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Electron Arrangement | Definitions
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Electron Arrangement | Definitions
Aufbau Principle
Electrons always occupy the lowest available energy level first.
Energy Level
A region of definite energy within the atom that electrons can occupy.
Energy Sublevel
A subdivision of an energy level containing one or more atomic orbitals, all of equal energy.
Atomic Orbital
A region in the space of an atom where the probability of finding an electron is relatively high.
Electron Duality
Electrons have the properties of waves as well as particles.
Heisenberg's Uncertainty Principle
It is not possible to determine both the exact position and the velocity of an electron in an atom simultaneously.
Continuous Spectrum
When white light is passed through a prism, the resulting continuous band of colours from red to violet is known as a continuous spectrum.
Emission Spectrum
The series of coloured lines of definite wavelength observed against a dark background. The emission spectrum for each element is unique to that element.
Spectroscope
The instrument used to view the emission spectrum of an element.
Line Spectrum
The series of coloured lines of definite wavelength observed against a dark background.
Absorption Spectrum
The series of dark lines observed against a coloured background after white light has been passed through an element.
Ground State
The lowest energy state for an electron.
Excited State
When an electron occupies a higher energy state than the ground state by absorbing enough energy.
Hund's Rule
When two or more orbitals of equal energy are available to electrons, the electrons occupy them singly before filling them in pairs.
Pauli Exclusion Principle
No more than two electrons can occupy an orbital and they can only do so if they have opposite spin.
Atomic Radius
Half the distance between nuclei of two atoms of the same element that are joined together by a single covalent bond.
1st Ionisation Energy
The minimum energy in kJ required to remove one mole of the most loosely bound electrons from one mole of gaseous atoms in their ground state.
2nd Ionisation Energy
The minimum energy in kJ required to remove one mole of the most loosely bound electrons from one mole of gaseous monopositive atoms to produce one mole of dipositive ions.
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Aufbau Principle
Electrons always occupy the lowest available energy level first.
Energy Level
A region of definite energy within the atom that electrons can occupy.
Energy Sublevel
A subdivision of an energy level containing one or more atomic orbitals, all of equal energy.
Atomic Orbital
A region in the space of an atom where the probability of finding an electron is relatively high.
Electron Duality
Electrons have the properties of waves as well as particles.
Heisenberg's Uncertainty Principle
It is not possible to determine both the exact position and the velocity of an electron in an atom simultaneously.
Continuous Spectrum
When white light is passed through a prism, the resulting continuous band of colours from red to violet is known as a continuous spectrum.
Emission Spectrum
The series of coloured lines of definite wavelength observed against a dark background. The emission spectrum for each element is unique to that element.
Spectroscope
The instrument used to view the emission spectrum of an element.
Line Spectrum
The series of coloured lines of definite wavelength observed against a dark background.
Absorption Spectrum
The series of dark lines observed against a coloured background after white light has been passed through an element.
Ground State
The lowest energy state for an electron.
Excited State
When an electron occupies a higher energy state than the ground state by absorbing enough energy.
Hund's Rule
When two or more orbitals of equal energy are available to electrons, the electrons occupy them singly before filling them in pairs.
Pauli Exclusion Principle
No more than two electrons can occupy an orbital and they can only do so if they have opposite spin.
Atomic Radius
Half the distance between nuclei of two atoms of the same element that are joined together by a single covalent bond.
1st Ionisation Energy
The minimum energy in kJ required to remove one mole of the most loosely bound electrons from one mole of gaseous atoms in their ground state.
2nd Ionisation Energy
The minimum energy in kJ required to remove one mole of the most loosely bound electrons from one mole of gaseous monopositive atoms to produce one mole of dipositive ions.