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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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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. How to Find an Empirical Formula Given Grams
increasing
Integrated First-Order Rate Law
Root Mean Square Velocity
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

2. Cl¹?
Faraday
Sigma Bond
bromate
chloride

3. AX4
tetrahedral
Force = mass x acceleration
meth-
are

4. A monoatomic cation takes name from...
AH
alkene
Equilibrium constant
Its element

5. Speed of light - C
f
triple point
3.0x108m/s
q/moles

6. Organic w/ -OH group
surroundings
alcohol
Counterions
Molecular Compounds

7. PO4³?
Adding
phosphate
0
Molality

8. 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

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9. H + donor
Bronsted-Lowry Acid
Arrhenius equation
Speed of light
Aufbau Principle

10. The total energy of the universe is constant - all systems tend towards minimum energy
X of a = moles a/total moles
carbohydrates
1st law of thermodynamics
l (second quantum number)

11. Speed per molecule of gas
pi=(nRT)/v
no precipitate forms
wavelength
v3kT/m

12. Elements which have unpaired electrons and highly affected by magnetic fields
Solvent
third
paramagnetic
viscosity

13. NO2¹?
ionic
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
nitrite
Hund's Rule

14. Kinetic Energy per mol
3/2RT
End Point
-one
Bronsted-Lowry acid

15. 96 -485 C/mol e-
cyanide
Multiplying
Faraday
1 atm

16. Substances that form H+ when dissolved in water; proton donors
London dispersion forces
Acids
trigonal bipyramidal
Colligative properties

17. q H2O = ?
strong acids
msAT
STP
exothermic

18. If anion ends in -ate - acid name ends in...
alkane
-ic acid
Cation
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

19. r=k[A]^2
Second-Order Rate Law
alkane
Arrhenius acid
titrant buret

20. Delta H (AH) = ?
q/moles
Le Chatelier's Principle
Balmer Series
hex-

21. Average speed of gas
v3RT/M(in kg)
Molality
Atomic Mass Unit
London dispersion forces

22. Kinetic Energy per molecule
1/2mv²
?Hvap
Closed System
Entropy (S)

23. AX6
Molar Mass of Element/ Total Molar Mass %
Beta Particles-
-2 - with peroxide -1
octahedral

24. Carboxylic acid ending
square pyramidal
-oic acid
solid CO2
?Tf= kf x molality

25. 1 sigma bond
Molal BP Elevation Constant
non-
single bond
System

26. AX5
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Tetrahedral
sublimation
trigonal bipyramidal

27. 90° - d^2sp^3
Octahedral
Kinetic Molecular Theory - for ideal gases
E
base and hydrogen gas

28. Point where acid completely neutralizes base
Multiplying
equivalence point
heat capacity
electrolyte

29. When gas expands ...
Negative work value; work done by system
Polar Covalent
Equilibrium Expression
Hydrogen bonding

30. The chemical formed when a base accepts a proton
Hydrogen bonding
conjugate acid
Balmer Series
Ligand

31. Dalton's Law of Partial Pressures (to find partial pressure formula)
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
P of a =(X of a)(total pressure)
but-
entropy

32. F¹?
precipitate
Coordination Compound
-one
flouride

33. E=mc^2
purple --> pink
meth-
-oate
Theory of Relativity

34. Color of Sr (flame test)
red
heat capacity
Strong acid weak base rxn
A Roman numeral

35. AP doesn't deal with ...-order reaction - don't pick it!
Principal Quantum Number
third
Magnetic Quantum Number (ml)
Chemical Kinetics

36. How to Find an Empirical Formula Given Percentages
high pressure - low temperature
Heisenberg Uncertainty Principle
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
heat of vaporization

37. Heat required to raise the system 1°C
wavelength
Colligative properties
trigonal pyramidal
heat capacity

38. Solid to liquid
no precipitate forms
melting
Atmospheric Pressure
like

39. Energy needed to break a bond
Molecule
bond energy
carbonate
excess reactant

40. Boiling point elevation formula
period
?Tb= kb x molality
Effusion
Solute

41. Increase Volume
Alpha Particles-
Endothermic
Dalton's Law of Partial Pressures
Increase Temperature

42. All cations are soluble with bromide - chloride and iodide EXCEPT
?Tf= kf x molality
First-Order Half Life
Entropy (S)
Ag+ - Pb2+ - Hg2+

43. Absorbs/takes in heat (positive value)
Endothermic
Theory of Relativity
nu
supercritical fluid

44. In a given atom no two electrons can have the same set of four quantum numbers
iodide
Trigonal Bipyramidal
Pauli Exclusion Principle
0

45. Reactant which doesn't get used up completely in a chemical reaction
Hess's Law
Acid + Base --> Salt + Water
spontaneous
excess reactant

46. Thickness
specific heat
viscosity
-(q of H2O + q of cal)
Chemical Bonds

47. Loss of electrons - increase in oxidation #
STP
red
oxidation
Dipole Moment

48. Coffee Cup Calorimeter
Constant Pressure
CAT
Formal Charge
reduction

49. Atomic #
square planar
# protons (atom is defined by this)
yellow
Manometer

50. Atoms with the same number of protons but a different number of neutrons
activation energy
Pressure
Isotopes
s orbitals