Home > Uncategorized > Introduction to Solid State Chemistry Lecture 7

Introduction to Solid State Chemistry Lecture 7

Today’s lecture is 48 minutes. Wow! Looks like MIT has people who talk during classes as well.

x”+kx=f is the simple harmonic oscillator or SHO. Electronic structure dictates properties.

n+l relationship
fill in ascending n for equivalent N+L values
2s 2p
3s 3p 3d
4s 4p 4d
5s 5p 5d

Ionization energy increases across a row. Photoelectron spectroscopy or PSS is used for the measurement of IE. Dislodge electrons by hitting them with photons. We know the energy in, we know the energy out, the difference is the binding energy.
Energy incident = kinetic energy + binding energy

Xray can blast out the electrons, 1A. 100A would be UV rays. XPS and UPS have intensity versus energy.

The K shell is n=1. The L shell is n=2. Valence electrons are responsible for chemical reactivity and describes electrons in the outermost shell.

AVEE average valence electron energy. 11eV for most metals. Valence electrons are weakly held, a good electron donor. 75% of the periodic table.

High values of AVEE are greater than 13 eV. Valence electrons are tightly held, poor electron donor, good acceptor.

11eV to 13eV can act as either depending upon what surrounds it.

ns2 np6 for noble gases.

Sodium 3s1, 5.2 metal, Na = e- + Na+. It has to find an electron acceptor.

Electron transfer chemical reactions lead to full valence shell occupancy.

ionic bonding by electronic transfer. Ionic bondings lead to solids at room temperature.

Electrometallurgy is his area of research. 7.87 steel, 1.76 for Mg

As a powder or strip MG will ignite. As a billet it will not.

Ionic solids with a high temperature lead to ionic liquids.
MgCl2 = Mg2+ + 2Cl-

Mg can be used as a substitute to steel. It’s expensive to make.

normal NTs: CO, NO, HS2
HABC hemmorage, airway, breathing, ciruclation

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