Matter and Its Properties PDF

MATTER & ITS PROPERTIES GENERAL CHEMISTRY 1 OBJECTIVE/S: At the end of the lesson, you should be able to: 1.Distinguish between the physical and chemical properties of matter. 2.Use properties of matter to identify substances and to separate them. 3.Describe various simple separat...

MATTER & ITS PROPERTIES GENERAL CHEMISTRY 1 OBJECTIVE/S: At the end of the lesson, you should be able to: 1.Distinguish between the physical and chemical properties of matter. 2.Use properties of matter to identify substances and to separate them. 3.Describe various simple separation techniques such as distillation, chromatography, etc.  Outline States of Properties of Classification of Matter Matter Matter Solid Physical Pure Liquid properties Substance Chemical Mixture Gas properties Matter  anything that occupies space and has mass  Is composed of tiny particles called atoms.  Matter can be classified into three (3) states: 1. Solid 2. Liquid 3. Gas States of matter  Molecular Behavior Properties of Gas Liquid Solid Matter Volume/Shape not definite definite volume definite volume volume and but indefinite and definite shape shape of container shape Density low high high Compressibilty easy to compress cannot be Cannot be appreciably appreciably compressed compressed Motion and Random, fast, Random, medium Vibration in place; arrangement of cover large speed, limited ordered Molecules distances; distances;Disorder arrangement total disorder Properties of Matter  Properties are characteristics of substance which enable us to identify the substance and differentiate it from other substances. All matter can be described either physical or chemical properties. Physical Properties The physical properties of matter are perceived by the senses. It can be observed, measured, and tested without changing the composition of matter. Examples:Color, odor, taste, hardness, boiling point. Physical properties can either be intensive and extensive properties.  Physical Properties Intensive are propertiesProperties that do not  Extensive Properties are properties that depend depend on the amount of on the amount of matter matter present or being present or being tested. measured. Example: mass, length, and Example: Color, hardness, shape boiling point  Some physical properties of matter Hardness - refers to ability of a material to resist scrathching. Melting point - is the temperature where solid changes to liquid. Boiling point - is the temperature where liquid changes to gas. Luster - is a property of a material that pertains to the interaction of light on the surface of metal. Malleability - is the ability of a metal to be hammered or shaped into thin sheets without breaking or cracking. Density - is defined as the mass of an object per unit volume.  Chemical properties The chemical properties are properties involved change in the substance’s composition during chemical reaction. Example: Flammability, reactivity, toxicity, oxidation Changes in Matter The changes that matter undergoes may be Physical or Chemical. Physical Change - do not alter the identity of a substance. Example: Evaporation, Solidification Chemical Change - produce new compounds with a different chemical composition and a different set of properties. Example: Photosynthesis Chemical change Example: Photosynthesis - is the process through which plants transform solar energy to chemical energy 6CO2 + 6H2O --------> C6H12O6 + 6O2 Classification of Matter Matter can be classified into two (2) composition: (1) pure substance (2) mixture 1. Pure Substance Contains only one type of particle and has a uniform composition. it cannot be separated by physical means Pure substances can be classified into (a) elements and (b) compounds 1.1 Elements are substances composed of only one kind of atom. Elements can be classified into three (3): (a) metal (b) non metal (c)metalloids  1.1.1 Metals Metals constitiute the greatest number of elements in the periodic table. Example of metals: Gold (Au), Silver (Ag), Iron (Fe) Properties of Metals Metals are lustrous in nature Metals are malleable Metals are ductile Metals are good conductor Metals are solid in room temperature except Mercury Most metals arerd and have high densities 1.1.2 Nonmetals Nonmetals are elements that lack or do not have the characteristics of metals. example of nonmetals: Oxygen (O), Iodine (I), Chlorine (Cl) Properties of Nonmetal have a dull appearance brittle poor conductors of heat and electricity good insulators have low densities 1.1.3 Metalloids Metalloids are elements which have the properties of both metals and nonmetals. Examples of metalloids: Boron (B), Arsenic (As) 1.2 Compounds  substances composed of two or more kinds of atoms that are chemically bonded together in fixed proportions. Example: H2O (water), NaCl (Sodium chloride) Compounds can be classified into three (3): (a) acids (b) bases (c) salts  1.2.1 Acids An acid is compound that donates H+ ions in an aqueous solution. It tastes sour and turns blue litmus paper to red. Example: Acetic Acid (Vinegar) Hydrochloric Acid (HCl) Soft drinks  1.2.2 Base A base is a compound that accepts H+ ions in an aqueous solution. It taste bitter and turns red litmus paper to blue. Example: Sodium Hydroxide (NaOH) Ammonia (NH3) Detergent powder 1.2.3 Salt Salt is a compound that is formed when an acid and a base react. This reaction, which forms salt and water,is called neutralization. HCl + NaOH ------> H2O + NaCl Example of salt: table salt (NaCl) calcium carbonate 2.Mixtures Mixtures are made up of two or more substances which are mixed together but are not chemically combined. Mixture can be classified as (a) Homogeneous mixture (b) Heterogeneous mixture 2.1 Homogeneous Mixture has only one phase and a uniform composition all throughout. A solution is a homogeneous mixture. example: sugar and water solution 2.2 Heterogeneous Mixture has two or more phases. example: halo-halo A heterogeneous mixture can be; (a) Colloids (b) Suspension  2.2.1 Colloids Colloids, which are also called colloidal dispersions, are heterogeneous mixtures that have particles bigger than those of a solution but smaller than those of a solution. example: Aerosols - gas as the dispersed medium, and th dispersed phase is either solid or liquid. 2.2.2 Suspension are heterogeneous mixtures that have particles bigger than those of colloids. Example: sand and water mixture A major difference between colloid and a suspension it its particle size.  Reference/s: General Chemistry 1 for Senior High School. C&E Publishing, Inc., 2017