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Gen Chem Chpt. 4
Periodic Trends
| Question | Answer |
|---|---|
| Elements are grouped by | Similar chemical and physical properties by Mendeleev |
| Who redefined the periodic table by atomic number | Henry Moseley |
| Electron configuration | specifies the arrangement of electrons un the atomic orbitals of an atom |
| Pauli Exclusion Principle | no two electrons in an atom in the ground state can have to same four quantum numbers (n, l, ms, ml) Ex: cannot have (2,1,1,2) |
| Aufbau Principle | building up of the elements by adding protons and electrons (lowest to highest energy |
| orbitals that have the same energy | degenerate (due to Hunds rule) |
| Hunds Rule | degenerate orbitals must all contain one electron before it can contain two electrons in an orbital |
| Paramagnetic | any orbital that does not have a full orbital; weakly attracted to the magnetic field |
| diamagnetic | electrons with a full orbital ( akali earth metals, 3d10, ad noble gases); weakly repelled by magnetic field |
| what makes it possible to abbreviate the writing of electron configurations? | the noble gas core |
| what are the electrons known to contribute to noble gas core? | core electrons |
| transition elements | are located mostly in d block and either have readily lose electrons to acquire an incompletely filled d shell |
| effective nuclear charge (Zeff) | the nuclear charge that is "felt" by the valence electrons. It is usually lower than the nuclear charge due to shielding by the core electrons |
| Atomic radius | distance between the atom's nucleus and its valence shell; decreases as it goes down to up and left to right on the periodic table |
| metallic radius | atomic radius of a metal atoms |
| covalent radius | atomic radius of a nonmetal atom; one half the distance between adjacent , identical nuclei in a substance |
| ionization energy (IE) | the energy required to remove an electron form an atoms. |
| The first Ionization Energy (IE1) | smaller than the subsequent ionization energies; removes any valence electrons; tend to increase across the periodic table from left to right and from up down to up |
| Electron Affinity (EA) | is the energy released when an atom in the gas phase accepts the electron ( A (g) + e- -> A- (g) - tend to increase across periodic table and is a chemical property |
| anion | ion with a negative charge |
| Properties of metals | ductile, malleable, lustrous and good conductors of heat; typicaly lose electrons to for cations -metallic character decreases across periodic table |
| diagonal relationship | the similar properties shared by elements in different groups and periods |
| Isoelectronic series | consists of one or more ions and a noble gas, all of which have identical electron configurations. - the greater the nuclear charge the smaller the radius |
| shielding | the partial obstruction of nuclear charge by core electrons |
Created by:
landryw
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