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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. AX4E
permanganate
paramagnetic
seesaw
Surroundings
2. Energy required for melting to occur
Gamma Ray-
1st law of thermodynamics
perchlorate
heat of fusion
3. What is defined by you taken from the whole universe
experimental yield
Aufbau Principle
System
spontaneity
4. Energy involved in gaining an electron to become a negative ion
electron affinity
e-
activation energy
Molecular
5. Energy needed to vaporize a mole of a liquid
?Hvap
Tetrahedral
s (fourth quantum number)
charge
6. When gas expands ...
prop-
Principal Quantum Number
sublimation
Negative work value; work done by system
7. ?H when 1 mol of bonds is broken in the gaseous state
Dalton's Law
Aufbau Principle
purple
Bond enthalpy
8. All forms of energy except for heat
work
Closed System
AE= AH - RTAn
Lone Pair
9. These orbitals are perpendicular
red
not spontaneous
p orbitals
2nd law of thermodynamics
10. Planck's constant - used to calculate energy w/frequency
geometric isomers
6.63x10?³4Js
Solute
hept-
11. (organics) six carbons
hex-
alkane
Hund's Rule
Volume Metric Flask & Pipet
12. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
d
Barometer
soluble
Isotopes
13. The reactant that is being oxidized - brings about reduction
Finding Empirical Formulas
reduction agent
viscosity
geometric isomers
14. Carbonates - Hydroxides - Oxides - Phosphates - Sulfides
Bronsted-Lowry base
q/moles
s orbitals
insoluble
15. CrO4²?
rate
Bases
chromate
supercritical fluid
16. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
phosphate - sulfide - carbonate - sulfate
voltaic cells
Polar Covalent
Allotrope
17. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
Chemical Kinetics
Arrhenius acid
State Functions
Delta H or Enthalpy Change
18. Mol/kg of solvent - used in calculating colligative properties
Theory of Relativity
0 degrees C - 1 atm
Finding Empirical Formulas
Molality
19. Substances w/ critical temperatures below 25°C
permanent gases
salt bridge
-ous acid
Net Ionic Equation
20. R in ideal gas law
Magnetic Quantum Number (ml)
see-saw
0.0821 atm L/mol K
analyte
21. Speed per molecule of gas
hydroxide
LE Model
v3kT/m
allotrope
22. Ending for alcohols
C=(mass)(specific heat)
-ol
Specific Heat (s)
acid
23. Ecell= E°cell -RT/nF x lnQ
octahedral
Ag+ - Pb2+ - Hg2+
LeChatelier's Principle
Nernst Equation
24. Where there are no electrons
Nodes
p+
seesaw
condensation
25. Proton donors
m (third quantum number)
Bond Energy
Bronsted-Lowry acid
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
26. Type of system in which nothing is transfered (no mass or energy); ideal
Isolated System
Quantum Model
methoxy-
Bond Order
27. =vM2/M1
permanganate
Hydrogen bonding
r1/r2
msAT
28. Atoms with the same number of protons but a different number of neutrons
oct-
?Tf= kf x molality
Isotopes
Molecular Compounds
29. Mixing of gases
Oxidizing Agent
Multiplying
Diffusion
-ic acid
30. Work = ?
Hund's Rule
isothermal
Ampere
-(P)(Change in V)
31. Amine prefix
melting
Weight
Amino-
n (first quantum number)
32. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
strong acid strong base rxn
hydro-ic acid
Boltzmann distribution
Pauli Exclusion Principle
33. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
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183
34. Experimental yield/theoretical yieldx100
% yield
single bond
different # of neutrons
Antibonding Molecular Orbital
35. ?T=k*m(solute)
Standard Temperature and Pressure
dec-
8.31J/Kmol
Molal BP Elevation Constant
36. 109.5° - sp^3
viscosity
Pauli Exclusion Principle
Tetrahedral
dec-
37. Spectrum of light when an electron drops to energy level n=2
-(P)(Change in V)
Hess's Law
Dipole-dipole forces
Balmer Series
38. ... compounds are most conductive
ionic
no precipitate forms
1.38x10?²³J/K
geometric isomers
39. Idea Gas Law (actual rules)
Counterions
-ol
Valence Electrons(assigned)
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
40. The driving force for a spontaneous is an increase in entropy of the universe
end point
Entropy (S)
increasing
0.512°C
41. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
P of a =(X of a)(total pressure)
voltaic cells
Cation
standard solution
42. When n=3 ->2 - color=
Molecular Compounds
red
blue
ionic
43. Substances that form H+ when dissolved in water; proton donors
complex ions
Molality
Acids
Bronsted-Lowry acid
44. Positive enthalpy - heat flows into system
system
Decrease Volume and Increase Temperature
P1= X1P1°
endothermic
45. [A]0/2k
triple point
-oate
Zero-Order Half Life
conjugate base
46. In a given atom no two electrons can have the same set of four quantum numbers
Pauli Exclusion Principle
Bond Energy
titrant buret
mol
47. Force acting over distance
chromate
Alkali metals
End Point
Work
48. Increase Volume
Atmospheric Pressure
red
Increase Temperature
Equilibrium Expression
49. The energy required to raise 1 g of substance 1 degree C
-one
Specific Heat (s)
Isolated System
Acids
50. 1 sigma bond - 1 pi bond
Molecular
Entropy (S)
double bond
Exothermic