Download
1 / 51
E N D
Essential QuestionsHow does the state of matter define its properties?What are the real-life examples of molecules, atoms & ions?How are atoms, molecules & ions alike and how are they different?How can matter be classified?What are the essential components of solutions?Why is water the universal solvent?In what ways can matter be quantified?What units should be used to quantify matter?What are the chemical & physical properties of pure substances?How can chemical and physical changes be determined in a laboratory setting?
The Breakdown of Matter EQ: How can matter be classified?
Heterogeneous Mixtures • Hetero = different • Geneous = origin or beginning • has separations and/or boundaries • can see to different parts • Are ALL mixtures
HomogeneousMixtures • Homeo = same • Geneous = origin or beginning • matter of the SAME make-up • (no boundaries)
SolutionsEQ: What are the essential components of solutions? • Homogeneous mixtures • Physically NOT chemical combined • Solute = the substance BEING dissolved • Solvent = the substance DOING the dissolving
Examples of Solutions • Alloys = solid mixture or solution (brass, 14K gold, steel) • Air = gas mixture or solution • Liquid solutions = sweet tea, coffee, milk, tap water EQ: Why is water the universal solvent?
Solution Properties • Soluble = the solute is able to dissolve in the solvent • Insoluble = the solute is NOT able to dissolve in the solvent
Descriptions of a Solution • Diluted Solutions = small amount of solute and/or a large amount of solvent • Concentrated Solutions = large amount of solute and/or a small amount of solvent • Saturated Solution = a solution that will NOT dissolve any more solute
An increase in temperature will allow more solute to dissolve in a solvent. The molecules of the solvent move faster and further apart allowing more room for more solute molecules.
Name three properties of solutions: 1. __________________________________ 2. __________________________________ 3. __________________________________ 3 Name two types of mixtures & two types of pure substances. 1. ____________________________________ 2. ____________________________________ 2 1 What is the one key in distinguishing between homogeneous and heterogeneous mixtures 1. _____________________________________
Pure Substances • chemically pure substances • only one part or one kind of matter • Elements = found on the periodic table • Compounds = 2 or more elements that have combined CHEMICALLY EQ: How are atoms, molecules & ions alike and how are they different?
ElementsEQ: What are the real-life examples of molecules, atoms & ions? • 90 natural occurring elements • found on the periodic table • Atoms = smallest part of an element • represented by symbols
Compounds • 2 or more elements that have combined CHEMICALLY • Molecules = smallest part of a compound • represented by formulas
States of Matter • Also called Phases of Matter • Solids • Liquids • Vapors (gases)
Solids • Have a definite shape • Have a definite volume • Particles VIBRATE in place
Liquids • Have NO definite shape • Have definite volume • particles SLIDE freely
Gases (vapor) • Have NO definite shape • Have NO definite volume • particles fill the volume of the container
Solids, Liquids & Gases • Solids = can form crystals = solid where the particle are arranged into repeating patterns. • Liquids = physical property of Viscosity = “thickness” – the resistance to flow. • Gases = volume of gases depend greatly on pressure and temperature. EQ: How does the state of matter define its properties?
Phase Changes • Melting • Freezing • Vaporization • Condensation • Sublimation • physical changes
Melting • the process of changing from a solid to a liquid • energy is being put into the substance • melting point = the temperature at which melting occurs – physical property • the melting point of water is 0ºC
Freezing • the process of changing from a liquid to a solid • energy is being pulled out of the substance • freezing point =same temperature as the melting point • (used mainly in weather)
Vaporization • the process of changing from a liquid to a gas • energy in being put into the substance • evaporation • boiling
Evaporation • vaporization that occurs at the surface of the liquid
Boiling • vaporization that occurs throughout the liquid • boiling point= the temperature at which boiling occurs • the boiling point of water is 100ºC
Condensation • the process of changing from a gas to a liquid • energy is being pulled out of the substance
Sublimation • the process of changing from a solid to a gas • energy is being put into the substance • ex: dry ice (CO2)
Name three phases of matter: 1. __________________________________ 2. __________________________________ 3. __________________________________ 3 Name two types of vaporization. 1. ____________________________________ 2. ____________________________________ 2 1 What is the so different about sublimation? 1. _____________________________________
Properties of Matter • characteristics that can identify and describe matter. • Physical Properties • Chemical Properties EQ: What are the chemical & physical properties of pure substances?
Physical Properties • observable properties • physical change = changes that occur while the substance remains the same. • ex: phase change
Examples of Physical Properties • density (d=m/v) • color • melting point & boiling point • hardness • phase of matter • malleable • ductile • taste • conductivity • luster • texture • solubility
Chemical Properties • properties that describes how the substance interacts with other substances or will act chemically • chemical change = an actual chemical reaction takes place and a NEW substance is formed • ex: combustion
Examples of Chemical Properties • flammability • reactivity • combustion • oxidation • reacts with _____ • endothermic • exothermic • forms a precipitate
Chemical ChangeEQ: How can chemical and physical changes be determined in a laboratory setting? • Color change • Temperature change = reaction is either endothermic or exothermic • Gas given off • Precipitate formed = solid formed in the reaction of two liquids
Energy (temperature) Changes in Reactions • Endothermic reactions • Energy is put into the reaction • Reaction stops as soon as energy is no longer put into the reaction • Ex: cooking • Exothermic reactions • Energy is given off in the reactions • Ex: burning
Exothermic Reactions • May require energy to be put into to the reaction in order to start or activate the reaction • Activation Energy = energy required to start an exothermic reaction
Reducing Activation Energy • Catalysts are often used to reduce the activation energy required to start an exothermic reaction
Chemical change vs. Physical change • ask the question, “Has a new substance been formed?” • “yes” = chemical change • “no” = physical change
Examples of Problems • ex: 2H2 + O2 2H2O • hydrogen gas combines with oxygen gas to form water • a new substance is formed • a chemical reaction occurs EQ: How can chemical and physical changes be determined in a laboratory setting?
Examples of Problems • : N2 + O2 + CO2 = air • nitrogen gas combines with oxygen gas and carbon dioxide gas and a few other gases mix • NO chemical reaction takes place • physical change has taken place in the gases
Examples of Problems • Ice melting • Phases change • Solid Liquid • No new substance is formed…it is still water • Physical change
Malleable • A physical property that describes being able to be flatten or pounded onto sheets • This property is associated with metals.
Ductile • A physical property that describes being able to be drawn into a wire. • This property is associated with metals.
Luster • A physical property that describes how a substance reflects light • This property is often associated with minerals, gem stones, metals and nonmetals.
Oxidation • A chemical property describing a substance reaction with oxygen • slow oxidation = rusting, tarnish, corrosion • fast oxidation = burning, exploding, combustion
