Chemistry Final Exam Questions And Answers – Flashcards
Unlock all answers in this set
Unlock answers| Femto (f) |
| 10-15 |
| Pico (p) |
| 10-12 |
| Nano (n) |
| 10-9 |
| Micro (µ) |
| 10-6 |
| Mega (M) |
| 106 |
| Giga (G) |
| 109 |
| Convert Celcius to Fahrenheit |
| 9/5(°C)+32 |
| Convert Fahrenheit to Celcius |
| 5/9(°F-32) |
| Difference between -ous and -ic in a cation |
-ous = lower charge -ic = higher charge |
| Nonmetal cations have what nomenclature ending? |
| -ium |
| Monatomic anions (and some simple polyatomic anions) have what nomenclature ending? |
| -ide |
| Polyatomic anions containing oxygen (oxyanions) can have which nomenclature endings? |
| -ate most commonly, and -ite when there is one fewer oxygen atom but the same charge |
| Which prefixes can oxyanions have? |
per- when there is one more oxygen atom than the oxyanion ending in -ate hypo- when there is one fewer oxygen atom than the oxyanion ending in -ite |
| Anions derived by adding H+ to an oxyanion are named by adding which prefix(es)? |
| hydrogen or dihydrogen as appropriate |
| Acids containing anions whose names end in -ide are named by |
| changing the -ide ending to -ic, adding the prefix hydro-, then following with the word "acid" |
| Acids containing anions whose names end in -ate or -ite are named by |
| changing -ate to -ic or -ite to -ous, the adding the word "acid" |
| Avogadro's number |
| 6.02*1023 |
| Any metal on the activity series list can by oxidized by |
| the ions of elements -below- it |
| Titration is |
| combining a sample of a solution with a standard solution that it will react with. For instance, taking an unknown concentration of HCl, reacting it with a known concentration of NaOH, and seeing how much salt/water is made. |
| Equivalence point |
| the point in titration at which stoichiometrically equivalent quantities of reactants are brought together |
| Kinetic energy = |
| 1/2mv2 where v = speed |
| Potential energy = |
| mgh, where g = gravitational constant (9.8m/s2) |
| Electrostatic potential energy (between charged particles) = |
| kQ1Q2/d, where k = constant of proportionality (8.99*109) and Q1 and Q2 are the charges of the atoms |
| work = |
force * distance also, -P * change in volume |
| enthalpy (H) = |
| E + PV |
| change in enthalpy = |
change in energy + P * change in V or change in (E+PV) or the heat gained or lost at constant pressure |
| heat capacity |
| amount of energy required to raise temp by 1 K |
| specific heat |
heat capacity of one gram of a substance or quantity of heat transferred/grams*change in temp |
| heat of solution = |
| specific heat*grams*change in temp = negative heat of reaction |
| heat of reaction = |
| negative heat capacity * change in temp |
| Planck's constant |
6.626*10-34 energy of photon=E=hv where h = Planck's constant Matter can only emit energy in multiples of h |
| Rydberg equation |
1/wavelength = (Rydberg constant)*(1/n12 - 1/n22) where Rydberg's constant = 1.097*107 and n1 and n2 are the principle quantum numbers, with n2 being larger than n1 |
| relationship of wavelength to momentum |
| wavelength = h/mv where h = Planck's constant and v = frequency |
| Heisenberg's uncertainty principle |
uncertainty of position * uncertainty (change in) mv is greater than or equal to h/4π Therefore, to find the uncertainty of position, do h/(4πm * change in v) |
| order for filling orbitals |
| 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p |
| effective nuclear charge = |
| number of protons - number of core electrons |
| lattice energy |
| energy required to separate an ionic compound into its ions |
| dipole moment |
quantitative measurement of the magnitude of a dipole Qr, where Q = charge and r = distance |
| formal charge |
| find the number of electrons on the Lewis structure of that atom that are either bonded or nonbonded, then subtract the number of electrons the atom usually has by the Lewis structure electrons |
| enthalpy of a reaction |
| energy of breaking bonds - energy of bonds made |
| trigonal planar electron domain geometry |
3 electron domains 120 degrees |
| tetrahedral electron domain geometry |
4 electron domains 109.5 degrees |
| trigonal bipyramidal electron domain geometry |
5 electron domains 120 degrees and 90 degrees |
| octahedral electron domain geometry |
6 electron domains 90 degrees |
| bent molecular geometry |
| trigonal planar or trigonal pyramidal - 1 |
| trigonal pyramidal molecular geometry |
| tetrahedral - 1 |
| seesaw molecular geometry |
| trigonal bipyramidal - 1 |
| T-shaped molecular geometry |
| seesaw - 1 |
| square pyramidal molecular geometry |
| octahedral - 1 |
| square planar molecular geometry |
| square pyramidal - 1 |
| hybrid orbitals |
count number of lobes on geometry two = sp three = sp2 four = sp3 five = sp3d |
| bond order |
| 1/2(# bonding electrons - # antibonding electrons) |
| pressure = |
| force/area |
| convert between units of pressure |
| 1 atm = 760 mm Hg = 760 torr = 1.01325 * 105 Pa |
| Boyle's law |
| PV=constant |
| Charles' law |
| V/T=constant |
| Avogadro's law |
| V/n=constant |
| density of gas |
P * molar mass (g/mol) ----- RT |
| average kinetic energy of gas molecules |
1/2 * m * u2 where u is the root-mean-square speed, the speed of a molecule possessing average kinetic energy |
| relationship of root-mean-square speed to molar mass and temp |
| u = square root of (3RT/molar mass) |
| Graham's law of effusion |
r1r2=square root of (molar mass1/molar mass2) = u1/u2 where r = rate of effusion |
| van der Waals equation |
| (P + n2a/V2)(V - nb) = nRT |
| combined gas law |
| P1V1/T1=P2V2/T2 |
| dispersion forces tend to increase in strength with |
| larger molecules |
| Hydrogen bonding is between |
| the hydrogen atom in a polar bond (particularly H-F, H-O, or H-N) and nonbonding electron pair on a nearby small electronegative ion or atom (usually an F, O, or N in another molecule) |
| molecular solid |
made of atoms or molecules London dispersion, dipole-dipole, and hydrogen fairly soft, low to moderately high melting point, poor thermal and electrical conduction |
| covalent-network solids |
made of atoms covalent bonds very hard, very high melting point, variable thermal and electrical conduction |
| ionic solids |
made of positive and negative ions electrostatic attractions hard and brittle, high melting point, poor thermal and electrical conduction |
| metallic solids |
made of atoms metallic bonds soft to very hard, low to very high melting point, excellent thermal and electrical conduction, malleable and ductile |
| Henry's law |
| solubility of gas in liquid = Henry's law constant * partial pressure of gas over solution |
| parts per million or billion |
| mass of component in solution/total mass of solution * 106 or *109 |
| molality |
| moles of solute/kilograms of solvent |
| colligative properties |
| depend on collective effect of number of solute particles |
| Raoult's law |
| partial pressure of solvent vapor above solution = mole fraction of solvent in solution * vapor pressure of pure solvent |
| increase in boiling point by solute or decrease in freezing point by solute = |
| molality * molal boiling-point-elevation constant or molal freezing-point-depression constant |
| osmotic pressure = |
| (n/V)RT |
