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. Proton (symbol)
vaporization
square planar
moles of solute/ L of solution
p+
2. 109.5° - sp^3
London dispersion forces
Tetrahedral
System
Cell Potential (Ecell)
3. Unusually strong dipole forces found when H is bonded to N - O - or F
Hydrogen bonding
Its element
d orbitals
base and hydrogen gas
4. Electrons in a hydrogen atom move around the nucleus only in circular orbits
Quantum Model
Exothermic
carbohydrates
insoluble
5. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
complex ions
conjugate base
N=N.(0.5)^time/time half-life
strong bases
6. l=1
Pressure of H2O must be Subtracted
square planar
p
salt bridge
7. Force acting over distance
Constant Pressure
Entropy (S)
Work
log[H+]
8. Ptotal=Pa+Pb+Pc....
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
9. Speed of Diffusion/Effusion formula
% yield
rate gas A/rate gas B = square root (mm A/ mm B)
not spontaneous
+1 - except if bonded to Alkali Metal -1
10. Equation to find Ea from reaction rate constants at two different temperatures
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
endothermic
triple bond
sublimation
11. When ____ significant digits - round answer to least decimal place
trigonal bipyramidal
Adding
-oic acid
0
12. A monoatomic anion is named by taking...
square planar
+1 - except if bonded to Alkali Metal -1
AH
Its root and adding -ide
13. O²?
oxide
Pauli Exclusion Principle
AE = q + w
condensation
14. AX5
Chemical Bonds
p+
trigonal bipyramidal
different # of neutrons
15. Force per unit area
Molal FP Depression Constant
Exothermic
Volume Metric Flask & Pipet
Pressure
16. n+m (these are orders of reactants)
purple
Cathode
3/2RT
Overall Reaction Order
17. Henry's Law - solubility of gases is directly proportional to the partial pressure of the gas
Cg=kPg
5% rule
Antibonding Molecular Orbital
single bond
18. If anion ends in -ide - acid name ends in
Negative work value; work done by system
trigonal pyramidal
Pi Bond
hydro-ic acid
19. Color of Sr (flame test)
Octahedral
activated complex (transition state)
red
Theoretical yield
20. Average speed of gas
Pressure
v3RT/M(in kg)
Linear
Hydrogen bonding
21. H + donor
Bronsted-Lowry Acid
k=Ae^(-Ea/RT)
dec-
Hess's Law
22. AP doesn't deal with ...-order reaction - don't pick it!
+1 - except if bonded to Alkali Metal -1
r1/r2
Alkaline earth metals
third
23. Half cell in which oxidation occurs
8.314 J/K mol
anode
moles solute/kg solvent
base
24. Group 2 metals
chloride
Alkaline earth metals
hydrocarbons
g solute/g solvent x 100
25. R=
+1 - except if bonded to Alkali Metal -1
8.31J/Kmol
alcohol
Diffusion
26. The reactant in the oxidizing reaction that forces the reduction reaction to occur
entropy (S)
Integrated Second-Order Rate Law
Arrhenius equation
Reducing Agent
27. OH¹?
hydroxide
2nd law of thermodynamics
k=Ae^(-Ea/RT)
blue-green
28. Electron pairs found in the space between the atoms
Entropy (S)
methoxy-
Bonding Pairs
P1V1/N1T1=P2V2/N2T2
29. Change in Energy (AE) = ? (in terms of work)
experimental yield
AE = q + w
Valence Electrons(assigned)
strong bases
30. BrO3¹?
Amino-
oxide
bromate
experimental yield
31. Atoms with the same number of protons but a different number of neutrons
H
Covalently w/in themselves - Ionicly bonded w/ each other
Balmer Series
Isotopes
32. All _________ compounds are electrolytes
Allotrope
sulfide
Ionic
nitrate
33. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
alkene
Manometer
0.0826Latm/Kmol
strong acids
34. Mass percent
equilibrium
g solute/g solvent x 100
Acid + Base --> Salt + Water
Cathode
35. Ionizes to produce OH- Ions
Weight
spontaneity
Arrhenius Base
moles solute/kg solvent
36. All cations are soluble with bromide - chloride and iodide EXCEPT
Hydrogen bonding
nitrite
Ag+ - Pb2+ - Hg2+
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
37. Carboxylic acid ending
Linear
-oic acid
Enthalpy of Solution
% error
38. The total entropy is always increasing - all systems tend towards maximum entropy
2nd law of thermodynamics
see-saw
strong acid strong base rxn
Zero-Order Half Life
39. In a given atom no two electrons can have the same set of four quantum numbers
Force = mass x acceleration
oct-
nitrite
Pauli Exclusion Principle
40. Color of K (flame test)
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Molarity
melting
purple
41. Positive ion
Bronsted-Lowry Base
perchlorate
Cation
System
42. Mol/kg of solvent - used in calculating colligative properties
Integrated First-Order Rate Law
Hund's Rule
Molality
effects of IMF
43. CO3²?
LE Model
Alkaline earth metals
r1/r2
carbonate
44. Spectrum of light when an electron drops to energy level n=2
Balmer Series
Law of Definite Proportion
T-shape
entropy
45. Change that occurs at constant temperature
AE = q + w
isothermal
a precipitate forms
0
46. Color of Ca (flame test)
red/orange
1atm=?mmHg/Torr
Weight
perchlorate
47. Larger molecules which have higher mass and therefore electron density have stronger...
A Roman numeral
mol
London dispersion forces
fusion
48. Raising heat - adding catalyst - heighten concentration - bigger surface area
methods of increasing rate
are
isothermal
1atm=?Pa
49. The chemical formed when a base accepts a proton
Adding
conjugate acid
Cathode
conjugate base
50. ?H when 1 mol of bonds is broken in the gaseous state
Bond enthalpy
A Roman numeral
third
Pauli Exclusion Principle