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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. Change in Energy = ? (in terms of constant pressure; for gasses)
violet
e-
AE= AH - RTAn
solid CO2

2. 2 or more covalently bonded atoms
Open System
Trigonal Bipyramidal
Molecule
Arrhenius base

3. Kinetic Energy of an individual particle formula
M = square root (3RT/mm)
voltaic cells
non-
AE = q + w

4. CO3²?
carbonate
Anode
Integrated Zero-Order Rate Law
% yield

5. 109.5° - sp^3
Tetrahedral
Heat
phosphate
1 atm = 760 mmHg = 101.3 kPa

6. Amount of product produced when limiting reactant is used up
LE Model
Finding Empirical Formulas
Theoretical yield
Allotrope

7. A solution that resists a change in its pH
London Dispersion Forces
Buffered Solution
phosphate
Law of Definite Proportion

8. (organics) five carbons
pent-
Molar Heat Capacity
sublimation
Molality

9. The transfer of energy between two objects due to temperature difference
Theoretical yield
but-
Heat
Pauli Exclusion Principle

10. AX4E2
Pressure of H2O must be Subtracted
square planar
vapor pressure
double bond

11. Happens at lines in phase change charts
equilibrium
Weight
Polar Covalent
-(q of H2O + q of cal)

12. Half-life equation
3rd law of thermodynamics
8.31J/Kmol
N=N.(0.5)^time/time half-life
Electronegativity

13. I¹?
flouride
perchlorate
Van't Hoff factor
iodide

14. The heat changed in a chemical reaction.
base and hydrogen gas
Faraday
Thermochemistry
equilibrium

15. How fast or slow a reaction occurs - becomes slower as it reaches equilibrium
Buffer
chlorite
green/yellow
rate

16. Anything occupying space and with mass
no precipitate forms
Molality
Bronsted-Lowry Acid
Matter

17. Metal oxide + H20 ->
electron affinity
-(P)(Change in V)
base
Percent Yield

18. Volume of gas @STP
Enthalpy of Solution
Cg=kPg
Arrhenius acid
22.4L

19. Variable for energy of e- - goes from 1 -2 -3 on up
indicator
n (first quantum number)
Q>K
chlorate

20. 0°C and 1 atm
STP
Negative work value; work done by system
allotrope
Antibonding Molecular Orbital

21. 101 -325 Pa
Quantum Model
Bonding Pairs
H2 - F2 - N2 - O2 - Cl2 - Br2 - I2
1atm=?Pa

22. Increase Volume
Its root and adding -ide
Quantum Mechanical Model
Increase Temperature
system

23. K=[C]^l[D]^m/[A]^j[B]^k; products/reactants; solids don't count
Equilibrium Expression
activated complex (transition state)
endless
Percent Yield

24. Instrument used to measure the pressure of a not-atmospheric gas (open or closed system)
Temperature
Le Chatelier's Principle
heat of vaporization
Manometer

25. If anion ends in -ate - acid name ends in...
green/yellow
-ic acid
Aufbau Principle
Ideal Gas Law

26. When more than one valid Lewis structure can be written for a particular molecule; represented by double-headed arrows
Resonance
electron affinity
soluble
endless

27. Color of K (flame test)
Q<K
purple
double bond
wavelength

28. Energy required for melting to occur
supercritical fluid
London dispersion forces
heat of fusion
trigonal bipyramidal

29. Oxidation # of Ions
charge
Ligand
Reaction Quotient (Q)
Alkali metals

30. A method of investigation involving observation and theory to test scientific hypotheses
Molar Mass of Element/ Total Molar Mass %
Dipole-dipole forces
Transition metals
Scientific Method

31. Atomic #
London dispersion forces
# protons (atom is defined by this)
meth-
Lone Pair

32. Mole Fraction
-oic acid
anode
charge
X of a = moles a/total moles

33. Ecell= E°cell -RT/nF x lnQ
Nernst Equation
red/orange
5% rule
viscosity

34. Type of system in which the energy and mass may leave or enter
k=Ae^(-Ea/RT)
Open System
perchlorate
bromate

35. Coffee Cup Calorimeter
conjugate base
blue-green
Constant Pressure
Decrease Volume and Increase Temperature

36. The reactant in the oxidizing reaction that forces the reduction reaction to occur
complex ions
Arrhenius equation
hex-
Reducing Agent

37. Delta H (AH) = ?
q/moles
increasing
first
base and hydrogen gas

38. Non-Ideal Gas Conditions
Le Chatelier's Principle
1 atm
octahedral
high pressure - low temperature

39. Elements in groups 3-12
d orbitals
Transition metals
Metalliods
rate

40. AX3E
trigonal pyramidal
g solute/g solvent x 100
boiling point
0

41. 96 -485 C/mol e-
Law of Conservation of Mass
Exothermic
Faraday
d

42. Ptotal=P1+P2+P3+...

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43. When gas expands ...
Molecule
Molar Mass of Element/ Total Molar Mass %
Second-Order Half Life
Negative work value; work done by system

44. Spontaneous emission of radiation
single bond
Radioactivity
hydrocarbons
rate gas A/rate gas B = square root (mm gas B/ mm gas A)

45. To find activation energy use the...
electron affinity
Arrhenius equation
non-
Normality

46. States molecules at a given temp. vary in kinetic energy along a bell-curve of molecular velocities
indicator
diamagnetic
Boltzmann distribution
cyanide

47. Specific heat of water
high pressure - low temperature
4.184
Integrated First-Order Rate Law
Molar Heat Capacity

48. If anion ends in -ite - acid name ends in...
Integrated Zero-Order Rate Law
-oic acid
Adding
-ous acid

49. Horizontals on the periodic table
Second-Order Half Life
titrant buret
period
endless

50. Reverse rxn occurs when
E
red/orange
Q>K
22.4L