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Chapter 1 Matter and Change pp. 4- 27 1 Ch. 1 - Matter I. Introduction (p.5-7) What is Chemistry? Branches of Chemistry 2 What is Chemistry? The study of the composition, structure, and properties of matter and the changes it undergoes. Chemistry is a physical science. A basic understanding of chemistry is central to all other sciences. Chemistry is also central to our everyday lives. 3 Branches of Chemistry Inorganic Chemistry - study of substances without carbon Organic Chemistry - study of all substances containing carbon Biochemistry- study of the chemistry of living organisms 4 Ch. 1 - Matter II. Classification of Matter (p.15-17, 397-398) – Classifying Matter by Composition 5 Classifying Matter by Composition Homogeneous – matter with a uniform composition Heterogeneous - matter without a uniform composition Substance- A pure type of matter that does not vary from sample to sample. Includes elements and compounds 6 Classifying Matter by Composition Elements- simplest kind of matter, made of one type of atom An atom is the smallest unit of an element that maintains the properties of that element. Cannot be broken down into simpler substances by ordinary chemical means Ex. gold, copper, oxygen (on the periodic table) 7 Elements are Pure Substances 8 Element – composed of identical atoms – EX: copper wire, aluminum foil Classifying Matter by Composition Compounds – matter composed of the atoms of two or more elements chemically bonded Compounds can be broken down by chemical methods When they are broken down, the components have completely different properties than the compound. Ex. Sugar, salt, water, carbon dioxide 9 Compounds are Pure Substances Compound – composed of 2 or more elements in a fixed ratio – properties differ from those of individual elements – EX: table salt (NaCl) 10 Classifying Matter by Composition A mixture is a blend of two or more kinds of matter, each of which retains its own identity and properties. A mixture is mixed together physically. Variable composition, often expressed by a percent composition by mass or volume (Ex. 5% salt and 95% water) 11 Classifying Matter by Composition A heterogeneous mixture is not the same throughout (not uniform). Examples: M & M’s, Chocolate chip cookie, gravel, soil, rocks such as granite, blood, milk, salad, ocean water, etc. 12 Homogeneous mixtures are also called solutions. Ex. Salt water and Kool –aid Mixtures Variable combination of 2 or more pure substances. Heterogeneous 13 Homogeneous Mixtures Solution – homogeneous – very small particles – no Tyndall effect – particles don’t settle – EX: rubbing alcohol 14 Tyndall Effect Mixtures 15 Colloid – heterogeneous – medium-sized particles – Tyndall effect – particles don’t settle – EX: milk Mixtures 16 Suspension – heterogeneous – large particles – Tyndall effect – particles settle – EX: fresh-squeezed lemonade Mixtures 17 Examples: – mayonnaise colloid – muddy water suspension – fog colloid – saltwater solution – Italian salad dressing suspension Classify It Examples: – magnesium – Pizza – Calcium chloride – Orange juice – Club soda 18 Classify It Examples: – magnesium element – pizza hetero. mixture – Calcium compound chloride 19 – Orange juice hetero. mixture – Club soda Homo. (solution) Composition of Matter Flowchart MATTER yes MIXTURE yes Is the composition uniform? Homogeneous Mixture (solution) no Can it be physically separated? PURE SUBSTANCE no Heterogeneous Mixture yes Can it be chemically decomposed? Compound no Element Classifying at the Molecular Level Mixture Element Compound 21 Ch. 1 - Matter III. States of Matter (p.12) – Classifying Matter by the Kinetic Molecular Theory – States of Matter 22 Classifying Matter by Kinetic Molecular Theory KMT – Particles of matter are always in motion. – The kinetic energy (speed) of these particles increases as temperature increases. 23 Four States of Matter 24 Solids – very low KE - particles vibrate but can’t move around – fixed shape – fixed volume Four States of Matter 25 Liquids – low KE - particles can move around but are still close together – variable shape – fixed volume Four States of Matter 26 Gases – high KE - particles can separate and move throughout container – variable shape – variable volume Four States of Matter 27 Plasma – very high KE - particles collide with enough energy to break into charged particles (+/-) – gas-like, variable shape & volume – stars, fluorescent light bulbs, CRTs States of Matter Definite Definite Particle position Volume? Shape? and movement Solid Liquid Gas 28 YES YES NO YES Packed tightly, vibrate about fixed pt NO Close together, can move past each other - flow NO Far apart, move rapidly - flow Ch. 1 - Matter IV. Properties & Changes in Matter (p.11-14) – Extensive vs. Intensive – Physical vs. Chemical 29 Extensive vs. Intensive Extensive Property – depends on the amount of matter present Intensive Property – depends on the identity of substance, not the amount 30 Extensive vs. Intensive 31 Examples: – boiling point intensive – volume extensive – mass extensive – density intensive – conductivity intensive Physical vs. Chemical Physical Property – can be observed without changing the identity of the substance Chemical Property – describes the ability of a substance to undergo changes in identity 32 Physical vs. Chemical 33 Examples: – melting point physical – flammable chemical – density physical – magnetic physical – tarnishes in air chemical Physical vs. Chemical Physical Change – changes the form of a substance without changing its identity – properties remain the same Chemical Change – changes the identity of a substance – products have different properties 34 Physical Changes in Matter Condense Freeze Evaporate Melt Solid 35 Liquid Gas Physical Changes in Matter 36 Sublimation is a process in which a solid changes directly to a gas without going through the solid phase. Physical vs. Chemical 37 Examples: – rusting iron chemical – dissolving in water physical – burning a log chemical – melting ice physical – grinding spices physical Indications of chemical change 1 Production of heat, light, sound, or electricity 2.) Production of a gas 3.) Formation of a precipitate 4.) A change in color 5.) A change in odor 38 Separating Mixtures Mixtures are separated by their physical properties. Primary methods of separating mixtures are: filtration distillation centrifuge chromatography 39 Separating Mixtures Filtration is a method used to separate the components of mixtures that contain an insoluble solid and a liquid. Example: sand and water 40 Separating Mixtures Distillation is a method of separating substances in a mixture by evaporation of a liquid and subsequent condensation of its vapor. Example: desalination of salt water 41 Separating Mixtures Centrifuge (see p. 16) Used to separate solid-liquid mixtures such as those in blood. The centrifuge spins rapidly and causes the solid to settle to the bottom. Ex. Separating blood 43 Separating Mixtures Chromatography is a method of separating mixtures that uses a stationary phase and a mobile phase. Paper chromatography can be used to separate pigments because they move at different rates on the paper. 44 Ch. 1 - Matter V. Elements (p.20-24) – Extensive vs. Intensive – Physical vs. Chemical 45 Elements There are 92 naturally occurring elements Each has a 1 or two letter symbol First letter always capitalized second letter is lower case 46 Elements The periodic table shows the elements organized by their chemical properties Columns on the table represent groups or families of elements with similar chemical properties Properties vary across the horizontal rows or periods 47 Elements Three general classes of elements are metals, nonmetals, and metalloids. Metals are on the left and in the center of the periodic table. Nonmetals are on the right. Metalloids are on the zig-zag dividing line. 48 Metals 49 Nonmetals 50 Semi-metals or Metalloids 51 Noble Gases 52 Properties of metals Metals have certain properties: shiny luster, reflect heat and light, ductile, malleable,very tensile, good conductor of heat and electricity. All metals except mercury are solids at room temperature. 53 Properties of nonmetals Nonmetals have certain properties: poor conductor of heat and electricity, dull luster and brittle if solids, many nonmetals are gases. Bromine is a dark red liquid. 54 55 Properties of metalloids Metalloids have properties of metal and nonmetals, they are semiconductors, they are all solids. Metalloids are B, Si, Ge, As, Sb, Te, Po, and At 56 57 Elements Noble gases (Group 18) are nonmetals that are essentially non-reactive elements. They are gases at room temperature 58 Elements to memorize 59 Quiz # 1 – Symbols and correct spelling for elements # 1-46 Quiz #2 - Symbols and correct spelling for elements # 47-92