Test your basic knowledge |

AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
If you are not ready to take this test, you can study here.
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. Donates a single H+ Ion (... other prefixes also)
Monoprotic
0.0826Latm/Kmol
alcohol
Quantum Mechanical Model

2. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
End Point
Metalliods
Zero-Order Half Life
strong acids

3. Positive ion
Bond Order
Cation
e-
M = square root (3RT/mm)

4. IMF that occurs with FON
Equilibrium constant
First-Order Rate Law
increasing
Hydrogen bonding

5. Carboxylic acid ending
titrant buret
Barometer
-oic acid
22.4L

6. Theoretical yield-experimental yield/theoretical yieldx100
% error
bromate
endothermic
-oic acid

7. Increase Pressure
Decrease Volume and Increase Temperature
Monoprotic
seesaw
log[H+]

8. Nonmetal oxide + H2O ->
Coordination Compound
Barometer
Principal Quantum Number
acid

9. Ending for alcohols
blue-green
oxidation
-ol
Principal Quantum Number

10. Where reduction occurs
Principal Quantum Number
Cathode
msAT
Acid + Base --> Salt + Water

11. I¹?
trigonal bipyramidal
iodide
Pauli Exclusion Principle
0

12. 1/([A]0*k)
Integrated Rate Law
Second-Order Half Life
4.184
are not

13. C2O4²?
chlorate
Closed System
sulfide
oxalate

14. Loss of electrons - increase in oxidation #
base and hydrogen gas
-2 - with peroxide -1
chlorite
oxidation

15. HF+ OH??H2O
period
Diffusion
weak acid strong base rxn
oxalate

16. If heat capacity isn't mentioned - you can assume that q of cal is = ?
adiabatic
Osmotic Pressure
0
X of a = moles a/total moles

17. Oxidation # of Compounds
entropy
-oate
0
hept-

18. 1 sigma bond
Q>K
single bond
Finding Empirical Formulas
geometric isomers

19. Point at which vapor pressure=air pressure above
square pyramidal
boiling point
Hydrogen bonding
ln (k1/k2) = (Ea/R)(1/T2-1/T1)

20. Spectrum of light when an electron drops to energy level n=2
trigonal bipyramidal
Temperature
Balmer Series
-(q of H2O + q of cal)

21. AX3
eth-
methods of increasing rate
Arrhenius base
trigonal planar

22. These orbitals are diagonal
Cathode
d orbitals
Solvent
AE= AH - RTAn

23. Metal oxide + H20 ->
Polar Covalent
Diffusion
end point
base

24. 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

Warning: Invalid argument supplied for foreach() in /var/www/html/basicversity.com/show_quiz.php on line 183

25. Change in Energy = ? (in terms of constant pressure; for gasses)
AE= AH - RTAn
Coordination Compound
fusion
tetrahedral

26. Energy involved in gaining an electron to become a negative ion
electron affinity
hydrocarbons
condensation
vapor pressure

27. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
Dipole Moment
not spontaneous
iodide
Hund's Rule

28. Negative enthalpy - heat flows into surroundings
End Point
red
exothermic
Increase Temperature

29. Heat needed to change 1 g of substance to 1°C
5% rule
heat of fusion
specific heat
E

30. (organics) five carbons
Integrated Zero-Order Rate Law
insoluble
M1V1=M2V2
pent-

31. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
Molecular Compounds
Reaction Quotient (Q)
a precipitate forms

32. When n=5 ->2 - color=
q/moles
3.0x108m/s
blue-violet
Buffer

33. Symbol for Enthalpy
Allotrope
titrant buret
H
Osmotic Pressure

34. Temperature-pressure point after which gas can no longer form liquid
Colligative properties
Valence Electrons(assigned)
critical point
0

35. Mass #
# protons + # neutrons
Buffered Solution
reduction agent
# protons (atom is defined by this)

36. 101 -325 Pa
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
(moles of products that are gasses) - (moles of reactants that are gasses)
Ag+ - Pb2+ - Hg2+
1atm=?Pa

37. In ideal gas law problem - when it says "atmospheric" ...
Second-Order Half Life
STP
8.31J/Kmol
Pressure of H2O must be Subtracted

38. AX4E
Its root and adding -ide
Decrease Volume and Increase Temperature
see-saw
hept-

39. Symbol for Total Heat absorbed or released
q
hydro-ic acid
4.184
1 atm

40. =vM2/M1
r1/r2
X of a = moles a/total moles
chlorite
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

41. This MUST be determined experimentally
rate law
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
8.31J/Kmol
sublimation

42. If anion ends in -ide - acid name ends in
wavelength
hydro-ic acid
-ous acid
Reducing Agent

43. Variable for spin of electron (+.5 or -.5)
s (fourth quantum number)
melting point
Osmotic Pressure
Electron Spin Quantum Number

44. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
sublimation
Weight
Manometer
s

45. Work = ?
Molal FP Depression Constant
Negative work value; work done by system
Speed of light
-(P)(Change in V)

46. Newton's Second Law
electrolyte
heat of vaporization
Linear
Force = mass x acceleration

47. (organics) triple-bonded compound
alkyne
meth-
Entropy (S)
nitrate

48. Color of Cs (flame test)
acetate
salt bridge
critical point
blue

49. 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
period
Solubility Product (Ksp)
Finding Empirical Formulas
melting point

50. Spontaneous emission of radiation
Molal BP Elevation Constant
alkyne
Radioactivity
Acids