General Chemistry 1 - Electronic Structure and Periodicity of an Atom and Chemical Bonding (5th year, Grade 11 Senior High School)
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Course
Chemistry
Institution
This document includes lecture notes about the topics: 1) Electronic Structure of Atom, 2) Electronic Structure and Periodicity, and 3) Chemical Bonding. Specific topics covered are listed as keywords of this document. It makes use of graphics and visuals to help you understand the topic.
Lesson 6 - Electronic Structure of Atom (Nery, 1. 𝑛 – principal quantum number
11E) - Distance of the electron from the nucleus
- + (positive) integer (1, 2, 3…)
QUANTUM THEORY
Quantum theory - enables us to predict and
understand the critical role that electrons play in
chemistry.
1. How many electrons are present in a particular
atom? > Distance and probability that you’ll find an electron
2. What energies do individual electrons possess? > Radial probability - concerned with the location
3. Where in the atom can electrons be found?
2. 𝑙 – angular momentum quantum number
- Shape of the volume of space occupied
- Starts from 0 to 1 … until n-1
- Bawal equal; ex. n = 2; 0, 1
> Sharp (spherical)
> Quantum Superposition - ability of a quantum > Principal (angle-shaped)
system to be in multiple states at the same time until > Diffuse (four-clover leaf)
is it measured > Fundamental (wide complex)
> Wavelength (λ) decreases as momentum (p)
increases 3. 𝑚𝑙 – magnetic quantum number
> Electrons have dual nature, both particle and wave - orientation in space (is it along the x-axis?
- Came from Einstein’s idea of light y? z?)
> Lumalaki ang material, lumiliit ang wavelength - ml = -l to +l
ℎ
> Wavelength Formula: λ = 𝑝
- Ex.
l = 0; ml = 0
Schrödinger Wave Equation l = 1; ml = -1, 0, 1
In 1926 Schrodinger wrote an equation that l = 2; ml = -2, -1, 0, 1, 2
described both the particle and wave nature of
the electron
> Nodal plane - halos walang electron
Schrodinger’s equation can only be solved exactly
for the hydrogen atom but must approximate its
solution for multi-electron systems.
, QUANTUM NUMBERS
The quantum numbers making up the electronic
configuration.
Electron shell - region of space about a nucleus that
contains electrons that have approximately the same
energy and that spend most of their time
approximately the same distance from the nucleus;
4. 𝑚𝑠 – spin quantum number electrons same value of n
- orientation of electron spin > Sometimes called energy level no. 1
1 1
- − 2
or + 2 > point 0 is the nucleus
negative: counterclockwise; positive:
clockwise
Electron subshell - a region of space within an
electron shell that contains electrons that have the
What we can get from q.n. are: same energy.
- Existence - Electrons same value of n and l
- Possible amount of energy
Electron orbital - a region of space within an
electron subshell where an electron with a specific
energy is most likely to be found.
Pauli exclusion principle - no two electrons in an - Electrons same value of n, l, and ml
atom can have the same four quantum numbers
• Shell - electrons with the same value of n
• Subshell - electrons with the same values of n and l
• Orbital - electrons with the same values of n, l, and
ml
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