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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. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
yellow --> green
conjugate base
boiling point
Molarity
2. Force that holds atoms together
Bond Order
Calorimetry
Beta Particles-
Chemical Bonds
3. ClO3²?
chlorate
Calorimetry
conjugate base
entropy
4. Boiling point elevation formula
nitrite
Solvent
electron affinity
?Tb= kb x molality
5. kf of water
Oxidizing Agent
1.86°C
complex ions
Root Mean Square Velocity
6. These orbitals are perpendicular
indicator
deposition
p orbitals
Solvent
7. ?T=k*m(solute)
Molal BP Elevation Constant
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
methoxy-
Ideal Gas Law
8. Organic w/ -OH group
sulfide
CAT
entropy
alcohol
9. Oxidation # of Halogens
Faraday
soluble
-1
Matter
10. What is defined by you taken from the whole universe
AE = q + w
Ag+ - Pb2+ - Hg2+
AH
System
11. Verticals on the periodic table
group
Law of Conservation of Mass
no precipitate forms
complex ions
12. Force acting over distance
viscosity
Bronsted-Lowry base
Work
pent-
13. q rxn = ?
-(q of H2O + q of cal)
1/2mv²
precipitate
London dispersion forces
14. A solid or gas that can be formed when 2 or more aqueous reactants come together
Acid Dissociation Constant
Quantum Numbers
precipitate
# protons + # neutrons
15. Effusion of a gas is inversely proportional to the square root of the molar mass
16. Combined Gas Law Formula
P1V1/N1T1=P2V2/N2T2
Heat Capacity (C)
Dalton's Law of Partial Pressures
base and hydrogen gas
17. Only contains ions that change in reaction
moles solute/kg solvent
octahedral
Net Ionic Equation
Open System
18. AX5E
Second-Order Half Life
spontaneous
p+
square pyramidal
19. [A]=-kt + [A]0
Integrated Zero-Order Rate Law
Molar Mass of Element/ Total Molar Mass %
Specific Heat (s)
Q<K
20. (A) - C/s
Hydrogen bonding
0
Ampere
Dalton's Law of Partial Pressures
21. HF+ OH??H2O
first
-(q of H2O + q of cal)
Chemical Kinetics
weak acid strong base rxn
22. High-speed electrons
trigonal bipyramidal
system
1 atm = 760 mmHg = 101.3 kPa
Beta Particles-
23. Like dissolves...
specific heat
Integrated Rate Law
period
like
24. The measurement of heat changes
Arrhenius Base
Calorimetry
n0
Covalently w/in themselves - Ionicly bonded w/ each other
25. frequency symbol
reduction
nu
Atomic Mass Unit
% error
26. 2+ charge
Alpha Particles-
Manometer
1st law of thermodynamics
Strong acid weak base rxn
27. AX3E2
Monoprotic
geometric isomers
End Point
t-shape
28. C=2.9979*10^8 m/s
Speed of light
Positive work value; work done on system
titrant buret
hept-
29. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
red/orange
Chemical Kinetics
-oic acid
moles of solute/ L of solution
30. Two molecules with identical connectivity but different geometries
geometric isomers
melting point
Nodes
Enthalpy of Solution
31. q H2O = ?
msAT
1atm=?mmHg/Torr
Acid Dissociation Constant
Pressure
32. Liquid to gas
meth-
vaporization
titrant buret
Normality
33. Puts H? into solution
0
Arrhenius acid
Zero-Order Rate Law
cyanide
34. 120° - sp^2
Trigonal Planar
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
k=Ae^(-Ea/RT)
Arrhenius Base
35. Tools NEEDED for dilution
Molality
Volume Metric Flask & Pipet
period
Solution
36. Kinetic Energy is proportional to ______
Temperature
Colligative properties
Molecular
Tetrahedral
37. Formula used when diluting stock solution (to find amount of water or stock needed)
Colligative properties
Root Mean Square Velocity
linear
M1V1=M2V2
38. Ptotal=P1+P2+P3+...
39. Solid to liquid
melting
green/yellow
Dipole Moment
Second-Order Half Life
40. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
rate law
Cg=kPg
insoluble
Gamma Ray-
41. High-energy light
Gamma Ray-
Quantum Mechanical Model
period
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
42. Within a sublevel - place one e? per orbital before pairing them
43. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Colligative properties
moles of solute/ L of solution
Antibonding Molecular Orbital
condensation
44. (organics) double-bonded compound
alkene
vapor pressure
Effusion
f
45. The total entropy is always increasing - all systems tend towards maximum entropy
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Volume Metric Flask & Pipet
2nd law of thermodynamics
Oxidizing Agent
46. BrO3¹?
0
viscosity
Percent Yield
bromate
47. Variable for spin of electron (+.5 or -.5)
strong acids
s (fourth quantum number)
# protons + # neutrons
work
48. AX6
octahedral
trigonal planar
dichromate
anode
49. Idea Gas Law (actual rules)
vapor pressure
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
-al
no precipitate forms
50. Ka=[products]^m/[reactants]^n
hydrolysis
Acid Dissociation Constant
heat capacity
# protons (atom is defined by this)