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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. AX4E2
Net Ionic Equation
0.512°C
square planar
Molar Mass of Element/ Total Molar Mass %

2. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
Kinetic Molecular Theory - for ideal gases
Coordination Compound
Isolated System
titrant buret

3. Average speed of gas
-oic acid
Quantum Model
v3RT/M(in kg)
pent-

4. Phase change from gas to solid
N=N.(0.5)^time/time half-life
anode
deposition
Dipole-dipole forces

5. Ketone suffix
-one
d orbitals
meth-
chlorite

6. In covalent bonds - prefixes are used to tell...
oxalate
Amount of atoms present
surroundings
-oate

7. These orbitals are spherical
phosphate - sulfide - carbonate - sulfate
s orbitals
Solubility Product (Ksp)
n (first quantum number)

8. Hydroxides are soluble or insoluble?
oxide
Integrated Rate Law
insoluble
-oic acid

9. AX5E
Speed of light
Equilibrium Expression
square pyramidal
C=(mass)(specific heat)

10. R=
base
m (third quantum number)
Equilibrium Expression
0.0826Latm/Kmol

11. (organics) two carbons
triple point
f
1/2mv²
eth-

12. High-energy light
seesaw
Limiting reactant
Quantum Mechanical Model
Gamma Ray-

13. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
but-
paramagnetic
End Point
base

14. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
lambda
Multiplying
London Dispersion Forces
96500

15. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
Van't Hoff factor
X of a = moles a/total moles
like

16. AX2 - AX2E3
k=Ae^(-Ea/RT)
% error
Constant Pressure
linear

17. Increase Volume
Faraday
Increase Temperature
3rd law of thermodynamics
3.0x108m/s

18. (organics) five carbons
Atomic Mass Unit
Allotrope
Ionic
pent-

19. Where oxidation occurs
Weight
weak acid strong base rxn
Naming Binary Ionic Compounds
Anode

20. q rxn = ?
-(q of H2O + q of cal)
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Equilibrium constant
Aufbau Principle

21. kf of water
v3RT/M(in kg)
Matter
1.86°C
wavelength

22. Ptotal=Pa+Pb+Pc....

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23. Significant Digits of counted things
Endothermic
endless
-oate
analyte

24. (organics) seven carbons
hept-
Tetrahedral
first
high pressure - low temperature

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

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26. AX4E
see-saw
effects of IMF
nu
Manometer

27. HF+ OH??H2O
0
weak acid strong base rxn
group
Oxidizing Agent

28. 1/[A] vs. time is a ...-order reaction
effects of IMF
Bases
amine
second

29. Boiling point elevation formula
?Tb= kb x molality
not spontaneous
Solute
Heat Capacity (C)

30. Variable for type of orbital
Increase Temperature
l (second quantum number)
trigonal bipyramidal
base and hydrogen gas

31. If heat capacity isn't mentioned - you can assume that q of cal is = ?
Amount of atoms present
blue-green
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
0

32. Tools NEEDED for dilution
Molar Heat Capacity
1atm=?mmHg/Torr
Volume Metric Flask & Pipet
Ionic Compounds

33. Coffee Cup Calorimeter
deposition
+1 - except if bonded to Alkali Metal -1
critical point
Constant Pressure

34. 1/([A]0*k)
Pauli Exclusion Principle
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
permanent gases
Second-Order Half Life

35. Ability of an atom in a molecule to attract shared electrons to itself
Naming Binary Ionic Compounds
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
dec-
Electronegativity

36. Anything occupying space and with mass
Matter
Magnetic Quantum Number (ml)
Theoretical yield
purple --> pink

37. 120° - sp^2
Trigonal Planar
Chemical Bonds
Ionic
oxide gas and water

38. Spectrum of light when an electron drops to energy level n=2
deposition
Molality
1atm=?mmHg/Torr
Balmer Series

39. As protons are added to the nucleus - electrons are similarly added
C + 273
oxidation
Pi Bond
Aufbau Principle

40. How to Find a Weighted Average
spontaneity
Overall Reaction Order
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
cathode

41. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
Multiplying
Sigma Bond
Nodes

42. Boiling point - melting point - viscosity - vapor pressure - surface tension
effects of IMF
Valence Electrons(assigned)
heat capacity
red

43. Elements on staircase on periodic table
Linear
Metalliods
Hess's Law
alkene

44. Melting
cohesion
fusion
strong acids
third

45. A single substance that may be an acid or a base (i.e. water)
Standard Temperature and Pressure
Manometer
(moles of products that are gasses) - (moles of reactants that are gasses)
Amphoteric

46. 180° - sp
Linear
acid
moles solute/kg solvent
Zero-Order Rate Law

47. PV=nRT
trigonal bipyramidal
Dalton's Law of Partial Pressures
Ideal Gas Law
geometric isomers

48. SO3²?
wavelength
sulfite
melting point
rate gas A/rate gas B = square root (mm A/ mm B)

49. 109.5° - sp^3
Molar Mass of Element/ Total Molar Mass %
E
Tetrahedral
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

50. Variable for spin of electron (+.5 or -.5)
second
s (fourth quantum number)
Trigonal Bipyramidal
Law of Conservation of Mass