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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. Negative enthalpy - heat flows into surroundings
Cell Potential (Ecell)
boiling point
Nodes
exothermic

2. Point where acid completely neutralizes base
equivalence point
-ic acid
methods of increasing rate
Standard Temperature and Pressure

3. Two molecules with identical connectivity but different geometries
geometric isomers
Tetrahedral
phosphate
1.86°C

4. BrO3¹?
bromate
end point
seesaw
M1V1=M2V2

5. The reactant that is being reduced - brings about oxidation
base
Tetrahedral
oxidizing agent
Octahedral

6. Forward rxn occurs when
triple point
Q<K
Molal BP Elevation Constant
Osmotic Pressure

7. If anion ends in -ate - acid name ends in...
Quantum Numbers
-2 - with peroxide -1
cathode
-ic acid

8. Average Kinetic Energy Formula
Atmospheric Pressure
Average KE = 1/2(mass)(average speed of all particles)
weak acid strong base rxn
Volume Metric Flask & Pipet

9. 90°&120° - dsp^3
Joule
f
Trigonal Bipyramidal
specific heat

10. Color of Na (flame test)
yellow
Constant Volume
Overall Reaction Order
Valence Electrons(assigned)

11. The line running between the atoms
p orbitals
Sigma Bond
22.4L
like

12. Average speed of gas
trigonal pyramidal
p orbitals
Molar Mass of Element/ Total Molar Mass %
v3RT/M(in kg)

13. The total entropy is always increasing - all systems tend towards maximum entropy
sulfate
freezing
2nd law of thermodynamics
s orbitals

14. For significant digits - leading zeros ____ significant
heat capacity
Radioactivity
are not
1atm=?Pa

15. Anything occupying space and with mass
hydro-ic acid
Matter
?Tf= kf x molality
surroundings

16. Describe various properties of one orbital
Quantum Numbers
boiling point
London dispersion forces
g solute/g solvent x 100

17. IMF that occurs with FON
purple --> pink
Increase Temperature
Hydrogen bonding
Pauli Exclusion Principle

18. Change in Energy (AE) = ? (in terms of work)
AE = q + w
P of a =(X of a)(total pressure)
Calorimeter
are

19. A device in which chemical energy is changed to electrical energy
Galvanic Cell
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
lambda
Nodes

20. Atomic #
triple point
# protons (atom is defined by this)
3/2RT
First-Order Half Life

21. Speed of light - C
green/yellow
3.0x108m/s
complex ions
Counterions

22. Heat needed to change 1 g of substance to 1°C
specific heat
weak acid strong base rxn
perchlorate
Quantum Mechanical Model

23. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
pent-
Bronsted-Lowry Base
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2

24. If anion ends in -ide - acid name ends in
hydro-ic acid
Adding
Covalently w/in themselves - Ionicly bonded w/ each other
lambda

25. Solution in flask being titrated
X of a = moles a/total moles
Quantum Model
analyte
Aufbau Principle

26. The energy required to raise 1 g of substance 1 degree C
Specific Heat (s)
T-shape
1.86°C
t-shape

27. How to Find a Weighted Average
Matter
C + 273
?Tf= kf x molality
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

28. CN¹?
Solubility Product (Ksp)
cyanide
0 degrees C - 1 atm
Integrated First-Order Rate Law

29. Experimental yield/theoretical yieldx100
triple bond
deposition
% yield
State Functions

30. Everything in the universe that is not defined by you as part of the system
Surroundings
Molarity
Heat
oxide

31. The measurement of heat changes
Calorimetry
System
r1/r2
Coordination Compound

32. (organics) one carbon
high pressure - low temperature
Integrated Rate Law
oxide gas and water
meth-

33. Metal oxide + H20 ->
base
Solubility Product (Ksp)
single bond
% yield

34. Substances w/ critical temperatures below 25°C
permanent gases
-ous acid
Amount of atoms present
Buffered Solution

35. Similar to atomic orbitals - except between molecules
Counterions
Solute
Molecular Orbitals (MOs)
Equivalence Point

36. AP doesn't deal with ...-order reaction - don't pick it!
spontaneity
third
Volt
l (second quantum number)

37. Variable for energy of e- - goes from 1 -2 -3 on up
First-Order Half Life
Calorimetry
2nd law of thermodynamics
n (first quantum number)

38. AX5E
chlorate
Metalliods
eth-
square pyramidal

39. An equilibrium expression
Solubility Product (Ksp)
London dispersion forces
linear
Buffered Solution

40. 1/[A] vs. time is a ...-order reaction
Root Mean Square Velocity
hydroxide
analyte
second

41. n+m (these are orders of reactants)
-ol
electron affinity
Overall Reaction Order
supercritical fluid

42. The reactant in the oxidizing reaction that forces the reduction reaction to occur
AE = q + w
Reducing Agent
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
1 atm

43. All forms of energy except for heat
Hydrogen bonding
work
chromate
Naming Binary Ionic Compounds

44. q H2O = ?
msAT
allotrope
Hybridization
mol Fraction

45. Ionizes to produce H+ ions
Arrhenius Acid
-one
endless
Beta Particles-

46. ?Hsoln=?H1+?H2+?H3+...
Enthalpy of Solution
Specific Heat (s)
exothermic
Law of Multiple Proportions

47. Point at which liquid?gas occurs
Open System
zero
boiling point
s orbitals

48. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Angular Momentum Quantum Number
Trigonal Bipyramidal
rate
London dispersion forces

49. Measure of the average kinetic energy of all the particles in a substance
Temperature
-(q of H2O + q of cal)
22.4L
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

50. Absorbs/takes in heat (positive value)
Enthalpy of Solution
cohesion
like
Endothermic