Unit 1: Matter

Essential Question What are the characteristics of the various states of matter?

Definitions Intermolecular force: the attractive forces between molecules Kinetic energy: energy in motion

Picture or description Shape (fixed or variable) State Particles Picture or description Shape (fixed or variable) Volume (fixed or variable) IMF (strong or weak) Kinetic Energy (High or Low) Solid Liquid Gas

Endothermic vs. Exothermic Endothermic: When a system absorbs energy from its surroundings. Increases in KE, feels cold Exothermic: a system releases energy to its surroundings, decreases in KE, feels warm

Solid Gas Liquid

Phase Diagram List 3 things you notice about the phase diagram

Phase Diagram What do A, B, and C represent?

Critical point The point at which the boundary between two phases ceases to exist No distinction between liquid and gas

Triple Point The point where either state of matter is possible. Any slight change will determine which state of matter is present.

Phase Diagrams What would the phase of carbon dioxide be at temperature 250 K and pressure 100 bars?

Phase Diagrams What state(s) of matter can exist at 250K?

You Try! Construct a temperature vs. energy plot based on the given information. Starting at 0 Joules, energy is added to a substance at a constant rate until 500 Joules have been added. The temperature of the substance increases from -10oC to 110oC. The melting point occurs at 5oC and the boiling point occurs at 85oC. Once your plot is finished label areas related to the heat of fusion and the heat of vaporization.

Energy vs. Temp Diagram

Plasmas A gas that is made up of highly energized, positively and negatively charged ions. Neon sign Stars Lightning Grapes in a microwave. https://www.youtube.com/watch?v=RwTjsRt0Fzo

Liquid crystals Turn and Talk: what is a liquid crystal?

Liquid crystals  a state of matter that has properties between those of a liquid, but particles are arranged like that of a solid crystal. Computer screen Soaps  

Do Now! Dry ice is frozen carbon dioxide that goes from a solid state straight to a gas state. 1. Name the phase transition. 2. Is the phase transition endothermic or exothermic? How do you know?

Physical Properties observed or measured without changing the composition of matter Ex: Boiling point, brittleness, mass, etc

Chemical Properties Properties of matter that deal with the chemical makeup or interactions with other matter. Ex. Flammability corrosive pH

Physical vs. Chemical properties

COPPER Physical Properties: Dense (8.96 g/mL) Heavy (63.55 g/mol) High boiling point (2562 °C)

EXAMPLE: Chemical Properties Which of these is a chemical property of hydrogen gas? a. Has a molar mass of 2.02 g/mol b. Reacts easily with oxygen c. Melting point is -434.5 °F d. Found in planets and stars

Physical Vs. Chemical change Physical Change: Changes the physical form of the substance, but NOT the chemical makeup. Chemical Change: Changes the chemical make-up/properties of a substance.

5 signs of a chemical change: Color change Formation of a solid Odor Production Production of energy (sound, light, heat) Formation of a gas (bubbles)

Physical Change Most commonly phase changes, or dissolving in water.

Physical Change or chemical change? Dry ice sublimes when exposed to normal, atmospheric conditionsIron metal is melted Iron combines with oxygen to form rust Kool-Aid dissolves in water Copper in Statue of Liberty changes from golden orange color to blue-green

Practice Determine if the following are Phys/Chem Properties. The boiling point of ethyl alcohol is 78 °C Diamond is very hard. Sugar ferments to form ethyl alcohol A block of aluminum has a mass of 56g.

Warm Up! 1. Physical changes are usually ___________ changes. 2. List 3 of the 5 ways you can tell that a chemical reaction has taken place

BELL RINGER! Which is more dense? Ice or water? Why or how do you know?

Density (ρ) A physical property that defines a substance Density is defined as mass (grams) per unit volume (mL or cm3) D= m/v 1mL = 1 cm3 Density of water= 1g/mL

D=m/v

Density In a solution, more dense component will be on bottom of less dense ← Least Dense Vinegar Oil ← Most Dense

Density https://www.youtube.com/watch?v=zlkpZZW29b0

Let’s Practice! Take out a calculator! Worksheet due tomorrow!

BELL RINGER! Think! What happens when you put red hot nickel into water? Describe what will happen. https://www.youtube.com/watch?v=l3LOhYRY59Y

What happened? Why did the water not start boiling right away? Think about energy transfer!

What will happen when you put a red hot ball of nickel into a bowl of Jell-O?’ https://www.youtube.com/watch?v=OkiJFRS9Zsw

Specific Heat Used to define a substance Amount of energy needed to change the temperature of 1g, 1°C. Stated another way: how easily something changes temperature. Used frequently to determine the heat lost/gained Water→4.184 J/g °C Aluminum→ 0.902 J/g °C Q = m · C · ΔT

Specific heat triangle

Practice: if 1,000 joules of energy were added to each of the substances below, which would have the highest change in temperature?     Metal Specific Heat   a. Beryllium 1.82 J/g•°C b. calcium 0.653 J/g•°C c. copper 0.385 J/g•°C d. gold 0.129 J/g•°C

If a substance changes temperature from 65 degrees Celsius to 35 degrees Celsius, calculate the change in temp.

Law of Conservation of Energy Energy is neither created nor destroyed in a closed system In an insulated system, heat lost by one substance is gained by the other -Q = Q -mm C mΔTm = mw C wΔTw

Let’s Practice!!!!

Do you remember this?

Do you remember this? State Particles Picture Shape (fixed or variable) Volume (fixed or variable) IMF (strong or weak) Solid Liquid Gas

Solid Gas Liquid

Do you remember this? Endothermic vs. exothermic? Plasma and liquid crystals?

Do you remember this? Lab instruments?

Phase Diagram What do A, B, and C represent?

Do you remember this? Physical vs. chemical changes? What changes are physical? How can you tell that a chemical change has occurred? (there are 5)

Density? Sink or float? Equation?