1. What is Matter and what are the Basics?

2. Atom:
The basic particle of an element.

3. NUCLEUS - the center or core of an atom, where the protons and neutrons are located
PROTONS - the positively charged particles in an atom
NEUTRONS - the neutral particles in an atom
ELECTRONS - the negatively charged particles in an atom
VALENCE ELECTRONS - electrons that are involved in transfer or sharing

4. Element:
A pure substance that cannot be broken down into any other substance by chemical or physical means.

5. Atomic Mass: The atomic mass of an element is the sum of the number of protons AND neutrons. (unit “amu”)
For example, carbon has six protons. One isotope of carbon also has 6 neutrons. This means that its atomic mass is 12, or 6 protons + 6 neutrons.
Another isotope of carbon has 8 neutrons. This means that its atomic mass would be 14, or 6 protons + 8 neutrons.

6. Atomic Number:
The number above the symbol, 17, is the element's atomic number. The atomic number of an element is the number of protons in each atom of that element. For example, every atom of chlorine has 17 protons. Its atomic number is 17.

7. I knew how to observe and then infer!
The Periodic Table
In 1869 Dmitri Mendeleev ( ) succeeded in organizing the 62 elements known at that time into a system of rows and columns on the basis of increasing mass and similar chemical and physical properties. Since the organization exhibited a periodic repetition of similar properties, it became known as the Periodic Table of the Elements. It has become one of modern chemistry's most useful resources.
Mendeleev: figured out the beginnings of the Periodic Table! (Russian)

8. Periods: the horizontal rows of the P. Table. There are 7
Periods: the horizontal rows of the P. Table. There are 7. As you move from left to right, properties of the elements change according to a pattern.
Groups: Also known as families, the 18 vertical rows The elements in each group have similar characteristics.
Each family of the periodic table has its own characteristic properties based on its number of valence electrons.

9. Isotope: elements having the same # of protons, BUT different numbers of neutrons…
In this case each isotope has one proton but a different number of neutrons

10. Radioactive isotopes: an atom that has a nucleus that gives off radiation because it is not “stable” These isotopes are used in medicine as they are traceable as they travel through your body.

12. Molecule:
Groups of two or more atoms held together by chemical bonds.
Chemical bond:
Force of attraction between two atoms.

13. Compound: A pure substance made of two or more elements chemically combined in a set ratio.
Why is the bucky ball not a compound?

14. COVALENT BOND - a chemical bond formed when two atoms share electrons.

15. IONIC BOND - the attraction between two oppositely charged ions.
ION - an atom or group of atoms that has become electrically charged.

16. Another way of looking at “Bonds”

17. Chemical Reaction: A reaction in which new substances are formed.

18. Chemical reactions occur when chemical bonds break or when new bonds form.
2 H2 + O2   -->   2 H2O
                                                
Reactants Products
reaction

19. What does this diagram tell you about C, H, O, N?

20. 1808 - John Dalton - ATOMIC THEORY (England)
                                                                                             
                                                                                             
John Dalton - ATOMIC THEORY (England)
1.       Atoms can’t be broken into smaller pieces
2.       Atoms of different elements are different
3.       Atoms of two or more elements can be combined to form compounds
4.       Atoms of each element have a unique mass
5.       The masses of the elements in a compound are always in a constant ratio