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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. Substances w/ critical temperatures below 25°C
permanent gases
Law of Conservation of Energy
end point
Trigonal Planar
2. Resistance to flow
0
viscosity
are not
zero
3. STP
sulfate
0 degrees C - 1 atm
excess reactant
red
4. Temperature-pressure point after which gas can no longer form liquid
Cg=kPg
Formal Charge
Allotrope
critical point
5. The energy required to raise 1 g of substance 1 degree C
Increase Temperature
Cation
Specific Heat (s)
square pyramidal
6. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
Law of Multiple Proportions
Bond Order
Strong acid weak base rxn
v3RT/M(in kg)
7. Speed per molecule of gas
?Hvap
Le Chatelier's Principle
tetrahedral
v3kT/m
8. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Chemical Kinetics
Net Ionic Equation
Dalton's Law
second
9. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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10. Newton's Second Law
Force = mass x acceleration
trigonal bipyramidal
are not
heat of vaporization
11. Boltzmann constant - used in calculating speed of gas per molecule
X of a = moles a/total moles
1.38x10?²³J/K
Volt
s (fourth quantum number)
12. Ester suffix
second
2nd law of thermodynamics
hex-
-oate
13. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
g solute/g solvent x 100
Multiplying
electrolyte
Equilibrium Expression
14. A monoatomic anion is named by taking...
Boltzmann distribution
wavelength
Its root and adding -ide
supercritical fluid
15. The chemical formed when a base accepts a proton
X of a = moles a/total moles
end point
Equivalence Point
conjugate acid
16. 101 -325 Pa
bromate
Entropy (S)
1atm=?Pa
not spontaneous
17. 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)
Colligative properties
Integrated First-Order Rate Law
Molecular Compounds
Strong acid weak base rxn
18. Electrons in a hydrogen atom move around the nucleus only in circular orbits
paramagnetic
r1/r2
Quantum Model
high pressure - low temperature
19. All _________ compounds are electrolytes
Temperature
Nodes
Graham's Law
Ionic
20. High-speed electrons
P1V1/N1T1=P2V2/N2T2
-ous acid
indicator
Beta Particles-
21. Bomb Calorimeter
Limiting reactant
Constant Volume
lambda
Surroundings
22. Osmotic pressure formula
End Point
?Tb= kb x molality
pi=(nRT)/v
LE Model
23. AX4
tetrahedral
heat capacity
effects of IMF
Electronegativity
24. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
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25. Two molecules with identical connectivity but different geometries
activated complex (transition state)
Magnetic Quantum Number (ml)
geometric isomers
anode
26. 6.022x10^23
mol
Strong acid weak base rxn
Adding
red
27. R in instances that pertain to energy
State Functions
3.0x108m/s
8.314 J/K mol
heat capacity
28. A homogeneous mixture with 1 phase
flouride
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Solution
base and hydrogen gas
29. Group 1 metals
Limiting reactant
Alkali metals
alkane
octahedral
30. Expresses how the concentrations depend on time
Integrated Rate Law
London Dispersion Forces
Zero-Order Half Life
P of a =(X of a)(total pressure)
31. Half cell in which oxidation occurs
anode
1 atm
Quantum Model
single bond
32. 0°C and 1 atm
a precipitate forms
STP
Chemical Bonds
Gamma Ray-
33. These orbitals are perpendicular
octahedral
p orbitals
Molality
end point
34. Variable for type of orbital
l (second quantum number)
Galvanic Cell
First-Order Half Life
square planar
35. Specific heat of water
P1= X1P1°
purple --> pink
4.184
endothermic
36. In ideal gas law problem - when it says "atmospheric" ...
eth-
a precipitate forms
van't Hoff Factor
Pressure of H2O must be Subtracted
37. Measure of the average kinetic energy of all the particles in a substance
electron affinity
g solute/g solvent x 100
excess reactant
Temperature
38. The reactant in the reduction reaction that forces the oxidation reaction to occur
Heisenberg Uncertainty Principle
zero
Oxidizing Agent
trigonal pyramidal
39. Solution in flask being titrated
p+
analyte
flouride
l (second quantum number)
40. Energy required for melting to occur
iodide
heat of fusion
paramagnetic
vaporization
41. Color of Ba (flame test)
Coordination Compound
green/yellow
Anion
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
42. Isotope
red
Hess's Law
Molarity
different # of neutrons
43. Pure metal or metal hydride + H20 ->
3/2RT
base and hydrogen gas
charge
-ic acid
44. Kinetic Energy per mol
Limiting reactant
3/2RT
triple point
phosphate - sulfide - carbonate - sulfate
45. Absorbs/takes in heat (positive value)
Endothermic
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
activated complex (transition state)
activation energy
46. Wavelength symbol
heat capacity
Bronsted-Lowry acid
lambda
4.184
47. To find activation energy use the...
Q>K
Molar Mass of Element/ Total Molar Mass %
Bonding Pairs
Arrhenius equation
48. HF+ OH??H2O
effects of IMF
weak acid strong base rxn
zero
Octahedral
49. Loss of electrons - increase in oxidation #
oxidation
?Hvap
Effusion
green/yellow
50. 1 sigma bond
flouride
single bond
van't Hoff Factor
methoxy-