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CHEM EXAM 3
| Term | Definition |
|---|---|
| electronegativity (EN) | measure of attraction of an atom for bonding electrons in a chemical bond |
| a high EN means it wants to bond to | more electrons |
| Polarity | an uneven distribution of electrons |
| electrons in O-H are pulled closer to O because it has a higher | electronegativity |
| Delta | difference |
| To find the polarity bonds | look at their EN and find the difference. For example H is 2.2 and F is 4.0 so the polarity is 1.8 |
| The higher the difference in polarity the | more electronegative |
| covalent bonds | share electrons |
| ionic bonds | transfer electrons, creating cations and anions |
| covalent bonds with the same or similar EN | are non-polar, with an EN difference of less than 0.5 |
| covalent bonds with different EN | are polar, with an EN difference between 0.5 and 1.8 |
| ionic bonds are when electrons are transferred creating cations and anions, resulting in | a high polarity, with an EN difference of above 1.8 |
| Bond Dipole | separation of partial + and - charges along the physical bond of a molecule |
| Hydrogen has a EN of 2.20 and fluorine has a EN of 3.98 so the positive charge will start with | hydrogen and arrow will end on Fluorine |
| Bond polarity does not equal | molecular polarity |
| On the electrostatic potential map more blue is a | positive charge |
| on the electrostatic potential map, the more red is a | negative |
| a molecule containing only nonpolar bonds is | non polar |
| diatomic elements with the same element (N2, O2, Cl2) are | non polar |
| all hydrocarbons (CH4, C2H6) are | non polar |
| a molecule that contains only polar bonds may be | polar |
| bond polarity depends on the | 3d shape |
| diatomic molecules are polar if they contain | different elements (CO, NO) |
| no lone pairs and all terminal atoms are the same (CO2, SO3) means it is | non polar |
| if there is one lone pair on central atom (SO2, NH3) it is | polar |
| intermolecular forces (IMF) | attraction between molecules |
| Boiling point of water is | 100 degrees celsius |
| why is the boiling point of water higher than H2S? | there is hydrogen bonding, and a higher IMF needs more heat to break up their liquid state |
| IMF Force: Dispersion Force | weakest type, temporary dipoles |
| IMF: Dipole-Dipole Attractions | only in polar molecules, permanent dipoles. |
| IMF: Hydrogen Bonding | strongest type, only with Hydrogen and Oxygen, Nitrogen, and/or Fluorine |
| Intramolecular forces | occuring within a molecule, strong chemical bond |
| Intermolecular forces | occurring between different molecules, weaker physical bond |
| connects water molecules to other water molecules | intermolecular forces |
| connects O-H in water | intramolecular forces |
| the change in EN connects to | the polarity of chemical bonds |
| the polarity of chemical bonds + molecular shape= | polarity of molecules |
| the polarity of molecules leads to | Intermolecular forces |
| intermolecular forces leads to | boiling point, melting point, and solubility |
| water has a high boiling point due to having the strongest | intermolecular forces |
| solid water has a _____ density than liquid water | lower |
| when water is solidified the | mass does not change but volume will increase |
| solution | homogenous mixture of one solvent with 1+ solute |
| solvent | component of solution with a larger mass |
| mass of solute + mass of solvent = | mass of solution |
| concentration of solutions = | mass of solute/mass of solution |
| the molarity concentration = | # of moles / liters of solution |
| moles = | mass/molar mass |
| all units in concentration problems will be | liters and grams |
| double displacements | ionic compounds react and cations and anions get exchanged between reactants |
| example of double displacements | NaCl (aq) + AgNO3 -> NaNO3 (aq) + AgCl(s) |
| Electrolyte | substance that is electrically conductive when it dissolves in water |
| Strong electrolytes | soluble ionic compounds, strong acids and strong bases |
| Nonelectrolyte | molecular compound which remain intact and don't separate into ions |
| soluble | a solute than can fully dissolve into a solvent to form uniform homogenous mixture |
| insoluble | chemical that does not dissolve into the solvent |
| Polar solvents dissolve | polar solutes |
| Non polar solvents dissolve | nonpolar solutes |
| water is | polar due to its bent shape |
| Hydrocarbons (CH) solutes | are always polar |
| Ionic compounds (metal and non metal) solutes | are polar |
| Alcohol and ethanol solutes | are polar |
| The solvent H2O (water) is | polar |
| The solvent CH (hydrocarbons) is | non polar |
| The solvent CCl4 is | non polar |
| Hydroxyl Groups | are molecular compounds (OH) |
| IMF promotes | solubility |
| Sucrose (C12H22O12) | nonelectrolyte because it intact when dissolving, is molecular compound, and doesn't produce ions |
| The more hydroxyl groups the | more solubility |
| Acid | substance that results hydrogen ions H+ (protons) in aqueous solutions |
| H+ (hydrogen ion) means the same things as | H3O+ (hydronium ion) |
| Nitrate | NO3- |
| Sulfate | SO4 ^2- |
| Ammonium | NH4 + |
| Carbonate | CO3 ^2- |
| Phosphate | PO4 ^2- |
| Strong Acids | acid that disassociates completely. It is completely separated, one single arrow |
| Weak Acids | only dissociates to a small extent, a reversible process with a double arrow |
| Base | produces hydroxide ions (OH-) different than hydroxyl groups because this is an ionic compound due to it -1 charge |
| Strong Base | dissociates completely, one arrow |
| weak base | dissociates incompletely, two arrows |
| Equilibrium reaction | goes in both directions, has a forward and reverse reaction |
| reverse reaction | product and reactant are switched |
| acid and base neutralization | protons (H+) from an acid combine with hydroxide ions (OH-) from base to form water molecules |
| Molecular equations | acid + base -> ionic compound + water |
| Ionic equations | breaking of acid, base, and ionic compound into ions |
| total ionic equation | equation with ions subbed in for the acid, base, and ionic compound |
| spectator ions | always the ionic compound |
| net ionic equation | H+ + OH- ->H2O |
| example of spectator ions in this equation: HNO3 + KOH -> KNO3 + H2O | NO3 and K |
| In acid base neutralization | H+ and OH- must equal each other |
| acidic solutions | contain more H+ than OH- |
| basic solutions | contain more OH- than H+ |
| Neutral | equal amount of H+ and OH- |
| the amount of H+ and OH- will equal | 10x10^-14 |
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