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Chem Final!!
Be afraid. Be very afraid.
191
Chemistry
10th Grade
06/12/2010

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Term
luminousintensity
Definition
candela (cd)
Term
mega-
Definition
(M) - Mm = 1E6 m
Term
deci-
Definition
(d) - dm = 1/10 m
Term
micro-
Definition
(μ) -μm = 1E-6 m
Term
nano-
Definition
(n) - nm = 1E-9 m
Term
pico-
Definition
(p) - pm = 1E-12 m
Term
femto-
Definition
(f) - fm = 1E-15 m
Term
Celsius to Fahrenheit conversion equation
Definition
°F = 9/5°C + 32
Term
Celsius to Kelvin conversion equation
Definition
K = °C + 273.15
Term
P
Definition
phosphorus
Term
Sc
Definition
scandium
Term
Mn
Definition
manganese
Term
Rb
Definition
rubidium
Term
Mo
Definition
molybdenum
Term
Sb
Definition
antimony
Term
Pt
Definition
platinum
Term
Hg
Definition
mercury
Term
Te
Definition
tellurium
Term
Ra
Definition
radium
Term
Be
Definition
beryllium
Term
Ti
Definition
titanium
Term
Cr
Definition
chromium
Term
Se
Definition
selenium
Term
Kr
Definition
krypton
Term
Sr
Definition
strontium
Term
Sn
Definition
tin
Term
Cs
Definition
cesium
Term
W
Definition
tungsten
Term
Rn
Definition
radon
Term
Th
Definition
thorium
Term
NH3
Definition
ammonia
Term
NH4+
Definition
ammonium
Term
C2H3O2-
Definition
acetate
Term
MnO4-
Definition
permanganate
Term
hypo ~ ite
Charge?
How many O atoms?
Definition
-1
1
Term
~ ite
Charge?
How many O atoms?
Definition
-1
2
Term
~ ate
Charge?
How many O atoms?
Definition
-1
3
Term
per ~ ate
Charge?
How many O atoms?
Definition
-1
4
Term
IO3-
Definition
iodate
Term
BrO3-
Definition
bromate
Term
CO3-2
Definition
carbonate
Term
O2-2
Definition
peroxide
Term
CrO4-2
Definition
chromate
Term
Cr2O7-2
Definition
dichromate
Term
SO3-2
Definition
sulfite
Term
SO4-2
Definition
sulfate
Term
C2O4-2
Definition
oxalate
Term
C4H4O2-2
Definition
tartrate
Term
PO4-3
Definition
phosphate
Term
SCN-
Definition
thiocyanate
Term
Group I
Definition
Alkali Metals
Term
Group II
Definition
Alkaline Earth Metals
Term
Group III
Definition
Boron Family
Term
Group IV
Definition
Carbon Family
Term
Group V
Definition
Nitrogen Family
Term
Group VI
Definition
Oxygen Family
Term
Group VII
Definition
Halogen Family
Term
Group VIII
Definition
Noble Gases
Term
Electron
Charge?
Mass?
Definition
-1
~1/1837 amu
Term
Proton
Charge?
Mass?
Definition
+1
1 amu
Term
Neutron
Charge?
Mass?
Definition
No charge
1 + ~ 1/1837 amu
Term
Neutron
Charge?
Mass?
Definition
No charge
1 + ~ 1/1837 amu
Term
(A / Z) X

What do each stand for? (X is supposed to be very large, and A and Z should actually be over one another.)
Definition
A- mass number (protons + neutrons)
Z- atomic number (protons)
X- element symbol
Term
Mercury (I)
Definition
Hg2+2
Term
Mercury (II)
Definition
Hg+2
Term
Silver ion
Definition
Ag+
Term
Zinc ion
Definition
Zn+2
Term
Nickel ion
Definition
Ni+2
Term
Formula for determining average atomic mass
Definition
Average atomic mass = [(isotopic mass)(relative abundance %) + ...]
Term
How to Find An Empirical Formula (Given the Masses of Several Elements)
Definition
1. Find how many moles there are of each element
2. Divide all the mole amounts by the smallest mole amount.
3. The quotient for a given element is how many atoms of it are in the empirical formula.
Term
How to Find the Limiting Reactant
Definition
1. Get a balanced equation.
2. Using stoichiometry, determine which reactant produces fewer moles of one of the products. This is the limiting reactant.
3. To determine how much is left of the non-limiting reactant, find how much of the non-limiting reactant is required to fully react with the limiting reactant. Subtract this amount from the original amount of the non-limiting reactant.
Term
mono-
Definition
1
Term
di-
Definition
2
Term
tri-
Definition
3
Term
tetra-
Definition
4
Term
penta-
Definition
5
Term
hexa-
Definition
6
Term
hepta-
Definition
7
Term
octa-
Definition
8
Term
meth-
Definition
1 carbon
Term
eth-
Definition
2 carbons
Term
prop-
Definition
3 carbons
Term
but-
Definition
4 carbons
Term
pent-
Definition
5 carbons
Term
hex-
Definition
6 carbons
Term
hept-
Definition
7 carbons
Term
oct-
Definition
8 carbons
Term
non-
Definition
9 carbons
Term
dec-
Definition
10 carbons
Term
-ane
Definition
# hydrogens = 2(# carbons) + 2
Term
-ene
Definition
# hydrogens = 2(# carbons)
Term
-yne
Definition
# hydrogens = 2(# carbons) - 2
Term
Non Oxoacid
Definition
hydro ~ ic acid
Term
Oxoacid
Definition
polyatomic prefix + [(ate --> ic) or (ite --> ous)] acid
Term
Metal oxide + H2O -->
Definition
Metal hydroxide
Term
Metal oxide + CO2 -->
Definition
Metal carbonate
Term
Metal chloride + O2 -->
Definition
Metal chlorate
Term
(Group I or II Metal) + H20 -->
Definition
Metal hydroxide + H2
Term
(Other Metals) + H2O -->
Definition
Metal oxide + H2
Term
Avogadro Constant
Definition
1 mole = 6.02E23 atoms/molecules
Term
1 mole gas at STP = ___ L
Definition
22.4
Term
___ torr = ___ atm = ___ kPa
Definition
760 torr (mmHg) = 1 atm = 101.325 kPa
Term
Charles' Law
Definition
P = KT
V1/T1 = V2/T2
Term
Boyle's Law
Definition
PV = K
P1V1 = P2V2
Term
Combined Gas Law
Definition
PV = KT
P1V1/T1 = P2V2/T2
Term
Ideal Gas Law
Definition
PV = nRT
P (atm)
V (L)
n (mol)
R - .0821 L*atm / mol * K
T (K)
Term
Formula for the density of a gas
Definition
density = P * molar mass / RT
Term
Ideal Gas Constant
Definition
R - .0821 L*atm / mol * K
Term
Graham's Law
Definition
rate 1 / rate 2 = SQUARE ROOT (molar mass 2 / molar mass 1)
Term
Equation for q (using specific heat)
Definition
q = m * Cp * ΔT
Term
Specific Heat of Water
Definition
4.18 J / g * °C
Term
Equation for q (using the heat of fusion or vaporization)
Definition
q = m * ΔH(fusion or vaporization)
Term
Heat of Fusion of Water
Definition
334 J/g for H2O fusion
Term
Liquid --> Solid
Definition
Freezing
Term
Solid --> Liquid
Definition
Melting
Term
Liquid --> Gas
Definition
Vaporization
Term
Solid --> Gas
Definition
Sublimation
Term
Gas --> Liquid/Solid
Definition
Condensation
Term
A + BX --> AX + B will occur if...
Definition
A is more reactive than B.
Term
A double replacement reaction will only occur if...
Definition
It yields a precipitate.
Term
c = ___ = ___ * ___
Definition
c = 3.00E8 m/s = νλ
Term
ν (nu)
Definition
frequency (Hz or s-)
Term
λ (lambda)
Definition
wavelength (m)
Term
Equation to Calculate the Energy of a Photon
Definition
Ephoton = hν
Term
Planck's Constant
Definition
h = 6.62E-34 J*s
Term
n = 1
Definition
Ground State
Term
n > 1
Definition
Excited State
Term
n
Name?
Values?
Meaning?
Definition
Principal Quantum Number
Integers
Determines which electron shell
Term
l
Name?
Values?
Meaning?
Definition
Angular Momentum
From 0 to (n-1)
Determines which subshell
Term
l = 0
Letter?
Shape?
Definition
s
sphere
Term
l = 1
Letter?
Shape?
Definition
p
peanut
Term
l = 2
Letter?
Shape?
Definition
d
too complicated
Term
l = 3
Letter?
Shape?
Definition
f
just no
Term
ml
Name?
Values?
Meaning?
Definition
Magnetic Quantum Number
From -l to l (0 included)
Determines which orbital in the subshell
Term
ms
Name?
Values?
Meaning?
Definition
Magnetic Spin Number
1/2 or -1/2
Determines spin up or spin down
Term
Pauli Exclusion Principle
Definition
No two electrons around the same nucleus can have the exact same combination of n, l, ml, and ms-- at least ms has to be different
Term
Aufbau Principle
Definition
Fill lowest orbitals first
Term
Hund's Rule
Definition
Electrons prefer to be unpaired
Term
Electron Configuration of Cr
Definition
[Ar] 4s1 3d5
NOT [Ar] 4s2 3d4
Term
Electron Configuration of Cu
Definition
[Ar] 4s1 3d10
NOT [Ar] 4s2 3d9
Term
isoelectronic
Definition
same electron configuration, different elements
Example: F-, Ne, Na+
Term
Zeff
Definition
Effective nuclear charge; increases going down vertically, increases going right horizontally
Term
Atomic size
Definition
Increases going down vertically, increases going left horizontally
Term
Electron Affinity (EA)
Definition
Ability of atom to trade one electron; increases going down vertically, increases going left horizontally... however, the more negative the EA, the better the atom can trade one electron, which means the element with the smallest EA value (in the upper right-hand corner) is most able to trade one electron
Term
Ionization Energy (IE)
Definition
Energy required to remove one electron from an atom; increases going up vertically, increases going right vertically
Term
Electronegativity (EN)
Definition
Ability of atom to attract an electron in a bond; increases going up vertically, increases going right vertically
Term
nonpolar covalent bond
Definition
no difference in EN
Example: F -- F
Term
polar covalent bond (dipole moment)
Definition
slight difference in EN
Example: H (~+) -- F (~-)
Term
ionic bonding
Definition
large difference in EN
Example: Li (+) -- F (-)
Term
Electron Pairs (Total/Bonding/Lone):
2 / 2 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
linear
180°
sp
np
Term
Electron Pairs (Total/Bonding/Lone):
3 / 3 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
trigonal planar
120°
sp2
np
Term
Electron Pairs (Total/Bonding/Lone):
3 / 2 / 1
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
bent
<120°
sp2
p
Term
Electron Pairs (Total/Bonding/Lone):
4 / 4 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
tetrahedral
109.5°
sp3
np
Term
Electron Pairs (Total/Bonding/Lone):
4 / 3 / 1
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
trigonal pyramidal
<109.5°
sp3
p
Term
Electron Pairs (Total/Bonding/Lone):
4 / 2 / 2
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
bent
<<109.5°
sp3
p
Term
Electron Pairs (Total/Bonding/Lone):
5 / 5 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
trigonal bipyramidal
180° / 120° / 90°
sp3d
np
Term
Electron Pairs (Total/Bonding/Lone):
5 / 4 / 1
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
see-saw
180° / <120° / 90°
sp3d
p
Term
Electron Pairs (Total/Bonding/Lone):
5 / 3 / 2
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
T-shaped
180° / 90°
sp3d
p
Term
Electron Pairs (Total/Bonding/Lone):
5 / 2 / 3
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
linear
180°
sp3d
np
Term
Electron Pairs (Total/Bonding/Lone):
6 / 6 / 0
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
octahedral
180° / 90°
sp3d2
np
Term
Electron Pairs (Total/Bonding/Lone):
6 / 5 / 1
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
square pyramidal
180° / 90°
sp3d2
p
Term
Electron Pairs (Total/Bonding/Lone):
6 / 4 / 2
Geometry?
Bond Angle[s]?
Hybridization?
Polarity?
Definition
square planar
180° / 90°
sp3d2
np
Term
The addition of solutes...
Definition
Lowers the vapor pressure, which elevates the boiling point and depresses the freezing point
Term
Freezing or Boiling Point Equation
Definition
ΔT(b or f) = K(b or f) * m * i
K(b or f) --> a constant
m --> molality (moles solute / kg solvent)
i --> Van't Hoff Factor, or the number of particles the solute dissociates into in solution (i = 1 for hydrocarbons)
Term
Van der Waals Forces
Definition
dipole - dipole
dipole - dipole induced
London Forces (up mass, up LF)
Term
hydrogen "bonding"
Definition
H is attached to F, O, N
Term
Rate Law Expression
Definition
Rate = k[A]^n
Term
The Driving Force Behind Chemical Reactions!
(An Equation)
Definition
ΔG = ΔH - TΔS
Term
-ΔG -->
+ΔG -->
Definition
spontaneous
non-spontaneous
Term
-ΔH -->
+ΔH -->
Definition
exothermic
endothermic
Term
-ΔS -->
+ΔS -->
Definition
orderly
chaotic
Term
Hess's Law
Definition
ΔH = SUM(ΔH of products) - SUM(ΔH of reactants)
Term
Equilibrium Expression
Definition
Keq = [products]^coefficients / [reactants]^coefficients
Term
Raise the pressure and shift...
Definition
To the side with fewer gas molecules
Term
Lower the pressure and shift...
Definition
To the side with more gas molecules
Term
Arrhenius acid
Definition
Produces H3O+ in H20
Term
Arrhenius base
Definition
Produces OH- in H2O
Term
Bronsted-Lowry acid
Definition
Proton (H+) donor
Term
Bronsted-Lowry base
Definition
Proton (H+) acceptor
Term
Lewis acid
Definition
Electron pair acceptor
Term
Lewis base
Definition
Electron pair donor
Term
Kw = [H3O+][OH-] = ___
Definition
1E-14
Term
pH = ___
Definition
-log[H3O+]
Term
Ka (strong acid) = ___
Definition
Very large
Term
Four strong acids TYNTK
Definition
HCl, HClO4, HNO3, H2SO4
Term
With acids, the equilibrium always shifts to the side with...
Definition
The weaker acid
Term
John Dalton (Credit to RK)
Definition
"captain obvious" (he basically took the obscured findings of previous scientists/philosophers and mashed them into his encompassing theory)
THEORY... 1) all elements are composed of atoms (which are indivisible and indestructable), 2) all atoms of the same element are alike 3) atoms of different elements are different 4) compounds are formed by combinations of atoms in a whole # ratio
Model - single, solid, circular blob
Term
JJ Thomson (Credit to RK)
Definition
took Crooke's tube (cathode ray tube) and improved upon his findings to observe particles (later dubbed and therefore discovered as "electrons")
Model - "plum pudding" model (positively charged aura of sorts with electrons floating around inside)
Term
Robert Miliken (Credit to RK)
Definition
oil drop experiment; he ionized drops of oil and tried to suspend them against gravity and messed around with charges and stuff... he eventually discovered the charge of the electron (1.602E-19 but we don't have to know that)
Model - "plum pudding" model (positively charged aura of sorts with electrons floating around inside)
Term
Somethingfirstname Rutherford (Credit to RK)
Definition
gold foil experiment; he shot particles at a section of gold foil and observe their deflection... and concluded that they were bouncing off of a central, positively charged nucleus (and therefore discovered protons)
Model - planetary model (electrons encircling the positive nucleus)
Term
Neils Bohr (Credit to RK)
Definition
wondered why electrons weren't immediately attracted into the nucleus. He decided that there were shells surrounding the atom that electrons orbited in with different energy states. He quantized the atom with a gas discharge tube.
Model - Bohr - shell model (protons in center with orbits of electrons surrounding)
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