Download Unit 06 Chapter 7 Notes

Unit 6
Chapter 7 Atomic Structure and Periodicity
Section 1: Electromagnetic Radiation
Define each of the following terms or answer each of the following questions prior to
class.
1) Electromagnetic radiation2) Wavelength-
3) Frequency4) Why is electromagnetic radiation important?
Equations: Identify each of the variables in the following equations.
1) λν = c c = speed of light 2.9979 x 108 m/s
Homework:
Section 2: The Nature of Matter
1) Particles2) Waves-
3) What did Max Planck discover?
4) Quantized –
5) What was Einstein’s proposal regarding electromagnetic radiation?
6) Does particulate matter exhibit wave properties?
7) Diffraction8) Diffraction pattern –
Equations: Identify each of the variables in the following equations.
1) ∆E = nhν
h = 6.626 x 10-34 J*s (n is an integer and v is frequency)
2
2) E = mc
3) m = h/( λυ)
Homework:
Section 3: The Atomic Spectrum of Hydrogen
1) What is the emission spectrum of hydrogen gas?
2) What is meant by excited atoms?
3) Is the hydrogen emission spectrum a continuous or line spectrum?
Section 4: The Bohr Model
1) Describe the quantum model of the atom developed by Niels Bohr.
2) Ground State3) What is wrong with Bohr’s model?
Equations: Identify each of the variables in the following equations.
1) E = -2.178 x 10-18 J (Z2/ n2)
2) ∆E = Efinal – Einitial
a. When ∆E is negative, then energy is released.
Homework:
Section 5: The Quantum Mechanical Model of the Atom
1) Developed by: Heisenberg, de Broglie, and Schrodinger
2) Standing Wave: waves that are stationary, that do not gravel down the length of
the string, similar to the electron’s motion around the nucleus
a. There must be a
of ½ wavelengths in any of the
motions of the string
3) Orbital4) How does the electron moving around the nucleus?
5) Heisenberg uncertainty principle:
6) Probability distribution-
7) How do chemists define the size of an orbital?
Section 6: Quantum Numbers
1) Principal Quantum Number- n –
2) Angular momentum quantum number –
a. l = 0 is referred to as s
b. l = 1 is referred to as p
c. l = 2 is referred to as d
d. l = 3 is referred to as f
3) Magnetic Quantum Number – ml –
Homework:
Section 7: Orbital Shapes and Energies
1) Nodes- a
2) Describe the shape of each of the following orbitals:
3) Energy levels of orbitals are determined by what?
Study: Summary of hydrogen atom – pg
Section 8: Electron Spin and the Pauli Principle
1) Why is it thought that electrons spin?
2) Electron spin quantum number- ms-
3) Pauli Exclusion PrincipleSection 9 Polyelectronic Atoms
1) Polyelectronic atom2) What are the 3 energy contributions that need to be considered in atoms?
3) Electron correlation problem:
4) How do we correct for the electron correlation problem?
5) Electron shielding or screening6) How do the orbitals for polyelectronic atoms compare to the orbitals of hydrogen?
7) Indicate how you can determine the energy of orbitals for polyelectronic atoms.