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Periodicity
| Question | Answer |
|---|---|
| Heisenberg uncertainty principle | a principle stating that there is a fundamental limitation to how precisely both the position and momentum of a particle can be known at a given time |
| Electron affinity | the energy change associated with the addition of an electron to a gaseous atom |
| Transition metals | several series of elements in which inner orbitals (d or f orbitals) are being filled |
| Orbital | a specific wave function for an electron in an atom. Probability of electron location |
| Actinides | a group of 14 elements following actinium in the periodic table, in which the 5f orbitals are being filled |
| angular momentum quantum number | l, the quantum number relating to the shape of an atomic orbital, which can assume any integral value from 0 to n-1 for each value of n |
| main-group, or representative, elements | elements in the groups labeled 1A, 2A, 3A, 4A, 5A, 6A, 7A, and 8A in the periodic table. the group number gives the sum of the valence s and p electrons |
| principle quantum number | n, the quantum number relating to the size and energy of an orbital; it can have any positive integer value |
| core electron | an inner electron in an atom; one not in the outermost (valence) principle quantum level |
| Pauli exclusion principle | in a given atoms, no two electrons can have the same set of four quantum numbers |
| Aufbau principle | the principle stating that as protons are added one by one to the nucleus to build up the elements, electrons are similarly added to hydrogen-like orbitals |
| magnetic quantum number | ml, the quantum number relating to the orientation of an orbital in space relative to the other orbitals with the same l quantum number. it can have integral values between l and -l, including zero |
| metalloids | elements along the division line in the periodic table between metals and nonmetals. These elements exhibit both metallic and nonmetallic properties. |
| electronic spin quantum number | ms, a quantum number representing one of the two possible values for electron spin; either +1/2 or -1/2 |
| valence electrons | the electrons in the outermost principle quantum level of an atom |
| atomic radii | half the distance between the nuclei in a molecule consisting of identical atoms |
| Hund's rule | the lowest energy configuration for an atom is the one having the maximum number of unpaired electrons allowed by the Pauli exclusion principle in a particular set of degenerate orbitals, all with unpaired electrons having parallel spins |
| first ionization energy | the energy required to remove the first electron in an atom, forming the +1 cation |
| second ionization energy | the energy required to remove the second electron in ana atom, forming the +2 cation |
| isoelectronic ions | atoms or ions that contain the same number of electrons despite having different number of protons |
| electronegativity | the tendency of an atom in a molecule to attract shared electrons to itself |
Created by:
shudonmiller
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