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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. Proton donors
Angular Momentum Quantum Number
Bronsted-Lowry acid
triple point
van't Hoff Factor

2. % yield
activation energy
Calorimeter
mol Fraction
actual yield/theoretical yield x 100%

3. Calculation from K to C
C + 273
Q<K
Trigonal Planar
Specific Heat Capacity

4. Group 1 and heavier Group 2 bases
Volt
group
strong bases
Pressure of H2O must be Subtracted

5. These orbitals are diagonal
d orbitals
oxide gas and water
1.86°C
rate law

6. Does the same as equilibrium expression - except it uses initial concentrations
Molality
Reaction Quotient (Q)
red
AE= AH - RTAn

7. The rest of the universe (in thermodynamics)
Buffered Solution
surroundings
red
cohesion

8. A device used to measure Delta H
Calorimeter
Theoretical yield
Arrhenius Base
Oxidizing Agent

9. Describe various properties of one orbital
Zero-Order Half Life
Law of Conservation of Mass
hex-
Quantum Numbers

10. Horizontals on the periodic table
v3kT/m
period
Ionic
Molecule

11. I¹?
iodide
London dispersion forces
Molar Mass of Element/ Total Molar Mass %
log[H+]

12. Dirrect Method Formula
sublimation
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
increasing
van't Hoff Factor

13. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
First-Order Rate Law
rate
Matter
Atmospheric Pressure

14. Heat capacity formula
C=(mass)(specific heat)
-1
0
Covalently w/in themselves - Ionicly bonded w/ each other

15. 6.022x10^23
mol
Dipole Moment
Molality
Its element

16. Pressure Units/Conversions
1 atm = 760 mmHg = 101.3 kPa
Bond Energy
viscosity
Dipole-dipole forces

17. Heat needed to change 1 g of substance to 1°C
-al
double bond
Colligative properties
specific heat

18. .69/k
adiabatic
First-Order Half Life
Law of Multiple Proportions
hydro-ic acid

19. All _________ compounds are electrolytes
-(P)(Change in V)
Hydrogen bonding
-al
Ionic

20. Group 2 metals
adhesion
moles of solute/ L of solution
Alkaline earth metals
Ideal Gas Law

21. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
Ag+ - Pb2+ - Hg2+
AE= AH - RTAn
H
Formal Charge

22. Substance in which something is dissolved in a solution (higher [ ])
charge
solid CO2
Solvent
Constant Pressure

23. ClO2¹?
boiling point
k=Ae^(-Ea/RT)
chlorite
chromate

24. ln[A] vs. time is a ...-order reaction
Law of Multiple Proportions
first
Equivalence Point
linear

25. Color of Ba (flame test)
green/yellow
PV=nRT
oxalate
STP

26. S²?
log[H+]
Q<K
Law of Conservation of Energy
sulfide

27. Gas to liquid
condensation
E
Alkali metals
surroundings

28. A single substance that may be an acid or a base (i.e. water)
dichromate
Amphoteric
activated complex (transition state)
no precipitate forms

29. Happens at lines in phase change charts
s
Closed System
equilibrium
0

30. OH¹?
activation energy
f
hydroxide
green/yellow

31. Mol of solute/kg of solvent
Molality
vaporization
Heat
freezing

32. Instrument used to measure the pressure of atmospheric gas
t-shape
Barometer
red
hydrolysis

33. Larger molecules which have higher mass and therefore electron density have stronger...
weak acid strong base rxn
lambda
see-saw
London dispersion forces

34. Variable for energy of e- - goes from 1 -2 -3 on up
Lone Pair
n (first quantum number)
Trigonal Bipyramidal
base and hydrogen gas

35. 1/[A] vs. time is a ...-order reaction
Standard Temperature and Pressure
oxide gas and water
second
Solution

36. Ptotal=Pa+Pb+Pc....

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37. C=2.9979*10^8 m/s
complex ions
Speed of light
blue-green
no precipitate forms

38. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
Ligand
conjugate base
AE= AH - RTAn
non-

39. How to Balance a Redox Equation
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
second
% error
% yield

40. Point at which liquid?gas occurs
nitrate
boiling point
cyanide
Molality

41. Measure of the change in enthalpy
1atm=?Pa
flouride
msAT
Delta H or Enthalpy Change

42. Mixing of gases
square planar
Diffusion
vapor pressure
increasing

43. 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)
Anode
Dipole-dipole forces
Molecular Compounds
carbonate

44. 1 sigma bond
single bond
Reaction Quotient (Q)
phosphate - sulfide - carbonate - sulfate
+1 - except if bonded to Alkali Metal -1

45. SO4²?
sulfate
End Point
0.512°C
chromate

46. BrO3¹?
1.38x10?²³J/K
cyanide
Molarity
bromate

47. Mass #
analyte
endless
hydrocarbons
# protons + # neutrons

48. Substances above the critical temperature and pressure in which the pressure is so high that density and flowing ability of a "gas" resembles that of a liquid
alcohol
supercritical fluid
Equilibrium constant
Alkali metals

49. Solution in flask being titrated
Galvanic Cell
Bases
blue-green
analyte

50. A device in which chemical energy is changed to electrical energy
X of a = moles a/total moles
Galvanic Cell
trigonal pyramidal
titrant buret