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Periodicity

Quiz yourself by thinking what should be in each of the black spaces below before clicking on it to display the answer.
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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  
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Electron affinity   the energy change associated with the addition of an electron to a gaseous atom  
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Transition metals   several series of elements in which inner orbitals (d or f orbitals) are being filled  
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Orbital   a specific wave function for an electron in an atom. Probability of electron location  
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Actinides   a group of 14 elements following actinium in the periodic table, in which the 5f orbitals are being filled  
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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  
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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  
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principle quantum number   n, the quantum number relating to the size and energy of an orbital; it can have any positive integer value  
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core electron   an inner electron in an atom; one not in the outermost (valence) principle quantum level  
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Pauli exclusion principle   in a given atoms, no two electrons can have the same set of four quantum numbers  
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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  
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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  
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metalloids   elements along the division line in the periodic table between metals and nonmetals. These elements exhibit both metallic and nonmetallic properties.  
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electronic spin quantum number   ms, a quantum number representing one of the two possible values for electron spin; either +1/2 or -1/2  
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valence electrons   the electrons in the outermost principle quantum level of an atom  
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atomic radii   half the distance between the nuclei in a molecule consisting of identical atoms  
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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  
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first ionization energy   the energy required to remove the first electron in an atom, forming the +1 cation  
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second ionization energy   the energy required to remove the second electron in ana atom, forming the +2 cation  
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isoelectronic ions   atoms or ions that contain the same number of electrons despite having different number of protons  
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electronegativity   the tendency of an atom in a molecule to attract shared electrons to itself  
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