Matter

Matter vs. Energy The universe is made up of matter and energy. Has mass and takes up space (volume) Is usually a “thing” Energy: Does not have mass or take up space Energy moves matter!!!!!! ** Energy is the ability to make things move. Light, heat, sound, motion, and electricity are all forms of energy.

Properties of Matter All matter has characteristics, or properties These properties can either be: Chemical Physical

Physical Properties Physical property- any property of matter that can be observed or measured without changing the identity of the matter Examples color shape taste density state/phase malleability D = M V

Volume and Density Volume= length X width X height Density= mass (g) volume (mL or cm3) 1 mL = 1 cm3 Which is more dense?

Physical Properties States of matter: Bose-Einstein Solid Liquid Gas Plasma (Newest State)

Bose-Einstein Condensate Exist at extremely cold temperatures (around absolute zero or -460 oF) Particles are super unexcited Particles lock or “clump” together so firmly that they move as a single unit

Solid Particles are tightly compact Particles vibrate without the ability to move freely Definite shape and volume Solid Animation

Liquid Particles are tightly compact, but able to move around close to each other No definite shape, but definite volume Liquid Animation

Gas Particles can easily spread out or move close together Particle move freely and with a lot of energy No definite shape or volume Gas Simulation

Plasma Particles broken apart and move freely with extremely high energy Exist at extremely high temps (several million degrees Celsius) Not too common on earth, but the most common form of matter in the universe Examples: Florescent and neon lights, lightning, fire Why do you think this is the most common form/state of matter in the universe?

Physical Properties Physical states of matter result from the amount of energy that the particles composing the matter have. More energy = more movement for the particles If you were to compare an ice cube and the steam created from boiling water, which would you think has more energy?

Types of Energy Potential- stored energy Kinetic energy- energy a moving object has Temperature-average kinetic energy of all atoms in a substance Thermal energy- sum of both the kinetic and potential energy of the atoms of a substance

Physical Properties What about this states of matter continuum could be considered a little misleading? Taken from: http://www.chem4kids.com/files/matter_becondensate.html

Changes in States (Physical Changes) Why do you think Bose-Einstein and plasma are not equally distanced from the other three states of matter? Plasma Disposition Vaporization (Evaporation/Boiling) Gas Liquid Condensation Melting Solid Freezing Sublimation Bose-Einstein All changes in state require a change in energy

Heating Curve The heating curve below shows how adding more thermal energy results in changes in the states of water boiling point melting point

Thermal Expansion Thermal expansion- the increase in the size of a substance when the temperature is increased. Hot air balloons rise due to the thermal expansion of air Colder water will contract and sink Density and temp The exception of this is water because when it becomes ice it expands and floats

Physical Properties of Fluids Fluid- any substance that can flow, like a liquid or gas Buoyancy- the ability of a fluid to exert an upward force on an object immersed in it. Archimedes principle-the buoyant force on an object is equal to the weight of the fluid displaced by that object

Density and Buoyancy Density= mass (g) volume (mL or cm3) Because saltwater has the additional mass of salt in the water and is more dense, things are more buoyant in saltwater than fresh Generally if an object is more dense than the fluid, it will sink If an object is less dense it will float

Physical Properties of Fluids Pascals principle- pressure applied to a fluid is transmitted throughout the fluid P (Pascals)= Force (Newton) Area (m2) where one Pascal is a N/m2

Check for Understanding As you sit here, atmospheric pressure from the air is pushing on you If the atmospheric pressure at sea level is 101 kPa (or N/m2), and the average human’s area is 1.80 m2, with how much force does the atmosphere push on the average human?

Check for Understanding As you sit here, atmospheric pressure from the air is pushing on you If the atmospheric pressure at sea level is 101 kPa (or N/m2), and the average human’s area is 1.80 m2, with how much force does the atmosphere push on the average human? P = F so F = PA A F (N) = 101 kPa X 1.80 m2 = 101,000Pa X 1.80 m2 F (N) = 182,000 Pa m2 = 182,000 N

Physical Properties of Fluids Bernoulli’s principle- fluid velocity increases when the flow of the fluid is restricted

Physical Properties of Fluids Viscosity- the resistance of a fluid to flowing. Maple syrup is very viscous, even more so cold than when warm Water is not viscous at all

Physical Properties of Gases Boyle’s Law- decrease the volume of a container of gas and hold the temp constant, pressure from the gas will increase Conversely, increase the volume of a container of gas holding the temp constant, pressure from the gas will decrease

Boyle’s Law Boyle’s Law as an equation: PiVi = PfVf where i=initial and f=final If a weather balloon has a volume of 100L when it is released at sea level where the pressure is 101 kPa, what will be the balloon’s volume when it reaches an altitude where the pressure is 43 kPa? PiVi = PfVf so = PiVi = Vf Pf Vf = 100L X 101,000Pa = 235L 43,000 Pa

Check for Understanding Boyle’s Law as an equation: PiVi = PfVf where i=initial and f=final If a balloon has a volume of 11L when it is released at sea level where the pressure is 101 kPa, what will be the balloon’s volume when it reaches an altitude where the pressure is 86 kPa?

Check for Understanding Boyle’s Law as an equation: PiVi = PfVf where i=initial and f=final If a balloon has a volume of 11L when it is released at sea level where the pressure is 101 kPa, what will be the balloon’s volume when it reaches an altitude where the pressure is 86 kPa? PiVi = PfVf so = PiVi = Vf Pf Vf = 11L X 101,000Pa = 12.9L 86,000 Pa

Physical Properties of Gases Charles’s Law- the volume of a gas increases with increasing temperature as long as the pressure on the gas is constant

Charles’s Law Charles’s Law as an equation: Vi = Vf where i=initial and f=final Ti Tf and temperature must be measured in Kelvin K = oC + 273 Remember: 0K is absolute zero 273K is the freezing point of water 373K is the boiling point of water

Charles’s Law A 2L balloon at room temperature (20.0oC) is placed in a refrigerator at 3.0oC. What will be the balloon’s volume be after it cools? K = oC + 273 So Ti = 293K and Tf = 276K Vi = Vf so Vi X Tf = Vf Ti Tf Ti Vf = 2L X 276K = 1.89 L (it shrinks!) 293K

Check for Understanding What would be the final volume if the balloon was put in a -18oC freezer?

Check for Understanding What would be the final volume if the balloon was put in a -18oC freezer? K = oC + 273 So Ti = 293K and Tf = 255K Vi = Vf so Vi X Tf = Vf Ti Tf Ti Vf = 2L X 255K = 1.7 L (it shrinks smaller!) 293K

Physical Properties of Solids Malleable- able to be hammered or pressed out of shape without breaking This is a property of many metals

Composition of Matter All matter has a composition, what it’s made of Different kinds of composition are: Pure substances- type of matter with a fixed composition that can’t be separated physically Element Compound Mixture- can be separated physically Solutions Colloids Mechanical mixture

MATTER PURE SUBSTANCES (non-mixtures) MIXTURES COLLOIDS ELEMENTS COMPOUNDS SOLUTIONS SUSPENSIONS HOMOGENEOUS MECHANICAL MIXTURES HETEROGENEOUS

Pure Substances Element- made up of one kind of atom that can’t be broken down into simpler substances by physical or chemical means 90 occur naturally on Earth 25 were synthesized (made) by scientists

Pure Substances Compound- substance composed of two or more different elements (atoms) that are chemically combined Examples: H2O, CO2,CO, NO2,

characteristics of these Mixtures Mixtures- combination of two or more substances that do not combine chemically, but remain the same individual substances; Can be separated by physical means Two types: Heterogeneous Homogeneous Based on the prefixes “hetero” and “homo,” what do you think are characteristics of these two types of mixtures?

Heterogeneous Mixtures “Hetero” = different Consists of visibly different substances or phases (solid, liquid, gas) Mechanical mixture- visibly not wholly one Example: Notice the visibly different substances in these mechanical mixtures Pizza Trail Mix

Heterogeneous Mixtures Suspension- special type of heterogeneous mixture of larger particles that eventually settle

Heterogeneous Mixtures Colloids- heterogeneous mixture with particles that never settle Milk and paint Have a foggy appearance because its particles are large enough to scatter light, unlike a solution

Homogeneous Mixtures “Homo” = same Has the same uniform appearance and composition throughout; maintain one phase (solid, liquid, gas) Commonly referred to as solutions Example: Notice the uniform appearance Salt Water

Homogeneous Mixtures Solution- a mixture of two or more substances that is identical throughout Can be physically separated Composed of solutes and solvents Salt water is considered a solution. How can it be physically separated? the substance in the smallest amount and the one that dissolves in the solvent the substance in the larger amount that dissolves the solute Iced Tea Mix (solute) Water (solvent) Iced Tea (solution) Colloids (milk, fog, jello) are considered solutions

Solutes Change Solvents The amount of solute in a solution determines how much the physical properties of the solvent are changed Examples: Lowering the Freezing Point Raising the Boiling Point The freezing point of a liquid solvent decreases when a solute is dissolved in it. Ex. Pure water freezes at 320F (00C), but when salt is dissolved in it, the freezing point is lowered. This is why people use salt to melt ice. The boiling point of a solution is higher than the boiling point of the solvent. Therefore, a solution can remain a liquid at a higher temperature than its pure solvent. Ex. The boiling point of pure water is 2120F (1000C), but when salt is dissolved in it, the boiling point is higher. This is why it takes salt water longer to boil than fresh water.

Concentration Concentration- the amount of solute dissolved in a solvent at a given temperature Described as dilute if it has a low concentration of solute Described as saturated if it has a high concentration of Described as supersaturated if contains more dissolved solute than normally possible

Solubility The amount of solute that dissolves in a certain amount of a solvent at a given temperature and pressure to produce a saturated solution Influenced by: What do we call things that are not soluble? Temperature Pressure Solids increased temperature causes them to be more soluble and vice versa Gases increased temperature causes them to be less soluble and vice versa Ex. Iced Coffee Solids increased pressure has no effect on solubility Gases increased pressure causes them to be more soluble and vice versa Ex. Soda, “The Bends”

Chemical Properties Chemical property- any property of matter that describes a substance based on its ability to change into a new substance Examples flammability reactivity with vinegar reactivity with oxygen Iron + Oxygen  Iron oxide (rust) 2Fe + 3O2  Fe2O3

Chemical or Physical Property? Paper is white Boiling point of H2O is 100oC Zinc reacts with hydrochloric acid and creates hydrogen gas Nitrogen does not burn Sulfur smells like rotten eggs Physical Property Physical Property Chemical Property Chemical Property Physical Property

Comparing Physical and Chemical Properties Substance/Matter Physical Property Chemical Property Helium Less dense than air Nonflammable Wood Grainy texture Flammable Baking soda White powder Reacts with vinegar to produce bubbles Powdered sugar Does not react with vinegar Rubbing alcohol Clear liquid Red food coloring Red color Reacts with bleach and loses color Iron Malleable Reacts with oxygen

Changes in Matter Matter is constantly changing There are two types of changes in matter: Chemical Physical

Physical changes are not indicative of a chemical reaction Physical change- a change in shape, size, color, or state a change without a change in chemical composition Examples tearing paper cutting your hair change in state Some mixtures can be separated based on their physical properties The Mixtures Lab Physical changes are not indicative of a chemical reaction

Changes in States (Physical Changes) Why do you think Bose-Einstein and plasma are not equally distanced from the other three states of matter? Plasma Disposition Vaporization (Evaporation/Boiling) Gas Liquid Condensation Melting Solid Freezing Sublimation Bose-Einstein All changes in state require a change in energy

Physical Changes Simulation 1 Simulation 2 Chemistry of Chocolate This is what happens when energy is added and taken away

Chemical Changes Chemical change- a change in which a substance becomes another substance having different properties A change that is not reversible using ordinary physical means Changes that usually cause, heat, sound, light, odor, fizzing/foaming, color changes Examples mixing vinegar & baking soda burning a piece of wood soured milk A chemical analysis is the only 100% way to know a chemical change has occurred.

Chemical Changes Chemical reaction- the process by which a chemical change occurs Types of chemical reactions Synthesis (creating) Decomposition (separating) Combustion (burning) Displacement/Replacement (switching of atoms)

Chemical Changes During chemical changes, atoms are rearranged, and chemical bonds are broken and reformed One or more substances change to produce one or more different substances What does H2 & O2 gas create? Out of the four types of reactions, which would describe the chemical reaction taking place to the right? H2 O2

Chemical or Physical Change? Bending a Paper Clip Baking a cake The sublimation of carbon dioxide Crushing an aluminum can Vinegar and baking soda combining to create salt and water Physical Change Chemical Change Physical Change Physical Change Chemical Change

Law of Conservation of Mass Proposed by Antoine Lavoisier In a chemical reaction, atoms are neither created nor destroyed All atoms present in the reactants are also present in the products Chemical equations must be balanced to show the conservation of mass In its present form, does this chemical equation show a conservation of mass? 2 H2 + O2  2 H2O Reactants Products How would you balance this equation to show the conservation of mass? H  2 O  2 4 2 H  2 O  1 4 2