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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Ionization energy
Chemical Kinetics
Half equivalence point
2. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
Balmer series
VSEPR
Dispersion Forces
atomic theory
3. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
pH
atomic radius
Ionic Bond
Percent yield
4. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital
Spin quantum number
molecular weight
Reaction mechanism
single displacement reaction
5. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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6. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
VSEPR
Le chateliers Principle
Emperical Formula
Henderson Hasselbalch Equation
7. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Bronsted - Lowry definition
heisenberg uncertainty principle
Ionic Bond
Amphoteric
8. A reaction in which atoms of one element take the place of atoms of another element in a compound
Formal Charge
azimuthal quantum number
Group 2A
single displacement reaction
9. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
Molar solubility
law of constant composition
atomic radius
10. The lowest allowable energy state of an atom
Disproportionation
Acid dissociation constant
Ground state
Dipole
11. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
single displacement reaction
Formal Charge
Noble gases
12. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
quanta
Molar solubility
law of constant composition
Emperical Formula
13. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Henderson Hasselbalch Equation
Molarity
s orbital
Conjugate acids and Bases
14. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
Reaction mechanism
electron affinity
Lewis definition
angular momentum in the bohr model
15. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
Solubility Product Constant
VSEPR
solvation
mole
16. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Avagadros number
solvation
atomic theory
Halogens
17. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
physical reaction
Chemical Kinetics
Formula weight
Azeotrope
18. The process by which one or more substances change to produce one or more different substances
Redox Half Reaction
Effective nuclear charge
chemical reaction
Common ion effect
19. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
redox reaction
Planck's Constant
Raoult's Law
20. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Azeotrope
Aqueous Solution
atomic radius
theoretical yield
21. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Rydberg constant
Halogens
Dispersion Forces
Ion dipole interactions
22. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
Group 2A
Free radical
ionic cmpound
23. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
energy state
Strong acid
effective nuclear charge
Molecular orbital
24. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
molecule
electron configuration
Effective nuclear charge
Octet Rule
25. 2.18 x 10^-18 J/electron
quanta
angular momentum in the bohr model
Rydberg constant
Electronegativity
26. A definite stable energy that a physical system can have
energy state
electron configuration
actinide series
Halogens
27. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Triple point
bond length
Reaction mechanism
mole
28. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
Hydrogen bonding
single displacement reaction
pI
Ion product
29. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Aqueous Solution
heisenberg uncertainty principle
lewis base
Chemical Kinetics
30. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
Equivalence point
Water dissociation Constant
sigma bond
periodic trends
31. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Electrolyte
compound
Normality
solvation
32. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
electrolysis
Nucleus
Equivalence point
33. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Emperical Formula
Group 2A
Equivalence point
quanta
34. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
angular momentum in the bohr model
Net ionic equation
Arrhenius Definition
The bohr model
35. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Graham's Law
single displacement reaction
ionic cmpound
36. Chalcogens - - Oxide O
STP
Dipole
Common ion effect
Group 6A
37. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
Ion
Theoretical yield
representative elements
hydrogen bonding
38. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
Disproportionation
Ion dipole interactions
angular momentum in the bohr model
39. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Dipole
Normality
Ground state
Lewis definition
40. Property of the elements that can be predicted from the arrangement of the periodic table
single displacement reaction
periodic trends
pI
Equlibrium constant
41. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation
Conjugate acids and Bases
Equlibrium constant
Arrhenius Definition
STP
42. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Principle quantum number
Group 2A
Reaction mechanism
Avagadros number
43. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Mass number
Net ionic equation
Rate determining step
decomposition reaction
44. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
empirical formula
Ion product
Lewis acid base reaction
Strong acid
45. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
pH
atomic radius
Network covalent
empirical formula
46. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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47. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
gram equivalent weight
pI
Atomic weight
Proton
48. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Rate law
lewis base
quantum numbers
Neutralization reaction
49. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Buffer
Half equivalence point
Covalent Bond
subshell
50. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
sigma bond
Combination Reaction
compound
Electrolyte
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