SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. Ester suffix
# protons + # neutrons
Resonance
Enthalpy of Solution
-oate
2. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Hybridization
yellow --> green
Angular Momentum Quantum Number
Monoprotic
3. Mol/kg of solvent - used in calculating colligative properties
alkyne
Boltzmann distribution
Molality
1atm=?mmHg/Torr
4. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
Counterions
Finding Empirical Formulas
-ic acid
Arrhenius equation
5. AX4E2
Calorimeter
Joule
a precipitate forms
square planar
6. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Constant Pressure
first
Cg=kPg
Root Mean Square Velocity
7. HF+ OH??H2O
high pressure - low temperature
weak acid strong base rxn
phosphate
iodide
8. Stronger IMF= lower... weaker IMF= higher...
Dalton's Law
Joule
vapor pressure
T-shape
9. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
10. kf of water
PEACe 1)each molecule is a Point in space 2)Elastic collisions 3) no force of Attraction 4) no energy lost or gained to Collisions
Average KE = 1/2(mass)(average speed of all particles)
Quantum Model
1.86°C
11. x can be ignored when % ionization is <5%
Equilibrium constant
N=N.(0.5)^time/time half-life
titrant buret
5% rule
12. All cations are soluble with sulfate EXCEPT
+1 - except if bonded to Alkali Metal -1
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Gamma Ray-
r1/r2
13. PO4³?
phosphate
Counterions
Matter
m (third quantum number)
14. Resistance to flow
Scientific Method
actual yield/theoretical yield x 100%
viscosity
Second-Order Half Life
15. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
Anion
blue-green
r1/r2
16. Connects the 2 half cells in a voltaic cell
Linear
Weight
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
salt bridge
17. Osmotic pressure=MRT
Osmotic Pressure
London Dispersion Forces
Principal Quantum Number
Angular Momentum Quantum Number
18. (organics) two carbons
Coordination Compound
eth-
Law of Multiple Proportions
-oic acid
19. Puts OH? into solution
Linear
surroundings
Arrhenius base
permanganate
20. Kinetic Energy is proportional to ______
Van't Hoff factor
Temperature
Multiplying
single bond
21. Loss of electrons - increase in oxidation #
tetrahedral
M1V1=M2V2
oxidation
s (fourth quantum number)
22. Molecules' tendency to stick to the container
3rd law of thermodynamics
Law of Multiple Proportions
prop-
adhesion
23. When n=5 ->2 - color=
blue-violet
8.314 J/K mol
oxidation
supercritical fluid
24. Atoms combine in fixed whole # ratios
5% rule
hydrocarbons
Law of Multiple Proportions
pent-
25. Reverse rxn occurs when
London Dispersion Forces
s (fourth quantum number)
Q>K
Principal Quantum Number
26. Oxidation # of Compounds
freezing
condensation
Covalently w/in themselves - Ionicly bonded w/ each other
0
27. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Alkaline earth metals
Polar Covalent
log[H+]
spontaneous
28. OH¹?
Allotrope
Entropy (S)
nitrate
hydroxide
29. Ionizes to produce OH- Ions
Arrhenius Base
Magnetic Quantum Number (ml)
a precipitate forms
mol
30. Electron pairs found in the space between the atoms
salt bridge
-al
Bonding Pairs
surroundings
31. SO4²?
strong acids
Atmospheric Pressure
sulfate
d
32. Weakest IMFs - found in all molecules
Hess's Law
Average KE = 1/2(mass)(average speed of all particles)
-oate
London dispersion forces
33. q cal = ?
Arrhenius Base
carbonate
CAT
equilibrium
34. If heat capacity isn't mentioned - you can assume that q of cal is = ?
Radioactivity
electron affinity
0
Quantum Numbers
35. Specific heat of water
perchlorate
4.184
hydro-ic acid
permanent gases
36. Composition Formula
Molar Mass of Element/ Total Molar Mass %
Dalton's Law
alkene
melting
37. Amount of heat needed to change a system by 1°C
heat capacity
complex ions
Cation
Delta H or Enthalpy Change
38. Force acting over distance
Work
n0
5% rule
Buffer
39. #NAME?
Amino-
E
Acids
Force = mass x acceleration
40. (N) number of equivalents per liter of solution
Effusion
Density
-al
Normality
41. Forward rxn occurs when
cohesion
Pauli Exclusion Principle
Q<K
Strong acid weak base rxn
42. Rate of Diffusion/Effusion formula
Hydrogen bonding
trigonal bipyramidal
96500
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
43. How to Balance a Redox Equation
Gamma Ray-
Arrhenius Base
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
Ligand
44. AX4
% error
end point
tetrahedral
alkyne
45. r=k[A]^2
alkyne
Force = mass x acceleration
mol Fraction
Second-Order Rate Law
46. 0.00°C - 1 atm
methoxy-
viscosity
Standard Temperature and Pressure
PV=nRT
47. frequency symbol
Temperature
trigonal planar
nu
red
48. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
a precipitate forms
Ionic Compounds
heat capacity
pi=(nRT)/v
49. q H2O = ?
oct-
msAT
Integrated Second-Order Rate Law
red
50. (organics) one carbon
Ideal Gas Law
meth-
-2 - with peroxide -1
22.4L