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. Occupies the space above and below a sigma bond
system
triple bond
Ionic
Pi Bond

2. Elements which have all electrons paired and relatively unaffected by magnetic fields
Atmospheric Pressure
violet
diamagnetic
First-Order Half Life

3. How to Find an Empirical Formula Given Grams
?Hvap
s (fourth quantum number)
1) Convert to moles 2) divide by lowest moles 3) if any halfs - double all values 4) plug into Compound
Pi Bond

4. Theoretical yield-experimental yield/theoretical yieldx100
Integrated Second-Order Rate Law
% error
strong bases
flouride

5. K
Equilibrium constant
trigonal bipyramidal
Decrease Volume and Increase Temperature
like

6. Change in Energy (AE) = ? (in terms of work)
AE = q + w
STP
equilibrium
Acids

7. Ideal Gas Law Formula
1) multiply each AMU by the percentage that represents that isotopes occurrence in nature 2) then add all the AMUs together.
PV=nRT
Average KE = 1/2(mass)(average speed of all particles)
Antibonding Molecular Orbital

8. (# of valence e- on free atom) - (# of valence e- assigned to atom in molecule)
M1V1=M2V2
Closed System
Pressure of H2O must be Subtracted
Formal Charge

9. Rate of Diffusion/Effusion formula
v3kT/m
Electron Spin Quantum Number
Trigonal Planar
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

10. 1 sigma bond
M1V1=M2V2
Constant Volume
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
single bond

11. BrO3¹?
bromate
iodide
seesaw
Graham's Law

12. 180° - sp
Linear
Radioactivity
Thermochemistry
Exothermic

13. Electron (symbol)
hydro-ic acid
hydroxide
e-
Covalently w/in themselves - Ionicly bonded w/ each other

14. E=mc^2
methoxy-
Theory of Relativity
are
Integrated Rate Law

15. (msubs) Can only be +1/2 or -1/2
chlorate
d orbitals
trigonal bipyramidal
Electron Spin Quantum Number

16. IMF that occurs with FON
Arrhenius acid
Density
Hydrogen bonding
Bronsted-Lowry Acid

17. Bomb Calorimeter
moles of solute/ L of solution
spontaneous
0.0826Latm/Kmol
Constant Volume

18. In a titration - the point where the indicator changes (just after moles of solid are equal to moles of base)
Molality
f
End Point
Molar Mass of Element/ Total Molar Mass %

19. Happens at lines in phase change charts
d
equilibrium
Radioactivity
Resonance

20. Unit of electrical potential; J/C
AE= AH - RTAn
linear
Volt
endothermic

21. 90° - d^2sp^3
Octahedral
LeChatelier's Principle
ln (k1/k2) = (Ea/R)(1/T2-1/T1)
p+

22. Where oxidation occurs
Reducing Agent
Anode
r1/r2
Heat Capacity (C)

23. Oxidation # of Ions
but-
perchlorate
adhesion
charge

24. Unusually strong dipole forces found when H is bonded to N - O - or F
second
v3kT/m
Hydrogen bonding
Acids

25. Significant Digits of Conversion Factors
activated complex (transition state)
endless
-(P)(Change in V)
0.0826Latm/Kmol

26. If anion ends in -ide - acid name ends in
Chemical Kinetics
hydro-ic acid
viscosity
purple --> pink

27. [A] vs. time is a ...-order reaction
Equilibrium Expression
endless
zero
Calorimetry

28. ?Hsoln=?H1+?H2+?H3+...
paramagnetic
Enthalpy of Solution
Molecular Orbitals (MOs)
base and hydrogen gas

29. Connects the 2 half cells in a voltaic cell
salt bridge
Allotrope
fusion
Alkaline earth metals

30. PV=nRT
Ideal Gas Law
P1V1/N1T1=P2V2/N2T2
endothermic
First-Order Half Life

31. IMF that exists in polar molecules
Zero-Order Half Life
Hydrogen bonding
Dipole-dipole forces
equilibrium

32. Expresses how the concentrations depend on time
Boltzmann distribution
Arrhenius base
Integrated Rate Law
Hund's Rule

33. # bonding e- - # antibonding e-/2
square planar
Bond Order
bromate
8.31J/Kmol

34. A monoatomic cation takes name from...
Reducing Agent
Its element
square planar
Chemical Bonds

35. Ionizes to produce H+ ions
Arrhenius Acid
Calorimeter
Equilibrium Expression
Integrated Second-Order Rate Law

36. ln[A]=-kt + ln[A]0
Arrhenius Base
Electronegativity
Integrated First-Order Rate Law
1.86°C

37. Mole Fraction
van't Hoff Factor
X of a = moles a/total moles
n0
Alkali metals

38. Raising heat - adding catalyst - heighten concentration - bigger surface area
Naming Binary Ionic Compounds
methods of increasing rate
1) Assume percentages are g (where you have 100 g) 2) convert to moles 3) divide by lowest value 4) plug into compound
AH rxn = (Sum of AH of formation of products) - (Sum of AH of formation of reactants)

39. Gas to solid
Volume Metric Flask & Pipet
salt bridge
flouride
deposition

40. Different form of same element
nu
allotrope
effects of IMF
Cation

41. These orbitals are spherical
Valence Electrons(assigned)
s orbitals
Work
red/orange

42. 101 -325 Pa
Bond Order
1atm=?Pa
s orbitals
triple bond

43. R=
LE Model
Hydrogen bonding
0.0826Latm/Kmol
Sigma Bond

44. Atoms combine in fixed whole # ratios
Law of Multiple Proportions
Bond Order
Theoretical yield
viscosity

45. O²?
oxide
Bronsted-Lowry Base
Manometer
Solute

46. OH¹?
hydroxide
H
Entropy (S)
salt bridge

47. Delta H (AH) = ?
q/moles
Naming Binary Ionic Compounds
moles of solute/ L of solution
Law of Multiple Proportions

48. If heat capacity isn't mentioned - you can assume that q of cal is = ?
Monoprotic
endless
C=(mass)(specific heat)
0

49. Force that holds atoms together
Chemical Bonds
single bond
alkane
vapor pressure

50. Mass reactants= mass products
Law of Conservation of Mass
t-shape
octahedral
adhesion

Major Subjects
Tests & Exams AP CLEP DSST GRE SAT GMAT	Certifications CISSP go to https://www.isc2.org/ PMP ITIL RHCE MCTS More...	IT Skills Android Programming Data Modeling Objective C Programming Basic Python Programming Adobe Illustrator More...	Business Skills Advertising Techniques Business Accounting Basics Business Strategy Human Resource Management Marketing Basics More...
Soft Skills Body Language People Skills Public Speaking Persuasion Job Hunting And Resumes More...	Vocabulary GRE Vocab SAT Vocab TOEFL Essential Vocab Basic English Words For All Global Words You Should Know Business English More...	Languages AP German Vocab AP Latin Vocab SAT Subject Test: French Italian Survival Norwegian Survival More...	Engineering Audio Engineering Computer Science Engineering Aerospace Engineering Chemical Engineering Structural Engineering More...
Health Sciences Basic Nursing Skills Health Science Language Fundamentals Veterinary Technology Medical Language Cardiology Clinical Surgery More...	English Grammar Fundamentals Literary And Rhetorical Vocab Elements Of Style Vocab Introduction To English Major Complete Advanced Sentences Literature Homonyms More...	Math Algebra Formulas Basic Arithmetic: Measurements Metric Conversions Geometric Properties Important Math Facts Number Sense Vocab Business Math More...	Other Major Subjects Science Economics History Law Performing-arts Cooking Logic & Reasoning Trivia

Test your basic knowledge |

AP Chemistry

Sorry!:) No result found.

Can you answer 50 questions in 15 minutes?

Let me suggest you:

Browse all subjects

Browse all tests

Most popular tests

Major Subjects

Tests & Exams

Certifications

IT Skills

Business Skills

Soft Skills

Vocabulary

Languages

Engineering

Health Sciences

English

Math

Other Major Subjects

Browse all subjects

Browse all tests

Most popular tests