence in Solution: Atoms are not typically independent in solution; they may bond or combine with other atoms to form molecules or compounds. Formation: Atoms can combine to form molecules by sharing electrons through covalent bonds. Electron-Proton Balance: Generally, atoms have an equal number of electrons and protons within their nucleus. Stability: Atoms on their own can be considered stable under normal conditions.

Chapter3: Organic Compound Naming Organic chemistry, a branch of chemistry devoted to the study of carbon-containing compounds, serves as the cornerstone of life and the creation of various synthetic materials. In this chapter, we explore the systematic nomenclature that assigns precise names to this diverse array of molecules. From the straightforward identification of simple hydrocarbons to the nuanced navigation of functional groups, mastering organic chemistry naming is a fundamental skill for any aspiring chemist. This journey will unravel the language of molecules, shedding light on the intricate relationships and properties encoded within the rich tapestry of carbon-based compounds. Overview This chapter embarks on a journey through the fascinating world of organic chemistry, focusing on the nomenclature and structural representation of various organic compounds. It serves as a foundational guide to understanding the diverse families of compounds that constitute organic chemistry, from the simplest hydrocarbons to complex biological molecules. We’ll explore the structure, properties, and naming conventions of alkanes, alkenes, alkynes, alcohols, ethers, aldehydes, ketones, carboxylic acids, amines, and the iconic benzene ring. The chapter further delves into the realm of biological compounds, shedding light on lipids, carbohydrates, and proteins—the molecules of life. By elucidating the rules of organic compound naming and illustrating their structural nuances, this chapter lays the groundwork for mastering organic chemistry’s language and its applications in biology, medicine, and materials science. Objectives ● Understand the basics of organic compound naming: Grasp the systematic approach to naming organic compounds based on their structure and functional groups. ● Identify and name different types of hydrocarbons: Recognize and apply naming conventions for alkanes, alkenes, and alkynes based on their carbon chain structures and bonding. ● Describe and name functional group-containing compounds: Navigate through the nomenclature of alcohols, ethers, aldehydes, ketones, carboxylic acids, and amines, understanding their key functional groups. ● Explain the structure and naming of benzene derivatives: Understand the unique properties of benzene and how its derivatives are named and represented structurally. ● Distinguish between major classes of biological compounds: Identify lipids, carbohydrates, and proteins, appreciating their structural diversity and significance in living organisms. ● Apply structural representation techniques: Use structural formulas to accurately represent the molecular structure of various organic compounds. A. Hydrocarbons Hydrocarbons, the cornerstone of organic chemistry, constitute a vast family of compounds composed solely of hydrogen and carbon atoms. These simple yet versatile molecules form the structural basis of At the end of this chapter, you should be able to:

organic compounds, ranging from the familiar methane in natural gas to the complex structures found in proteins and plastics. Classically categorized into alkanes, alkenes, and alkynes, hydrocarbons serve as the fundamental building blocks for more intricate organic molecules.

Aromatic Hydrocarbons

Alkanes

Alkenes

Alkynes

Characterized only by single bonds between carbon atoms C–C . Alkanes are relatively non-reactive and are excellent fuels.

Characterized by having at least 1 double bond C=C .

Characterized by having at least one carbon-carbon triple bond C≡C .

Aromatic hydrocarbons, also known as arenes, consist of carbon atoms arranged in planar, cyclic structures.

Notable

● Structural representation in chemistry refers to the graphical depiction of a molecule’s arrangement, indicating the connectivity of its atoms and the type of bonds between them.

EthaneC 2 H 6

EtheneC 2 H 4

EthyneC 2 H 2

B. Structural Representation The structural representation of hydrocarbons is crucial in unraveling the intricate world of organic chemistry. In essence, it involves creating visual blueprints that showcase how carbon and hydrogen atoms are connected within these compounds and the types of bonds they form.

Name

Representation

Example (propane)

It uses chemical symbols to indicate the elements present and subscript numbers to denote the quantity of each type of atom in the molecule.

C 3 H 8

Molecular Formula

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