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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. Gas to liquid
% error
hex-
vaporization
condensation
2. The chemical formed when a base accepts a proton
Volume Metric Flask & Pipet
Bond Energy
conjugate acid
Molecular
3. Amount of heat needed to change a system by 1°C
heat capacity
square pyramidal
Boltzmann distribution
AH
4. Dalton's Law of Partial Pressures (to find partial pressure formula)
P of a =(X of a)(total pressure)
equivalence point
experimental yield
Effusion
5. Boiling point elevation formula
?Tb= kb x molality
Volt
Bond Order
different # of neutrons
6. J/°Cg or J/Kg
Bronsted-Lowry base
Hess's Law
Acids
Specific Heat Capacity
7. Spectrum of light when an electron drops to energy level n=2
deposition
Pauli Exclusion Principle
Balmer Series
-al
8. For significant digits - trailing zeros _____ significant
First-Order Rate Law
are
Trigonal Bipyramidal
yellow
9. When _____ significant digits - round answer to least significant digit
Multiplying
permanent gases
Formal Charge
Surroundings
10. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
Pressure
alkane
complex ions
critical point
11. Substance being dissolved in a solution (lower [ ])
Bond Energy
boiling point
Isolated System
Solute
12. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Molality
First-Order Half Life
5% rule
Magnetic Quantum Number (ml)
13. Substance in which something is dissolved in a solution (higher [ ])
P of a =(X of a)(total pressure)
Solvent
5% rule
endless
14. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
melting
Aufbau Principle
p orbitals
15. Proton acceptors - must have an unshared pair of e?s
Bronsted-Lowry base
rate law
M1V1=M2V2
Volume Metric Flask & Pipet
16. When n=3 ->2 - color=
oxidizing agent
q
red
5% rule
17. Mass percent
square pyramidal
n (first quantum number)
g solute/g solvent x 100
Tetrahedral
18. Solution used in titration
titrant buret
Aufbau Principle
London dispersion forces
single bond
19. H + donor
State Functions
Bronsted-Lowry Acid
linear
purple
20. A monoatomic anion is named by taking...
3rd law of thermodynamics
not spontaneous
Speed of light
Its root and adding -ide
21. Atomic #
alkyne
# protons (atom is defined by this)
State Functions
Closed System
22. Substances w/ critical temperatures below 25°C
sulfite
purple --> pink
period
permanent gases
23. R in ideal gas law
mol Fraction
0.0821 atm L/mol K
p orbitals
heat of vaporization
24. Isotope
permanganate
different # of neutrons
vaporization
Constant Pressure
25. Unusually strong dipole forces found when H is bonded to N - O - or F
Hydrogen bonding
square pyramidal
yellow --> green
Arrhenius base
26. Point at which liquid?gas occurs
increasing
First-Order Rate Law
boiling point
-2 - with peroxide -1
27. A solid or gas that can be formed when 2 or more aqueous reactants come together
Nernst Equation
Molality
N=N.(0.5)^time/time half-life
precipitate
28. Larger molecules which have higher mass and therefore electron density have stronger...
STP
London dispersion forces
Buffered Solution
anode
29. [A]0/2k
8.31J/Kmol
v3kT/m
Delta H or Enthalpy Change
Zero-Order Half Life
30. STP
chlorate
electron affinity
0 degrees C - 1 atm
deposition
31. Force that holds atoms together
Chemical Bonds
Second-Order Half Life
Hybridization
Root Mean Square Velocity
32. IMF that occurs with FON
permanent gases
Hydrogen bonding
Pauli Exclusion Principle
Pressure of H2O must be Subtracted
33. 90°&120° - dsp^3
period
experimental yield
Trigonal Bipyramidal
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
34. 6.022x10^23
mol
reduction
chloride
Quantum Mechanical Model
35. Oxidation # of free elements
Quantum Mechanical Model
catalyst
strong bases
0
36. Substance that - when dissolved - is conductive
H
3/2RT
electrolyte
Q<K
37. Increase Volume
first
methods of increasing rate
triple bond
Increase Temperature
38. Force acting over distance
Work
group
-oic acid
Acid Dissociation Constant
39. NH4¹?
Le Chatelier's Principle
-ic acid
ammonium
AE = q + w
40. The reactant in the reduction reaction that forces the oxidation reaction to occur
sulfide
Oxidizing Agent
Atmospheric Pressure
see-saw
41. Energy needed to vaporize a mole of a liquid
bond energy
Molecular Orbitals (MOs)
titrant buret
?Hvap
42. q cal = ?
CAT
but-
second
iodide
43. Coffee Cup Calorimeter
Constant Pressure
Increase Temperature
Allotrope
Isotopes
44. Osmotic pressure=MRT
Osmotic Pressure
Transition metals
London dispersion forces
1.86°C
45. 101 -325 Pa
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
methods of increasing rate
adiabatic
1atm=?Pa
46. Thickness
bond energy
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Hund's Rule
viscosity
47. Carbon - hydrogen - oxygen compounds
pent-
carbohydrates
Bronsted-Lowry acid
Calorimetry
48. Uses a spontaneous redox rxn to generate electrical energy - consists of 2 half cells
Theoretical yield
Resonance
voltaic cells
n0
49. The driving force for a spontaneous is an increase in entropy of the universe
-al
Entropy (S)
Calorimeter
Force = mass x acceleration
50. Idea Gas Law (actual rules)
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
1atm=?Pa
6.63x10?³4Js
Formal Charge