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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. negative ion
Oxidizing Agent
Anion
Net Ionic Equation
Electron Spin Quantum Number

2. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Buffer
eth-
hydrocarbons
Law of Multiple Proportions

3. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Valence Electrons(assigned)
complex ions
blue-violet
Molecular

4. Pressure Units/Conversions
Cg=kPg
anode
Counterions
1 atm = 760 mmHg = 101.3 kPa

5. Where reduction occurs
Law of Conservation of Mass
Cathode
second
Formal Charge

6. I¹?
iodide
0
third
seesaw

7. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Counterions
Integrated Second-Order Rate Law
Bond enthalpy
rate

8. Oxoacid solution (such as HSO4-) forms...
Chemical Kinetics
oxide gas and water
trigonal bipyramidal
actual yield/theoretical yield x 100%

9. Molecules' tendency to stick to the container
STP
a precipitate forms
Limiting reactant
adhesion

10. Reverse rxn occurs when
E
Q>K
titrant buret
Formal Charge

11. J/°Cmol or J/Kmol
bent
Equilibrium constant
Integrated Rate Law
Molar Heat Capacity

12. AX6
charge
Acids
octahedral
insoluble

13. ln[A]=-kt + ln[A]0
Adding
Quantum Mechanical Model
blue-green
Integrated First-Order Rate Law

14. A single substance that may be an acid or a base (i.e. water)
s orbitals
0.0826Latm/Kmol
Anion
Amphoteric

15. l=3
nitrite
Heisenberg Uncertainty Principle
viscosity
f

16. Symbol for Total Heat absorbed or released
Molecular Orbitals (MOs)
q
0
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

17. Oxidation # of Hydrogen
+1 - except if bonded to Alkali Metal -1
octahedral
Law of Conservation of Mass
yellow --> green

18. Group 2 metals
Antibonding Molecular Orbital
Molecular
State Functions
Alkaline earth metals

19. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Chemical Kinetics
sublimation
Molarity
oxidation

20. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
Ligand
Valence Electrons(assigned)
voltaic cells
condensation

21. Ionizes to produce OH- Ions
?Hvap
sulfate
purple --> pink
Arrhenius Base

22. 2+ charge
Bases
Monoprotic
increasing
Alpha Particles-

23. Entropy in the universe is always...
surroundings
increasing
cyanide
square pyramidal

24. Peak of energy diagram
alcohol
Enthalpy of Solution
activated complex (transition state)
chlorite

25. The total energy of the universe is constant - all systems tend towards minimum energy
0
1st law of thermodynamics
equivalence point
hydroxide

26. Symbol for Enthalpy
H
non-
Speed of light
Amount of atoms present

27. neutron (symbol)
STP
iodide
n0
amine

28. If Q<Ksp
Increase Temperature
force x distance = work done
no precipitate forms
Mass

29. AX4
p+
Specific Heat Capacity
p orbitals
tetrahedral

30. Mass percent
Molar Mass of Element/ Total Molar Mass %
g solute/g solvent x 100
Law of Multiple Proportions
prop-

31. The chemical formed when a base accepts a proton
but-
phosphate - sulfide - carbonate - sulfate
Aufbau Principle
conjugate acid

32. Speed per molecule of gas
weak acid strong base rxn
v3kT/m
London Dispersion Forces
adhesion

33. (organics) single-bonded compound
group
alkane
carbohydrates
M1V1=M2V2

34. Oxidation # of Oxygen
Atomic Mass Unit
Calorimetry
-2 - with peroxide -1
conjugate acid

35. AX5E
square pyramidal
Finding Empirical Formulas
conjugate base
Galvanic Cell

36. The mixing of native atomic orbitals to form special orbitals for bonding
Solubility Product (Ksp)
Ligand
charge
Hybridization

37. CrO4²?
Solution
AE= AH - RTAn
chromate
square pyramidal

38. If anion ends in -ate - acid name ends in...
-ous acid
5% rule
-ic acid
Bronsted-Lowry Acid

39. R in instances that pertain to energy
8.314 J/K mol
Bond enthalpy
Gamma Ray-
base

40. We cannot simultaneously determine an atom's exact path or location
Hund's Rule
0
Law of Definite Proportion
Heisenberg Uncertainty Principle

41. When gas compresses ...
Work
Positive work value; work done on system
a precipitate forms
-ous acid

42. The part of the universe one is focused upon (in thermodynamics)
system
Molal FP Depression Constant
non-
blue

43. Color of Cs (flame test)
blue
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Ionic
1st law of thermodynamics

44. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
mol
Gamma Ray-
group

45. NO3¹?
Sigma Bond
nitrate
like
condensation

46. High-speed electrons
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
red
Beta Particles-
Constant Pressure

47. Aldehyde suffix
chloride
moles solute/kg solvent
C=(mass)(specific heat)
-al

48. Type of system in which the energy may escape - but the mass is conserved
van't Hoff Factor
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Closed System
Q<K

49. Equation to find Ea from reaction rate constants at two different temperatures
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Arrhenius acid
Hydrogen bonding
charge

50. Group 1 and heavier Group 2 bases
strong bases
% yield
1/2mv²
bond energy