Properties of Matter

Essential Questions How does the state of matter define its properties Essential Questions How 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 Anything with MASS & VOLUME (solid, liquid, gas) Pure Substances Mixtures EQ: How can matter be classified?

MIXTURES Mixtures = two or more substances PHYSICALLY combined. Can be PHYSICALLY separated

Heterogeneous Mixtures Hetero = different Geneous = origin or beginning has separations and/or boundaries can see to different parts Are ALL mixtures

Heterogeneous Mixtures Physically combined substances

Homogeneous Mixtures Homeo = same Geneous = origin or beginning matter of the SAME make-up (no boundaries)

Others  alloys, colloids, etc. Homogeneous Mixtures Homogeneous Mixtures Solutions Others  alloys, colloids, etc.

Homogeneous Mixtures Homogeneous Mixtures Solutions Solute Solvent

Solutions EQ: What are the essential components of solutions? Homogeneous mixtures Physically NOT chemical combined Solute = the substance BEING dissolved Solvent = the substance DOING the dissolving

EQ: Why is water the universal solvent? 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.

3 2 1 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 Pure Substances Elements Compounds

EQ: How are atoms, molecules & ions alike and how are they different? 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?

Elements EQ: 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

Elements & Compounds Pure Substances Elements Atoms Symbols Compounds Molecules 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

EQ: How does the state of matter define its properties? 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 is 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)

3 2 1 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. _____________________________________

EQ: What are the chemical & physical properties of pure substances? 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 Change EQ: 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

Density The amount of matter in a given amount of space Density = mass ÷ volume D = m/v D = ? Mass = m = 96.5 grams Volume = v = 5 cm3 D = 96.5 g / 5 cm3 = 19.3 g/cm3 19.3 g/cm3 is the density of gold The density of water = 1.0 g/mL Density

BUOYANCE The ability of a fluid (liquid or gas) to exert an upward force on an object immersed in it. If buoyant force = object’s weight the object will float

GAS LAWS Boyle’s Law: pressure and volume Volume decreases as Pressure increases Pressure decreases as Volume increases

Gas Laws Charles’s Law: temperature & volume Volume increases as Temperature increases Volume decreases as Temperature decreases