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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 line running between the atoms
Alpha Particles-
Work
Sigma Bond
Finding Empirical Formulas

2. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
# protons (atom is defined by this)
Hydrogen bonding
red

3. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Boltzmann distribution
Coordination Compound
rate
supercritical fluid

4. The total entropy is always increasing - all systems tend towards maximum entropy
Alpha Particles-
insoluble
Q>K
2nd law of thermodynamics

5. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Formal Charge
s (fourth quantum number)
phosphate - sulfide - carbonate - sulfate
Hydrogen bonding

6. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
Molecular Compounds
Pi Bond
Molecular
Magnetic Quantum Number (ml)

7. STP
viscosity
0 degrees C - 1 atm
Calorimeter
Amphoteric

8. Organic w/ -OH group
Second-Order Rate Law
alcohol
exothermic
sublimation

9. C2O4²?
Pressure of H2O must be Subtracted
red
oxalate
increasing

10. ClO3²?
Hydrogen bonding
chlorate
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
Calorimetry

11. Diatomic Molecules
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
3rd law of thermodynamics
Hund's Rule
Colligative properties

12. If Q>Ksp
a precipitate forms
Molal FP Depression Constant
Pauli Exclusion Principle
Atmospheric Pressure

13. Symbol for Total Heat absorbed or released
q
equilibrium
salt bridge
Theory of Relativity

14. Wavelength symbol
Beta Particles-
lambda
boiling point
pi=(nRT)/v

15. Stronger IMF= lower... weaker IMF= higher...
eth-
vapor pressure
n (first quantum number)
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

16. Group 1 metals
melting point
AE= AH - RTAn
Alkali metals
Percent Yield

17. SO4²?
conjugate base
Entropy (S)
sulfate
Octahedral

18. How to Find an Empirical Formula Given Percentages
Chemical Kinetics
8.31J/Kmol
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Heat

19. A device in which chemical energy is changed to electrical energy
red
Density
Galvanic Cell
k=Ae^(-Ea/RT)

20. Elements which have all electrons paired and relatively unaffected by magnetic fields
bromate
Dipole Moment
Nernst Equation
diamagnetic

21. If anion ends in -ite - acid name ends in...
van't Hoff Factor
-ous acid
96500
Dipole Moment

22. IMF that exists in polar molecules
methoxy-
s (fourth quantum number)
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Dipole-dipole forces

23. 760 mmHg - 760 torr
entropy
1/2mv²
1 atm
deposition

24. When n=3 ->2 - color=
Specific Heat (s)
0
red
Arrhenius Acid

25. Generally insoluble anions (names)
vapor pressure
# protons + # neutrons
Galvanic Cell
phosphate - sulfide - carbonate - sulfate

26. Degree of disorder in a system
chromate
conjugate base
entropy (S)
s

27. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
0.0821 atm L/mol K
permanganate
22.4L
Law of Multiple Proportions

28. Aldehyde suffix
Boltzmann distribution
prop-
Bond Order
-al

29. ln[A]=-kt + ln[A]0
Overall Reaction Order
weak acid strong base rxn
Integrated First-Order Rate Law
base

30. ClO4¹?
Metalliods
perchlorate
Zero-Order Rate Law
log[H+]

31. AX4E
seesaw
Angular Momentum Quantum Number
iodide
chlorite

32. Newton's Second Law
Force = mass x acceleration
Arrhenius Base
meth-
critical point

33. Kinetic Energy of an individual particle formula
Multiplying
M = square root (3RT/mm)
Covalently w/in themselves - Ionicly bonded w/ each other
Molarity

34. Carbon - hydrogen - oxygen compounds
# protons (atom is defined by this)
Le Chatelier's Principle
carbohydrates
s orbitals

35. E=mc^2
Covalently w/in themselves - Ionicly bonded w/ each other
Trigonal Planar
5% rule
Theory of Relativity

36. Ionizes to produce OH- Ions
Arrhenius Base
Speed of light
amine
Force = mass x acceleration

37. AX6
octahedral
Equilibrium constant
Weight
specific heat

38. A molecule having a center of positive charge and a center of negative charge
yellow --> green
Dipole Moment
Hund's Rule
Graham's Law

39. r=k
Zero-Order Rate Law
Quantum Numbers
salt bridge
A Roman numeral

40. Electron (symbol)
e-
?Tb= kb x molality
Endothermic
permanent gases

41. 1 sigma bond
Ampere
single bond
insoluble
Quantum Numbers

42. A measure of resistance of an object to a change in its state of motion
chlorite
viscosity
Molecular Orbitals (MOs)
Mass

43. All cations are soluble with sulfate EXCEPT
condensation
Cathode
Open System
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+

44. How to Find a Weighted Average
phosphate - sulfide - carbonate - sulfate
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
hydro-ic acid
Limiting reactant

45. Rate of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
endless
Barometer
blue

46. Non-Ideal Gas Conditions
chlorate
high pressure - low temperature
Ionic
diamagnetic

47. Color of Cs (flame test)
heat capacity
equivalence point
k=Ae^(-Ea/RT)
blue

48. 2 or more covalently bonded atoms
Open System
Molecule
nitrate
condensation

49. Combined Gas Law Formula
Heat Capacity (C)
chromate
system
P1V1/N1T1=P2V2/N2T2

50. Boiling point elevation formula
Pauli Exclusion Principle
carbonate
?Tb= kb x molality
work