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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. x can be ignored when % ionization is <5%
bond energy
Constant Volume
not spontaneous
5% rule

2. R in ideal gas law
chromate
msAT
vapor pressure
0.0821 atm L/mol K

3. Gas to liquid
condensation
cohesion
Quantum Mechanical Model
equivalence point

4. OH¹?
Trigonal Planar
hydroxide
ether
reduction agent

5. 101 -325 Pa
Density
1atm=?Pa
eth-
Calorimetry

6. A given compound always has exactly the same proportion of elements by mass
Law of Definite Proportion
Oxidizing Agent
green/yellow
Covalently w/in themselves - Ionicly bonded w/ each other

7. Freezing point depression formula
?Tf= kf x molality
oxide
experimental yield
standard solution

8. 1.Calculate moles of each atom in molecule 2.Divide each mole number by smallest mole number 3.If necessary - multiply every mole number to get a whole number 4.Moles of each atom is subscript in empirical formula
Atomic Mass Unit
Finding Empirical Formulas
Bases
A Roman numeral

9. Larger molecules which have higher mass and therefore electron density have stronger...
ether
equilibrium
London dispersion forces
(moles of products that are gasses) - (moles of reactants that are gasses)

10. 1/[A]=kt + 1/[A]0
Theory of Relativity
standard solution
Integrated Second-Order Rate Law
spontaneity

11. A neutral molecule/ion having a lone e- pair that can be used to form a bond to a metal ion
Ag+ - Pb2+ - Hg2+
Ligand
chlorite
amine

12. H + donor
Beta Particles-
f
Bronsted-Lowry Acid
First-Order Half Life

13. Molality =
bromate
end point
moles solute/kg solvent
p orbitals

14. Group 2 metals
Integrated Rate Law
Alkaline earth metals
triple point
Bronsted-Lowry Acid

15. High-energy light
bromate
Gamma Ray-
P1= X1P1°
Tetrahedral

16. Function in which it doesn't matter HOW the changes take place - only that they do; you can use to formula Final - Initial ( i.e. energy - pressure - volume - temperature - sort of moles)
State Functions
Colligative properties
Oxidizing Agent
flouride

17. Point at which liquid?gas occurs
oxidation
3rd law of thermodynamics
lambda
boiling point

18. Polyatomic Ions (bonding)
Amino-
Density
entropy (S)
Covalently w/in themselves - Ionicly bonded w/ each other

19. To find activation energy use the...
Arrhenius equation
P of a =(X of a)(total pressure)
-oic acid
chloride

20. AX5
Bonding Pairs
trigonal bipyramidal
phosphate - sulfide - carbonate - sulfate
Electron Spin Quantum Number

21. Ka=[products]^m/[reactants]^n
1st law of thermodynamics
Equilibrium constant
Acid Dissociation Constant
Anode

22. Kinetic Energy per mol
Pi Bond
Ampere
Mass
3/2RT

23. E?s fill the lowest energy orbital first - then work their way up
rate law
l (second quantum number)
Aufbau Principle
1/2mv²

24. AX4E
-al
8.31J/Kmol
see-saw
Force = mass x acceleration

25. Oxidation # of Halogens
Faraday
Mass
period
-1

26. ClO2¹?
chlorite
square pyramidal
q/moles
Pauli Exclusion Principle

27. CO3²?
carbonate
linear
Ideal Gas Law
Naming Binary Ionic Compounds

28. AX3
q/moles
trigonal planar
no precipitate forms
Its root and adding -ide

29. Volume of gas @STP
22.4L
rate gas A/rate gas B = square root (mm gas B/ mm gas A)
3/2RT
meth-

30. Each orbital can hold two e?s each w/ opposite spins
Pauli Exclusion Principle
Colligative properties
Bronsted-Lowry base
Theoretical yield

31. Donates a single H+ Ion (... other prefixes also)
Monoprotic
are not
C + 273
Osmotic Pressure

32. Half-life equation
Cation
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)
N=N.(0.5)^time/time half-life
supercritical fluid

33. Increase Volume
e-
Increase Temperature
Acid + Base --> Salt + Water
oxide

34. 0.00°C - 1 atm
First-Order Half Life
Standard Temperature and Pressure
Percent Yield
methods of increasing rate

35. If K<1 - then Gº>0 and reaction will be...at chemical equilibrium
0
pent-
not spontaneous
heat capacity

36. Thickness
Second-Order Half Life
Cell Potential (Ecell)
viscosity
Mass

37. l=3
End Point
Aufbau Principle
f
are not

38. If anion ends in -ate - acid name ends in...
base and hydrogen gas
amine
-ic acid
Decrease Volume and Increase Temperature

39. 2 or more covalently bonded atoms
acid
Molecule
22.4L
Cg=kPg

40. A single substance that may be an acid or a base (i.e. water)
electron affinity
methods of increasing rate
1 atm = 760 mmHg = 101.3 kPa
Amphoteric

41. Unusually strong dipole forces found when H is bonded to N - O - or F
Hydrogen bonding
vapor pressure
Temperature
double bond

42. #NAME?
Molarity
titrant buret
E
Pressure

43. Calculation from K to C
C + 273
1st law of thermodynamics
s orbitals
dichromate

44. ?T=k*m(solute)
Molal BP Elevation Constant
Cathode
double bond
Density

45. Different form of same element
-ol
allotrope
Arrhenius equation
Metalliods

46. How to Find a Weighted Average
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
trigonal planar
Pressure of H2O must be Subtracted
oxidizing agent

47. Chemical composition of dry ice
pi=(nRT)/v
solid CO2
P1V1/N1T1=P2V2/N2T2
C=(mass)(specific heat)

48. Energy required to break a bond
Bond Energy
Ampere
log[H+]
adiabatic

49. negative ion
Electronegativity
electrolyte
Anion
Oxidation is Loss Reduction is Gain

50. q H2O = ?
msAT
Endothermic
Adding
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