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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. PV=nRT
Ideal Gas Law
Boltzmann distribution
like
Isolated System
2. (organics) double-bonded compound
Radioactivity
0.0821 atm L/mol K
oxidizing agent
alkene
3. The weight exerted by a column of air or the pressure exerted by the Earth's atmosphere
Bonding Pairs
Faraday
Atmospheric Pressure
Anode
4. Point where acid completely neutralizes base
equivalence point
Constant Volume
phosphate - sulfide - carbonate - sulfate
M1V1=M2V2
5. frequency symbol
Law of Definite Proportion
0
nu
titrant buret
6. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Pressure of H2O must be Subtracted
prop-
yellow --> green
indicator
7. Happens at lines in phase change charts
Negative work value; work done by system
dichromate
Principal Quantum Number
equilibrium
8. The driving force for a spontaneous is an increase in entropy of the universe
Its element
Entropy (S)
Joule
Heat
9. Raising heat - adding catalyst - heighten concentration - bigger surface area
methods of increasing rate
sublimation
Second-Order Half Life
Hydrogen bonding
10. Type of system in which the energy and mass may leave or enter
Open System
red
soluble
sublimation
11. A method of investigation involving observation and theory to test scientific hypotheses
Scientific Method
Temperature
STP
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
12. Temperature-pressure point after which gas can no longer form liquid
oxide gas and water
Specific Heat Capacity
trigonal planar
critical point
13. q rxn = ?
Hund's Rule
Second-Order Rate Law
Atmospheric Pressure
-(q of H2O + q of cal)
14. Molecules' tendency to stick to the container
oct-
Amino-
adhesion
-(P)(Change in V)
15. Similar to atomic orbitals - except between molecules
Molecular Orbitals (MOs)
Effusion
Theoretical yield
?Tb= kb x molality
16. Speed of Diffusion/Effusion formula
weak acid strong base rxn
rate gas A/rate gas B = square root (mm A/ mm B)
Molecular Orbitals (MOs)
pent-
17. Atomic #
strong acid strong base rxn
% yield
# protons (atom is defined by this)
0
18. Theoretical yield-experimental yield/theoretical yieldx100
% error
Root Mean Square Velocity
excess reactant
voltaic cells
19. 90° - d^2sp^3
p
Octahedral
Exothermic
Calorimeter
20. R=
Cg=kPg
0.0826Latm/Kmol
Buffer
Finding Empirical Formulas
21. Reverse rxn occurs when
-al
triple bond
Sigma Bond
Q>K
22. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
seesaw
msAT
Resonance
Ideal Gas Law
23. Mass/volume
Density
-ic acid
CAT
Theory of Relativity
24. S²?
bent
Dalton's Law of Partial Pressures
sulfide
C + 273
25. As protons are added to the nucleus - electrons are similarly added
conjugate acid
Manometer
Aufbau Principle
Enthalpy of Solution
26. A measure of resistance of an object to a change in its state of motion
Work
Mass
Molal FP Depression Constant
sulfate
27. Carboxylic acid ending
-oic acid
Valence Electrons(assigned)
d
Positive work value; work done on system
28. Force per unit area
Pressure
yellow --> green
Speed of light
Theory of Relativity
29. Spectrum of light when an electron drops to energy level n=2
Balmer Series
Joule
0 degrees C - 1 atm
v3kT/m
30. The chemical formed when an acid donates a proton
Acid + Base --> Salt + Water
Arrhenius Base
conjugate base
base
31. Mols A/ total mols - XA
mol Fraction
lambda
electron affinity
8.314 J/K mol
32. Change without heat transfer between the system and its surroundings
adiabatic
like
AE = q + w
oxidizing agent
33. % yield
Quantum Model
Increase Temperature
tetrahedral
actual yield/theoretical yield x 100%
34. Pressure Units/Conversions
Bonding Pairs
1 atm = 760 mmHg = 101.3 kPa
insoluble
Valence Electrons(assigned)
35. Does the same as equilibrium expression - except it uses initial concentrations
sulfate
non-
reduction
Reaction Quotient (Q)
36. Molecules' tendency to stick to one another
cohesion
-ous acid
1.38x10?²³J/K
Amphoteric
37. Mixing of gases
wavelength
Adding
Nodes
Diffusion
38. AX2E - AX2E2
Monoprotic
Speed of light
bent
double bond
39. A monoatomic cation takes name from...
see-saw
Its element
insoluble
Naming Binary Ionic Compounds
40. 96 -485 C/mol e-
boiling point
(moles of products that are gasses) - (moles of reactants that are gasses)
Molarity
Faraday
41. Variable for type of orbital
Isotopes
activated complex (transition state)
l (second quantum number)
strong bases
42. Dirrect Method Formula
Molal FP Depression Constant
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Bond Order
Cell Potential (Ecell)
43. Cl¹?
square planar
voltaic cells
chloride
moles solute/kg solvent
44. Atoms with the same number of protons but a different number of neutrons
prop-
Isotopes
Theoretical yield
?Tf= kf x molality
45. Proton donors
Ionic Compounds
London dispersion forces
Bronsted-Lowry acid
permanganate
46. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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47. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
Negative work value; work done by system
Endothermic
-al
48. If heat capacity isn't mentioned - you can assume that q of cal is = ?
Lone Pair
endless
0
triple bond
49. We cannot simultaneously determine an atom's exact path or location
system
P of a =(X of a)(total pressure)
Boltzmann distribution
Heisenberg Uncertainty Principle
50. 760mmHg/Torr
period
3rd law of thermodynamics
1atm=?mmHg/Torr
third