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SCH4U Canadian Grade 12 Chemistry Notes
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- Chemistry
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- 12th Grade
SCH4U Canadian Grade 12 Chemistry Notes
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SCH4U - Exam Review PackageAtomic Structure Review
1. Describe the contributions of the following scientists to our current understanding of the
atomic structure and quantum theory:
a. Bohr Planetary Model:
- Energy orbits the nucleus in shells
- Electrons travel within energy level without losing or
gaining energy
- ↑ distance from nucleus = ↑ energy
b. Heisenberg Uncertainty Principle:
- Due to its wave and particle nature, we can never know
the position and speed of an electron
- Velocity = wave nature
- Position = particle nature
c. Schrodinger Quantum Model:
- “Cloud of probability” illustrates the possibilities of
where the electron may lie as their distinct position is
unknown
d. Pauli Pauli’s Exclusion Principle:
- Electrons sharing an orbital must have opposite spins
e. Rutherford Nuclear Model: Gold Foil Experiment
- Alpha particles were fired at thin metal foils though a
small portion of it was deflected back
- Result: dense nucleus surrounded by a cloud of negative
charge
f. Thomson Plum Pudding Model:
- Cathode rays were deflected by charged objects = atoms
are mostly made of negatively charged particles
- Negative subatomic particles (electrons) were scattered
around a positive cloud within atoms
2. Based on the quantum mechanical model of the atom:
a. What is an “orbital”
i. Orbital: probability distribution maps for electrons (represented through
wave function)
b. What is the maximum electron carrying capacity of the following energy levels:
i. Equation: [x2(2)]
, n = 1 (2 electrons)
n = 2 (8 electrons)
n = 3 (18 electrons)
n = 4 (32 electrons)
n = 5 (50 electrons)
c. What orbital subshells would be found in the following energy levels:
n = 1 (s subshell)
n = 2 (p subshell)
n = 3 (d subshell)
n = 4 (f subshell)
n = 5 (g subshell)
d. How would the electrons be distributed amongst the orbital sublevels in n = 5 (ex:
number of e- per subshell)
Remember: 4 quantum numbers
- n = principal quantum number (size and energy)
- l = angular momentum quantum number (shape)
- Subshells within the main energy level
- Values (n - 1) = 4 subshells
- ml = magnetic quantum number (orientation of orbitals)
- Ranging from integers -5 to 5
- Total 25 orbitals
- ms = spin quantum number (direction of electron spin)
- Since there are 25 orbitals, there are 50 electrons
3. Electron configuration:
a. Write the ground state electron configuration of a neutral atom of nitrogen
i. Atomic number 7
ii. 1s22s22p3
b. Assign the quantum numbers to each of the electrons in your nitrogen atom
i. n=2
ii. l=1
iii. ml = -1, 0, 1
iv. ms = +½
c. Write the ground state complete electron configuration for iron, Fe.
i. Atomic number 26
ii. 1s22s22p63s23p63d64s2
d. Draw an orbital energy level diagram for titanium, Ti.
i. INCOMPELTE
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