Test your basic knowledge |

AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. Gas to solid
period
Root Mean Square Velocity
deposition
endothermic

2. kb of water
0.512°C
Formal Charge
hydroxide
M = square root (3RT/mm)

3. pH=
log[H+]
deposition
22.4L
green/yellow

4. Organic w/ -O-
high pressure - low temperature
complex ions
insoluble
ether

5. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
Le Chatelier's Principle
alkene
Ampere

6. 1/([A]0*k)
Q>K
standard solution
work
Second-Order Half Life

7. Substance being dissolved in a solution (lower [ ])
Solute
strong acids
pent-
Counterions

8. Positive enthalpy - heat flows into system
Galvanic Cell
endothermic
Sigma Bond
activated complex (transition state)

9. (organics) nine carbons
non-
Molarity
rate gas A/rate gas B = square root (mm A/ mm B)
Bronsted-Lowry Base

10. Ionizes to produce H+ ions
square planar
Arrhenius Acid
Heat Capacity (C)
eth-

11. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
ether
period
Molecular Compounds
Oxidizing Agent

12. Peak of energy diagram
Normality
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
activated complex (transition state)
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

13. Oxidation # of Compounds
-ol
0
Pressure
Zero-Order Half Life

14. Substances that form H+ when dissolved in water; proton donors
triple point
excess reactant
Acids
Oxidizing Agent

15. Group 1 and heavier Group 2 bases
strong bases
Strong acid weak base rxn
vapor pressure
Sigma Bond

16. Substance in which something is dissolved in a solution (higher [ ])
Antibonding Molecular Orbital
Solvent
Root Mean Square Velocity
Amino-

17. Effusion of a gas is inversely proportional to the square root of the molar mass

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

18. Heat capacity formula
p
Strong acid weak base rxn
C=(mass)(specific heat)
entropy (S)

19. Type of system in which the energy may escape - but the mass is conserved
Closed System
Endothermic
condensation
Bond Energy

20. Amine prefix
Acid + Base --> Salt + Water
Bronsted-Lowry acid
Amino-
prop-

21. Generally insoluble anions (names)
-1
salt bridge
phosphate - sulfide - carbonate - sulfate
Colligative properties

22. Oxidation # of Polyatomic Ions
strong bases
Coordination Compound
0
charge

23. High-energy light
Gamma Ray-
high pressure - low temperature
oxalate
Equilibrium constant

24. CO3²?
Law of Conservation of Mass
carbonate
m (third quantum number)
nitrite

25. (organics) three carbons
specific heat
C + 273
amine
prop-

26. 180° - sp
Octahedral
Manometer
Q<K
Linear

27. MnO4¹?
red
heat capacity
permanganate
catalyst

28. AX3E2
Molarity
Covalently w/in themselves - Ionicly bonded w/ each other
T-shape
cohesion

29. Speed of Diffusion/Effusion formula
triple bond
rate gas A/rate gas B = square root (mm A/ mm B)
a precipitate forms
hydrocarbons

30. Volume of gas @STP
22.4L
dichromate
octahedral
nu

31. #NAME?
strong bases
E
22.4L
n0

32. The actual amount of product produced in an experiment
Hund's Rule
Enthalpy of Solution
Balmer Series
experimental yield

33. Planck's constant - used to calculate energy w/frequency
Surroundings
6.63x10?³4Js
phosphate - sulfide - carbonate - sulfate
Entropy (S)

34. Connects the 2 half cells in a voltaic cell
chromate
salt bridge
Counterions
Boltzmann distribution

35. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
viscosity
Buffer
Ionic Compounds
end point

36. Point at which vapor pressure=air pressure above
Balmer Series
Osmotic Pressure
Arrhenius equation
boiling point

37. (organics) double-bonded compound
Closed System
alkene
heat capacity
pi=(nRT)/v

38. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Amount of atoms present
rate
Density
Aufbau Principle

39. frequency symbol
nu
heat of fusion
first
Arrhenius Base

40. Combined Gas Law Formula
P1V1/N1T1=P2V2/N2T2
Aufbau Principle
condensation
Barometer

41. Carboxylic acid ending
London dispersion forces
(moles of products that are gasses) - (moles of reactants that are gasses)
Its element
-oic acid

42. Elements on staircase on periodic table
Metalliods
catalyst
+1 - except if bonded to Alkali Metal -1
Specific Heat Capacity

43. Tools NEEDED for dilution
Volume Metric Flask & Pipet
purple
3/2RT
force x distance = work done

44. 760 mmHg - 760 torr
Amount of atoms present
Molality
1 atm
violet

45. Mol/L - concentration of a solution
Molarity
s orbitals
cathode
increasing

46. The measurement of heat changes
conjugate acid
Ionic Compounds
Calorimetry
Pressure of H2O must be Subtracted

47. CrO4²?
chromate
Bronsted-Lowry Acid
geometric isomers
high pressure - low temperature

48. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
Pressure of H2O must be Subtracted
pent-
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
insoluble

49. AX3E
dichromate
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Anion
trigonal pyramidal

50. Unit of electrical potential; J/C
Thermochemistry
Volt
London dispersion forces
Multiplying