GENERAL CHEMISTRY Chapter 1: Matter & Its Properties 1.1 Particular Nature of Matter MATTER - Anything that has mass & occupies space (has volume) Anything that takes up space and can be weighed Often taken to mean anything that is composed of atoms and molecules IDENTIFICATION OF MATTER AS PER CHEMISTS Physical characteristics - Color -Size -Mass -Shape Chemical Characteristics -Interacts with another types of matter Ex.Corrosion: Rust in Science/Chemistry Matter is anything that is made of protons, neutron, & electron Subatomic particles is the basic foundation of atoms. Subatomic Particles -Basic foundation of atoms PROTON (+) NEUTRON ( ) ELECTRON (-) STRUCTURE OF MATTER ATOM - Building blocks of matter In constant motion Composed of PROTON, NEUTRON, ELECTRONS NUCLEUS: Center of Atom PROTONS AND NEUTRONS are always inside the nucleus. ELECTRONS of an atom are found orbiting the nucleus of the atom. (-) (+) () All substances are composed of invisible particles called ATOM. Combination of atoms leads to millions of materials with different properties. Atoms are made up of a positively recharged center, nucleus (+) ELEMENTARY PARTICLES (Quarks): smaller than subatomic particles. WHICH IS NOT A MATTER -Time -Radiation -Rainbow -Energy -Thoughts -Gravity -Sound -Sunlight -Microwave -Heat -Magnetism 1.2 States of Matter LOW TEMP – HIGH TEMP (Phases of Matter) Fermionic Condensate (Coldest) Boss-Einstein Condensate Solid Liquid Gas Plasma Quark-Gluon Plasma (Hottest) 1.FERMIONIC CONDENSATE -a superfluid phase formed by fermionic particles at very low temperature, formed by FERMIONS. FERMIONS -Zero Energy -Anti-Social Elementary Particle -Coldest -Can be seen in laboratories 2.BOSE-EINSTEIN CONDENSATE (BEC) -A state of matter created when particles called BOSONS, are cooled to near absolute zero (-273 centigrade or -460 Farenheit) BOSONS -Social Elementary Particle -Elementary Particle opposite to fermion 3.SOLID -A state of matter where there is a definite MASS, VOLUME, & SHAPE. 4.LIQUID -A nearly incompressible fluid that conforms to the shape of its container but retains a nearly constant volume independent of pressure. Liquids has definite MASS and VOLUME but no definite shape. 5.GAS -A substance that is gaseous, or vaporous state of matter. This state of matter has NO definite mass, volume, and shape. 6.PLASMA -Appears when the atoms are in excited state -In heat or extreme temperature (ex.sun,fire,star) 7.QUARK-GLUON PLASMA -A new state of nuclear existing at extremebly high temperatures and densities when composite states called HADRON (proton.neutron,electron) lose their identity & dissolve into a soup of their constituent-quarks & gluons. -Quite connected to bigbang theory. PROCESS INVOLVED IN CHANGING PHASES OF MATTER Through our naked eye, we can only observe solid, liquid ang gas. Water exists in three stages: Water : liquid ice : solid water vapor: gas Need ENERGY to change the phases of matter. The relationship between temperature spaces between the molecules are directly proportional; the farther the spaces the hotter the temperature and vice versa. ENERGY: when energy is added to a substance that energy causes the particles in the substance to move faster. PHASE CHANGE -Energy content is responsible for the different phases of matter. -The higher the energy content the faster the phase change - (DIRECTLY PROPORTIONAL) 2 TYPES OF PHASE CHANGE 1. Endothermic change (Adding Energy) 2. Exothermic change (Removing Energy) ENDOTHERMIC CHANGE (Adding Energy) -Phase change that requires the addition of energy. (endo: inside , therm: heat) Phase change that are endothermic: 1. Melting (solid – liquid) 2. Sublimation (Solid – gas) 3. Boiling (liquid – gas) 4. Vaporization (liquid – gas) 5. Evaporization (liquid to gas) 1. MELTING (Solid to Liquid) - Melting is the changing of liquid to solid when the substance absorbs energy. MELTING POINTS TABLE SALT: 801 C DIAMOND: 3700 C WATER: 0 C / 32 F MP = FP 2. SUBLIMATION (Solid to Gas) -Solid to gas phase change occurs -Ex. Dry ice goes directly from solid carbon dioxide to gas. -Opposite of sublimation if deposition (gas to solid) 3. BOILING (Liquid to Gas) -If enough heat energy is applied to a substance particles inside the liquid can change to gas. These particles travel to the surface of the liquid. BOILING POINT WATER: 100 C TABLE SALT: 1413 C DIAMOND: 4300 C 4. VAPORIZATION (Liquid to Gas) -Vaporization is the changing of a liquid to a gas when the substance absorbs heat energy. -It occurs in the surface Vaporization VS. Boiling (Difference) Vaporization – on the surface Boiling – Transfers the temperature from the bottom to the surface. 5. EVAPORIZATION (Liquid to Gas) -It is the cooling process -As water in the perpiration evaporates from your skin it absorbs and carries away heat energy from your body. Perspiration: Helpful thing to maintain your homeostasis Homeostasis: Yourself – surroundings EXOTHERMIC CHANGE (Removing Energy) -Phase change that requires the removal of energy. (exo: outside , therm: heat) Phase change that are exothermic: 1. Freezing ( liquid - solid ) 2.Condensation ( gas – liquid ) 3.Deposition (gas –solid) 1. FREEZING (Liquid to Solid) - Opposite of melting; liquid changing to solid is freezing. -Freezing occurs when a substance loses heat energy -The freezing point of a substance is equal to the melting point. 2. CONDENSATION (Gas to liquid) -Gases can change phase also in a gas to liquid phase change -A substance in the gas phase that loses heat will change into liquid. This is called CONDENSATION. -“They tend to equalize their temperature with the surrounding” -Water vapor in surrounding air loses heat energy when it comes in contact with the cold gas; water vapor condenses. 3. DEPOSITION (Gas to solid) 1.3 Physical and Chemical Properties of Matter COMPOSITION -the components of a sample of matter -their relative proportion Ex. Co2 - C + 2O = Co2 H2O - 2H + O = H2o PROPERTIES -Qualities or attributes that we can use to distinguish one sample of matter from others. 2 CATEGORIES 1. PHYSICAL PROPERTIES 2. CHEMICAL PROPERTIES 1.Physical Properties -A trait of matter than can be observed or measured without changing the chemical composition of the matter. Physical Change – No chemical reaction allowed. - Retain its identity 1. Color: - How the object absorbs & reflects light. 2. Texture: - How the substance looks & feels. 3. Temperature: - A measure of the average kinetic energy (energy of motion) of particles in a substance. 4. Mass: - Amount of matter in an object (in g or kg) DIFFERENCE OF MASS & WEIGHT MASS WEIGHT Not affected by gravity Affected by gravity 5. Volume: - The amount of space an object occupies. (in ml, L, cm, m, etc.) 6. Density: - Ration of mass to volume; reflects the degree of packing of particles in matter. DENSITY OF MATTER Highest Density Lowest Density Hydrogen Osmium (23 g/cm^2) 7. Luster: - the wat that a substance reflects light (metallic, non-metallic, glassy, pearly, dull) 8. Ductility: - Ability of a substance to be stretched into a wire (wire-like). 9. Malleability: - Ability of a substance to be hammered flat and to retain the old shape. 10. State (Phase) of matter (S,L,G…) - Solid, Liquid, Gas 11. Melting point/Freezing point: - The exact temperature at which solid becomes a liquid or a liquid becomes solid. INTENSIVE VS. EXTENSIVE PROPERTIES OF MATTER INTENSIVE PROPERTY: - Does not depend on amount of substance present. - Ex. 1kg nail: nail 2kg nail: is still a nail - Are determined by the chemical composition of the particles and their structure (arrangement) EXTENSIVE PROPERTY: - One that does depend on the amount of substance present. - Depend only on the numbers of particles not on their composition or internal arrangement. 2. CHEMICAL PROPERTIES (Attributes) -A trait of matter that can only be observed if a substance has the property. In the process of testing the chemical property. Chemical Change -Chemical Reaction -Identity Changes 1. Reactivity with Oxygen - Rusting - Tarnishing 2. Reactivity with water - Reactivity with water means how easily and quickly an element or a compound reacts with water - Some substances are water-reactive, meaning they spontaneously undergo a chemical reaction with water, as they are highly reducing in nature - Examples of water-reactive substances are alkali metals and alkaline earth materials. 3. Reacting with acids & Basics 4. Combustibility / Flammability - Combustibility is the ability of solid to be fired. - Flammability: a liquid that is put to fire. 5. Chemical Formula (Chemical Composition) - What something is made of is always… “All chemical properties are intensive. None are extensive” -Because chemical properties never depend on how much/ the amount. -Intensive properties make the best characteristic properties because intensive properties are determined by the composition & structure. 1.4 Classification of Matter -Mixture -Pure Substance = PURE SUBSTANCE = -SOMETHING THAT CAN NOT BE BROKEN DOWN INTO SIMPLER MATTERS USING PHYSICAL METHODS. 2 TYPES OF PURE SUBSTANCE 1. ELEMENTS – Simplest kind of pure substance. 2. COMPOUNDS - A compound is a substance made up of two or more different chemical elements combined in a fixed ratio. “NOT ALL ELEMENTS ARE EQUALLY COMMON” MOST ELEMENTS CAN EXIST AS A SINGLE ATOM DIATOMIC GASES HYDROGEN H2 NITROGEN N2 OXYGEN O2 FLOURINE F2 CHLORINE Cl2 BROMINE Br2 IODINE L2 ALLOTROPES -different structural forms of the same element. e x a m p l e: OXYGEN HAS 3 ALLOTROPES O2: O3: O4: Monotomic Oxygen Diatomic Oxygen Molecule Ozone Molecule Allotropes of Carbon Diamond Fullereness Graphite Carbon Nanotubes All are pure substance. Each has different structure. = COMPOUNDS = » » » » » » 2 OR MORE ELEMENTS BOUNDED TOGETHER COMPOSED OF MULTIPLE ELEMENTS CANNOT BE BROKEN DOWN BY PHYSICAL METHODS CAN BE BROKEN DOWN BY CHEMICAL REACTIONS COMPOUNDS CAN DECOMPOSE HAVE DEFINITE COMPOSITION The properties of compounds are very different from the properties of elements that make them up. ex. Na + Cl = NaCl (Sodium Chloride) Na (Sodium) : explosive Cl (Chlorine) : poisonous NaCl: No longer poisonous or explosive = MIXTURE = -SOMETHING THAT CAN BE BROKEN DOWN INTO SIMPLER MATERIALS USING PHYSICAL METHODS. 3 POSSIBLE TYPES OF MIXTURE 1. Element + Another element 2. Compound + Another compound 3. Element + Compound MAIN (2) TYPES OF MIXTURE: 1. HOMOGENOUS MIXTURE 2. HETEROGENOUS MIXTURE MAIN TYPES OF MIXTURE HOMOGENOUS MIXTURE -parts are distributed evenly. (uniform) HETEROGENOUS MIXTURE -parts are distributed unevenly. Ex. Salt water Ex.Spaghetti, Meatballs, water + oil mixture Solutions – homogenous liquid mixture Alloys – homogenous metallic mixture -.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-.-. COMPOUND VS. MIXTURE COMPOUND MIXTURE -Properties of compound are -The properties of mixture are totally different from the realted. properties of elements that make them up. MATTER FLOWCHART METHODS OF SEPARATING MIXTURES INTO THEIR OWN COMPOUND 1. Mechanical Separation (Often done by hand) -Takes advantage of physical properties such as colors & shapes. -In other words arranging Ex. Recycling plastic, paper, metal 2. Magnetic Separation -Takes advantage of the physical property of magnetism. 3. Filtration (Uses filtering material) -Takes advantage of the physical property of the state of matter. 2 TYPES OF FILTERING 1. Solid – Liquid : coffee maker 2. Solid – Solid : Sand sieve 4. Decanting -Solid/Liquid on product -To pour off a liquid, leaving another solid or liquid behind -Decantation is a process for the separation of mixtures of immiscible liquids or of a liquid and a solid mixture such as a suspension -Does not use filtering material 5. Distillation -The separation of a mixture of liquid -Distillation, the process involving the conversion of a liquid into vapor that is subsequently condensed back to liquid form. -A simple distillation definition or distillation meaning is a process of purifying a liquid compound by heating it into a vapor that is then condensed back into a liquid. By heating a liquid to the temperature at which it turns into a vapor, it is separated from any possible impurities that are dissolved within it. 6. Evaporation -vaporizing a liquid -liquid to gas 7. Density separation -Always liquid product -This process step is meant to separate materials based on their weight to process them further in different lines. Smart and compact solutions based on density principles allow separation of materials with specific gravity characteristics. 8. Centrifuge -Circular motion helps denses components sink to the bottom faster. -Centrifugation is a technique used for the separation of particles from a solution according to their size, shape, density, viscosity of the medium and rotor speed. The particles are suspended in a liquid medium and placed in a centrifuge tube. The tube is then placed in a rotor and spun at a define speed. 9. Paper Chromatography -Uses the property of molecules attraction to separate a mixture. 10. Fractional Crystallization -dissolved substance crystallize out of a solution once their solubility limit is reached as the solution cools.
