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| Relatively slow rates of chemical reation are associated with which of the following? |
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Definition
| Strong bonds in reactant molecules |
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| Standard enthalpy change for Na2O + H2O= 2NaOH |
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Definition
| change in G, H, and S are negative |
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| change in H for I2 + 3Cl2= 2ICl3 |
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Definition
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| two unshared pairs of electrons on central atom |
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Definition
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| Molecule with only one double bond |
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Definition
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| Molecule with the largest dipole moment |
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Definition
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| trigonal pyramidal geometry |
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Definition
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| change in H for 3C2H2= C6H6 |
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Definition
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Definition
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Definition
| change in G negative, change in H and S positive |
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Term
| most positive oxidation number |
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| compound that shows resonance |
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Definition
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Definition
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Definition
| formation of a crystalline solid from a supersaturated solution |
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| electrons shared by hydrogen and oxygen |
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Definition
| spend more time around oxygen |
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Definition
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Definition
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| number of structures for NO3- |
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Definition
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Term
| molecule that violates octet rule |
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Definition
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| number of electrons on FCl3 |
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Definition
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Term
| bond energy for CH4 + 4F2= CF4 + 4HF |
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Definition
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Term
| shape of AX5 with one nonbonding pair of electrons |
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Definition
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Term
| shape of AX3 with two lone pairs of electrons |
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Definition
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Term
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Definition
| trigonal pyramidal and trigonal planar |
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Term
| molecule that is nonpolar |
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Definition
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Definition
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| square planar hybridization |
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Definition
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Definition
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Definition
| compressing one mole of Ne at constant temperature from .5 to 1.5 atm |
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Term
| first law of thermodynamics |
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Definition
| energy cannot be created or destroyed but must be conserved |
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Term
| second law of thermodynamics |
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Definition
| entropy of the universe is increasing |
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Definition
| amount of energy required to raise one gram of a substance one degree Celsius |
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Term
| heat released when 9.25 moles of Fe is reacted with oxygen |
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Definition
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Term
| change in H for P4O10 + 6PCl5 =10Cl3PO |
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Definition
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Definition
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| kinetic molecular theory does not say |
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Definition
| gas particles move at speeds close to the speed of light |
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Definition
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Term
| Average atomic or molecular speed closest to N2 molecules at 0 C and 1 Atm |
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Definition
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Term
| greatest density at 0 C and 1 Atm |
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Definition
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Term
| Values that decrease when ideal gas is cooled by 25 degrees |
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Definition
| average distance between molecules and average speed of molecules |
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Term
| percent of CaCO3 by mass in limestone |
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Definition
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Term
| safest and most effective way to treat an acid splash on skin |
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Definition
| flush affected area with water and then with a dilute NaHCO3 |
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Term
| moles of HI needed to produce 2.5 moles of I2 |
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Definition
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Term
| why does water boil at a lower temperature on a mountain |
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Definition
| equilibrium water vapor pressure equal the atmospheric pressure at a lower temperature |
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Term
| partial pressures of gasses |
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Definition
| He less than Ne less than Ar |
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Term
| gas that deviates most form ideal behavior |
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Definition
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Term
| the a coefficient in van der Waals equation |
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Definition
| forces of attraction between molecules |
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Term
| how many protons, neutrons, and electrons are in Sr-90 |
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Definition
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Term
| Quantum numbers of ground-state gallium |
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Definition
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Term
| pauli exclusion principle |
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Definition
| indicates that an atomic orbital can hold no more than two electrons |
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Term
| dissolves in water to form a colorless solution |
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Definition
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Term
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Definition
| iodine liberates free bromine from a solution of bromide ion |
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Term
| barium sulfate is least soluble in a .01 molar solution of what |
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Definition
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Term
| what color is the flame when a solution of sodium chloride is vaporized in a flame |
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Definition
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Term
| use of a visible-light spectrophotometer |
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Definition
| determining the concentration of a solution of Cu(NO3)2 |
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Term
| based on ionization energies in chart, element X is what |
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Definition
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Term
| what happens to atomic radius as atomic number increases from 11-17 |
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Definition
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Term
| Rutherford's gold atom experiment |
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Definition
| neutrons are at the center of an atom |
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Term
| yellow precipitate forms when NaI is added to what |
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Definition
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Term
| not soluble in water but soluble in dilute hydrochloric acid |
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Definition
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Term
| what will separate Pb from other ions |
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Definition
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Term
| contains exactly two unpaired electrons |
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Definition
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Term
| contains only one electron in the highest occupied energy sublevel |
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Definition
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Term
| purple in aqueous solution |
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Definition
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Term
| white and soluble in water |
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Definition
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Definition
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| greatest percentage of which compound can be recovered by cooling a saturated solution of that compound from 90 degrees C to 30 C |
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Definition
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Term
| which property decreases across the periodic table form sodium to chlorine |
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Definition
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Term
| why is there a different nuclear charge on Na and Ne |
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Definition
| Na has a higher neutron-to-proton ratio than Ne |
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Term
| sodium chloride is least soluble in what |
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Definition
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Definition
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Definition
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| with chart, which ions could be present in solution at a concentration of .1 M |
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Definition
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Term
| what pure white crystalline solid dissolves in water to yeild a base and liberate gas when acid is added to it |
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Definition
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Term
| mixture is made by adding AgNO3 to Na2CrO4, what does it look like |
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Definition
| yellow before, red precipitate |
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Term
| precipitate made when AgNO3 is added to Na2CrO4 |
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Definition
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Term
| compare Cl zero and Cl negative |
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Definition
| Cl zero atom contains fewer electrons than the Cl negative ion |
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Definition
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Definition
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Term
| greatest difference between its first and second ionization energies |
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Definition
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Definition
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| wavelength of sodium light |
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Definition
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Term
| energy of photon of red light |
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Definition
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Term
| ionic equation for NaCl +AgNO3= NaNO3+ AgCl |
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Definition
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Definition
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Definition
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Term
| precipitate formed from ammonium phosphate and calcium sulfate |
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Definition
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Term
| orbital designation for an electron with n=4 and L=3 |
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Definition
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Term
| electron configuration that isn't possible |
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Definition
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Term
| not possible configuration for an atom in excited state |
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Definition
| 1s^2 2s^2 2p^6 3s^2 3p^6 3d^10 4s^2 |
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Definition
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| electron affinity equation |
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Definition
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Definition
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Definition
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Definition
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Definition
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| empirical formula of CH2 and mass of 83.5 what is molecular formula |
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Definition
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Term
| empirical formula for compound made of carbon and hydrogen that is 14.3% H |
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Definition
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Term
| gram molar mass of Al(NO3)3 |
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Definition
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Term
| 2 L container will hold 4g of what |
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Definition
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Term
| 8g of N2H4 and 92g of N2O2 mixed, how much H2O is made |
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Definition
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Term
| propane burns in excess oxygen, what is coefficient of O2 |
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Definition
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Term
| volume of H2 when excess Mg is added to .4 M HCl |
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Definition
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Term
| volume of O2 required to react with excess CS2 to make 4 L of CO2 |
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Definition
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Term
| mass of CuSO4 with water required to make .1 M copper sulfate |
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Definition
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Term
| compound with 1.1 mole of K, .55 moles of Te and 1.65 moles of O |
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Definition
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Term
| partial pressure of SO2 in flask |
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Definition
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Term
| greatest rate of effusion through pinhole |
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Definition
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Term
| mass ratio of chromium to oxygen closest to 1.6 to 1 |
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Definition
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Term
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Definition
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Term
| change the boiling point of a liquid |
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Definition
| smaller container, more moles, higher altitude |
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Term
| info needed to calculate molarity |
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Definition
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Term
| formula for hydrocarbon with 1.88 density |
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Definition
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Term
| with info, density of sample is |
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Definition
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Term
| what gas effuses at half rate of NH3 |
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Definition
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Term
| mass of Au made when .05 moles of Au2S3 is reduced with excess H2 |
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Definition
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Term
| coefficient of O2 for C10H12O4S +O2= CO2 + H2O |
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Definition
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Term
| what happens to gas in tank when more oxygen is added |
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Definition
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Term
| empirical formula for 62.2% Hf and 37.4% Cl |
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Definition
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Term
| pressure of flask of NH4NO3 at 400 K |
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Definition
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Term
| percent water in hydrate Na2Co3 times 10H2O |
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Definition
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Term
| height of column of water of barometer |
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Definition
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Term
| object moves from moon to Earth |
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Definition
| mass will stay same and weight will increase |
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Term
| formula for Hydrogen arsenide |
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Definition
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Term
| when real gas is most like ideal gas |
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Definition
| low pressure and high temperature |
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Term
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Definition
| have no volume or attractive forces between them |
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