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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. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Atmospheric Pressure
chlorate
perchlorate
base and hydrogen gas

2. Theoretical yield-experimental yield/theoretical yieldx100
% error
Calorimeter
Integrated Second-Order Rate Law
n (first quantum number)

3. Ending for alcohols
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
-ol
heat of fusion
Acid + Base --> Salt + Water

4. Mole Fraction
X of a = moles a/total moles
hex-
effects of IMF
square planar

5. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
Atomic Mass Unit
spontaneity
Finding Empirical Formulas
entropy (S)

6. OH¹?
Ionic
octahedral
permanganate
hydroxide

7. When n=3 ->2 - color=
Normality
n (first quantum number)
red
Second-Order Rate Law

8. Bomb Calorimeter
trigonal planar
phosphate - sulfide - carbonate - sulfate
cohesion
Constant Volume

9. 2+ charge
trigonal bipyramidal
Alpha Particles-
0.512°C
mol Fraction

10. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
Gamma Ray-
pent-
seesaw
insoluble

11. Phase change from solid to gas
sublimation
T-shape
Law of Multiple Proportions
Overall Reaction Order

12. F¹?
Aufbau Principle
flouride
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
Decrease Volume and Increase Temperature

13. A measure of randomness or disorder
Nernst Equation
entropy
cathode
3/2RT

14. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
alkene
solid CO2
Theoretical yield
Chemical Kinetics

15. Delta H (AH) = ?
Equivalence Point
q/moles
square planar
Amphoteric

16. x can be ignored when % ionization is <5%
Pi Bond
5% rule
moles solute/kg solvent
AH

17. Phase change from gas to solid
Isolated System
isothermal
Constant Pressure
deposition

18. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
hex-
voltaic cells
C=(mass)(specific heat)
amine

19. Type of system in which nothing is transfered (no mass or energy); ideal
m (third quantum number)
Isolated System
Equivalence Point
group

20. AX5
octahedral
trigonal bipyramidal
Integrated First-Order Rate Law
Buffered Solution

21. 0.00°C - 1 atm
Standard Temperature and Pressure
Molal FP Depression Constant
oxidation
nitrate

22. AP doesn't deal with ...-order reaction - don't pick it!
Aufbau Principle
hydro-ic acid
-oic acid
third

23. Heat needed to change 1 g of substance to 1°C
specific heat
1 atm
Quantum Model
not spontaneous

24. Carboxylic acid ending
-oic acid
like
Quantum Numbers
catalyst

25. These orbitals are spherical
trigonal bipyramidal
heat of fusion
strong acid strong base rxn
s orbitals

26. U(rms)=(3RT/M)^1/2
Isolated System
Root Mean Square Velocity
s
-1

27. l=2
group
LeChatelier's Principle
d
Isotopes

28. 6.022x10^23
precipitate
mol
p+
oxide gas and water

29. When n=4 ->2 - color=
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Equilibrium constant
blue-violet
blue-green

30. The minimum energy that molecules must possess for collisions to be effective - Ea
Integrated Zero-Order Rate Law
non-
Volt
activation energy

31. Chemical composition of dry ice
octahedral
solid CO2
Octahedral
blue

32. 1/[A] vs. time is a ...-order reaction
second
not spontaneous
isothermal
Molality

33. Arrhenius equation
Arrhenius base
Molecular
k=Ae^(-Ea/RT)
acid

34. Half-life equation
First-Order Half Life
sulfide
N=N.(0.5)^time/time half-life
rate law

35. Thickness
viscosity
blue-green
Acids
Hydrogen bonding

36. For significant digits - leading zeros ____ significant
are not
-ic acid
Counterions
Heat Capacity (C)

37. 180° - sp
sulfide
vaporization
AE = q + w
Linear

38. Oxidation # of Hydrogen
specific heat
+1 - except if bonded to Alkali Metal -1
Heat Capacity (C)
Molality

39. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change

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40. Calculation from K to C
C + 273
p
weak acid strong base rxn
first

41. Increase Volume
work
Cathode
Dipole Moment
Increase Temperature

42. 120° - sp^2
Zero-Order Half Life
Trigonal Planar
London dispersion forces
P of a =(X of a)(total pressure)

43. Mass reactants= mass products
Anode
entropy
E
Law of Conservation of Mass

44. Speed of Diffusion/Effusion formula
sulfate
rate gas A/rate gas B = square root (mm A/ mm B)
Ag+ - Pb2+ - Hg2+
viscosity

45. 760mmHg/Torr
Hybridization
0
1atm=?mmHg/Torr
charge

46. Kinetic Energy per molecule
1/2mv²
Le Chatelier's Principle
Arrhenius Acid
-(P)(Change in V)

47. 0°C and 1 atm
London dispersion forces
STP
System
Atmospheric Pressure

48. The mixing of native atomic orbitals to form special orbitals for bonding
Bronsted-Lowry base
Hybridization
carbohydrates
spontaneity

49. Horizontals on the periodic table
period
Law of Conservation of Mass
Effusion
q

50. Group 1 metals
m (third quantum number)
Exothermic
Alkali metals
Electron Spin Quantum Number