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Final Exam
Chemistry: The Central Science Ch. 1-13 (no 12)
76
Chemistry
Undergraduate 1
05/12/2009

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Term
Femto (f)
Definition
10-15
Term
Pico (p)
Definition
10-12
Term
Nano (n)
Definition
10-9
Term
Micro (µ)
Definition
10-6
Term
Mega (M)
Definition
106
Term
Giga (G)
Definition
109
Term
Convert Celcius to Fahrenheit
Definition
9/5(°C)+32
Term
Convert Fahrenheit to Celcius
Definition
5/9(°F-32)
Term
Difference between -ous and -ic in a cation
Definition

-ous = lower charge

-ic = higher charge

Term
Nonmetal cations have what nomenclature ending?
Definition
-ium
Term
Monatomic anions (and some simple polyatomic anions) have what nomenclature ending?
Definition
-ide
Term
Polyatomic anions containing oxygen (oxyanions) can have which nomenclature endings?
Definition
-ate most commonly, and -ite when there is one fewer oxygen atom but the same charge
Term
Which prefixes can oxyanions have?
Definition

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

Term
Anions derived by adding H+ to an oxyanion are named by adding which prefix(es)?
Definition
hydrogen or dihydrogen as appropriate
Term
Acids containing anions whose names end in -ide are named by
Definition
changing the -ide ending to -ic, adding the prefix hydro-, then following with the word "acid"
Term
Acids containing anions whose names end in -ate or -ite are named by
Definition
changing -ate to -ic or -ite to -ous, the adding the word "acid"
Term
Avogadro's number
Definition
6.02*1023
Term
Any metal on the activity series list can by oxidized by
Definition
the ions of elements -below- it
Term
Titration is
Definition
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.
Term
Equivalence point
Definition
the point in titration at which stoichiometrically equivalent quantities of reactants are brought together
Term
Kinetic energy =
Definition
1/2mv2 where v = speed
Term
Potential energy =
Definition
mgh, where g = gravitational constant (9.8m/s2)
Term
Electrostatic potential energy (between charged particles) =
Definition
kQ1Q2/d, where k = constant of proportionality (8.99*109) and Q1 and Q2 are the charges of the atoms
Term
work =
Definition

force * distance

also, -P * change in volume

Term
enthalpy (H) =
Definition
E + PV
Term
change in enthalpy =
Definition

change in energy + P * change in V

or

change in (E+PV)

or

the heat gained or lost at constant pressure

Term
heat capacity
Definition
amount of energy required to raise temp by 1 K
Term
specific heat
Definition

heat capacity of one gram of a substance

or

quantity of heat transferred/grams*change in temp

Term
heat of solution =
Definition
specific heat*grams*change in temp = negative heat of reaction
Term
heat of reaction =
Definition
negative heat capacity * change in temp
Term
Planck's constant
Definition

6.626*10-34

energy of photon=E=hv where h = Planck's constant

Matter can only emit energy in multiples of h

Term
Rydberg equation
Definition

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

Term
relationship of wavelength to momentum
Definition
wavelength = h/mv where h = Planck's constant and v = frequency
Term
Heisenberg's uncertainty principle
Definition

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)

Term
order for filling orbitals
Definition
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p
Term
effective nuclear charge =
Definition
number of protons - number of core electrons
Term
lattice energy
Definition
energy required to separate an ionic compound into its ions
Term
dipole moment
Definition

quantitative measurement of the magnitude of a dipole

Qr, where Q = charge and r = distance

Term
formal charge
Definition
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
Term
enthalpy of a reaction
Definition
energy of breaking bonds - energy of bonds made
Term
trigonal planar electron domain geometry
Definition

3 electron domains

120 degrees

Term
tetrahedral electron domain geometry
Definition

4 electron domains

109.5 degrees

Term
trigonal bipyramidal electron domain geometry
Definition

5 electron domains

120 degrees and 90 degrees

Term
octahedral electron domain geometry
Definition

6 electron domains

90 degrees

Term
bent molecular geometry
Definition
trigonal planar or trigonal pyramidal - 1
Term
trigonal pyramidal molecular geometry
Definition
tetrahedral - 1
Term
seesaw molecular geometry
Definition
trigonal bipyramidal - 1
Term
T-shaped molecular geometry
Definition
seesaw - 1
Term
square pyramidal molecular geometry
Definition
octahedral - 1
Term
square planar molecular geometry
Definition
square pyramidal - 1
Term
hybrid orbitals
Definition

count number of lobes on geometry

two = sp

three = sp2

four = sp3

five = sp3d

Term
bond order
Definition
1/2(# bonding electrons - # antibonding electrons)
Term
pressure =
Definition
force/area
Term
convert between units of pressure
Definition
1 atm = 760 mm Hg = 760 torr = 1.01325 * 105 Pa
Term
Boyle's law
Definition
PV=constant
Term
Charles' law
Definition
V/T=constant
Term
Avogadro's law
Definition
V/n=constant
Term
density of gas
Definition

P * molar mass (g/mol)

-----

RT

Term
average kinetic energy of gas molecules
Definition

1/2 * m * u2

where u is the root-mean-square speed, the speed of a molecule possessing average kinetic energy

Term
relationship of root-mean-square speed to molar mass and temp
Definition
u = square root of (3RT/molar mass)
Term
Graham's law of effusion
Definition

r1r2=square root of (molar mass1/molar mass2) = u1/u2

where r = rate of effusion

Term
van der Waals equation
Definition
(P + n2a/V2)(V - nb) = nRT
Term
combined gas law
Definition
P1V1/T1=P2V2/T2
Term
dispersion forces tend to increase in strength with
Definition
larger molecules
Term
Hydrogen bonding is between
Definition
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)
Term
molecular solid
Definition

made of atoms or molecules

London dispersion, dipole-dipole, and hydrogen

fairly soft, low to moderately high melting point, poor thermal and electrical conduction

Term
covalent-network solids
Definition

made of atoms

covalent bonds

very hard, very high melting point, variable thermal and electrical conduction

Term
ionic solids
Definition

made of positive and negative ions

electrostatic attractions

hard and brittle, high melting point, poor thermal and electrical conduction

Term
metallic solids
Definition

made of atoms

metallic bonds

soft to very hard, low to very high melting point, excellent thermal and electrical conduction, malleable and ductile

Term
Henry's law
Definition
solubility of gas in liquid = Henry's law constant * partial pressure of gas over solution
Term
parts per million or billion
Definition
mass of component in solution/total mass of solution * 106 or *109
Term
molality
Definition
moles of solute/kilograms of solvent
Term
colligative properties
Definition
depend on collective effect of number of solute particles
Term
Raoult's law
Definition
partial pressure of solvent vapor above solution = mole fraction of solvent in solution * vapor pressure of pure solvent
Term
increase in boiling point by solute or decrease in freezing point by solute =
Definition
molality * molal boiling-point-elevation constant or molal freezing-point-depression constant
Term
osmotic pressure =
Definition
(n/V)RT
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