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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. Energy needed to vaporize a mole of a liquid
?Hvap
purple
Formal Charge
Kinetic Molecular Theory - for ideal gases

2. Point at which liquid?gas occurs
alkyne
charge
boiling point
titrant buret

3. Where there are no electrons
P1= X1P1°
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
Magnetic Quantum Number (ml)
Nodes

4. Horizontals on the periodic table
amine
Anode
equilibrium
period

5. Group 1 - Ammonium - Nitrates - Acetates - Sulfates - Halides
soluble
% yield
-ol
Electronegativity

6. % yield
p
Root Mean Square Velocity
First-Order Rate Law
actual yield/theoretical yield x 100%

7. Formula used when diluting stock solution (to find amount of water or stock needed)
Multiplying
M1V1=M2V2
Amino-
Beta Particles-

8. Coffee Cup Calorimeter
Covalently w/in themselves - Ionicly bonded w/ each other
Constant Pressure
permanent gases
8.314 J/K mol

9. Colors of Reaction when (MnO4 -) --> (Mn2+)
Decrease Volume and Increase Temperature
n0
Arrhenius base
purple --> pink

10. Boiling point elevation formula
square pyramidal
catalyst
equivalence point
?Tb= kb x molality

11. How to Find an Empirical Formula Given Grams
like
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Barometer
Average KE = 1/2(mass)(average speed of all particles)

12. Idea Gas Law (actual rules)
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
d
P1V1/N1T1=P2V2/N2T2
Law of Definite Proportion

13. OIL RIG
ammonium
Oxidation is Loss Reduction is Gain
Molarity
Bronsted-Lowry Base

14. Symbol for the heat absorbed or lost molecularly (PER MOLE)
soluble
deposition
AH
m (third quantum number)

15. Point where acid completely neutralizes base
Ideal Gas Law
flouride
p
equivalence point

16. Stronger IMF= lower... weaker IMF= higher...
1atm=?Pa
p+
vapor pressure
-(q of H2O + q of cal)

17. Substance that - when dissolved - is conductive
are
electrolyte
sublimation
Naming Binary Ionic Compounds

18. The total energy of the universe is constant - all systems tend towards minimum energy
Solution
1st law of thermodynamics
Molecular Compounds
Tetrahedral

19. Significant Digits of counted things
endless
Isolated System
Molality
Multiplying

20. Carbon & hydrogen compounds
hydrocarbons
heat capacity
q/moles
Closed System

21. r=k[A]
cohesion
Its element
3.0x108m/s
First-Order Rate Law

22. Isotope
different # of neutrons
Alpha Particles-
Counterions
Coordination Compound

23. Oxidation # of Compounds
permanganate
H
0
allotrope

24. ?T=k*m(solute)
red
Polar Covalent
Molal FP Depression Constant
nitrite

25. H?+OH??H2O
strong acid strong base rxn
endless
P of a =(X of a)(total pressure)
STP

26. A solution that resists a change in its pH
paramagnetic
Buffered Solution
analyte
adhesion

27. ?T=k*m(solute)
Molal BP Elevation Constant
Integrated First-Order Rate Law
Hund's Rule
Le Chatelier's Principle

28. Has values from 0 to (n-1); tells shape of atomic orbitals
hydro-ic acid
Angular Momentum Quantum Number
insoluble
insoluble

29. SI unit of energy; Kg*m^2/s^2
r1/r2
paramagnetic
8.314 J/K mol
Joule

30. (organics) three carbons
prop-
Chemical Kinetics
spontaneity
complex ions

31. Osmotic pressure=MRT
Sigma Bond
f
Osmotic Pressure
Tetrahedral

32. If Q>Ksp
Solvent
a precipitate forms
oxidation
Van't Hoff factor

33. We cannot simultaneously determine an atom's exact path or location
Calorimeter
Heisenberg Uncertainty Principle
sulfate
v3RT/M(in kg)

34. F¹?
Boltzmann distribution
State Functions
p
flouride

35. Substances w/ critical temperatures below 25°C
Solute
triple point
permanent gases
system

36. HCl - HBr - HI - HNO3 - HClO4 - H2SO4
Limiting reactant
non-
strong acids
STP

37. Elements which have unpaired electrons and highly affected by magnetic fields
ammonium
paramagnetic
diamagnetic
Nernst Equation

38. ?Hsoln=?H1+?H2+?H3+...
actual yield/theoretical yield x 100%
chlorate
m (third quantum number)
Enthalpy of Solution

39. SO3²?
a precipitate forms
sulfite
X of a = moles a/total moles
bent

40. In covalent bonds - prefixes are used to tell...
Arrhenius equation
Molar Mass of Element/ Total Molar Mass %
Ionic Compounds
Amount of atoms present

41. Absorbs/takes in heat (positive value)
Endothermic
ionic
Molecular Orbitals (MOs)
Monoprotic

42. MnO4¹?
4.184
Nodes
permanganate
indicator

43. The reactant in the reduction reaction that forces the oxidation reaction to occur
Zero-Order Half Life
hex-
0
Oxidizing Agent

44. Puts OH? into solution
Constant Pressure
-2 - with peroxide -1
nitrate
Arrhenius base

45. Osmotic pressure formula
Zero-Order Half Life
pi=(nRT)/v
analyte
?Tf= kf x molality

46. Happens at lines in phase change charts
Resonance
permanent gases
oxide
equilibrium

47. Two molecules with identical connectivity but different geometries
geometric isomers
Alkali metals
Chemical Bonds
LeChatelier's Principle

48. Positive enthalpy - heat flows into system
Beta Particles-
Formal Charge
endothermic
-ous acid

49. Positive ion
Monoprotic
Cation
Dipole-dipole forces
Thermochemistry

50. (organics) eight carbons
Antibonding Molecular Orbital
oct-
yellow --> green
surroundings