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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. O²?
pent-
ionic
oxide
0
2. NO3¹?
1.86°C
STP
sulfate
nitrate
3. Elements in groups 3-12
phosphate - sulfide - carbonate - sulfate
Van't Hoff factor
End Point
Transition metals
4. Weakest IMFs - found in all molecules
LE Model
Galvanic Cell
Osmotic Pressure
London dispersion forces
5. Color of Li (flame test)
96500
End Point
Constant Volume
red
6. Higher in energy than the atomic orbitals of which it is composed
activation energy
Radioactivity
Antibonding Molecular Orbital
-oate
7. R=
8.31J/Kmol
cathode
perchlorate
oct-
8. Specific heat of water
chloride
Antibonding Molecular Orbital
Van't Hoff factor
4.184
9. Average speed of gas
v3RT/M(in kg)
melting
Barometer
Polar Covalent
10. negative ion
Anion
Counterions
Matter
entropy
11. These orbitals are spherical
Sigma Bond
Speed of light
s orbitals
rate gas A/rate gas B = square root (mm A/ mm B)
12. Has values from 0 to (n-1); tells shape of atomic orbitals
triple point
square pyramidal
purple
Angular Momentum Quantum Number
13. When n=3 ->2 - color=
Average KE = 1/2(mass)(average speed of all particles)
red
acetate
Molar Mass of Element/ Total Molar Mass %
14. Calculation from K to C
X of a = moles a/total moles
Ag+ - Pb2+ - Hg2+
State Functions
C + 273
15. Solution used in titration
Theory of Relativity
titrant buret
cyanide
Solution
16. Change in Energy = ? (in terms of constant pressure; for gasses)
Boltzmann distribution
96500
k=Ae^(-Ea/RT)
AE= AH - RTAn
17. AX4E
Net Ionic Equation
see-saw
iodide
Decrease Volume and Increase Temperature
18. The likelihood that a rxn will occur "by itself"
spontaneity
Equilibrium constant
oct-
supercritical fluid
19. C2O4²?
oxalate
Volt
blue-violet
Oxidizing Agent
20. Variable for type of orbital
Diffusion
l (second quantum number)
Nernst Equation
Specific Heat (s)
21. Formula used when diluting stock solution (to find amount of water or stock needed)
M1V1=M2V2
bond energy
Law of Multiple Proportions
octahedral
22. IMF that exists in polar molecules
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
excess reactant
Dipole-dipole forces
London dispersion forces
23. Speed of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm A/ mm B)
Anion
Volume Metric Flask & Pipet
Atmospheric Pressure
24. For significant digits - trailing zeros _____ significant
carbohydrates
square pyramidal
are
# protons + # neutrons
25. Symbol for Enthalpy
H
96500
r1/r2
n (first quantum number)
26. 1 sigma bond - 1 pi bond
double bond
Scientific Method
P1= X1P1°
5% rule
27. 6.022x10^23
Strong acid weak base rxn
AH
melting
mol
28. The mixing of native atomic orbitals to form special orbitals for bonding
specific heat
Hybridization
-oic acid
Gamma Ray-
29. Carbon - hydrogen - oxygen compounds
Effusion
carbohydrates
-ic acid
trigonal bipyramidal
30. l=0
Alkali metals
Dipole-dipole forces
s
Hybridization
31. A homogeneous mixture with 1 phase
# protons + # neutrons
Solution
London dispersion forces
moles solute/kg solvent
32. q cal = ?
CAT
endless
geometric isomers
sulfide
33. The part of the universe one is focused upon (in thermodynamics)
Atmospheric Pressure
Tetrahedral
heat capacity
system
34. Cr2O7²?
Root Mean Square Velocity
dichromate
Bond enthalpy
H
35. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Law of Multiple Proportions
Resonance
catalyst
specific heat
36. K
?Tb= kb x molality
adhesion
Equilibrium constant
electrolyte
37. When ____ significant digits - round answer to least decimal place
Cathode
v3kT/m
P of a =(X of a)(total pressure)
Adding
38. The measurement of heat changes
Calorimetry
A Roman numeral
Specific Heat (s)
double bond
39. The total energy of the universe is constant - all systems tend towards minimum energy
Dalton's Law
1st law of thermodynamics
0
v3RT/M(in kg)
40. When gas expands ...
chlorite
Matter
Negative work value; work done by system
Speed of light
41. A molecule having a center of positive charge and a center of negative charge
Dipole Moment
activated complex (transition state)
oxidizing agent
C + 273
42. Actual Yield/Theoretical Yield*100%
2nd law of thermodynamics
alkyne
Van't Hoff factor
Percent Yield
43. These orbitals are perpendicular
p orbitals
Counterions
methoxy-
-one
44. Heat required to raise the system 1°C
8.31J/Kmol
oxide
heat capacity
square planar
45. Mols A/ total mols - XA
# protons + # neutrons
mol Fraction
Faraday
3/2RT
46. A measure of resistance of an object to a change in its state of motion
linear
Monoprotic
AE = q + w
Mass
47. Point at which liquid?gas occurs
Galvanic Cell
boiling point
0.512°C
Mass
48. A weak acid that changes color at or near the equivalence point
End Point
fusion
Anode
indicator
49. Ionizes to produce OH- Ions
permanent gases
Scientific Method
Arrhenius Base
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
50. Tools NEEDED for dilution
yellow --> green
Van't Hoff factor
Volume Metric Flask & Pipet
Limiting reactant