1. D ECEMBER 2, 2014 Objective: To calculate the numbers of protons, neutrons, and electrons in an atom using the periodic table Describe the structure of at atom Journal: What do you study in chemistry?

2. C HEMISTRY – A TOMS

3. A TOMS The smallest particle into which an element can be divided and still be the same substance All living things are made of atoms

4. S UBATOMIC P ARTICLES Protons: Positively charged Located in the nucleus Neutrons: No charge (neutral) Located in the nucleus Electrons: Negatively charged Located in the electron cloud (orbitals)

5. E LECTRON C ONFIGURATION The location within the electron cloud where the electrons are most likely to be found 1 st shell holds maximum of 2 electrons All other shells hold a maximum of 8 electrons

6. A TOMIC S TRUCTURE

7. P ERIODIC T ABLE

8. E LEMENTS ON THE P ERIODIC T ABLE

9. A TOMIC N UMBER Biggest size number in each box when looking at the periodic table Atomic Number = Number of Protons = Number of Electrons

10. A TOMIC W EIGHT The total number of protons and neutrons added together Small number underneath the symbol when looking at the periodic table

11. H OW TO FIND NUMBERS OF … Number of protons = Atomic Number Number of electrons = Atomic Number Number of neutrons = Atomic Weight – Atomic Number *Round atomic weight to the nearest whole number before subtracting

12. N OVEMBER 18, 2013 Objective: To describe how atoms bond together to form compounds using valence electrons Journal: How many protons, neutrons and electrons are in gold?

13. B ONDING TO M AKE C OMPOUNDS

14. M OLECULE A group of atoms held together by covalent bonds

15. C OMPOUND A substance composed of two or more elements that are combined

16. V ALANCE E LECTRONS The number of electrons in the outer shell. Used for bonding

17. O CTET R ULE When bonding, each atom wants to have a full outer shell (8 valance electrons) ***Exception is Hydrogen, which can only hold two electrons in its outer shell

18. T YPES OF B ONDING Covalent Bonding Ionic Bonding Hydrogen Bonding

19. C OVALENT B ONDS When bonds form between atoms by sharing valence electrons

20. I ONIC B ONDS When bonds form between atoms by either gaining or losing electrons Results in the compound having either a positive or negative charge

21. I ONS When an atom has an electrical charge it is called an ion If an atom gains an electron it has a negative charge If an atom loses an electron it has a positive charge

22. P OLARITY When shared electrons are attracted to one atom more strongly than another, so it has a slightly negative charge The other atom that the electrons are less strongly attracted to has a slightly positive charge

23. S OLUBILITY Like dissolves like Substances with like charges will dissolve one another, but substances with opposite charges will not

24. H YDROGEN B OND When a hydrogen atom has a partial positive charge that is very strong it attracts to the negative pole of specific other molecules Oxygen, Nitrogen, Fluorine This is a very strong bond, but not as strong as a covalent bond.