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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
Don't refresh. All questions and answers are randomly picked and ordered every time you load a test.

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. Happens at lines in phase change charts
Its element
M = square root (3RT/mm)
system
equilibrium

2. AP doesn't deal with ...-order reaction - don't pick it!
adhesion
third
5% rule
Hydrogen bonding

3. Raising heat - adding catalyst - heighten concentration - bigger surface area
like
Force = mass x acceleration
hept-
methods of increasing rate

4. Moles of solute/volume of soln(L)
v3kT/m
Molarity
melting point
Oxidation is Loss Reduction is Gain

5. Energy required to break a bond
Solvent
Molality
Bond Energy
?Tb= kb x molality

6. HF+ OH??H2O
A Roman numeral
weak acid strong base rxn
boiling point
d orbitals

7. frequency symbol
nu
Heisenberg Uncertainty Principle
Entropy (S)
Speed of light

8. The measurement of heat changes
Bonding Pairs
Calorimetry
CAT
entropy (S)

9. Connects the 2 half cells in a voltaic cell
electrolyte
1 atm = 760 mmHg = 101.3 kPa
salt bridge
Resonance

10. Ionizes to produce OH- Ions
Arrhenius Base
Mass
deposition
Integrated Rate Law

11. Elements which have all electrons paired and relatively unaffected by magnetic fields
Law of Conservation of Energy
Principal Quantum Number
diamagnetic
trigonal bipyramidal

12. Thickness
red
Root Mean Square Velocity
viscosity
Bond Order

13. Positive enthalpy - heat flows into system
-oate
endothermic
1atm=?mmHg/Torr
iodide

14. (organics) seven carbons
ether
Hybridization
Hydrogen bonding
hept-

15. Where reduction occurs
Cathode
Gamma Ray-
Solution
t-shape

16. Measure of the average kinetic energy of all the particles in a substance
acetate
Temperature
melting
Cell Potential (Ecell)

17. NO3¹?
Molecular Orbitals (MOs)
-one
Molar Mass of Element/ Total Molar Mass %
nitrate

18. # bonding e- - # antibonding e-/2
wavelength
adiabatic
-ous acid
Bond Order

19. I=moles of particles/moles of solute dissolved

20. Type of system in which the energy may escape - but the mass is conserved
Closed System
Integrated First-Order Rate Law
rate gas A/rate gas B = square root (mm A/ mm B)
s (fourth quantum number)

21. Mols A/ total mols - XA
moles of solute/ L of solution
Constant Volume
mol Fraction
Integrated Rate Law

22. Mass/volume
soluble
Density
purple --> pink
LeChatelier's Principle

23. A monoatomic cation takes name from...
melting
Its element
force x distance = work done
sublimation

24. 0.00°C - 1 atm
fusion
-oate
Standard Temperature and Pressure
reduction agent

25. Absorbs/takes in heat (positive value)
End Point
LE Model
bent
Endothermic

26. These orbitals are spherical
surroundings
Equilibrium constant
Acid Dissociation Constant
s orbitals

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

28. If anion ends in -ite - acid name ends in...
Molar Mass of Element/ Total Molar Mass %
Kinetic Molecular Theory - for ideal gases
isothermal
-ous acid

29. l=1
Law of Multiple Proportions
geometric isomers
insoluble
p

30. Variable for energy of e- - goes from 1 -2 -3 on up
Law of Multiple Proportions
meth-
n (first quantum number)
Cation

31. Proton donors
oxide gas and water
Bronsted-Lowry acid
Hess's Law
Heisenberg Uncertainty Principle

32. AX5E
1/2mv²
square pyramidal
heat capacity
Resonance

33. Amine prefix
Quantum Model
Its element
0.0826Latm/Kmol
Amino-

34. (organics) five carbons
Colligative properties
pent-
Aufbau Principle
LeChatelier's Principle

35. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
t-shape
Law of Multiple Proportions
conjugate base
Manometer

36. Average Kinetic Energy Formula
not spontaneous
Thermochemistry
Hydrogen bonding
Average KE = 1/2(mass)(average speed of all particles)

37. H+ Acceptor
Bronsted-Lowry Base
seesaw
Quantum Numbers
Barometer

38. If Q>Ksp
condensation
Le Chatelier's Principle
a precipitate forms
LeChatelier's Principle

39. Speed of light - C
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
equilibrium
yellow
3.0x108m/s

40. negative ion
Pressure of H2O must be Subtracted
Nernst Equation
1atm=?mmHg/Torr
Anion

41. MnO4¹?
lambda
Van't Hoff factor
permanganate
moles of solute/ L of solution

42. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
green/yellow
Manometer
Weight
strong acids

43. Describe various properties of one orbital
Arrhenius Acid
rate
Quantum Numbers
Bronsted-Lowry base

44. A weak acid that changes color at or near the equivalence point
indicator
heat of vaporization
force x distance = work done
perchlorate

45. 1/([A]0*k)
square pyramidal
Second-Order Half Life
Open System
Molar Mass of Element/ Total Molar Mass %

46. Has values 1 -2 -3 -...; tells energy levels
electron affinity
Principal Quantum Number
0 degrees C - 1 atm
Zero-Order Rate Law

47. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
% error
Boltzmann distribution
Covalently w/in themselves - Ionicly bonded w/ each other
e-

48. Arrhenius equation
n0
k=Ae^(-Ea/RT)
Closed System
London Dispersion Forces

49. AH of formation for a substance in its stablest form (how it is found in nature)
Ideal Gas Law
0
Endothermic
pi=(nRT)/v

50. Hydroxides are soluble or insoluble?
n0
insoluble
rate
alkyne