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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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1. AX4E
equivalence point
are
see-saw
1st law of thermodynamics

2. Kinetic Energy per mol
3/2RT
Coordination Compound
Acids
Bond Energy

3. Happens at lines in phase change charts
equilibrium
prop-
hydrocarbons
violet

4. Delta H (AH) = ?
q/moles
Nodes
Pi Bond
Linear

5. Elements on staircase on periodic table
critical point
Average KE = 1/2(mass)(average speed of all particles)
Buffer
Metalliods

6. Electron (symbol)
spontaneous
conjugate base
Bonding Pairs
e-

7. Organic w/ -OH group
purple
Principal Quantum Number
alcohol
exothermic

8. Type of system in which the energy and mass may leave or enter
Open System
nitrate
-ic acid
a precipitate forms

9. (A) - C/s
Temperature
blue
trigonal bipyramidal
Ampere

10. When gas expands ...
Monoprotic
Solubility Product (Ksp)
increasing
Negative work value; work done by system

11. #NAME?
see-saw
Pressure of H2O must be Subtracted
Strong acid weak base rxn
E

12. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium

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13. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
actual yield/theoretical yield x 100%
Covalently w/in themselves - Ionicly bonded w/ each other

14. Amine prefix
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
condensation
Amino-
T-shape

15. All cations are soluble with sulfate EXCEPT
equivalence point
q
phosphate
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+

16. Cation first - anion second
Integrated Second-Order Rate Law
Balmer Series
lambda
Naming Binary Ionic Compounds

17. AX5
n (first quantum number)
trigonal bipyramidal
high pressure - low temperature
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound

18. 760 mmHg - 760 torr
sulfate
work
1 atm
alkane

19. ClO2¹?
phosphate - sulfide - carbonate - sulfate
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
specific heat
chlorite

20. Temperature-pressure point after which gas can no longer form liquid
critical point
charge
0
equivalence point

21. AX3
trigonal planar
AH
N=N.(0.5)^time/time half-life
Isotopes

22. R=
moles solute/kg solvent
8.31J/Kmol
T-shape
Molarity

23. pH=
high pressure - low temperature
log[H+]
Amino-
Negative work value; work done by system

24. Point at which the titrated solution changes color
green/yellow
Dipole Moment
end point
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

25. Non-Ideal Gas Conditions
amine
E
supercritical fluid
high pressure - low temperature

26. Kinetic Energy per molecule
1/2mv²
yellow --> green
Molecule
P1= X1P1°

27. A weak acid that changes color at or near the equivalence point
s orbitals
indicator
yellow
exothermic

28. AH of formation for a substance in its stablest form (how it is found in nature)
reduction
0
Molecular
alcohol

29. l=2
-2 - with peroxide -1
Cell Potential (Ecell)
Bases
d

30. These orbitals are diagonal
AE = q + w
AE= AH - RTAn
Force = mass x acceleration
d orbitals

31. 90° - d^2sp^3
Kinetic Molecular Theory - for ideal gases
chromate
Octahedral
Bases

32. Energy needed to vaporize a mole of a liquid
Buffered Solution
?Hvap
analyte
Bond Energy

33. AX4
period
triple point
3rd law of thermodynamics
tetrahedral

34. Thickness
Strong acid weak base rxn
Law of Multiple Proportions
viscosity
Open System

35. Ester suffix
Gamma Ray-
-one
Scientific Method
-oate

36. Heat required to raise the system 1°C
acetate
heat capacity
Closed System
Calorimetry

37. Unit of electrical potential; J/C
Sigma Bond
Hybridization
-(q of H2O + q of cal)
Volt

38. Where oxidation occurs
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
excess reactant
Anode
phosphate

39. (organics) ten carbons
single bond
spontaneity
dec-
Trigonal Planar

40. A device in which chemical energy is changed to electrical energy
freezing
Electron Spin Quantum Number
Galvanic Cell
3/2RT

41. Volume of gas @STP
Buffer
-(q of H2O + q of cal)
sulfide
22.4L

42. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
insoluble
bond energy
Law of Conservation of Mass
increasing

43. The total entropy is always increasing - all systems tend towards maximum entropy
no precipitate forms
catalyst
equilibrium
2nd law of thermodynamics

44. Higher in energy than the atomic orbitals of which it is composed
mol
Antibonding Molecular Orbital
1atm=?Pa
1 atm

45. Mols A/ total mols - XA
Bronsted-Lowry Base
AE= AH - RTAn
Quantum Model
mol Fraction

46. Coffee Cup Calorimeter
Constant Pressure
Polar Covalent
high pressure - low temperature
P of a =(X of a)(total pressure)

47. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
insoluble
trigonal planar
voltaic cells
Positive work value; work done on system

48. J/°Cmol or J/Kmol
Resonance
Coordination Compound
Radioactivity
Molar Heat Capacity

49. Loss of electrons - increase in oxidation #
Heat
oxidation
Second-Order Half Life
exothermic

50. Phase change from gas to solid
0
purple
deposition
Cell Potential (Ecell)