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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. NO3¹?
+1 - except if bonded to Alkali Metal -1
Faraday
nitrate
base and hydrogen gas

2. Solution used in titration
Osmotic Pressure
like
1 atm = 760 mmHg = 101.3 kPa
titrant buret

3. (organics) eight carbons
precipitate
octahedral
electron affinity
oct-

4. SO3²?
Hund's Rule
sulfite
Integrated Rate Law
equilibrium

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

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6. 1/([A]0*k)
freezing
Second-Order Half Life
rate
third

7. A device used to measure Delta H
Law of Multiple Proportions
P1= X1P1°
Quantum Mechanical Model
Calorimeter

8. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change

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9. ClO4¹?
perchlorate
Molal BP Elevation Constant
0.0821 atm L/mol K
Second-Order Half Life

10. When n=3 ->2 - color=
-oate
red
Effusion
weak acid strong base rxn

11. Idea Gas Law (actual rules)
oxide
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
Delta H or Enthalpy Change
soluble

12. HF+ OH??H2O
bond energy
voltaic cells
weak acid strong base rxn
condensation

13. r=k
Zero-Order Rate Law
non-
p orbitals
chlorite

14. Ester suffix
-oate
red/orange
3/2RT
strong acids

15. Type of system in which the energy and mass may leave or enter
Formal Charge
Open System
Cell Potential (Ecell)
Osmotic Pressure

16. Change in Energy = ? (in terms of constant pressure; for gasses)
Law of Conservation of Mass
Atmospheric Pressure
Resonance
AE= AH - RTAn

17. Peak of energy diagram
Ag+ - Pb2+ - Hg2+
activated complex (transition state)
Equilibrium constant
prop-

18. Change without heat transfer between the system and its surroundings
amine
Magnetic Quantum Number (ml)
permanganate
adiabatic

19. Does the same as equilibrium expression - except it uses initial concentrations
Multiplying
Reaction Quotient (Q)
nitrate
t-shape

20. Oxidation # of Halogens
End Point
-1
anode
diamagnetic

21. 1 sigma bond - 1 pi bond
Root Mean Square Velocity
double bond
1 atm
v3RT/M(in kg)

22. Substances w/ critical temperatures below 25°C
melting
permanent gases
Temperature
Equivalence Point

23. Oxidation # of Compounds
msAT
hex-
0
viscosity

24. R in ideal gas law
v3RT/M(in kg)
k=Ae^(-Ea/RT)
0.0821 atm L/mol K
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

25. (N) number of equivalents per liter of solution
Normality
Amount of atoms present
Solute
endless

26. Force acting over distance
Decrease Volume and Increase Temperature
non-
Enthalpy of Solution
Work

27. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
Alkali metals
1/2mv²
Molal BP Elevation Constant
not spontaneous

28. IMF that exists in polar molecules
Dipole-dipole forces
titrant buret
End Point
Buffer

29. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
complex ions
Molecular Compounds
force x distance = work done
Constant Pressure

30. Group 1 metals
Alkali metals
Hybridization
g solute/g solvent x 100
Molal FP Depression Constant

31. If heat capacity isn't mentioned - you can assume that q of cal is = ?
indicator
Temperature
s orbitals
0

32. Organic w/ -O-
# protons + # neutrons
?Hvap
ether
indicator

33. A given compound always has exactly the same proportion of elements by mass
Sigma Bond
Law of Definite Proportion
Atomic Mass Unit
electrolyte

34. A method of investigation involving observation and theory to test scientific hypotheses
Arrhenius Base
Scientific Method
Constant Pressure
equilibrium

35. Point at which vapor pressure=air pressure above
0.512°C
Polar Covalent
boiling point
vaporization

36. .69/k
Law of Multiple Proportions
Q<K
First-Order Half Life
Specific Heat Capacity

37. Pairs of electrons localized on an atom
6.63x10?³4Js
Ideal Gas Law
Lone Pair
Arrhenius Acid

38. Raoult's Law - relations between vapor pressure and concentrations
trigonal bipyramidal
P1= X1P1°
rate
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

39. Ketone suffix
-one
Work
-ous acid
Ionic

40. Mols A/ total mols - XA
mol Fraction
alkane
heat of fusion
Valence Electrons(assigned)

41. R=
trigonal bipyramidal
8.31J/Kmol
third
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

42. Like dissolves...
Molar Heat Capacity
Anion
like
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

43. 1/[A]=kt + 1/[A]0
AH
Integrated Second-Order Rate Law
Temperature
boiling point

44. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
1/2mv²
-one
insoluble
ionic

45. Rate of Diffusion/Effusion formula
standard solution
are
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
electrolyte

46. Elements on staircase on periodic table
chlorate
blue-violet
non-
Metalliods

47. Generally insoluble anions (names)
phosphate - sulfide - carbonate - sulfate
trigonal planar
M = square root (3RT/mm)
excess reactant

48. Freezing point depression formula
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
methoxy-
ether
?Tf= kf x molality

49. When gas compresses ...
Positive work value; work done on system
square planar
Pi Bond
v3RT/M(in kg)

50. Higher in energy than the atomic orbitals of which it is composed
oxidation
Antibonding Molecular Orbital
Ligand
spontaneous