Understanding Advanced Chemistry Through Problem Solving

The Learner's ApproachVolume 1: Physical Chemistry and Inorganic Chemistry

Kim Seng Chan, Jeanne Tan

• Publisher: WSPC
• Year: 2014
• ISBN:
  9789814578929
• Topic: Physical Sciences
• Subtopic: Inorganic Chemistry

Written for students taking either the University of Cambridge Advanced Level examinations or the International Baccalaureate examinations, this guidebook covers essential topics and concepts under both stipulated chemistry syllabi. The book is written in such a way as to guide the reader through the understanding and applications of essential chemical concepts using the problem solving approach. The authors have also retained the popular discourse feature from their previous two books — Understanding Advanced Physical Inorganic Chemistry and Understanding Advanced Organic and Analytical Chemistry — to help the learners better understand and see for themselves, how the concepts should be applied during solving problems. Based on the Socratic Method, questions are implanted throughout the book to help facilitate the reader's development in forming logical conclusions of concepts and the way they are being applied to explain the problems. In addition, the authors have also included important summaries and concept maps to help the learners to recall, remember, reinforce and apply the fundamental chemical concepts in a simple way.

Topics are explored through an explanatory and inquiry-based approach. They are interrelated and easy to understand, with succinct explanations/examples being included, especially on areas that students frequently find difficult. Topics address the whys and hows behind key concepts to be mastered, so that the concepts are made understandable and intuitive for students. The focus is on conceptual learning so as to equip students with knowledge for critical learning and problem solving.

Existing A-level or IB guidebooks generally introduce concepts in a matter-of-fact manner. This book adds a unique pedagogical edge which few can rival. Through their many years of teaching experiences, the authors have acquired a sound awareness of common students' misconceptions which are relayed through the questions and thus help to reinforce concepts learnt. This book is essential and useful to help the students to be adequately prepared for their high stake examinations.

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Contents:

• Part I: Physical Chemistry:
  • Atomic Structure and the Periodic Table
  • Chemical Bonding
  • Ideal Gas and Gas Laws
  • Chemical Thermodynamics
  • Reaction Kinetics
  • Chemical Equilibria
  • Ionic Equilibria
  • Redox Chemistry and Electrochemical Cells
• Part II: Inorganic Chemistry:
  • The Periodic Table: Chemical Periodicity
  • Chemistry of Groups 2 and 7
  • Introduction to Transition Metals and Their Chemistry

Readership: JC students and teaching professionals in Chemistry.
Key Features:

• The book provides fundamental important scaffolding to aid students in creating their own understanding of the chemical concepts
• The book encourages critical thinking and meaningful applications, using the basic concepts learnt
• The book guides the students to integrate the various concepts they have learnt into a coherent and meaningful conceptual network

PART I

PHYSICAL CHEMISTRY

CHAPTER 1

ATOMIC STRUCTURE AND THE PERIODIC TABLE

1.	Naturally occurring boron consists of two isotopes, ^10B and ^11B, having abundances of 19.7% and 80.3%, respectively.
	(a)	Explain the terms isotope and relative isotopic mass.

Explanation for isotope:

An element may consist of two or more atoms which have the same number of protons, also known as the atomic number, but different number of neutrons. These atoms are known as isotopes.

Do you know?

—The number of protons is equivalent to the number of electrons for isotopes. Hence, an isotope is an electrically neutral species.

—Isotopes have the same chemical properties as they have identical electronic configuration, and chemical reaction only involves the movement of electrons. The nucleus is intact during a chemical reaction.

—Isotopes have different physical properties such as melting point and boiling point. Isn’t it more difficult to vaporize a heavier atom from its liquid state because of its heavier mass?

Explanation for relative isotopic mass:

Relative isotopic mass is the mass of one atom of the isotope of an element relative to 1/12 of the mass of one atom of ¹²C.

Do you know?

—Relative isotopic mass is a dimensionless quantity as it is measured relatively to the mass of one atom of ¹²C.

—The difference in the masses of isotopes arises because of the difference in the number of neutrons. The sum of protons and neutrons is known as the mass number or nucleon number.

—The value is similar to the mass number of the isotope, which is sum of protons and neutrons. This is because the bulk mass of an atom is attributed to what is present in the nucleus.

—The mass of an isotope seems to be a whole number. This is not true because in reality, the actual relative isotopic mass is less than the mass of all nucleons added up. This phenomenon is known as mass defect. The difference in the masses, which is less than 1%, arises because part of the mass has been converted into binding energy according to E = mc², which is necessary to hold the nucleons together in the nucleus.

—Relative isotopic mass can be determined using mass spectrometry.

Q	Why is ^12C used as the reference standard?

A:Avogadro’s number or Avogadro’s Constant (N_A) is a common constant used in both chemistry and physics. Avogadro’s number is formally defined as the number of carbon-12 atoms in 12 g of carbon-12, which is approximately 6.022 × 10²³. Historically, carbon-12 was chosen as the reference standard because its atomic mass could be measured with particular accuracy. In addition, carbon-12 is commonly present in many substances.

(b)	Calculate the relative atomic mass of naturally occurring boron.

Explanation:

The relative atomic mass (A_r) of an element is dependent on (i) whether it has more than one isotope, and (ii) the composition of the various isotopes. Hence, to determine the relative atomic mass, we need the following formula:

A_r = Σ(Percentage composition × Relative isotopic mass)

Thus, A_r of boron = (0.197 × 10 + 0.803 × 11) = 10.8.

Do you know?

—Since the dimensionless relative isotopic mass is used in the calculation of the relative atomic mass, the latter is also a dimensionless...

Table of contents

• Cover Page
• Title Page
• Copyright Page
• Contents
• Preface
• Acknowledgements
• Part I Physical Chemistry
• Part II Inorganic Chemistry
• Index