Term
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Definition
tells the size and energy of orbital
n |
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Term
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Definition
tells the shape of the orbital
l
l = 0 - n-1 |
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Term
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Definition
tells the spatial orientation of the orbital
ml
l= -l → +l |
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Term
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Definition
tells the direction of the spin and electron has in an orbital
ms = +1/2 or -1/2
+1/2 is clockwise
-1/2 is counterclockwise |
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Term
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Definition
| electrons are arranged in order of increasing energy |
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Term
| Pauling exclusion principle |
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Definition
| Only 2 electrons may occupy an orbital and they must have opposite spins |
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Term
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Definition
| Electrons are filled singly in degenerate orbitals before pairing. |
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Term
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Definition
| Energy required to remove an electron from an isolated, gaseous atom or ion in its ground state. |
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Term
| Ionization energy...endothermic or exothermic? |
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Definition
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Term
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Definition
| The potential energy change associated with the addition of 1 mole of electrons to one mole of gaseous atoms or ions. |
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Term
| Electron Affinity...exothermic or endothermic? |
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Definition
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Term
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Definition
| Attraction of electrons in a bond to an atom. |
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Term
| Difference in electronegativity creates a ... |
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Definition
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Term
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Definition
| Energy required to completely separate the ions in one mole of a solid compound from each other to form a cloud of gaseous ions. |
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Definition
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Term
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Definition
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Term
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Definition
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Term
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Definition
| Non-directional bond between metals and nonmetals. |
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Term
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Definition
| Polar and non polar bonds between non-metals that consists of sharing electrons in the valence shell of the atoms. |
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Term
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Definition
| Attraction between the ions of a metal and the sea of electrons in another metal. |
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Term
| Attraction of ions to a sea of electrons explains what properties of metals. |
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Definition
Conductivity
Ductility
Malleability |
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Term
| Three principles of Valence Bond Theory |
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Definition
1. Covalent bonds form when electrons in the valence shells of two atoms overlap. These electrons must have opposite spins.
2. The size of the overlap determines the strength of the bond.
3. The shape of some molecules can only be explained by using hybrid orbitals. |
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Term
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Definition
| The mathematical mixing of pure s, p and d orbitals to generate new degenerate orbitals (hybrid orbitals). |
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Term
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Definition
| Energy required to break bonds (endothermic process). |
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Term
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Definition
| Pairs of electrons that are shared between two atoms. |
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Term
Molecular Orbital Theory (MO)
Bond order equation |
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Definition
Bond order = (# bonding e-) - (# antibonding e-)
2 |
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Term
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Definition
Pressure (P)
Volume (V)
Temperature (T)
Number of moles (n) |
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Term
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Definition
| Standard Temperature and Pressure |
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Term
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Definition
273.15 K
1 atm (760 torr)
22.4 L/mol
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Term
| Density of gases are measured in |
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Definition
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Term
| Densities of solids and liquids are measured in |
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Definition
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Term
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Definition
| Force of collisions of the gas distributed over the surface area of the container walls. |
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Term
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Definition
| The pressure of a fixed sample of any gas is inversely proportional to its volume at constant temperature. |
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Term
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Definition
| The volume of a gas is directly proportional to its temperature in K at constant pressure. |
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Term
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Definition
| The pressure of a gas is directly proportional to its temperature at constant volume. |
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Term
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Definition
| The volume of a gas is directly proportional to the number of moles at constant pressure and temperature. |
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Term
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Definition
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Term
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Definition
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Term
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Definition
| Gas that has no volume, is not attracted or repelled by another atom and is not slowed down by collisions. |
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Term
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Definition
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Term
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Definition
| The rate of effusion of a gas varies inversely with the square root of its density at constant pressure and temperature. |
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