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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. 120° - sp^2
Trigonal Planar
Second-Order Half Life
3/2RT
spontaneity
2. Heat capacity formula
Average KE = 1/2(mass)(average speed of all particles)
Naming Binary Ionic Compounds
C=(mass)(specific heat)
Q<K
3. Symbol for Enthalpy
H
Molarity
Its root and adding -ide
square pyramidal
4. Average Kinetic Energy Formula
Average KE = 1/2(mass)(average speed of all particles)
condensation
M = square root (3RT/mm)
viscosity
5. Energy involved in gaining an electron to become a negative ion
Valence Electrons(assigned)
electron affinity
oxide
paramagnetic
6. Temperature-pressure point after which gas can no longer form liquid
Hybridization
critical point
Solute
s
7. Matter can't be created nor destroyed
Law of Conservation of Mass
# protons (atom is defined by this)
red/orange
Temperature
8. When n=6 ->2 - color=
P of a =(X of a)(total pressure)
Manometer
alkane
violet
9. If K>1 - then Gº<0 and reaction will be...at chemical equilibrium
complex ions
violet
pi=(nRT)/v
spontaneous
10. AX4
3/2RT
Gamma Ray-
permanent gases
tetrahedral
11. Where there are no electrons
Nodes
?Hvap
boiling point
Atomic Mass Unit
12. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Buffer
triple bond
are
first
13. Equation to find Ea from reaction rate constants at two different temperatures
Sigma Bond
Electronegativity
Ampere
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
14. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
-al
chlorate
+1 - except if bonded to Alkali Metal -1
15. Force acting over distance
Aufbau Principle
Work
Cation
are
16. Solid to gas
sublimation
g solute/g solvent x 100
f
-ous acid
17. Where reduction occurs
% yield
deposition
Cathode
Integrated First-Order Rate Law
18. The mixing of native atomic orbitals to form special orbitals for bonding
deposition
Hybridization
Integrated Rate Law
solid CO2
19. Molecules' tendency to stick to one another
0.0826Latm/Kmol
cohesion
Speed of light
alkyne
20. Energy can't be created nor destroyed
Closed System
strong bases
Density
Law of Conservation of Energy
21. Kinetic Energy of an individual particle formula
methods of increasing rate
H
M = square root (3RT/mm)
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
22. ?T=k*m(solute)
hex-
bent
Constant Volume
Molal BP Elevation Constant
23. ln[A]=-kt + ln[A]0
Integrated First-Order Rate Law
chlorate
adhesion
red
24. Type of system in which the energy and mass may leave or enter
Normality
Open System
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
E
25. Oxidation # of Compounds
0
Heat Capacity (C)
N=N.(0.5)^time/time half-life
Molecule
26. 109.5° - sp^3
Tetrahedral
amine
Anode
8.314 J/K mol
27. Increase Volume
Barometer
viscosity
Joule
Increase Temperature
28. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Nodes
Strong acid weak base rxn
Ionic Compounds
ether
29. Pressure Units/Conversions
heat capacity
soluble
State Functions
1 atm = 760 mmHg = 101.3 kPa
30. These orbitals are diagonal
Work
m (third quantum number)
Normality
d orbitals
31. 96 -485 C/mol e-
Faraday
H
Sigma Bond
Resonance
32. r=k
CAT
Zero-Order Rate Law
l (second quantum number)
Scientific Method
33. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Manometer
allotrope
m (third quantum number)
Volume Metric Flask & Pipet
34. R=
Strong acid weak base rxn
boiling point
8.31J/Kmol
square planar
35. In covalent bonds - prefixes are used to tell...
p+
Amount of atoms present
ether
P1= X1P1°
36. Studies the rate at which a chemical process occurs and sheds light on its reaction mechanism
Chemical Kinetics
strong acid strong base rxn
Delta H or Enthalpy Change
supercritical fluid
37. Higher in energy than the atomic orbitals of which it is composed
strong acid strong base rxn
Solvent
Antibonding Molecular Orbital
-oic acid
38. pH=
log[H+]
Linear
Amount of atoms present
1atm=?mmHg/Torr
39. Gain of electrons - decrease in oxidation #
reduction
Mass
Increase Temperature
Pi Bond
40. Spectrum of light when an electron drops to energy level n=2
prop-
Balmer Series
heat of vaporization
activated complex (transition state)
41. (organics) seven carbons
hept-
oct-
Integrated Rate Law
bond energy
42. C2H3O2¹?
Solubility Product (Ksp)
acetate
Molal BP Elevation Constant
specific heat
43. O²?
0
oxide
alkene
freezing
44. Work = ?
base
Cg=kPg
-(P)(Change in V)
Atmospheric Pressure
45. IMF that exists in polar molecules
conjugate base
activated complex (transition state)
?Tb= kb x molality
Dipole-dipole forces
46. Amine prefix
activation energy
excess reactant
Amino-
sulfite
47. r=k[A]
Pressure of H2O must be Subtracted
Closed System
0
First-Order Rate Law
48. The chemical formed when a base accepts a proton
Resonance
meth-
State Functions
conjugate acid
49. These orbitals are perpendicular
Molecule
bromate
p orbitals
red
50. AX6
octahedral
Anode
Colligative properties
melting
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