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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. Pure metal or metal hydride + H20 ->
base and hydrogen gas
dec-
?Tb= kb x molality
London dispersion forces
2. Elements in groups 3-12
Density
Hybridization
heat capacity
Transition metals
3. Reverse rxn occurs when
Chemical Bonds
# protons + # neutrons
Q>K
Isolated System
4. Liquid to solid
Quantum Mechanical Model
lambda
1.38x10?²³J/K
freezing
5. When ____ significant digits - round answer to least decimal place
methods of increasing rate
end point
s
Adding
6. Carbon - hydrogen - oxygen compounds
carbohydrates
isothermal
3/2RT
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
7. Formula used when diluting stock solution (to find amount of water or stock needed)
2nd law of thermodynamics
Bronsted-Lowry Base
Volt
M1V1=M2V2
8. Amount of product produced when limiting reactant is used up
Pressure
Cathode
Theoretical yield
Exothermic
9. The likelihood that a rxn will occur "by itself"
M = square root (3RT/mm)
spontaneity
alkene
Joule
10. Atomic #
supercritical fluid
# protons (atom is defined by this)
Covalently w/in themselves - Ionicly bonded w/ each other
Law of Conservation of Energy
11. NO3¹?
single bond
Dalton's Law of Partial Pressures
nitrate
Finding Empirical Formulas
12. #NAME?
AE= AH - RTAn
triple bond
Law of Multiple Proportions
E
13. q H2O = ?
seesaw
P1= X1P1°
msAT
electrolyte
14. Variable for energy of e- - goes from 1 -2 -3 on up
complex ions
Balmer Series
q/moles
n (first quantum number)
15. Mass/volume
phosphate - sulfide - carbonate - sulfate
Electronegativity
Density
London dispersion forces
16. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
Bond Order
not spontaneous
Molarity
Radioactivity
17. Passage of gas through tiny orifice
Effusion
cohesion
Reducing Agent
voltaic cells
18. Energy needed to vaporize a mole of a liquid
nitrate
?Hvap
0
reduction
19. All cations are soluble with bromide - chloride and iodide EXCEPT
Antibonding Molecular Orbital
Ag+ - Pb2+ - Hg2+
strong bases
viscosity
20. 1/[A] vs. time is a ...-order reaction
second
Polar Covalent
rate
0
21. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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22. Solid to liquid
blue-green
rate gas A/rate gas B = square root (mm A/ mm B)
melting
Pressure of H2O must be Subtracted
23. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
Covalently w/in themselves - Ionicly bonded w/ each other
Percent Yield
Cg=kPg
London Dispersion Forces
24. The chemical formed when a base accepts a proton
permanent gases
conjugate acid
-2 - with peroxide -1
Bases
25. 0.00°C - 1 atm
hydrocarbons
methods of increasing rate
Standard Temperature and Pressure
double bond
26. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
p orbitals
square planar
moles solute/kg solvent
Polar Covalent
27. Non-Ideal Gas Conditions
carbonate
high pressure - low temperature
deposition
are
28. Color of K (flame test)
linear
base and hydrogen gas
purple
0
29. Thickness
Tetrahedral
viscosity
Ag+ - Pb2+ - Hg2+
activated complex (transition state)
30. Oxidation # of free elements
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
1 atm
green/yellow
0
31. The reactant in the reduction reaction that forces the oxidation reaction to occur
Oxidizing Agent
8.314 J/K mol
diamagnetic
0.0821 atm L/mol K
32. Oxidation # of Hydrogen
but-
Bronsted-Lowry Acid
+1 - except if bonded to Alkali Metal -1
red
33. ln[A]=-kt + ln[A]0
London dispersion forces
Integrated First-Order Rate Law
Law of Conservation of Mass
-ous acid
34. Where oxidation occurs
Calorimeter
P1= X1P1°
1st law of thermodynamics
Anode
35. Faraday's constant
q/moles
Heat Capacity (C)
adhesion
96500
36. (organics) three carbons
prop-
reduction
strong acid strong base rxn
Balmer Series
37. Does the same as equilibrium expression - except it uses initial concentrations
Enthalpy of Solution
Reaction Quotient (Q)
geometric isomers
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
38. Effusion of a gas is inversely proportional to the square root of the molar mass
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39. These orbitals are spherical
oxidizing agent
End Point
s orbitals
Cathode
40. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
m (third quantum number)
Ampere
insoluble
Counterions
41. Energy required to break a bond
Ionic
Work
Ampere
Bond Energy
42. BrO3¹?
Integrated First-Order Rate Law
bromate
msAT
Molarity
43. (organics) seven carbons
hept-
m (third quantum number)
yellow
Hund's Rule
44. Heat needed to change 1 g of substance to 1°C
specific heat
work
Constant Pressure
trigonal bipyramidal
45. Moles of solute/volume of soln(L)
Linear
Pressure
Molarity
Density
46. 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
Alpha Particles-
Finding Empirical Formulas
cyanide
First-Order Half Life
47. Change in Energy = ? (in terms of constant pressure; for gasses)
Average KE = 1/2(mass)(average speed of all particles)
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
CAT
AE= AH - RTAn
48. Boiling point - melting point - viscosity - vapor pressure - surface tension
Calorimeter
effects of IMF
Molar Heat Capacity
methods of increasing rate
49. Half cell in which reduction occurs
cathode
Kinetic Molecular Theory - for ideal gases
work
Surroundings
50. Phase change from gas to solid
Pauli Exclusion Principle
deposition
4.184
Net Ionic Equation