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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. 101 -325 Pa
P1= X1P1°
oxide
alkane
1atm=?Pa
2. ln[A]=-kt + ln[A]0
triple point
Electron Spin Quantum Number
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
Integrated First-Order Rate Law
3. U(rms)=(3RT/M)^1/2
methods of increasing rate
CAT
Root Mean Square Velocity
sublimation
4. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
State Functions
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
viscosity
H
5. Nonmetal oxide + H2O ->
Polar Covalent
alkene
acid
Arrhenius Base
6. ... compounds are most conductive
Integrated First-Order Rate Law
adhesion
ionic
# protons (atom is defined by this)
7. O²?
State Functions
Reaction Quotient (Q)
zero
oxide
8. (organics) double-bonded compound
Barometer
single bond
carbonate
alkene
9. Where there are no electrons
Nodes
conjugate acid
surroundings
Equivalence Point
10. Oxoacid solution (such as HSO4-) forms...
nitrate
0.512°C
oxide gas and water
p orbitals
11. n+m (these are orders of reactants)
1atm=?Pa
Net Ionic Equation
Overall Reaction Order
effects of IMF
12. AX3E2
hydrolysis
0
Calorimeter
T-shape
13. Half cell in which oxidation occurs
-al
m (third quantum number)
anode
p
14. Color of Cs (flame test)
5% rule
entropy
see-saw
blue
15. Equation to find Ea from reaction rate constants at two different temperatures
AE = q + w
H
London dispersion forces
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
16. IMF that occurs with FON
# protons + # neutrons
Allotrope
Hydrogen bonding
Mass
17. Weakest IMFs - found in all molecules
third
d orbitals
London dispersion forces
Solute
18. frequency symbol
0.0826Latm/Kmol
nu
T-shape
Buffer
19. Carbon & hydrogen compounds
acetate
Hydrogen bonding
hydrocarbons
Mass
20. Boltzmann constant - used in calculating speed of gas per molecule
1.38x10?²³J/K
Adding
LE Model
green/yellow
21. AX4
London dispersion forces
tetrahedral
dichromate
LeChatelier's Principle
22. Boiling point elevation formula
insoluble
p
0
?Tb= kb x molality
23. x can be ignored when % ionization is <5%
5% rule
Cathode
-oic acid
Net Ionic Equation
24. Type of system in which the energy may escape - but the mass is conserved
red/orange
Bronsted-Lowry acid
Cation
Closed System
25. The lowest energy configuration for an atom is the one having the max number of unpaired electrons allowed by the Pauli principle in a set of degenerate orbitals
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26. Increase Volume
mol
Polar Covalent
Increase Temperature
solid CO2
27. AX6
octahedral
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
heat capacity
strong acid strong base rxn
28. Speed of Diffusion/Effusion formula
prop-
t-shape
rate gas A/rate gas B = square root (mm A/ mm B)
rate
29. r=k[A]^2
Normality
Zero-Order Half Life
Second-Order Rate Law
s
30. High-energy light
Gamma Ray-
Bronsted-Lowry Base
Trigonal Bipyramidal
Molarity
31. Electron (symbol)
e-
adhesion
Hybridization
g solute/g solvent x 100
32. A device used to measure Delta H
Pressure
Calorimeter
red
-ous acid
33. SI unit of energy; Kg*m^2/s^2
s
-1
base
Joule
34. All cations are soluble with bromide - chloride and iodide EXCEPT
Ag+ - Pb2+ - Hg2+
red
Limiting reactant
moles solute/kg solvent
35. STP
melting
0 degrees C - 1 atm
standard solution
charge
36. If anion ends in -ate - acid name ends in...
Gamma Ray-
entropy (S)
Force = mass x acceleration
-ic acid
37. Colors of Reaction when (Cr2O7 2-) --> (Cr 3+)
Galvanic Cell
Speed of light
yellow --> green
6.63x10?³4Js
38. AX3E2
Balmer Series
Acid + Base --> Salt + Water
Molality
t-shape
39. R in ideal gas law
Arrhenius equation
adhesion
Molal FP Depression Constant
0.0821 atm L/mol K
40. Volume of gas @STP
prop-
22.4L
mol Fraction
ether
41. Energy required to break a bond
entropy (S)
endless
Work
Bond Energy
42. Mass percent
Integrated Zero-Order Rate Law
methoxy-
g solute/g solvent x 100
spontaneity
43. AX2 - AX2E3
linear
?Tb= kb x molality
nitrate
Molecular Compounds
44. (msubs) Can only be +1/2 or -1/2
Beta Particles-
rate law
Electron Spin Quantum Number
Percent Yield
45. Force that holds atoms together
Chemical Bonds
cathode
v3kT/m
-one
46. Energy needed to vaporize a mole of a liquid
precipitate
?Hvap
seesaw
Alkaline earth metals
47. % yield
actual yield/theoretical yield x 100%
specific heat
Trigonal Planar
Cation
48. Force acting over distance
AE= AH - RTAn
Work
Barometer
Hydrogen bonding
49. Describe various properties of one orbital
-2 - with peroxide -1
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
hex-
Quantum Numbers
50. The amount of energy/heat required to raise some substance 1 degree C
Strong acid weak base rxn
Heat Capacity (C)
Molecular Compounds
chloride