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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. Average Kinetic Energy Formula
conjugate acid
-1
Average KE = 1/2(mass)(average speed of all particles)
Molecular
2. Different form of same element
q
-ous acid
allotrope
indicator
3. AX3E2
purple
t-shape
vaporization
effects of IMF
4. AH of formation for a substance in its stablest form (how it is found in nature)
Acid Dissociation Constant
Principal Quantum Number
0
Quantum Model
5. Degree of disorder in a system
spontaneity
entropy (S)
alkene
Buffer
6. AX5E
8.314 J/K mol
square pyramidal
C + 273
pi=(nRT)/v
7. Generally insoluble anions (names)
-(q of H2O + q of cal)
anode
Theoretical yield
phosphate - sulfide - carbonate - sulfate
8. Driving force of the electrons
salt bridge
Law of Conservation of Mass
Cell Potential (Ecell)
not spontaneous
9. AX3E2
Ampere
Exothermic
T-shape
Allotrope
10. kf of water
pent-
dec-
Trigonal Planar
1.86°C
11. NO2¹?
Delta H or Enthalpy Change
Nodes
-oic acid
nitrite
12. Hydroxides are soluble or insoluble?
insoluble
spontaneity
Dipole Moment
CAT
13. Ionizes to produce H+ ions
moles of solute/ L of solution
Arrhenius Acid
LE Model
oxalate
14. The reactant in the reduction reaction that forces the oxidation reaction to occur
Oxidizing Agent
Density
alkyne
blue-green
15. All cations are soluble with sulfate EXCEPT
rate gas A/rate gas B = square root (mm A/ mm B)
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Covalently w/in themselves - Ionicly bonded w/ each other
T-shape
16. A device used to measure Delta H
not spontaneous
Law of Definite Proportion
Calorimeter
lambda
17. Oxidation # of Oxygen
square pyramidal
trigonal bipyramidal
-one
-2 - with peroxide -1
18. Effusion of a gas is inversely proportional to the square root of the molar mass
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19. A solution that resists a change in its pH
permanent gases
Bond enthalpy
exothermic
Buffered Solution
20. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
1.38x10?²³J/K
Lone Pair
Solubility Product (Ksp)
21. Mass percent
Le Chatelier's Principle
salt bridge
-1
g solute/g solvent x 100
22. A monoatomic cation takes name from...
blue-green
Its element
no precipitate forms
Amphoteric
23. Group 1 metals
Diffusion
Alkali metals
condensation
hept-
24. Gas to liquid
London Dispersion Forces
condensation
Molar Mass of Element/ Total Molar Mass %
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
25. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
hydrolysis
-(P)(Change in V)
flouride
Kinetic Molecular Theory - for ideal gases
26. C=2.9979*10^8 m/s
1 atm = 760 mmHg = 101.3 kPa
not spontaneous
Speed of light
Law of Conservation of Mass
27. Reverse rxn occurs when
% yield
1 atm = 760 mmHg = 101.3 kPa
Q>K
Boltzmann distribution
28. The driving force for a spontaneous is an increase in entropy of the universe
Normality
Entropy (S)
Theoretical yield
Exothermic
29. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
Atomic Mass Unit
different # of neutrons
not spontaneous
London dispersion forces
30. Ester suffix
-oate
Alpha Particles-
Bronsted-Lowry base
linear
31. Organic reaction in which two functional groups come together - resulting in the release of water
titrant buret
red
ammonium
condensation
32. 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)
Amphoteric
supercritical fluid
fusion
Ionic Compounds
33. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
strong bases
Finding Empirical Formulas
Joule
increasing
34. Speed per molecule of gas
Increase Temperature
v3kT/m
Arrhenius base
Chemical Kinetics
35. If heat capacity isn't mentioned - you can assume that q of cal is = ?
double bond
salt bridge
Calorimeter
0
36. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
Atomic Mass Unit
acetate
Work
Colligative properties
37. Loss of electrons - increase in oxidation #
dichromate
t-shape
oxidation
strong acids
38. 101 -325 Pa
N=N.(0.5)^time/time half-life
m (third quantum number)
vapor pressure
1atm=?Pa
39. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Calorimeter
Quantum Model
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
Amino-
40. A weak acid that changes color at or near the equivalence point
First-Order Half Life
Electronegativity
1/2mv²
indicator
41. Equation to find Ea from reaction rate constants at two different temperatures
Q<K
freezing
Isolated System
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
42. Reactant that's completely used up in a chemical reaction
Limiting reactant
Arrhenius Base
Finding Empirical Formulas
spontaneous
43. Instrument used to measure the pressure of atmospheric gas
Integrated Rate Law
Barometer
-(q of H2O + q of cal)
London Dispersion Forces
44. #NAME?
wavelength
base
Amphoteric
E
45. Colors of Reaction when (MnO4 -) --> (Mn2+)
Polar Covalent
chlorate
purple --> pink
Coordination Compound
46. pH=
log[H+]
amine
Open System
Reducing Agent
47. I=moles of particles/moles of solute dissolved
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48. Energy required to break a bond
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
Theoretical yield
Bond Energy
linear
49. These orbitals are spherical
Magnetic Quantum Number (ml)
+1 - except if bonded to Alkali Metal -1
mol Fraction
s orbitals
50. These orbitals are perpendicular
p orbitals
s (fourth quantum number)
d orbitals
bond energy