SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. Volume of gas @STP
analyte
ether
22.4L
-al
2. Positive enthalpy - heat flows into system
allotrope
Allotrope
endothermic
Hund's Rule
3. Mols A/ total mols - XA
heat capacity
Arrhenius equation
g solute/g solvent x 100
mol Fraction
4. The mixing of native atomic orbitals to form special orbitals for bonding
Hybridization
meth-
Pressure of H2O must be Subtracted
Pauli Exclusion Principle
5. Substances that form OH- when dissolved in water; proton acceptors
Bases
Molality
trigonal pyramidal
oxide gas and water
6. Dirrect Method Formula
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Positive work value; work done on system
E
rate gas A/rate gas B = square root (mm A/ mm B)
7. Does the same as equilibrium expression - except it uses initial concentrations
Reaction Quotient (Q)
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Ampere
Percent Yield
8. The driving force for a spontaneous is an increase in entropy of the universe
vapor pressure
Entropy (S)
spontaneity
Isotopes
9. Where oxidation occurs
voltaic cells
vapor pressure
Octahedral
Anode
10. Substance in which something is dissolved in a solution (higher [ ])
Arrhenius Base
Dalton's Law of Partial Pressures
purple --> pink
Solvent
11. C2H3O2¹?
3rd law of thermodynamics
n0
acetate
yellow --> green
12. Phase change from gas to solid
Equilibrium constant
supercritical fluid
Kinetic Molecular Theory - for ideal gases
deposition
13. Freezing point depression formula
strong acid strong base rxn
?Tf= kf x molality
Finding Empirical Formulas
H
14. Kinetic Energy per mol
3/2RT
Open System
Pi Bond
critical point
15. Temperature-pressure point after which gas can no longer form liquid
methoxy-
Cell Potential (Ecell)
Arrhenius equation
critical point
16. Arrhenius equation
STP
allotrope
k=Ae^(-Ea/RT)
endothermic
17. S²?
standard solution
effects of IMF
sulfide
P of a =(X of a)(total pressure)
18. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
permanent gases
nu
supercritical fluid
sulfite
19. An element with several different forms - each with different properties (i.e. graphite & diamond)
Increase Temperature
melting
Isotopes
Allotrope
20. Larger molecules which have higher mass and therefore electron density have stronger...
Dipole-dipole forces
London dispersion forces
# protons (atom is defined by this)
Alpha Particles-
21. The reactant that is being oxidized - brings about reduction
Alkali metals
p
3/2RT
reduction agent
22. AX5E
square pyramidal
Amount of atoms present
X of a = moles a/total moles
State Functions
23. 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)
PV=nRT
Ionic Compounds
Chemical Kinetics
like
24. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
1.86°C
-1
Calorimeter
complex ions
25. Different form of same element
e-
Theoretical yield
allotrope
ammonium
26. These orbitals are diagonal
Temperature
alcohol
supercritical fluid
d orbitals
27. Isotope
different # of neutrons
fusion
Arrhenius Base
Transition metals
28. Color of Ba (flame test)
pi=(nRT)/v
London Dispersion Forces
green/yellow
Standard Temperature and Pressure
29. C=2.9979*10^8 m/s
Closed System
Bond Order
Speed of light
n0
30. AX5
trigonal bipyramidal
seesaw
experimental yield
Molar Mass of Element/ Total Molar Mass %
31. Similar to atomic orbitals - except between molecules
Molecular Orbitals (MOs)
Graham's Law
Coordination Compound
allotrope
32. Molarity (M)
moles of solute/ L of solution
hydro-ic acid
1/2mv²
Specific Heat Capacity
33. Amine prefix
pent-
Amino-
# protons (atom is defined by this)
Angular Momentum Quantum Number
34. Kinetic Energy is proportional to ______
f
Temperature
Molality
-ol
35. AX4E
seesaw
Solubility Product (Ksp)
analyte
second
36. As protons are added to the nucleus - electrons are similarly added
Aufbau Principle
% yield
boiling point
v3RT/M(in kg)
37. The chemical formed when an acid donates a proton
equilibrium
Reducing Agent
8.31J/Kmol
conjugate base
38. In a titration - the point where moles of acid are equal to moles of base (just before the indicator changes color)
trigonal planar
Overall Reaction Order
Closed System
Equivalence Point
39. Substance being dissolved in a solution (lower [ ])
Solute
chlorate
work
Molarity
40. ?Hsoln=?H1+?H2+?H3+...
Work
E
trigonal bipyramidal
Enthalpy of Solution
41. Measure of the average kinetic energy of all the particles in a substance
Net Ionic Equation
Temperature
equilibrium
electron affinity
42. I=moles of particles/moles of solute dissolved
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
43. Colors of Reaction when (MnO4 -) --> (Mn2+)
Reducing Agent
E
purple --> pink
Trigonal Planar
44. NH4¹?
Root Mean Square Velocity
ammonium
ether
Equilibrium Expression
45. If Q>Ksp
reduction
22.4L
a precipitate forms
London dispersion forces
46. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
hydrolysis
bent
Weight
phosphate
47. Kinetic Energy of an individual particle formula
Aufbau Principle
State Functions
see-saw
M = square root (3RT/mm)
48. A solution that resists a change in pH - contains both a weak acid and its conjugate base
deposition
Effusion
Buffer
Transition metals
49. Ending for alcohols
Hund's Rule
titrant buret
geometric isomers
-ol
50. Expresses how the concentrations depend on time
Integrated Rate Law
-1
second
specific heat