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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. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
yellow --> green
conjugate base
boiling point
Molarity

2. Force that holds atoms together
Bond Order
Calorimetry
Beta Particles-
Chemical Bonds

3. ClO3²?
chlorate
Calorimetry
conjugate base
entropy

4. Boiling point elevation formula
nitrite
Solvent
electron affinity
?Tb= kb x molality

5. kf of water
Oxidizing Agent
1.86°C
complex ions
Root Mean Square Velocity

6. These orbitals are perpendicular
indicator
deposition
p orbitals
Solvent

7. ?T=k*m(solute)
Molal BP Elevation Constant
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
methoxy-
Ideal Gas Law

8. Organic w/ -OH group
sulfide
CAT
entropy
alcohol

9. Oxidation # of Halogens
Faraday
soluble
-1
Matter

10. What is defined by you taken from the whole universe
AE = q + w
Ag+ - Pb2+ - Hg2+
AH
System

11. Verticals on the periodic table
group
Law of Conservation of Mass
no precipitate forms
complex ions

12. Force acting over distance
viscosity
Bronsted-Lowry base
Work
pent-

13. q rxn = ?
-(q of H2O + q of cal)
1/2mv²
precipitate
London dispersion forces

14. A solid or gas that can be formed when 2 or more aqueous reactants come together
Acid Dissociation Constant
Quantum Numbers
precipitate
# protons + # neutrons

15. Effusion of a gas is inversely proportional to the square root of the molar mass

16. Combined Gas Law Formula
P1V1/N1T1=P2V2/N2T2
Heat Capacity (C)
Dalton's Law of Partial Pressures
base and hydrogen gas

17. Only contains ions that change in reaction
moles solute/kg solvent
octahedral
Net Ionic Equation
Open System

18. AX5E
Second-Order Half Life
spontaneous
p+
square pyramidal

19. [A]=-kt + [A]0
Integrated Zero-Order Rate Law
Molar Mass of Element/ Total Molar Mass %
Specific Heat (s)
Q<K

20. (A) - C/s
Hydrogen bonding
0
Ampere
Dalton's Law of Partial Pressures

21. HF+ OH??H2O
first
-(q of H2O + q of cal)
Chemical Kinetics
weak acid strong base rxn

22. High-speed electrons
trigonal bipyramidal
system
1 atm = 760 mmHg = 101.3 kPa
Beta Particles-

23. Like dissolves...
specific heat
Integrated Rate Law
period
like

24. The measurement of heat changes
Arrhenius Base
Calorimetry
n0
Covalently w/in themselves - Ionicly bonded w/ each other

25. frequency symbol
reduction
nu
Atomic Mass Unit
% error

26. 2+ charge
Alpha Particles-
Manometer
1st law of thermodynamics
Strong acid weak base rxn

27. AX3E2
Monoprotic
geometric isomers
End Point
t-shape

28. C=2.9979*10^8 m/s
Speed of light
Positive work value; work done on system
titrant buret
hept-

29. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
red/orange
Chemical Kinetics
-oic acid
moles of solute/ L of solution

30. Two molecules with identical connectivity but different geometries
geometric isomers
melting point
Nodes
Enthalpy of Solution

31. q H2O = ?
msAT
1atm=?mmHg/Torr
Acid Dissociation Constant
Pressure

32. Liquid to gas
meth-
vaporization
titrant buret
Normality

33. Puts H? into solution
0
Arrhenius acid
Zero-Order Rate Law
cyanide

34. 120° - sp^2
Trigonal Planar
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
k=Ae^(-Ea/RT)
Arrhenius Base

35. Tools NEEDED for dilution
Molality
Volume Metric Flask & Pipet
period
Solution

36. Kinetic Energy is proportional to ______
Temperature
Colligative properties
Molecular
Tetrahedral

37. Formula used when diluting stock solution (to find amount of water or stock needed)
Colligative properties
Root Mean Square Velocity
linear
M1V1=M2V2

38. Ptotal=P1+P2+P3+...

39. Solid to liquid
melting
green/yellow
Dipole Moment
Second-Order Half Life

40. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
rate law
Cg=kPg
insoluble
Gamma Ray-

41. High-energy light
Gamma Ray-
Quantum Mechanical Model
period
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

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

43. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Colligative properties
moles of solute/ L of solution
Antibonding Molecular Orbital
condensation

44. (organics) double-bonded compound
alkene
vapor pressure
Effusion
f

45. The total entropy is always increasing - all systems tend towards maximum entropy
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Volume Metric Flask & Pipet
2nd law of thermodynamics
Oxidizing Agent

46. BrO3¹?
0
viscosity
Percent Yield
bromate

47. Variable for spin of electron (+.5 or -.5)
strong acids
s (fourth quantum number)
# protons + # neutrons
work

48. AX6
octahedral
trigonal planar
dichromate
anode

49. Idea Gas Law (actual rules)
vapor pressure
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
-al
no precipitate forms

50. Ka=[products]^m/[reactants]^n
hydrolysis
Acid Dissociation Constant
heat capacity
# protons (atom is defined by this)