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Chemistry test 3
Chapters 7-9
| Term | Definition |
|---|---|
| Electron spin | describes the negatively charged electron spinning on an axis |
| spin quantum number | ms, has two possible values/spin states: +1/2 and -1/2 |
| upward spin | ms = +1/2 |
| downward spin | ms = -1/2 |
| spin paired | two electrons with opposite spin, produces no magnetic field |
| diamagnetic | a species with no unpaired electrons, weakly repelled by a magnet |
| paramagnetic | a species with unpaired electrons, weakly attracted by a magnet |
| ferromagnetic | strong magnetic properties of iron and its alloys, which is a special type of parramagnetism, strongly attracted by a magnet |
| electron configurations | show how electrons are distributed in orbitals of an atom - predicted for the atom's ground state (lowest energy) |
| Pauli Exclusion Principle | no two electrons within an atom can have the same set of four quantum numbers (n, l, mt, and ms) - no more than 2 electrons in an orbital |
| Aufbau principle | to write the ground state configuration of an atom, start with the lowest energy sublevel and work up, fill each sublevel before beginning the next one |
| Hund's Rule of Maximum Multiplicity | the lowest-energy electron configuration is the one where the maximum number of electrons is unpaired |
| Noble gas notation | shortcut for writing the electron configurations of the other elements, start with configuration of the nearest noble gas and add to it |
| core electrons | noble gas notation represents these, they are in filled shells |
| Cr | [Ar] 4s1 3d5 |
| Mo | [Kr] 5s1 4d5 |
| Cu | [Ar] 4s1 3d10 |
| Ag | [Kr] 5s1 4d10 |
| Au | [Xe] 6s1 4f14 5d10 |
| octet rule | atoms tend to gain, lose, or share electrons in such a way as to end up with 8 electrons in their outer shell |
| valence electrons | outershell electrons |
| covalent bond | a bond formed when 2 atoms share a pair of electrons |
| structural formula | a formula which shows atoms and bonds connecting them |
| Lewis Structures | structural formulas which are symbolic pictures of molecules showing atoms, covalent bonds, and all other outershell electrons |
| VSEPR | valence shell electron pair repulsion theory - pairs of valence electrons around an atom repel each other and try to keep as far apart as possible - used to predict the geometries of molecules |
| linear | 2 electron sets, 2 terminal atoms, 0 lone pairs |
| triangular planar | 3 electron sets, 3 terminal atoms, 0 lone pairs |
| bent | 3 electron sets, 2 terminal atoms, 1 lone pair |
| tetrahedron | 4 electron sets, 4 terminal atoms, 0 lone pairs |
| trigonal pyramid | 4 electron sets, 3 terminal atoms, 1 lone pair |
| bent (2) | 4 electrons sets, 2 terminal atoms, 2 lone pairs |
| trigonal bipyramid | 5 electron sets, 5 terminal atoms, 0 lone pairs |
| see-saw | 5 electron sets, 4 terminal atoms, 1 lone pair |
| T-shaped | 5 electron sets, 3 terminal atoms, 2 lone pairs |
| linear (2) | 5 electron sets, 2 terminal atoms, 3 lone pairs |
| octahedron | 6 electron sets, 6 terminal atoms, 0 lone pairs |
| square pyramid | 6 electron sets, 5 terminal atoms, 1 lone pair |
| square planar | 6 electron sets, 4 terminal atoms, 2 lone pairs |
Created by:
imr36093
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