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AP Chemistry

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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. PV=nRT
Ideal Gas Law
State Functions
Endothermic
fusion

2. l=1
endothermic
p
msAT
triple point

3. Elements which have unpaired electrons and highly affected by magnetic fields
Oxidation is Loss Reduction is Gain
hex-
paramagnetic
zero

4. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals

5. For significant digits - leading zeros ____ significant
Negative work value; work done by system
are not
purple --> pink
0

6. Polyatomic Ions (bonding)
Increase Temperature
chloride
Octahedral
Covalently w/in themselves - Ionicly bonded w/ each other

7. Osmotic pressure=MRT
Galvanic Cell
Osmotic Pressure
prop-
Linear

8. Weakest IMFs - found in all molecules
0
soluble
endless
London dispersion forces

9. When n=4 ->2 - color=
endless
blue-green
moles of solute/ L of solution
-al

10. Point at which solid?liquid occurs
melting point
Zero-Order Half Life
N=N.(0.5)^time/time half-life
mol Fraction

11. q rxn = ?
log[H+]
Formal Charge
-(q of H2O + q of cal)
but-

12. Two molecules with identical connectivity but different geometries
second
v3kT/m
geometric isomers
exothermic

13. Atomic #
Coordination Compound
fusion
# protons (atom is defined by this)
equivalence point

14. Proton donors
Bronsted-Lowry acid
are
flouride
AE = q + w

15. 120° - sp^2
boiling point
Ampere
Trigonal Planar
Polar Covalent

16. #NAME?
Hydrogen bonding
E
Aufbau Principle
LE Model

17. Color of Sr (flame test)
State Functions
Hydrogen bonding
0
red

18. x can be ignored when % ionization is <5%
Molecular
Polar Covalent
Average KE = 1/2(mass)(average speed of all particles)
5% rule

19. Volume of gas @STP
Beta Particles-
s orbitals
22.4L
Cg=kPg

20. A weak acid that changes color at or near the equivalence point
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
-oic acid
indicator
Arrhenius Base

21. When n=6 ->2 - color=
are
bent
violet
# protons (atom is defined by this)

22. AX4E2
square planar
Allotrope
condensation
v3kT/m

23. The entropy of a pure perfectly formed crystal @0K is 0
Solvent
3rd law of thermodynamics
Open System
First-Order Rate Law

24. Variable for orientation of orbital (-1 through +1)
Manometer
m (third quantum number)
Positive work value; work done on system
Negative work value; work done by system

25. kb of water
period
0.512°C
# protons + # neutrons
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+

26. (organics) six carbons
hex-
Limiting reactant
entropy
Molality

27. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
bent
third
complex ions
nitrate

28. Freezing point depression formula
Bronsted-Lowry Acid
Polar Covalent
?Tf= kf x molality
nitrite

29. Mol of solute/kg of solvent
Le Chatelier's Principle
Exothermic
Molality
Isotopes

30. ?Hsoln=?H1+?H2+?H3+...
0
Enthalpy of Solution
Tetrahedral
Formal Charge

31. Change in moles (An) =?
Ionic Compounds
First-Order Rate Law
(moles of products that are gasses) - (moles of reactants that are gasses)
flouride

32. (A) - C/s
Ampere
-one
blue-violet
Molar Mass of Element/ Total Molar Mass %

33. Boiling point elevation formula
0 degrees C - 1 atm
Amino-
?Tb= kb x molality
dichromate

34. % yield
boiling point
First-Order Rate Law
actual yield/theoretical yield x 100%
Oxidizing Agent

35. AX4E2
square planar
0
Hess's Law
are not

36. # bonding e- - # antibonding e-/2
Bond Order
f
?Tb= kb x molality
first

37. (organics) ten carbons
dec-
soluble
?Hvap
chloride

38. Mixing of gases
viscosity
Diffusion
Acids
indicator

39. (organics) three carbons
prop-
-1
effects of IMF
entropy

40. Ether prefix
sulfate
trigonal planar
Allotrope
methoxy-

41. C2O4²?
Amino-
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
oxalate
Allotrope

42. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
s orbitals
Kinetic Molecular Theory - for ideal gases
Colligative properties
strong bases

43. Colors of Reaction when (MnO4 -) --> (Mn2+)
purple --> pink
Second-Order Half Life
Overall Reaction Order
cohesion

44. Kinetic Energy of an individual particle formula
iodide
Molal BP Elevation Constant
M = square root (3RT/mm)
Kinetic Molecular Theory - for ideal gases

45. Involves quantum numbers
Quantum Mechanical Model
critical point
msAT
base

46. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium

47. Raising heat - adding catalyst - heighten concentration - bigger surface area
p
Amino-
Formal Charge
methods of increasing rate

48. The chemical formed when an acid donates a proton
conjugate base
Calorimeter
acid
trigonal bipyramidal

49. kf of water
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
1.86°C
Force = mass x acceleration
Molarity

50. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
strong acids
Mass
0
hydroxide