1. Matter and Energy
Applied Chemistry

2. Matter and Energy The universe is made of matter and energy. Energy
Definition: The capacity to do work or produce heat.
Common unit: calorie abbreviated cal
SI unit: Joule abbreviated J

3. Types of Energy
Radiant Energy is energy transferred through waves without matter.
Ex. Sunlight
Kinetic Energy is energy of motion.
Walking, Running, Water flowing
Potential Energy is energy of position or stored energy.
Ball at the top of a hill, battery

4. Potential and Kinetic Energy

5. Forms of Energy Mechanical, Heat, Chemical, Electrical, Radiant, Sound, Nuclear

6. Law of Conservation of Energy
Energy is neither created nor destroyed.
Energy can change from one form to another.

7. Matter Definition: anything that has mass and volume.
States of matter:
Solid s
Liquid l
Gas g
Plasma

8. Identification Table Name Shape Volume Density Solid Definite Liquid
Indefinite
Gas
Plasma

9. Matter Change is state is also known as a phase change.
Temperature vs. Heat Animation

10. States of Matter Solid Liquid Gas deposition melting sublimation
freezing
condensing
vaporizing
Liquid
Gas

11. Properties or Characteristics of Matter
A physical property is a property observed or measured without changing the material.
Example: color, density, shape, melting point, boiling point
A chemical property is a property that refers to the ability of a material to undergo a change that alters its structure.
Examples: flammability, light sensitivity

12. Changes in Matter All changes involve a change in energy.
Physical changes: Do NOT change the identity of a substance.
Ex) size, shape, state, and dissolving
Chemical changes: Do change the identity of a substance.
Ex) burning, digesting food, rusting

13. Signs of a chemical change
Change in color
Formation of a precipitate (cloudiness; solid formed from 2 solutions)
Production of a gas (bubbles; fizzing)
Increase or decrease in temperature
Change or production of an odor

14. iron + oxygen  rust (iron(II) oxide)
Chemical Equations
a shorthand way to write a chemical change (reaction)
Starting materials are called reactants
Newly formed materials are called products
Reactants products
iron oxygen  rust (iron(II) oxide)
yields

15. Law of Conservation of Matter
Matter is neither created nor destroyed. It only changes FORM.
Shown by the French chemist Antoine Lavoisier in the 1700s. He is known as the Father of Chemistry.
mass of reactants = mass of products

16. Classification of Matter

17. Elements Contain only 1 type of atom.
Cannot be broken down by ordinary means. (physical or chemical)
Ancient Greeks believed there were only 4 elements. (earth, air, fire, and water)
92 naturally occurring elements. Others are short-lived, man-made elements.

18. Elements
A symbol is a shorthand way of writing the name of an element.
Represents 1 atom of an element.
Consists of 1 or 2 letters.
1st letter is ALWAYS capitalized.
Subsequent letter is lower case.
3-letter symbols are temporary designations assigned by IUPAC.

19. Elements
Using your periodic table, find the symbols for the following elements:
Hydrogen
Helium
Carbon
Chlorine
The number of elements as a solid, liquid, or gas at room temperature.
2 liquids
11 gases
Others are solids H He C Cl

20. Compounds
Contain 2 or more DIFFERENT elements that are chemically combined.
Can be broken down by chemical processes, such as heat and electricity.
Smallest part of a compound is a molecule.

21. Compounds
A formula is a shorthand way of writing the name of a compound. It shows…
Which elements are present
The ratio of the elements present.

22. Examples of Formulas
H2O: the 2 is called a subscript that tells you that 2 atoms of hydrogen combine with 1 atom of oxygen to form 1 molecule of water.
3H2O is read as 3 molecules of water. The 3 is called the coefficient. There are 6 hydrogen atoms and 3 oxygen atoms

23. Identify the following substances as elements or compounds.
Co Element
CS Compound
CO Compound
Mg Element
Note: If two capital letters are present, it is a compound.

24. Counting Atoms in Compound
Step 1: List all elements present
Step 2: Identify the coefficient
Step 3: Count the number of atoms of each element in the compound.
Step 4: Multiply the coefficient by the subscript
Step 5: Add up all the atoms

25. Counting Atoms
Na2SO4 7 atoms
Ca(OH)2 5 atoms
3 Fe2(SO3)3 42 atoms

26. Pure Substances

27. Mixtures
Mixtures contain elements or compounds that are mixed together but not chemically joined.
Types of Mixtures
Homogeneous Mixture or Solution
Heterogeneous Mixture or Mechanical Mixture

28. Homogeneous Mixtures Uniform throughout Not visibly different
Examples:
Gasoline
Food coloring
14 carat gold (alloy)
Air
Brass (alloy)
lemonade

29. Brass is an alloy of copper and zinc.
Examples of Alloys
Brass is an alloy of copper and zinc.
Steel is an alloy of carbon and iron.
Bronze is an alloy of copper and tin.

30. Heterogeneous Mixtures
Not uniform throughout
Visibly different
Examples:
Oil & vinegar
Salad
Concrete
Vegetable Soup
Sand and water

31. Homogeneous vs. Heterogeneous Mixtures

32. Separation of Heterogeneous Mixtures: Filtration
Separate suspended particles from a clear liquid by pouring through a screen, filter, or porous substance.
Filtrate: the liquid that passes through the filter
Residue: the solid left on the filter
Examples: car filter, pool filter

33. Filtration

34. Separation of Heterogeneous Mixtures: Magnetic Method & Decanting
Separate magnetic substances from nonmagnetic substances.
Examples: iron filings and sulfur
recycling center
Decanting
Separate liquids due to a difference in density
Example: oil from water

35. Heterogeneous liquids can be decanted.

36. Decanting Diagram

37. Separation of Homogeneous Mixtures: Chromotography
Separate pigments of ink using strips of paper.
Remember Pete Cheat Lab
Examples: dyes and chlorophyll

38. Chromatography

39. Separation of Homogeneous Mixtures: Distillation
Separate solution by a difference in boiling point. The liquids will vaporize and then condense back to a liquid.
Ex. Salt water, crude oil
Distillation Demo
A Closer Look at Distillation

40. Distillation

41. Separation of Homogeneous Mixtures: Crystallization
Separate a solution by evaporating the liquid and the solid will recrystallize.
Examples: rock candy, salt water

42. Crystallization