1. Ch. 8 Earth Chemistry

2. Properties Physical properties: boiling point, melting point, color, luster, density, electrical conductivity, magnetism Chemical properties: how a substance will interact with another substance (reactive, unreactive)

3. What do we know about matter?

4. What do we know about an atom?

5. Experiments that led to the discovery of subatomic Particles Rutherford’s Gold foil experiment Question posed: How will a tiny particle pass through closely packed atoms? – Took an element: pure gold – Shoot a alpha particle at the gold (helium nucleus:2 protons – 2 neutrons)

6. Rutherford’s Hypothesis: If the mass of the atom was distributed evenly throughout the atom, then there would be very little to deflect the alpha particles as they passed through the atom. Rutherford’s Result: Most alpha particles went straight through the gold foil but a small amount were deflected at great angles!

7. Atomic Structure Atom 1.Protons (+ Charge) 2.Neutron (Neutral) 3.Electrons ( - Charge)

8. Atomic Structure Atom 1.Protons (+ Charge) 2.Neutron (Neutral) 3.Electrons ( - Charge) Nucleus

9. Atomic Number The number of protons in an element Identifies the element

10. In an uncharged atom, # protons = # electrons

11. What is the atomic number of Carbon? How many protons does carbon have? How many electrons does carbon have?

12. Mass number Represents the protons and neutrons found in an atom of an element Why aren’t electrons included in the mass number?

13. What defines an atom as one type of element instead of another???? In other words, what makes one atom a Carbon and the next atom Nitrogen?

14. What if the number of protons in an atom stays the same but I add or remove neutrons….. What would change about that atom?

15. Isotopes Elements that have the same number of protons but different number of electrons

16. The periodic table organizes atoms with similar chemical properties in columns The similar properties of atoms in these groups are due to the number of electrons in their outer most electron orbital

17. Valence Electrons The electrons in the outer most electron orbital What pattern do you notice about the number of valence electrons for the elements in each column?

18. Chemical Bonds Ionic Bonds – electron transfers result in charged atoms called ions – Ions with opposite charges attract forming an ionic compound

19. Ionic Bond Example

20. Predicting typical charges of ions formed

21. How do ions form? How are positive ions formed? How are negative ions formed?

22. Predicting formulas for ionic compounds If one ion has a +2 charge, and the other has a -1 charge, how many of each ion would you need for your charges to balance in your final molecule? +2

23. Predicting formulas for ionic compounds If one ion has a +2 charge, and the other has a -1 charge, how many of each ion would you need for your charges to balance in your final molecule? +2

24. Predicting formulas for ionic compounds If one ion has a +2 charge, and the other has a -1 charge, how many of each ion would you need for your charges to balance in your final molecule? Mg 2+ and Cl - MgCl 2 +2

25. Covalent Bond - attraction between atoms that share electrons – Occurs between 2 or more nonmetals Example: Carbon dioxide CO 2

26. Chemical Formulas Show the scientist the amount of each element in a particular chemical Example: Water Chemical Formula: H 2 O – There are 2 hydrogen and 1 oxygen in every water molecule

27. Mixtures Parts keep their individual properties Can be separated by physical means – Solution: one substance is evenly dispersed in another Example: Ocean Water (Water & Salt) – Alloy: 2 or more metals