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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. For significant digits - leading zeros ____ significant
Diffusion
are not
Molecular Compounds
Open System

2. The weighted average of all the isotopes that an atom can have (in g/mol)
Theory of Relativity
electron affinity
0
Atomic Mass Unit

3. As protons are added to the nucleus - electrons are similarly added
Aufbau Principle
AE = q + w
Bronsted-Lowry acid
LeChatelier's Principle

4. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
sublimation
methoxy-
vaporization
insoluble

5. kb of water
0.512°C
-2 - with peroxide -1
p orbitals
rate

6. Cr2O7²?
dichromate
2nd law of thermodynamics
Integrated First-Order Rate Law
Molality

7. The total entropy is always increasing - all systems tend towards maximum entropy
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Coordination Compound
2nd law of thermodynamics
-1

8. IMF that occurs with FON
Enthalpy of Solution
Adding
Hydrogen bonding
red

9. F¹?
Oxidizing Agent
flouride
pi=(nRT)/v
trigonal bipyramidal

10. E?s fill the lowest energy orbital first - then work their way up
Sigma Bond
equilibrium
but-
Aufbau Principle

11. Idea Gas Law (actual rules)
phosphate
non-
van't Hoff Factor
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

12. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Nernst Equation
Aufbau Principle
Chemical Kinetics
trigonal pyramidal

13. Mols A/ total mols - XA
trigonal pyramidal
endless
mol Fraction
l (second quantum number)

14. Point where acid completely neutralizes base
Galvanic Cell
equivalence point
double bond
1atm=?mmHg/Torr

15. H+ Acceptor
insoluble
blue-violet
X of a = moles a/total moles
Bronsted-Lowry Base

16. Unit of electrical potential; J/C
Monoprotic
high pressure - low temperature
Volt
Average KE = 1/2(mass)(average speed of all particles)

17. Expresses how the concentrations depend on time
Integrated Rate Law
indicator
linear
isothermal

18. Elements which have all electrons paired and relatively unaffected by magnetic fields
permanent gases
diamagnetic
deposition
Molal BP Elevation Constant

19. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Dalton's Law of Partial Pressures
hex-

20. Ending for alcohols
Oxidation is Loss Reduction is Gain
precipitate
-ol
Anode

21. ClO4¹?
perchlorate
tetrahedral
% error
nitrate

22. Substances that form H+ when dissolved in water; proton donors
chlorate
Acids
Integrated Rate Law
titrant buret

23. Gas to solid
(moles of products that are gasses) - (moles of reactants that are gasses)
strong bases
deposition
condensation

24. SO4²?
sulfate
Dipole Moment
van't Hoff Factor
Enthalpy of Solution

25. Substance that - when dissolved - is conductive
perchlorate
Effusion
electrolyte
endless

26. Nonmetal oxide + H2O ->
acid
Law of Multiple Proportions
Integrated First-Order Rate Law
yellow --> green

27. Experimental yield/theoretical yieldx100
Hydrogen bonding
% yield
hydroxide
rate law

28. =vM2/M1
Linear
r1/r2
Q<K
Alkali metals

29. The actual amount of product produced in an experiment
s
electrolyte
Pauli Exclusion Principle
experimental yield

30. Molecules' tendency to stick to the container
heat of fusion
adhesion
equilibrium
strong bases

31. Coffee Cup Calorimeter
see-saw
strong acid strong base rxn
Constant Pressure
Closed System

32. Spontaneous emission of radiation
Strong acid weak base rxn
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Radioactivity
spontaneity

33. Group 2 metals
Alkaline earth metals
Linear
period
Oxidizing Agent

34. Atoms combine in fixed whole # ratios
non-
trigonal bipyramidal
Integrated Rate Law
Law of Multiple Proportions

35. H + donor
Bronsted-Lowry Acid
group
mol
Dipole-dipole forces

36. AX4
1st law of thermodynamics
A Roman numeral
tetrahedral
yellow

37. If anion ends in -ate - acid name ends in...
C=(mass)(specific heat)
(moles of products that are gasses) - (moles of reactants that are gasses)
Dipole-dipole forces
-ic acid

38. r=k[A]
period
First-Order Rate Law
supercritical fluid
reduction agent

39. The rest of the universe (in thermodynamics)
nitrate
surroundings
titrant buret
Reducing Agent

40. Electrons in a hydrogen atom move around the nucleus only in circular orbits
London Dispersion Forces
carbonate
Q<K
Quantum Model

41. If anion ends in -ide - acid name ends in
hydro-ic acid
AE = q + w
-oate
q

42. Measure of the change in enthalpy
permanent gases
Delta H or Enthalpy Change
Second-Order Rate Law
6.63x10?³4Js

43. Heat capacity formula
Anode
amine
k=Ae^(-Ea/RT)
C=(mass)(specific heat)

44. All cations are soluble with sulfate EXCEPT
adiabatic
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Nodes
Cation

45. Atoms with the same number of protons but a different number of neutrons
-oate
q/moles
Isotopes
Law of Conservation of Mass

46. Chemical composition of dry ice
0
solid CO2
Bond Energy
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

47. Point at which vapor pressure=air pressure above
oxidation
sublimation
charge
boiling point

48. If anion ends in -ite - acid name ends in...
Percent Yield
oxalate
-ous acid
Bond enthalpy

49. Involves quantum numbers
LE Model
Atomic Mass Unit
Quantum Mechanical Model
solid CO2

50. Gain of electrons - decrease in oxidation #
reduction
-oate
paramagnetic
Law of Definite Proportion