Basic Principles of Inorganic Chemistry: Making the Connections
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This book is ideal for students taking chemistry as a subsidiary subject as well as honours degree students.InhaltsverzeichnisMoles and Molarity The Structure of the Atom Electron Configuration and the Build-up to the Periodic Tabl.
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- Title
- Basic Principles of Inorganic Chemistry: Making the Connections
- Author
- Hathaway, Brian J.|Murphy, Clair|Murphy, Brian
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- ROYAL SOCIETY OF CHEMISTRY
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- 1998
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- New
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- Soft cover
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- English
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- 0854045740
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- 9780854045747
General chemistry textbooks are usually lengthy and present chemistry to the student as an unconnected list of facts. In inorganic chemistry, emphasis should be placed on the connections between valence shell electron configuration and the physical and chemical properties of the element. Basic Principles of Inorganic Chemistry: Making the Connections is a short, concise book that emphasises these connections, in particular the chemistry of the Main Group compounds. With reference to chemical properties, Lewis Structures, stoichiometry and spider diagrams, students will be able to predict or calculate the chemistry of simple polyatomic compounds from the valence shell configuration and will no longer be required to memorise vast amounts of factual chemistry. This book is ideal for students taking chemistry as a subsidiary subject as well as honours degree students.
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Basic Principles of Inorganic Chemistry
Making the Connections
By Brian Murphy, Clair Murphy, Brian J. HathawayThe Royal Society of Chemistry
All rights reserved.
Contents
Chapter 1 Moles and Molarity, 1,
Aims and Objectives, 1,
States of Matter, 1,
Elements, Atoms and Molecules, 1,
Elements, Mixtures and Compounds (Molecules), 2,
Simple Chemical Names, 3,
Cations and Anions, 3,
Types of Chemical Formula, 4,
Atomic Weight, 4,
Avogadro's Number, 5,
Empirical Formula, 5,
Chemical Equations, 6,
Balancing Chemical Equations, 7,
Molar Solutions, 8,
Volumetric Reactions, 9,
Volumetric Titrations, 10,
Limiting Reactions, 11,
Worked Example No. 1, 11,
Worked Example No. 2, 13,
Chapter 2 The Structure of the Atom, Electron Configuration and the Build-up to the Periodic Table, 14,
Aims and Objectives, 14,
The Structure of the Atom, 14,
Bohr Model of the Atom, 17,
The Build-up Process for the Periodic Table, 27,
Chapter 3 The Physical Properties of the Elements and the Periodic Table, 31,
Aims and Objectives, 31,
The Periodic Table, 31,
Variation in the Atomic Radii, 34,
Variation in the Ionisation Potentials, 34,
Variation in the Electron Affinities or Attachment Enthalpies, 37,
Summary, 38,
Chapter 4 Chemical Properties of the Elements and the Periodic Table, 39,
Aims and Objectives, 39,
Introduction, 39,
Characteristic or Group Oxidation Numbers, 41,
Oxidation Numbers, 43,
Rules for the Determination of Oxidation Numbers, 44,
Main Group Variable Valence, 44,
Transition Metal Variable Valence, 46,
Chemical Stoichiometry, 49,
The Calculation of Chemical Stoichiometry Factors – Worked Examples, 51,
Redox Reactions, 52,
Covalent Bonds, 53,
Polyatomic Covalent Molecules, 56,
Molecular Orbital Theory of Diatomic Molecules, 56,
Bond Order, 60,
Chapter 5 The Lewis Structures of Molecules, Cations and Anions, Including Oxyanions, 61,
Aims and Objectives, 61,
Introduction, 61,
The Working Method for Drawing Lewis Structures, 64,
Example 1: Methane (CH4) and Carbon Tetrachloride (CCl4), 65,
Example 2: The Ammonium Cation (NH4-) and the Tetrafluorborate Anion (BF4-), 66,
Example 3: Ammonia (NH3) and Water (OH2), 68,
Example 4: Beryllium Dihydride (BeH2) and Boron Trifluoride (BF3, 69,
Example 5: Phosphorus Pentchloride (PCl5) and Sulfur Hexafluoride (SF6), 70,
Example 6: l,l,-Dichloromethanone (C12CO) and Ethene (C2H4), 71,
Example 7: Ethyne (C2H2), 73,
The Oxyacids and Oxyanions of the Main Group Elements, 74,
The Position of the Hydrogen Atoms in the Oxyacids, 74,
The Free Valence of the Terminal Oxygen Atoms, 76,
Resonance in the Structures of the Oxyanions, 78,
The Application of the Working Method to the Lewis Structures of the Oxyanions, 79,
Example 1: Carbonic Acid, H2CO3, 79,
Example 2: Sulfuric Acid, H2SO4, 81,
The Use of Formal Charges, 84,
Summary, 86,
Chapter 6 Shape and Hybridisation, 88,
Aims and Objectives, 88,
The Shapes of Covalent Molecules, 88,
The Working Method for Using VSEPR Theory, 92,
Deviations from Regular Shapes, 94,
The Advantages of VSEPR Theory, 95,
The Disadvantages of VSEPR Theory, 95,
The Shape of Dinuclear Molecules, 95,
Hybridisation of Atomic Orbitals, 99,
Hybridisation in Polynuclear Molecules, 104,
Summary, 106,
Chapter 7 A Features of Interest Approach to Systematic Inorganic Chemistry, 107,
Aims and Objectives, 107,
Introduction, 107,
The Preparation of Simple Compounds from the Elements, 109,
The Reactions of Simple Compounds, 113,
Reaction with Water, 113,
Volumetric Reactions, 114,
The Effect of Heat, 115,
Features of Interest of Simple Compounds – Working Method, 116,
The Applicaton of the Working Method to a Selection of Simple Compounds,
Example 1: Methane, (CH4), 119,
Example 2: Hydrochloric Acid (HCl), 120,
Example 3: Sodium Chloride (NaCl), 121,
Example 4: Phosphorus Pentachloride (PCl5), 122,
Example 5: Copper (II) Oxide, (CuO), 123,
Example 6: Iron (II) Chloride (FeCl2), 124,
Example 7: Iron (II) Sulfate Hexahydrate ([Fe(OH2)6]SO4), 125,
Example 8: Carbonic Acid (H2CO3), 126,
Writing an Essay or Report from a Spider Diagram, 128,
Conclusions, 130,
Suggested Ways Forward, 130,
Phase II – Features of Interest, 130,
Phase III – Features of Interest, 131,
The Advantages of the Features of Interest Approach, 139,
The Disadvantages of the Features of Interest Approach, 139,
Appendices, 144,
Periodic Table of the Elements, 148,
Subject Index, 149,
CHAPTER 1
Moles and Molarity
AIMS AND OBJECTIVES
This introductory chapter describes the simple ideas of atoms and molecules, types of chemical formula and their molecular weight for students who have not studied chemistry before. Chemical equations and balanced chemical equations are introduced through the reactions used in an introductory practical laboratory course. The concepts of molarity and molar solutions are introduced through solving volumetric problems, to enable the student to start a laboratory course in practical Inorganic Chemistry.
STATES OF MATTER
Chemistry is the science and study of the material world. It is generally accepted that there are three states of matter, solid, liquid and gaseous, and the chemicals that make up the materials of the world involve the chemical elements or molecules.
ELEMENTS, ATOMS AND MOLECULES
The physical state of an element relates to the three states of matter, and the precise state for an element is largely determined by the temperature. Thus at room temperature the element iron is a solid, bromine is a liquid and fluorine is a gas.
In the gaseous state at room temperature helium (He) is a mono-atomic gas, and the formula of the element helium is written as He. However, the gaseous form of hydrogen and oxygen at room temperature involves diatomic molecules, namely, H2 and O2. This difference is largely determined by the individual electron configuration of the elements, and their ability to form bonds to each other, rather than remain (in the gaseous state) as atomic species of the elements.
The way in which the elements of the Periodic Table react together is largely determined by the electron configuration of the individual elements as this determines the ratio in which two elements combine to form a molecule:
Atom 1 + Atom 2 [right arrow] Molecule H + Cl [right arrow] HCl 2 Atom H + 1 Atom O [right arrow] 1 Molecule H2O
The number of atoms of each element in a molecule determines the ratio of the elements in the molecule and is referred to as the stoichiometry of the molecule. In the molecule of HCl the ratio of H:Cl is 1:1, and the molecule has a stoichiometry of 1:1. In H2O the ratio of H:O is 2:1, and its stoichiometry is 2:1.
ELEMENTS, MIXTURES AND COMPOUNDS (MOLECULES)
An element consists of only one type of atom, i.e. helium, hydrogen or iron. A mixture may contain more than one type of substance that can be physically separated into its components, whereas a compound contains more than one type of element, usually with a definite stoichiometry, and cannot be separated into its elements by any simple physical method. Thus the element iron may be obtained as a magnetic black powder that can be mixed with yellow sulfur to give a blackish yellow mixture, from which the iron metal can be separated by means of a magnet. However, if the mixture is heated, a reaction occurs to give a black solid of FeS, iron(II) sulfide, on cooling, from which the iron present cannot be separated by the use of a magnet. The black solid FeS is referred to as a compound of Fe and S which has lost the properties of the elemental Fe and S and has unique properties of its own. Similarly, molecules of H2 and O2 react to give molecules of water, H2O:
2H2(g) + O2(g) [right arrow] 2H2O(1)
but while H2 and O2 are gases at room temperature, H2O is a liquid. In these new compounds the compound elements are said to have reacted chemically together to give a new compound, FeS and H2O, respectively, with definite stoichiometries between the atoms, namely, 1:1 in FeS and 2:1 in H2O.
SIMPLE CHEMICAL NAMES
The most simple compounds are those which contain only two elements, one metallic and one non-metallic (explained later). The metal is given the full element name, and the non-metal has the ending -ide.
Thus: NaCl sodium chloride
MgO magnesium oxide
CaS calcium sulfide
BN boron nitride
If the stoichiometry of the two elements is not 1:1, prefixes are used thus:
1:1 mono – carbon monoxide CO
1:2 di – carbon dioxide CO2
1:3 tri – sulfur trioxide SO3
1:4 tetra – carbon tetrachloride CCl4
1:5 penta – phosphorus pentachloride PCl5
1:6 hexa – sulfur hexafluoride SF6
Note: where more than one atom is present the number is written as a post-subscript.
Compounds with more than two elements cannot end in -ide and for those where the third element is oxygen, the endings -ite or -ate are used:
magnesium sulfide MgS
magnesium sulfite MgSO3
magnesium sulfate MgSO4
CATIONS AND ANIONS
In compounds such as NaCl, the lattice is made up of cations (positively charged species) of Na+ and anions (negatively charged species) of Cl-, Na+Cl-, such that the formula, NaCl, has an overall neutral charge. In Na2SO4 the overall neutral charge is maintained, but the compound contains two Na+ cations to one SO42- anion, with the latter referred to as an oxyanion, in this case a sulfate oxyanion. In aqueous solution the oxyanions occur as discrete species, in the case of the sulfate anion with a 2 – negative overall charge.
TYPES OF CHEMICAL FORMULA
In chemistry, different types of chemical formula are used to give different types of information.
(a) Empirical Formula: this is the simplest whole number ratio of the atoms in a molecule; thus in ethanoic acid the empirical formula is CH2O.
(b) Molecular Formula: this is the actual number of atoms making up the molecule; thus in ethanoic acid the molecular formula is C2H4O2i.e. twice the empirical formula.
(c) Structural Formula: this shows the various ways of representing the actual arrangement of atoms in the molecule, i.e.
[FORMULA NOT REPRODUCIBLE IN ASCII]
ATOMIC WEIGHT
The atomic weight or relative atomic mass of an element is the mass of one atom of that element relative to that of the most abundant form of carbon taken as 12 units. On this scale the atomic weight of hydrogen is 1, oxygen is 16, and copper is 63.54a.m.u. Table 1.1 lists the atomic weights of the first 18 elements of the Periodic Table.
On this scale the molecular formula of ethanoic acid, C2H4O2 has a molecular weight of:
2C(12) + 4H(1) + 20(16), i.e. (24 + 4 + 32 = 60)
namely, 60 atomic mass units (a.m.u.), i.e. the gram mole or molecular weight of ethanoic acid is 60. The gram mole of ethanoic acid is then 60 g and contains:
24 gram atoms of carbon
4 gram atoms of hydrogen
32 gram atoms of oxygen
Total: 60 grams.
AVOGADRO'S NUMBER
As the gram mole of a molecule (60 for ethanoic acid) is defined relative to the gram atom of carbon = 12 g, the actual number of atoms in 12 g carbon has been experimentally determined as 6.022 x 1023 atoms. This is referred to as Avogadro's Number, and is the number of atoms in the gram atomic weight of any element, i.e. 19 g fluorine, 32 g sulfur or 63.5 g copper. It then follows that the number of molecules in the gram molecular weight of a molecule (1 gram mole) is also 6.022 x 1023, Avogadro's Number. Thus one mole of ethanoic acid, 60 g, contains 6.022 x 1023 molecules of ethanoic acid. Equally, one mole of dihydrogen, H2, 2g, one mole of water, H2O, 18 g, and one mole of sulfuric acid H2SO4, 98 g, each contains 6.022 x 1023 molecules.
It also follows that 1 g of a molecule will contain Avogadro's Number divided by the gram molecule weight (1 mole) of the molecule:
[??] 1 g ethanoic acid contains 6.022 x 1023/60 molecules = 1.0037 x 1022 molecules
Likewise:
1 g hydrogen (0.5 1 gram mole) contains 3.011 x 1023 molecules 1 g sulfuric acid (1/98 1 gram mole) contains 6.145 x 1021 molecules.
EMPIRICAL FORMULA
This only expresses the relative number of atoms of each element in a compound. Nevertheless, it is the first step in the experimental determination of the molecular formula of a compound from its percentage composition.
1. Thus: A contains 42.9% C and 57.1% O; calculate its empirical/molecular formula
Atomic Wt. % %/At. Wt.Ratio
Carbon 12 42.9 42.9/12 = 3.58 1
Oxygen 16 57.1 57.1/16 = 3.58 1
[??] Empirical formula is C1 O1, or CO (carbon monoxide).
2. A contains 79.9% C and 20.1YO H:
Atomic Wt. % %/At. Wt.Ratio
Carbon 12 79.9 79.9/12 = 6.67 1
Hydrogen 1 20.1 20.1/1 = 20.1 3 CH3
3. A contains 37.5% C; 12.5% H; 50.0% O:
Atomic Wt. % %/At. Wt.Ratio
Carbon 12 37.5 37.5/12 = 3.12 1
Hydrogen 1 12.5 12.5/1 = 12.5 4
Oxygen 16 50.0 50.0/16 = 3.12 1 CH4O
4. A contains 43.7% P; 56.3% O:
Atomic Wt. % %/At. Wt.Ratio
Phosphorus 31 43.7 43.7/31 = 1.4 2
Oxygen 16 56.3 56.3/16 = 3.5 5 P2O5
5. Given the molecular formula of ethanoic acid, CH3CO2H what percentages of C, H and N are present?
CH3CO2H [equivalent to] C2H4O2 [equivalent to] 2 x CH2O
Empirical weight = 12 + 2 + 16 = 30 and the molecular weight = 24 + 4 + 32 = 60.
% C = 24/60 x 100 = 40.0% C
% H = 4/60 x 100 = 6.67% H
% O = 32/60 x 100 = 53.3% O
CHEMICAL EQUATIONS
Chemistry involves the study of the ways in which the elements and compounds react with each other. We have already seen:
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in which two pairs of elements react to form a compound. Some more complicated balanced equations are:
[FORMULA NOT REPRODUCIBLE IN ASCII]
Notice because of the balancing of charges, 1 mole of each of the reactants produces 2 moles of NaCl. Equally:
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Such reactions contain a great deal of information; thus in the reaction:
[FORMULA NOT REPRODUCIBLE IN ASCII]
could be represented alternatively:
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in a structural notation. It also contains more quantitative information:
1. 1 mole N2 reacts with 3 moles H2 to give 2 moles NH3;
2. 28g (1 mole) N2 reacts with 6g (3 moles) H2 to give 34g (2 moles) NH3;
3. 1 g N2 requires 6/28 g H2 for complete reaction to give 34/28 g NH3;
4. 1 g N2 in excess H2 will only yield 34/28 g NH3.
BALANCING CHEMICAL EQUATIONS
Such chemical equations must obey certain rules:
1. The reactants are written to the left-hand side, LHS, the products to the right-hand side, RHS, of the reaction arrow [right arrow].
2. Each side of the equation must have the same number of each kind of atoms, i.e. the equation must balance.
3. The common gaseous elements are shown as diatomic – H2, O2, N2, C12 – and solid elements as atoms – C, P, S, Cu or alternatively as C∞, P4, S8, Cu∞.
4. The overall ionic charges must be the same on each side of the equation.
For example, to balance the equation:
Al + HCl [right arrow] AlCl3 + H2.
steps 1–4 must be followed:
1. The products involve 3Cl, while the reactants involve only 1Cl [??] Al + 3HCl [right arrow] AlCl3 + H2
2. The reactants involve 3H, the products 2H [??] Al + 2 x 3HCl [right arrow] AlCl3 + 3H2
3. The reactants involve 6Cl, the products 3Cl [??] 2Al + 6HCl [right arrow] 2AlCl3 + 3H2
and the equation is now balanced.
(Continues...)
Excerpted from Basic Principles of Inorganic Chemistry by Brian Murphy, Clair Murphy, Brian J. Hathaway. Copyright © 1998 The Royal Society of Chemistry. Excerpted by permission of The Royal Society of Chemistry.
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- Main features of the product or service
The key features of the goods and/or services can be found in the respective quote.
- Prices and payment arrangements
5.1 The prices mentioned in the respective offers represent total prices, as do the shipping costs. They include all the price components, including all the incidental taxes.
5.2 The dispatch costs that are incurred are not included in the purchase price. They can be viewed by clicking the appropriate button on our website or in the respective quote, are shown separately over the course of the order transaction and must additionally be borne by you, insofar as free delivery is not confirmed.
5.3 The payment methods that are available to you are shown by clicking the appropriate button on our website or are disclosed in the respective quote.
5.4 Unless otherwise specified for the respective payment methods, the payment claims arising from the contract that has been concluded become payable immediately.
- Delivery conditions
6.1 The delivery conditions, delivery date and existing supply restrictions, if applicable, can be found by clicking the appropriate button on our website or in the respective quote.
Unless a different period is specified in the item description or our delivery conditions, the goods are delivered within 3-5 days after the conclusion of the contract (in case an advance payment has been agreed upon, after the payment authorisation).
6.2 If you are a consumer, the following is statutorily regulated: The risk of the sold item accidentally being destroyed or degraded during shipping only passes over to you when the item in question is delivered, regardless of whether or not the shipping operation is insured. This condition does not apply if you have independently commissioned a transport company that has not been specified by us or a person who has otherwise been appointed to execute the shipping operation.
If you are a businessman, the delivery and shipping operations take place at your own risk.
- Statutory warranty right
Liability for defects is governed by the “Warranty” provisions in our General Terms and Conditions of Business (Part I).
last update: 01.01.2022
Data protection declaration
Unless stated otherwise below, the provision of your personal data is neither legally nor contractually obligatory, nor required for conclusion of a contract. You are not obliged to provide your data. Not providing it will have no consequences. This only applies as long as the processing procedures below do not state otherwise.
“Personal data” is any information relating to an identified or identifiable natural person.
Responsible person
Contact us at any time. The contact details of the person responsible for data processing can be found in our legal notice.
Collection, processing, and transfer of personal data in orders
When you submit an order we only collect and use your personal data insofar as this is necessary for the fulfilment and handling of your order as well as processing of your queries. The provision of data is necessary for conclusion of a contract. Failure to provide it will prevent the conclusion of any contract. The processing will occur on the basis of Article 6(1) b) GDPR and is required for the fulfilment of a contract with you.
Your data is transferred here for example to the shipping companies and dropshipping providers, payment service providers, service providers for handling the order and IT service providers that you have selected. We will comply strictly with legal requirements in every case. The scope of data transmission is restricted to a minimum.
Duration of storage
After contractual processing has been completed, the data is initially stored for the duration of the warranty period, then in accordance with the retention periods prescribed by law, especially tax and commercial law, and then deleted after the period has elapsed, unless you have agreed to further processing and use.
Rights of the affected person
If the legal requirements are fulfilled, you have the following rights according to art. 15 to 20 GDPR: Right to information, correction, deletion, restriction of processing, data portability. You also have a right of objection against processing based on art. 6 (1) GDPR, and to processing for the purposes of direct marketing, according to art. 21 (1) GDPR.
Right to complain to the regulatory authority
You have the right to complain to the regulatory authority according to art. 77 GDPR if you believe that your data is not being processed legally.
Right to object
If the data processing outlined here is based on our legitimate interests in accordance with Article 6(1)f) GDPR, you have the right for reasons arising from your particular situation to object at any time to the processing of your data with future effect.
If the objection is successful, we will no longer process the personal data, unless we can demonstrate compelling legitimate grounds for the processing that outweigh your interests or rights and freedoms, or the processing is intended for the assertion, exercise or defence of legal claims.
last update: 10.01.2022