Chemical Building Blocks

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Chemical Building Blocks Atomic theories, models and electronic structure

QUIZ: ½ sheet of paper An analyst measured a 3.3 x 10-2 L sample and found it weighed 385 mg. Report its density in g/mL. (Proper SF) Give an example of the ff. A colloid A pure substance An intensive property An extensive property A chemical property Parts of the atom (3pts., bonus of 1 pt. each for other subatomic particles)

History of the Atomic Theory

Dalton’s Atomic Theory Matter is composed of extremely small particles called atoms. All atoms of a given element are identical, having the same size, mass and chemical properties. The atoms of one element are different from the atoms of all other elements. Compounds are composed of atoms of different elements combined in fixed proportions. Chemical reactions only involve the rearrangement of atoms. Atoms are not created or destroyed in chemical reactions.

Law of Conservation of Mass

Law of Multiple Proportions

Cathode Ray Tube

Cathode ray tube television

Radioactivity

(Uranium compound)

Atomic Models Plum pudding model

Rutherford’s gold foil experiment

Rutherford’s atomic model

Discovery of the Neutron Chadwick’s equation:

Parts of the atom Protons Electrons Neutrons Atomic number and mass number isotopes

Test Yourself! How many neutrons are there in the 90Sr nucleus? A rubidium isotope has 50 neutrons. What is its mass no.? How many neutrons does 90Mo have? How many neutrons are in bromine-81? Which of the following isotopes are of the same element? Name the isotopes. 90 90 88 88 93 X X X X X 37 35 37 38 38

Electromagnetic spectrum

Photoelectric effect Einstein

Continuous vs. Line Spectra

Bohr’s Model Allowed energy states Energy is quantized (flame test)

Heisenberg’s uncertainty principle An observer always has an effect on the observed Location and momentum of electron Schrodinger’s wave equations: quantum numbers (n, l, m, ms)

Orbitals

Possible orientations of d-orbitals

The f orbitals

Orbital energy levels in hrdrogen atom Energy only depends on principal quantum number n n=3 n=2 n=1

Orbital energy levels in multi-electron atom Energy depends on n and l n=3 l = 2 n=3 l = 1 n=3 l = 0 n=2 l = 1 n=2 l = 0 n=1 l = 0

Outermost subshell containing electrons

Additional exercises For n=4, what are the possible values of l and ml? Which of the following are permissible sets of quantum numbers for an electron in a hydrogen atom? (n,l,ml) (2,2,-2) (4,3,-1) (1,0,0) (6,3,-4)