The arrangement of electron around the atom
Quiz yourself by thinking what should be in
each of the black spaces below before clicking
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| Danish scientist who contributed greatly to our knowledge of the electrons arrangement in the atom | Niels Bohr
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| Emission Spectrum | The light emitted from a element when heated. light passed through gasoues sample. black wavelengths. atom goes from excited to ground
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| Colour of Lithium flame | Crimson
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| Colour of Potassium flame | Lilac
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| Colour of Sodium flame | Yellow/Orange
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| Colour of Barium flame | Green
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| Colour of Strontium flame | Red
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| Colour of Copper Flame | Blue/Green
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| Orbital (Bohr Definition) | The fixed path an electron takes as it revolves around the nucleus
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| Energy Level | The fixed amount of energy that an electron in an atom has.
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| Level an electron starts on before energy is applied | Ground state
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| Level an atom moves to after energy has been applied | Excited
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| Equation used to calculate the energy given off by an electron | E=hf
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| What does h stand for in E=hf | Planck s Constant
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| The correct order of the sublevels | s p d f
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| 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
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| 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%)
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| Shape of an s orbital | spherical
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| Shape of a p orbital | dumbbell
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| 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
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| 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
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| n1 n2 n3? | n1= lyman series. invisible/florence. n2= balmer seris. visible. n3=paschen series. invisble ir
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| absorbption spectrum | white light. gasoues sample of element. light emmited has wavelegths missing. atom goes from ground to excited
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| 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
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| 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
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| 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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