1. Essential objectives: Describe the difference between ions and isotopes. Compare the major types of chemical bonds and how do they differ.

2. UNIT 2 MINERALS Minerals form raw materials manufactured products. Aluminum, graphite, copper, talc, silver, gold, gemstones, and silicon.

3. Malachite: Ore of copper and a gemstone.

4. Quartz: Source of silicon used in making computer chips

5. Galena: Ore of lead

6. Gemstones!

7. 1.States of Matter. a.Solids- atoms/molecules organized fixed structures/defined shape. Atoms limited vibration. b.Liquids fluid mixtures atoms/molecules existing charged atoms/molecules form ions. Form loose associations through brief electronic bonds. Liquid no fixed structures. c.Gases fluid atoms/molecules rapid motion, freely moving no fixed structure. Gases expand to fill available space.

8. Elements: Different types atoms that, in pure form, cannot be divided into smaller units without changing their properties. Atom: Smallest division of element, that still possesses chemical properties unique to element. Compounds: 2 or more atoms bonded together. Composed of atoms of same element, or combinations of several different elements.

9. Nucleus contains: Protons = Particles mass of 1.0 positive electrical charge. Neutrons = mass of1.0 neutral electrical charge. electrons electrons Orbiting the nucleus are electrons having essentially no mass and a negative charge. A single atom neutrons protons

10. Number of protons in nucleus of element atomic number. Elements are distinguished from each other by their atomic number. nucleus Model of one atom Examples: All Helium atoms have 2 protons “ Carbon “ “ 6 “ “ Uranium “ “ 92 “

11. 2. Atomic mass # protons plus # neutrons. Most elements have different versions differ slightly in mass because they have different # neutrons in nucleus, isotopes. Many isotopes are unstable, disintegrate through radioactive decay – particles and/or energy are emitted from the nucleus. Ex. Carbon 14

12. l# protons determines type of atom 6 protons = carbon l# neutrons in atoms can vary. l# neutrons + # protons = atomic “mass”. lHere are the three isotopes of Carbon: 6 protons & 6 neutrons: mass number = 12 6 protons & 7 neutrons: mass number = 13 6 protons & 8 neutrons: mass number = 14 13 C 12 C 14 C How we write it Carbon example:

13. equals # of protons

14. 3. When atoms gain or lose electrons they take on an electrical charge- an ion. Atoms with + charge are cations. Atoms with - charge are anions. 4. Compounds are made /combining different elements.

15. 5. Minerals- naturally occurring compounds classification by their chemical composition /internal (atomic) structure. Characteristic – naturally occurring, inorganic, solid, possess an orderly internal structure, and have a defined chemical composition.

16. Quartz contains: silicon (Si) and silicon (Si) and oxygen (O) oxygen (O) element name symbol Example: Quartz Chemical formula for quartz is: SiO 2

17. F Atomic Bonding Bonding between atoms! 3 main ways: “Ionic bonding” - loaning electrons “Covalent bonding” - sharing electrons “Metallic bonding” - electrons free to move about from atom to atom

18. Sharing Electrons: Covalent Bonding Shared electrons Nucleus

19. Example: Table Salt: Sodium (Na) and Chlorine (Cl) Sodium gives up an electron becoming a positively-charged charged cation. Chlorine picks up the electron from Sodium taking becoming a negatively charged anion.

20. Example: Sodium (Na) and Chlorine (Cl) Atoms arrange in orderly fashion: w/ alternating sodium and chlorine atoms, so each negative ion is surrounded by positive ions, and visa versa.