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Electron and Atom
The arrangement of electron around the atom
| Question | Answer |
|---|---|
| Danish scientist who contributed greatly to our knowledge of the electrons arrangement in the atom | Niels Bohr |
| Emission Spectrum | The light emitted from a element when heated. light passed through gasoues sample. black wavelengths. atom goes from excited to ground |
| Colour of Lithium flame | Crimson |
| Colour of Potassium flame | Lilac |
| Colour of Sodium flame | Yellow/Orange |
| Colour of Barium flame | Green |
| Colour of Strontium flame | Red |
| Colour of Copper Flame | Blue/Green |
| Orbital (Bohr Definition) | The fixed path an electron takes as it revolves around the nucleus |
| Energy Level | The fixed amount of energy that an electron in an atom has. |
| Level an electron starts on before energy is applied | Ground state |
| Level an atom moves to after energy has been applied | Excited |
| Equation used to calculate the energy given off by an electron | E=hf |
| What does h stand for in E=hf | Planck s Constant |
| The correct order of the sublevels | s p d f |
| Heisenbergs Uncertainty Principle | It is impossible to measure at the same time the velocity and the position of an electron, we can only talk about the probability of an electrons position |
| New definition of an orbital | An orbital is the region around the nucleus within which there is a high probability of finding an electron. (95%) |
| Shape of an s orbital | spherical |
| Shape of a p orbital | dumbbell |
| Limitations of Bohr Theory? | Only works for Hydrogen, not other elements Did not take into account energy sub levels Did not take into account orbitals |
| bohr theory | electrons move around in fixed paths. orbits. definite energy level. cannot gain or loose enrergy in an energy level. when thr absorb energy they move up a level. excited state. unstabel. fall back down go ground state. stabel. light emmited |
| n1 n2 n3? | n1= lyman series. invisible/florence. n2= balmer seris. visible. n3=paschen series. invisble ir |
| absorbption spectrum | white light. gasoues sample of element. light emmited has wavelegths missing. atom goes from ground to excited |
| how do we know atoms have energy levels? | only definite amounts of energy emmited this implies atons can only occupy definitr energy level. thus atoms have definite enrgy levels |
| why does hydrogen emmision spectrum have so many colours? | many atoms of hydrogen in a sample. electrons in atoms have diferent energynlevels. therefore different amounts of energy are emitted and different colours emitted |
| sub levels | sub divisions of energy levels. groúp of atomic orbitals in an atom that have thr same amount of energ |
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cbschemistry
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