Properties of Matter-WEEK1.pptx.pdf

Introduction to Inorganic Chemistry Objectives: ▪Define and Differentiate Inorganic chemistry from other chemistry subjects ▪Recall basic concepts of chemistry ▪Discuss importance of Inorganic chemistry in Pharmaceutical industry Chemistry Definition ‘is the field of study concerned with the...

Introduction to Inorganic Chemistry Objectives: ▪Define and Differentiate Inorganic chemistry from other chemistry subjects ▪Recall basic concepts of chemistry ▪Discuss importance of Inorganic chemistry in Pharmaceutical industry Chemistry Definition ‘is the field of study concerned with the characteristics, composition and transformations of matter’ Inorganic Chemistry Definition UNIT I: REVIEW OF THE BASIC CONCEPTS OF INORGANIC CHEMISTRY Basic concepts of Matter Properties of Matter Matter: Anything that has mass and takes up space Mass: the amount of matter in an object measured with a balance Volume: the amount of space an object takes up measured with a ruler or graduated cylinder Physical Properties ▪Are characteristics or features that describe matter ▪Are true only for a certain amount of matter Examples include: ▪color ▪smell ▪size ▪temperature ▪shape ▪state ▪texture Chemical Properties ◦is a characteristic of a substance that describes the way the substance undergoes or resists change to form a new substance. ◦For example, copper objects turn green when exposed to moist air for long periods of time Characteristic Properties ▪properties that do not change with changes in mass or volume ▪are properties of a substance, not a specific object Ex. sugar – phys. prop- white - char. Prop – solubility, melting pt, sweet Examples include: ▪boiling point ▪hardness ▪melting point ▪pH ▪solubility ▪flammability ▪conductivity ▪density Properties of Matter include: ▪ How it looks (shiny, dull, colored) ▪ How it feels (hard, soft, rough, smooth) ▪ How it smells (sweet, salty, flowery) ▪ How it sounds (loud, soft, hollow) ▪ How it tastes (sweet salty, bitter, sour) ▪ What it does (bounce, bubble, tear) Physical or Chemical Property? ▪Iron metal rusts in an atmosphere of moist air. ▪Mercury metal is a liquid at room temp. ▪Nickel metal dissolves in acid to produce a light green sol. ▪Potassium metal has a melting point f 63 degrees Celsius. States of Matter ▪Solid ▪Liquid ▪Gas ▪Plasma States of Matter ▪Based upon particle arrangement ▪Based upon energy of particles ▪Based upon distance between particles Solids ▪ Have definite shape and definite volume ▪ Particles are tightly packed, vibrating about a fixed position Liquids ▪ Do not have definite shape but do have definite volume ▪ Particles are loosely packed Gases ▪ Do not have definite shape or definite volume ▪ Particles are very far apart and move freely  Plasma ▪ an ionized gas. ▪ a very good conductor of electricity and is affected by magnetic fields. ▪ Plasmas, like gases have an indefinite shape and an indefinite volume. 3. Aurora (Northern Lights) Changes in Matter  What are physical changes of matter? Change of Appearance ▪ It is a change that affects one or more physical properties of a substance. ▪ The appearance, shape, or size of a substance may be altered during a physical change. ▪ Physical changes, such as changes in state(boiling water), dissolving sugar in water, cutting paper, crushing an aluminum can, do not change the chemical identity of a substance.  What are chemical changes of matter? Change from the Inside ▪ A chemical change is the process by which one or more substances change into entirely new substances. ▪ Chemical changes are not the same as chemical properties. ▪ Burning is a chemical change; flammability is a chemical property. How can you tell a chemical change has happened? ▪ Odors can be produced during a chemical change. ▪ Fizzing and foaming may mean gases are being produced. ▪ The production of gas is often evidence of a chemical change. ▪ Boiling also can produce gas bubbles, but boiling is a physical change. ▪ A precipitate is a solid that falls out of solution. ▪ The formation of a precipitate can indicate a chemical change. ▪ Energy changes from one form to another can be evidence of a chemical change. ▪ Changes in temperature and color can be signs of a chemical change. Will heating the water in this beaker cause a physical or chemical change?  Physical and Chemical Changes Physical Changes in Matter Chemical Changes in ▪Volume Matter ▪Mixture ✔New Matter is found ▪ Burning ▪Solution ▪ Rusting ▪Solid ▪ Cooking ▪ Film processing ▪Liquid ▪Mass ▪Shape ▪Texture Conservation is the Law What is the law of conservation of mass? French chemist Antoine Lavoisier studied chemical changes in which substances appeared to gain or lose mass.. The law of conservation of mass states that in ordinary chemical and physical changes, mass is not created or destroyed. It is only transformed into different substances. Physical or Chemical Change? ▪ The fashioning of a piece of wood into a round table leg ▪ The vigorous reaction of potassium metal w/ water to produce hydrogen gas ▪ Straightening a bent piece of iron w/ a hammer ▪ The ignition and burning of a match Classifying Matter by Composition composition includes: ✔ types of particles ✔ arrangement of the particles ✔ attractions and attachments between the particles Classification of Matter by Composition ▪ Matter whose composition does not change from one sample to another is called a pure substance. ▪ made of a single type of atom or molecule ▪ Because the composition of a pure substance is always the same, all samples have the same characteristics.  Matter whose composition may vary from one sample to another is called a mixture. two or more types of atoms or molecules combined in variable proportions Because composition varies, different samples have different characteristics.  Classification of Matter by Composition 1) made of one type of 1) made of multiple types of particle particles 2) All samples show the 2) Samples may show same intensive different intensive properties. properties. Classification of Pure Substances⎯Elements ▪ Pure substances that cannot be decomposed into simpler substances by chemical reactions are called elements. – decomposed = broken down – basic building blocks of matter – composed of single type of atom though those atoms may or may not be combined into molecules  Classification of Pure Substances⎯Compounds ▪ Substances that can be decomposed are called compounds. – chemical combinations of elements – composed of molecules that contain two or more different kinds of atoms – All molecules of a compound are identical, so all samples of a compound behave the same way  Classification of Pure Substances 1) made of one 1) made of one type of atom type of (some elements molecule, or found as array of ions multi-atom 2) units contain molecules in two or more nature) different kinds 2) combine of atoms together to make compounds  Classification of Mixtures ▪ homogeneous = mixture that has uniform composition throughout – Every piece of a sample has identical characteristics, though another sample with the same components may have different characteristics. – atoms or molecules mixed uniformly ▪ heterogeneous = mixture that does not have uniform composition throughout – contains regions within the sample with different characteristics – atoms or molecules not mixed uniformly  Classification of Mixtures 1) made of 1) made of multiple multiple substances, substances, whose but appears to presence can be one be seen substance 2) Portions of a 2) All portions of sample have an individual different sample have composition the same and properties. composition and properties. Importance in pharmacy and pharmaceutical industry ▪ Identify the characteristics of products ▪ Formulation considerations ▪ Drug design strategies ▪ Pharmacokinetics studies