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Test your basic knowledge |
MCAT Chemistry
Start Test
Study First
Subjects
:
mcat
,
science
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. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Ion
Dipole Dipole interaction
Halogens
gram equivalent weight
2. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Group 2A
Molarity
Redox Half Reaction
polymer
3. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
crystalline solid
Effective nuclear charge
Resonance structure
d orbital
4. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
redox reaction
Bronsted Lowry
Molecular orbital
5. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
Phase diagram
atomic emission spectrum
Water dissociation Constant
6. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
Reaction mechanism
Dispersion Forces
quantum numbers
representative elements
7. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Network covalent
Amphoteric
mole
Electronegativity
8. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
Phase diagram
Solubility Product Constant
Principle quantum number
Nonpolar covalent bond
9. Two or more atoms held together by covalent bonds
Pauli exclusion principle
molecule
Reaction mechanism
Nonpolar covalent bond
10. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
s orbital
bond energy
Atomic absorption Spectra
11. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
single displacement reaction
Halogens
electron affinity
Titration
12. The lowest allowable energy state of an atom
STP
actinide series
Molecular orbital
Ground state
13. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Equlibrium constant
Lyman series
Noble gases
Covalent Bond
14. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
Rydberg constant
Water dissociation Constant
representative elements
redox reaction
15. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Concentration
pH
gram equivalent weight
Chemical Kinetics
16. Common definition of acids as proton (H+) donors and bases as proton acceptors
law of constant composition
Reaction order
angular momentum in the bohr model
Bronsted - Lowry definition
17. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Ionization energy
pi bonds
representative elements
18. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
empirical formula
atomic theory
Group 6A
Rate determining step
19. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Amphoteric
Group 6A
Resonance structure
20. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
molecule
Effusion
polymer
Neutralization reaction
21. 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.
Graham's Law
Effusion
Ion
Ion product
22. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Net ionic equation
pi bonds
Conjugate acids and Bases
23. (chemistry) p(otential of) H(ydrogen)
Halogens
Titration
pH
Azeotrope
24. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
solvation
Pauli exclusion principle
theoretical yield
Lyman series
25. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Ion
Atomic absorption Spectra
Lewis definition
pi bonds
26. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Aqueous Solution
Acid dissociation constant
lathanide series
decomposition reaction
27. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Ground state
crystalline solid
decomposition reaction
Reaction order
28. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
indicator
Buffer
Molarity
Noble gases
29. A base that can accept two moles of H+ per mole of itself (ex: SO4
Principle quantum number
Group 3A
Half equivalence point
Diprotic Base
30. Rare earth element group (elements 58-71)
azimuthal quantum number
Raoult's Law
lathanide series
electron configuration
31. 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
electron affinity
Strong acid
d orbital
32. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
atomic radius
Ionization energy
azimuthal quantum number
33. A horizontal row of elements in the periodic table
Period
Neutralization reaction
Rate determining step
solvation
34. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Ion dipole interactions
Solution equilibrium
electron configuration
Charles and Gay Lussac's Law
35. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Ionization energy
actinide series
s orbital
Vapor pressure
36. A reaction in which atoms of one element take the place of atoms of another element in a compound
Equivalence point
Normality
single displacement reaction
gram equivalent weight
37. Any sample of a given compound will contain the same elements in the identical mass ratio.
Formal Charge
Effusion
law of constant composition
STP
38. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
pH
Solution equilibrium
Bronsted Lowry
compound
39. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
Formula weight
crystalline solid
heisenberg uncertainty principle
40. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
Halogens
Colligative properties
Titration
Free radical
41. The Percent by mass of each element in a compound.
Percent composition
Group 2A
Graham's Law
Vapor pressure
42. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Vapor pressure
Lewis definition
VSEPR
Hydrogen bonding
43. A dynamic condition in which two opposing changes occur at equal rates in a closed system
quantum numbers
Ion
Nucleus
Equilibrium
44. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
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45. 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
Molecular orbital
The bohr model
Effusion
chemical reaction
46. Slightly less reactive than alkali metals - comprise group II
Molecular orbital
Theoretical yield
Alkaline earths
mole
47. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Group 6A
Group 1A
indicator
Lewis definition
48. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
crystalline solid
electron configuration
sigma bond
49. The slowest elementary step which is the limit for the rate of the other steps
Normality
Halogens
Noble gases
Rate determining step
50. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Equilibrium
Triple point
Dipole Dipole interaction
sigma bond