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Chapter 3
Exam 2
| Question | Answer |
|---|---|
| What are some types of electromagnetic energy on the electromagnetic spectrum? | gamma rays, x rays, ultraviolet rays, etc. |
| Three parts of light as a wave are: | frequency, wavelength, and amplitude. |
| What does visible light have to do with atomic structure? (2 things) | 1. atoms give off light and other kinds of electromagnetic energy when energetically excited. 2. unlike white light, the light given off by excited atoms is not a continuous spectrum of wavelength. |
| What is significant about white light? (3 things) | 1. light from a light bulb or the sun is white light. 2. contains a continuous distribution of wavelengths spanning the entire visible spectrum. 3. when a narrow beam of white light passes through a prism, wavelengths go at diff rates. |
| What did Johanna Balmer do? | First to discover a pattern in line spectra. Discovered that the wavelengths of the four lines in the hydrogen spectrum can be expressed by an equation. |
| How did line spectra come about? | Scientists realized that energized atoms emit light of specific wavelengths. |
| Einstein's photoelectric effect | a beam of light behaves as if it was a stream of particles (photons) whose energy is related to their frequency by the equation: E=hv (h= 6.626 x10 -34 J x S ) Planck's constant |
| what do energetic atoms do? | emit light of specific wavelengths |
| what is a fact about wavelength and frequency | they are inversely related |
| What did Max Planck propose? | that light came in small bundles or quanta. These bundles of light are called photons. |
| what do energies of photons depend on? | the frequency of the light wave associated with them by the following equation. (E=hv) |
| What does the Bohr model useful for? | describing line spectra but its only applicable for small, relatively simple atoms. |
| What is Schrodinger's quantum mechanical model of the atom useful for? | electrons do not move around the nucleus in defined orbits. |
| What is the Heisenberg uncertainty principle | it is impossible to know precisely where an electron is and what path it follows. |
| principle quantum numbers are? | positive integers (n=1, 2,3, etc). |
| what is a wave function characterized by? | three parameters called quantum numbers. |
| what is the first type of parameter that a wave function is characterized by? | Angluar momentum- momentum quantum number l defines the 3d shape of oribital. |
| quantum number l: equals? | 0, 1, 2, 3, 4.. |
| subshell notation equals? | spdfg.. |
| what is an orbital with n=3 and l=2 called? | a 3d orbital |
| How does the quantum mechanical model account for line spectra and the solutions of the Balmer-Rydberg equation? (3 things) | 1. each electron occupies an orbital with a specific energy level 2. electrons can occupy the orbital they have the energy for. 3.energetically excited e-'s are unstable & return back to original orbital. |
| what do the three quantum numbers (n, l and m1) define? | energy, shape and spatial orientation. |
| what is the fourth quantum number? | Ms- spin, +1/2 or -1/2 |
| what is the pauli exclusion principle | no two electrons in an atom can have the same 4 quantum numbers. |
| what is the Aufbau principle? | lower energy orbitals fill before high energy orbitals. AKA- bus rule |
| what is electron repulsion? | outer shell electrons are pushed farther from nucleus than the inner shell electrons, thus are held less tightly. |
| What is electron shielding? | we say the outer electrons are "shielded" from the nucleus by the inner electrons. |
| what is the effective nuclear charge? | Zeff=Zactual-Electron Shielding |
| what is the electron configuration for aluminum? | 1s2 2s2 2p6 3s2 2p1 |
| what is the shorthand electron configuration for aluminum? | [Ne]3s2 3p1 |
| what is the trend followed for electron configurations and atomic radii when going down a group in the periodic table? | going down a group (column) in the periodic table we are increasing the principle quantum number so the shells get larger and the radii of atoms increase. |
| what is the trend followed for electron configurations and atomic radii when going across a period (row) in the periodic table? | the principle quantum numbers are increasing, so the shells get larger and the radii or atoms decrease. |
| what happens when the Zeff increases? | the electrons are pulled more tightly towards the nucleus. |
Created by:
maeallyn93
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