Presentation is loading. Please wait.

Presentation is loading. Please wait.

I. Classification of Matter MATTER (anything that has mass & takes up space)

Similar presentations

Presentation on theme: "I. Classification of Matter MATTER (anything that has mass & takes up space)"— Presentation transcript:

1 I. Classification of Matter MATTER (anything that has mass & takes up space)

2 MATTER PURE SUBSTANCE (matter with a definite composition) Ex- water, helium, carbon dioxide, sodium

3 MATTER MIXTURE (2 or more pure substances combined in ANY ratio) Ex- lemonade, concrete, shaving cream

4 Pure Substances COMPOUND (2 or more elements chemically bonded together) Ex- sodium chloride, water, glucose, CLUE- chemical formulas have 2 capital letters; it is NOT on the periodic table

5 Pure Substances ELEMENT (cannot be broken down any further) Ex- carbon, oxygen, lithium, hydrogen CLUE- It is any substance written on the periodic table

6 Mixtures SOLUTION (a homogeneous mixture that cannot be filtered & will NEVER settle upon standing)homogeneous Ex- saline solution, grape juice CLUE- It is clear (might be clear & colored)

7 Mixtures COLLOIDAL SUSPENSION (a homogeneous mixture that cannot be filtered & will EVENTUALLY settle upon standing) Ex- mayo, milk, fog, cool whip CLUE- it creates the Tyndall EffectTyndall Effect

8 Mixtures COURSE SUSPENSION (a heterogeneous mixture that can be filtered & will QUICKLY settle upon standing) Ex- Italian Dressing, OJ CLUE- it has distinguishable “pieces” in it.

9 SOLUTION ALLOY (a special type of solution where 2 or more METALS mix together----a “metallic solution”) Ex- brass (zinc & copper); pewter (tin & lead); steel (iron & carbon) CLUE- It is NOT on the periodic table

10 VOCABULARY HELP: Homogeneous: ___________________________ ________________________________________ when a material appears the SAME throughout

11 Heterogeneous: __________________________ ________________________________________ When a material appears to be DIFFERENT throughout

12 Tyndall Effect: ___________________________ _______________________________________ Real Life Examples: the effect of light scattering on particles in a colloid that makes it appear to be cloudy under the light. (even though it might look clear otherwise) -Fog -The reason we see the sky as blue

13 Mixture Demonstrations: Watch the following demos to describe different mixtures. One of each type of mixture (solution, colloid, & course suspension) will be demonstrated. Pick at least one of each type of mixture and write/draw it to describe what happened. LABEL the demo as an example of either a solution, colloid or course suspension & GIVE YOUR PROOF. Type of Mixture DemonstrationProof COLLOID SOLUTION COARSE SUSPENSION

14 II. Physical Properties of matter that we will use to help us separate a solution? A. ___________________________ Magnetism Demonstration – Magnetism:

15 B. ___________________________ C. ____________________________ 1. Lab techniques that uses phase change separation. a. ____________________________ ____________________________ ___________________________ Density Phase Changes Distillation – uses different boiling points of the pure substances involved to separate and CAPTURE all of the substances of the mixture

16 Distillation Demo:

17 b. ______________________ D. ___________________________ 1. Lab techniques that use particle size separation. a. ____________________________ ____________________________ Crystallization – separation technique that uses the boiling point to capture ONLY the substance with the HIGHEST boiling point Particle Size Filtering – using a screen or paper to help retain the larger items, while the smaller pass through





22 E.__________________________________Can dissolve in water (Soluble in water)

23 III. Characteristics of Solutions A. Parts of a Solution Solvent – the substance doing the dissolving Solute – the substance being dissolved

24 B. Terms related to solutions: 1. Soluble -___________________________ _________________________________ ex – 2. Insoluble - _________________________ __________________________________ ex - Able to dissolve in each other Salt is soluble in water NOT able to dissolve in each other Water is insoluble in water

25 3. concentration - _________________________ _____________________________________ 4. Diluted solution - _______________________ ______________________________________ 5. Concentrated solution - __________________ ______________________________________ the amount of solute in a solution when you add more solvent to a solution in order to decrease the overall concentration when you remove solvent from a solution in order INCREASE the overall concentration

26 C. Rate of solution: 1. Definition: ________________________ ________________________________ the speed at which a solvent is able to dissolve a solute

27 2. Ways to increase the speed at which the solvent dissolves the solute. a. _____________________________ Demo: b. _____________________________ Demo: c. _____________________________ Demo: Increase temperature Increase surface area Stir or Shake

28 D. How do You Describe The Amount of Solute in a Solution? 1. Definition of each: a. Unsaturated- _____________________ ________________________________ Does not have all of the solute that it could at a given temperature

29 i. if you add one more piece of _____________ to an unsaturated solution, it will _______________ into the beaker of solution. solute dissolve

30 b. Saturated - ____________________________ _____________________________________ i. if you add one more piece of _____________ to a saturated solution, it will __________________ in the beaker. Has all of the solute that it can at a given temperature solute Stay as a crystal

31 c. supersaturated - _______________________ ____________________________________ i. if you add one more piece of _____________ to a super-saturated solution, it will __________________ in the beaker. Has more solute than it SHOULD at a given temperature solute crystalize

32 Demonstration – Super Saturated Solution:

33 E. Solubility and Solubility Curves 1. Solubility - __________________________ ___________________________________ 2. Solubility Curve – __________________________ ________________________________________ The total amount of solute necessary to make a saturated solution at a GIVEN TEMPERATURE a graph that illustrates the solubility of given solutes in certain solvents

34 1.What is the title of this graph? 2.What is the x-axis label? 3.What is the x-axis unit of measurement? 4.What is the y-axis label? 5.What is the y-axis unit of measurement? 6.What is the general trend expressed by this graph?

35 UNSATURATED- anything under the line SUPERSATURATED- anything above the line SATURATED - anything on the line

36 1.What is the temperature of a saturated solution of 36 g / 100 g of water? 2.What is the solubility of BaCl2 at 60 C? 3.If a solution has 40 g of BaCl2 dissolved in 100 g of water and it is at 70 C, how would you characterize it?

37 4. How would you create a supersaturated solution?

38 c. Common trend between temperature and heat i. as temperature __________________, solubility _________________. increases

39 1.Which salt is the most soluble at 70 C? 2.Which salt’s solubility is least affected by temperature? 3.Which salt’s solubility is most affected by temperature?

Download ppt "I. Classification of Matter MATTER (anything that has mass & takes up space)"

Similar presentations

Ads by Google