SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. How to Find an Empirical Formula Given Percentages
Antibonding Molecular Orbital
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
Multiplying
M1V1=M2V2
2. Different form of same element
Manometer
Dipole-dipole forces
allotrope
Enthalpy of Solution
3. Only contains ions that change in reaction
Net Ionic Equation
Alpha Particles-
Trigonal Planar
flouride
4. Change that occurs at constant temperature
paramagnetic
isothermal
0 degrees C - 1 atm
viscosity
5. Combined Gas Law Formula
catalyst
P1V1/N1T1=P2V2/N2T2
spontaneity
Nernst Equation
6. l=1
p
1/2mv²
Hybridization
blue
7. STP
0 degrees C - 1 atm
Radioactivity
Quantum Model
0.0821 atm L/mol K
8. The rest of the universe (in thermodynamics)
Counterions
surroundings
Aufbau Principle
-ous acid
9. PV=nRT
conjugate acid
Ideal Gas Law
oxide gas and water
Strong acid weak base rxn
10. Phase change from solid to gas
chlorite
Molecular Orbitals (MOs)
complex ions
sublimation
11. Mol/L - concentration of a solution
Molarity
Constant Pressure
pi=(nRT)/v
Law of Definite Proportion
12. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
hydrolysis
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
Boltzmann distribution
oxidizing agent
13. A device in which chemical energy is changed to electrical energy
high pressure - low temperature
electron affinity
Galvanic Cell
Positive work value; work done on system
14. When ____ significant digits - round answer to least decimal place
Weight
Adding
double bond
Buffered Solution
15. Pairs of electrons localized on an atom
d orbitals
red
msAT
Lone Pair
16. As protons are added to the nucleus - electrons are similarly added
chromate
Ideal Gas Law
Aufbau Principle
Entropy (S)
17. Loss of electrons - increase in oxidation #
-ic acid
Thermochemistry
Constant Pressure
oxidation
18. The minimum energy that molecules must possess for collisions to be effective - Ea
cohesion
Ag+ - Pb2+ - Hg2+
octahedral
activation energy
19. # bonding e- - # antibonding e-/2
Volt
ether
Bond Order
fusion
20. Everything in the universe that is not defined by you as part of the system
hydrolysis
Strong acid weak base rxn
Matter
Surroundings
21. ?H when 1 mol of bonds is broken in the gaseous state
Joule
LeChatelier's Principle
Bond enthalpy
high pressure - low temperature
22. Raoult's Law - relations between vapor pressure and concentrations
?Tb= kb x molality
P1= X1P1°
zero
heat capacity
23. BrO3¹?
s (fourth quantum number)
bromate
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
salt bridge
24. The chemical formed when an acid donates a proton
conjugate base
force x distance = work done
Integrated Rate Law
Colligative properties
25. Weakest IMFs - found in all molecules
Transition metals
London dispersion forces
Arrhenius equation
Polar Covalent
26. AX3E2
Solute
London Dispersion Forces
T-shape
1st law of thermodynamics
27. Forward rxn occurs when
prop-
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
Q<K
Acid Dissociation Constant
28. Ending for alcohols
yellow
Law of Multiple Proportions
-ol
0
29. These orbitals are perpendicular
Dipole Moment
Cg=kPg
red
p orbitals
30. Half cell in which oxidation occurs
anode
dichromate
Resonance
condensation
31. 6.022x10^23
are
mol
dichromate
hydrocarbons
32. Elements which have unpaired electrons and highly affected by magnetic fields
paramagnetic
Molarity
k=Ae^(-Ea/RT)
lambda
33. (organics) five carbons
Surroundings
pent-
-one
1 atm
34. Color of Li (flame test)
Effusion
London Dispersion Forces
red
CAT
35. If anion ends in -ide - acid name ends in
vaporization
Theory of Relativity
p+
hydro-ic acid
36. Molarity (M)
Exothermic
Percent Yield
moles of solute/ L of solution
nitrite
37. 109.5° - sp^3
Arrhenius equation
q
0
Tetrahedral
38. The reactant that is being reduced - brings about oxidation
Pauli Exclusion Principle
oxidizing agent
experimental yield
-one
39. Calculation from K to C
Density
reduction
Amphoteric
C + 273
40. 1 sigma bond - 2 pi bonds
Closed System
red/orange
phosphate - sulfide - carbonate - sulfate
triple bond
41. Symbol for the heat absorbed or lost molecularly (PER MOLE)
Transition metals
AE= AH - RTAn
AH
precipitate
42. Proton acceptors - must have an unshared pair of e?s
red
London dispersion forces
square pyramidal
Bronsted-Lowry base
43. Solution used in titration
1atm=?Pa
titrant buret
condensation
3.0x108m/s
44. Ability of an atom in a molecule to attract shared electrons to itself
not spontaneous
% yield
Electronegativity
square planar
45. Carbon & hydrogen compounds
Heat
Lone Pair
0.0821 atm L/mol K
hydrocarbons
46. Speed per molecule of gas
Work
v3kT/m
Second-Order Rate Law
indicator
47. AX6
Arrhenius equation
LeChatelier's Principle
octahedral
Strong acid weak base rxn
48. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
allotrope
5% rule
melting point
49. Thickness
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Surroundings
Diffusion
viscosity
50. Aldehyde suffix
isothermal
AH
-al
Open System