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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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This is a study tool. The 3 wrong answers for each question are randomly chosen from answers to other questions. So, you might find at times the answers obvious, but you will see it re-enforces your understanding as you take the test each time.

1. PO4³?
Quantum Model
base
phosphate
alkane

2. How to Find an Empirical Formula Given Percentages
different # of neutrons
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Solvent
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

3. AX4E
Aufbau Principle
violet
specific heat
seesaw

4. STP
endless
v3kT/m
phosphate
0 degrees C - 1 atm

5. Describe various properties of one orbital
Quantum Numbers
M = square root (3RT/mm)
0 degrees C - 1 atm
Volt

6. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
m (third quantum number)
Percent Yield
strong acids
Theoretical yield

7. CN¹?
methoxy-
6.63x10?³4Js
cyanide
Ideal Gas Law

8. Experimental yield/theoretical yieldx100
Bases
soluble
% yield
Effusion

9. H?+NH3?NH4
nitrate
3rd law of thermodynamics
Strong acid weak base rxn
Counterions

10. AX3
Covalently w/in themselves - Ionicly bonded w/ each other
catalyst
trigonal planar
diamagnetic

11. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Acid + Base --> Salt + Water
endless
Thermochemistry
Force = mass x acceleration

12. Color of K (flame test)
see-saw
purple
Cg=kPg
Colligative properties

13. AX4E2
Amino-
square planar
purple
see-saw

14. OIL RIG
Reducing Agent
Oxidation is Loss Reduction is Gain
strong acids
endothermic

15. Kinetic Energy is proportional to ______
Second-Order Rate Law
Temperature
Arrhenius base
Radioactivity

16. Spectrum of light when an electron drops to energy level n=2
Molarity
Trigonal Planar
yellow --> green
Balmer Series

17. (organics) one carbon
Thermochemistry
meth-
Temperature
permanent gases

18. Mols A/ total mols - XA
mol Fraction
Normality
Integrated Rate Law
-2 - with peroxide -1

19. Similar to atomic orbitals - except between molecules
Percent Yield
Pressure
electrolyte
Molecular Orbitals (MOs)

20. Group 2 metals
1 atm = 760 mmHg = 101.3 kPa
Alkaline earth metals
Molecular Orbitals (MOs)
chromate

21. l=1
Dipole-dipole forces
3rd law of thermodynamics
Coordination Compound
p

22. Expresses how the concentrations depend on time
triple point
allotrope
Integrated Rate Law
Amphoteric

23. Verticals on the periodic table
Pauli Exclusion Principle
analyte
Bronsted-Lowry base
group

24. Faraday's constant
96500
perchlorate
Volume Metric Flask & Pipet
Standard Temperature and Pressure

25. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
activation energy
Theoretical yield
Formal Charge
Law of Conservation of Mass

26. Non-Ideal Gas Conditions
Aufbau Principle
high pressure - low temperature
boiling point
End Point

27. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
rate
P of a =(X of a)(total pressure)
f
Ideal Gas Law

28. C=2.9979*10^8 m/s
Integrated Zero-Order Rate Law
Boltzmann distribution
Speed of light
Tetrahedral

29. This MUST be determined experimentally
experimental yield
linear
rate law
% error

30. H+ Acceptor
Bronsted-Lowry Base
Acid + Base --> Salt + Water
complex ions
First-Order Half Life

31. Heat required to raise the system 1°C
endless
heat capacity
conjugate base
exothermic

32. Ester suffix
activation energy
-oate
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
oxidation

33. AX5E
Diffusion
Chemical Kinetics
Atomic Mass Unit
square pyramidal

34. Does the same as equilibrium expression - except it uses initial concentrations
trigonal planar
analyte
Constant Volume
Reaction Quotient (Q)

35. Thickness
octahedral
Delta H or Enthalpy Change
Trigonal Bipyramidal
viscosity

36. F¹?
Bases
Increase Temperature
flouride
-oic acid

37. H?+OH??H2O
mol
strong acid strong base rxn
isothermal
cyanide

38. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
Molecular Compounds
Adding
triple point
Second-Order Half Life

39. How to Balance a Redox Equation
Hund's Rule
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
Buffer
p+

40. Horizontals on the periodic table
freezing
hydrolysis
Standard Temperature and Pressure
period

41. The part of the universe one is focused upon (in thermodynamics)
Solubility Product (Ksp)
Molecular
pent-
system

42. Electron (symbol)
e-
but-
Trigonal Bipyramidal
group

43. Cl¹?
yellow --> green
chloride
Equilibrium constant
octahedral

44. Osmotic pressure=MRT
Osmotic Pressure
alkyne
C=(mass)(specific heat)
v3RT/M(in kg)

45. Oxidation # of free elements
Allotrope
0
Hydrogen bonding
Temperature

46. Absorbs/takes in heat (positive value)
amine
Endothermic
6.63x10?³4Js
pi=(nRT)/v

47. A device used to measure Delta H
nitrate
period
M1V1=M2V2
Calorimeter

48. Point at which solid?liquid occurs
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
melting point
conjugate base
endless

49. [A]0/2k
N=N.(0.5)^time/time half-life
Zero-Order Half Life
Polar Covalent
bromate

50. E=mc^2
Theory of Relativity
Surroundings
Sigma Bond
heat of fusion