development of the atomic model. atomos: cannot be divided solid balls
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Development of the Atomic Model
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Atomos: cannot be divided Solid balls
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5 principles Atoms are basic building block Atoms of same element are identical Atoms of different elements are different Atoms of different elements can combine in
definite proportions to form compounds Atoms are indivisible by chemical processes
First use of symbols
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Atom can be subdivided. Discovered electrons. Plum pudding model
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Oil drop experiment Charge of an electron
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Gold foil experiment Atom is mostly empty space Atom has a small, dense, positively
charged nucleus at its center.
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Bohr noticed a constant quantum leap Reasoned that electrons could not be
random Reasoned that they were in set orbits, set
distances away from nucleus. Planetary orbital model
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Bombarded Be with alpha particles New beam produced Not deflected by magnetic field, ie not
charged Approx same mass as protons The neutron
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Heisenberg Uncertainty Principle: you cannot know both the velocity and position of an electron in motion
Pauli Exclusion Principle: no two electrons can have the same four quantum numbers
Schroedinger equation: predicts the wave nature of an electron
Hund’s Rule: unoccupied orbitals will be filled before occupied orbitals are reused
Aufbau principle: electrons fill orbitals starting at the lowest available (possible) energy states before filling higher states
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Wave nature of electrons Orbitals
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Proton Neutron Electron Protons and Neutrons are composed of
quarks
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In the nucleus Positive charge About 1840 x larger than electron Mass = 1
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In the nucleus No charge About 1840 x larger than electron Mass = a little bit more than 1
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Outside the nucleus in the electron cloud Negative charge About 1/1840 as large as a proton Mass = essentially 0
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The number of protons is the atomic number. This identifies an element.
If the proton number changes, the element changes
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Isotope: a different version of an element. All chemical properties remain the same. The only difference is neutron number, and this can cause some isotopes to be radioactive.
Mass number: protons + neutrons. This identifies an isotope.
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The number of protons is the atomic number. This identifies an element.
If the proton number changes, the element changes
Mass number identifies an isotope
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Neutron number = mass number – atomic number
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Average atomic mass equals the sum of the masses of each isotope times its abundance.
Refer to your average atomic mass lab Refer to pages 172-177
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Electrons exist in probability clouds called orbitals.
The 4 currently identified orbitals are: s p d f
Others have been postulated
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Sphere 2 electron max
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6 electron limit 3 suborbitals, 2 electrons each
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10 electron limit 5 suborbitals, 2 electrons each
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14 electron limit 7 suborbitals, 2 electrons each
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Like electron addresses 4
Principal Orbital or azimuthal Magnetic Spin
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Measures energy level Values range from 1-7
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Indicates orbital: s, p, d, f s=0 p=1 d=2 f=3
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Indicates which suborbital
2px
2py
2pz
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Satisfies the Pauli exclusion principle Since electrons in the same orbital must
have opposite spins Values are EITHER + ½ or – ½
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First, learn the order of orbital filling. The slant diagram will help you with this.
Second, remember the orbital capacities. s: 2 electrons, p: 6 electrons, 3 suborbitals, d: 10 electrons, 5 suborbitals, f: 14 electrons, 7 suborbitals You can count these on the chart
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Electrons are energized by the flame. They jump to a higher energy level (quantum leap). When they fall down to their ground state, they fall the same distance and release the same amount of energy (quanta) as light each time, so its always the same color.