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. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
zero
group
yellow --> green
f
2. 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
Bond enthalpy
P1V1/N1T1=P2V2/N2T2
supercritical fluid
Equilibrium Expression
3. Two molecules with identical connectivity but different geometries
geometric isomers
meth-
Cell Potential (Ecell)
are
4. Weakest IMFs - found in all molecules
London dispersion forces
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
T-shape
Alkali metals
5. All cations are soluble with sulfate EXCEPT
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
adhesion
isothermal
0 degrees C - 1 atm
6. (organics) triple-bonded compound
electron affinity
methoxy-
alkyne
experimental yield
7. Dalton's Law of Partial Pressures (to find partial pressure formula)
Oxidation is Loss Reduction is Gain
Limiting reactant
P of a =(X of a)(total pressure)
Matter
8. Mixing of gases
Diffusion
n0
Molecular Compounds
1atm=?Pa
9. r=k[A]
iodide
soluble
First-Order Rate Law
Principal Quantum Number
10. 109.5° - sp^3
s orbitals
Tetrahedral
Force = mass x acceleration
Molecular
11. Color of Ca (flame test)
wavelength
carbohydrates
red/orange
no precipitate forms
12. Cation first - anion second
Naming Binary Ionic Compounds
work
Second-Order Rate Law
Molar Mass of Element/ Total Molar Mass %
13. Change in Energy = ? (in terms of constant pressure; for gasses)
AE= AH - RTAn
Formal Charge
Specific Heat Capacity
alkyne
14. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
heat capacity
Ligand
-al
Amphoteric
15. Type of system in which nothing is transfered (no mass or energy); ideal
Isolated System
Net Ionic Equation
eth-
trigonal pyramidal
16. Faraday's constant
Bronsted-Lowry Base
Acids
Balmer Series
96500
17. How to Find an Empirical Formula Given Grams
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Its root and adding -ide
Ionic Compounds
experimental yield
18. (organics) eight carbons
Molar Heat Capacity
0
oct-
Covalently w/in themselves - Ionicly bonded w/ each other
19. Energy involved in gaining an electron to become a negative ion
H
Multiplying
electron affinity
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
20. Substances w/ critical temperatures below 25°C
oct-
permanent gases
d orbitals
hydro-ic acid
21. Energy required for liquid?gas
heat of vaporization
Limiting reactant
Temperature
heat capacity
22. Molarity (M)
Angular Momentum Quantum Number
Oxidation is Loss Reduction is Gain
moles of solute/ L of solution
Bronsted-Lowry Base
23. 760mmHg/Torr
3rd law of thermodynamics
Integrated Rate Law
1atm=?mmHg/Torr
Equilibrium constant
24. Measure of the average kinetic energy of all the particles in a substance
experimental yield
sulfite
Temperature
Weight
25. Group 2 metals
Alkaline earth metals
C=(mass)(specific heat)
Coordination Compound
methoxy-
26. Chemical composition of dry ice
Limiting reactant
rate gas A/rate gas B = square root (mm A/ mm B)
different # of neutrons
solid CO2
27. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
phosphate
Manometer
second
trigonal planar
28. Kinetic Energy per mol
6.63x10?³4Js
3/2RT
-ol
-ous acid
29. The heat changed in a chemical reaction.
0.0826Latm/Kmol
Thermochemistry
Buffered Solution
Aufbau Principle
30. The chemical formed when a base accepts a proton
precipitate
conjugate acid
indicator
-(P)(Change in V)
31. Force that holds atoms together
Increase Temperature
Pauli Exclusion Principle
Chemical Bonds
Average KE = 1/2(mass)(average speed of all particles)
32. AX5E
square pyramidal
square planar
lambda
Chemical Bonds
33. Everything in the universe that is not defined by you as part of the system
Octahedral
0.0826Latm/Kmol
Surroundings
e-
34. [A]=-kt + [A]0
Calorimeter
Integrated Zero-Order Rate Law
Bond Order
entropy
35. AX2E - AX2E2
Specific Heat Capacity
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
bent
0
36. Has values from 0 to (n-1); tells shape of atomic orbitals
Angular Momentum Quantum Number
supercritical fluid
Solution
like
37. Kinetic Energy of an individual particle formula
M = square root (3RT/mm)
experimental yield
v3RT/M(in kg)
end point
38. (organics) three carbons
insoluble
Aufbau Principle
prop-
s
39. R in instances that pertain to energy
8.314 J/K mol
1st law of thermodynamics
End Point
-2 - with peroxide -1
40. Ptotal=P1+P2+P3+...
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
41. PV=nRT
rate law
Ideal Gas Law
a precipitate forms
Thermochemistry
42. kf of water
purple
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
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
1.86°C
43. Different form of same element
Hund's Rule
allotrope
Solute
linear
44. Point at which vapor pressure=air pressure above
Boltzmann distribution
boiling point
Increase Temperature
AE = q + w
45. Kinetic Energy per molecule
Exothermic
Cg=kPg
Temperature
1/2mv²
46. Planck's constant - used to calculate energy w/frequency
2nd law of thermodynamics
6.63x10?³4Js
Van't Hoff factor
are
47. Substances that form H+ when dissolved in water; proton donors
Le Chatelier's Principle
Acids
titrant buret
Dipole-dipole forces
48. If anion ends in -ite - acid name ends in...
seesaw
-ous acid
deposition
exothermic
49. Force per unit area
Pressure
Electronegativity
d orbitals
square pyramidal
50. AX3
Heat Capacity (C)
conjugate acid
Tetrahedral
trigonal planar