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Chem 111- Unit 3
| Question | Answer |
|---|---|
| ammonium | NH4+ |
| hydronium | H3O+ |
| acetate | CH3COO- |
| hydroxide | OH- |
| chlorate | ClO3- |
| perchlorate | ClO4- |
| nitrate | NO3- |
| permanganate | MnO4- |
| carbonate | CO3 2- |
| hydrogen carbonate | HCO3- |
| dichromate | Cr2O7 2- |
| phosphate | PO4 3- |
| sulfate | SO4 2- |
| empirical formula | defines the smallest whole number ratio of the atoms (usually ionic) |
| molecular formula | accounts for all atoms present in the molecule (usually covalent) |
| structural formula | shows atoms and bonding pattern |
| diatomic molecules | hydrogen, nitrogen, oxygen, halogens |
| 1 mole | 6.022E10^23 things |
| mass percent | the amount of mass each atom contributes to the total mass of the unit |
| which atoms can have an expanded octet? | anything in period 3 or higher |
| determining best Lewis structure (4) | -smaller formal charges -fewer formal charges -more negative charge for more electronegative atoms (v/v) -*some believe the octet rule is always best |
| formal charge | the charge on an atom based on the drawn Lewis structure (# valence e's - assigned e's) |
| electronegativity | the relative ability of a bonded atom to attract electrons (top right= highest) |
| resonance structures | different ways of representing the same molecule w/ different bonding patterns |
| electron delocalization | electrons delocalized due to different possible arrangements of single and double bonds |
| bond order | (bonding pairs)/(positions) |
| atoms that may have less than an octet | Be & B |
| molecules that may have an unpaired electron | free radicals- NO, NO2 |
| geometry & angle- 2 atoms around central | linear, 180 |
| geometry & angle- 3 atoms around central | trigonal planar, 120 |
| geometry & angle- 4 atoms around central | tetrahedral, 109.5 |
| geometry & angle- 5 atoms around central | trigonal bipyramidal, 90 (axial) & 120 (equatorial) |
| geometry & angle- 6 atoms around central | octahedral, 90 |
| VSEPR | (valence shell electron pair repulsion) electrons are located as far apart as possible to minimize repulsions |
| 2 outer atoms, 1 lone pair | bent, <120 |
| 3 outer atoms, 1 lone pair | trigonal pyramidal, <109.5 |
| 2 outer atoms, 2 lone pairs | bent, <109.5 |
| 4 outer atoms, 1 lone pair | seesaw, <90, <120 **equatorial position |
| 3 outer atoms, 2 lone pairs | t-shaped, <90 **equatorial position |
| 2 outer atoms, 3 lone pairs | linear, 180 **equatorial position |
| 5 outer atoms, 1 lone pair | square pyramid, <90 |
| 4 outer atoms, 2 lone pairs | square planar, 90 |
| d hybrid orbital used | when there are <4 atoms around the central atom |
| lone pairs & orbitals | paired in hybrid orbitals |
| double bond type(s) | 1 pi bond, 1 sigma bond |
| triple bond type(s) | 2 pi bonds, 1 sigma bond |
| central atom w/ formal charge | add/subtract an electron |
| sigma bonds | end-to-end overlaps of orbitals |
| pi bonds | side-to-side overlaps of orbitals |
Created by:
melaniebeale
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