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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. Ideal Gas Law Formula
phosphate
PV=nRT
charge
viscosity
2. Color of K (flame test)
purple
96500
P1V1/N1T1=P2V2/N2T2
Amphoteric
3. A measure of resistance of an object to a change in its state of motion
Law of Conservation of Mass
Molecular
weak acid strong base rxn
Mass
4. A single substance that may be an acid or a base (i.e. water)
Hund's Rule
Colligative properties
Amphoteric
Gamma Ray-
5. 90° - d^2sp^3
v3RT/M(in kg)
Octahedral
non-
Graham's Law
6. Has values 1 -2 -3 -...; tells energy levels
Principal Quantum Number
melting
a precipitate forms
second
7. (organics) seven carbons
hept-
Monoprotic
bromate
Anode
8. 0.00°C - 1 atm
0 degrees C - 1 atm
C=(mass)(specific heat)
e-
Standard Temperature and Pressure
9. Oxidation # of Halogens
acetate
hept-
-1
freezing
10. Molecules' tendency to stick to one another
boiling point
Coordination Compound
non-
cohesion
11. Where oxidation occurs
hept-
period
Anode
Zero-Order Rate Law
12. l=2
Zero-Order Rate Law
oxidation
Its root and adding -ide
d
13. Kinetic Energy of an individual particle formula
g solute/g solvent x 100
M = square root (3RT/mm)
Octahedral
force x distance = work done
14. Actual Yield/Theoretical Yield*100%
Lone Pair
5% rule
Entropy (S)
Percent Yield
15. 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
Amphoteric
deposition
Equilibrium Expression
16. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Valence Electrons(assigned)
k=Ae^(-Ea/RT)
Polar Covalent
end point
17. The total entropy is always increasing - all systems tend towards maximum entropy
Its root and adding -ide
2nd law of thermodynamics
Integrated Second-Order Rate Law
activated complex (transition state)
18. The chemical formed when a base accepts a proton
Heat
ammonium
0.512°C
conjugate acid
19. When n=5 ->2 - color=
blue-violet
hydro-ic acid
titrant buret
96500
20. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Hydrogen bonding
Pressure of H2O must be Subtracted
moles of solute/ L of solution
21. (organics) triple-bonded compound
Law of Multiple Proportions
alkyne
Ligand
actual yield/theoretical yield x 100%
22. A weak acid that changes color at or near the equivalence point
indicator
Ligand
London dispersion forces
Net Ionic Equation
23. C2H3O2¹?
nu
acetate
1.38x10?²³J/K
equivalence point
24. K
double bond
alkene
Equilibrium constant
Specific Heat (s)
25. (organics) two carbons
Anion
3/2RT
Specific Heat Capacity
eth-
26. Variable for type of orbital
allotrope
l (second quantum number)
m (third quantum number)
Net Ionic Equation
27. Donates a single H+ Ion (... other prefixes also)
Dalton's Law of Partial Pressures
System
oxidizing agent
Monoprotic
28. Force per unit area
Linear
Radioactivity
A Roman numeral
Pressure
29. Boltzmann constant - used in calculating speed of gas per molecule
entropy (S)
Octahedral
Cation
1.38x10?²³J/K
30. Organic w/ -NH2
Ionic Compounds
amine
square planar
fusion
31. The actual amount of product produced in an experiment
Integrated Second-Order Rate Law
Osmotic Pressure
deposition
experimental yield
32. 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)
T-shape
Integrated Second-Order Rate Law
Calorimeter
Kinetic Molecular Theory - for ideal gases
33. Positive ion
0
Cation
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Calorimetry
34. Solution used in titration
s (fourth quantum number)
titrant buret
Transition metals
n0
35. Puts OH? into solution
Integrated Rate Law
Arrhenius base
Valence Electrons(assigned)
chloride
36. Organic w/ -OH group
# protons (atom is defined by this)
alcohol
?Tf= kf x molality
Open System
37. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Dipole-dipole forces
Resonance
moles of solute/ L of solution
1 atm = 760 mmHg = 101.3 kPa
38. Heat required to raise the system 1°C
Second-Order Rate Law
Reducing Agent
Osmotic Pressure
heat capacity
39. q H2O = ?
see-saw
Effusion
-ol
msAT
40. Oxidation # of Oxygen
1atm=?mmHg/Torr
22.4L
q/moles
-2 - with peroxide -1
41. Mol of solute/kg of solvent
seesaw
Molality
-(q of H2O + q of cal)
Scientific Method
42. Electron pairs found in the space between the atoms
-ic acid
trigonal bipyramidal
LeChatelier's Principle
Bonding Pairs
43. Metal oxide + H20 ->
alkyne
yellow
base
f
44. Amount of gravitational force exerted on an object
Weight
0.0821 atm L/mol K
like
trigonal pyramidal
45. l=3
f
endless
pent-
perchlorate
46. These orbitals are spherical
meth-
s orbitals
geometric isomers
Pi Bond
47. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
London dispersion forces
Molal FP Depression Constant
0.512°C
48. The driving force for a spontaneous is an increase in entropy of the universe
blue-violet
Entropy (S)
Sigma Bond
Constant Volume
49. Speed of Diffusion/Effusion formula
Dipole-dipole forces
2nd law of thermodynamics
rate gas A/rate gas B = square root (mm A/ mm B)
third
50. A solution that resists a change in pH - contains both a weak acid and its conjugate base
Equivalence Point
Buffer
equivalence point
single bond