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16485 results in Anthem Press

Page 364 of 825

The 'Imagined Sound' of Australian Literature and Music
  • Edited by Joseph Cummins
  • Published by:
    Anthem Press
    Published online:
    18 September 2019
    Print publication:
    20 September 2019
  • 'Imagined Sound' is a unique cartography of the artistic, historical and political forces that have informed the post-World War II representation of Australian landscapes. It is the first book to formulate the unique methodology of 'imagined sound', a new way to read and listen to literature and music that moves beyond the dominance of the visual, the colonial mode of knowing, controlling and imagining Australian space. Emphasising sound and listening, this approach draws out and re-examines the key narratives that shape and are shaped by Australian landscapes and histories, stories of first contact, frontier violence, the explorer journey, the convict experience, non-Indigenous belonging, Pacific identity and contemporary Indigenous Dreaming. 'Imagined Sound' offers a compelling analysis of how these narratives are reharmonised in key works of literature and music.

IB Chemistry Revision Guide
  • Edited by Ray Dexter
  • Published by:
    Anthem Press
    Published online:
    18 September 2019
    Print publication:
    16 September 2019
  • A very challenging subject IB chemistry requires tremendous effort to understand fully and attain a high grade. 'IB Chemistry Revision Guide' simplifies the content and provides clear explanations for the material.

  • 14 - Option B: Biochemistry

  • Edited by Ray Dexter
  • Book:
    IB Chemistry Revision Guide
    Published by:
    Anthem Press
    Published online:
    18 September 2019
    Print publication:
    16 September 2019, pp 178-201

  • Summary

    This covers the material in Option B: Biochemistry.

    CORE

    SPREAD 1: Introduction to biochemistry

    The diverse functions of biological molecules depend on their structures and shapes.

    Metabolic reactions take place in highly controlled aqueous environments.

    Reactions of breakdown are called catabolism, and reactions of synthesis are called anabolism.

    Biopolymers form by condensation reactions and are broken down by hydrolysis reactions.

    Photosynthesis is the synthesis of energy-rich molecules from carbon dioxide and water using light energy.

    Respiration is a complex set of metabolic processes providing energy for cells.

    What is biochemistry?

    It's the branch of science concerned with the chemical and physico-chemical processes and substances that occur within living organisms, in other words, the chemistry of the body.

    This mainly involves organic reactions, but there are inorganic aspects to some reactions. Given that molecules involved in biological function are inevitably organic and organic molecules have functional groups at specific locations on the chain, it is no surprise that a lot of the functions of these biological molecules depend on their structure and their shape. The intermolecular forces, in particular hydrogen bonds, are also of great importance.

    The other significant factor to understand is that the solvent in which the reactions are carried out is also crucial. It's water of course, water that is under a very tight set of conditions. Water is a solvent, a reagent, a coolant, a temperature control and a transport medium.

    A few significant terms:

    Metabolism— these are the name given to the set of chemical reactions that happen in cells that are crucial for sustaining reactions. They are also known as metabolic reactions.

    These metabolic reactions can be further broken down into:

    Catabolism: reactions where organic matter is broken down to use for in respiration and other energy-based needs.

    Anabolism: reactions where new molecules are made from the energy provided by catabolic reactions, such as proteins or nucleic acids.

    Biopolymers— these are, as the name suggests, polymers found in organisms: there are three sorts— polysaccharides, poly peptides (proteins) and polynucleotides (DNA, RNA). As with all condensation polymers they can be broken down by hydrolysis reactions (reaction with water) and can be created by the elimination of a small molecule from between the polymers: more later.

    Photosynthesis— the synthesis of energy-rich molecules (like sugars) from carbon dioxide and water using light energy.

  • 9 - Acids and Bases

  • Edited by Ray Dexter
  • Book:
    IB Chemistry Revision Guide
    Published by:
    Anthem Press
    Published online:
    18 September 2019
    Print publication:
    16 September 2019, pp 92-105

  • Summary

    This chapter covers the IB syllabus content in Sections 8 and 18.

    SPREAD 1: What is an acid?

    A Bronsted–Lowry acid is a proton/H+ donor and a Bronsted–Lowry base is a proton/H+ acceptor.

    Introduction

    Acids and bases have been known about since ancient times, although defining precisely what an acid and a base is perhaps a little harder.

    The most useful definition of an acid for IB students is the Brønsted–Lowry definition:

    An acid is a proton donor. By proton here we mean a hydrogen ion (H+) that consists only of a proton.

    A base is a proton acceptor. By this we usually mean a compound that contains hydroxide ions (OH-) that can accept a proton to form water.

    In more simple terms an acid is a compound that releases hydrogen ions when dissolved in water. The technical term for this is DISSOCIATION.

    It is often easier to see this in terms of equations:

    The HCl donates its proton to the OH-ion in the base to form water.

    As an ionic equation:

    More complicated examples of acid–base behavior still fit the same, simple, logical ionic equation. For example, in the generation of an electrophile for benzene in the organic section (Chapter 11).

    Here the sulfuric acid acts as an acid and the nitric acid acts as the base! The donated proton is shown in bold.

    Products of neutralization

    Reactions involving acids and bases produce compounds called “salts.” Such reactions are known as neutralization reactions. Salts are more properly defined as “compounds where the H+ of an acid has been replaced by another positive ion.”

    An alkali is a subgroup of bases that are soluble in water.

    Some typical acids

    The three common mineral acids are:

    Hydrochloric acid (HCl)

    Sulfuric acid (H2SO4)

    Nitric acid (HNO3)

    Knowing the formulas of these three acids is considered absolutely essential for any chemistry course.

    There are thousands of weak acids. Their structures and reactions will be looked at in more detail in the organic chemistry course, but it is important that when writing equations with such acids you show exactly which hydrogen is donated.

  • 16 - Medicinal Chemistry

  • Edited by Ray Dexter
  • Book:
    IB Chemistry Revision Guide
    Published by:
    Anthem Press
    Published online:
    18 September 2019
    Print publication:
    16 September 2019, pp 222-238

  • Summary

    This chapter covers the material covered in Option Module D: Medicinal Chemistry.

    CORE

    SPREAD 1: Pharmaceutical products and drug action

    In animal studies, the therapeutic index is the lethal dose of a drug for 50% of the population (LD50) divided by the minimum effective dose for 50% of the population (ED50).

    In humans, the therapeutic index is the toxic dose of a drug for 50% of the population (TD50) divided by the minimum effective dose for 50% of the population (ED50).

    The therapeutic window is the range of dosages between the minimum amounts of the drug that produce the desired effect and a medically unacceptable adverse effect.

    Dosage, tolerance, addiction and side effects are considerations of drug administration.

    Bioavailability is the fraction of the administered dosage that reaches the target part of the human body.

    The main steps in the development of synthetic drugs include identifying the need and structure, synthesis, yield and extraction.

    Drug–receptor interactions are based on the structure of the drug and the site of activity.

    Basics: What is a drug or medicine?

    These are chemicals that have a known biological effect on humans or other animals. In the positive sense drugs and medicines are substances that can cure, prevent or help diagnose disease, or enhance physical well-being. Drugs of course can be misused for recreational purposes, especially hallucinogens.

    All drugs have side-effects, an effect the drug has on the body that is secondary to the one intended. These can have adverse effects, or can be beneficial. Sometimes side-effects are of great concern, some will be minor. The seriousness of the disease the drug is being used for will affect the amount of side-effects tolerated in the drug.

    Methods of administering drugs

    It is important that drugs get into the blood stream as quickly as possible in order for them to reach the site where their effects will be needed. This can be via the stomach, lungs or directly into the bloodstream.

    There are five common ways in which drugs can be administered.

  • • Orally— in the form of tablets or medicines.

  • • Inhalation— in the form of nasal sprays.

  • • Via the skin— for treatment of skin conditions and other localized irritation.

  • 2 - Stoichiometric Relationships

  • Edited by Ray Dexter
  • Book:
    IB Chemistry Revision Guide
    Published by:
    Anthem Press
    Published online:
    18 September 2019
    Print publication:
    16 September 2019, pp 7-14

  • Summary

    This chapter's contents refer to the material covered in Topic 1 of the IB Chemistry Specification.

    SPREAD 1: Writing formulae

  • • Atoms of different elements combine in fixed ratios to form compounds, which have different properties from their component elements.

  • • Mixtures contain more than one element and/or compound that are not chemically bonded together and so retain their individual properties.

  • • Mixtures are either homogeneous or heterogeneous.

  • • Calculating relative molecular mass (RMM). Molar mass (Mr) has the units g mol-1.

    • You can't begin a chemistry course until you have these basic ideas sorted out. Simplistically there are three types of substance: element, compound and mixture.

    Elements are substances made of only one type of atom. Elements cannot be broken down into anything simpler that will have a form of chemical existence. They behave differently from their constituent elements. For example, table salt (sodium chloride) is a relatively benign white solid that isn't toxic, whereas the elements sodium and chlorine are both very dangerous, as we will see.

    Compounds are substances made of two or more elements chemically bonded together (see Chapter 4). Compounds can be written in the form of chemical formulae. This shows the fixed ratio of elements in the compound. For example, in magnesium carbonate, the formula is MgCO3— one magnesium, one carbon and three oxygens.

    What is the difference between copper sulfide and copper sulfate?

    In simple terms “ide” can be taken to mean combined in a compound, so copper sulfide is just copper and sulfur CuS. “Ate” can be taken to mean “with oxygen as well,” so copper sulfate is CuSO4. The exact nature of “ate” will be discussed further in the chapter on bonding.

    Mixtures are elements or compounds (or both) chemically uncombined. Mixtures that contain chemicals in the same chemical state are called homogeneous (from the Greek hom.— the same, genou.— combining from). A good example is air. Heterogenous mixtures contain chemicals in different states (heter.— different). An example would be sea water. As the components in a mixture are not chemically combined they retain their individual characteristics.

    Substances can occur in three states: solid (s), liquid (l) and gas (g). If you have a solution (a mixture of a substance dissolved in water) then it is called aqueous (aq) (from the Latin via French for water). These bracketed signs should appear next to any chemical formulae in equations.

  • 1 - Measurement and Data Processing

  • Edited by Ray Dexter
  • Book:
    IB Chemistry Revision Guide
    Published by:
    Anthem Press
    Published online:
    18 September 2019
    Print publication:
    16 September 2019, pp 1-6

  • Summary

    This chapter's contents refer to the material covered in Topics 11.1 and 11.2 of the IB Chemistry Specification.

    CORE

    SPREAD 1: Uncertainties and errors in measurement and results

    Qualitative data includes all non-numerical information obtained from observations not from measurement.

    Quantitative data are obtained from measurements, and are always associated with random errors/uncertainties, determined by the apparatus, and by human limitations such as reaction times.

    Propagation of random errors in data processing shows the impact of the uncertainties on the final result.

    Introduction

    All lab work in any science subject isn't perfect. Mistakes will be made. Some will be human error; some will be related to the equipment used. No experimental result has true validity unless these errors are acknowledged and worked into any result. Remember, an error is something that prevents you from getting the true, correct result.

    Before we look at the errors let's clarify a few terms related to lab work:

    Qualitative data: This is all information obtained from observations not from measurement. For example, a color change or the formation of a precipitate is a qualitative observation. There can be no mathematical content to such observations.

    Quantitative data: This is where the numbers come in. This data is obtained from measurements and often requires mathematical processing.

    In experiments we typically measure a variable. The independent variable is affected when another variable is changed (the dependent variable). For example, in an experiment to measure how temperature affects the speed of a reaction, the independent variable is the temperature and the dependent variable would be the measured time.

    Although errors can be made in recording qualitative data, the majority of errors are associated with quantitative data.

    What sort of errors are there?

    Essentially three types of error exist:

    Systematic error: These are errors that are due to the procedure or equipment you have used. For example, an experiment to measure the quantity of gas produced (see Chapter 7) will have to overcome the gap between mixing the reagents and the gas hitting a gas syringe. Some gas will be lost. As this would be a fault of the procedure the error should be the same each time.

  • 7 - Chemical Kinetics

  • Edited by Ray Dexter
  • Book:
    IB Chemistry Revision Guide
    Published by:
    Anthem Press
    Published online:
    18 September 2019
    Print publication:
    16 September 2019, pp 75-83

  • Summary

    This chapter covers material from Topics 6 and 16 of the IB syllabus.

    CORE

    SPREAD 1: Collision theory and rates of reaction

    Species react as a result of collisions of sufficient energy and proper orientation.

    The rate of reaction is expressed as the change in concentration of a particular reactant/product per unit time.

    Concentration changes in a reaction can be followed indirectly by monitoring changes in mass, volume and color.

    Introduction

    Chemical reactions occur: we know that, but one of the truths of all chemical reaction is that we can have some influence in how quickly the reaction goes.

    Kinetics is a topic that has almost certainly been met in studying chemistry on prior courses and this book will not dwell on the basics, although there are essentially five ways in which this can be sped up:

  • • Increasing the concentration of one or more of the reagents.

  • • Increasing the temperature at which the experiment is carried out.

  • • Increasing the pressure exerted on gaseous reagents.

  • • Increasing the surface area of solid reactants.

  • • Adding a suitable catalyst.

    • Students would not be expected to recall these but might be expected to recall why they affect reaction rate.

    For a chemical reaction to occur reactant particles (which could be atoms, molecules, ions or radicals) must collide in the right orientation and with sufficient energy. All chemical reactions have an activation energy that is uniquely associated with it (see previous chapter); this must be overcome if the collision is to be successful. The orientation is related to precisely where the collision occurs on each molecule. This is less relevant for ions, which are often spherical but for complicated organic molecules only one small part of the molecule might actually be “reactive” to the other reagent.

    What is rate of reaction?

    Students often get confused as to what reaction rate actually is, confusing it with time. Reaction rate is the speed of the chemical reaction, and it is usually expressed as the change in concentration of a particular reactant/product per unit time:

    For example, moldm-3s-1

    However if a reaction is particularly slow this could be changed to be per minute, or even per hour.

Page 364 of 825