1. Unit 3 Matter Organization and Changes Chapters 3, 4, and 5

2. Idea of the Atom Democritus (BC) –Had the original idea that all matter was made of a small ‘invisible’ units –Called these atoms Dalton (1800’s) –Proposed his theory of matter and the atom –Widely accepted because of his evidence

3. Dalton’s Atomic Theory Every element is made of tiny, unique particles that cannot be divided Atoms of the same element are exactly alike Atoms of different elements can join to form molecules

4. Current Atomic Model Atoms can be divided –Protons Positive charged –Electrons Negative charged –Neutrons No charge Call these subatomic particles

5. Current Atomic Model Nucleus Has protons and neutrons in it Electrons are around the nucleus Number of Protons = Number of Electrons Tells us the atom is neutral (no charge)

6. Describing the Atom Mass Number –Number of protons added to the number of neutrons protons neutrons 9+9= 18

7. Mass Number Also known as the Atomic Mass Can be found on the periodic table

8. Describing the Atom Atomic Number –Number of protons in the atom –Found on the periodic table

9. Isotopes Atoms of the same element that have a different number of neutrons Changes the mass number of the element Hydrogen has three isotopes –Hydrogen-1, Hydrogen-2, and Hydrogen-3 Mass number

10. Critical Thinking If Dalton were still alive, he might argue: “Atoms are neutral so they can’t be made of charged particles.” Explain why this is not true.

11. Periodic Table Periods Groups

12. Periodic Table Activity 1.Elements in the group 2.Where the group is located on the periodic table 3.Chemical properties of the elements in the group 4.Physical properties of elements in the group 5.Types of elements in the group (metals, nonmetals, metalloids) 6.Interesting facts about the elements in the group Each person picks one element. Need to find how that element relates to human life. (Is it important in nutrition? Does it make something we use everyday? Etc.)

13. Bohr’s Addition to the Atom Electrons circle the nucleus like planets orbit the sun Electrons can only orbit in set energy levels –The further the orbit is from the nucleus, the more energy it has

14. Bohr’s Atomic Model Nucleus Energy Level 1 Energy Level 3 Energy Level 4 Energy Level 2

15. Bohr’s Atomic Model Number of electrons in the energy level furthest from the nucleus are the valence electrons Nitrogen has seven electrons. How many valence electrons are there? 2 electrons in energy level 1 5 electrons in energy level 2 Highest energy level

16. Periodic Table

17. Happy Atoms Atoms are happy when they are stable Atoms are stable when they have a full outer energy level –Outer energy level has 8 valence electrons

18. Ions Atom that has lost or gained an electron Causes a change in the charge of the atom

19. Ions Lithium atom Charge = neutral Lithium ion Charge = 1+ Neutron Proton Electron

20. Ions Fluorine atom Charge = neutral Fluorine ion Charge = 1- Neutron Proton Electron

21. Ions Chlorine – adds 1 electron Sodium – takes away 1 electron Calcium – takes away 2 electrons Sulfur – adds 2 electrons Aluminum – takes away 3 electrons Nitrogen – adds 3 electrons Charge 1- 1+ 2+ 2- 3+ 3-

22. Compounds Held together by chemical bonds –Force holding the atoms of the elements together Three types of chemical bonds –Ionic –Covalent –Metallic

23. Structure and Properties The stronger the bond – the stronger the structure The stronger the bond – the higher the boiling point The stronger the bond – the higher the melting point The stronger the bond - the more solid the substance

24. Breaking Chemical Bonds Chemical bonds can be broken –Requires energy to break the bond The stronger the bond - the more energy needed to break it Chemical bonds are broken during chemical reactions

25. Forming Chemical Bonds Chemical bonds can be formed –Requires energy to form the bonds The stronger the bond - the more energy needed to form it Chemical bonds are formed during chemical reactions

26. Chemical Reactions Na+Cl 2 NaCl Reactants Products Chemical reactions rearrange atoms! Reacts in the beginning Produced at the end

27. Chemical Reactions Energy is transferred during chemical reactions Energy exists in many forms –Light –Sound –Electricity –Heat

28. Reaction Rates How fast or slow a reaction happens is affected by –Temperature –Pressure –Surface area –Concentration –Size and shape –Catalyst

29. Reaction Rates Temperature –Increase temperature = increase reaction rate –Potato cooks faster in hot water than cold Pressure –Increase pressure = increase reaction rate –Coal burns faster at higher pressure Surface area –Increase surface area = increase reaction rate –Cut potato cooks faster than uncut

30. Reaction Rates Concentration –Higher concentration = increase reaction rate –More bleach causes lighter color Size and shape –Smaller size = increase reaction rate –Large piece of zinc reacts slower than a small Catalyst –If it is present = increase reaction rate –Add protease to digest protein