1. Introduction The structure of matter- 2. What is matter?
2. Any object or substance that has mass and takes up space.

2. 3. What are atoms?
Atoms are tiny particles that make up all matter AND the smallest particle of an element.
4. Describe the nucleus.
Interesting fact: the smallest nucleus is located in a light hydrogen atom; the largest- uranium.
The nucleus is at the center of the atom. The nucleus contains neutrons and protons. The nucleus spins.

4. 5. What are protons?
5. Protons have a positive electric charge, have a mass of 1, and how many protons determine the element.
6. What are neutrons?
6. Neutrons have no electric charge and have a mass of 1; located in the nucleus.

5. 7. What are electrons?
7. Electrons have a negative electric charge; have a mass of almost 0; electrons fly around the nucleus almost at the speed of light when in orbit.

6. Let’s Review

7. 8. What are ions?
8. Ions are atoms with an extra or missing electron. When ions have a ( an):
extra electron, the charge is negative
A missing electron , the charge is positive
Remember that normal atoms have the same number of electrons and protons

8. 9. What are elements?
9. Elements are substances made from just one kind of an atom.
There are 90 different types of elements in nature.
More than 20 elements are man made.

9. There are 90 different types of elements in nature.
Element Discussion
There are 90 different types of elements in nature.
More than 20 elements are man made.
It it is important to remember that when looking at the periodic table of the elements, “naturally occurring” does not necessarily mean “abundant.” Many naturally occurring elements are in fact quite rare, although some were once more abundant. Levels of elements also change depending on where you are: helium. For example, is rare on Earth, but abundant around the Sun.

10. the structure of matter
Write 3
to 4 sentences
About what you learned
about
the structure of matter

11. 10. What is the Periodic Table of Elements?
10. The periodic table is an arrangement of elements according to their atomic numbers.

15. 11. An atomic number is the number of PROTONS in the nucleus.
11. What is an atomic number?
11. An atomic number is the number of PROTONS in the nucleus.

16. 26 Fe
Iron
55.845

17. A hydrocarbon ( this atom is natural gas)
12. What is a chemical symbol?
12. The first letter is always an upper case and the others are lower case. letter is always upper case and others are lower case
A hydrocarbon ( this atom is natural gas)

18. 14. Non metals are located on the right and metals on the left.
13 What is atomic mass?
13.Atomic mass is:
Protons + Neutrons
14. How are metals and non metals arranged on the Periodic Table?
14. Non metals are located on the right and metals on the left.

20. 15. Ionic bonds are formed by the attraction between
15. What are ionic bonds?
15. Ionic bonds are formed
by the attraction between
two oppositely charged
ions.
Usually occurs between positive metals and negative nonmetals.
Common example: table salt

22. 16. Covalent bonds are bonds in which atoms share electrons.
16. What are covalent bonds?
16. Covalent bonds are bonds in which atoms share electrons.
H2O is an example

23. 17.What is
a molecule?
17. A molecule is formed when two or more atoms join together chemically.
Methane gas

24. Sulfuric Acid Molecule : Contains sulfur, Hydrogen, and Oxygen

25. 17. What is a compound?
17. A compound is made of two or more elements that are chemically combined.

26. Good conductors of electricity
18. What are characteristics of metallic bonds?
18.High boiling points
Good conductors of electricity
Requires much energy to break apart ( usually)

27. How many carbon atoms? Hydrogen atoms? Oxygen atoms?
19. What is a formula?
19. A formula lists how many of each element that makes up a compound.
H2O = 2 Atoms of Hydrogen and 1 atom of Oxygen
C6H12O6 = glucose
How many carbon atoms? Hydrogen atoms? Oxygen atoms?

28. 20. Mixtures are combinations of substances that are NOT bonded.
20 What are mixtures?
20. Mixtures are combinations of substances that are NOT bonded.

29. 21. What Is a heterogeneous mixture?
21 A MIXTURE is a combination of two or more substances that are not chemically united and do not exist in fixed proportions to each other. Most natural substances are mixtures.
If broken apart, could the parts be seen separately
( raisins, oats, etc)

30. 22. What Is a homogeneous mixture?
22. Homogeneous mixture is when substances are mixed evenly throughout the solution. *Many homogeneous mixtures are commonly referred to as solutions.

31. What is a mixture?

32. 23. What are the parts of a solution?
23. Parts of a solution include:
solute – substance being dissolved
solvent – substance in which the solute dissolves

33. Draw the difference between a
heterogeneous and homogeneous solution; Draw the difference between a solvent and a solute.

34. Unit 4 – Properties and Changes

35. 1.What are physical properties?
1. Physical properties are observed through the senses.

36. 2. Examples of Physical changes
Color, shape, hardness, texture, etc.
Density – amount of matter in a given volume
Buoyancy – ability to float in water
Ductility – ability to be stretched, bent, etc. without breaking
Solubility – amount that will dissolve in another substance

37. The Hindenburg Disaster

38. 4. Acids form hydrogen ions when dissolved in water
3. What are the characteristics of acids?
3. Acids:
corrode metals
taste sour
pH of 1-6 (7 is neutral)
4. What is the relationship between acids and water?
4. Acids form hydrogen ions when dissolved in water

41. 5. What are the characteristics of bases?
feel slippery
taste bitter
react with fats (good for
soap)
pH of 8-14

42. 6. What is the relationship between bases and water?
6. Bases form hydroxide ions when dissolved in water (also called alkaline)

44. 7. Acids and bases…………
7. React to form salt and water.
8. PH SCALE 8.

45. 9. What are physical changes?
9. Physical changes do not change one substance to another ( i.e. bending, breaking)

47. 10. List the states or phases of matter.
10. Solid:
has definite shape and volume; particles vibrate without moving around
Liquid :
has definite volume but not shape; particles are touching and move freely
Gas:
has no definite volume or shape ;particles are far apart and move very rapidly
Plasma:
superhot charged particles; stars
Bose-Einstein Condensate – super cold and super dense solid

50. 11What is melting?
11. Melting occurs when solids forms liquids.
12. What is evaporation ?
12. Evaporation occurs when liquids develop into gases.

51. 13. Condensation occurs when gases form into liquids.
13. What is condensation?
13. Condensation occurs when gases form into liquids.

52. 14. Freezing occurs when – liquids become solids
14. What is freezing?
14. Freezing occurs when – liquids become solids

53. 15. Sublimation occurs when solid forms into gas (skips liquid)
15. What is sublimation?
15. Sublimation occurs when solid forms into gas (skips liquid)

54. 16. Deposition occurs when gases form into a solid
16. What is deposition?
16. Deposition occurs when gases form into a solid

58. 19. 19. Describe chemical reactions. Law of Conservation of Matter :
Chemicals react to form different chemicals
All reactions either release energy or absorb energy
Law of Conservation of Matter :
matter cannot be created or destroyed
whatever matter goes in must
come out