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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. C2O4²?
Dipole-dipole forces
oxalate
Mass
Heisenberg Uncertainty Principle

2. Phase change from solid to gas
sublimation
Hund's Rule
1/2mv²
catalyst

3. OH¹?
% yield
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
strong acid strong base rxn
hydroxide

4. If anion ends in -ite - acid name ends in...
Lone Pair
alcohol
System
-ous acid

5. ?T=k*m(solute)
charge
Zero-Order Rate Law
Molal FP Depression Constant
Allotrope

6. Proton acceptors - must have an unshared pair of e?s
oxalate
Bronsted-Lowry base
Electronegativity
Pressure of H2O must be Subtracted

7. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Atmospheric Pressure
Antibonding Molecular Orbital
Diffusion
-oate

8. Type of system in which the energy and mass may leave or enter
reduction agent
pi=(nRT)/v
Open System
Formal Charge

9. K
Law of Conservation of Mass
Force = mass x acceleration
amine
Equilibrium constant

10. The measurement of heat changes
s
sublimation
octahedral
Calorimetry

11. ln[A]=-kt + ln[A]0
Integrated First-Order Rate Law
Magnetic Quantum Number (ml)
Hund's Rule
Le Chatelier's Principle

12. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Ionic Compounds
1atm=?mmHg/Torr
insoluble
Heisenberg Uncertainty Principle

13. Ka=[products]^m/[reactants]^n
Molal BP Elevation Constant
N=N.(0.5)^time/time half-life
Acid Dissociation Constant
Coordination Compound

14. Symbol for the heat absorbed or lost molecularly (PER MOLE)
22.4L
AH
Principal Quantum Number
weak acid strong base rxn

15. l=1
Naming Binary Ionic Compounds
Pi Bond
p
System

16. frequency symbol
cathode
nu
strong acid strong base rxn
STP

17. ?T=k*m(solute)
d
Molal BP Elevation Constant
bromate
AE = q + w

18. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Nodes
m (third quantum number)
Acid + Base --> Salt + Water
?Tf= kf x molality

19. q cal = ?
CAT
0.0826Latm/Kmol
Ionic
double bond

20. A molecule having a center of positive charge and a center of negative charge
Effusion
specific heat
reduction agent
Dipole Moment

21. Elements on staircase on periodic table
Heisenberg Uncertainty Principle
third
1atm=?mmHg/Torr
Metalliods

22. Peak of energy diagram
activated complex (transition state)
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
high pressure - low temperature
Increase Temperature

23. Force per unit area
Hund's Rule
Pressure
-al
Molal BP Elevation Constant

24. Organic w/ -NH2
v3RT/M(in kg)
Arrhenius equation
amine
work

25. Lowers activation energy
catalyst
moles solute/kg solvent
Molar Heat Capacity
heat capacity

26. ?Hsoln=?H1+?H2+?H3+...
Enthalpy of Solution
Oxidizing Agent
Trigonal Bipyramidal
vaporization

27. Point at which the titrated solution changes color
Exothermic
Alkaline earth metals
end point
p orbitals

28. Ptotal=P1+P2+P3+...

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29. Specific heat of water
adiabatic
rate gas A/rate gas B = square root (mm A/ mm B)
Negative work value; work done by system
4.184

30. Generally insoluble anions (names)
chlorate
phosphate - sulfide - carbonate - sulfate
A Roman numeral
Covalently w/in themselves - Ionicly bonded w/ each other

31. Variable for spin of electron (+.5 or -.5)
vaporization
analyte
Molarity
s (fourth quantum number)

32. Entropy in the universe is always...
n (first quantum number)
Formal Charge
increasing
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

33. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Boltzmann distribution
q/moles
Speed of light
Sigma Bond

34. U(rms)=(3RT/M)^1/2
Thermochemistry
Trigonal Bipyramidal
sulfite
Root Mean Square Velocity

35. r=k[A]
First-Order Rate Law
Linear
purple --> pink
Arrhenius Acid

36. (N) number of equivalents per liter of solution
4.184
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
C=(mass)(specific heat)
Normality

37. l=3
f
Heisenberg Uncertainty Principle
heat capacity
H

38. Reverse rxn occurs when
Q>K
Equivalence Point
Matter
titrant buret

39. Positive enthalpy - heat flows into system
endothermic
Calorimeter
PV=nRT
Monoprotic

40. 760 mmHg - 760 torr
methoxy-
-ous acid
0
1 atm

41. A given compound always has exactly the same proportion of elements by mass
Second-Order Half Life
g solute/g solvent x 100
Law of Definite Proportion
log[H+]

42. Diatomic Molecules
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
wavelength
Ampere
zero

43. Solid to liquid
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
melting
(moles of products that are gasses) - (moles of reactants that are gasses)
purple

44. 101 -325 Pa
Le Chatelier's Principle
zero
1atm=?Pa
endless

45. AX4
Resonance
Q>K
tetrahedral
Molecular Orbitals (MOs)

46. When n=4 ->2 - color=
blue-green
moles of solute/ L of solution
like
voltaic cells

47. Connects the 2 half cells in a voltaic cell
eth-
t-shape
salt bridge
m (third quantum number)

48. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
Finding Empirical Formulas
Molarity
Adding
Mass

49. For significant digits - leading zeros ____ significant
Acid Dissociation Constant
1.86°C
t-shape
are not

50. 2+ charge
Alpha Particles-
t-shape
catalyst
Negative work value; work done by system

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AP Chemistry

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