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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. Energy required to break a bond
s orbitals
Bond Energy
Constant Pressure
spontaneous

2. Mole Fraction
1.86°C
wavelength
X of a = moles a/total moles
eth-

3. H?+OH??H2O
strong acid strong base rxn
Aufbau Principle
Quantum Model
voltaic cells

4. Resistance to flow
viscosity
Acids
P1= X1P1°
Constant Volume

5. l=2
d
Speed of light
Increase Temperature
activation energy

6. R in ideal gas law
zero
q
sulfate
0.0821 atm L/mol K

7. Delta H (AH) = ?
q/moles
Molarity
prop-
London dispersion forces

8. AX3
Bond enthalpy
red
Quantum Mechanical Model
trigonal planar

9. Oxoacid solution (such as HSO4-) forms...
but-
Hund's Rule
Heat
oxide gas and water

10. All forms of energy except for heat
sulfide
London dispersion forces
blue
work

11. Cl¹?
chloride
sulfate
Law of Multiple Proportions
Reducing Agent

12. Pure metal or metal hydride + H20 ->
analyte
Enthalpy of Solution
pent-
base and hydrogen gas

13. Reactant that's completely used up in a chemical reaction
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Law of Conservation of Mass
Limiting reactant
pi=(nRT)/v

14. kb of water
Force = mass x acceleration
0.512°C
diamagnetic
yellow

15. Point at which the titrated solution changes color
end point
M1V1=M2V2
-oic acid
endless

16. When n=3 ->2 - color=
red
excess reactant
Aufbau Principle
hydroxide

17. The heat changed in a chemical reaction.
Thermochemistry
Coordination Compound
chromate
Reaction Quotient (Q)

18. pH=
red
log[H+]
Reducing Agent
Its element

19. When _____ significant digits - round answer to least significant digit
Increase Temperature
Multiplying
Nernst Equation
specific heat

20. 96 -485 C/mol e-
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
Faraday
deposition
Molality

21. Energy can't be created nor destroyed
Law of Conservation of Energy
flouride
Cation
p+

22. C2O4²?
Hund's Rule
M1V1=M2V2
Transition metals
oxalate

23. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
Surroundings
bromate
H
State Functions

24. Mol/kg of solvent - used in calculating colligative properties
red
n (first quantum number)
purple --> pink
Molality

25. In ideal gas law problem - when it says "atmospheric" ...
seesaw
p
Pressure of H2O must be Subtracted
Second-Order Rate Law

26. NO2¹?
-oate
nitrite
Hund's Rule
sublimation

27. q H2O = ?
Galvanic Cell
chlorate
Electron Spin Quantum Number
msAT

28. [A]=-kt + [A]0
Integrated Zero-Order Rate Law
Bronsted-Lowry Acid
anode
Magnetic Quantum Number (ml)

29. The chemical formed when an acid donates a proton
group
Lone Pair
Tetrahedral
conjugate base

30. Melting
fusion
Integrated Rate Law
# protons + # neutrons
purple

31. A solution used in titrations whose concentration is known
Volt
geometric isomers
high pressure - low temperature
standard solution

32. We cannot simultaneously determine an atom's exact path or location
melting point
Heisenberg Uncertainty Principle
Molality
London dispersion forces

33. Entropy in the universe is always...
mol
endless
d orbitals
increasing

34. 2 or more covalently bonded atoms
Bond Order
P of a =(X of a)(total pressure)
isothermal
Molecule

35. Gas to liquid
Oxidation is Loss Reduction is Gain
condensation
trigonal planar
freezing

36. AX5E
square pyramidal
Kinetic Molecular Theory - for ideal gases
State Functions
(moles of products that are gasses) - (moles of reactants that are gasses)

37. NH4¹?
Mass
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Speed of light
ammonium

38. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Acid + Base --> Salt + Water
Molal BP Elevation Constant
spontaneity
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+

39. (msubs) Can only be +1/2 or -1/2
Electron Spin Quantum Number
second
are
Bronsted-Lowry acid

40. 120° - sp^2
Trigonal Planar
Delta H or Enthalpy Change
C + 273
work

41. Type of system in which nothing is transfered (no mass or energy); ideal
8.31J/Kmol
Isolated System
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
yellow

42. When n=5 ->2 - color=
not spontaneous
Positive work value; work done on system
blue-violet
Law of Conservation of Energy

43. Change in moles (An) =?
?Tb= kb x molality
Solute
high pressure - low temperature
(moles of products that are gasses) - (moles of reactants that are gasses)

44. AX4E
spontaneous
see-saw
Molar Heat Capacity
f

45. Happens at lines in phase change charts
Cell Potential (Ecell)
l (second quantum number)
yellow --> green
equilibrium

46. Spontaneous emission of radiation
salt bridge
Radioactivity
cohesion
d orbitals

47. Organic w/ -OH group
-al
Solution
Finding Empirical Formulas
alcohol

48. Isotope
different # of neutrons
pi=(nRT)/v
iodide
Coordination Compound

49. Oxidation # of Hydrogen
Polar Covalent
Aufbau Principle
flouride
+1 - except if bonded to Alkali Metal -1

50. The likelihood that a rxn will occur "by itself"
spontaneity
actual yield/theoretical yield x 100%
hept-
Zero-Order Rate Law