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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. Speed of light - C
3.0x108m/s
blue-green
Atmospheric Pressure
1atm=?Pa

2. Oxidation # of Hydrogen
Solution
+1 - except if bonded to Alkali Metal -1
d
-1

3. A monoatomic anion is named by taking...
insoluble
Its root and adding -ide
Equilibrium Expression
Enthalpy of Solution

4. Horizontals on the periodic table
period
freezing
0
Law of Multiple Proportions

5. When n=3 ->2 - color=
Barometer
are not
Heisenberg Uncertainty Principle
red

6. A device in which chemical energy is changed to electrical energy
Law of Definite Proportion
endothermic
actual yield/theoretical yield x 100%
Galvanic Cell

7. [A]=-kt + [A]0
conjugate base
1 atm
Specific Heat (s)
Integrated Zero-Order Rate Law

8. Puts OH? into solution
Arrhenius base
M1V1=M2V2
Hund's Rule
specific heat

9. Chemical composition of dry ice
solid CO2
Enthalpy of Solution
Dipole Moment
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

10. AX4E
specific heat
?Tf= kf x molality
triple point
see-saw

11. The driving force for a spontaneous is an increase in entropy of the universe
Entropy (S)
Chemical Kinetics
Amino-
-2 - with peroxide -1

12. High-speed electrons
acetate
mol
-oic acid
Beta Particles-

13. Positive enthalpy - heat flows into system
endless
Linear
endothermic
Dipole-dipole forces

14. Universal IMF for nonpolar molecules
Antibonding Molecular Orbital
London dispersion forces
Arrhenius base
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

15. As protons are added to the nucleus - electrons are similarly added
red
nitrite
Arrhenius equation
Aufbau Principle

16. Instrument used to measure the pressure of atmospheric gas
iodide
Barometer
Root Mean Square Velocity
Galvanic Cell

17. Color of Sr (flame test)
red
Pressure of H2O must be Subtracted
octahedral
Antibonding Molecular Orbital

18. How to Find an Empirical Formula Given Grams
Net Ionic Equation
Temperature
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Coordination Compound

19. Higher in energy than the atomic orbitals of which it is composed
condensation
viscosity
Molal FP Depression Constant
Antibonding Molecular Orbital

20. A solid or gas that can be formed when 2 or more aqueous reactants come together
precipitate
Faraday
Metalliods
-ol

21. Boltzmann constant - used in calculating speed of gas per molecule
entropy
Speed of light
Second-Order Rate Law
1.38x10?²³J/K

22. All _________ compounds are electrolytes
insoluble
AE= AH - RTAn
equilibrium
Ionic

23. r=k
Zero-Order Rate Law
v3RT/M(in kg)
critical point
reduction agent

24. Coffee Cup Calorimeter
Constant Pressure
Surroundings
Molal BP Elevation Constant
Reaction Quotient (Q)

25. The chemical formed when an acid donates a proton
bromate
octahedral
conjugate base
Ideal Gas Law

26. The transfer of energy between two objects due to temperature difference
Heat
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Acid + Base --> Salt + Water
A Roman numeral

27. Donates a single H+ Ion (... other prefixes also)
Monoprotic
Ampere
?Tf= kf x molality
Dalton's Law

28. Raoult's Law - relations between vapor pressure and concentrations
Radioactivity
s orbitals
Pauli Exclusion Principle
P1= X1P1°

29. ClO3²?
Enthalpy of Solution
square planar
carbohydrates
chlorate

30. An equilibrium expression
endless
Solubility Product (Ksp)
Work
1 atm = 760 mmHg = 101.3 kPa

31. Color of K (flame test)
carbonate
purple
Resonance
heat capacity

32. Ending for alcohols
a precipitate forms
Gamma Ray-
Constant Volume
-ol

33. Oxidation # of Halogens
alcohol
A Roman numeral
-1
1 atm

34. The line running between the atoms
blue
purple
Sigma Bond
effects of IMF

35. Mass percent
cyanide
Reaction Quotient (Q)
trigonal bipyramidal
g solute/g solvent x 100

36. Variable for energy of e- - goes from 1 -2 -3 on up
conjugate base
n (first quantum number)
oct-
Counterions

37. 101 -325 Pa
Molecular Orbitals (MOs)
hept-
1atm=?Pa
AE= AH - RTAn

38. F¹?
d orbitals
sublimation
flouride
Aufbau Principle

39. Delta H (AH) = ?
End Point
allotrope
melting point
q/moles

40. Anions or cations as needed to produce a compound with non net charge
Counterions
methods of increasing rate
high pressure - low temperature
Scientific Method

41. Cl¹?
Sigma Bond
# protons (atom is defined by this)
Solubility Product (Ksp)
chloride

42. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Chemical Kinetics
deposition
prop-
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

43. The reactant in the reduction reaction that forces the oxidation reaction to occur
Oxidizing Agent
deposition
purple --> pink
Principal Quantum Number

44. Aldehyde suffix
-al
strong acids
Net Ionic Equation
insoluble

45. Determined by the formula h/m(in kg)v - (v=velocity)
STP
deposition
Monoprotic
wavelength

46. Heat capacity formula
C=(mass)(specific heat)
adhesion
Integrated Zero-Order Rate Law
rate gas A/rate gas B = square root (mm A/ mm B)

47. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Polar Covalent
Reducing Agent
Anion
tetrahedral

48. Amine prefix
Bond Energy
catalyst
Amino-
+1 - except if bonded to Alkali Metal -1

49. Substances w/ critical temperatures below 25°C
alcohol
trigonal bipyramidal
Increase Temperature
permanent gases

50. (organics) one carbon
meth-
London dispersion forces
nu
l (second quantum number)