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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. (organics) six carbons
Molecular Compounds
Theory of Relativity
hex-
octahedral
2. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
rate
ionic
square pyramidal
8.314 J/K mol
3. AX2E - AX2E2
Average KE = 1/2(mass)(average speed of all particles)
Heat Capacity (C)
bent
weak acid strong base rxn
4. Significant Digits of Conversion Factors
London Dispersion Forces
oct-
Ionic
endless
5. 2 or more covalently bonded atoms
acetate
Molecule
Chemical Kinetics
System
6. BrO3¹?
nitrite
bromate
pent-
3.0x108m/s
7. If Q>Ksp
Molar Mass of Element/ Total Molar Mass %
dec-
a precipitate forms
Law of Conservation of Mass
8. 0°C and 1 atm
Anode
STP
# protons + # neutrons
Sigma Bond
9. Kinetic Energy is proportional to ______
Dipole Moment
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
sublimation
Temperature
10. Color of Sr (flame test)
methods of increasing rate
experimental yield
red
Specific Heat (s)
11. For significant digits - leading zeros ____ significant
are not
Counterions
A Roman numeral
perchlorate
12. A monoatomic anion is named by taking...
Second-Order Rate Law
purple --> pink
Its root and adding -ide
charge
13. IMF that occurs with FON
Calorimetry
Temperature
-ous acid
Hydrogen bonding
14. Carbon & hydrogen compounds
Heat
insoluble
hydrocarbons
Molecular Orbitals (MOs)
15. Ideal Gas Law Formula
bromate
PV=nRT
Dalton's Law
Ligand
16. (organics) triple-bonded compound
alkyne
0
specific heat
First-Order Rate Law
17. The reactant in the reduction reaction that forces the oxidation reaction to occur
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
square pyramidal
Oxidizing Agent
oxide
18. When n=6 ->2 - color=
CAT
violet
Work
effects of IMF
19. Organic w/ -NH2
red
Anion
amine
entropy
20. Phase change from solid to gas
2nd law of thermodynamics
oct-
sublimation
but-
21. The reactant in the oxidizing reaction that forces the reduction reaction to occur
moles of solute/ L of solution
Reducing Agent
Acids
Root Mean Square Velocity
22. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
charge
v3kT/m
but-
23. Higher in energy than the atomic orbitals of which it is composed
Antibonding Molecular Orbital
Q>K
Law of Definite Proportion
Bronsted-Lowry Base
24. Type of system in which the energy and mass may leave or enter
msAT
Open System
Hybridization
Coordination Compound
25. 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
LE Model
Bases
hydro-ic acid
isothermal
26. C=2.9979*10^8 m/s
Weight
Speed of light
Law of Multiple Proportions
Isolated System
27. Energy required for liquid?gas
Molar Heat Capacity
heat of vaporization
exothermic
vapor pressure
28. These orbitals are spherical
hydro-ic acid
s orbitals
actual yield/theoretical yield x 100%
purple
29. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
-oic acid
paramagnetic
dec-
30. Group 1 metals
Molality
hept-
Volume Metric Flask & Pipet
Alkali metals
31. Solid to gas
System
Law of Definite Proportion
sublimation
rate gas A/rate gas B = square root (mm A/ mm B)
32. (A) - C/s
Strong acid weak base rxn
heat of vaporization
acid
Ampere
33. The chemical formed when a base accepts a proton
conjugate acid
Cell Potential (Ecell)
Solvent
diamagnetic
34. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Bond enthalpy
Cg=kPg
hex-
Finding Empirical Formulas
35. In covalent bonds - prefixes are used to tell...
Solute
Hund's Rule
Amount of atoms present
Mass
36. Increase Volume
Magnetic Quantum Number (ml)
Increase Temperature
Aufbau Principle
-oate
37. Different form of same element
dichromate
allotrope
phosphate - sulfide - carbonate - sulfate
s (fourth quantum number)
38. (organics) single-bonded compound
-one
alkane
Bases
0.512°C
39. Where reduction occurs
Chemical Bonds
red
triple point
Cathode
40. r=k[A]
Scientific Method
critical point
First-Order Rate Law
Oxidizing Agent
41. Mass reactants= mass products
State Functions
rate
strong bases
Law of Conservation of Mass
42. frequency symbol
Amphoteric
Its element
nu
Adding
43. Measure of the average kinetic energy of all the particles in a substance
Temperature
Isolated System
Open System
?Hvap
44. Energy (definition)
n (first quantum number)
force x distance = work done
1/2mv²
Amphoteric
45. Universal IMF for nonpolar molecules
London dispersion forces
Finding Empirical Formulas
entropy
heat capacity
46. 1/[A]=kt + 1/[A]0
Quantum Numbers
Integrated Second-Order Rate Law
purple
Cation
47. E?s fill the lowest energy orbital first - then work their way up
Aufbau Principle
Dipole Moment
Law of Conservation of Energy
Atomic Mass Unit
48. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Kinetic Molecular Theory - for ideal gases
Metalliods
1.38x10?²³J/K
Acid + Base --> Salt + Water
49. AX5
alcohol
Barometer
System
trigonal bipyramidal
50. Kinetic Energy per molecule
Linear
Nodes
solid CO2
1/2mv²
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