1. Do Now: Solve the following using the correct number of significant figures. 1)7.76 m + 2.1 m = 2)5.750 cg - 1.1 cg = 3)5555 kg + 444 kg = 4)1.23 m x 3.2 m = 5)6.9 mm / 3 mm =

2. YWBAT Explain how Democritus and John Dalton described atoms

3. History of Atomic Theory http://ed.ted.com/lessons/the-2-400-year- search-for-the-atom-theresa-doud

4. Do Now: 1.What models have you used? 2.What other models are you aware of? 3.Why do people use models?

5. YWBAT Explain how Democritus and John Dalton described atoms Identify instruments used to observe atoms. Identify three types of subatomic particles. Describe the structure of atoms according to the Rutherford atomic model.

6. Democritus Greek philosopher (460– 370BC) Among the first to suggest the existence of atoms. atomos – Greek word for indivisible Reasoned that atoms were indivisible and indestructible.

7. Dalton English chemist & school teacher 1766 – 1864 Used experimental methods to transform Democritus’ ideas into scientific theory Studied ratios in which elements combine in chemical reactions.

8. Dalton’s Atomic Theory 1.All elements are composed of tiny indivisible particles called atoms. Atoms of element A

9. Dalton’s Atomic Theory 2. Atoms of the same element are identical. The atoms of any one element are different from those of any other element. Atoms of element A Atoms of element B

10. Dalton’s Atomic Theory 3. Atoms of different elements can physically mix together or can chemically combine in simple whole-number ratios to form compounds. Mixture of atoms of elements A and B

11. Dalton’s Atomic Theory 4. Chemical reactions occur when atoms are separated from each other, joined, or rearranged in different combinations. Atoms of one element are never changed into atoms of another element as a result of a chemical reaction. Compound made by chemically combining atoms of elements A and B

12. Dalton’s Atomic Theory Do you think all parts of Dalton’s Atomic Theory are still believed to be true today?

13. Sizing Up The Atom A pure copper coin the size of a penny contains about 2.4 x 10 22 atoms 24,000,000,000,000,000,000,000 atoms * Note – Earth’s population is ~ 7 x 10 9 people

14. Sizing Up The Atom Individual atoms are observable with a Scanning Electron Microscope (SEM). SEMPollen grains

15. Structure of the Atom

16. What is in the box?

17. Subatomic Particles 1.Protons 2.Neutrons 3.Electrons

18. Electrons In 1897, physicist J.J. Thomson discovered the electron. Electrons are negatively charged subatomic particles https://www.youtube.com/watch?v=Rb6MguN0 Uj4

19. Protons In 1886, Eugene Goldstein observed a cathode ray tube and found rays traveling in the direction opposite to that of the cathode ray tubes. – He concluded they were composed of positive particles. – These positively charged subatomic particles are called protons

20. Neutrons In 1932, James Chadwick confirmed the existence of the neutron. – Neutrons are subatomic particles with no charge but with a mass nearly equal to that of a proton.

21. Subatomic Particles

22. How are these three subatomic particles (protons, neutrons, and electrons) put together in an atom?

23. Plum Pudding Model Thompson’s atomic model Electron’s stuck in a lump of positive charge, similar to raisins stuck in dough.

24. Rutherford’s Gold Foil Experiment In 1911, Ernest Rutherford, a former student of Thomson’s, tested the plum- pudding model. A narrow beam of alpha particles was directed at a very thin sheet of gold

25. Rutherford’s Gold Foil Experiment Most alpha particles went straight through, or were slightly deflected. A small fraction of the alpha particles bounced off the gold foil at very large angles.

26. Rutherford’s Atomic Model The Nuclear Atom Rutherford suggested a new theory of the atom based on the experimental results. – The atom is mostly empty space. – All the positive charge and amost all of the mass are concentrated in a small positively charged region (nucleus) – Protons & neutrons are in the positively charged nucleus – Electrons are distributed around the nucleus and occupy almost all the volume of the atom.

27. Rutherford’s Atomic Model The Nuclear Atom If an atom were the size of a football stadium, the nucleus would be the size of a marble.