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. Variable for energy of e- - goes from 1 -2 -3 on up
blue-violet
n (first quantum number)
Acids
London dispersion forces
2. 1.Volume of individual particles can be assumed to be zero 2.The particles are in constant motion - which causes pressure 3.Particles exert no forces on each other 4.The average kinetic energy of the particles is directly affected by temperature(K)
Kinetic Molecular Theory - for ideal gases
Equivalence Point
freezing
yellow
3. Carbon & hydrogen compounds
Coordination Compound
hydrocarbons
Equivalence Point
A Roman numeral
4. Half cell in which reduction occurs
hydroxide
cathode
8.314 J/K mol
nitrite
5. A molecule having a center of positive charge and a center of negative charge
Trigonal Planar
Balmer Series
Dipole Moment
Law of Conservation of Mass
6. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Open System
Integrated Second-Order Rate Law
meth-
Polar Covalent
7. Anions or cations as needed to produce a compound with non net charge
Solvent
Counterions
1atm=?Pa
Constant Pressure
8. Organic reaction in which two functional groups come together - resulting in the release of water
Reducing Agent
condensation
deposition
standard solution
9. Speed of light - C
Nodes
3.0x108m/s
paramagnetic
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
10. Significant Digits of counted things
triple bond
Atomic Mass Unit
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
endless
11. Forward rxn occurs when
Q<K
surroundings
Hess's Law
red
12. Pressure Units/Conversions
Tetrahedral
Second-Order Half Life
Matter
1 atm = 760 mmHg = 101.3 kPa
13. Higher in energy than the atomic orbitals of which it is composed
3rd law of thermodynamics
phosphate
Antibonding Molecular Orbital
iodide
14. Composition Formula
alcohol
Molar Mass of Element/ Total Molar Mass %
oxide
r1/r2
15. Entropy in the universe is always...
C + 273
moles of solute/ L of solution
increasing
Alpha Particles-
16. (organics) three carbons
prop-
Pressure of H2O must be Subtracted
% yield
-ol
17. A solution that resists a change in pH - contains both a weak acid and its conjugate base
t-shape
are not
Buffer
yellow --> green
18. Proton donors
+1 - except if bonded to Alkali Metal -1
1.38x10?²³J/K
Bronsted-Lowry acid
-(P)(Change in V)
19. Molality =
v3RT/M(in kg)
Arrhenius Base
moles solute/kg solvent
Work
20. l=3
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
f
Ag+ - Pb2+ - Hg2+ - Sr2+ - Ca2+ - Ba2+
Bronsted-Lowry base
21. Amount of heat needed to change a system by 1°C
heat capacity
Kinetic Molecular Theory - for ideal gases
octahedral
ionic
22. A monoatomic cation takes name from...
Its element
Kinetic Molecular Theory - for ideal gases
Reducing Agent
Aufbau Principle
23. An equilibrium expression
Solubility Product (Ksp)
Surroundings
voltaic cells
Trigonal Planar
24. Point at which solid?liquid occurs
Molar Heat Capacity
excess reactant
melting point
rate
25. Puts OH? into solution
(moles of products that are gasses) - (moles of reactants that are gasses)
0.0821 atm L/mol K
octahedral
Arrhenius base
26. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
Nernst Equation
soluble
1 atm = 760 mmHg = 101.3 kPa
moles of solute/ L of solution
27. Proton acceptors - must have an unshared pair of e?s
Nodes
Atmospheric Pressure
Strong acid weak base rxn
Bronsted-Lowry base
28. 1/([A]0*k)
Reaction Quotient (Q)
Dipole-dipole forces
d
Second-Order Half Life
29. neutron (symbol)
charge
n0
Decrease Volume and Increase Temperature
spontaneous
30. When n=3 ->2 - color=
red
Molecular Orbitals (MOs)
standard solution
paramagnetic
31. ?Hsoln=?H1+?H2+?H3+...
Hund's Rule
3rd law of thermodynamics
Enthalpy of Solution
condensation
32. Solution used in titration
Formal Charge
Volt
pi=(nRT)/v
titrant buret
33. Everything in the universe that is not defined by you as part of the system
Hydrogen bonding
Formal Charge
Surroundings
-(P)(Change in V)
34. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Theoretical yield
Equilibrium Expression
increasing
Metalliods
35. AX3E2
square planar
T-shape
Atomic Mass Unit
Average KE = 1/2(mass)(average speed of all particles)
36. 760mmHg/Torr
Amount of atoms present
STP
Law of Multiple Proportions
1atm=?mmHg/Torr
37. Mols A/ total mols - XA
mol Fraction
1.38x10?²³J/K
base and hydrogen gas
moles solute/kg solvent
38. Involves quantum numbers
Acid + Base --> Salt + Water
chromate
Quantum Mechanical Model
are
39. AX3E
Formal Charge
trigonal pyramidal
nitrite
d orbitals
40. Mass #
First-Order Rate Law
ether
Barometer
# protons + # neutrons
41. AX6
but-
octahedral
alcohol
C=(mass)(specific heat)
42. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
Bases
base and hydrogen gas
strong acids
end point
43. Pairs of electrons localized on an atom
alkyne
Lone Pair
paramagnetic
voltaic cells
44. Change that occurs at constant temperature
dec-
Arrhenius Acid
single bond
isothermal
45. Electron (symbol)
Constant Pressure
e-
eth-
d orbitals
46. Temperature-pressure combination at which solid - liquid - and gas states appear
Limiting reactant
moles of solute/ L of solution
AE= AH - RTAn
triple point
47. Aldehyde suffix
Amount of atoms present
-al
q/moles
s (fourth quantum number)
48. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
Closed System
Bond Order
msAT
49. r=k[A]^2
1.38x10?²³J/K
sublimation
Second-Order Rate Law
AE = q + w
50. Gas to solid
deposition
Thermochemistry
supercritical fluid
Gamma Ray-