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Matter and Change Chapter 1 Objectives • Define Chemistry • Define properties of matter Objectives • Identify and explain physical properties • • • • • Density melting point boiling point Conductivity Malleability • Identify and explain chemical properties • the ability to form new substances. • Distinguish between chemical and physical changes. Objectives – Explain the difference between pure substances (elements and compounds) and mixtures. – Differentiate between heterogeneous and homogeneous mixtures. – Describe the three normal states of matter (solid, liquid, gas) in terms of energy, particle motion, and phase transitions. Introduction to Chemistry • Chemistry – the study of matter and the changes it undergoes • the “central science” Matter • Anything that takes up space and has mass The States of Matter SOLID LIQUID GAS PLASMA States of Matter State of Matter Volume Shape Solid Definite Definite Liquid Definite Indefinite Gas Indefinite Indefinite Plasma Indefinite indefinite Changes in State • Name of Transitions between states of matter: – Melt/freeze – Boil/Condense – Sublimation/deposition • Mostly obtained by heating or cooling (add or remove energy) Condense Freeze Melt Solid Boil Liquid Gas Classification of Matter Matter • Matter is classified into different categories based on the composition of the material • Mixtures: matter consisting of a variable composition • Pure substances: matter made of definite composition Mixtures • Are heterogeneous or homogeneous • Are a physical blend of two or more pure substance • Have variable composition • Can be separated by physical change • Separation Techniques depend on type of mixture Heterogeneous Mixtures • Uneven blend of two or more pure substances • Different substances or phases of matter can be visibly seen • Can be separated by physical means like filtration Homogeneous Mixtures • Also known as solutions • Even blend of two or more pure substances • Look uniform throughout the mixture • Can be separated by physical means like distillation, crystallization or chromatography Separation Techniques Heterogeneous Filtration Homogeneous Distillation Crystallization Chromatography Study Buddy Review • What is a mixture? • What is the difference between a homogeneous and heterogeneous mixture? • Provide an example of homogeneous and heterogeneous mixture. Pure Substances • Matter made of material with a unique set of chemical and physical properties • Have constant composition • Cannot be separated by physical change • Are elements or compounds Elements • Pure substances that cannot be separated into simpler substances by a chemical change Compounds • Substance that contains two or more elements chemically combined in fixed (constant) proportions • Can be separated into elements by chemical change • Types: covalent or ionic http://cwis.nyu.edu/pages/mathmol/modules/water/water.html Study Buddy Review • What is a pure substance? • What is the difference between an element and a pure substance? • Provide an example of an element and a compound. • Where would you find a list of elements? Which is it? Mixture Element Compound Study Buddy Review • What is a mixture? • What is the difference between a homogeneous and heterogeneous mixture? • Provide an example of homogeneous and heterogeneous mixture. Physical and Chemical Properties Properties of Matter Physical Properties Property of an object that can be observed or measured without changing the substance • Examples and values for water: – Density – Color – Freezing Point 1 g / 1 mL or 1 g / cm3 colorless 0o C Density • Density is the mass per unit volume of a substance • D = mass / volume – Measured in g / mL or g / cm3 • Less dense objects float on more dense objects • Density of liquid water is more than density of ice (so ice floats in liquid water) Significance of Physical Properties • Help to identify a substance • Examples: –Density –Melting Point –Boiling Point Properties of Matter Chemical Properties Relates to a substance’s ability to undergo changes that transform it into different substances • Examples : – flammability – Ability to rust How do you know if chemical reaction occurred? • Chemical changes produce new, different substances – – – – Precipitate formed (solid) Gas formed (bubbling) Energy change occurs (colder or hotter) Color change (can also be physical—be careful!) Significance of Chemical Properties • Chemical changes are chemical reactions • Examples: –Combustion –Oxidation –neutralization Extensive and Intensive Properties • Extensive: depend on the amount of matter that is present • Examples: – Mass – Volume – energy • Intensive: do NOT depend on the amount of matter that is present • Examples: – Melting point – Density – temperature Law of Conservation of Energy • Law of Conservation of Energy: in all physical and chemical changes, energy is neither created or destroyed • Energy: the capacity to do work or produce heat • Measured in Joules (SI unit) Law of Conservation of Matter • Law of Conservation of Matter: in all chemical and physical changes, matter is neither created or destroyed • A chemical change is a really chemical reaction 4 Fe + 3 O2 2 Fe2O3 Reactants products • Antoine Lavoisier: – Made accurate and precise measurements during chemical reactions Study Buddy Review Classify each as a physical or chemical property of matter: • • • • • • • • • • Blue Color Ability to Rust Density Flammability Reacts with a base to form water Boiling Point Reacts with water to form a gas Luster Mass Odor