1. Protons, Neutrons, and Electrons

2. Subatomic Particle ChargeLocationRelative Mass ElectronNegativeOutside Nucleus Very Small ProtonPositiveInside Nucleus Large NeutronNeutralInside Nucleus Large

5. Protons = Atomic Number Electrons = Atomic Number in Neutral Atom Neutrons = Atomic Mass- Atomic Number Should make sense because all of the mass is inside the nucleus, so the mass minus the protons leaves the neutrons.

6. Protons? Neutrons? Electrons?

10. Short Hand Writing of Elements

12. Rules For Atom Building You must fill the S’s before the P’s You must fill the P’s before the D’s Once you have the board filled with the right amount of marbles you need to record it on your paper. You will also start doing electron configuration. We will do an example when you go to stations

15. Isotopes Isotopes – atoms of the same element that have the same atomic number (same protons) but different atomic masses due to different number of neutrons. Same Protons Different Neutrons Ex. Chlorine 37

17. Ions An atom or group of atoms that has a positive or negative charge, cations are positive, anions are negative. If an ion has a positive charge that means it LOST ELECTRONS If an ion has a negative charge that means it gained electrons Only about addition or subtraction of electrons.

18. Example: Carbon Ions What are the protons, neutrons, and electrons of each?