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Test your basic knowledge |
AP Chemistry
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Study First
Subjects
:
science
,
ap
,
chemistry
Instructions:
Answer 50 questions in 15 minutes.
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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. These orbitals are diagonal
chloride
d orbitals
sublimation
Aufbau Principle
2. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
Nernst Equation
Equivalence Point
Open System
Quantum Mechanical Model
3. Reactant which doesn't get used up completely in a chemical reaction
cohesion
Molecular Orbitals (MOs)
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
excess reactant
4. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
soluble
E
oxalate
Manometer
5. 1/([A]0*k)
Pressure
q/moles
Second-Order Half Life
Joule
6. SO4²?
sulfate
weak acid strong base rxn
f
group
7. Universal IMF for nonpolar molecules
PV=nRT
# protons (atom is defined by this)
London dispersion forces
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
8. Significant Digits of Conversion Factors
Molarity
endless
Dipole Moment
methods of increasing rate
9. Combined Gas Law Formula
Dipole Moment
M = square root (3RT/mm)
P1V1/N1T1=P2V2/N2T2
Quantum Model
10. Instrument used to measure the pressure of atmospheric gas
Temperature
Barometer
Matter
are
11. AX4
tetrahedral
Zero-Order Rate Law
Root Mean Square Velocity
Pi Bond
12. When n=5 ->2 - color=
Diffusion
?Tb= kb x molality
blue-violet
oxidizing agent
13. ln[A]=-kt + ln[A]0
allotrope
Integrated First-Order Rate Law
insoluble
?Hvap
14. 6.022x10^23
activated complex (transition state)
Allotrope
Solution
mol
15. If Q<Ksp
STP
Nodes
Cell Potential (Ecell)
no precipitate forms
16. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Transition metals
Formal Charge
adhesion
Anion
17. Rate of Diffusion/Effusion formula
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
State Functions
trigonal planar
red
18. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
Specific Heat (s)
reduction agent
strong acids
see-saw
19. Formula used when diluting stock solution (to find amount of water or stock needed)
M1V1=M2V2
chromate
Molality
Molecule
20. Forward rxn occurs when
Law of Conservation of Mass
Q<K
p+
Molecular
21. Energy required for melting to occur
heat of fusion
permanganate
heat of vaporization
l (second quantum number)
22. Substances w/ critical temperatures below 25°C
s (fourth quantum number)
permanent gases
heat capacity
activated complex (transition state)
23. (organics) five carbons
pent-
?Tb= kb x molality
work
alkane
24. Driving force of the electrons
Cell Potential (Ecell)
Ampere
oct-
oxide
25. Point where acid completely neutralizes base
phosphate
end point
T-shape
equivalence point
26. When n=6 ->2 - color=
violet
analyte
Reducing Agent
activated complex (transition state)
27. AX5E
Open System
Faraday
square pyramidal
msAT
28. Half cell in which reduction occurs
n0
hept-
cathode
strong acids
29. (organics) eight carbons
base
oct-
London dispersion forces
adiabatic
30. Oxidation # of Ions
Cell Potential (Ecell)
charge
Equilibrium Expression
Lone Pair
31. Heat needed to change 1 g of substance to 1°C
?Tf= kf x molality
specific heat
Theoretical yield
endless
32. Atoms combine in fixed whole # ratios
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
AH
Law of Multiple Proportions
activation energy
33. The minimum energy that molecules must possess for collisions to be effective - Ea
Gamma Ray-
square planar
activation energy
Formal Charge
34. F¹?
flouride
-1
melting point
voltaic cells
35. r=k
Zero-Order Rate Law
linear
Lone Pair
Sigma Bond
36. Osmotic pressure formula
Joule
Gamma Ray-
cathode
pi=(nRT)/v
37. The total energy of the universe is constant - all systems tend towards minimum energy
1st law of thermodynamics
fusion
Net Ionic Equation
Resonance
38. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
Endothermic
Antibonding Molecular Orbital
Heat
39. Equation to find Ea from reaction rate constants at two different temperatures
Negative work value; work done by system
End Point
salt bridge
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
40. 1 sigma bond - 2 pi bonds
sulfate
Coordination Compound
triple bond
1 atm
41. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Root Mean Square Velocity
yellow --> green
LeChatelier's Principle
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
42. C=2.9979*10^8 m/s
blue
Equilibrium Expression
Speed of light
condensation
43. ?T=k*m(solute)
Strong acid weak base rxn
oxidation
Molal BP Elevation Constant
Arrhenius acid
44. In covalent bonds - prefixes are used to tell...
Amount of atoms present
green/yellow
Oxidation is Loss Reduction is Gain
Calorimeter
45. 1 sigma bond - 1 pi bond
double bond
Surroundings
alcohol
Limiting reactant
46. Energy involved in gaining an electron to become a negative ion
0.0821 atm L/mol K
Bonding Pairs
Chemical Bonds
electron affinity
47. Like dissolves...
Overall Reaction Order
allotrope
l (second quantum number)
like
48. High-speed electrons
Beta Particles-
Bond Energy
Integrated Rate Law
are not
49. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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on line
183
50. CN¹?
Bronsted-Lowry Base
adhesion
supercritical fluid
cyanide
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