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Unit 9: Atomic Structure
Guiding Questions:
- How do we know what stars are made of?
- How are elements formed?
- Are all atoms of an element the same?
- How do we measure atoms if they are so small?
What you should learn:
- Atoms are made up of 3 subatomic particles and a lot of empty space; two particles make up the mass of the atom and are located in the nucleus and one, the electron, is located in the area outside of the nucleus.
- The color of light indicates the relative amount of energy of the light.
- Spectroscopic information can be used to identify elements because the amount of energy that can be absorbed or emitted is dependent on how much energy it takes to change the motion or position of a particle within an atom which is controlled by the atomic structure of the substance
More Specifically...:
IB Objectives: SL
HL
- History from Bohr - Schroedinger
- Give the relative energy associated with a particular color of light
- Describe and explain the difference between a continuous spectrum and a line spectrum
- Draw Bohr diagrams and indicate what happens to the electrons when light is absorbed and emitted.
- Relate emitted light to an element's characteristic spectra
- Draw an energy-level diagram, show transitions between different energy levels and relate to lines in the K-series: Balmer, Lyman, and Paschen
- UV range (Lyman) - transitions back to first energy level
- Visible range (Balmer) - transitions back to second energy level
- Infrared range (Paschen) transitions back to third energy level
- Convergence - energy levels get closer together as they get farther from nucleus??
- Solve problems using E = hv and E = RZ2(1/n22 - 1/n12)
- State that light can be considered a wave or a particle and that this is known as the wave-particle duality
- Determine the electron arrangement in main energy levels for each element through Z =20 (example: 2.8.7 or 2,8,7 for Z = 17)
- Compare and contrast the Bohr model of the atom with the quantum mechanical model in which,
- a. Electrons are both particle and wave
- b. The exact position of the electron cannot be known
- c. Electrons do not orbit the nucleus but are thought to exist in certain areas around the nucleus known as orbitals
- Electron Configurations
- Describe the shapes of the s, p, d, f orbitals
- Identify the four quantum numbers
- Draw orbital diagrams for a given element
- Draw electron configurations for a given element
- Convert between the noble gas configuration and the long-hand electron configuration
- Convert between orbital diagrams and electron configurations
- Recognize incorrect orbital diagrams and electron configurations and attribute the rule that is broken to:
- a. Hund
- b. Pauli or
- c. Aufbau
- Write electronic configuration of simple ions
Lecture Notes:
Assignments:
Labs:
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