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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. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
?Hvap
PV=nRT
Weight
Magnetic Quantum Number (ml)
2. Point at which solid?liquid occurs
Scientific Method
melting point
-(q of H2O + q of cal)
Bond Energy
3. Non-Ideal Gas Conditions
Delta H or Enthalpy Change
Angular Momentum Quantum Number
high pressure - low temperature
lambda
4. A solution used in titrations whose concentration is known
standard solution
Resonance
octahedral
s
5. Change without heat transfer between the system and its surroundings
0.0826Latm/Kmol
nu
insoluble
adiabatic
6. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
Integrated Zero-Order Rate Law
hydrocarbons
LE Model
spontaneous
7. Higher in energy than the atomic orbitals of which it is composed
Antibonding Molecular Orbital
-oate
Buffer
Alkali metals
8. 101 -325 Pa
standard solution
like
1atm=?Pa
carbohydrates
9. The reactant in the oxidizing reaction that forces the reduction reaction to occur
chloride
Finding Empirical Formulas
Nernst Equation
Reducing Agent
10. Mass #
geometric isomers
# protons + # neutrons
methoxy-
Diffusion
11. Gas to solid
Bronsted-Lowry Base
Constant Pressure
heat of vaporization
deposition
12. In ideal gas law problem - when it says "atmospheric" ...
Pressure of H2O must be Subtracted
bromate
P of a =(X of a)(total pressure)
0.0826Latm/Kmol
13. AH of formation for a substance in its stablest form (how it is found in nature)
Heisenberg Uncertainty Principle
Law of Conservation of Energy
Quantum Mechanical Model
0
14. Energy (definition)
blue-green
s (fourth quantum number)
M = square root (3RT/mm)
force x distance = work done
15. Ideal Gas Law Formula
Hybridization
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
allotrope
PV=nRT
16. #NAME?
Valence Electrons(assigned)
Integrated Rate Law
E
pent-
17. When ____ significant digits - round answer to least decimal place
C + 273
Adding
f
System
18. Newton's Second Law
system
Bonding Pairs
Force = mass x acceleration
sulfate
19. neutron (symbol)
reduction
n0
t-shape
Enthalpy of Solution
20. R in ideal gas law
alkane
0.0821 atm L/mol K
Cation
high pressure - low temperature
21. CrO4²?
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
chromate
insoluble
Percent Yield
22. U(rms)=(3RT/M)^1/2
endothermic
Pressure
violet
Root Mean Square Velocity
23. Liquid to solid
C + 273
Resonance
catalyst
freezing
24. For significant digits - leading zeros ____ significant
are not
octahedral
Finding Empirical Formulas
Integrated Rate Law
25. Oxidation # of Polyatomic Ions
octahedral
double bond
Covalently w/in themselves - Ionicly bonded w/ each other
charge
26. Assumes that a molecule is composed of atoms that are bound together by sharing pairs of electrons using the atomic orbitals of the bound atoms
T-shape
LE Model
anode
strong acid strong base rxn
27. When gas expands ...
Bond Energy
a precipitate forms
Pauli Exclusion Principle
Negative work value; work done by system
28. The chemical formed when an acid donates a proton
alkene
conjugate base
Ionic Compounds
0
29. Matter can't be created nor destroyed
(moles of products that are gasses) - (moles of reactants that are gasses)
Oxidizing Agent
Hybridization
Law of Conservation of Mass
30. Molecules' tendency to stick to one another
Ionic Compounds
vapor pressure
spontaneity
cohesion
31. Ability of an atom in a molecule to attract shared electrons to itself
Colligative properties
# protons + # neutrons
Electronegativity
Quantum Numbers
32. A homogeneous mixture with 1 phase
AE = q + w
Finding Empirical Formulas
Solution
1.86°C
33. A monoatomic cation takes name from...
-(q of H2O + q of cal)
Its element
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
London dispersion forces
34. AX4E
adhesion
methoxy-
see-saw
Osmotic Pressure
35. ... compounds are most conductive
Formal Charge
Q>K
catalyst
ionic
36. All cations are soluble with sulfate EXCEPT
entropy (S)
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Calorimeter
deposition
37. (organics) seven carbons
sulfide
hept-
Speed of light
Molecular
38. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
oxide
Root Mean Square Velocity
complex ions
Equivalence Point
39. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Chemical Kinetics
standard solution
Boltzmann distribution
Calorimeter
40. negative ion
Trigonal Bipyramidal
Decrease Volume and Increase Temperature
+1 - except if bonded to Alkali Metal -1
Anion
41. 2 or more covalently bonded atoms
Increase Temperature
yellow
Molecule
0.0821 atm L/mol K
42. Tools NEEDED for dilution
p orbitals
period
Volume Metric Flask & Pipet
green/yellow
43. K
Equilibrium constant
red/orange
Electronegativity
Percent Yield
44. A measure of randomness or disorder
titrant buret
d orbitals
entropy
Naming Binary Ionic Compounds
45. I¹?
Solute
Formal Charge
boiling point
iodide
46. Calculation from K to C
sulfite
Antibonding Molecular Orbital
C + 273
permanent gases
47. The reactant in the reduction reaction that forces the oxidation reaction to occur
f
third
Zero-Order Rate Law
Oxidizing Agent
48. Has values from 0 to (n-1); tells shape of atomic orbitals
Hybridization
Transition metals
allotrope
Angular Momentum Quantum Number
49. ?T=k*m(solute)
Molal FP Depression Constant
single bond
Molecule
Bronsted-Lowry acid
50. (organics) nine carbons
Weight
violet
boiling point
non-