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3 Chem Live
Arrangement of electrons in the atom
Term | Definition |
---|---|
Line Spectrum | A series of narrow coloured lines |
Atomic Emission Spectra | Atoms emit light, giving a series of coloured lines on a black background |
Atomic Absorption Spectra | Atoms absorb light, giving a series of black lines on a coloured background. |
Spectrometer | Instrument used to carry out measurements on spectra |
Energy level | Discrete or fixed amount of energy that an electron in an atom may have. |
Ground State | is one in which the electrons occupy the lowest available energy level |
Excited state | is one in which the electrons occupy higher energy levels than those available in the ground state |
Bohr Theory | E*-E =hf |
Paschen | series of lines in the Infra red region |
Balmer | series of lines in the visible region |
Lyman | series of lines in the Ultra violet spectrum |
Energy Sublevel | is a subdivision of the main energy level and consists of one or more orbitals of the same energy. |
Orbital | is a region in space where there is a high probability of finding an electron. |
Heisenberg's Uncertainty Principle | states that it is impossible to measure at the same time both the velocity and the position of an electron. |
De Broglie | Suggested that all moving particles have a wave motion associated with them |
Atom | The smallest particle of an element that can take part in a chemical reaction |
Cation | A positively charged ion |
Diffraction | A change in direction of a wave as it passes through an opening |
Electron | Negatively charged particle present in all atoms and located in orbitals outside the nucleus |
Element | A substance which cannot be decomposed or broken down into simpler substances by chemical methods |
Atomic Absorption spectrum used for | detecting the analysis of heavy metals (lead, mercury & cadmium) in water or blood & to test for gunshot residue. |
Limitations of Bohrs Theory | He did not take into account the wave nature of an electron, was in conflict with Heisenbergs uncertainty principle and couldn't account for the splitting of certain lines in the spectra and didn't account for the presence of sublevels. |
Bohrs model of an electron | An electron travelling in a precise path at a precise distance from the nucleus |
S orbital | Spherical shaped |
P orbital | dumbbell-shaped |
P sublevel | consists of the 3 p orbitals px, py & pz. |
When an electron transitions from n=3 to n=2 what colour is observed in the balmer series | Red |
How many lines in the Balmer series | 4, when the electron drop from n =3 it's Red, n=4 it's teal, n=5 it's Blue, n=6 it's indigo, |