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AP Chemistry

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Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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1. Absorbs/takes in heat (positive value)
permanganate
square planar
Endothermic
Molecular

2. A device used to measure Delta H
Calorimeter
v3kT/m
reduction
Anode

3. Pure metal or metal hydride + H20 ->
base and hydrogen gas
Ag+ - Pb2+ - Hg2+
% yield
8.314 J/K mol

4. (A) - C/s
flouride
Ampere
trigonal planar
Matter

5. AX4E2
Electron Spin Quantum Number
square planar
r1/r2
Root Mean Square Velocity

6. R in ideal gas law
moles solute/kg solvent
0.0821 atm L/mol K
Boltzmann distribution
actual yield/theoretical yield x 100%

7. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
log[H+]
Bonding Pairs
bent

8. ln[A]=-kt + ln[A]0
blue-green
Integrated First-Order Rate Law
Acids
Force = mass x acceleration

9. Elements on staircase on periodic table
oxide gas and water
Metalliods
ionic
Nernst Equation

10. Speed of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm A/ mm B)
bromate
Ionic Compounds
hydrolysis

11. NH4¹?
Equilibrium constant
ammonium
P1V1/N1T1=P2V2/N2T2
Adding

12. Negative enthalpy - heat flows into surroundings
3/2RT
exothermic
carbohydrates
fusion

13. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
surroundings
London Dispersion Forces
Increase Temperature
Bases

14. U(rms)=(3RT/M)^1/2
Specific Heat Capacity
blue-green
Root Mean Square Velocity
Oxidation is Loss Reduction is Gain

15. Unusually strong dipole forces found when H is bonded to N - O - or F
Law of Conservation of Energy
Hund's Rule
methoxy-
Hydrogen bonding

16. Forward rxn occurs when
Closed System
are not
m (third quantum number)
Q<K

17. How to Find an Empirical Formula Given Percentages
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
viscosity
a precipitate forms
Hund's Rule

18. Stronger IMF= lower... weaker IMF= higher...
ionic
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
vapor pressure
Oxidation is Loss Reduction is Gain

19. The reactant that is being reduced - brings about oxidation
4.184
Balmer Series
Density
oxidizing agent

20. AX5
trigonal bipyramidal
Strong acid weak base rxn
bent
experimental yield

21. High-energy light
P1V1/N1T1=P2V2/N2T2
chlorite
Gamma Ray-
Its root and adding -ide

22. Mols A/ total mols - XA
cyanide
mol Fraction
Hund's Rule
X of a = moles a/total moles

23. Universal IMF for nonpolar molecules
heat capacity
rate
London dispersion forces
Isotopes

24. Change without heat transfer between the system and its surroundings
0
adiabatic
Surroundings
AH

25. 1/[A] vs. time is a ...-order reaction
Integrated Zero-Order Rate Law
Ligand
Diffusion
second

26. Substances that form H+ when dissolved in water; proton donors
Bond enthalpy
?Hvap
Acids
melting point

27. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
excess reactant
f
0 degrees C - 1 atm
strong acids

28. Substance that - when dissolved - is conductive
2nd law of thermodynamics
8.314 J/K mol
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
electrolyte

29. Energy needed to break a bond
dec-
1atm=?Pa
bond energy
Resonance

30. Half cell in which reduction occurs
Constant Volume
cathode
Hybridization
oxidizing agent

31. Mass/volume
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
Density
Nernst Equation
analyte

32. This MUST be determined experimentally
boiling point
rate law
Hydrogen bonding
square pyramidal

33. Oxidation # of Halogens
Amount of atoms present
yellow --> green
H
-1

34. If heat capacity isn't mentioned - you can assume that q of cal is = ?
s orbitals
0
d orbitals
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

35. Ptotal=P1+P2+P3+...

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36. Work = ?
adiabatic
-(P)(Change in V)
Van't Hoff factor
Hund's Rule

37. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
reduction agent
AE = q + w
Colligative properties
heat of fusion

38. Ketone suffix
Bronsted-Lowry base
-one
-ic acid
specific heat

39. AX4
tetrahedral
Valence Electrons(assigned)
2nd law of thermodynamics
hydroxide

40. Change that occurs at constant temperature
Force = mass x acceleration
Ligand
Its root and adding -ide
isothermal

41. ?Hsoln=?H1+?H2+?H3+...
-ic acid
Bronsted-Lowry acid
adhesion
Enthalpy of Solution

42. Molarity (M)
moles of solute/ L of solution
strong bases
Closed System
1/2mv²

43. Symbol for the heat absorbed or lost molecularly (PER MOLE)
activation energy
AH
charge
# protons + # neutrons

44. H + donor
Bronsted-Lowry Acid
force x distance = work done
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
triple point

45. Each orbital can hold two e?s each w/ opposite spins
are not
r1/r2
Pauli Exclusion Principle
acetate

46. A molecule having a center of positive charge and a center of negative charge
Metalliods
Ampere
Dipole Moment
-ol

47. Similar to atomic orbitals - except between molecules
Molecular Orbitals (MOs)
Q>K
conjugate base
Quantum Model

48. Actual Yield/Theoretical Yield*100%
Ampere
Percent Yield
lambda
solid CO2

49. Color of Li (flame test)
red
rate gas A/rate gas B = square root (mm A/ mm B)
Hydrogen bonding
Chemical Kinetics

50. Within a sublevel - place one e? per orbital before pairing them

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AP Chemistry

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