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. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
Endothermic
Le Chatelier's Principle
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
hydrolysis

2. Boiling point - melting point - viscosity - vapor pressure - surface tension
effects of IMF
Endothermic
Octahedral
Temperature

3. Moles of solute/volume of soln(L)
hept-
Molarity
see-saw
heat of vaporization

4. Amount of heat needed to change a system by 1°C
Cg=kPg
equilibrium
heat capacity
boiling point

5. J/°Cg or J/Kg
chromate
Specific Heat Capacity
oxidizing agent
nu

6. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
rate
square pyramidal
Volt
Ionic Compounds

7. Entropy in the universe is always...
k=Ae^(-Ea/RT)
increasing
Amount of atoms present
complex ions

8. Mol/L - concentration of a solution
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
strong acids
Molarity
not spontaneous

9. q cal = ?
heat of vaporization
non-
Average KE = 1/2(mass)(average speed of all particles)
CAT

10. #NAME?
Buffer
E
group
not spontaneous

11. Mol of solute/kg of solvent
-one
Molality
t-shape
base

12. When n=6 ->2 - color=
p orbitals
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
Q>K
violet

13. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
End Point
hydrolysis
nitrite
Le Chatelier's Principle

14. Organic reaction in which two functional groups come together - resulting in the release of water
London dispersion forces
condensation
Lone Pair
1.86°C

15. When n=4 ->2 - color=
indicator
rate
period
blue-green

16. CrO4²?
charge
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
chromate
Integrated Zero-Order Rate Law

17. Diatomic Molecules
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
2nd law of thermodynamics
96500

18. Ability of an atom in a molecule to attract shared electrons to itself
Electronegativity
-ous acid
g solute/g solvent x 100
London dispersion forces

19. ... compounds are most conductive
PV=nRT
Hess's Law
ionic
chlorite

20. Theoretical yield-experimental yield/theoretical yieldx100
% error
different # of neutrons
Acid Dissociation Constant
London dispersion forces

21. Universal IMF for nonpolar molecules
London dispersion forces
Hydrogen bonding
pi=(nRT)/v
-ic acid

22. Idea Gas Law (actual rules)
Nodes
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
Anode
oxidizing agent

23. Horizontals on the periodic table
nitrate
period
blue-green
p

24. Substance in which something is dissolved in a solution (higher [ ])
5% rule
Multiplying
alkane
Solvent

25. Occupies the space above and below a sigma bond
# protons (atom is defined by this)
reduction
Enthalpy of Solution
Pi Bond

26. Metal oxide + H20 ->
square planar
s orbitals
Acid + Base --> Salt + Water
base

27. What is defined by you taken from the whole universe
System
Ionic
+1 - except if bonded to Alkali Metal -1
r1/r2

28. Energy needed to vaporize a mole of a liquid
Molecular
?Hvap
octahedral
Calorimeter

29. Only contains ions that change in reaction
triple point
0 degrees C - 1 atm
Hydrogen bonding
Net Ionic Equation

30. These orbitals are spherical
condensation
Bronsted-Lowry Base
Equilibrium Expression
s orbitals

31. ClO4¹?
v3kT/m
perchlorate
group
square planar

32. Color of Sr (flame test)
increasing
M1V1=M2V2
Decrease Volume and Increase Temperature
red

33. Substance that - when dissolved - is conductive
electrolyte
0.0826Latm/Kmol
condensation
carbohydrates

34. AX3
Volume Metric Flask & Pipet
-one
Beta Particles-
trigonal planar

35. HF+ OH??H2O
weak acid strong base rxn
see-saw
0
rate law

36. Positive enthalpy - heat flows into system
?Tf= kf x molality
1st law of thermodynamics
Isolated System
endothermic

37. For significant digits - leading zeros ____ significant
conjugate acid
zero
are not
Calorimeter

38. .69/k
1st law of thermodynamics
First-Order Half Life
p+
P1= X1P1°

39. PO4³?
trigonal pyramidal
phosphate
base and hydrogen gas
complex ions

40. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
complex ions
heat of vaporization
AE= AH - RTAn

41. [A] vs. time is a ...-order reaction
v3RT/M(in kg)
zero
paramagnetic
1 atm

42. Cation first - anion second
-ol
Quantum Numbers
Naming Binary Ionic Compounds
spontaneity

43. (A) - C/s
viscosity
Ampere
oxide gas and water
single bond

44. Ionizes to produce H+ ions
red
end point
dec-
Arrhenius Acid

45. neutron (symbol)
heat capacity
n0
Reducing Agent
C=(mass)(specific heat)

46. Amount of gravitational force exerted on an object
Decrease Volume and Increase Temperature
permanent gases
-ous acid
Weight

47. Half cell in which reduction occurs
alkene
Electron Spin Quantum Number
cathode
CAT

48. l=3
Speed of light
Surroundings
f
Entropy (S)

49. Pure metal or metal hydride + H20 ->
Joule
base and hydrogen gas
Matter
-(q of H2O + q of cal)

50. Involves quantum numbers
Quantum Mechanical Model
M1V1=M2V2
adiabatic
work