Chemistry The Science of Matter Pages 4-9 in the text

Do Now List at least 5 chemicals that you are familiar with from past experience.

Learning Objective Understand composition and their impact on the properties of matter Be able to classify chemical vs. physical changes

Chemistry The science that investigates the structure and properties of matter Matter: anything that takes up space and has mass Mass: the measure of the amount of matter that an object contains NOT Matter- Heat Light Radio waves etc.

Matter continued Structure: refers to what it is made of and of how it is organized Properties: Describe the characteristics and behavior of matter including the changes it undergoes

Behavior of Matter Determined by BOTH The elements it contains Arrangement of those elements

Example Salt vs. Water Sodium and Chloride Hydrogen and Oxygen Contain different elements --- Have different properties!

Example Aspirin Vs Table Sugar Both contain only Carbon, Hydrogen and Oxygen molecules --- same composition Different Structures Cause Different Behaviors!

Example Two Different Artificial Sweeteners Aspartame Saccharine Different Compositions Both have: C, H, O and N and are sweet Only Saccharine has Na+ and S Their arrangement must be a factor!

Identifying Properties Many are easy to observe by simple tests Use heat, magnets, electricity etc Color State: solid, liquid or gas at room temp and pressure Soft or hard Does it burn? Does it dissolve in water? These are from a macroscopic perspective Things you can touch, taste, feel, smell and see

What is it made of? This question is harder to answer Must take measurements Must observe chemical changes Macroscopic Observations Submicroscopic perspective To understand hidden structure influences behavior

Physical change vs. Chemical change Doesn't change what the substance is. A new substance is formed and energy is either given off or absorbed. Can be reversed Cannot be reversed with the substance changed back without extraordinary means, if at all.

Examples Physical Change Chemical Change Paper cut into pieces, small pieces are still paper Paper burned is no longer paper Dissolve sugar in water Make a cake with flour, water, sugar and other ingredients and bake them, it would take extraordinary means to separate the various ingredients out to their original form.

Physical Vs. Chemical Change Worksheet (10 minutes) In pairs complete the given handout You may use your notes Be sure that you are prepared to share your answers with the class

Share Answers (3 min/group) Each table shares their answers with the class. Be sure to explain why you chose your answer. ALL STUDENTS MUST RECORD THE CORRECT ANSWER ON THEIR HANDOUT!

Thanks for doing your best work! Exit Ticket – Answer individually Write your name! Please number your index card 1-5 List 5 different properties of matter which can be used to identify a substance. Define Chemical change Define physical change List 3 examples of a chemical change List 3 examples of a physical change. PLACE YOUR EXIT TICKET IN THE TRAY ON YOUR WAY OUT! Thanks for doing your best work!

Chemical properties vs. Physical properties Chemical Property • Flammability: The ability to burn • Ability to rust: Reacts with oxygen to produce rust • Reactivity with vinegar: Reacts with vinegar to produce new substances Physical Property • Transparency: The property of letting light pass through something • Boiling point: Temperature at which a substance goes from liquid to gas • Melting point: Temperature at which a substance goes from solid to a liquid • Brittleness: Tendency to crack or break • Ductility: Ability to bend without breaking • Elasticity: Ability to be stretched or compressed then return to original size • Density: Mass per unit volume

Let’s look closely at Density It is an important property of matter It is used to identify substances It is also used to separate mixtures Definition of Density: the mass of a specific unit of volume It is expressed in the following equation; D= m/v or density = mass volume

Density In solids it is usually expressed as; grams per cubic meter g/cm3 Kilograms per cubic meter Kg/m3 In liquids it is usually expressed as; grams per liter g/L grams per cubic centimeter

Example of Density Calculations If a piece of rock has a mass of 14g and a volume of 5 cm3, what is the density? Step 1: Write the given and ensure proper units m =14 g V= 5 cm3 Step 2: Write the formula D= m/v Step 3: Substitute the given into the formula D = 14g / 5 cm3 Step 4: solve D=2.8 g/cm3

Your turn to work! Alone, Silently Read the first 2 pages (4 min) Highlight or underline any concepts which we have already mentioned as important, in ppt. Circle any new information Use a sticky note to write out any questions you have

Now you try some problems! Work with your partner to answer questions for practice exercise 1 and 3 (10 min) You may use a calculator Write out all steps Label all units Be prepared to put your answer on the board!

Review answers

Submicroscopic Level of Matter Matter is made of Atoms Atoms So small they can not be seen with the most powerful light microscope So small that if a period at the end of a sentence were made of Carbon atoms it would be made of 100 quintillion carbon atoms (100, 000,000,000,000,000,000) Counting them at 3 per second would take you a trillion years! Scanning Tunneling Microscope (STM) creates computer images which are a visible perspective showing atomic location

Scanning Tunneling Microscope (STM) individual iron atoms on a silver substrate

Using Chemical Models Show types and numbers of atoms Show arrangement of the atoms and space filled

Why Models? Submicroscopic structural representation Explains observed behavior Used to predict behavior not yet observed Built on investigation and experimentation

Show Connections Between Atoms

Classifying Matter Substance: matter with constant composition Element: Made of only one type of atom Compound: 2 or more elements that are chemically combined Mixture: Matter with variable composition Heterogeneous Mixture: Made up of more than 1 phase Homogeneous Mixture: also called solutions, made up of only 1 phase

Mixtures A material that is made of 2 or more things which are not combined chemically Each of the parts still keep their own identities Made by blending, but NOT forming chemical bonds or chemical change! Most everyday matter occurs as mixtures

Heterogeneous and Homogeneous Mixtures A classification of matter based on composition Homogeneous mixture: no clumping or grouping but rather a uniform dispersal of the material it is made of. Ex. Air; made of N2, O2, CO2 and other gases A liquid in which there is a solvent and a solute is called a solution Heterogeneous mixture: it is easy to identify all if the different components

Heterogeneous mixture

Heterogeneous mixture

Colloids (look homogeneous but microscopically heterogenous) Hair spray Smoke Cloud Whipped cream Shaving cream Blood Styrofoam Gello

Dispersion (Heterogeneous) Dust Milk Hand cream Gravel Granite Sponge

Homogeneous Mixtures

Solutions (homogeneous) Air (gas) Martini (liquid) Salt water (liquid) Plastic (solid)

Substances Homogeneous materials that contain only 1 kind of matter Have definite composition and properties Substances which can not be broken down into a simpler substance is an ELEMENT. Substances which can be broken down into a simpler substance is a COMPOUND. They are made of 2 or more elements

Elements Made of only one kind of atom Can not be made simplified by physical or chemical means Can exist as atoms (carbon) or molecules (N2)

Compounds Consist of 2 or more DIFFERENT atoms bound together (H2O) Can be broken down into smaller types of matter by chemical means only. Have properties which are different than the elements they are made of Always contain the same ratio of its components atoms ( ex 2 hydrogen's to 1 oxygen, in water)

Classify the Following Ocean water- Calcium- Vitamin C- Dry ice – Copper- Grain alcohol- after shave lotion- Hamburger- Al foil – Milk- Salt- Iron nail-

Answers Ocean water- solution Calcium- element Vitamin C- Compound ( L-asorbic acid) Dry ice – compound (CO2) Copper- element Grain alcohol- compound (C2H5OH) after shave lotion- heterogenous mixture Hamburger- hetero Al foil – element Milk- solution Salt- cmpd Iron nail- element

Learning Objectives Investigate various ways to separate mixtures Identify the properties of the matter that allow for a particular method of separation

REMEMBER Mixtures Are made of 2 or more things which are not combined chemically Each of the parts still keep their own identities Made by blending, but NOT forming chemical bonds or chemical change! Most everyday matter occurs as mixtures

Separating Mixtures Mixtures can be separated through a physical process, (the identity of the substance remains unchanged). Using their Physical properties Bringing about physical changes to separate the mixture into its components (different substances it is made of)

REMEMBER: Physical Properties Density: Mass per unit volume Solubility in water : Does it dissolve in water? State of mater: at room temp and pressure Transparency: lets light pass through Boiling point: Temperature at which a substance goes from liquid to gas Melting point: Temperature at which a substance goes from solid to a liquid Brittleness: Tendency to crack or break Ductility: Ability to bend without breaking Elasticity: Ability to be stretched or compressed then return to original size

Making a Mixture AND SAND SUGAR

The Mixture

How can we separate it? What do you think? Work with your lab partner to come up with a suggested method. (10 minutes) You may use your class notes, but your brain is your best asset. Write your thoughts in your notebooks. Do not be afraid to try!

Report out on ideas So, what did you come up with? Share your thoughts! (10 minutes)

What can we do? Method #1 Use a pair of tweezers and a microscope to physically separate the particles Requires a lot of time and patience

Method #2 Step #1 Recall the properties of water and of sand Sugar dissolves in water Sand does NOT Use the difference! Method #2

Step #2 Recall the properties again sand will not pass through a filter Sugar and water solution will Use the difference!

Step #3 Recall the properties of sugar and water water will ! sugar will not evaporate (change state) at 100 degrees Celsius water will ! Use the difference! Step #4

You have the two pure substances again! Sand in the filter! Sugar in the bottom of the beaker!

Learning objective Understand the relationship between chemical change and energy change

Mixtures vs. Pure substances Mixtures can be separated based physical properties and through physical change Pure substances can only be separated through chemical changes Separated from compounds into elements H2O- H and O2 Made into compounds from elements H + O  H2O

Chemical Change and Energy All chemical changes involve some sort of energy change! Many chemical changes (reactions) release energy Exothermic reactions: release energy as heat Some reactions absorb energy Endothermic reactions: absorb heat energy

Epsom salt and laundry detergent Demo Epsom salt and laundry detergent

Lab Thursday! Paper Chromatography! A method of separating mixtures based on their ability to dissolve or on the size of particles.

More methods of separating mixtures Paper chromatography Separating the dyes in ink Dyes are usually made of several basic colors called pigments Using the property of these dyes Soluble in water we will separate the pigments

Develop a question! Make a claim (hypothesis) Follow the Procedure Answer the lab analysis questions Draw a conclusion Ask a new question Create a poster presentation of your results

Be sure to study your notes and your review sheets! Unit Test on Monday! Be sure to study your notes and your review sheets!