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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. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
6.63x10?³4Js
Van't Hoff factor
Normality
spontaneous
2. Mass percent
log[H+]
g solute/g solvent x 100
f
oxide gas and water
3. Elements in groups 3-12
Amount of atoms present
m (third quantum number)
London Dispersion Forces
Transition metals
4. A given compound always has exactly the same proportion of elements by mass
triple point
Law of Definite Proportion
green/yellow
geometric isomers
5. Peak of energy diagram
l (second quantum number)
activated complex (transition state)
Graham's Law
sulfide
6. When ____ significant digits - round answer to least decimal place
Electronegativity
oxide
Finding Empirical Formulas
Adding
7. Thickness
conjugate acid
Finding Empirical Formulas
Temperature
viscosity
8. Instrument used to measure the pressure of atmospheric gas
N=N.(0.5)^time/time half-life
Covalently w/in themselves - Ionicly bonded w/ each other
Barometer
-ol
9. Energy required to break a bond
Negative work value; work done by system
effects of IMF
Bond Energy
t-shape
10. Oxidation # of Polyatomic Ions
LeChatelier's Principle
0
Molecular
charge
11. The mixing of native atomic orbitals to form special orbitals for bonding
Pressure
Hybridization
like
blue
12. ?Hsoln=?H1+?H2+?H3+...
22.4L
Anode
Positive work value; work done on system
Enthalpy of Solution
13. The energy required to raise 1 g of substance 1 degree C
specific heat
red
Specific Heat (s)
hept-
14. SO3²?
standard solution
g solute/g solvent x 100
different # of neutrons
sulfite
15. Change without heat transfer between the system and its surroundings
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
M1V1=M2V2
adiabatic
hept-
16. J/°Cmol or J/Kmol
but-
Hydrogen bonding
Molar Heat Capacity
Angular Momentum Quantum Number
17. Non-Ideal Gas Conditions
?Tb= kb x molality
high pressure - low temperature
Second-Order Half Life
mol Fraction
18. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
but-
voltaic cells
insoluble
s
19. Ptotal=P1+P2+P3+...
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183
20. Proton (symbol)
p+
Calorimetry
pi=(nRT)/v
msAT
21. Oxidation # of Oxygen
Barometer
London Dispersion Forces
-2 - with peroxide -1
Atomic Mass Unit
22. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
Acid Dissociation Constant
LE Model
precipitate
alcohol
23. l=1
Arrhenius Acid
p
analyte
Electronegativity
24. When n=5 ->2 - color=
deposition
methoxy-
blue-violet
Barometer
25. AX5E
square pyramidal
Manometer
Theory of Relativity
spontaneity
26. (organics) single-bonded compound
Isotopes
Reaction Quotient (Q)
alkane
Molecular
27. How to Find a Weighted Average
1atm=?mmHg/Torr
third
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
period
28. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Cg=kPg
Mass
l (second quantum number)
Colligative properties
29. Passage of gas through tiny orifice
chlorite
Effusion
Molecule
London dispersion forces
30. Kinetic Energy per mol
3/2RT
-ic acid
Naming Binary Ionic Compounds
dichromate
31. Delta H (AH) = ?
phosphate - sulfide - carbonate - sulfate
Law of Conservation of Mass
q/moles
Trigonal Planar
32. 2 or more covalently bonded atoms
96500
Molecule
v3RT/M(in kg)
equivalence point
33. C2H3O2¹?
Solvent
acetate
Quantum Model
msAT
34. Cr2O7²?
P1V1/N1T1=P2V2/N2T2
dichromate
Chemical Bonds
Dipole-dipole forces
35. Organic w/ -O-
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
ether
reduction agent
Arrhenius base
36. Kinetic Energy of an individual particle formula
End Point
M = square root (3RT/mm)
Amphoteric
Closed System
37. If anion ends in -ate - acid name ends in...
Matter
Zero-Order Half Life
-ic acid
Covalently w/in themselves - Ionicly bonded w/ each other
38. E=mc^2
f
endless
Theory of Relativity
-one
39. Solution used in titration
titrant buret
activated complex (transition state)
melting
Trigonal Planar
40. AX3E
trigonal pyramidal
work
Decrease Volume and Increase Temperature
P of a =(X of a)(total pressure)
41. O²?
Hund's Rule
bent
22.4L
oxide
42. Coffee Cup Calorimeter
trigonal bipyramidal
Constant Pressure
-one
STP
43. Tools NEEDED for dilution
boiling point
Temperature
Volume Metric Flask & Pipet
reduction
44. Raising heat - adding catalyst - heighten concentration - bigger surface area
heat capacity
Polar Covalent
trigonal planar
methods of increasing rate
45. AX3E2
melting
Weight
n (first quantum number)
t-shape
46. Speed of light - C
Antibonding Molecular Orbital
cyanide
Molar Heat Capacity
3.0x108m/s
47. r=k[A]
Constant Pressure
indicator
First-Order Rate Law
Arrhenius acid
48. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
London Dispersion Forces
eth-
conjugate acid
Pauli Exclusion Principle
49. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
rate
heat capacity
red
Molar Mass of Element/ Total Molar Mass %
50. ClO3²?
rate
weak acid strong base rxn
Lone Pair
chlorate