1. The Atom

2. The atom has three parts: 1) P rotons 2) N eutrons 3) E lectrons

3. Protons Protons: Protons: 1) Found in the nucleus 2) Mass: one (1) Atomic Mass Unit 3) have a (+) positive charge, 1 P ROTON = 1 P OSITIVE Charge 1 P ROTON = 1 P OSITIVE Charge

4. Protons (Cont’d) On the periodic table, each element is numbered. This number equals the number of Protons in the nucleus. On the periodic table, each element is numbered. This number equals the number of Protons in the nucleus.

5. Neutrons Also found in the nucleus. Also found in the nucleus. Mass: one (1) Atomic Mass Unit. Mass: one (1) Atomic Mass Unit. They have NO charge. Neutron = Neutral They have NO charge. Neutron = Neutral

6. Electrons Found around the nucleus (like planets around the Sun) An Electron’s mass is almost nothing…almost Have a negative (-) charge ELECTRONS = NEGATIVE

7. Standard Atomic Notation Be 9 4 Mass Number = mass of all the protons and neutrons in the nucleus Atomic Number = number of protons in the nucleus and the number of electrons orbiting the nucleus Element Symbol – eg. Beryllium To find the number of neutrons in the nucleus, subtract atomic number from mass number. There would be 9 – 4 or 5 neutrons in a Beryllium atom

8. Remember The periodic table is organized by atomic number (the number of protons the element has in its nucleus) The periodic table is organized by atomic number (the number of protons the element has in its nucleus) Protons are + and electrons are - Protons are + and electrons are - The number of protons = the number of electrons (positives = negatives) The number of protons = the number of electrons (positives = negatives)

9. Let’s try some! Have your periodic table ready Have your periodic table ready How many protons, neutrons and electrons in one atom of: How many protons, neutrons and electrons in one atom of: Hydrogen? Hydrogen? Carbon? Carbon? Beryllium? Beryllium? Calcium? Calcium? Fluorine? Fluorine? 1 p+, 1 e-, 0 n 20 p+, 20 e-, 20 n 6 p+, 6 e-, 6 n 4 p+, 4 e-, 5 n 9 p+, 9 e-, 10 n

10. Bohr-Rutherford Diagrams Named after the work done by Neils Bohr and Ernest Rutherford (nobody before them gets any respect!) Named after the work done by Neils Bohr and Ernest Rutherford (nobody before them gets any respect!) Flattened model of the inside of an atom Flattened model of the inside of an atom Unique for each atom Unique for each atom

11. Electron Shells First Shell, maximum 2 electrons

12. 2 elements in first row (period) Why only 2 in the first shell?

13. Electron Shells Second Shell, Maximum 8 electrons

14. Why 8 in the second shell? 8 elements in second period

15. Electron Shells Third shell, max # 8 electrons Note: Magnesium only needs 2 electrons in this shell because it has 12 total

16. Bohr-Rutherford Diagrams Eg. Magnesium

17. Guess this element 82 protons = element 82 which is LEAD 82 protons = element 82 which is LEAD

18. The Noble Gases Column to the far right of the periodic table, He, Ne, Ar, Kr, Xe, & Rn

19. So, how would Magnesium look like Neon? MagnesiumNeon

20. So, if Mg lost two Electrons, but still had the same number of Protons, what is its Charge? +2

21. Charges The outer electrons on an atom are called: Valence electrons. The outer electrons on an atom are called: Valence electrons. Atoms want a Bohr-Rutherford Diagram that look like the Noble Gases because… Atoms want a Bohr-Rutherford Diagram that look like the Noble Gases because… have the most stable structure have the most stable structure Won’t react when mixed Won’t react when mixed Usually, this means the atom ends up with a Charge. Usually, this means the atom ends up with a Charge.

22. Fluorine What does F need to look like a Noble gas? If we add one Electron, what will the Charge of the atom be? - 1

23. Ions Ion= a Charged atom in which the number of ELECTRONS (-) is different from the number of PROTONS (+). Ion= a Charged atom in which the number of ELECTRONS (-) is different from the number of PROTONS (+). Ionic Charge= is the number of positive (+) or negative (-) Charges on an atom. Ex: Mg +2 Ionic Charge= is the number of positive (+) or negative (-) Charges on an atom. Ex: Mg +2

24. Groups MgBe (Berylium)

25. So… Even though each element has a different # of PROTONS and ELECTRONS, each element in a group has a similar Bohr- Rutherford Diagram Even though each element has a different # of PROTONS and ELECTRONS, each element in a group has a similar Bohr- Rutherford Diagram This means they want to gain or lose the same number of Electrons. This means they want to gain or lose the same number of Electrons. It also means elements in a Group will react similarly in Chemical Reactions It also means elements in a Group will react similarly in Chemical Reactions