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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. Like dissolves...
Law of Conservation of Mass
s
like
iodide

2. Elements on staircase on periodic table
Metalliods
solid CO2
second
Quantum Model

3. Oxidation # of Hydrogen
Multiplying
analyte
+1 - except if bonded to Alkali Metal -1
Theoretical yield

4. 6.022x10^23
mol
reduction agent
acid
Formal Charge

5. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Boltzmann distribution
Sigma Bond
blue
Allotrope

6. r=k
Zero-Order Rate Law
acid
p orbitals
condensation

7. IMF that exists in polar molecules
System
Temperature
geometric isomers
Dipole-dipole forces

8. Where oxidation occurs
strong acids
blue
catalyst
Anode

9. A molecule having a center of positive charge and a center of negative charge
Dipole Moment
Thermochemistry
Trigonal Planar
carbonate

10. Change in Energy = ? (in terms of constant pressure; for gasses)
tetrahedral
Exothermic
Bronsted-Lowry Base
AE= AH - RTAn

11. How to Balance a Redox Equation
Cell Potential (Ecell)
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
Constant Volume
g solute/g solvent x 100

12. Proton (symbol)
Constant Volume
excess reactant
Magnetic Quantum Number (ml)
p+

13. (organics) triple-bonded compound
Surroundings
standard solution
octahedral
alkyne

14. Substance in which something is dissolved in a solution (higher [ ])
Solvent
entropy
allotrope
cathode

15. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
salt bridge
0
blue

16. Has values 1 -2 -3 -...; tells energy levels
reduction
q/moles
Bronsted-Lowry acid
Principal Quantum Number

17. Increase Volume
Increase Temperature
dec-
1/2mv²
Thermochemistry

18. Absorbs/takes in heat (positive value)
Nernst Equation
trigonal bipyramidal
Endothermic
nitrate

19. Negative enthalpy - heat flows into surroundings
exothermic
Adding
but-
group

20. AX6
condensation
Scientific Method
supercritical fluid
octahedral

21. Work = ?
STP
Molecular
-(P)(Change in V)
0.512°C

22. Matter can't be created nor destroyed
Law of Conservation of Mass
titrant buret
Dalton's Law
mol Fraction

23. Type of system in which the energy may escape - but the mass is conserved
vapor pressure
Closed System
Open System
are not

24. When n=6 ->2 - color=
violet
3rd law of thermodynamics
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Net Ionic Equation

25. Color of K (flame test)
5% rule
Quantum Numbers
purple
hept-

26. Atoms with the same number of protons but a different number of neutrons
blue-violet
pent-
LeChatelier's Principle
Isotopes

27. 90° - d^2sp^3
-(q of H2O + q of cal)
phosphate - sulfide - carbonate - sulfate
supercritical fluid
Octahedral

28. These orbitals are spherical
s orbitals
H
Molar Heat Capacity
Hess's Law

29. Point at which solid?liquid occurs
melting point
hydrocarbons
London dispersion forces
vaporization

30. If Q>Ksp
single bond
s
a precipitate forms
Solubility Product (Ksp)

31. Molality =
moles solute/kg solvent
Aufbau Principle
Heisenberg Uncertainty Principle
first

32. Osmotic pressure=MRT
-oate
first
meth-
Osmotic Pressure

33. Point at which vapor pressure=air pressure above
boiling point
C + 273
yellow --> green
triple bond

34. These orbitals are diagonal
d orbitals
Its root and adding -ide
catalyst
Trigonal Bipyramidal

35. Loss of electrons - increase in oxidation #
strong bases
oxidation
Average KE = 1/2(mass)(average speed of all particles)
Amino-

36. The energy required to raise 1 g of substance 1 degree C
ether
Specific Heat (s)
equilibrium
soluble

37. 120° - sp^2
Trigonal Planar
permanent gases
Quantum Mechanical Model
sulfate

38. The amount of energy/heat required to raise some substance 1 degree C
Heat Capacity (C)
6.63x10?³4Js
first
Isotopes

39. Wavelength symbol
lambda
X of a = moles a/total moles
Pressure of H2O must be Subtracted
force x distance = work done

40. AX4E2
reduction agent
Electronegativity
square planar
LE Model

41. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Molecule
Acid + Base --> Salt + Water
Joule
heat capacity

42. Spectrum of light when an electron drops to energy level n=2
Matter
Zero-Order Rate Law
phosphate
Balmer Series

43. Osmotic pressure formula
Delta H or Enthalpy Change
activation energy
Linear
pi=(nRT)/v

44. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
voltaic cells
Specific Heat (s)
excess reactant
sulfite

45. Organic w/ -NH2
Molecular Compounds
alkene
g solute/g solvent x 100
amine

46. kf of water
Second-Order Rate Law
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
sulfite
1.86°C

47. A monoatomic cation takes name from...
boiling point
spontaneous
effects of IMF
Its element

48. Proton acceptors - must have an unshared pair of e?s
Bronsted-Lowry base
are
adhesion
Volume Metric Flask & Pipet

49. Planck's constant - used to calculate energy w/frequency
6.63x10?³4Js
Isolated System
Resonance
% yield

50. Thickness
phosphate - sulfide - carbonate - sulfate
cyanide
carbonate
viscosity