1.  Review  Movie  Notes  Homework

2. KK  Cu  Br  Xe

3. Cr  Complete Electron configuration  Orbital Diagram  Bohr’s Model

4.  Chlorine consists of the following isotopes:  Calculate the weighted average atomic mass. IsotopeMassAbundance 35 Cl34.9688575.771% 37 Cl36.9659024.229%

5. Song Time

6. Atomic Theory Polka  Dalton, Thomson, Rutherford and Bohr. Schrödinger and Heisenberg, and many, many more. Used their brains to venture in the realm of inner space and found the world of the atom was a weird and wondrous place.

7.  Dalton did experiments and said, “I think it’s clear, atoms are tiny indestructible spheres.”

8.  Thomson worked with cathode rays and said, “I disagree. A plum-pudding model makes much more sense to me.”

9.  A new chapter in atomic theory started to unfold when Rutherford played around with atoms made of gold. When a few of his alpha particles came bounding back, he hypothesized a nucleus had knocked them off the track.

10.  Dalton, Thomson, Rutherford and Bohr. Schrödinger and Heisenberg, and many, many more. Used their brains to venture in the realm of inner space and found the world of the atom was a weird and wondrous place.

11.  Bohr saw spectral lines for hydrogen and said, “It seems to me.. Electrons move in orbits with specific energies.”

12.  Heisenberg said, “Forget it, there’s no way to know the orbit or a path, where the electron’s gonna go.”

13.  Schrödinger used lots and lots of fancy mathematics, and made a model of the atom based on quantum mechanics. It has orbitals and those are based on probability. The atom is a fuzzy blob of pure uncertainty.

14.  Dalton, Thomson, Rutherford and Bohr. Schrödinger and Heisenberg, and many, many more. Used their brains to venture in the realm of inner space and found the world of the atom was a weird and wondrous place.

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17.  With the PT arranged by atomic number, trends appear within the physical properties of the elements both periodically and within a family

18.  The size of an atom  Periodic Trend  Decreases with increase in nuclear charge  Number of protons  Protons pull electrons in with greater force  Family Trend  Increases with increase in number of energy levels.  Each new period adds an additional orbit.

19.  Cations  Smaller than parent atom  Lost e - emptying energy level and nucleus can pull remaining e - closer.  Anions  Larger than parent atom  Gained e - ; electrons repel each other so size enlarged.

20.  The energy required to remove an electron  Periodic Trend  Increases with increased nuclear charge  Electrons are closer to nucleus which does not want to lose its electrons  Family Trend  Decreases with additional energy levels  Electrons are further from nucleus and easier to remove; shielding

21.  The ability to attract an electron  Periodic Trend  Increases with increased nuclear charge  Nucleus provides a stronger pull  Family Trend  Decreases with each additional energy level  Shielding

22.  Ability to react with other chemicals.  Family Trend for metals  Increases down a family  Family Trend for nonmetals  Decreases down a family