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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. Color of Na (flame test)
Surroundings
yellow
Finding Empirical Formulas
C + 273
2. Negative enthalpy - heat flows into surroundings
oxide gas and water
exothermic
Bronsted-Lowry Acid
activation energy
3. ln[A]=-kt + ln[A]0
Its root and adding -ide
Integrated First-Order Rate Law
heat of vaporization
ether
4. Electron (symbol)
London dispersion forces
Resonance
Quantum Model
e-
5. Peak of energy diagram
Sigma Bond
0
Open System
activated complex (transition state)
6. C2O4²?
v3kT/m
endothermic
oxalate
Molal BP Elevation Constant
7. Stronger IMF= lower... weaker IMF= higher...
indicator
trigonal planar
vapor pressure
Pi Bond
8. AX2 - AX2E3
Its element
linear
spontaneity
chlorite
9. BrO3¹?
Nodes
bromate
% error
period
10. Kinetic Energy per molecule
Bond Order
1/2mv²
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
diamagnetic
11. ?T=k*m(solute)
Molal BP Elevation Constant
solid CO2
6.63x10?³4Js
Law of Multiple Proportions
12. Color of Cs (flame test)
-one
alkene
blue
n0
13. Substances that form H+ when dissolved in water; proton donors
r1/r2
k=Ae^(-Ea/RT)
Trigonal Bipyramidal
Acids
14. Point at which liquid?gas occurs
Molecular Compounds
boiling point
Pauli Exclusion Principle
different # of neutrons
15. Temperature-pressure combination at which solid - liquid - and gas states appear
Pauli Exclusion Principle
triple point
msAT
Solvent
16. Organic reaction in which two functional groups come together - resulting in the release of water
Molal BP Elevation Constant
precipitate
condensation
Aufbau Principle
17. Horizontals on the periodic table
Calorimetry
period
l (second quantum number)
geometric isomers
18. % yield
Covalently w/in themselves - Ionicly bonded w/ each other
rate gas A/rate gas B = square root (mm A/ mm B)
actual yield/theoretical yield x 100%
A Roman numeral
19. PV=nRT
Overall Reaction Order
Molecular Orbitals (MOs)
Ideal Gas Law
Pressure
20. 180° - sp
3rd law of thermodynamics
Linear
Bronsted-Lowry Acid
Its root and adding -ide
21. Amount of gravitational force exerted on an object
Weight
Adding
square pyramidal
violet
22. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
Kinetic Molecular Theory - for ideal gases
heat capacity
are not
square planar
23. # bonding e- - # antibonding e-/2
Bond Order
Magnetic Quantum Number (ml)
H
viscosity
24. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
hept-
A Roman numeral
Density
Polar Covalent
25. [A]0/2k
Zero-Order Half Life
Allotrope
Reaction Quotient (Q)
square pyramidal
26. Reactant that's completely used up in a chemical reaction
weak acid strong base rxn
Increase Temperature
Limiting reactant
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
27. (organics) six carbons
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
hex-
Electron Spin Quantum Number
like
28. HF+ OH??H2O
?Tb= kb x molality
Balmer Series
weak acid strong base rxn
Force = mass x acceleration
29. Oxidation # of free elements
p+
Naming Binary Ionic Compounds
0
alcohol
30. All cations are soluble with bromide - chloride and iodide EXCEPT
Law of Conservation of Mass
Theoretical yield
Ag+ - Pb2+ - Hg2+
anode
31. l=0
sublimation
s
pent-
anode
32. Substance that - when dissolved - is conductive
Naming Binary Ionic Compounds
Work
rate
electrolyte
33. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
strong acids
electron affinity
Ideal Gas Law
zero
34. Average speed of gas
v3RT/M(in kg)
Theory of Relativity
Molecular Compounds
anode
35. In covalent bonds - prefixes are used to tell...
Amount of atoms present
methods of increasing rate
Lone Pair
dec-
36. C2H3O2¹?
Formal Charge
Amphoteric
acetate
3rd law of thermodynamics
37. Colors of Reaction when (MnO4 -) --> (Mn2+)
cohesion
Integrated Zero-Order Rate Law
blue
purple --> pink
38. If anion ends in -ite - acid name ends in...
Surroundings
-ous acid
force x distance = work done
insoluble
39. When n=3 ->2 - color=
supercritical fluid
blue
entropy (S)
red
40. Higher in energy than the atomic orbitals of which it is composed
Antibonding Molecular Orbital
linear
Mass
nitrite
41. Expresses how the concentrations depend on time
96500
van't Hoff Factor
Integrated Rate Law
Chemical Kinetics
42. Nonmetal oxide + H2O ->
acid
Endothermic
hydrolysis
heat capacity
43. (A) - C/s
endothermic
AE = q + w
Ampere
melting point
44. Substance being dissolved in a solution (lower [ ])
sulfide
Joule
Solute
0.0826Latm/Kmol
45. NO2¹?
hydro-ic acid
bond energy
Nodes
nitrite
46. AX6
0.0826Latm/Kmol
octahedral
v3RT/M(in kg)
red
47. Only contains ions that change in reaction
Net Ionic Equation
charge
Equilibrium constant
pi=(nRT)/v
48. R=
# protons (atom is defined by this)
8.31J/Kmol
Buffered Solution
Hybridization
49. pH=
log[H+]
Second-Order Half Life
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
geometric isomers
50. Phase change from solid to gas
Molal BP Elevation Constant
Solvent
sublimation
alkane