1. Chapter 3 Atoms : The Building Blocks of Matter

2. Foundations of Atomic Theory  Several basic laws were after the 1790’s (emphasis on quantitative analysis): Lavosier:  Law of conservation of mass  Law of conservation of mass : mass is neither created nor destroyed during ordinary chemical or physical processes. (Only re-arranged)  Mass of Reactants = Mass of Products  Law of conservation of energy  Law of conservation of energy : energy is neither created nor destroyed during ordinary chemical or physical processes. (Only changed from one form to another form)  Several basic laws were after the 1790’s (emphasis on quantitative analysis): Lavosier:  Law of conservation of mass  Law of conservation of mass : mass is neither created nor destroyed during ordinary chemical or physical processes. (Only re-arranged)  Mass of Reactants = Mass of Products  Law of conservation of energy  Law of conservation of energy : energy is neither created nor destroyed during ordinary chemical or physical processes. (Only changed from one form to another form)

3. Foundations of Atomic Theory Cont… Proust:  Law of definite proportions: chemical compounds contain the same elements in exactly the same proportions by mass regardless of the size of the sample.  Ex. NaCl always is composed of 39.34% sodium and 60.66% chlorine by mass. Proust:  Law of definite proportions: chemical compounds contain the same elements in exactly the same proportions by mass regardless of the size of the sample.  Ex. NaCl always is composed of 39.34% sodium and 60.66% chlorine by mass.

4. Foundations of Atomic Theory Cont…  Law of multiple proportions  Law of multiple proportions: if two or more different compounds are composed of the same 2 elements, the ratio of mass of the second element combined with a certain mass of the first is always a ratio of small whole numbers.  Ex. CO and CO 2 : For the same mass of carbon, the mass of the O in CO to the mass of O in CO 2 will be 1:2  Law of multiple proportions  Law of multiple proportions: if two or more different compounds are composed of the same 2 elements, the ratio of mass of the second element combined with a certain mass of the first is always a ratio of small whole numbers.  Ex. CO and CO 2 : For the same mass of carbon, the mass of the O in CO to the mass of O in CO 2 will be 1:2

5. Development of Atomic Models  John Dalton (1808): 1. All matter is composed of extremely small particles called atoms (cannot be subdivided, created, nor destroyed) 2. Atoms of the same element are identical; atoms of different elements are different 3. Atoms combine in simple whole number ratios to form compounds 4. In chemical reactions, atoms combine, separate, or are rearranged.  John Dalton (1808): 1. All matter is composed of extremely small particles called atoms (cannot be subdivided, created, nor destroyed) 2. Atoms of the same element are identical; atoms of different elements are different 3. Atoms combine in simple whole number ratios to form compounds 4. In chemical reactions, atoms combine, separate, or are rearranged.

6. Dalton’s Model of the Atom Because of Dalton’s atomic theory, most scientists in the 1800s believed that the atom was like a tiny solid ball that could not be broken up into parts. * small*indivisible *dense*uniform (same throughout) Like a steel ball-bearing or marble. Because of Dalton’s atomic theory, most scientists in the 1800s believed that the atom was like a tiny solid ball that could not be broken up into parts. * small*indivisible *dense*uniform (same throughout) Like a steel ball-bearing or marble.

7. J.J. Thomson (1897)  Used cathode rays to determine that atoms contained small negatively charged particles called electrons.  These particles were attracted to the positive plate and repelled by the negative plate.  It didn’t matter which gas was in the tube they all had the same results.  Used cathode rays to determine that atoms contained small negatively charged particles called electrons.  These particles were attracted to the positive plate and repelled by the negative plate.  It didn’t matter which gas was in the tube they all had the same results.

8. Cathode Ray Tube

9. Electron beam Beam deflected by Negative plate

10. Robert Millikan (1909)  Used the Millikan Oil Drop Experiment to prove the mass and charge of the electron

11. Thomson’s Model of the Atom  The atom has electrons.  Electrons are embedded in a “positive goo” to keep the atom Neutral  CHOCOLATE CHIP COOKIE DOUGH MODEL (Raisin bun, Plum- pudding, blueberry Muffin)  The atom has electrons.  Electrons are embedded in a “positive goo” to keep the atom Neutral  CHOCOLATE CHIP COOKIE DOUGH MODEL (Raisin bun, Plum- pudding, blueberry Muffin)

12.  Atoms must also contain positive charges to balance the negative electrons  Other particles must account for most of the mass of the atom  Atoms must also contain positive charges to balance the negative electrons  Other particles must account for most of the mass of the atom Issues Not Delt with by Thomson and Millikan

13. Ernest Rutherford (1911)  Gold Foil Experiment:  Assumed mass and charge were evenly distributed throughout the atom (“plum-pudding” model)  Shot alpha particles (2 protons + 2 neutrons) at thin sheet of gold  Expected most of the particles to pass with only slight deflection  Most particles did, but some showed wide-angle deflections (some back to the source).  discovery of the NUCLEUS of the atom  Gold Foil Experiment:  Assumed mass and charge were evenly distributed throughout the atom (“plum-pudding” model)  Shot alpha particles (2 protons + 2 neutrons) at thin sheet of gold  Expected most of the particles to pass with only slight deflection  Most particles did, but some showed wide-angle deflections (some back to the source).  discovery of the NUCLEUS of the atom

14. Ernest Rutherford Cont…  causes proton-proton, proton-neutron, neutron- neutron attractions  small, dense, positively charged center of the atom  number of PROTONS in the nucleus determines the atom’s identity  causes proton-proton, proton-neutron, neutron- neutron attractions  small, dense, positively charged center of the atom  number of PROTONS in the nucleus determines the atom’s identity

15. Gold Foil Experiment Lead Box

16. Rutherford Activity

17. New Atomic Model Positive Nucleus at center Negative Electrons sitting in Empty Space

18. Problem with the New Model  Electrons would be pulled into the center of the atom by the very positive nucleus. (Opposite charges attract)  We know that this doesn’t happen so how do the electrons keep from being pulled in ???  Electrons would be pulled into the center of the atom by the very positive nucleus. (Opposite charges attract)  We know that this doesn’t happen so how do the electrons keep from being pulled in ???

19. Forces in the Nucleus  Repulsive forces should exist between protons in the nucleus (like charges repel).  Strong (nuclear) force:  Attractive force that acts over very small distances in the nucleus.  Overcomes the repulsive forces caused by like charges, so the protons can all stay in the nucleus.  Repulsive forces should exist between protons in the nucleus (like charges repel).  Strong (nuclear) force:  Attractive force that acts over very small distances in the nucleus.  Overcomes the repulsive forces caused by like charges, so the protons can all stay in the nucleus.

20. Atomic Dimensions  Atomic radii: 40 to 270 pm  Nuclear radii: about 0.001 pm  Nuclear density: about 2 x 10 8 metric tons/cm 3  1 amu (atomic mass unit) = 1.660540 x 10 - 27 kg  Atomic radii: 40 to 270 pm  Nuclear radii: about 0.001 pm  Nuclear density: about 2 x 10 8 metric tons/cm 3  1 amu (atomic mass unit) = 1.660540 x 10 - 27 kg