Chemistry Day 5 Friday, August 31 st Tuesday, September 4 th, 2018
Do-Now Title: BrainPOP: States of Matter 1. Write down today s FLT 2. List two examples of gases 3. List two examples of things that are liquid 4. What do you think the difference between a liquid and a gas is? 5. How can you turn water into ice, and ice into water? What do you need to do? 6. Underneath your do-now, write brainpop practice and number 1-10 7. Turn in your lab packet when finished Finished? Take out your planner and table of contents.
Chapter 13 Notes Intro
Identifying Substances Matter that has a uniform and definite composition is called a substance Ex: Gold and Copper
States of Matter 3 states of matter: solid, liquid, and gas. All matter is made up of tiny particles
States of Matter Solid: dopamine Definite shape Definite volume. The particles in a solid are packed tightly together, have an orderly arrangement, and vibrate in place
Liquid: States of Matter Indefinite shape & definite volume. Flows. Liquids are not easily compressed The particles in a liquid have enough energy to move freely in random directions, but remain close to each other.
Gas: States of Matter Indefinite shape and volume (takes the shape and volume of its container) It s easily compressed because there s so much empty space. Gas particles move at high speeds and randomly.
Pair-Share-Respond 1. What are the 3 states of matter? 2. Describe each of the three states in terms of their shape and volume. 3. Describe each of the three states in terms of their molecules.
Ch. 13 Part A: The Nature of Gases
Kinetic Energy
Kinetic Energy Kinetic energy: Energy an object has because of its motion Think about it: To accelerate an object, we must apply a force. But once applied, energy has been transferred to the moving object. Kinetic energy is simply the energy an object has because of its motion
Kinetic Energy
Kinetic Energy All matter consists of tiny particles that are in constant motion. In a gas, these particles are molecules or atoms
Kinetic Energy & Gases In the 1800s, scientists were studying gases. How could they describe the properties of substances with no fixed shape or volume?
Kinetic Theory Applied to Gases 1. Gases are made of molecules. These are tiny spheres with insignificant volume 2. Molecules are in constant, random motion. They have kinetic energy. 3. Collisions are perfectly elastic. When molecules collide, they do not lose kinetic energy
Behavior of Gases
Properties of Gases The molecules in gases are in constant motion This allows gases to expand until it fills its container
Gas and Temperature As temperature increases, molecules move faster As temperature decreases, molecules move slower Avg KE is directly proportional to temperature NOTE: At absolute zero (Kelvin), there is no movement of particles.
Gas Pressure
Gas Pressure Pressure is defined as force per unit area For example, a high heel shoe exerts a greater pressure than a normal shoe due to the smaller area of contact Larger shoes spread out the force over a greater area
Gas Pressure Gas particles exert pressure when they collide with the walls of their container Individual gas molecules exert a minimal pressure Gas pressure is caused by collisions of many particles against objects
Air is a mixture of gases Air Pressure
Air Pressure Because air particles are in constant motion, they exert pressure. We call this pressure atmospheric pressure or air pressure
Gas Pressure
Atmospheric Pressure Atmospheric pressure = pressure due to collisions by air molecules. Pressure decreases with increasing altitudes
Barometer Barometer measures atmospheric pressure
Pair-Share-Respond 1. Define or describe kinetic energy 2. Identify the three parts of the kinetic molecular theory applied to gases 3. What happens to kinetic energy as temperature increases? 4. What is atmospheric pressure?
Measurements
Measurements In chemistry, we often use measurements at standard temperature and pressure (STP) Standard temperature and pressure (STP) = 273 K (0 C) and 1 atm pressure
Measurements In chemistry, we often use different units for the same measurement Ex/ temperature can be measured in Fahrenheit, Celsius, or Kelvin units 0 C = 32 CF = 273 K Consequently, we need to be able to convert between these units
Converting Between Units of Pressure Units of Pressure: Pascal (Pa) SI unit Kilopascal (kpa) Millimeters of mercury (mmhg) Atmospheres (atm) Torr
Converting Between Units of Pressure Conversion Factors for Pressure: 1atm = 760mmHg = 760torr = 101,325Pa = 101.325kPa
Converting Between Units of Pressure First: Write what you start with Second: Draw a conversion factor (ratio) this is called dimensional analysis New Units Given Number and units Given Units
Converting Between Units of Pressure Ex/ Convert 0.875 atm to mm Hg Recall:1atm = 760mmHg = 760torr = 101,325Pa = 101.325kPa Given Number and units
Now you try! Convert 98.35 kpa to atm Convert 9.1 torr to mm Hg
Chemistry Day 6 Wednesday, September 5 th Thursday, September 6 th, 2018
Do-Now Title: Ch. 13/14 CN Part B 1. Write down today s FLT 2. List and briefly describe the three states of matter. 3. Convert 74.35 kpa to atm. Show all work and units. 4. Convert 9.1 atm to mmhg. Show all work and units. 5. We will take notes under our do-now. Draw or fold your column for cornell notes. Finished? Take out your planner and table of contents.
FLT I will be able to describe the properties of liquids and solids by completing Ch. 13/14 Notes B Standard HS-PS1-4: Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.
Recall
States of Matter 3 states of matter: solid, liquid, and gas. All matter is made up of tiny particles
The Nature of Liquids
The Nature of Liquids Liquids have an indefinite shape and a definite volume The molecules in liquids are always moving, so they have kinetic energy This allows them to take the shape of their container just like gases
Gas Particles vs. Liquid Particles Gas particles are different than liquid particles: 1. Liquid particles attract each other, but gas particles do not.
Gas Particles vs. Liquid Particles Gas particles are different than liquid particles: 2. Because of their attraction, liquid particles are closer together. Liquids have a definite volume
Gas Particles vs. Liquid Particles Gas particles are different than liquid particles: 3. Liquids are more dense than gases. Liquid molecules are more closely packed together.
Changing State Liquids can turn into gases and vice versa
What s happening? Vaporization = liquid à gas/vapor
Evaporation Evaporation = vaporization at the surface of a liquid that is not boiling
Evaporation Liquids evaporate faster when heated AVG KE increases Liquid particles are able to move faster and separate
Vapor Pressure Vapor Pressure = pressure exerted by a vapor over a liquid Water vapor collects above the liquid and exerts pressure due to collisions
Boiling Point Remember: liquids are attracted to each other. They LIKE being close together. Adding heat adds energy so that particles can overcome the attractive forces and enter the gaseous state.
Boiling Point Boiling Point (BP) = temperature at which the VP of the liquid is equal to the external pressure on the liquid. Molecules even at the bottom of the liquid have enough energy to vaporize, so they rise to the surface
Pair-Share-Respond 1. Identify two ways that liquids differ from gases 2. Distinguish between the terms vaporization and evaporation 3. Why does heating increase the rate of evaporation? 4. Define the term vapor pressure
The Nature of Solids
The Nature of Solids Solids have a definite shape and volume Solids à orderly arrangement, vibrate in fixed positions, and do not flow
Change of State Solids can turn into liquids and vice versa
Melting Point Melting point (MP) = temp at which solid à liquid = the same temp as the freezing point (liquid à solid) At the melting point, the vibrations are strong enough to overcome the attractions holding them in fixed positions.
Crystalline Structure Solid structures = Most are crystalline In a crystal the particles are arranged in an orderly, repeating, three-dimensional pattern called a crystal lattice.
Crystalline Structure Are ALL solids crystalline? Some solids may be amorphous. Amorphous solids = lack uniform, geometric arrangement
Allotropes Allotropes = Some solid substances can exist in more than one form Ex. Allotropes of carbon (diamonds and graphite) Different structures give allotropes different properties
Pair-Share-Respond 1. Describe how you would draw a solid 2. Distinguish between the terms crystalline structure and amorphous solids 3. What are allotropes?
Chemistry Day 7 Friday, September 7 th Monday, September 10 th, 2018
Do-Now Title: Ch. 13/14 Notes C 1. Write down today s FLT 2. List the three states of matter and list an example for each 3. List two similarities between gases and liquids 4. is the change of a liquid into a vapor 5. Explain why changing the temperature can help speed up the process of evaporation. 6. We will take notes under our do-now. Draw or fold your column for cornell notes. Finished? Take out your planner and table of contents.
FLT I will be able to identify the temperature and pressure conditions for states of matter by completing Ch. 13/14 Notes C Standard HS-PS1-4: Develop a model to illustrate that the release or absorption of energy from a chemical reaction system depends upon the changes in total bond energy.
Changes of State
Changes of State: Draw This Sublimation Melting Vaporization Freezing Condensation KE Increases
Changes of State Sublimation = Direct change from solid to vapor (without passing through liquid phase)
Changes of State Sublimation can occur because solids and liquids have vapor pressure Sublimation occurs in solids with vapor pressures that exceed atmospheric pressure at or near room temperature.
Sublimation Applications: Freeze-dried goods, coolants, and air fresheners.
Phase Diagrams Phase Diagram = Diagram that shows the relationships among solid, liquid, and vapor states of a substance
Phase Diagrams Shows the temperature and pressure at which substances exist at each state You can locate the normal melting point, normal boiling point, triple point, and critical point on the diagram
Triple Point
Phase Diagrams Triple Point = Set of conditions at which the three phases exist in equilibrium At the critical point, the physical properties of the liquid and gaseous states are identical
That s it J
States of Matter Inquiry Mini- Lab