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Chapter 5: Chemistry
This is a review over chapter 5 "electrons in Atoms" in Person chemistry book
| Question/Term | Answer/definition |
|---|---|
| Rutherford's atomic model | Explained only a few simple properties of atoms. It could not explain the chemical properties of elements. |
| The Bohr Model | Changed initial model to incorperate newer discoveries about how the energy of an atom changes when an atom absorbs or emits lights. He considered this to be the atom, hydrogen, which has one electron. |
| energy levels | the fixed energies an electron can have |
| quantum | the amount of energy required to move an electron from one energy level to another. |
| quantum mechanical model | Determines the allowed energies an electron can have and how likely it is to find the electron in various locations around the nucleus of an atom. |
| atomic orbital | describes the probability of finding an electron at various locations around the nucleus. |
| shape of s orbital | circular |
| p orbital shape | shaped like an 8 |
| d orbital shape | flower, or double passifire |
| electron configuration | they ways in which electrons are arranged in various orbitals around the nuclei of atoms. |
| aufbau principle | elecrtons occupy the orbitals of lowest energy first. |
| Pauli exclusion principle | an atomic orbital may describe at the most two electrons |
| spin | a quantum mechanical property of electrons and may be thorught of as clockwise or counterclockwise |
| Hund's rule | Electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible. |
| amplitude | the wave's height from zero to the crest |
| wavelength | represented by lambda and is the distance between the crests. |
| frequency | the SI unit of cycles per second |
| electromagnetic radiation | includes radio waves, microwaves, infrared waves, visible light, ultraviolet waves, X-rays, and gamma rays |
| spectrum | when sunlight passes through a prisum, the different wavelengths seperate into a _____ of colors. |
| Atomic emission spectrum | the wavelengths of spectral lines are characteristics of the element, and they make of the spectral lines are characteristic of the element. |
| Planck's constant | the constant (h), which has a value of 6.626*10^-34 |
| photoelectric effect | electrons are ejected when light shines on a metal |
| photons | Einstein's proposed that light cold be described as quanta of energy that behave as if they were particles. |
| ground state | when the electron has its lowest possible energy. |
| Heisenberg uncertainty principle | state that it is impospossible to know bothe the velocity and the position of a particle at the same time. |
Created by:
hihello2007
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