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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. A weak acid that changes color at or near the equivalence point
p+
-1
indicator
not spontaneous

2. The line running between the atoms
Force = mass x acceleration
Sigma Bond
Bronsted-Lowry base
Molecule

3. Significant Digits of Conversion Factors
endless
Mass
yellow --> green
q/moles

4. AX4E2
Resonance
Molarity
v3RT/M(in kg)
square planar

5. 120° - sp^2
pent-
Trigonal Planar
third
viscosity

6. Color of Na (flame test)
Endothermic
# protons (atom is defined by this)
Osmotic Pressure
yellow

7. q rxn = ?
isothermal
endless
-(q of H2O + q of cal)
0

8. Mass/volume
high pressure - low temperature
Ideal Gas Law
6.63x10?³4Js
Density

9. AX5E
London Dispersion Forces
conjugate base
square pyramidal
increasing

10. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Magnetic Quantum Number (ml)
-ol
Electron Spin Quantum Number
Heisenberg Uncertainty Principle

11. Change in moles (An) =?
-2 - with peroxide -1
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Pi Bond
(moles of products that are gasses) - (moles of reactants that are gasses)

12. 6.022x10^23
Atomic Mass Unit
-1
Temperature
mol

13. Reverse rxn occurs when
not spontaneous
End Point
anode
Q>K

14. Mixing of gases
yellow
Diffusion
Ampere
Bond Order

15. Anions or cations as needed to produce a compound with non net charge
Hydrogen bonding
permanent gases
Counterions
base and hydrogen gas

16. A solid or gas that can be formed when 2 or more aqueous reactants come together
precipitate
Overall Reaction Order
22.4L
Faraday

17. Ketone suffix
London dispersion forces
Enthalpy of Solution
k=Ae^(-Ea/RT)
-one

18. If Q<Ksp
Theoretical yield
no precipitate forms
Molecular Orbitals (MOs)
phosphate - sulfide - carbonate - sulfate

19. Molecules' tendency to stick to one another
Ionic
force x distance = work done
like
cohesion

20. Unusually strong dipole forces found when H is bonded to N - O - or F
Arrhenius Base
group
Resonance
Hydrogen bonding

21. Has values from 0 to (n-1); tells shape of atomic orbitals
allotrope
Increase Temperature
Angular Momentum Quantum Number
chlorate

22. How to Find an Empirical Formula Given Percentages
pent-
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
a precipitate forms
Anion

23. In covalent bonds - prefixes are used to tell...
Percent Yield
3/2RT
Amount of atoms present
eth-

24. Force acting over distance
Principal Quantum Number
Hess's Law
Equilibrium constant
Work

25. When _____ significant digits - round answer to least significant digit
Heisenberg Uncertainty Principle
Multiplying
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Faraday

26. (organics) ten carbons
Manometer
are not
blue-violet
dec-

27. Weakest IMFs - found in all molecules
heat capacity
London dispersion forces
Pauli Exclusion Principle
# protons + # neutrons

28. Phase change from gas to solid
Law of Multiple Proportions
deposition
oct-
rate gas A/rate gas B = square root (mm A/ mm B)

29. Boiling point elevation formula
?Tb= kb x molality
spontaneity
Molal FP Depression Constant
Equilibrium constant

30. R=
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
0.0826Latm/Kmol
Heat Capacity (C)
Barometer

31. CrO4²?
chromate
freezing
Aufbau Principle
Aufbau Principle

32. A device in which chemical energy is changed to electrical energy
Hess's Law
analyte
0
Galvanic Cell

33. #NAME?
Valence Electrons(assigned)
E
equivalence point
k=Ae^(-Ea/RT)

34. The total energy of the universe is constant - all systems tend towards minimum energy
first
1st law of thermodynamics
P of a =(X of a)(total pressure)
yellow --> green

35. kb of water
0.512°C
Van't Hoff factor
deposition
1 atm

36. These orbitals are perpendicular
p orbitals
melting point
specific heat
Ionic Compounds

37. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
yellow
dec-
activation energy
Cg=kPg

38. Elements which have all electrons paired and relatively unaffected by magnetic fields
Increase Temperature
1/2mv²
oxidation
diamagnetic

39. H?+OH??H2O
fusion
strong acid strong base rxn
trigonal planar
Solute

40. 1/([A]0*k)
Bond enthalpy
voltaic cells
0
Second-Order Half Life

41. Type of system in which the energy may escape - but the mass is conserved
Reducing Agent
Speed of light
Bonding Pairs
Closed System

42. H?+NH3?NH4
Closed System
excess reactant
Limiting reactant
Strong acid weak base rxn

43. E?s fill the lowest energy orbital first - then work their way up
Molal BP Elevation Constant
Aufbau Principle
catalyst
# protons + # neutrons

44. Gas to solid
conjugate acid
Open System
v3RT/M(in kg)
deposition

45. NO2¹?
no precipitate forms
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
critical point
nitrite

46. Ptotal=Pa+Pb+Pc....

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47. Molecules' tendency to stick to the container
adhesion
base
hydrocarbons
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

48. Heat required to raise the system 1°C
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
chlorate
Calorimetry
heat capacity

49. Tools NEEDED for dilution
trigonal planar
Volume Metric Flask & Pipet
condensation
precipitate

50. (organics) eight carbons
are not
System
P of a =(X of a)(total pressure)
oct-