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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. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
Ampere
Amount of atoms present
Anion

2. Reactant that's completely used up in a chemical reaction
triple bond
AE = q + w
Limiting reactant
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

3. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
different # of neutrons
Closed System
Integrated Zero-Order Rate Law

4. l=3
f
catalyst
blue-green
Specific Heat Capacity

5. The total energy of the universe is constant - all systems tend towards minimum energy
1st law of thermodynamics
Covalently w/in themselves - Ionicly bonded w/ each other
Valence Electrons(assigned)
nu

6. Metal oxide + H20 ->
single bond
Heisenberg Uncertainty Principle
base
electron affinity

7. Cation first - anion second
Formal Charge
period
cathode
Naming Binary Ionic Compounds

8. q rxn = ?
m (third quantum number)
1.86°C
Average KE = 1/2(mass)(average speed of all particles)
-(q of H2O + q of cal)

9. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Integrated Second-Order Rate Law
Its element
Arrhenius base
Molecular

10. Energy needed to break a bond
Colligative properties
Coordination Compound
period
bond energy

11. When n=5 ->2 - color=
blue-violet
1atm=?mmHg/Torr
Alkali metals
n0

12. The reactant that is being reduced - brings about oxidation
oxidizing agent
conjugate base
Work
Resonance

13. Faraday's constant
96500
Law of Conservation of Energy
amine
methoxy-

14. IMF that occurs with FON
Heisenberg Uncertainty Principle
moles solute/kg solvent
diamagnetic
Hydrogen bonding

15. Tools NEEDED for dilution
Volume Metric Flask & Pipet
isothermal
alkyne
p+

16. Heat needed to change 1 g of substance to 1°C
+1 - except if bonded to Alkali Metal -1
carbonate
Anode
specific heat

17. An equilibrium expression
pi=(nRT)/v
Solubility Product (Ksp)
van't Hoff Factor
condensation

18. Puts OH? into solution
Arrhenius base
m (third quantum number)
second
Constant Pressure

19. Negative enthalpy - heat flows into surroundings
moles of solute/ L of solution
Amphoteric
exothermic
ionic

20. Ending for alcohols
phosphate - sulfide - carbonate - sulfate
-ol
Transition metals
Pauli Exclusion Principle

21. 1 sigma bond
single bond
Arrhenius acid
Dalton's Law of Partial Pressures
p+

22. Atomic #
# protons (atom is defined by this)
X of a = moles a/total moles
Surroundings
square pyramidal

23. Chemical composition of dry ice
STP
solid CO2
Calorimeter
iodide

24. The entropy of a pure perfectly formed crystal @0K is 0
T-shape
3rd law of thermodynamics
M = square root (3RT/mm)
Hund's Rule

25. Molarity (M)
increasing
carbohydrates
moles of solute/ L of solution
Q<K

26. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Buffer
end point
Magnetic Quantum Number (ml)
soluble

27. A measure of resistance of an object to a change in its state of motion
double bond
Solution
rate gas A/rate gas B = square root (mm A/ mm B)
Mass

28. (A) - C/s
0
precipitate
alkyne
Ampere

29. negative ion
mol
Closed System
Multiplying
Anion

30. Positive ion
group
Cation
Solute
London dispersion forces

31. NO3¹?
P1= X1P1°
oxidation
nitrate
Ag+ - Pb2+ - Hg2+

32. A solid or gas that can be formed when 2 or more aqueous reactants come together
Strong acid weak base rxn
Aufbau Principle
precipitate
Atmospheric Pressure

33. (organics) six carbons
Transition metals
Trigonal Planar
Equivalence Point
hex-

34. Oxidation # of Halogens
Enthalpy of Solution
Strong acid weak base rxn
-1
phosphate

35. Like dissolves...
End Point
triple point
heat capacity
like

36. ?H when 1 mol of bonds is broken in the gaseous state
not spontaneous
Acid + Base --> Salt + Water
dichromate
Bond enthalpy

37. x can be ignored when % ionization is <5%
5% rule
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
Its element
nitrate

38. IMF that exists in polar molecules
Dipole-dipole forces
Amphoteric
d orbitals
CAT

39. Spontaneous emission of radiation
Radioactivity
Standard Temperature and Pressure
vapor pressure
endless

40. Kinetic Energy per mol
3/2RT
Effusion
Arrhenius Acid
Molar Heat Capacity

41. A monoatomic anion is named by taking...
T-shape
red
Its root and adding -ide
Pressure of H2O must be Subtracted

42. The weighted average of all the isotopes that an atom can have (in g/mol)
Tetrahedral
Atomic Mass Unit
blue-violet
alkene

43. Substance that - when dissolved - is conductive
electrolyte
Temperature
reduction agent
entropy (S)

44. kf of water
precipitate
C=(mass)(specific heat)
Formal Charge
1.86°C

45. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
third
voltaic cells
1.38x10?²³J/K
purple

46. The reactant in the oxidizing reaction that forces the reduction reaction to occur
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
q
Normality
Reducing Agent

47. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
Isolated System
dichromate
8.314 J/K mol

48. The energy required to raise 1 g of substance 1 degree C
trigonal planar
1/2mv²
Molarity
Specific Heat (s)

49. Unusually strong dipole forces found when H is bonded to N - O - or F
Amphoteric
Hydrogen bonding
C + 273
Allotrope

50. When n=6 ->2 - color=
-2 - with peroxide -1
violet
critical point
viscosity