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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. Ending for alcohols
-ol
single bond
3/2RT
square pyramidal

2. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
supercritical fluid
cathode
Hund's Rule
Volume Metric Flask & Pipet

3. J/°Cmol or J/Kmol
rate gas A/rate gas B = square root (mm A/ mm B)
Molar Heat Capacity
Pauli Exclusion Principle
ether

4. AX4E2
5% rule
?Hvap
Molar Mass of Element/ Total Molar Mass %
square planar

5. Elements which have all electrons paired and relatively unaffected by magnetic fields
Cg=kPg
diamagnetic
Allotrope
Counterions

6. Change that occurs at constant temperature
isothermal
nu
chromate
Normality

7. R=
Enthalpy of Solution
Nernst Equation
8.31J/Kmol
1st law of thermodynamics

8. CrO4²?
amine
Force = mass x acceleration
q
chromate

9. Involves quantum numbers
STP
Quantum Mechanical Model
v3kT/m
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

10. AX6
specific heat
Law of Conservation of Mass
Joule
octahedral

11. Diatomic Molecules
p+
Dalton's Law
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
red

12. O²?
oxide
Entropy (S)
Molality
Amphoteric

13. Puts H? into solution
T-shape
Ideal Gas Law
Arrhenius acid
Integrated First-Order Rate Law

14. Each orbital can hold two e?s each w/ opposite spins
Weight
chloride
Pauli Exclusion Principle
different # of neutrons

15. A monoatomic cation takes name from...
M = square root (3RT/mm)
Its element
conjugate base
sulfite

16. Solid to gas
Its root and adding -ide
sublimation
condensation
Molarity

17. Coffee Cup Calorimeter
Constant Pressure
vapor pressure
complex ions
like

18. Kinetic Energy per molecule
activated complex (transition state)
n0
Diffusion
1/2mv²

19. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
Principal Quantum Number
insoluble
Cg=kPg
system

20. The reactant in the reduction reaction that forces the oxidation reaction to occur
Oxidizing Agent
Barometer
6.63x10?³4Js
Molality

21. 120° - sp^2
Solubility Product (Ksp)
-oate
Trigonal Planar
Manometer

22. Has values 1 -2 -3 -...; tells energy levels
Principal Quantum Number
square pyramidal
P of a =(X of a)(total pressure)
First-Order Half Life

23. To find activation energy use the...
Arrhenius equation
Boltzmann distribution
paramagnetic
a precipitate forms

24. PO4³?
0
0 degrees C - 1 atm
phosphate
Temperature

25. AX3E
Limiting reactant
Hess's Law
g solute/g solvent x 100
trigonal pyramidal

26. 760mmHg/Torr
1atm=?mmHg/Torr
voltaic cells
log[H+]
Lone Pair

27. (organics) triple-bonded compound
endless
indicator
alkyne
Anode

28. 90° - d^2sp^3
Octahedral
moles of solute/ L of solution
Buffered Solution
Pauli Exclusion Principle

29. Metal oxide + H20 ->
Net Ionic Equation
Calorimeter
base
prop-

30. Mols A/ total mols - XA
r1/r2
Integrated Rate Law
Balmer Series
mol Fraction

31. (N) number of equivalents per liter of solution
not spontaneous
Molar Mass of Element/ Total Molar Mass %
-ous acid
Normality

32. Actual Yield/Theoretical Yield*100%
Percent Yield
dec-
are not
CAT

33. Boiling point elevation formula
Dipole Moment
H
Nodes
?Tb= kb x molality

34. Tools NEEDED for dilution
allotrope
Volume Metric Flask & Pipet
AE = q + w
yellow

35. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Polar Covalent
hydrocarbons
strong acids
moles of solute/ L of solution

36. The total entropy is always increasing - all systems tend towards maximum entropy
Equivalence Point
oxalate
flouride
2nd law of thermodynamics

37. Oxidation # of Ions
experimental yield
M = square root (3RT/mm)
charge
condensation

38. Oxoacid solution (such as HSO4-) forms...
pi=(nRT)/v
s orbitals
Isolated System
oxide gas and water

39. Atomic #
London dispersion forces
Constant Volume
d orbitals
# protons (atom is defined by this)

40. Ptotal=Pa+Pb+Pc....

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41. Energy involved in gaining an electron to become a negative ion
heat capacity
electron affinity
q/moles
exothermic

42. (organics) nine carbons
non-
-ous acid
third
Le Chatelier's Principle

43. Entropy in the universe is always...
increasing
condensation
5% rule
strong bases

44. The reactant that is being oxidized - brings about reduction
AE= AH - RTAn
cathode
reduction agent
analyte

45. Mass reactants= mass products
Law of Conservation of Mass
analyte
Molal FP Depression Constant
yellow --> green

46. Half cell in which oxidation occurs
(moles of products that are gasses) - (moles of reactants that are gasses)
Molarity
moles of solute/ L of solution
anode

47. Substance being dissolved in a solution (lower [ ])
Alpha Particles-
Solute
freezing
meth-

48. Planck's constant - used to calculate energy w/frequency
6.63x10?³4Js
van't Hoff Factor
activation energy
endless

49. Mol/L - concentration of a solution
Aufbau Principle
P of a =(X of a)(total pressure)
Molarity
Alpha Particles-

50. Bomb Calorimeter
p orbitals
Constant Volume
Average KE = 1/2(mass)(average speed of all particles)
red