MODULE 1 UNIT 1.pdf

INCHEM 211 Department of Chemical Engineering...

INCHEM 211 Department of Chemical Engineering Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document, without Property of and for the exclusive usethe prior written of SLU. permission Reproduction, of SLU, storing is strictlysystem, in a retrieval prohibited. distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  INCHEM 211: INORGANIC CHEMISTRY Inorganic chemistry is the study of synthesis, structures, reactions as well as properties of inorganic compounds. Inorganic compounds typically refer to materials not containing carbon-hydrogen bonds, including metals, salts and minerals. Its practical applications include the development of catalysts, surfactants, coatings, fuels, materials superconductors and drugs. At the end of this course, you should be able to apply appropriate theories, principles, concepts and skills in Inorganic chemistry to your profession. To ensure that you will demonstrate the above cited learning outcomes, this course originally designed to be delivered in 54 contact hours was structured into eight modules. Each module contains several units with its own topic learning outcomes and topic outline. Each unit contains activities designed using the 5E constructivist model of learning, developed by Rodger Bybee that encourages students to engage, explore, explain, elaborate and evaluate their learning of topics covered therein. This means that at the end of each unit, each module, in the course as a whole, you will be assessed on your progress in attaining the course learning outcomes. Outcomes based education dictates that only when you can clearly demonstrate the course learning outcomes by the end of this course, can you be given a passing mark. TABLE OF CONTENTS Module 1 Foundations of Chemistry Unit 1: Introduction: Matter Unit 2: Energy Unit 3: Chemical Symbols, Notations and Nomenclature Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  MODULE 1: FOUNDATIONS OF CHEMISTRY UNIT ONE - INTRODUCTION: MATTER ENGAGE ENGAGE ENGAGE ENGAGE ENGAGE ENGAGE WHY STUDY CHEMISTRY? Have you ever wondered why ice melts and water evaporates? Why leaves turn colors and how a battery generates electricity? Why keeping foods cold slows their spoilage and how our bodies use food to maintain life? Chemistry supplies answers to these questions and countless others like them. Chemistry is the study of the properties of materials and the changes they undergo. One of the joys of learning chemistry is seeing how chemical principles operate in all aspects of our lives, from everyday activities like lighting a match to more far-reaching matters like the development of drugs to cure cancer. Indeed, chemistry lies near the heart of man matters of public concern: improvement of health care, conservation of natural resources, and protection of the environment, provision of our everyday needs for food, clothing and shelter. Unfortunately, some chemicals also have the potential of harming our health or the environment. It is in our best interest as educated citizens and consumers to understand the profound effects, both positive and negative, that chemicals have on our lives and to strike an informed balance about their uses. Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  WHAT IS INORGANIC CHEMISTRY? Chemistry covers a wide range of topics that’s why it’s convenient to classify these topics into branches. Inorganic Chemistry is one of them. To understand further about Inorganic Chemistry, it is best to start with its opposite counterpart, the Organic Chemistry. We hear about organic mostly in terms of food, where it means that whatever we’re about to eat was grown without the use of pesticides. But in chemistry, the word organic means you’re dealing with carbon compounds. Carbon is an element you might be familiar with. It’s an element that is present in all forms of life and it is the fourth most abundant element in the universe. Organic Chemistry is basically the study of carbon-hydrogen bonds. Inorganic Chemistry, on the other hand, is the opposite. It is the study of the formation, synthesis and properties of compounds that do not contain carbon-hydrogen bonds. There are around 100 000 known inorganic compounds, while there are around two million organic compounds. Examples of inorganic compounds include: Sodium Chloride NaCl Used as table salt Silicon Dioxide SiO2 Used in computer chips and solar cells Sapphire Al2O3 A well-known gemstone Sulfuric Acid H2SO4 Chemical widely used in the production of fertilizers and some household products Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  EXPLORE EXPLORE EXPLORE EXPLORE EXPLORE EXPLORE WHAT IS MATTER? Chemistry involves studying the properties and behaviour of matter. Matter is the physical material of the universe; it is anything that has mass and occupies space. This module (when printed), your body, the clothes you are wearing, and the air you are breathing are all samples of matter. MATTER MADE OF ATOMS An atom is the smallest unit of matter that retains all of the chemical properties of a particular substance. For example, a gold coin is simply a very large number of gold atoms molded into the shape of a coin, with small amounts of other, contaminating components. Gold atoms cannot be broken down into anything smaller while still retaining the properties of gold. A gold atom gets its properties from the tiny subatomic particles it’s made up of. EXPLAIN EXPLAIN EXPLAIN EXPLAIN EXPLAIN EXPLAIN PART A: STRUCTURE OF AN ATOM An atom consists of two regions. The first is the tiny atomic nucleus, which is in the center of the atom and contains positively charged particles called protons and neutral, uncharged, particles called neutrons. The second, much larger, region of the atom is a “cloud” of electrons, negatively charged particles that orbit around the nucleus. Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  The attraction between the positively charged protons and negatively charged electrons holds the atom together. Most atoms contain all three of these types of subatomic particles—protons, electrons, and neutrons. Hydrogen (H) is an exception because it typically has one proton and one electron, but no neutrons. Atoms can combine to form molecules, O which are held together in specific shapes. H Common example is water. Two hydrogen atoms and one oxygen atom combine to form one molecule of water. H PART B: STATES OF MATTER A sample of matter can be a gas, a liquid or a solid. These three forms of matter are called the states of matter. The states of matter differ in some of their observable properties. A gas (also known as vapour) has no fixed volume or shape; rather, it conforms to the volume and shape of its container. A gas can be compressed to occupy a smaller volume, or it can expand to occupy a larger one. A liquid has a distinct volume independent of its container but has no specific shape. It assumes the shape of the portion of the container it occupies. A solid has both a definite shape and a definite volume; it is rigid. Neither liquids nor solids can be compressed to any appreciable extent. The properties of the states can be understood on the molecular level. In a gas, the molecules are far apart and are moving at high speed, colliding repeatedly with each other and with the walls of the container. In a liquid, the molecules are packed more closely together, but still move rapidly, allowing them to slide over each other; thus, liquids pour easily. In a solid the molecules are held tightly together, usually in definite arrangements, in which the molecules can wiggle only slightly in their otherwise fixed positions. Thus, solids have rigid shapes. Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  EXERCISE NO. 1 To test yourself, answer what is asked. Correct answers are found at the end of this module. Given the state of matter (gas, liquid or solid) for each of the following under ordinary conditions of temperature and pressure: Substance State of Matter Zinc Mercury Ethyl Alcohol Oxygen Sodium Chloride PART C: CLASSIFICATION OF MATTER Most forms of matter that we encounter – for example, the air we breathe (a gas), gasoline for cars (a liquid), and the sidewalk on which we walk (a solid) – are not chemically pure. We can, however, resolve, or separate, these kinds of matter into different pure substances. A pure substance is matter that has a fixed composition and distinct properties. For example, water and ordinary table salt, the primary components of seawater, are pure substances. We can classify substances as ether elements or compounds. Elements are substances that cannot be decomposed into simpler substances. Each element is composed of only one kind of atom. Compounds, in contrast, are composed of two or more elements, and thus contain two or more kinds of atoms. Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  MATTER NO YES IS IT UNIFROM THROUGHOUT? HETEROGENEOU HOMOGENEOUS S MIXTURE MIXTURE NO YES CAN IT BE SEPARATED BY PHYSICAL MEANS? PURE HOMOGENEOUS SUBSTANCE MIXTURE NO CAN IT BE DECOMPOSED YES INTO OTHER SUBSTANCES BY CHEMICAL PROCESSES? ELEMENT COMPOUND Most of the matter we encounter consists of mixtures of different substances. Mixtures are combinations of two or more substances in which each substance retains its own chemical identity and hence its own properties. Whereas pure substances have fixed compositions, the compositions of mixtures can vary. For example, a cup of sweetened coffee can contain either a little sugar or a lot. The substances making up a mixture (such as sugar and water) are called components of the mixture. Some mixtures, such as sand, rocks and wood, do not have the same composition, properties, and appearance throughout the mixture. Such mixtures are heterogeneous. Mixtures that are uniform throughout are homogeneous. Air is a homogeneous mixture of the gaseous substances nitrogen, oxygen and smaller amounts of other substances. The nitrogen in air has all the properties that pure nitrogen does because both the pure substance and the mixture contain the same nitrogen molecules. Salt, sugar and many other substances Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  dissolve in water to form homogeneous mixtures. Homogeneous mixtures are also called solutions. Air is a gaseous solution; gasoline is a liquid solution; brass is a solid solution. EXERCISE NO. 2 Classify each of the following as a pure substance or a mixture; if a mixture, indicate whether it is homogeneous or heterogeneous: (a) concrete; (b) seawater; (c) magnesium; (d) gasoline. PART D: PROPERTIES OF MATTER Every substance has a unique set of properties – characteristics that allow us to recognize it and to distinguish it from other substances. The properties of matter can be grouped into two categories: physical and chemical. We can measure physical properties without changing the identity and composition of the substance. These properties include color, odor, density, meting point, boiling point and hardness. Chemical properties describe the way a substance may change or react to form other substances. For example, a common chemical property is flammability, the ability of a substance to burn in the presence of oxygen. Another example is iron, when it combines with oxygen in the presence of water, forms rust. Properties of matter can also fall into one of these two categories. Some properties – such as melting point and density – do not depend on the amount of the sample being examined. These properties, called intensive properties, are particularly useful in chemistry because many can be used to identify substances. Temperature is another example of intensive property. If the gallon and cup of milk are each at 20oC, when they are combined, the temperature remains at 20oC. Extensive properties of substances depend on the quantity of the sample and include measurements of mass and volume. Extensive properties relate to the amount of substances present. For example, a gallon of milk has a larger mass and volume than a cup of milk. Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  EXERCISE NO. 3 Identify the following properties as either extensive or intensive: Property Category (Extensive or Intensive) Volume Temperature Humidity Heat Boiling Point PART E: PHYSICAL CHANGES AND CHEMICAL CHANGES As with the properties of a substance, the changes that substances undergo can be classified as either physical or chemical. During physical changes a substance changes its physical appearance but not its composition. The evaporation of water is a physical change. When water evaporates, it changes from the liquid state to the gas state, but its composition does not change; it is still water. All changes of state (for example, from liquid to gas or from liquid to solid) are physical changes. In chemical changes (also called chemical reactions), a substance is transformed into a chemically different substance. For example, when hydrogen burns in air, it undergoes a chemical change in which it is converted to water. Chemical changes can be dramatic. The following account describes a young man’s first experiences with chemical reactions. The writer is Ira Remsen, author of popular chemistry text published in 1901. While reading a textbook of chemistry, I came upon the statement “nitric acid acts upon copper”, and I determined to see what this meant. Having located some nitric acid, I had only to learn what the words “act upon” meant. In the interest of knowledge I was even willing to sacrifice one of the few copper cents then in my possession. I put one of them on the table, opened a bottle labelled “nitric acid”, poured some of the liquid on the copper, and prepared to make an observation. But what was this wonderful thing I beheld? The cent was already changed, and it was no small change either. A greenish-blue liquid foamed and fumed over the cent and over the table. The air became colored dark red. How could I stop this? I tried by picking the cent up and throwing it out the window. I learned another fact: nitric acid acts upon fingers. The pain led to another unpremeditated experiment. I draw my fingers across my trousers and discovered nitric acid acts upon trousers. That was the most impressive experiment I have ever performed. I tell of it even now with interest. It was a revelation to me. Plainly the only way to learn about such remarkable kinds of action is to see the results, to experiment, to work in the laboratory. Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  EXERCISE NO. 4 Label each of the following as either a physical process or a chemical process: Process Type of Change Corrosion of aluminium metal Melting of ice Pulverizing an aspirin Digesting a candy bar Explosion of nitroglycerin ELABORATE ELABORATE ELABORATE ELABORATE Formative Assessment (Graded Assignment): 1. Classify each of the following as a pure substance, a heterogeneous mixture or a heterogeneous mixture: a) air; b) tomato juice; c) iodine crystals; d) a glass of milk; e) concrete; and f) a 1 peso coin. 2. Determine whether the following occurrences are due to physical changes or chemical changes: a) a burning match stick; b) a piece of metal getting warmer; c)Water condensing on the sides of a cold glass of water; and d) Soot(carbon) deposited on the exhaust of a car. 3. Identify whether the following properties are intensive or extensive in nature: a)Solubility; b) Weight; c) Flash point; and d) Density. EVALUATE EVALUATE EVALUATE EVALUATE You have reviewed some important concepts of matter and acquired additional and new knowledge on some important advancement. You should be able to apply these concepts. Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.  References: Brown, Le May & Bursten. (1997). Chemistry, The Central Science, 7th Ed. USA: Prentice Hall International. ANSWERS TO EXERCISES: EXERCISE NO. 1: 1. solid 2. liquid 3. liquid 4. gas 5. solid EXERCISE NO. 2: 1. Mixture – Heterogeneous 2. Mixture – Homogeneous 3. Pure Substance 4. Mixture – Homogeneous EXERCISE NO.3: 1. Extensive property 2. Intensive property 3. Intensive property 4. Extensive property 5. Intensive property EXERCISE NO.4: 1. Chemical change 2. Physical change 3. Physical change 4. Chemical change 5. Chemical change Property of and for the exclusive use of SLU. Reproduction, storing in a retrieval system, distributing, uploading or posting online, or transmitting in any form or by any means, electronic, mechanical, photocopying, recording, or otherwise of any part of this document. without the prior written permission of SLU, is strictly prohibited.