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. Amount of product produced when limiting reactant is used up
permanganate
flouride
Theoretical yield
nitrite
2. Unusually strong dipole forces found when H is bonded to N - O - or F
T-shape
Hydrogen bonding
Electron Spin Quantum Number
prop-
3. ClO4¹?
Antibonding Molecular Orbital
X of a = moles a/total moles
Solution
perchlorate
4. Energy required for liquid?gas
Law of Conservation of Mass
heat of vaporization
seesaw
Strong acid weak base rxn
5. PO4³?
octahedral
Oxidizing Agent
phosphate
weak acid strong base rxn
6. These orbitals are perpendicular
bromate
Constant Pressure
p orbitals
alkyne
7. Negative enthalpy - heat flows into surroundings
Pauli Exclusion Principle
pi=(nRT)/v
System
exothermic
8. Specific heat of water
4.184
Counterions
f
Scientific Method
9. Heat required to raise the system 1°C
heat capacity
freezing
sulfide
boiling point
10. Delta H (AH) = ?
CAT
catalyst
Law of Multiple Proportions
q/moles
11. I¹?
iodide
Cg=kPg
0
voltaic cells
12. Consists of a complex ion - a transition metal with attached ligands - and counterions
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
adhesion
Pressure of H2O must be Subtracted
Coordination Compound
13. ?H when 1 mol of bonds is broken in the gaseous state
v3kT/m
cyanide
Exothermic
Bond enthalpy
14. (organics) one carbon
meth-
Bronsted-Lowry Acid
endless
Heisenberg Uncertainty Principle
15. For significant digits - leading zeros ____ significant
rate
are not
oxide
Multiplying
16. Only contains ions that change in reaction
Magnetic Quantum Number (ml)
Net Ionic Equation
Amount of atoms present
State Functions
17. Ka=[products]^m/[reactants]^n
Acid Dissociation Constant
msAT
n (first quantum number)
triple bond
18. (organics) triple-bonded compound
alkyne
Bond Energy
1 atm = 760 mmHg = 101.3 kPa
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
19. Symbol for Enthalpy
Law of Conservation of Mass
perchlorate
H
E
20. Variable for type of orbital
nitrate
1 atm = 760 mmHg = 101.3 kPa
l (second quantum number)
Molecular Orbitals (MOs)
21. Energy required to break a bond
strong acids
Bond Energy
Arrhenius base
like
22. Theoretical yield-experimental yield/theoretical yieldx100
% error
AH
m (third quantum number)
Pressure of H2O must be Subtracted
23. An element with several different forms - each with different properties (i.e. graphite & diamond)
soluble
Allotrope
Van't Hoff factor
-ous acid
24. Isotope
single bond
Zero-Order Half Life
System
different # of neutrons
25. Organic reaction in which water breaks apart a molecule (splitting into two hydroxides)
are
Second-Order Half Life
tetrahedral
hydrolysis
26. Ecell= E°cell -RT/nF x lnQ
Nernst Equation
Law of Multiple Proportions
0.0821 atm L/mol K
Strong acid weak base rxn
27. Color of Ca (flame test)
red/orange
Specific Heat (s)
acetate
Bond enthalpy
28. Raising heat - adding catalyst - heighten concentration - bigger surface area
green/yellow
methods of increasing rate
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
strong acid strong base rxn
29. Speed of light - C
acetate
C=(mass)(specific heat)
3.0x108m/s
moles of solute/ L of solution
30. The intermolecular attractions resulting from the constant motion of electrons and the creation of instantaneous dipoles
nitrite
London Dispersion Forces
Cg=kPg
Dipole Moment
31. Point where acid completely neutralizes base
equivalence point
Joule
cohesion
Zero-Order Rate Law
32. The total energy of the universe is constant - all systems tend towards minimum energy
conjugate base
n0
1st law of thermodynamics
Manometer
33. # bonding e- - # antibonding e-/2
Increase Temperature
Bond Order
mol Fraction
Hund's Rule
34. (A) - C/s
P1= X1P1°
Transition metals
Ampere
Solution
35. Boiling point elevation formula
?Tb= kb x molality
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Oxidizing Agent
mol
36. AX4E
Reducing Agent
see-saw
Calorimeter
Scientific Method
37. Entropy in the universe is always...
dec-
H
Formal Charge
increasing
38. Increase Pressure
square pyramidal
Decrease Volume and Increase Temperature
hept-
Le Chatelier's Principle
39. Force acting over distance
e-
Work
iodide
C + 273
40. Change in Energy = ? (in terms of constant pressure; for gasses)
lambda
red
Normality
AE= AH - RTAn
41. Expresses how the concentrations depend on time
boiling point
Integrated Rate Law
Barometer
P1V1/N1T1=P2V2/N2T2
42. Significant Digits of counted things
Law of Conservation of Energy
endless
Limiting reactant
Solution
43. Increase Volume
STP
8.314 J/K mol
Increase Temperature
Solvent
44. All forms of energy except for heat
work
green/yellow
oxide
Equilibrium constant
45. All cations are soluble with bromide - chloride and iodide EXCEPT
seesaw
pent-
Ag+ - Pb2+ - Hg2+
acetate
46. ln[A]=-kt + ln[A]0
C + 273
carbonate
Integrated First-Order Rate Law
Arrhenius acid
47. 96 -485 C/mol e-
Faraday
Solvent
Coordination Compound
Finding Empirical Formulas
48. Carboxylic acid ending
# protons (atom is defined by this)
Quantum Numbers
-oic acid
-oate
49. Higher in energy than the atomic orbitals of which it is composed
p orbitals
Pressure
sulfide
Antibonding Molecular Orbital
50. A measure of resistance of an object to a change in its state of motion
Mass
p
Van't Hoff factor
Heat Capacity (C)