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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. The amount of energy/heat required to raise some substance 1 degree C
tetrahedral
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
Heat Capacity (C)
2nd law of thermodynamics
2. The entropy of a pure perfectly formed crystal @0K is 0
3rd law of thermodynamics
Pressure of H2O must be Subtracted
Sigma Bond
Temperature
3. Cl¹?
AE = q + w
chloride
3rd law of thermodynamics
Cell Potential (Ecell)
4. If needed - indicate charge of metal(cation) by...
A Roman numeral
Quantum Model
n (first quantum number)
T-shape
5. An equilibrium expression
alkyne
rate law
3rd law of thermodynamics
Solubility Product (Ksp)
6. Faraday's constant
Heat
purple
Equivalence Point
96500
7. 120° - sp^2
trigonal bipyramidal
oxide
Trigonal Planar
l (second quantum number)
8. Reactant that's completely used up in a chemical reaction
Limiting reactant
Entropy (S)
Surroundings
Pauli Exclusion Principle
9. Atoms with the same number of protons but a different number of neutrons
yellow
Isotopes
8.314 J/K mol
base and hydrogen gas
10. neutron (symbol)
n0
Hess's Law
-(P)(Change in V)
double bond
11. An element with several different forms - each with different properties (i.e. graphite & diamond)
melting point
a precipitate forms
l (second quantum number)
Allotrope
12. Mols A/ total mols - XA
Formal Charge
Naming Binary Ionic Compounds
mol Fraction
3/2RT
13. Oxidation # of Compounds
(moles of products that are gasses) - (moles of reactants that are gasses)
Amino-
0
Law of Conservation of Mass
14. The total energy of the universe is constant - all systems tend towards minimum energy
Covalently w/in themselves - Ionicly bonded w/ each other
rate
AH
1st law of thermodynamics
15. The part of the universe one is focused upon (in thermodynamics)
system
Constant Volume
End Point
Normality
16. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
non-
strong acids
Allotrope
supercritical fluid
17. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
spontaneous
alkane
Allotrope
Molecular Orbitals (MOs)
18. Liquid to solid
rate
freezing
titrant buret
6.63x10?³4Js
19. Solid to gas
ether
Molecular
sublimation
chromate
20. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
p+
H
insoluble
Oxidizing Agent
21. Releases/gives off heat (negative value)
Exothermic
see-saw
Integrated Zero-Order Rate Law
Decrease Volume and Increase Temperature
22. Solution in flask being titrated
Reducing Agent
not spontaneous
Equilibrium Expression
analyte
23. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
soluble
strong bases
P1V1/N1T1=P2V2/N2T2
Arrhenius acid
24. Elements on staircase on periodic table
Metalliods
permanent gases
Hydrogen bonding
different # of neutrons
25. Color of Ba (flame test)
Arrhenius Acid
green/yellow
specific heat
Theoretical yield
26. Mass #
Matter
# protons + # neutrons
double bond
ionic
27. H?+OH??H2O
strong acid strong base rxn
surroundings
Molarity
group
28. Anything occupying space and with mass
Kinetic Molecular Theory - for ideal gases
Matter
alcohol
k=Ae^(-Ea/RT)
29. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Magnetic Quantum Number (ml)
State Functions
Isotopes
surroundings
30. Phase change from gas to solid
deposition
Decrease Volume and Increase Temperature
3/2RT
LE Model
31. 1 sigma bond
Atmospheric Pressure
Matter
single bond
Molar Heat Capacity
32. For significant digits - leading zeros ____ significant
are not
Q>K
boiling point
analyte
33. Negative enthalpy - heat flows into surroundings
Dipole Moment
exothermic
oct-
p orbitals
34. Energy involved in gaining an electron to become a negative ion
cohesion
Molarity
red
electron affinity
35. Mol/kg of solvent - used in calculating colligative properties
base and hydrogen gas
Molality
Pi Bond
freezing
36. Idea Gas Law (actual rules)
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
acid
% yield
ether
37. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
melting point
Ligand
PV=nRT
P of a =(X of a)(total pressure)
38. I=moles of particles/moles of solute dissolved
39. How to Find a Weighted Average
First-Order Rate Law
see-saw
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
methods of increasing rate
40. A weak acid that changes color at or near the equivalence point
Resonance
indicator
Diffusion
alkane
41. Ionizes to produce H+ ions
melting point
Arrhenius Acid
violet
Cell Potential (Ecell)
42. Degree of disorder in a system
Pressure of H2O must be Subtracted
entropy (S)
Dipole-dipole forces
?Tf= kf x molality
43. Experimental yield/theoretical yieldx100
C + 273
First-Order Half Life
% yield
Bond Energy
44. Puts H? into solution
analyte
Aufbau Principle
Arrhenius acid
sulfite
45. 1 sigma bond - 2 pi bonds
Constant Pressure
Faraday
triple bond
p
46. 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
47. Heat capacity formula
Solvent
C=(mass)(specific heat)
Molar Mass of Element/ Total Molar Mass %
surroundings
48. Molecules' tendency to stick to one another
cohesion
Pressure of H2O must be Subtracted
Chemical Kinetics
analyte
49. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
Boltzmann distribution
Speed of light
0 degrees C - 1 atm
reduction
50. (organics) ten carbons
oxide gas and water
dec-
-ol
22.4L