Test your basic knowledge |

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. 760 mmHg - 760 torr
octahedral
% yield
Temperature
1 atm

2. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
geometric isomers
v3kT/m
Boltzmann distribution
trigonal bipyramidal

3. Delta H (AH) = ?
system
q/moles
oxalate
chlorite

4. J/°Cg or J/Kg
square pyramidal
e-
Specific Heat Capacity
First-Order Rate Law

5. R=
Bronsted-Lowry Acid
8.31J/Kmol
high pressure - low temperature
Endothermic

6. Energy (definition)
5% rule
Heat
Equilibrium constant
force x distance = work done

7. PO4³?
Calorimetry
v3kT/m
1atm=?Pa
phosphate

8. Cation first - anion second
Arrhenius acid
cyanide
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
Naming Binary Ionic Compounds

9. Change that occurs at constant temperature
Equilibrium Expression
isothermal
endless
strong acid strong base rxn

10. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Ag+ - Pb2+ - Hg2+
methods of increasing rate
entropy
Equilibrium Expression

11. 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)
Electronegativity
0.0821 atm L/mol K
sublimation
Molecular Compounds

12. q rxn = ?
T-shape
s (fourth quantum number)
-(q of H2O + q of cal)
methoxy-

13. Larger molecules which have higher mass and therefore electron density have stronger...
second
London dispersion forces
Integrated Rate Law
Arrhenius Base

14. 0°C and 1 atm
purple --> pink
m (third quantum number)
P1V1/N1T1=P2V2/N2T2
STP

15. Substances w/ critical temperatures below 25°C
Bronsted-Lowry acid
Work
permanent gases
-(P)(Change in V)

16. C2O4²?
oxalate
Adding
H
force x distance = work done

17. Equation to find Ea from reaction rate constants at two different temperatures
p orbitals
endothermic
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
supercritical fluid

18. Compound in which there is a bond between two non-metals; when naming them you use the numerical prefixes (may NOT be reduced i.e. S2F4 may not become SF2)
Ionic Compounds
Acids
Integrated Second-Order Rate Law
Standard Temperature and Pressure

19. NH4¹?
Faraday
Trigonal Bipyramidal
ammonium
Closed System

20. An element with several different forms - each with different properties (i.e. graphite & diamond)
Allotrope
equivalence point
anode
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.

21. Increase Volume
nu
Increase Temperature
-ic acid
C=(mass)(specific heat)

22. Polyatomic Ions (bonding)
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
Covalently w/in themselves - Ionicly bonded w/ each other
sulfate
methoxy-

23. All forms of energy except for heat
P of a =(X of a)(total pressure)
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
work
hydrolysis

24. Positive ion
Cation
Principal Quantum Number
Reducing Agent
sublimation

25. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
Amount of atoms present
Bronsted-Lowry base
alkane

26. Speed of Diffusion/Effusion formula
Chemical Bonds
rate gas A/rate gas B = square root (mm A/ mm B)
Amount of atoms present
Polar Covalent

27. PV=nRT
Endothermic
Ideal Gas Law
Reducing Agent
titrant buret

28. A homogeneous mixture with 1 phase
blue-green
2nd law of thermodynamics
Solution
Anion

29. (organics) three carbons
dichromate
prop-
oxalate
-oate

30. Color of Ba (flame test)
1atm=?mmHg/Torr
alkane
-oic acid
green/yellow

31. The amount of energy/heat required to raise some substance 1 degree C
v3RT/M(in kg)
but-
Specific Heat (s)
Heat Capacity (C)

32. Melting
fusion
Pauli Exclusion Principle
# protons + # neutrons
Bond Order

33. Connects the 2 half cells in a voltaic cell
salt bridge
Pauli Exclusion Principle
Solute
hept-

34. If Q>Ksp
Acid Dissociation Constant
a precipitate forms
chlorate
A Roman numeral

35. 1 sigma bond
Specific Heat Capacity
Percent Yield
N=N.(0.5)^time/time half-life
single bond

36. These orbitals are diagonal
Molal BP Elevation Constant
Molar Heat Capacity
d orbitals
Linear

37. A solution that resists a change in pH - contains both a weak acid and its conjugate base
First-Order Rate Law
trigonal planar
van't Hoff Factor
Buffer

38. Bond bond in which atoms aren't so different that electrons are completely transferred but are different enough that unequal sharing occurs
Polar Covalent
State Functions
Atomic Mass Unit
see-saw

39. ClO2¹?
chlorite
catalyst
zero
f

40. Color of Na (flame test)
different # of neutrons
Volume Metric Flask & Pipet
yellow
entropy (S)

41. ClO4¹?
Principal Quantum Number
perchlorate
oxidation
cohesion

42. (organics) eight carbons
Percent Yield
permanent gases
chromate
oct-

43. ?H when 1 mol of bonds is broken in the gaseous state
Faraday
-ol
Tetrahedral
Bond enthalpy

44. Color of Cs (flame test)
Molal FP Depression Constant
blue
mol Fraction
Reducing Agent

45. High-energy light
Gamma Ray-
melting
trigonal planar
pent-

46. Variable for spin of electron (+.5 or -.5)
s (fourth quantum number)
s orbitals
Arrhenius acid
Pressure

47. Like dissolves...
C=(mass)(specific heat)
second
like
# protons (atom is defined by this)

48. Group 2 metals
0 degrees C - 1 atm
Overall Reaction Order
Constant Volume
Alkaline earth metals

49. Atomic #
(moles of products that are gasses) - (moles of reactants that are gasses)
# protons (atom is defined by this)
Aufbau Principle
Transition metals

50. AX3E
amine
Bond Order
Integrated Zero-Order Rate Law
trigonal pyramidal