PCI-01.pdf

1 MATTER The Study of Chemistry the branch of chemistry that focuses on the study of compounds that do not contain carbon- hydrogen bonds. explores the properties, behavior, and reactions of a vast array of substances, including: Metals: Iron, copper, gold, etc. Minerals: Quar...

1 MATTER The Study of Chemistry the branch of chemistry that focuses on the study of compounds that do not contain carbon- hydrogen bonds. explores the properties, behavior, and reactions of a vast array of substances, including: Metals: Iron, copper, gold, etc. Minerals: Quartz, calcite, feldspar, etc. Salts: Sodium chloride (table salt), potassium nitrate, etc. Gases: Oxygen, nitrogen, carbon dioxide, etc. Study of matter “Physical Science”, “Central Science”, :ABC of Pharmacy Practice” Key Areas of Inorganic Chemistry Synthesis: Creating new inorganic compounds with desired properties. Structure: Determining the arrangement of atoms in inorganic molecules. Reactivity: Understanding how inorganic compounds interact with other substances. Properties: Studying the physical and chemical characteristics of inorganic compounds. APPLICATIONS OF Inorganic Chemistry Materials science: Developing new materials for electronics, construction, and energy storage. Catalysis Creating catalysts for industrial processes and environmental cleanup. Medicine: Developing inorganic compounds for drug delivery and medical imaging. Agriculture: Producing fertilizers and pesticides. Environmental science: Studying the chemistry of pollutants and developing remediation strategies. MATTER Anything that ocupies space and has mass Made up of “small indivisible particles” called ATOMS UNIT OF MEASUREMENT MASS Refers to the amount of matter present in an object. Intrinsic to the object, doesn't change with location. WEIGHT A measure of the force exerted on an object due to gravity. Depends on both mass and gravitational acceleration. Equal to Mass X Gravitational Pull 2 types of measurement Fundamental (base) units These are the basic units of measurement that cannot be expressed in terms of other units. They are independent and form the foundation for other units. SI base units name of unit symbol LENGTH meter MASS kilogram TIME seconds TEMPERATURE Kelvin AMOUNT OF SUBSTANCE moles 2 types of measurement DERIVED UNITS These units are obtained by combining one or more fundamental units They depend on the fundamental units for their definition. DERIVED units name of unit symbol AREA meter^2 VOLUME meter^3 VELOCITY meter/seconds ACCELERATION meter/seconds^2 FORCE kilogram-meter/sec^2 PRESSURE kilogram/meter-sec^2 WORK (ENERGY) kilogram-meter^2/sec^2 temperature CELCIUS kelvin Commonly used in most of the world. SI unit for temperature and is used in It is based on that water freezes at 0deg.C. scientific calculations and and boils at 100deg.C measurements. C to K = C = (F-32) x 5/9 Absolute Zero: C = (F - 32) * 5/9 This is the lowest possible temperature, defined as 0 Kelvin. 0 Kelvin = -273.15 deg.C Fahrenheit Commonly used in the United States. It is based on that water freezes at 32F and k = C + 273.15 boils at 212F F = (c x 9/5) + 32 general formula 160 + 9 (C) = 5 (F) fundamental states of matter solid According to form: Amorphous: non perfect order/shape Crystalline: perfect order/shape Eg. Crystalline Insulin According to ability to absorb water: hygroscopic absorb water but does not liquify Eg. cellulose sugar Deliquescent liquify upon absorption of water Eg. All chlorides EFFLORESCENT releases water of crystallization Eg. sulfates, sodium carbonate fundamental states of matter LIQUID has a definite volume but no definite shape The amount of liquid remains constant regardless of its container. GAS state of matter that has neither a definite shape nor a definite volume. This means it will expand to fill the container it is in. fundamental states of matter PLASMA 4th State of Matter aka supercritical fluid, liquid crystal a highly energized state where matter is ionized, meaning it has lost or gained electrons. bose einstein condensate 5th state of matter matter that exist at absolute zero temperature Absolute Zero = -273.15 C  solid liquid gas shape volume compression very slight slight high ifa strength molecular motion vibrate glide/flow random constant motion  liquid solid gas plasma  matter mixture pure substance homogenous heterogenous elements compounds Eg. solution colloid atom molecule suspension element Simplest form of matter Contains 1 type of material Pure chemical substances Currently, there are 118 elements Examples: oxygen (O), hydrogen (H), gold (Au), carbon (C). COMPOUND formed by the chemical combination of two or more different elements in fixed proportions. Can be broken down into simpler substances through chemical means. Examples: water (H₂O), salt (NaCl), carbon dioxide (CO₂). MIXTURE A combination of two or more substances that are not chemically combined. retain their own properties and can be separated using physical methods. homogenous mixture HETEROGENOUS mixture These have a uniform composition These have a non-uniform composition throughout with visible different parts Example: Examples: Salt water Oil and water Sugar dissolved in water Sand and water Air Pizza Alloys (like brass or bronze) Trail mix FUNDAMENTAL LAWS OF MATTER LAW OF DEFINITE PROPORTION Aka Proust’s Law, Law of Constant Composition A given compound always contains exactly the same proportion of elements by mass. FUNDAMENTAL LAWS OF MATTER LAW OF MULTIPLE PROPORTION When two elements form a series of compounds, the ratios of the masses of the second element that combine with a fixed mass of the first element are simple whole numbers. law of definite proportions same ratio elements same compound law of multiple proportions different elements different compound ratio FUNDAMENTAL LAWS OF MATTER LAW OF conservation of energy The law of conservation of energy states that energy cannot be created or destroyed; it can only change form. FUNDAMENTAL LAWS OF MATTER LAW OF conservation of mass and energy The law of conservation of mass and energy states that the total amount of mass and energy in a closed system remains constant over time. Mass can be converted into energy, and energy can be converted into mass. The relationship between mass and energy is described by Einstein's famous equation: classification of mixture Based on NATURE of particles Based on SIZE of particles classification of mixture Based on nature of particles heterogenous HOMOGENOUS Multiple Phases Single Phase Physically distinct; multiple phases Consistent or uniform parts throughout Eg. sand and water mixture Eg. NaCl dissolved in water, syrup, alloys Based on size of particles solution uniform mixture composed of solute and solvent suspension aka coarse mixture finely divided solid materials distributed in a liquid colloid particles of solute are not broken down to the size of the molecules but are small enough to remain suspended and evenly dispersed throughout the medium Tyndall effect the scattering of light by particles in a colloid When a beam of light passes through a colloid, the particles in the colloid scatter the light in all directions. colloids Dividing line between solution and hemogenous mixture The particles in a colloid are larger than those in a solution but smaller than those in a suspension. properties of colloids: Tyndall effect Light scattering BROWNIAN MOVEMENT continuous, random, zigzag motion of colloidal particles. ADSORPTION adhesion of atoms, ions, or molecules from a gas, liquid, or dissolved solid to a surface. CHARGED ELECTRICALLY helps to stabilize the colloid by preventing the particles from coming together and coagulating. separation of mixtures decantation Difference in specific gravity or density distillation EVAPORATION process by which a liquid changes into a gas or vapor. CONDENSATION process by which a gas or vapor changes into a liquid separation of mixtures EVAPORATION Escape of molecules from liquid to gaseous or vapor state magnetic separation Ferromagnetism to separate magnetic materials from the non-magnetic components separation of mixtures filtration used to separate solid particles from a liquid or gas by passing the mixture through a porous material called a filter. COMPONENTS: Filtrate: The liquid or gas that passes through the filter. Residue: The solid particles retained by the filter. separation of mixtures filtration used to separate solid particles from a liquid or gas by passing the mixture through a porous material called a filter. COMPONENTS: Filtrate: The liquid or gas that passes through the filter. Residue: The solid particles retained by the filter. separation of mixtures SORTING Mechanical separation classifying components based on their physical properties. centrifugation Employ centrifugal force to increase or speed up the settling of a precipitate separation of mixtures fractional crystallization Chromatography lowering the temperature so that the more Difference in solvent afiinity insoluble component crystallizes first Science of separation Based on difference in solubilities properties of matter Extrinsic Intrinsic aka Extensive properties aka Intensive properties Properties dependent on the amount of Properties independent on the amount of substance present. substance present; constant Eg Eg. Weight Density, Specific gravity Volume Melting point, Boiling point Pressure Organoleptic properties Heat content Colligative Properties: Vapor pressure lowering Boiling point elevation Freezing point depression Osmotic pressure changes in matter physical change Change in phase; no new substance is formed CHEMICAL CHANGE Change in both extrinsic and intrinsic properties; new substance is formed Change in structure, properties, composition of the nucleus of an atom nuclear change resulting in the transformation of the element into another element Eg. Nuclear Fission & Nuclear Fusion nuclear change nuclear fission Splitting of a heavy atom nuclear fusion Union of 2 light atoms to form a bigger molecule chemical reactions direct union aka Synthesis, Combination Simple substance --> Complex substance a + B = Ab DECOMPOSITION aka Analysis, Combustion Reaction Complex substance --> Simple substance Ex: Combustion Reaction ab = A + B chemical reactions single replacement reaction Depends on the Activity Series A + BC --> b + ac Double replacement aka Metathesis Eg. Neutralization Reaction AB + cd --> AD + BC activity series aka Electromotive Series Useful for predicting Displacement Reaction For metals Metals located above hydrogen can displace hydrogen gas from acids Metals located above the series are more active and can displace salts of metals from solution Metals located below the series are easily reduced into their metallic states For non-metals F2 > Cl 2 > Br2 > I2 evidences of chemical change Evolution of gas Formation of a precipitate Emission of light Generation of electrochemistry Production of mechanical energy Absorption or Liberation of heat processes involved in chemical change OXIDATION VI-LEORA OXIDATION = (+) OXYGEN DEHYDROGENATION = (-) HYDROGEN REDUCTION VD-GEROA HYDROGENATION = (+) HYDROGEN REDUCTION = (-) OXYGEN processes involved in chemical change NEUTRALIZATION chemical reaction that occurs when an acid and a base react with each other to form water and a salt. hydrolysis chemical reaction where water is used to break down a compound. processes involved in chemical change saponification chemical process that involves the conversion of fats or oils into soap and glycerol through reaction with an alkali fermentation metabolic process that converts carbohydrates, such as sugar, starch, or cellulose, into alcohol or organic acids, using microorganisms (yeasts or bacteria) under anaerobic conditions. finding out oxidation numbers oxidation number Charge on an atom in a compound Rule: Assign a number (charge) to every atom Oxidation state rules: Pure elements are all zero F is -1 Metals: 1a are +1. 2a are +2, al is +3 h is usually +1 (can be -1 with a metal o is usually -2 (except for peroxides (-1) halogens are usually -1  try this out S8 H2O H2O2 LiH AlH3 LiAlH4 NaH2PO4  ACTIVITY Manganese MnO4 - Chromium Cr2O7 2- Chlorine HClO3 3- Arsenic AsO4 Chromium CrO4 2-