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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. A molecule having a center of positive charge and a center of negative charge
Molal BP Elevation Constant
Dipole Moment
see-saw
f
2. The total energy of the universe is constant - all systems tend towards minimum energy
entropy (S)
Constant Volume
1st law of thermodynamics
P of a =(X of a)(total pressure)
3. Group 1 and heavier Group 2 bases
Molality
Polar Covalent
strong bases
Integrated Zero-Order Rate Law
4. Elements which have unpaired electrons and highly affected by magnetic fields
Linear
supercritical fluid
Radioactivity
paramagnetic
5. Has values 1 -2 -3 -...; tells energy levels
Heat Capacity (C)
equivalence point
Principal Quantum Number
Molecular Compounds
6. Cation first - anion second
msAT
experimental yield
Naming Binary Ionic Compounds
acid
7. SI unit of energy; Kg*m^2/s^2
Molecular
Heisenberg Uncertainty Principle
Joule
activation energy
8. Significant Digits of counted things
Heisenberg Uncertainty Principle
endless
LeChatelier's Principle
Linear
9. Consists of a complex ion - a transition metal with attached ligands - and counterions
Coordination Compound
Q<K
deposition
square planar
10. Energy can't be created nor destroyed
Law of Conservation of Energy
Heat
Scientific Method
Delta H or Enthalpy Change
11. When n=4 ->2 - color=
heat capacity
blue-green
Chemical Kinetics
Decrease Volume and Increase Temperature
12. Instrument used to measure the pressure of atmospheric gas
Molar Heat Capacity
Barometer
equilibrium
Root Mean Square Velocity
13. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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14. Mol/L - concentration of a solution
Molarity
heat capacity
Bases
Transition metals
15. Formula used when diluting stock solution (to find amount of water or stock needed)
bent
3/2RT
bromate
M1V1=M2V2
16. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
Pauli Exclusion Principle
phosphate
3rd law of thermodynamics
17. I=moles of particles/moles of solute dissolved
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18. Group 2 metals
period
Chemical Kinetics
Trigonal Planar
Alkaline earth metals
19. Color of Ba (flame test)
green/yellow
Monoprotic
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
Ligand
20. q cal = ?
Thermochemistry
Enthalpy of Solution
M1V1=M2V2
CAT
21. Significant Digits of Conversion Factors
8.31J/Kmol
endless
Normality
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
22. 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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23. Forward rxn occurs when
Negative work value; work done by system
Atmospheric Pressure
Q<K
Volume Metric Flask & Pipet
24. Peak of energy diagram
activated complex (transition state)
0
-ol
Trigonal Bipyramidal
25. Oxoacid solution (such as HSO4-) forms...
oxide gas and water
Beta Particles-
P of a =(X of a)(total pressure)
M = square root (3RT/mm)
26. Elements on staircase on periodic table
1 atm = 760 mmHg = 101.3 kPa
condensation
Atmospheric Pressure
Metalliods
27. (organics) five carbons
activation energy
pent-
system
AE = q + w
28. Connects the 2 half cells in a voltaic cell
Oxidation is Loss Reduction is Gain
Amino-
salt bridge
Standard Temperature and Pressure
29. When n=3 ->2 - color=
base
Cation
triple point
red
30. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
First-Order Rate Law
4.184
trigonal bipyramidal
31. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
endless
Delta H or Enthalpy Change
equilibrium
32. Anything occupying space and with mass
phosphate
1 atm = 760 mmHg = 101.3 kPa
Bond enthalpy
Matter
33. (organics) double-bonded compound
n0
alkene
alkane
Adding
34. Generally insoluble anions (names)
phosphate - sulfide - carbonate - sulfate
Amount of atoms present
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Dalton's Law
35. Electrons in a hydrogen atom move around the nucleus only in circular orbits
moles of solute/ L of solution
Quantum Model
Molality
carbonate
36. An equilibrium expression
Hund's Rule
Solubility Product (Ksp)
Finding Empirical Formulas
Molar Mass of Element/ Total Molar Mass %
37. AX5
Atmospheric Pressure
trigonal bipyramidal
Matter
conjugate acid
38. Hydroxides are soluble or insoluble?
Dalton's Law of Partial Pressures
red
insoluble
Bond Order
39. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Manometer
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Atmospheric Pressure
Buffered Solution
40. AX3E
2nd law of thermodynamics
viscosity
condensation
trigonal pyramidal
41. Boiling point elevation formula
Law of Conservation of Mass
Integrated Rate Law
?Tb= kb x molality
g solute/g solvent x 100
42. Substance being dissolved in a solution (lower [ ])
22.4L
Solute
force x distance = work done
?Tb= kb x molality
43. Type of system in which nothing is transfered (no mass or energy); ideal
1 atm = 760 mmHg = 101.3 kPa
Isolated System
P1V1/N1T1=P2V2/N2T2
2nd law of thermodynamics
44. (organics) two carbons
Beta Particles-
Heisenberg Uncertainty Principle
v3kT/m
eth-
45. High-speed electrons
Beta Particles-
oxalate
v3kT/m
rate law
46. Cl¹?
Force = mass x acceleration
carbohydrates
chloride
Heat Capacity (C)
47. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Cg=kPg
Beta Particles-
London dispersion forces
lambda
48. Polyatomic Ions (bonding)
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Arrhenius Acid
0
Covalently w/in themselves - Ionicly bonded w/ each other
49. C2O4²?
oxalate
Oxidation is Loss Reduction is Gain
conjugate acid
s
50. R=
Its element
heat capacity
work
8.31J/Kmol