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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. Symbol for Enthalpy
hydroxide
Bronsted-Lowry base
H
electrolyte
2. Oxidation # of Oxygen
Cathode
Integrated Rate Law
Equilibrium Expression
-2 - with peroxide -1
3. R=
exothermic
Arrhenius acid
q/moles
0.0826Latm/Kmol
4. Mol/L - concentration of a solution
Molarity
London dispersion forces
log[H+]
P1V1/N1T1=P2V2/N2T2
5. Change in Energy = ? (in terms of constant pressure; for gasses)
Alpha Particles-
AE= AH - RTAn
Reaction Quotient (Q)
22.4L
6. Donates a single H+ Ion (... other prefixes also)
fusion
violet
Monoprotic
titrant buret
7. Energy needed to vaporize a mole of a liquid
bond energy
Endothermic
?Hvap
Joule
8. HF+ OH??H2O
C + 273
AE = q + w
weak acid strong base rxn
conjugate base
9. (N) number of equivalents per liter of solution
Octahedral
Normality
Naming Binary Ionic Compounds
Cell Potential (Ecell)
10. Oxidation # of Halogens
charge
Arrhenius Acid
-1
Multiplying
11. The minimum energy that molecules must possess for collisions to be effective - Ea
1.38x10?²³J/K
sulfate
trigonal planar
activation energy
12. Variable for orientation of orbital (-1 through +1)
Linear
m (third quantum number)
surroundings
Pi Bond
13. NO3¹?
nitrate
End Point
hydro-ic acid
-(P)(Change in V)
14. Connects the 2 half cells in a voltaic cell
salt bridge
Van't Hoff factor
catalyst
Gamma Ray-
15. Weakest IMFs - found in all molecules
London dispersion forces
Law of Definite Proportion
end point
n (first quantum number)
16. AX5
Principal Quantum Number
Anion
trigonal bipyramidal
1 atm = 760 mmHg = 101.3 kPa
17. The measurement of heat changes
Heisenberg Uncertainty Principle
Calorimetry
STP
hydrolysis
18. Point at which the titrated solution changes color
trigonal planar
oct-
end point
Law of Multiple Proportions
19. Proton acceptors - must have an unshared pair of e?s
permanent gases
methods of increasing rate
Solubility Product (Ksp)
Bronsted-Lowry base
20. Rate of Diffusion/Effusion formula
alkene
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
C + 273
Graham's Law
21. ... compounds are most conductive
double bond
chlorite
# protons + # neutrons
ionic
22. We cannot simultaneously determine an atom's exact path or location
Molar Mass of Element/ Total Molar Mass %
Heisenberg Uncertainty Principle
Temperature
dec-
23. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
cyanide
Formal Charge
single bond
s
24. Energy can't be created nor destroyed
critical point
entropy (S)
Law of Conservation of Energy
Matter
25. The total entropy is always increasing - all systems tend towards maximum entropy
square planar
2nd law of thermodynamics
Average KE = 1/2(mass)(average speed of all particles)
purple --> pink
26. 90° - d^2sp^3
# protons (atom is defined by this)
CAT
Octahedral
Finding Empirical Formulas
27. Entropy in the universe is always...
E
increasing
Limiting reactant
Ionic
28. Effusion of a gas is inversely proportional to the square root of the molar mass
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29. All _________ compounds are electrolytes
Chemical Kinetics
green/yellow
Ionic
dichromate
30. Change that occurs at constant temperature
Endothermic
Arrhenius Base
ammonium
isothermal
31. Kinetic Energy of an individual particle formula
melting point
solid CO2
M = square root (3RT/mm)
rate gas A/rate gas B = square root (mm A/ mm B)
32. For significant digits - leading zeros ____ significant
ether
H
C + 273
are not
33. The weighted average of all the isotopes that an atom can have (in g/mol)
0
Equivalence Point
endless
Atomic Mass Unit
34. Pairs of electrons localized on an atom
-(P)(Change in V)
n (first quantum number)
Lone Pair
hydroxide
35. R=
Amount of atoms present
Quantum Numbers
8.31J/Kmol
rate law
36. Change without heat transfer between the system and its surroundings
adiabatic
but-
Ideal Gas Law
charge
37. (organics) double-bonded compound
exothermic
London Dispersion Forces
alkene
Bases
38. (organics) six carbons
hex-
boiling point
CAT
% error
39. In ideal gas law problem - when it says "atmospheric" ...
adhesion
Pressure of H2O must be Subtracted
cyanide
alkane
40. 0.00°C - 1 atm
Equilibrium constant
Octahedral
Standard Temperature and Pressure
perchlorate
41. When n=4 ->2 - color=
?Tf= kf x molality
London dispersion forces
blue-green
Molality
42. Amount of heat needed to change a system by 1°C
triple point
heat capacity
s (fourth quantum number)
Linear
43. Oxidation # of free elements
Force = mass x acceleration
3.0x108m/s
0
boiling point
44. Has values from 0 to (n-1); tells shape of atomic orbitals
P of a =(X of a)(total pressure)
methoxy-
acetate
Angular Momentum Quantum Number
45. AX5E
square pyramidal
Exothermic
Metalliods
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
46. neutron (symbol)
Zero-Order Rate Law
Hund's Rule
Graham's Law
n0
47. Boltzmann constant - used in calculating speed of gas per molecule
3.0x108m/s
Temperature
Bases
1.38x10?²³J/K
48. Polyatomic Ions (bonding)
paramagnetic
Its root and adding -ide
Covalently w/in themselves - Ionicly bonded w/ each other
Net Ionic Equation
49. Oxidation # of Compounds
red
Allotrope
Ampere
0
50. l=2
-ous acid
hex-
Multiplying
d