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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. Boiling point - melting point - viscosity - vapor pressure - surface tension
allotrope
Atomic Mass Unit
chlorite
effects of IMF

2. Change in Energy = ? (in terms of constant pressure; for gasses)
Van't Hoff factor
Entropy (S)
AE= AH - RTAn
d orbitals

3. q cal = ?
CAT
are not
zero
Trigonal Bipyramidal

4. ClO4¹?
square pyramidal
Delta H or Enthalpy Change
Oxidation is Loss Reduction is Gain
perchlorate

5. When ____ significant digits - round answer to least decimal place
Zero-Order Rate Law
H
0
Adding

6. Speed per molecule of gas
eth-
3.0x108m/s
v3kT/m
Resonance

7. Arrhenius equation
k=Ae^(-Ea/RT)
Law of Definite Proportion
critical point
Alkaline earth metals

8. (organics) seven carbons
square planar
Scientific Method
hept-
solid CO2

9. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
Overall Reaction Order
conjugate acid
freezing

10. Volume of gas @STP
End Point
Density
mol
22.4L

11. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
alkene
Atmospheric Pressure
Dipole-dipole forces
# protons + # neutrons

12. High-speed electrons
0.0821 atm L/mol K
(moles of products that are gasses) - (moles of reactants that are gasses)
Beta Particles-
octahedral

13. Reverse rxn occurs when
system
Q>K
Overall Reaction Order
Endothermic

14. 1/[A] vs. time is a ...-order reaction
5% rule
Theoretical yield
Hybridization
second

15. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
E
hydrolysis
condensation
Surroundings

16. Mol/kg of solvent - used in calculating colligative properties
trigonal bipyramidal
Metalliods
Aufbau Principle
Molality

17. Ecell= E°cell -RT/nF x lnQ
m (third quantum number)
group
cyanide
Nernst Equation

18. 1/([A]0*k)
Cation
Second-Order Half Life
Bonding Pairs
p

19. 0°C and 1 atm
Amino-
Molecular Orbitals (MOs)
ionic
STP

20. Isotope
nitrite
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
different # of neutrons

21. Kinetic Energy per mol
3/2RT
London dispersion forces
conjugate acid
system

22. Cr2O7²?
Pauli Exclusion Principle
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
dichromate
square planar

23. Formula used when diluting stock solution (to find amount of water or stock needed)
Molality
M1V1=M2V2
entropy (S)
Molal BP Elevation Constant

24. If anion ends in -ite - acid name ends in...
-ous acid
Temperature
Ligand
Coordination Compound

25. 2+ charge
Counterions
# protons + # neutrons
Alpha Particles-
moles of solute/ L of solution

26. AX2E - AX2E2
Closed System
bent
a precipitate forms
Buffer

27. Within a sublevel - place one e? per orbital before pairing them

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28. Substances w/ critical temperatures below 25°C
London Dispersion Forces
0.0821 atm L/mol K
permanent gases
State Functions

29. AX4E
Force = mass x acceleration
see-saw
Net Ionic Equation
endless

30. When _____ significant digits - round answer to least significant digit
Oxidation is Loss Reduction is Gain
blue-green
Multiplying
trigonal bipyramidal

31. I=moles of particles/moles of solute dissolved

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32. The heat changed in a chemical reaction.
q/moles
Thermochemistry
not spontaneous
Atomic Mass Unit

33. Group 1 metals
s (fourth quantum number)
Alkali metals
nitrite
endothermic

34. 90°&120° - dsp^3
Trigonal Bipyramidal
precipitate
are not
London dispersion forces

35. PO4³?
Bronsted-Lowry base
phosphate
msAT
Beta Particles-

36. Variable for type of orbital
bent
boiling point
equilibrium
l (second quantum number)

37. The rest of the universe (in thermodynamics)
Zero-Order Rate Law
surroundings
chlorate
insoluble

38. Spontaneous emission of radiation
nu
standard solution
Dipole-dipole forces
Radioactivity

39. Ionizes to produce OH- Ions
ionic
Arrhenius Base
Atomic Mass Unit
Increase Temperature

40. Where there are no electrons
different # of neutrons
Nodes
-al
oxidizing agent

41. A monoatomic anion is named by taking...
Its root and adding -ide
M1V1=M2V2
6.63x10?³4Js
E

42. Loss of electrons - increase in oxidation #
oxidation
Zero-Order Half Life
n0
Formal Charge

43. Like dissolves...
+1 - except if bonded to Alkali Metal -1
Faraday
like
-oic acid

44. (organics) three carbons
trigonal bipyramidal
octahedral
prop-
Heisenberg Uncertainty Principle

45. A molecule having a center of positive charge and a center of negative charge
not spontaneous
London dispersion forces
Dipole Moment
Colligative properties

46. Type of system in which the energy may escape - but the mass is conserved
phosphate
mol
Closed System
bent

47. Mole Fraction
X of a = moles a/total moles
Zero-Order Rate Law
London dispersion forces
like

48. Donates a single H+ Ion (... other prefixes also)
Monoprotic
trigonal planar
Increase Temperature
Isotopes

49. % yield
actual yield/theoretical yield x 100%
Dalton's Law of Partial Pressures
square planar
Acid + Base --> Salt + Water

50. Stronger IMF= lower... weaker IMF= higher...
-ous acid
Arrhenius equation
Molar Heat Capacity
vapor pressure