Chem 101 Review (Pt 2) Flashcards
Wavelength
The distance between two consecutive peaks or troughs.
Frequency
The number of wave cycles that pass a specified point in space in a specified amount of time. Unit: per-second s^-1 or Hz
Magnitude
The magnitude of the displacement of the wave.
Speed of Light
c=2.998 * 10^8ms^-1
Paradoxes of the failures of Classical Models: Photoelectric Effect
A wave gives rise to a particle with corresponding energy. Supported the Wave-Particle Duality theory
The Bohr Model
For any particle in motion behaving like a Wave. Large objects that we use have very low wavelengths therefore they don’t act like particles
Bohr Model
We can have electrons only in quantized levels
Electron Behavior
-Electrons have kinetic energy in motion (want to move away)
-Nucleus keeps electrons orbiting around it (keeping them in check)
-Energy of ‘e’ is high away from nucleus and low close to nucleus
-Electrons transfer between quantum levels (shells)
What is quantum?
Energy quantized
Max Planks Expression
-Energy is released or absorbed in discreet ‘packets’, not in a continuum (spectrum).
-Energy therefore is quantized.
-The discrete ‘packets’ of energy are called ‘photons’
-Energy of ‘n’ photons (E)
Max Planks Equation
E= n.h.v (n=integer multiple; 1,2,3… h=Plank’s constant 6.626 * 10^-34 J.s (Joule seconds)
v= frequency
Balmer Rydberg Equation
-Represents “quantum leaps” of energy
Heisenberg Uncertainty Principle
It is fundamentally impossible to determine simultaneously and exactly both the momentum and position of a particle.
Possibility Density and Wavefunction
Orbitals: Energy, Shape and orientation
Electron Spins
Two electrons may be in the same shell, same orbital and same orientation. But at least their spins has to be unique.
Pauli Exclusion Principle
No two electrons in the same atom can have exactly the same set of all four quantum numbers.
Are core electrons hard or easy to remove?
Hard
Are valence electrons hard or easy to remove
Easy
Periodicity
Same group elements have similar character due to electron configuration similarity
Ionization Energy
Energy associated with the removal of ‘e’ from gaseous sample
Electron Affinity
Energy associated with the addition of ‘e’ from gaseous sample
Isoelectronic Series
Having the same electron configuration
