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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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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. Variable for energy of e- - goes from 1 -2 -3 on up
Cg=kPg
Dipole-dipole forces
g solute/g solvent x 100
n (first quantum number)

2. Organic w/ -NH2
Effusion
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
amine
0.0826Latm/Kmol

3. Arrhenius equation
reduction agent
Hybridization
pent-
k=Ae^(-Ea/RT)

4. Substances that form OH- when dissolved in water; proton acceptors
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
+1 - except if bonded to Alkali Metal -1
Equilibrium constant
Bases

5. AX4
Molecular Compounds
Molality
iodide
tetrahedral

6. Energy needed to vaporize a mole of a liquid
-oate
Molar Heat Capacity
viscosity
?Hvap

7. Symbol for Enthalpy
catalyst
H
Atomic Mass Unit
oxalate

8. Substances w/ critical temperatures below 25°C
standard solution
cyanide
permanent gases
Hund's Rule

9. How to Find a Weighted Average
Law of Multiple Proportions
1atm=?mmHg/Torr
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Cation

10. For significant digits - leading zeros ____ significant
Cation
condensation
Average KE = 1/2(mass)(average speed of all particles)
are not

11. [A]0/2k
-ic acid
Zero-Order Half Life
Ionic
CAT

12. Combined Gas Law Formula
lambda
Isolated System
P1V1/N1T1=P2V2/N2T2
Aufbau Principle

13. High-energy light
1 atm
Gamma Ray-
but-
standard solution

14. Solution used in titration
titrant buret
Q<K
0 degrees C - 1 atm
Constant Volume

15. Significant Digits of Conversion Factors
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
3rd law of thermodynamics
-2 - with peroxide -1
endless

16. AX5
Joule
trigonal bipyramidal
chlorite
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

17. Degree of disorder in a system
Enthalpy of Solution
entropy (S)
heat capacity
base and hydrogen gas

18. Ketone suffix
Scientific Method
Law of Conservation of Mass
-one
acid

19. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
rate law
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
London Dispersion Forces
no precipitate forms

20. Verticals on the periodic table
group
Positive work value; work done on system
Resonance
purple --> pink

21. Each orbital can hold two e?s each w/ opposite spins
chromate
Pauli Exclusion Principle
electron affinity
Reducing Agent

22. l=3
f
oxide gas and water
critical point
Molal FP Depression Constant

23. r=k[A]
Cell Potential (Ecell)
Metalliods
First-Order Rate Law
Thermochemistry

24. We cannot simultaneously determine an atom's exact path or location
Law of Multiple Proportions
Bonding Pairs
vapor pressure
Heisenberg Uncertainty Principle

25. A molecule having a center of positive charge and a center of negative charge
Dipole Moment
96500
Solvent
moles of solute/ L of solution

26. (organics) six carbons
M1V1=M2V2
strong acids
Bond Energy
hex-

27. 90° - d^2sp^3
pi=(nRT)/v
voltaic cells
Octahedral
g solute/g solvent x 100

28. Oxoacid solution (such as HSO4-) forms...
Hess's Law
Reducing Agent
endothermic
oxide gas and water

29. A solution used in titrations whose concentration is known
Amphoteric
standard solution
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
E

30. Rate of Diffusion/Effusion formula
Q>K
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
oxalate
Effusion

31. If anion ends in -ite - acid name ends in...
-ous acid
Buffer
Atomic Mass Unit
k=Ae^(-Ea/RT)

32. # bonding e- - # antibonding e-/2
Bond Order
Allotrope
CAT
salt bridge

33. R=
pi=(nRT)/v
t-shape
Electron Spin Quantum Number
8.31J/Kmol

34. Ester suffix
isothermal
Specific Heat (s)
First-Order Rate Law
-oate

35. (organics) nine carbons
0.0821 atm L/mol K
ammonium
1/2mv²
non-

36. Spectrum of light when an electron drops to energy level n=2
Metalliods
3.0x108m/s
Balmer Series
Endothermic

37. AX2 - AX2E3
Quantum Mechanical Model
linear
trigonal planar
hydro-ic acid

38. Pairs of electrons localized on an atom
Solubility Product (Ksp)
Lone Pair
Increase Temperature
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

39. Tools NEEDED for dilution
Volume Metric Flask & Pipet
-ol
group
Alkali metals

40. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Molecular
Hybridization
seesaw
Enthalpy of Solution

41. When _____ significant digits - round answer to least significant digit
Multiplying
Cg=kPg
hydroxide
indicator

42. The line running between the atoms
trigonal bipyramidal
square planar
Sigma Bond
Q<K

43. ln[A]=-kt + ln[A]0
heat capacity
Bronsted-Lowry acid
Integrated First-Order Rate Law
heat of vaporization

44. ?T=k*m(solute)
First-Order Rate Law
third
Hybridization
Molal FP Depression Constant

45. l=2
d
Solute
Constant Pressure
deposition

46. Color of Li (flame test)
seesaw
alkene
red
Pressure

47. AX4E2
Overall Reaction Order
0.0826Latm/Kmol
m (third quantum number)
square planar

48. AX4E2
permanganate
oxidation
square planar
A Roman numeral

49. How to Balance a Redox Equation
t-shape
Ideal Gas Law
k=Ae^(-Ea/RT)
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

50. Consists of a complex ion - a transition metal with attached ligands - and counterions
Coordination Compound
methods of increasing rate
Its root and adding -ide
iodide