1 / 35

I. Classification of Matter

I. Classification of Matter. MATTER (anything that has mass & takes up space). MATTER . PURE SUBSTANCE (matter with a definite composition) Ex- water, helium, carbon dioxide, sodium. MATTER . MIXTURE (2 or more pure substances combined in ANY ratio)

ulmer
Download Presentation

I. Classification of Matter

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

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

  11. 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

  12. Distillation Demo:

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

  14. Can dissolve in water (Soluble in water) E.__________________________________

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

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

  17. the amount of solute in a solution 3. concentration - _________________________ _____________________________________ 4. Diluted solution - _______________________ ______________________________________ 5. Concentrated 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

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

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

  20. 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

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

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

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

  24. Demonstration – Super Saturated Solution:

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

  26. What is the title of this graph? • What is the x-axis label? • What is the x-axis unit of measurement? • What is the y-axis label? • What is the y-axis unit of measurement? • What is the general trend expressed by this graph?

  27. SUPERSATURATED- anything above the line SATURATED - anything on the line UNSATURATED- anything under the line

  28. What is the temperature of a saturated solution of 36 g / 100 g of water? • What is the solubility of BaCl2 at 60 C? • 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?

  29. 4. How would you create a supersaturated solution?

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

  31. Which salt is the most soluble at 70 C? • Which salt’s solubility is least affected by temperature? • Which salt’s solubility is most affected by temperature?

More Related