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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. Arrhenius equation
?Hvap
red
k=Ae^(-Ea/RT)
Q>K

2. l=2
d
acetate
Galvanic Cell
voltaic cells

3. These orbitals are diagonal
yellow
non-
Principal Quantum Number
d orbitals

4. kb of water
Counterions
hex-
endothermic
0.512°C

5. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
oxalate
condensation
-al
hydrolysis

6. Tools NEEDED for dilution
Volume Metric Flask & Pipet
Solubility Product (Ksp)
Polar Covalent
trigonal pyramidal

7. Faraday's constant
activation energy
96500
4.184
T-shape

8. The likelihood that a rxn will occur "by itself"
spontaneity
Q<K
Electron Spin Quantum Number
Buffered Solution

9. Group 1 metals
Alkali metals
Formal Charge
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
Arrhenius base

10. Heat required to raise the system 1°C
Integrated Rate Law
first
Valence Electrons(assigned)
heat capacity

11. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Manometer
n (first quantum number)
Bases
0.0821 atm L/mol K

12. Average Kinetic Energy Formula
Antibonding Molecular Orbital
Hund's Rule
red
Average KE = 1/2(mass)(average speed of all particles)

13. Variable for energy of e- - goes from 1 -2 -3 on up
chloride
Bond Order
n (first quantum number)
violet

14. The entropy of a pure perfectly formed crystal @0K is 0
condensation
M1V1=M2V2
3rd law of thermodynamics
oct-

15. (organics) nine carbons
phosphate
-one
non-
Alkali metals

16. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
tetrahedral
q
Diffusion

17. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps

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18. These orbitals are spherical
s orbitals
Hydrogen bonding
methods of increasing rate
alcohol

19. All forms of energy except for heat
work
reduction
Second-Order Rate Law
Graham's Law

20. Osmotic pressure=MRT
sulfide
Osmotic Pressure
C + 273
square pyramidal

21. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
Molecule
Standard Temperature and Pressure
Molecular

22. OH¹?
hydroxide
-one
red
heat of fusion

23. Oxoacid solution (such as HSO4-) forms...
Molality
mol Fraction
oxide gas and water
msAT

24. Carbon - hydrogen - oxygen compounds
P of a =(X of a)(total pressure)
condensation
v3RT/M(in kg)
carbohydrates

25. Mass #
# protons + # neutrons
titrant buret
State Functions
Net Ionic Equation

26. An equilibrium expression
3rd law of thermodynamics
Molecular Compounds
Solubility Product (Ksp)
Pressure of H2O must be Subtracted

27. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
Force = mass x acceleration
soluble
carbohydrates
Quantum Numbers

28. Dalton's Law of Partial Pressures (to find partial pressure formula)
strong bases
bond energy
Mass
P of a =(X of a)(total pressure)

29. This MUST be determined experimentally
Linear
rate law
Theory of Relativity
green/yellow

30. The total entropy is always increasing - all systems tend towards maximum entropy
Bronsted-Lowry Acid
2nd law of thermodynamics
endless
increasing

31. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
Effusion
s
strong acid strong base rxn

32. Where reduction occurs
insoluble
Surroundings
linear
Cathode

33. How to Find a Weighted Average
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Pressure of H2O must be Subtracted
Constant Pressure
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

34. CO3²?
strong acids
carbonate
oxide
Aufbau Principle

35. Type of system in which the energy and mass may leave or enter
Open System
alkene
0.0826Latm/Kmol
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

36. A device in which chemical energy is changed to electrical energy
Galvanic Cell
t-shape
Force = mass x acceleration
Linear

37. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
Volt
Bond Energy
5% rule
Ligand

38. A monoatomic anion is named by taking...
prop-
Its root and adding -ide
carbohydrates
ammonium

39. How to Find an Empirical Formula Given Grams
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Dipole-dipole forces
A Roman numeral
C + 273

40. Energy needed to break a bond
trigonal bipyramidal
C + 273
bond energy
Lone Pair

41. Force per unit area
chloride
Constant Pressure
Covalently w/in themselves - Ionicly bonded w/ each other
Pressure

42. Amount of gravitational force exerted on an object
Weight
Transition metals
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
C=(mass)(specific heat)

43. Substance in which something is dissolved in a solution (higher [ ])
Solvent
Volt
First-Order Rate Law
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

44. (organics) double-bonded compound
8.31J/Kmol
1/2mv²
acetate
alkene

45. R=
Multiplying
8.31J/Kmol
red
purple

46. Pressure Units/Conversions
red
q/moles
H
1 atm = 760 mmHg = 101.3 kPa

47. Point at which solid?liquid occurs
a precipitate forms
melting point
Aufbau Principle
boiling point

48. Hydroxides are soluble or insoluble?
First-Order Half Life
Molarity
insoluble
3rd law of thermodynamics

49. AX5
A Roman numeral
trigonal bipyramidal
single bond
8.314 J/K mol

50. Ka=[products]^m/[reactants]^n
charge
Acid Dissociation Constant
oct-
rate