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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.
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1. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
The bohr model
Ion dipole interactions
Henderson Hasselbalch Equation
Collision theory of chemical Kinetics
2. An ionic compound that resists changes in its pH
Azeotrope
Formula weight
Buffer
lewis base
3. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Planck's Constant
Solvent
Hydrogen bonding
4. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
bond length
Group 3A
Amphoteric
polymer
5. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin
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6. The average distance between the nuclei of two bonded atoms
Emperical Formula
Resonance structure
bond length
Redox Half Reaction
7. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
lathanide series
Alkaline earths
Formula weight
8. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Avagadros number
compound
Ion dipole interactions
Noble gases
9. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Effusion
s orbital
quantum
molecule
10. Property of the elements that can be predicted from the arrangement of the periodic table
Henry's Law
law of constant composition
Diprotic Base
periodic trends
11. 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
Reaction mechanism
amorphous solid
Group 2A
12. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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13. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Ionization energy
d orbital
Molecular orbital
Rate law
14. 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
empirical formula
physical reaction
Activation energy
Equlibrium constant
15. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Lewis acid base reaction
Formula weight
physical reaction
STP
16. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Bronsted Lowry
solvation
d orbital
Diprotic Base
17. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Group 5A
pI
Ion dipole interactions
Dipole
18. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Activation energy
redox reaction
d orbital
molecule
19. 2.18 x 10^-18 J/electron
Acid dissociation constant
Azeotrope
Rydberg constant
electron configuration
20. 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
Group 3A
Aqueous Solution
Octet Rule
Hydrogen bonding
21. 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
und's rule
Ionization energy
Atomic weight
Acid dissociation constant
22. 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.
Mass number
VSEPR
Covalent Bond
Normality
23. Two or more atoms held together by covalent bonds
molecule
Henderson Hasselbalch Equation
representative elements
gram equivalent weight
24. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Pauli exclusion principle
chemical reaction
Mass number
25. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Strong acid
Equilibrium
Molarity
Amphoteric
26. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
Balmer series
Graham's Law
Effective nuclear charge
Magnetic quantum number
27. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy
Molecular orbital
single displacement reaction
s orbital
Lewis definition
28. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
actinide series
Normality
molecule
Lewis acid base reaction
29. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
physical reaction
Ion dipole interactions
Combination Reaction
30. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Dispersion Forces
theoretical yield
STP
Atomic absorption Spectra
31. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
Dispersion Forces
mole
Group 2A
32. In a solution - the substance that dissolves in the solvent
Equilibrium
Group 1A
energy state
Solute
33. 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-
Water dissociation Constant
Octet Rule
Reaction mechanism
Phase diagram
34. 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.
Group 3A
crystalline solid
amorphous solid
Ion product
35. A solution in which water is the solvent
Mass number
Aqueous Solution
Chemical Kinetics
chemical reaction
36. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Titration
Rate determining step
Electronegativity
Group 1A
37. Slightly less reactive than alkali metals - comprise group II
Dispersion Forces
Group 7A
Ground state
Alkaline earths
38. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Henderson Hasselbalch Equation
Reaction order
Dispersion Forces
atomic radius
39. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
percent composition
Solute
Neutralization reaction
Bronsted Lowry
40. Redox reaction - in which the same species is both oxidized and reduced.
Molar solubility
Disproportionation
Effusion
chemical reaction
41. Tells you how much solute is present compared to the amount of solvent
Common ion effect
Concentration
Lewis acid base reaction
Covalent Bond
42. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
sigma bond
Strong acid
Group 2A
STP
43. 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.
atomic radius
Network covalent
redox reaction
heisenberg uncertainty principle
44. 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.
Effective nuclear charge
transition elements
electrolysis
Aqueous Solution
45. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
d orbital
Bronsted Lowry
Mass number
Diffusion
46. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Neutralization reaction
Octet Rule
Arrhenius Definition
Lyman series
47. 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
Solvent
Spin quantum number
Net ionic equation
heisenberg uncertainty principle
48. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Period
Formal Charge
STP
redox reaction
49. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
VSEPR
pI
azimuthal quantum number
50. 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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