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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. Heat needed to change 1 g of substance to 1°C
Angular Momentum Quantum Number
Root Mean Square Velocity
methods of increasing rate
specific heat
2. Mol of solute/kg of solvent
Molality
Theoretical yield
AE= AH - RTAn
22.4L
3. AX2E - AX2E2
0
hydrolysis
Root Mean Square Velocity
bent
4. E=mc^2
Solubility Product (Ksp)
trigonal bipyramidal
-ous acid
Theory of Relativity
5. High-speed electrons
Beta Particles-
isothermal
oxide gas and water
Temperature
6. Equation to find Ea from reaction rate constants at two different temperatures
Standard Temperature and Pressure
Force = mass x acceleration
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
nitrate
7. Pairs of electrons localized on an atom
Lone Pair
Limiting reactant
Isotopes
vaporization
8. A given compound always has exactly the same proportion of elements by mass
allotrope
Law of Definite Proportion
8.31J/Kmol
charge
9. Ionizes to produce OH- Ions
Arrhenius Base
exothermic
ionic
?Tf= kf x molality
10. Has values from 0 to (n-1); tells shape of atomic orbitals
Dalton's Law
Alkaline earth metals
Angular Momentum Quantum Number
pent-
11. Energy needed to break a bond
bond energy
salt bridge
freezing
Acid Dissociation Constant
12. Mass percent
salt bridge
Transition metals
Multiplying
g solute/g solvent x 100
13. Point at which the titrated solution changes color
end point
Zero-Order Rate Law
Dipole Moment
endothermic
14. Chemical composition of dry ice
solid CO2
strong bases
P1= X1P1°
Galvanic Cell
15. NH4¹?
ammonium
trigonal bipyramidal
strong bases
chlorite
16. Electrons in a hydrogen atom move around the nucleus only in circular orbits
heat capacity
not spontaneous
CAT
Quantum Model
17. ClO3²?
amine
Hydrogen bonding
chlorate
Positive work value; work done on system
18. The reactant in the reduction reaction that forces the oxidation reaction to occur
moles solute/kg solvent
blue-violet
m (third quantum number)
Oxidizing Agent
19. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
Bond Energy
Law of Multiple Proportions
Solubility Product (Ksp)
20. CN¹?
Pauli Exclusion Principle
cyanide
AE = q + w
force x distance = work done
21. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
Its element
0
octahedral
Molecular Compounds
22. Kinetic Energy of an individual particle formula
double bond
Joule
M = square root (3RT/mm)
Cg=kPg
23. ln[A]=-kt + ln[A]0
Normality
allotrope
1.86°C
Integrated First-Order Rate Law
24. How to Find a Weighted Average
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
green/yellow
Hybridization
Sigma Bond
25. Actual Yield/Theoretical Yield*100%
Arrhenius Base
Naming Binary Ionic Compounds
Percent Yield
Metalliods
26. Peak of energy diagram
Calorimeter
Law of Multiple Proportions
third
activated complex (transition state)
27. Energy required to break a bond
Molarity
conjugate base
Bond Energy
yellow
28. Speed of light - C
end point
Q>K
3.0x108m/s
Reaction Quotient (Q)
29. .69/k
p orbitals
First-Order Half Life
mol
oct-
30. Puts H? into solution
Arrhenius acid
Le Chatelier's Principle
-one
permanent gases
31. AX3
Calorimetry
trigonal planar
Entropy (S)
exothermic
32. CrO4²?
chromate
vapor pressure
% yield
deposition
33. 760 mmHg - 760 torr
Molality
alkyne
exothermic
1 atm
34. Hydroxides are soluble or insoluble?
Bond enthalpy
phosphate - sulfide - carbonate - sulfate
s
insoluble
35. H?+NH3?NH4
square pyramidal
Equilibrium constant
Strong acid weak base rxn
0
36. #NAME?
Solute
chlorate
Ionic Compounds
E
37. Point at which solid?liquid occurs
melting point
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
Theory of Relativity
Acid + Base --> Salt + Water
38. Delta H (AH) = ?
a precipitate forms
Trigonal Bipyramidal
q/moles
First-Order Half Life
39. U(rms)=(3RT/M)^1/2
strong acid strong base rxn
Root Mean Square Velocity
single bond
are
40. Thickness
electron affinity
s
Zero-Order Rate Law
viscosity
41. The transfer of energy between two objects due to temperature difference
d orbitals
but-
base
Heat
42. Freezing point depression formula
Finding Empirical Formulas
0.512°C
?Tf= kf x molality
Ionic
43. 96 -485 C/mol e-
Bronsted-Lowry Base
Faraday
Angular Momentum Quantum Number
Pauli Exclusion Principle
44. Composition Formula
Zero-Order Half Life
Molar Mass of Element/ Total Molar Mass %
Counterions
equivalence point
45. l=1
p
Volume Metric Flask & Pipet
Ampere
solid CO2
46. Variable for spin of electron (+.5 or -.5)
Bond enthalpy
purple --> pink
Reaction Quotient (Q)
s (fourth quantum number)
47. AX4E
Antibonding Molecular Orbital
are not
C=(mass)(specific heat)
seesaw
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
Finding Empirical Formulas
Bronsted-Lowry Acid
q
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
49. (organics) nine carbons
Ideal Gas Law
endless
-1
non-
50. Has values 1 -2 -3 -...; tells energy levels
Acids
Principal Quantum Number
22.4L
Bronsted-Lowry Acid