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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. Amount of heat needed to change a system by 1°C
System
sulfate
reduction
heat capacity
2. All _________ compounds are electrolytes
hydroxide
0 degrees C - 1 atm
Ionic
Its element
3. U(rms)=(3RT/M)^1/2
Heat
iodide
Root Mean Square Velocity
(moles of products that are gasses) - (moles of reactants that are gasses)
4. Amount of product produced when limiting reactant is used up
Bond enthalpy
Theoretical yield
zero
allotrope
5. An equilibrium expression
green/yellow
Temperature
Solubility Product (Ksp)
E
6. Occupies the space above and below a sigma bond
Graham's Law
Allotrope
yellow --> green
Pi Bond
7. R in instances that pertain to energy
8.314 J/K mol
Surroundings
London dispersion forces
sublimation
8. Effusion of a gas is inversely proportional to the square root of the molar mass
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9. How to Find a Weighted Average
Law of Conservation of Energy
A Roman numeral
First-Order Rate Law
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
10. The line running between the atoms
Van't Hoff factor
square planar
Sigma Bond
STP
11. Elements which have unpaired electrons and highly affected by magnetic fields
viscosity
paramagnetic
alkene
yellow
12. (organics) one carbon
Buffer
meth-
red
viscosity
13. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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14. Force acting over distance
Work
Arrhenius base
Nodes
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
15. Solid to gas
sublimation
Naming Binary Ionic Compounds
blue-violet
red
16. #NAME?
Bond enthalpy
E
5% rule
voltaic cells
17. Like dissolves...
experimental yield
Cation
are not
like
18. kb of water
allotrope
msAT
0.512°C
-oate
19. 180° - sp
Closed System
nu
Linear
rate
20. Heat required to raise the system 1°C
heat capacity
Force = mass x acceleration
insoluble
like
21. AX6
-al
f
octahedral
-2 - with peroxide -1
22. AX3E
vapor pressure
isothermal
trigonal pyramidal
Percent Yield
23. Describe various properties of one orbital
viscosity
Quantum Numbers
Atmospheric Pressure
Gamma Ray-
24. E?s fill the lowest energy orbital first - then work their way up
vaporization
Aufbau Principle
effects of IMF
Gamma Ray-
25. The reactant that is being oxidized - brings about reduction
g solute/g solvent x 100
?Tf= kf x molality
Hybridization
reduction agent
26. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Percent Yield
purple --> pink
Manometer
Volume Metric Flask & Pipet
27. Mass/volume
Molality
Density
system
but-
28. All forms of energy except for heat
work
Dipole-dipole forces
0
Hund's Rule
29. The rest of the universe (in thermodynamics)
Molal FP Depression Constant
vaporization
-oic acid
surroundings
30. Universal IMF for nonpolar molecules
strong acid strong base rxn
s (fourth quantum number)
London dispersion forces
Temperature
31. How to Find an Empirical Formula Given Percentages
see-saw
g solute/g solvent x 100
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
1atm=?mmHg/Torr
32. Osmotic pressure=MRT
base and hydrogen gas
Hess's Law
Q<K
Osmotic Pressure
33. SI unit of energy; Kg*m^2/s^2
Weight
Joule
Resonance
P1V1/N1T1=P2V2/N2T2
34. Change in Energy (AE) = ? (in terms of work)
strong acids
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Entropy (S)
AE = q + w
35. A monoatomic cation takes name from...
Reducing Agent
moles of solute/ L of solution
Heat
Its element
36. The total entropy is always increasing - all systems tend towards maximum entropy
heat capacity
2nd law of thermodynamics
Multiplying
Volt
37. Generally insoluble anions (names)
phosphate - sulfide - carbonate - sulfate
Diffusion
hydrolysis
Specific Heat Capacity
38. Reactant which doesn't get used up completely in a chemical reaction
Aufbau Principle
isothermal
sulfide
excess reactant
39. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals
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40. Equation to find Ea from reaction rate constants at two different temperatures
bromate
Heat
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Enthalpy of Solution
41. Energy needed to break a bond
bond energy
Pauli Exclusion Principle
triple point
trigonal bipyramidal
42. S²?
Alkali metals
sulfide
d orbitals
permanganate
43. 6.022x10^23
d
1.86°C
mol
chloride
44. neutron (symbol)
alkane
Anion
rate law
n0
45. Speed of light - C
q
3.0x108m/s
-2 - with peroxide -1
Acid Dissociation Constant
46. Substance that - when dissolved - is conductive
electrolyte
hydrolysis
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
Manometer
47. These orbitals are spherical
alkyne
Colligative properties
rate
s orbitals
48. 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
log[H+]
A Roman numeral
Hybridization
Finding Empirical Formulas
49. Two molecules with identical connectivity but different geometries
geometric isomers
are not
sulfite
Bond Energy
50. Point at which vapor pressure=air pressure above
Solubility Product (Ksp)
boiling point
Angular Momentum Quantum Number
endless