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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. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Osmotic Pressure
voltaic cells
yellow --> green
-(P)(Change in V)

2. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Law of Multiple Proportions
State Functions
Atmospheric Pressure
solid CO2

3. Organic w/ -O-
ether
sublimation
Hydrogen bonding
C=(mass)(specific heat)

4. Measure of the change in enthalpy
charge
P1= X1P1°
Delta H or Enthalpy Change
fusion

5. Specific heat of water
q
-oic acid
strong acids
4.184

6. Anything occupying space and with mass
l (second quantum number)
Matter
Isolated System
-ol

7. A single substance that may be an acid or a base (i.e. water)
Amphoteric
Specific Heat Capacity
viscosity
Volume Metric Flask & Pipet

8. Group 2 metals
Alkaline earth metals
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
chlorite
8.31J/Kmol

9. Reverse rxn occurs when
Le Chatelier's Principle
Q>K
Joule
-ous acid

10. (organics) eight carbons
oct-
f
vaporization
Magnetic Quantum Number (ml)

11. CrO4²?
adiabatic
rate law
chromate
different # of neutrons

12. ln[A] vs. time is a ...-order reaction
first
red
violet
melting

13. Polyatomic Ions (bonding)
bent
equivalence point
l (second quantum number)
Covalently w/in themselves - Ionicly bonded w/ each other

14. Describe various properties of one orbital
sulfide
Quantum Numbers
freezing
reduction agent

15. Average Kinetic Energy Formula
Molar Mass of Element/ Total Molar Mass %
adhesion
Average KE = 1/2(mass)(average speed of all particles)
Graham's Law

16. 1/[A]=kt + 1/[A]0
Bases
Integrated Second-Order Rate Law
Octahedral
hydrolysis

17. Mixing of gases
ether
Diffusion
Multiplying
1st law of thermodynamics

18. When ____ significant digits - round answer to least decimal place
Adding
wavelength
Overall Reaction Order
third

19. Aldehyde suffix
Sigma Bond
-al
0.512°C
endothermic

20. Pressure Units/Conversions
1 atm = 760 mmHg = 101.3 kPa
heat capacity
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
Galvanic Cell

21. A method of investigation involving observation and theory to test scientific hypotheses
Volt
4.184
Principal Quantum Number
Scientific Method

22. When n=4 ->2 - color=
increasing
precipitate
see-saw
blue-green

23. AX3
trigonal planar
LE Model
CAT
-oate

24. Substance that - when dissolved - is conductive
Bronsted-Lowry Base
electrolyte
r1/r2
Bronsted-Lowry acid

25. Mol of solute/kg of solvent
Molality
Aufbau Principle
Alpha Particles-
titrant buret

26. Change in Energy (AE) = ? (in terms of work)
-(P)(Change in V)
Oxidizing Agent
Law of Multiple Proportions
AE = q + w

27. Force that holds atoms together
22.4L
Oxidation is Loss Reduction is Gain
Chemical Bonds
rate law

28. Ideal Gas Law Formula
van't Hoff Factor
(moles of products that are gasses) - (moles of reactants that are gasses)
PV=nRT
Faraday

29. Ptotal=P1+P2+P3+...

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30. Variable for energy of e- - goes from 1 -2 -3 on up
Cathode
Specific Heat (s)
n (first quantum number)
hydro-ic acid

31. If heat capacity isn't mentioned - you can assume that q of cal is = ?
Naming Binary Ionic Compounds
msAT
Acids
0

32. Releases/gives off heat (negative value)
nitrate
Bond Order
Exothermic
-ol

33. Horizontals on the periodic table
Theoretical yield
sublimation
Quantum Numbers
period

34. Newton's Second Law
Force = mass x acceleration
22.4L
Root Mean Square Velocity
0.0821 atm L/mol K

35. A device in which chemical energy is changed to electrical energy
Galvanic Cell
f
Molecule
Constant Volume

36. ClO2¹?
spontaneity
red
van't Hoff Factor
chlorite

37. These orbitals are spherical
0.512°C
Hydrogen bonding
Second-Order Half Life
s orbitals

38. 1 sigma bond
Hund's Rule
Specific Heat Capacity
see-saw
single bond

39. Energy needed to break a bond
bond energy
State Functions
Overall Reaction Order
Formal Charge

40. .69/k
First-Order Half Life
Anion
Percent Yield
high pressure - low temperature

41. Has values 1 -2 -3 -...; tells energy levels
eth-
AE= AH - RTAn
Principal Quantum Number
% error

42. Driving force of the electrons
pi=(nRT)/v
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
-(P)(Change in V)
Cell Potential (Ecell)

43. l=3
f
X of a = moles a/total moles
oxidation
condensation

44. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
LE Model
Bond enthalpy
0
red

45. Oxidation # of Hydrogen
increasing
+1 - except if bonded to Alkali Metal -1
Molecular Orbitals (MOs)
Zero-Order Half Life

46. AX4E
seesaw
spontaneity
Pauli Exclusion Principle
flouride

47. Force acting over distance
activation energy
Oxidation is Loss Reduction is Gain
effects of IMF
Work

48. Peak of energy diagram
deposition
force x distance = work done
activated complex (transition state)
octahedral

49. Mass/volume
Second-Order Rate Law
Molar Mass of Element/ Total Molar Mass %
Density
standard solution

50. 2 or more covalently bonded atoms
London dispersion forces
Hydrogen bonding
Molecule
strong acid strong base rxn