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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. Volume of gas @STP
Coordination Compound
square pyramidal
22.4L
Positive work value; work done on system
2. When gas expands ...
Negative work value; work done by system
CAT
% error
Van't Hoff factor
3. Substances w/ critical temperatures below 25°C
Increase Temperature
permanent gases
Resonance
Speed of light
4. Electron (symbol)
Aufbau Principle
Principal Quantum Number
e-
voltaic cells
5. R in ideal gas law
0.0821 atm L/mol K
conjugate base
purple
Formal Charge
6. 180° - sp
Linear
Multiplying
d
mol
7. H?+NH3?NH4
Force = mass x acceleration
precipitate
Strong acid weak base rxn
-ic acid
8. AX4
bent
allotrope
conjugate acid
tetrahedral
9. MnO4¹?
permanganate
Temperature
Reducing Agent
p+
10. The driving force for a spontaneous is an increase in entropy of the universe
Endothermic
log[H+]
melting
Entropy (S)
11. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Volt
rate
1st law of thermodynamics
?Hvap
12. Reverse rxn occurs when
equivalence point
Q>K
lambda
Effusion
13. AX5E
Integrated Zero-Order Rate Law
1atm=?mmHg/Torr
square pyramidal
q
14. U(rms)=(3RT/M)^1/2
Hybridization
Root Mean Square Velocity
Le Chatelier's Principle
Anion
15. Osmotic pressure=MRT
Osmotic Pressure
Bronsted-Lowry Acid
trigonal planar
violet
16. Point at which solid?liquid occurs
Thermochemistry
Reaction Quotient (Q)
Amount of atoms present
melting point
17. I¹?
Hund's Rule
Work
Faraday
iodide
18. Planck's constant - used to calculate energy w/frequency
trigonal pyramidal
Volume Metric Flask & Pipet
6.63x10?³4Js
g solute/g solvent x 100
19. If anion ends in -ate - acid name ends in...
methods of increasing rate
Integrated Zero-Order Rate Law
Transition metals
-ic acid
20. Amount of gravitational force exerted on an object
activation energy
Weight
Van't Hoff factor
Force = mass x acceleration
21. Kinetic Energy per mol
Law of Conservation of Mass
-ous acid
Formal Charge
3/2RT
22. Amount of product produced when limiting reactant is used up
Cathode
Coordination Compound
Theoretical yield
Entropy (S)
23. All _________ compounds are electrolytes
octahedral
salt bridge
Equilibrium constant
Ionic
24. Resistance to flow
P of a =(X of a)(total pressure)
Pressure of H2O must be Subtracted
Enthalpy of Solution
viscosity
25. Change without heat transfer between the system and its surroundings
Radioactivity
f
adiabatic
Second-Order Rate Law
26. Coffee Cup Calorimeter
prop-
violet
22.4L
Constant Pressure
27. Energy involved in gaining an electron to become a negative ion
Bases
P of a =(X of a)(total pressure)
electron affinity
Integrated Zero-Order Rate Law
28. AX2E - AX2E2
1.86°C
trigonal planar
vapor pressure
bent
29. Aldehyde suffix
Strong acid weak base rxn
no precipitate forms
-al
excess reactant
30. frequency symbol
nu
base and hydrogen gas
yellow --> green
activated complex (transition state)
31. Determined by the formula h/m(in kg)v - (v=velocity)
wavelength
Valence Electrons(assigned)
vapor pressure
strong acid strong base rxn
32. AX5
Enthalpy of Solution
8.314 J/K mol
surroundings
trigonal bipyramidal
33. Effusion of a gas is inversely proportional to the square root of the molar mass
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34. Absorbs/takes in heat (positive value)
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Integrated Zero-Order Rate Law
second
Endothermic
35. Mol/kg of solvent - used in calculating colligative properties
Molality
Scientific Method
Second-Order Half Life
Its root and adding -ide
36. For significant digits - trailing zeros _____ significant
Bronsted-Lowry Base
Acid + Base --> Salt + Water
bond energy
are
37. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Alkali metals
Bond Energy
Density
Polar Covalent
38. When n=4 ->2 - color=
blue-green
Electron Spin Quantum Number
Faraday
M = square root (3RT/mm)
39. I=moles of particles/moles of solute dissolved
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40. Cation first - anion second
insoluble
Naming Binary Ionic Compounds
Average KE = 1/2(mass)(average speed of all particles)
22.4L
41. A single substance that may be an acid or a base (i.e. water)
system
Amphoteric
g solute/g solvent x 100
Specific Heat (s)
42. Like dissolves...
reduction agent
ionic
ammonium
like
43. Variable for orientation of orbital (-1 through +1)
Delta H or Enthalpy Change
m (third quantum number)
Heat
condensation
44. Molarity (M)
-oic acid
Formal Charge
Percent Yield
moles of solute/ L of solution
45. Temperature-pressure point after which gas can no longer form liquid
Force = mass x acceleration
Alkaline earth metals
E
critical point
46. Specific heat of water
3rd law of thermodynamics
Negative work value; work done by system
4.184
like
47. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
strong bases
Dipole Moment
soluble
strong acids
48. Connects the 2 half cells in a voltaic cell
Covalently w/in themselves - Ionicly bonded w/ each other
salt bridge
Ionic
iodide
49. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
A Roman numeral
effects of IMF
Pauli Exclusion Principle
50. Each orbital can hold two e?s each w/ opposite spins
Isolated System
charge
Pauli Exclusion Principle
Bronsted-Lowry Base