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While you wait……. . • Find your assigned seat • Take out your notebook,

While you wait……. . • Find your assigned seat • Take out your notebook, a pen or pencil and a calculator • In your notebook title this unit properties of matter

Our plan for today…. • Introduction to properties of matter • Density mini lab

Our plan for today…. • Introduction to properties of matter • Density mini lab • Complete POGIL classification of matter activity

PROPERTIES OF MATTER Describing Matter

PROPERTIES OF MATTER Describing Matter

Learning Targets • Distinguish between pure substance and mixtures based on the characteristic properties

Learning Targets • Distinguish between pure substance and mixtures based on the characteristic properties of the substance and describe how you could use these properties to separate the mixture or pure substance into its components. •

How would you describe yourself so that someone else could identify you? • On

How would you describe yourself so that someone else could identify you? • On a separate sheet of paper, write as many physical descriptions of yourself as you can. Do not put your name on the paper.

Matter and its composition

Matter and its composition

Physical Properties • A property of matter that can be observed or measured without

Physical Properties • A property of matter that can be observed or measured without changing the identity of the matter. • Physical properties identify matter. • Examples include but are not limited to: • • • Density Malleability Ductility Solubility State Thermal Conductivity

Physical Properties • Density • Amount of mass in a given volume • A

Physical Properties • Density • Amount of mass in a given volume • A substance is always the same at a given pressure and temperature regardless of the size of the sample of the substance. • The density of one substance is usually different from that of another substance. • Density equals mass divided by volume. • D=m/v

Practice • A bar of copper has a mass of 216 g and a

Practice • A bar of copper has a mass of 216 g and a volume of 24 cmᴲ. • What is the density of copper?

More Practice • An ice cube has a volume of 36 cmᴲ. If the

More Practice • An ice cube has a volume of 36 cmᴲ. If the ice cube has a mass of 33. 2 g, what is the density of the ice cube? • What is the density of water? 1 g/cm³

Density Mini Lab • You are to design a way to determine unknown metals

Density Mini Lab • You are to design a way to determine unknown metals using the density formula. • You may use a graduated cylinder, an electronic balance and water

How did you determine? Data Table Sample Mass (g) Volume of water + (ml)

How did you determine? Data Table Sample Mass (g) Volume of water + (ml) sample (ml) Volume of sample (ml) Density (g/ml) Data and Observations

Metal Density (g/cm 3) Aluminum 2. 699 Chromium 7. 13 Copper 8. 89 Gold

Metal Density (g/cm 3) Aluminum 2. 699 Chromium 7. 13 Copper 8. 89 Gold 19. 33 Iron 7. 86 Lead 11. 347 Magnesium 1. 738 Mercury 13. 596 Nickel 8. 85 Osmium 22. 5 Potassium 0. 87 Silver 10. 6 Tin 7. 184 zinc 7. 19

Physical Property • Malleability • The ability to be pounded into thin sheets. •

Physical Property • Malleability • The ability to be pounded into thin sheets. • Example: • Aluminum can be rolled or pounded into sheets to make foil. • Ductility • The ability to be drawn or pulled into a wire • Example • Copper in wiring – soldering wires or joints

Physical Property • Solubility • The ability to dissolve in another substance. • Example:

Physical Property • Solubility • The ability to dissolve in another substance. • Example: • Sugar or salt dissolve in water • Three ways to increase solubility • Heat or make warmer • Grind or smash • Stir or mix

Physical Property • Thermal Conductivity • The ability to transfer thermal energy from one

Physical Property • Thermal Conductivity • The ability to transfer thermal energy from one area to another. • Examples: • Plastic foam is a poor conductor, so a hot drink won’t burn your hand. • The inside of the toaster (hot coils)

While you wait……. . • Find your assigned seat • Take out your notebook,

While you wait……. . • Find your assigned seat • Take out your notebook, and a pen or pencil • Pick up Captured chemicals lab

Physical Property • State of Matter • The physical form in which a substance

Physical Property • State of Matter • The physical form in which a substance exists at room temperature, such as: • Solid – matter has a definite shape and volume • Liquid – matter takes the shape of its container and has a definite volume • Gas – matter changes in both shape and volume

STATES OF MATTER SOLIDS • Particles of solids are tightly packed, vibrating about a

STATES OF MATTER SOLIDS • Particles of solids are tightly packed, vibrating about a fixed position. • Solids have a definite shape and a definite volume. Heat

STATES OF MATTER LIQUID § Particles of liquids are tightly packed, but are far

STATES OF MATTER LIQUID § Particles of liquids are tightly packed, but are far enough apart to slide over one another. § Liquids have an indefinite shape and a definite volume. Heat

STATES OF MATTER GAS § Particles of gases are very far apart and move

STATES OF MATTER GAS § Particles of gases are very far apart and move freely. § Gases have an indefinite shape and an indefinite volume. Heat

Chemical Property • A property of matter that describes a substance based on its

Chemical Property • A property of matter that describes a substance based on its ability to change into a new substance with different properties. • Combustibility • Flammability • Reactivity • Acids • Bases • Oxidation

Chemical Properties q Can be observed with your senses. q Are Not as easy

Chemical Properties q Can be observed with your senses. q Are Not as easy to observe as physical properties q. Example: q Flammability – Only when wood burns q Combustibility – Only when fireworks explode q Reactivity – Only when iron Oxidizes (rust)

Physical Change • A change that affects one or more physical properties of a

Physical Change • A change that affects one or more physical properties of a substance. • Do Not form new substances. • Can often be Undone • Example Butter on counter can be placed back in refrigerator. • Change of State • Solid to Liquid • Liquid to Gas

Chemical Change • A change that occurs when one or more substances are changed

Chemical Change • A change that occurs when one or more substances are changed into entirely new substances with different properties. • Can Not change back under normal conditions (some can be changed back by other chemical means) • Common Examples: • • Reactivity – Oxidation (rust) on a bicycle p. H (Acid / Base) – Effervescent tablets Flammability – Burnt wood Combustibility - Fireworks

5 Signs of a Chemical Change • The only sure way to know there

5 Signs of a Chemical Change • The only sure way to know there has been a chemical change is the observance of a new substance formed • Sometimes that is hard to do, so look for the signs…….

Sign 1 a Chemical Change • Odor Production-this is an odor far different from

Sign 1 a Chemical Change • Odor Production-this is an odor far different from what it should smell like • Ex: Rotting eggs, food in fridge, decomposing flesh

2 nd Sign of a Chemical Change • Change in Temperature • Exothermic-When energy

2 nd Sign of a Chemical Change • Change in Temperature • Exothermic-When energy is released do during the chemical change ex: wood burning

Change in Temperature • Endothermic- Energy is absorbed causing a decrease in temperature of

Change in Temperature • Endothermic- Energy is absorbed causing a decrease in temperature of the reactant material ex: cold pack in first aid kit

3 rd Sign of a Chemical Change in Color Ex: fruit changing color when

3 rd Sign of a Chemical Change in Color Ex: fruit changing color when it ripens, leaves changing color in the Autumn, dying your hair

4 th sign of a Chemical Change • Formation of Bubbles • This can

4 th sign of a Chemical Change • Formation of Bubbles • This can indicate the presence of a gas. Bubbles produced when boiling water is not a chemical change.

5 th Sign of a Chemical Change • Formation of a Precipitate • When

5 th Sign of a Chemical Change • Formation of a Precipitate • When two liquids are combined and a solid is produced

Captured Chemicals Lab Chemical vs. Physical changes Safety • Gloves • Goggles • Phones

Captured Chemicals Lab Chemical vs. Physical changes Safety • Gloves • Goggles • Phones are put away • Read instructions carefully

Exit Discussion • What are some of the chemical changes that you observed in

Exit Discussion • What are some of the chemical changes that you observed in the lab? • What combinations of chemicals are responsible for those changes

Exit Ticket • An unknown metal has a density. 8. 19 cm 3 and

Exit Ticket • An unknown metal has a density. 8. 19 cm 3 and a mass of 25 g, what is the volume? • A block of ice has a volume of 3. 14 cm 3 and a mass of 11. 4 g, what is the density • What is the difference between a physical and chemical property?