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AP Chemistry

Instructions:

Answer 50 questions in 15 minutes.
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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. Reactant that's completely used up in a chemical reaction
alkene
deposition
Decrease Volume and Increase Temperature
Limiting reactant

2. Tools NEEDED for dilution
M1V1=M2V2
Volume Metric Flask & Pipet
+1 - except if bonded to Alkali Metal -1
Reducing Agent

3. Driving force of the electrons
pi=(nRT)/v
mol
Cell Potential (Ecell)
m (third quantum number)

4. Solid to liquid
# protons (atom is defined by this)
melting
alcohol
n (first quantum number)

5. Liquid to solid
freezing
Ampere
l (second quantum number)
blue-green

6. 0.00°C - 1 atm
Standard Temperature and Pressure
Cation
Linear
-ic acid

7. AX3E2
charge
T-shape
wavelength
mol Fraction

8. Specific heat of water
4.184
Overall Reaction Order
Zero-Order Half Life
trigonal bipyramidal

9. Organic w/ -O-
ether
system
no precipitate forms
dichromate

10. Gas to solid
deposition
charge
Naming Binary Ionic Compounds
alkyne

11. 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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12. An element with several different forms - each with different properties (i.e. graphite & diamond)
perchlorate
Allotrope
% error
surroundings

13. Vapor pressure lowering - boiling point elevation - freezing point depression - osmotic pressure
carbonate
Colligative properties
titrant buret
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound

14. Ester suffix
1st law of thermodynamics
1 atm = 760 mmHg = 101.3 kPa
Specific Heat Capacity
-oate

15. Weakest IMFs - found in all molecules
p+
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
London dispersion forces
Molecular Orbitals (MOs)

16. Liquid to gas
blue-violet
Endothermic
vaporization
PV=nRT

17. Heat capacity formula
0.0821 atm L/mol K
C=(mass)(specific heat)
p+
-(P)(Change in V)

18. SO3²?
Principal Quantum Number
Polar Covalent
sulfite
End Point

19. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Formal Charge
AH
Alkaline earth metals
Magnetic Quantum Number (ml)

20. Temperature-pressure point after which gas can no longer form liquid
+1 - except if bonded to Alkali Metal -1
critical point
Quantum Numbers
Aufbau Principle

21. Ketone suffix
-one
Mass
hydrolysis
0.0826Latm/Kmol

22. Measure of the change in enthalpy
activation energy
Delta H or Enthalpy Change
zero
hydrolysis

23. Loss of electrons - increase in oxidation #
adhesion
red/orange
oxidation
Molality

24. Higher in energy than the atomic orbitals of which it is composed
cyanide
Antibonding Molecular Orbital
system
insoluble

25. In a given atom no two electrons can have the same set of four quantum numbers
octahedral
8.314 J/K mol
green/yellow
Pauli Exclusion Principle

26. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
not spontaneous
# protons + # neutrons
Bonding Pairs
Closed System

27. (msubs) Can only be +1/2 or -1/2
Electron Spin Quantum Number
% error
boiling point
yellow --> green

28. Ending for alcohols
Adding
melting point
-ol
Temperature

29. Molality =
Law of Multiple Proportions
sulfite
moles solute/kg solvent
hydrocarbons

30. Puts OH? into solution
charge
dec-
system
Arrhenius base

31. Non-Ideal Gas Conditions
k=Ae^(-Ea/RT)
Root Mean Square Velocity
Reaction Quotient (Q)
high pressure - low temperature

32. The actual amount of product produced in an experiment
experimental yield
salt bridge
Work
titrant buret

33. Measure of the average kinetic energy of all the particles in a substance
Temperature
reduction agent
ether
Ligand

34. r=k
Zero-Order Rate Law
Average KE = 1/2(mass)(average speed of all particles)
blue-violet
hydroxide

35. Newton's Second Law
Force = mass x acceleration
Valence Electrons(assigned)
Ligand
Molar Mass of Element/ Total Molar Mass %

36. Color of Sr (flame test)
isothermal
red
Osmotic Pressure
Solvent

37. Resistance to flow
# protons (atom is defined by this)
k=Ae^(-Ea/RT)
viscosity
no precipitate forms

38. The chemical formed when a base accepts a proton
Acid Dissociation Constant
2nd law of thermodynamics
conjugate acid
m (third quantum number)

39. 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
1.86°C
spontaneous
specific heat
Law of Multiple Proportions

40. AX4E
N=N.(0.5)^time/time half-life
seesaw
amine
experimental yield

41. Solution used in titration
PV=nRT
0
titrant buret
bromate

42. Polyatomic Ions (bonding)
Covalently w/in themselves - Ionicly bonded w/ each other
square planar
Sigma Bond
oxidation

43. Variable for type of orbital
l (second quantum number)
actual yield/theoretical yield x 100%
Arrhenius base
Law of Definite Proportion

44. Molecules' tendency to stick to the container
heat of vaporization
Arrhenius base
Bond Order
adhesion

45. Symbol for Total Heat absorbed or released
flouride
melting point
Chemical Kinetics
q

46. Entropy in the universe is always...
Law of Multiple Proportions
increasing
Volt
Counterions

47. Unusually strong dipole forces found when H is bonded to N - O - or F
Hydrogen bonding
Angular Momentum Quantum Number
dichromate
Matter

48. H + donor
Law of Conservation of Mass
Bronsted-Lowry Acid
octahedral
Average KE = 1/2(mass)(average speed of all particles)

49. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
but-
Open System
Ligand
Positive work value; work done on system

50. Two molecules with identical connectivity but different geometries
endless
geometric isomers
vapor pressure
Law of Conservation of Mass