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. Absorbs/takes in heat (positive value)
nu
Pi Bond
red
Endothermic
2. If a system @equilibrium is stressed - the system will shift so as to reestablish equilibrium
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
3. J/°Cmol or J/Kmol
Molar Heat Capacity
Molal FP Depression Constant
?Tf= kf x molality
spontaneous
4. OH¹?
standard solution
reduction
Arrhenius Acid
hydroxide
5. (organics) nine carbons
non-
purple --> pink
third
Law of Conservation of Energy
6. (organics) three carbons
prop-
Molecular
Quantum Mechanical Model
Its element
7. Cation first - anion second
0
Naming Binary Ionic Compounds
Alpha Particles-
sulfite
8. 0°C and 1 atm
Solubility Product (Ksp)
STP
yellow
deposition
9. Ability of an atom in a molecule to attract shared electrons to itself
Electronegativity
mol
d
activated complex (transition state)
10. Liquid to solid
rate law
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
actual yield/theoretical yield x 100%
freezing
11. Pure metal or metal hydride + H20 ->
k=Ae^(-Ea/RT)
strong bases
base and hydrogen gas
Molal FP Depression Constant
12. A measure of resistance of an object to a change in its state of motion
permanent gases
Mass
London dispersion forces
Trigonal Planar
13. PV=nRT
(moles of products that are gasses) - (moles of reactants that are gasses)
red
Ideal Gas Law
Octahedral
14. ?Hsoln=?H1+?H2+?H3+...
Enthalpy of Solution
Zero-Order Rate Law
Boltzmann distribution
spontaneity
15. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
8.314 J/K mol
Endothermic
Ligand
Kinetic Molecular Theory - for ideal gases
16. Phase change from gas to solid
Trigonal Planar
Principal Quantum Number
deposition
0
17. If Q>Ksp
-2 - with peroxide -1
a precipitate forms
Gamma Ray-
Amphoteric
18. 180° - sp
Linear
are
alkane
Molar Heat Capacity
19. Measure of the average kinetic energy of all the particles in a substance
Molecular Orbitals (MOs)
Calorimetry
Temperature
entropy (S)
20. Positive enthalpy - heat flows into system
Strong acid weak base rxn
endothermic
-one
Ionic Compounds
21. If heat capacity isn't mentioned - you can assume that q of cal is = ?
Quantum Model
Equilibrium Expression
deposition
0
22. Reactant which doesn't get used up completely in a chemical reaction
excess reactant
Counterions
Amino-
1.38x10?²³J/K
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)
adhesion
perchlorate
Ionic Compounds
equilibrium
24. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
dec-
Polar Covalent
q
M1V1=M2V2
25. ClO4¹?
Valence Electrons(assigned)
hydrolysis
perchlorate
green/yellow
26. neutron (symbol)
trigonal bipyramidal
n0
t-shape
Anode
27. R=
0 degrees C - 1 atm
+1 - except if bonded to Alkali Metal -1
ether
8.31J/Kmol
28. Dalton's Law of Partial Pressures (to find partial pressure formula)
+1 - except if bonded to Alkali Metal -1
Equilibrium constant
P of a =(X of a)(total pressure)
permanganate
29. 1/([A]0*k)
Gamma Ray-
Second-Order Half Life
A Roman numeral
Delta H or Enthalpy Change
30. Oxidation # of Halogens
Angular Momentum Quantum Number
-1
chlorate
Nernst Equation
31. What is defined by you taken from the whole universe
Bond Order
System
0.0821 atm L/mol K
?Tb= kb x molality
32. Temperature-pressure point after which gas can no longer form liquid
Anion
A Roman numeral
square planar
critical point
33. Increase Pressure
Hydrogen bonding
Decrease Volume and Increase Temperature
Constant Pressure
Positive work value; work done on system
34. Speed per molecule of gas
0
trigonal planar
adiabatic
v3kT/m
35. Half cell in which reduction occurs
red/orange
Enthalpy of Solution
cathode
purple --> pink
36. (msubs) Can only be +1/2 or -1/2
actual yield/theoretical yield x 100%
green/yellow
Constant Volume
Electron Spin Quantum Number
37. Mixing of gases
Diffusion
s
Limiting reactant
Standard Temperature and Pressure
38. When _____ significant digits - round answer to least significant digit
permanent gases
methoxy-
Multiplying
Chemical Bonds
39. Rate of Diffusion/Effusion formula
Buffered Solution
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
Arrhenius acid
oxidizing agent
40. l=0
C=(mass)(specific heat)
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
s
0
41. Energy required to break a bond
Coordination Compound
alkene
complex ions
Bond Energy
42. Force acting over distance
end point
triple bond
Bronsted-Lowry Acid
Work
43. 760 mmHg - 760 torr
excess reactant
1 atm
Integrated Second-Order Rate Law
surroundings
44. The total energy of the universe is constant - all systems tend towards minimum energy
wavelength
1st law of thermodynamics
% error
red/orange
45. These orbitals are perpendicular
First-Order Half Life
Law of Conservation of Mass
Antibonding Molecular Orbital
p orbitals
46. CrO4²?
trigonal bipyramidal
2nd law of thermodynamics
chromate
1atm=?Pa
47. Force per unit area
1atm=?Pa
Pressure
third
?Hvap
48. HF+ OH??H2O
Heisenberg Uncertainty Principle
weak acid strong base rxn
r1/r2
Solution
49. When n=4 ->2 - color=
blue-green
force x distance = work done
Arrhenius Acid
blue-violet
50. Neutralization Reaction (general format) (net ionic of which is always (H+) + (OH-) --> (H2O))
Acid + Base --> Salt + Water
M = square root (3RT/mm)
Ideal Gas Law
3.0x108m/s