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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. Average speed of gas
v3RT/M(in kg)
allotrope
Work
Quantum Mechanical Model
2. The likelihood that a rxn will occur "by itself"
supercritical fluid
oxide gas and water
AH
spontaneity
3. Change in moles (An) =?
(moles of products that are gasses) - (moles of reactants that are gasses)
rate law
Solvent
deposition
4. Oxidation # of Oxygen
Counterions
3/2RT
-2 - with peroxide -1
nitrate
5. negative ion
London dispersion forces
Anion
red/orange
Aufbau Principle
6. A molecule having a center of positive charge and a center of negative charge
insoluble
spontaneous
Dipole Moment
0
7. Anything occupying space and with mass
Matter
Molarity
salt bridge
nu
8. Osmotic pressure formula
pi=(nRT)/v
vapor pressure
seesaw
Nernst Equation
9. To find activation energy use the...
Antibonding Molecular Orbital
Arrhenius equation
96500
insoluble
10. Color of Na (flame test)
group
-(P)(Change in V)
equilibrium
yellow
11. Experimental yield/theoretical yieldx100
Buffered Solution
Zero-Order Half Life
% yield
Bronsted-Lowry acid
12. All (though really not all - but for our purposes all) ________ compounds are NOT electrolytes
ionic
Molecular
AH
C + 273
13. Degree of disorder in a system
experimental yield
0 degrees C - 1 atm
entropy (S)
22.4L
14. The minimum energy that molecules must possess for collisions to be effective - Ea
0
Kinetic Molecular Theory - for ideal gases
activation energy
Amino-
15. The line running between the atoms
Sigma Bond
Arrhenius base
E
Calorimeter
16. l=2
d
melting point
sulfide
Solubility Product (Ksp)
17. AX6
octahedral
Molal BP Elevation Constant
London dispersion forces
Solute
18. Heat needed to change 1 g of substance to 1°C
sulfate
specific heat
A Roman numeral
Le Chatelier's Principle
19. AX4E
see-saw
hex-
3.0x108m/s
Equilibrium constant
20. 2 or more covalently bonded atoms
ether
heat capacity
Molecule
# protons (atom is defined by this)
21. Calculation from K to C
# protons + # neutrons
permanent gases
moles solute/kg solvent
C + 273
22. CN¹?
soluble
strong bases
cyanide
octahedral
23. Colors of Reaction when (MnO4 -) --> (Mn2+)
purple --> pink
Amino-
0.512°C
moles of solute/ L of solution
24. Cr2O7²?
boiling point
dichromate
Entropy (S)
iodide
25. Point where acid completely neutralizes base
vapor pressure
Calorimeter
cyanide
equivalence point
26. J/°Cmol or J/Kmol
1/2mv²
Molar Heat Capacity
Equilibrium constant
complex ions
27. HF+ OH??H2O
n (first quantum number)
Adding
dichromate
weak acid strong base rxn
28. Electron pairs found in the space between the atoms
Chemical Bonds
single bond
Bond Order
Bonding Pairs
29. Raoult's Law - relations between vapor pressure and concentrations
Arrhenius equation
Buffered Solution
Monoprotic
P1= X1P1°
30. Half-life equation
N=N.(0.5)^time/time half-life
Strong acid weak base rxn
blue-green
cyanide
31. The total energy of the universe is constant - all systems tend towards minimum energy
P of a =(X of a)(total pressure)
1st law of thermodynamics
carbonate
Pi Bond
32. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
complex ions
sublimation
geometric isomers
Equivalence Point
33. PV=nRT
Quantum Model
Ideal Gas Law
blue
Quantum Numbers
34. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
green/yellow
Arrhenius Base
T-shape
35. Actual Yield/Theoretical Yield*100%
Percent Yield
Hybridization
Integrated Zero-Order Rate Law
condensation
36. (organics) three carbons
Hybridization
Nodes
2nd law of thermodynamics
prop-
37. 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
Beta Particles-
Finding Empirical Formulas
Bond enthalpy
Monoprotic
38. The part of the universe one is focused upon (in thermodynamics)
lambda
deposition
system
Its root and adding -ide
39. Theoretical yield-experimental yield/theoretical yieldx100
% error
moles solute/kg solvent
Zero-Order Rate Law
Atmospheric Pressure
40. Oxidation # of Compounds
0
Diffusion
E
third
41. Happens at lines in phase change charts
(moles of products that are gasses) - (moles of reactants that are gasses)
Cation
equilibrium
bent
42. Mole Fraction
X of a = moles a/total moles
Overall Reaction Order
Percent Yield
End Point
43. Electrons in a hydrogen atom move around the nucleus only in circular orbits
?Tf= kf x molality
Quantum Model
1atm=?mmHg/Torr
purple --> pink
44. For colligative properties for electrolytes - the # of mols of ions/ mols of solute
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45. Only contains ions that change in reaction
3/2RT
hex-
Heat Capacity (C)
Net Ionic Equation
46. Point at which the titrated solution changes color
Molarity
end point
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
Density
47. All _________ compounds are electrolytes
tetrahedral
Law of Multiple Proportions
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
Ionic
48. Anions or cations as needed to produce a compound with non net charge
melting point
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
Reducing Agent
Counterions
49. Ptotal=Pa+Pb+Pc....
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50. (# of lone pair e-)+1/2(# of shared e-)
violet
0
Valence Electrons(assigned)
Amino-