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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. Pairs of electrons localized on an atom
Angular Momentum Quantum Number
Q<K
heat capacity
Lone Pair
2. Where reduction occurs
p
?Tb= kb x molality
Cathode
Solvent
3. Oxidation # of free elements
indicator
Hydrogen bonding
0
ether
4. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
Molecular
soluble
oxalate
linear
5. Polyatomic Ions (bonding)
triple point
Covalently w/in themselves - Ionicly bonded w/ each other
Monoprotic
actual yield/theoretical yield x 100%
6. A weak acid that changes color at or near the equivalence point
Solvent
Nodes
indicator
specific heat
7. q cal = ?
Ligand
CAT
square planar
activated complex (transition state)
8. Mass #
reduction
Chemical Kinetics
# protons + # neutrons
Theory of Relativity
9. If heat capacity isn't mentioned - you can assume that q of cal is = ?
permanent gases
0
Reducing Agent
-al
10. Force per unit area
Ideal Gas Law
Pressure
Open System
Molal FP Depression Constant
11. [A]=-kt + [A]0
Integrated Zero-Order Rate Law
moles of solute/ L of solution
T-shape
-(P)(Change in V)
12. Boiling point - melting point - viscosity - vapor pressure - surface tension
effects of IMF
linear
Temperature
Second-Order Rate Law
13. Transition metals with ammonia - hydroxide - cyanide or thiocyanate form...
Tetrahedral
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
Alkaline earth metals
complex ions
14. l=0
s
Nernst Equation
m (third quantum number)
Molecule
15. 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)
Aufbau Principle
Kinetic Molecular Theory - for ideal gases
base
?Hvap
16. If a change is imposed on a system at equilibrium - the position of the equilibrium will shift in a direction that tends to reduce that change
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17. Melting
moles of solute/ L of solution
methoxy-
reduction agent
fusion
18. ln[A]=-kt + ln[A]0
Volt
boiling point
Integrated First-Order Rate Law
Bond Energy
19. Bomb Calorimeter
Ideal Gas Law
Constant Volume
activation energy
anode
20. Like dissolves...
perchlorate
v3kT/m
Diffusion
like
21. Raoult's Law - relations between vapor pressure and concentrations
force x distance = work done
P1= X1P1°
analyte
Trigonal Bipyramidal
22. Delta H (AH) = ?
-2 - with peroxide -1
but-
Molecular Compounds
q/moles
23. 1/[A] vs. time is a ...-order reaction
P1= X1P1°
moles solute/kg solvent
M1V1=M2V2
second
24. Speed of Diffusion/Effusion formula
Amphoteric
bromate
LeChatelier's Principle
rate gas A/rate gas B = square root (mm A/ mm B)
25. (msubs) Can only be +1/2 or -1/2
Integrated First-Order Rate Law
STP
?Hvap
Electron Spin Quantum Number
26. Lowers activation energy
standard solution
catalyst
AE= AH - RTAn
Oxidizing Agent
27. Ability of an atom in a molecule to attract shared electrons to itself
Work
Isotopes
Electronegativity
Allotrope
28. The transfer of energy between two objects due to temperature difference
Arrhenius Base
Heat
Hess's Law
Mass
29. x can be ignored when % ionization is <5%
Force = mass x acceleration
-oate
5% rule
M = square root (3RT/mm)
30. Half cell in which reduction occurs
Dipole Moment
cathode
Q<K
0 degrees C - 1 atm
31. Force that holds atoms together
seesaw
oct-
Chemical Bonds
amine
32. Color of Ca (flame test)
1.86°C
red/orange
Lone Pair
electron affinity
33. Energy required to break a bond
voltaic cells
Bond Energy
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
ammonium
34. Kinetic Energy per molecule
1/2mv²
alkane
% yield
Bronsted-Lowry Acid
35. C2O4²?
equilibrium
oxalate
work
high pressure - low temperature
36. frequency symbol
triple point
Van't Hoff factor
yellow --> green
nu
37. Loss of electrons - increase in oxidation #
oxidation
base and hydrogen gas
Hydrogen bonding
Q>K
38. Has values from -l to l - including zero; tells orientation of the orbital relative to other orbitals
Magnetic Quantum Number (ml)
r1/r2
trigonal bipyramidal
melting point
39. (organics) six carbons
Nodes
hex-
Law of Multiple Proportions
Chemical Bonds
40. In going from a particular set of reactants to a particular set of products - the change in enthalpy is the same whether the reaction takes place in one step or in a series of steps
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41. Change that occurs at constant temperature
alkane
ether
isothermal
cathode
42. BrO3¹?
bromate
Arrhenius Base
Amino-
Constant Pressure
43. Ionizes to produce OH- Ions
pent-
Aufbau Principle
lambda
Arrhenius Base
44. Phase change from solid to gas
meth-
Dipole Moment
sublimation
chloride
45. A homogeneous mixture with 1 phase
Solution
Aufbau Principle
First-Order Rate Law
Exothermic
46. .69/k
boiling point
Speed of light
Density
First-Order Half Life
47. Carbon - hydrogen - oxygen compounds
triple point
d orbitals
viscosity
carbohydrates
48. Describe various properties of one orbital
Quantum Numbers
Volt
Bond Order
Heat Capacity (C)
49. AX2E - AX2E2
phosphate
A Roman numeral
soluble
bent
50. ... compounds are most conductive
third
strong bases
Delta H or Enthalpy Change
ionic