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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. Anything occupying space and with mass
e-
Matter
Molarity
methoxy-

2. Kinetic Energy is proportional to ______
Temperature
supercritical fluid
Le Chatelier's Principle
Constant Pressure

3. Force per unit area
Pressure
1atm=?mmHg/Torr
CAT
Theory of Relativity

4. Dirrect Method Formula
Aufbau Principle
methoxy-
Quantum Mechanical Model
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

5. CO3²?
Covalently w/in themselves - Ionicly bonded w/ each other
1atm=?Pa
carbonate
third

6. Elements which have unpaired electrons and highly affected by magnetic fields
Aufbau Principle
paramagnetic
viscosity
chlorate

7. Positive enthalpy - heat flows into system
endothermic
Speed of light
acid
London dispersion forces

8. Wavelength symbol
lambda
spontaneity
allotrope
Ag+ - Pb2+ - Hg2+

9. Dalton's Law of Partial Pressures (to find partial pressure formula)
P of a =(X of a)(total pressure)
Amino-
% error
cathode

10. # bonding e- - # antibonding e-/2
Scientific Method
Bond Order
complex ions
acid

11. Moles of solute/volume of soln(L)
Molarity
supercritical fluid
Heat
1.38x10?²³J/K

12. Aldehyde suffix
First-Order Rate Law
system
Bronsted-Lowry acid
-al

13. E?s fill the lowest energy orbital first - then work their way up
Aufbau Principle
P of a =(X of a)(total pressure)
zero
v3kT/m

14. Significant Digits of counted things
Work
salt bridge
endless
hydrocarbons

15. Coffee Cup Calorimeter
4.184
Constant Pressure
adiabatic
Coordination Compound

16. AX2E - AX2E2
bent
s orbitals
m (third quantum number)
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

17. Increase Volume
Increase Temperature
Bronsted-Lowry Acid
cyanide
Calorimeter

18. In covalent bonds - prefixes are used to tell...
Calorimeter
Integrated First-Order Rate Law
a precipitate forms
Amount of atoms present

19. PO4³?
fusion
phosphate
Electronegativity
Solvent

20. If anion ends in -ide - acid name ends in
hydro-ic acid
cyanide
red
Second-Order Half Life

21. Combined Gas Law Formula
endless
P1V1/N1T1=P2V2/N2T2
sulfite
hydrolysis

22. Absorbs/takes in heat (positive value)
Endothermic
mol Fraction
soluble
strong acid strong base rxn

23. Measure of the average kinetic energy of all the particles in a substance
M1V1=M2V2
1st law of thermodynamics
p+
Temperature

24. The heat changed in a chemical reaction.
Barometer
Ionic Compounds
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
Thermochemistry

25. ln[A] vs. time is a ...-order reaction
first
sulfite
Quantum Numbers
ammonium

26. Symbol for Enthalpy
H
analyte
Electronegativity
Cathode

27. OIL RIG
bent
Normality
Oxidation is Loss Reduction is Gain
Aufbau Principle

28. When _____ significant digits - round answer to least significant digit
Trigonal Bipyramidal
prop-
Multiplying
ether

29. 120° - sp^2
Tetrahedral
Radioactivity
Trigonal Planar
Beta Particles-

30. Gas to liquid
hydrolysis
Chemical Kinetics
condensation
Aufbau Principle

31. Liquid to gas
PV=nRT
Equivalence Point
viscosity
vaporization

32. Molecules' tendency to stick to one another
cohesion
square planar
fusion
are not

33. Mixing of gases
Diffusion
permanganate
Reducing Agent
Mass

34. [A]0/2k
Zero-Order Half Life
Molecular Compounds
Dipole Moment
Pressure

35. Group 2 metals
Alkaline earth metals
nitrite
permanent gases
but-

36. Newton's Second Law
Force = mass x acceleration
LE Model
Hund's Rule
square planar

37. AX4E2
square planar
Zero-Order Half Life
s orbitals
Molality

38. In ideal gas law problem - when it says "atmospheric" ...
soluble
Integrated Zero-Order Rate Law
Pressure of H2O must be Subtracted
hydroxide

39. Kinetic Energy per molecule
Boltzmann distribution
Dipole Moment
1/2mv²
v3RT/M(in kg)

40. All cations are soluble with sulfate EXCEPT
linear
P of a =(X of a)(total pressure)
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Nodes

41. Type of system in which the energy and mass may leave or enter
mol
+1 - except if bonded to Alkali Metal -1
Polar Covalent
Open System

42. Driving force of the electrons
(moles of products that are gasses) - (moles of reactants that are gasses)
reduction
base and hydrogen gas
Cell Potential (Ecell)

43. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
Galvanic Cell
like
Hydrogen bonding

44. Liquid to solid
Bases
trigonal bipyramidal
Calorimetry
freezing

45. Anions or cations as needed to produce a compound with non net charge
Counterions
London dispersion forces
Anion
Bond enthalpy

46. Oxidation # of Compounds
0
square planar
s orbitals
hydro-ic acid

47. (organics) triple-bonded compound
Matter
alkyne
red
blue-violet

48. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
LeChatelier's Principle
supercritical fluid
Kinetic Molecular Theory - for ideal gases
Acids

49. Happens at lines in phase change charts
alkene
equilibrium
sublimation
AH

50. (organics) five carbons
alkene
Boltzmann distribution
pent-
oxidizing agent