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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. All cations are soluble with bromide - chloride and iodide EXCEPT
Covalently w/in themselves - Ionicly bonded w/ each other
8.314 J/K mol
Ag+ - Pb2+ - Hg2+
Effusion
2. High-speed electrons
Beta Particles-
LeChatelier's Principle
Molal BP Elevation Constant
red
3. Ability of an atom in a molecule to attract shared electrons to itself
Endothermic
Electronegativity
Gamma Ray-
Law of Multiple Proportions
4. Variable for energy of e- - goes from 1 -2 -3 on up
n (first quantum number)
phosphate
C + 273
Beta Particles-
5. Oxidation # of free elements
Law of Multiple Proportions
violet
trigonal planar
0
6. Increase Pressure
Decrease Volume and Increase Temperature
Molal FP Depression Constant
oct-
Theory of Relativity
7. If anion ends in -ide - acid name ends in
isothermal
conjugate acid
hydro-ic acid
A Roman numeral
8. Cl¹?
freezing
Anode
chloride
excess reactant
9. Amount of heat needed to change a system by 1°C
increasing
heat capacity
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
wavelength
10. Bomb Calorimeter
London dispersion forces
Constant Volume
Closed System
cohesion
11. The reactant in the reduction reaction that forces the oxidation reaction to occur
carbonate
Ionic
base and hydrogen gas
Oxidizing Agent
12. Average speed of gas
v3RT/M(in kg)
Average KE = 1/2(mass)(average speed of all particles)
Acid Dissociation Constant
Volt
13. (organics) two carbons
Law of Multiple Proportions
eth-
actual yield/theoretical yield x 100%
hex-
14. Higher in energy than the atomic orbitals of which it is composed
conjugate acid
Antibonding Molecular Orbital
Atomic Mass Unit
Strong acid weak base rxn
15. Generally insoluble anions (names)
Dipole Moment
3/2RT
Acids
phosphate - sulfide - carbonate - sulfate
16. Change in moles (An) =?
-al
(moles of products that are gasses) - (moles of reactants that are gasses)
alcohol
g solute/g solvent x 100
17. l=0
22.4L
weak acid strong base rxn
triple bond
s
18. Ionizes to produce OH- Ions
Arrhenius Base
surroundings
Dalton's Law
Buffered Solution
19. Positive enthalpy - heat flows into system
Ag+ - Pb2+ - Hg2+
Bronsted-Lowry acid
endothermic
excess reactant
20. ?T=k*m(solute)
Molal FP Depression Constant
Arrhenius base
AH
amine
21. CN¹?
zero
cyanide
Monoprotic
Finding Empirical Formulas
22. These orbitals are diagonal
Molarity
conjugate base
d orbitals
base
23. The weighted average of all the isotopes that an atom can have (in g/mol)
Atomic Mass Unit
T-shape
adhesion
-1
24. If needed - indicate charge of metal(cation) by...
activation energy
3/2RT
oxide gas and water
A Roman numeral
25. 90°&120° - dsp^3
third
% yield
96500
Trigonal Bipyramidal
26. Electrons in a hydrogen atom move around the nucleus only in circular orbits
not spontaneous
Quantum Model
sulfate
Chemical Bonds
27. Nonmetal oxide + H2O ->
acid
-ic acid
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
q
28. S²?
Theory of Relativity
Temperature
End Point
sulfide
29. Compound in which there is a bond between a metal and a non-metal; when naming - pay attention to ionic charges on periodic table (may be reduced)
Molecular Compounds
Specific Heat (s)
Pressure
g solute/g solvent x 100
30. Where there are no electrons
Nodes
Counterions
Increase Temperature
hex-
31. Substances w/ critical temperatures below 25°C
work
5% rule
permanent gases
Pressure of H2O must be Subtracted
32. Verticals on the periodic table
Nodes
heat capacity
group
pent-
33. When ____ significant digits - round answer to least decimal place
Adding
Angular Momentum Quantum Number
1atm=?Pa
0 degrees C - 1 atm
34. Ending for alcohols
q/moles
-ol
but-
cyanide
35. Gain of electrons - decrease in oxidation #
endothermic
1)Assign Oxidation #s 2) Half Reaction 3) Balance Moles 2) Balance add e- to balance Oxidation #s (RED-OX = reduction on left - Oxidation on right) 4) Add H+ or OH - to balance charge 5) Add H2O to balance hydrogens 4) Balance electrons by multiplyin
base and hydrogen gas
reduction
36. For significant digits - leading zeros ____ significant
London dispersion forces
m (third quantum number)
oxidation
are not
37. Connects the 2 half cells in a voltaic cell
salt bridge
Atomic Mass Unit
g solute/g solvent x 100
alkene
38. n+m (these are orders of reactants)
Overall Reaction Order
trigonal planar
rate law
-al
39. The actual amount of product produced in an experiment
experimental yield
adiabatic
Dalton's Law
dec-
40. Raoult's Law - relations between vapor pressure and concentrations
charge
Calorimeter
P1= X1P1°
q/moles
41. 2+ charge
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
Amount of atoms present
Alpha Particles-
System
42. AX6
equivalence point
square pyramidal
octahedral
?Tb= kb x molality
43. The reactant in the oxidizing reaction that forces the reduction reaction to occur
Reducing Agent
no precipitate forms
Molar Heat Capacity
prop-
44. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Polar Covalent
Solubility Product (Ksp)
-(P)(Change in V)
melting
45. When two elements form a series of compounds - the ratios of the masses of the second element that combine with 1g of the first element can always be reduced to whole numbers
trigonal bipyramidal
Law of Multiple Proportions
seesaw
Ionic Compounds
46. A solution that resists a change in its pH
Hess's Law
end point
Buffered Solution
rate gas A/rate gas B = square root (mm A/ mm B)
47. This MUST be determined experimentally
heat capacity
rate law
Coordination Compound
Root Mean Square Velocity
48. Type of system in which nothing is transfered (no mass or energy); ideal
Second-Order Half Life
Balmer Series
Solute
Isolated System
49. Passage of gas through tiny orifice
Integrated Second-Order Rate Law
Reducing Agent
Effusion
-1
50. (organics) single-bonded compound
Solution
+1 - except if bonded to Alkali Metal -1
alkane
oxidation