1. Elemenets, Compounds and Mixtures

2. GPS
S8P1 b. Describe the difference between pure substances (elements and compounds) and mixtures.

3. Matter can be classified as elements, compounds, or mixtures.
Matter can be classified as elements, compounds, or mixtures.
Elements and compounds are examples of pure substances.

4. Pure Substances
A substance in which there is only one type of particle.
Each element contains only one type of particle and these particles are called atoms.

5. Element
An Element is a substance that cannot be broken down into any other substances by chemical or physical means.
There over 100 known elements.
All matter is made up of elements.

6. 92 Elements are found in nature
The other 17 are made by scientists under special laboratory conditions.
Most elements are solids at room temperature.

7. Elements that are gasses: Oxygen, hydrogen, and nitrogen.
Examples of solid elements: iron, tin, lead, silver, gold, calcium, and copper.
Elements that are gasses: Oxygen, hydrogen, and nitrogen.

8. Some types of matter are made up of only one element.
Examples: iron nail only contains the element iron.
Aluminum foil is made up of only the element aluminum.

9. Physical Properties of Elements
Physical property can be observed or measures without changing the matter’s identity.
Each element can be identified by its unique set of properties.

10. Boiling point
Melting point
Density
Malleability
Ductility
State of matter

12. Chemical Properties
Chemical properties describe matter based on it ability to change into new matter that has different properties.
Reactivity with i.e. acid, oxygen
Flammability

13. Compound
Other substances are made up of more than one element and are known as compounds.
Examples:
Water – hydrogen and oxygen
Table salt – sodium and chlorine
Sugar – carbon, oxygen, and hydrogen

14. Compound
A Compound is a pure substance made of two or more elements chemically combined.
Basically, a compound is formed as a result of a chemical change.
Examples: H2O, H2SO4 (Sulfuric acid)

15. Compounds and Earth
Most of the matter making up the earth is composed of compounds.
Sugar is a compound – it is made up of carbon, hydrogen, and oxygen.
Table salt – sodium and chlorine.

16. Formula
A formula is a combination of symbols that shows the ratio of elements in a compound.
Example: C9H8O4 otherwise known as aspirin
C12H22O11 – Sugar!

17. Water is a familiar compound
Water is a familiar compound. Water is made up of two elements – hydrogen and oxygen. The chemical formula is H2O.
The 2 in the formula is a subscript. It tells the number of atoms of that element. So Hydrogen has how many atoms? How many oxygen?

18. FYI
The suffix “–ide” is often used in chemistry to form the names of compounds
Example: Iron Sulfide – iron and sulfur
Sodium Chloride – table salt

19. Mixture
A mixture consists of two or more substances that are in the same place together but are not chemically combined into a new substance.
Example: Garden soil

20. Types of Mixtures
A homogeneous mixture has the same uniform appearance and composition throughout. Many homogeneous mixtures are commonly referred to as solutions.
A heterogeneous mixture consists of visibly different substances or phases. The three phases or states of matter are gas, liquid, and solid.

21. Examples Air Vinegar Blood plasma Sugar water
Salt in water (dissolved)
Sand in water
Trail mix
Vinegar in oil
Milk
Chicken Soup

22. Mixture A solution is a type of mixture.
Individual components are mixed evenly throughout the mixture.
Example: saltwater

23. What is a Solution?
A solution is a mixture that appears to be a single substance.
At least two substances must be mixed in order to have a solution.
The SOLUTE is the substance being dissolved.
The SOLVENT is the substance in which the solute is dissolved.

25. Solubility
If you add too much sugar to a glass of lemonade, not all of the sugar can dissolve. Some of it sinks to the bottom. To find the maximum amount of sugar that can dissolve, you would need to know the solubility of sugar.
Solubility of a solute is the ability of the solute to dissolve in the solvent under certain conditions: temperature of the solution, chemical nature of the solvent and volume of the solvent.

26. Temperature
Solubility of a salt in a liquid increases with an increasing temperature.
Solubility of a gas in a liquid increases with decreasing temperature.

27. More solvent volume means more solute can dissolve.
Volumne
More solvent volume means more solute can dissolve.

28. Solubility Value
Mass of solute that can dissolve in a mass or volume of solvent at a certain temperature.

29. Definitions
SUPERSATURATED SOLUTIONS contain more solute than is possible to be dissolved
Supersaturated solutions are unstable. The supersaturation is only temporary, and usually accomplished in one of two ways:
Warm the solvent so that it will dissolve more, then cool the solution
Evaporate some of the solvent carefully so that the solute does not solidify and come out of solution.

30. Solubility curve
Saturated
Supersaturated
Unsaturated

31. Solubility curve Any point on a line represents a saturated solution.
In a saturated solution, the solvent contains the maximum amount of solute.
Example
At 90oC, 40 g of NaCl(s) in 100g H2O(l) represent a saturated solution.

32. Solubility curve
Any point below a line represents an unsaturated solution.
In an unsaturated solution, the solvent contains less than the maximum amount of solute.
Example
At 90oC, 30 g of NaCl(s) in 100g H2O(l) represent an unsaturated solution. 10 g of NaCl(s) have to be added to make the solution saturated.

33. Solubility curve
Any point above a line represents a supersaturated solution.
In a supersaturated solution, the solvent contains more than the maximum amount of solute. A supersaturated solution is very unstable and the amount in excess can precipitate or crystallize.
Example
At 90oC, 50 g of NaCl(s) in 100g H2O(l) represent a supersaturated solution. Eventually, 10 g of NaCl(s) will precipitate.

34. How are Mixtures and Compounds Different?
Mixtures are:
Made of two or more substances mixed together
Substances keep their own properties
Can be separated by physical means
Have no definite chemical composition

35. Compounds are… Made of two or more substances chemically combined
Substances lose their own properties
Can be separated only by chemical means
Have a definite chemical composition

36. Infer
When a certain poisonous gas is combined with a flammable metal, a fine white powder results. The powder is neither flammable nor poisonous. Is the powder a mixture or a compound? How do you know?

37. Answer
Compound
The substances lost their properties.