<p> Accelerated Chemistry Chapter 1 Notes Name ______(Student’s edition)</p><p>Chapter 1 problem set: 4, 5, 7, 9, 14, 18, 19, 20, 21, 24, 29</p><p>1.1 What is Chemistry?</p><p>Chemistry - the study of the , , and of substances and the they undergo. example – .</p><p>Most of the building materials, clothes, and medicines today are the result of .</p><p>Branches of Chemistry</p><p>- carbon chemistry - non-carbon chemistry - the study of energy and matter - the chemistry of living things - chemistry that identifies, quantifies, and qualifies</p><p>The Scientific Method - a logical way of solving problems</p><p>1. – state facts, collect data, search literature</p><p> qualitative vs. quantitative data ( vs. )</p><p>2. – organize data, analyze data, find relationships that lead to a hypothesis </p><p>Hypothesis – a statement - an educated guess about why a law occurs - may be discarded after later experiments or may become a law</p><p>Law - a describing a wide variety of behavior in nature Example: periodic law</p><p>3. Theorizing – how something occurs – often involves models Example: atomic theory</p><p>Theory - a generalization that explains a body of facts, but remains .</p><p>4. Testing – based on predicting the outcomes of an .</p><p>If testing fails, go back to steps 1, 2, or 3</p><p> page 1 1.2 Matter and Energy</p><p>Matter</p><p>Matter – anything that has and takes up .</p><p>Mass and weight – used interchangeably, but there is a difference…</p><p>Mass – quantity of , fixed amount</p><p>Weight - effect of on matter – changes with location</p><p>Law of Conservation of Mass – matter cannot be or in an ordinary chemical reaction (keyword being ordinary)</p><p>Energy </p><p>Energy – the ability to cause or do .</p><p>Kinetic – energy of </p><p>Potential – energy</p><p>Law of Conservation of Energy – energy can be from one form to another, but cannot be created or destroyed in an ordinary chemical reaction.</p><p>Why ordinary again? Extraordinary reactions ( ) happen where mass is converted into ( )</p><p>Types of energy – electrical, mechanical, chemical, sound, heat, electromagnetic radiation (energy of waves)</p><p>States of Matter</p><p>Phase of matter Solid Liquid Gas</p><p>Diffusion Particle closeness Definite volume Definite shape Compressibility Density Attractive Forces</p><p> page 2 Plasma – gas at extremely high temperature ( 1 x 108 K) where ______separate from the nucleus</p><p>Draw pictorial representations of phases of matter here:</p><p>Solid Liquid Gas</p><p>Properties and Changes of Matter</p><p>Properties – that enable us to distinguish one kind of matter from another</p><p>Physical property - Properties that can be observed without changing the of the material – 2 types of physical properties:</p><p>Intensive – of the amount ex. mp, bp, density, color, temperature</p><p>Extensive – on the amount ex. size, weight, mass, length, volume, heat</p><p>Chemical property – a property that can be observed when changing a substance into a substance ex: ______</p><p>Physical change – change in a substance which change the substance into something new. Ex. </p><p>Chemical change – a process where one or more substances are converted into other substances with characteristics.</p><p>Na (s) + Cl2 (g) → NaCl (s) reactant reactant product</p><p>Examples of chemical changes – .</p><p> page 3 Signs of a chemical change: ______</p><p>Precipitate – formation of a solid when mixing two </p><p>Energy and Changes in Matter - Chemical reactions involve energy</p><p>Exothermic ( heat) Endothermic ( heat)</p><p>Reactants → Products + Reactants + → Products water (l) → ice + heat → </p><p>Graph Graph</p><p>Other reactions – synthesis of water (exo), decomp. of CaCO3 (endo)</p><p> page 4 Classification of Matter Chart</p><p>Pure substance – a sample of Mixture – combination of two or matter where every particle is the ______more kinds of matter, but each ______its own properties</p><p>Element – substance that cannot be ______Homogeneous– uniform composition ______by ordinary chemical change where every sample is the same example – ______example – ______</p><p>Compound – substance that _____ be decomposed Heterogeneous – composition is _____ into 2 or more substances by chemical change uniform where samples are different example –______example – ______</p><p>All elements and compounds are homogeneous. Only some mixtures are homogeneous. Homogenous mixtures are transparent.</p><p>______– the smallest particle of some elements. Examples – ______</p><p>______– the smallest part of some elements and the smallest particle of all compounds Examples (elements) – ______Examples (compounds) – ______</p><p>Any element that is made of single atoms is also made of molecules, but the reverse is not necessarily true!</p><p>Classify these examples – Iron (Fe), milk, distilled water, tap water, chili, Co, CO, PbCl2</p><p>Law of Definite Composition – When a chemical compound is broken down, it always gives the same ______of its constituent elements (Joseph Proust – 1799)</p><p>Example – sugar C6H12O6 – ______(______)</p><p> page 5 1.3 The Chemical Elements</p><p>Draw picture of periodic table here – label group/family, period, metals, metalloids, nonmetals</p><p>Metals – (shine) Malleable (malleability) – ability to be into a sheet Ductility (ductile) – ability to be . High tensile strength – resistant to when pulled heat and electricity</p><p>Nonmetals – opposite of metals</p><p>Metalloids – some properties of metals and nonmetals – .</p><p>Nobel gases - .</p><p> page 6</p>