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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. n+m (these are orders of reactants)
Specific Heat (s)
Overall Reaction Order
sublimation
Molecular Compounds
2. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
3rd law of thermodynamics
endless
Amino-
3. Higher in energy than the atomic orbitals of which it is composed
Antibonding Molecular Orbital
actual yield/theoretical yield x 100%
Arrhenius equation
M1V1=M2V2
4. Color of Ba (flame test)
Solubility Product (Ksp)
LE Model
Theoretical yield
green/yellow
5. Symbol for the heat absorbed or lost molecularly (PER MOLE)
A Roman numeral
acid
AH
red
6. Cation first - anion second
oxidation
Naming Binary Ionic Compounds
Mass
v3kT/m
7. AX3E2
t-shape
precipitate
meth-
Diffusion
8. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
catalyst
charge
State Functions
oct-
9. r=k[A]^2
Amino-
triple bond
Second-Order Rate Law
Second-Order Half Life
10. Negative enthalpy - heat flows into surroundings
Cell Potential (Ecell)
Integrated Rate Law
exothermic
Ionic
11. All _________ compounds are electrolytes
Q>K
Ionic
Zero-Order Rate Law
paramagnetic
12. Combined Gas Law Formula
1atm=?mmHg/Torr
5% rule
Calorimeter
P1V1/N1T1=P2V2/N2T2
13. Nonmetal oxide + H2O ->
AE = q + w
acid
flouride
Tetrahedral
14. Symbol for Enthalpy
l (second quantum number)
standard solution
Heisenberg Uncertainty Principle
H
15. K
square planar
Equilibrium constant
endothermic
Faraday
16. Spontaneous emission of radiation
nitrate
Radioactivity
Standard Temperature and Pressure
strong acids
17. Elements in groups 3-12
1atm=?Pa
phosphate
Transition metals
q
18. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Equivalence Point
permanganate
hex-
Volume Metric Flask & Pipet
19. When n=4 ->2 - color=
blue-green
moles of solute/ L of solution
dec-
strong acids
20. Organic w/ -OH group
Law of Multiple Proportions
Angular Momentum Quantum Number
alcohol
flouride
21. 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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22. Reactant that's completely used up in a chemical reaction
Limiting reactant
voltaic cells
green/yellow
1.86°C
23. What is defined by you taken from the whole universe
Enthalpy of Solution
wavelength
System
Pressure
24. Forward rxn occurs when
Q<K
viscosity
g solute/g solvent x 100
Its root and adding -ide
25. Organic w/ -NH2
Zero-Order Half Life
amine
# protons (atom is defined by this)
Atomic Mass Unit
26. Point at which the titrated solution changes color
Density
Ag+ - Pb2+ - Hg2+
end point
chromate
27. Atoms with the same number of protons but a different number of neutrons
Negative work value; work done by system
Isotopes
v3kT/m
Dalton's Law
28. [A]=-kt + [A]0
ionic
London Dispersion Forces
Integrated Zero-Order Rate Law
Arrhenius Acid
29. =vM2/M1
double bond
r1/r2
Faraday
+1 - except if bonded to Alkali Metal -1
30. Where oxidation occurs
Heisenberg Uncertainty Principle
Anode
Heat Capacity (C)
ionic
31. (organics) six carbons
hex-
Molal BP Elevation Constant
solid CO2
Specific Heat Capacity
32. Connects the 2 half cells in a voltaic cell
salt bridge
Oxidation is Loss Reduction is Gain
Its element
acetate
33. H?+NH3?NH4
electron affinity
Arrhenius acid
Strong acid weak base rxn
oxidation
34. Delta H (AH) = ?
alkane
q/moles
X of a = moles a/total moles
Boltzmann distribution
35. All forms of energy except for heat
cathode
work
Integrated Zero-Order Rate Law
M = square root (3RT/mm)
36. Aldehyde suffix
Hydrogen bonding
-al
Molality
-oate
37. Oxidation # of Ions
Molecular Orbitals (MOs)
charge
allotrope
square planar
38. IMF that occurs with FON
Hydrogen bonding
Ampere
Temperature
Negative work value; work done by system
39. All cations are soluble with sulfate EXCEPT
square planar
adhesion
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Molecular
40. Force acting over distance
alkyne
96500
Work
-oic acid
41. CO3²?
Cathode
charge
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
carbonate
42. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
5% rule
Arrhenius acid
weak acid strong base rxn
43. AX3E
trigonal pyramidal
Law of Conservation of Energy
oxidation
-1
44. l=2
Ionic Compounds
Specific Heat (s)
5% rule
d
45. Mol of solute/kg of solvent
Joule
P of a =(X of a)(total pressure)
Molality
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
46. Molality =
Molecular Compounds
meth-
(moles of products that are gasses) - (moles of reactants that are gasses)
moles solute/kg solvent
47. Pairs of electrons localized on an atom
Constant Pressure
oxidation
Root Mean Square Velocity
Lone Pair
48. Diatomic Molecules
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
oxide gas and water
Equilibrium Expression
bond energy
49. Polyatomic Ions (bonding)
l (second quantum number)
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Ampere
Covalently w/in themselves - Ionicly bonded w/ each other
50. Carboxylic acid ending
-oic acid
f
1atm=?mmHg/Torr
second
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