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Test your basic knowledge |
AP Chemistry
Start Test
Study First
Subjects
:
science
,
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. Color of Cs (flame test)
3.0x108m/s
blue
96500
heat of vaporization
2. Boiling point elevation formula
% yield
1st law of thermodynamics
Transition metals
?Tb= kb x molality
3. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
adiabatic
Acid + Base --> Salt + Water
nu
Equivalence Point
4. Negative enthalpy - heat flows into surroundings
Its root and adding -ide
Calorimeter
Osmotic Pressure
exothermic
5. STP
alkyne
Dipole-dipole forces
oxidation
0 degrees C - 1 atm
6. ClO4¹?
adiabatic
Atmospheric Pressure
sublimation
perchlorate
7. Moles of solute/volume of soln(L)
d
Molarity
Cation
% yield
8. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
iodide
a precipitate forms
Cg=kPg
yellow --> green
9. Oxidation # of Polyatomic Ions
Dipole-dipole forces
charge
system
Root Mean Square Velocity
10. Oxoacid solution (such as HSO4-) forms...
Kinetic Molecular Theory - for ideal gases
Beta Particles-
System
oxide gas and water
11. Non-Ideal Gas Conditions
yellow --> green
Enthalpy of Solution
high pressure - low temperature
Solvent
12. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
chloride
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Electron Spin Quantum Number
13. R in instances that pertain to energy
Overall Reaction Order
8.31J/Kmol
Pressure of H2O must be Subtracted
8.314 J/K mol
14. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
Integrated Zero-Order Rate Law
Bronsted-Lowry Acid
Adding
End Point
15. Liquid to solid
Trigonal Bipyramidal
Ionic
phosphate
freezing
16. Mol/L - concentration of a solution
Molarity
Quantum Mechanical Model
r1/r2
sublimation
17. Resistance to flow
viscosity
PV=nRT
boiling point
heat capacity
18. How to Find a Weighted Average
blue-green
Polar Covalent
high pressure - low temperature
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
19. O²?
Molar Heat Capacity
oxide
allotrope
H
20. The minimum energy that molecules must possess for collisions to be effective - Ea
single bond
activated complex (transition state)
activation energy
E
21. PO4³?
phosphate
bent
indicator
Bonding Pairs
22. Elements which have unpaired electrons and highly affected by magnetic fields
paramagnetic
entropy
Electronegativity
H
23. Change that occurs at constant temperature
ammonium
strong acids
isothermal
Ionic Compounds
24. 6.022x10^23
mol
Heat
diamagnetic
s orbitals
25. The chemical formed when an acid donates a proton
Work
Solution
Dipole Moment
conjugate base
26. Forward rxn occurs when
% yield
complex ions
allotrope
Q<K
27. I¹?
zero
rate
iodide
Allotrope
28. Solution used in titration
Integrated Rate Law
boiling point
a precipitate forms
titrant buret
29. An equilibrium expression
Solubility Product (Ksp)
E
Volume Metric Flask & Pipet
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
30. High-speed electrons
Beta Particles-
Hund's Rule
p orbitals
Gamma Ray-
31. Oxidation # of Compounds
Bond Energy
Heat Capacity (C)
Molar Heat Capacity
0
32. J/°Cmol or J/Kmol
Molar Heat Capacity
Resonance
Principal Quantum Number
cathode
33. The amount of energy/heat required to raise some substance 1 degree C
hydro-ic acid
s (fourth quantum number)
s
Heat Capacity (C)
34. Atomic #
# protons (atom is defined by this)
Scientific Method
carbonate
equilibrium
35. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
Linear
t-shape
Positive work value; work done on system
36. What is defined by you taken from the whole universe
acetate
System
Bases
Its root and adding -ide
37. AX5E
melting
square pyramidal
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Joule
38. Describe various properties of one orbital
Quantum Numbers
AE= AH - RTAn
LeChatelier's Principle
# protons + # neutrons
39. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Kinetic Molecular Theory - for ideal gases
Finding Empirical Formulas
Formal Charge
increasing
40. Diatomic Molecules
spontaneous
Alkali metals
AE = q + w
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
41. A measure of randomness or disorder
Closed System
Acid Dissociation Constant
entropy
Joule
42. Energy required to break a bond
Bond Energy
0
Galvanic Cell
Arrhenius base
43. ln[A] vs. time is a ...-order reaction
Arrhenius acid
dec-
Faraday
first
44. Pairs of electrons localized on an atom
linear
M = square root (3RT/mm)
Lone Pair
Molality
45. # bonding e- - # antibonding e-/2
prop-
mol
System
Bond Order
46. Substance in which something is dissolved in a solution (higher [ ])
bent
Arrhenius base
Solvent
1st law of thermodynamics
47. Raising heat - adding catalyst - heighten concentration - bigger surface area
see-saw
moles of solute/ L of solution
methods of increasing rate
endless
48. AX4E
alkane
rate law
electron affinity
see-saw
49. Measure of the change in enthalpy
P1V1/N1T1=P2V2/N2T2
deposition
Delta H or Enthalpy Change
nitrite
50. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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