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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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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 weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Network covalent
crystalline solid
Lewis definition
Atomic weight
2. An atom or group of atoms that has a positive or negative charge
decomposition reaction
Ion
transition elements
representative elements
3. The average distance between the nuclei of two bonded atoms
Molality
pI
bond length
solvation
4. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
pi bonds
Ion dipole interactions
Acid dissociation constant
5. Numbers that specify the properties of atomic orbitals and of their electrons
Redox Half Reaction
quantum numbers
Group 5A
chemical reaction
6. Simplest whole # ration of atoms in a compound
Emperical Formula
Half equivalence point
periodic trends
crystalline solid
7. A reaction where a compound does Not change its molecular structure.
single displacement reaction
physical reaction
redox reaction
indicator
8. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Planck's Constant
Concentration
Molecular orbital
9. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
bond energy
Bronsted - Lowry definition
Ion
mole
10. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Group 2A
Balmer series
Percent yield
bond length
11. The percent by mass of each element in a compound
lathanide series
percent composition
Atomic weight
periodic trends
12. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
Redox Half Reaction
Nonpolar covalent bond
gram equivalent weight
13. 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.
Molality
electron affinity
Group 2A
Solute
14. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Nucleus
solvation
electrolysis
Strong acid
15. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Activation energy
Conjugate acids and Bases
actinide series
redox reaction
16. The energy required to break a chemical bond and form neutral isolated atoms
Disproportionation
lewis base
bond energy
Bronsted Lowry
17. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
Graham's Law
Rydberg constant
atomic theory
London forces
18. 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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19. 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
solvation
single displacement reaction
Common ion effect
Proton
20. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
Period
bond energy
Azeotrope
21. PH of a molecule at which it contains no net electric charge - isoelectric point.
crystalline solid
pI
Conjugate acids and Bases
Ion
22. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Atomic weight
indicator
Percent yield
Molality
23. 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
s orbital
Henderson Hasselbalch Equation
Le chateliers Principle
Hydrogen bonding
24. 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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25. 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-
Normality
Hydrogen bonding
Amphoteric
Water dissociation Constant
26. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
sigma bond
Electronegativity
pi bonds
chemical reaction
27. 5 valence electrons -3 ions - Nitride N
pH
Group 5A
London forces
Henderson Hasselbalch Equation
28. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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29. Sum of the protons and neutrons in an element often denoted by the letter A
quantum
Mass number
solvation
decomposition reaction
30. Having characteristics of both an acid and a base and capable of reacting as either
Decomposition reaction
redox reaction
Arrhenius Definition
Amphoteric
31. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Group 3A
periodic trends
STP
Group 7A
32. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
pH
Formula weight
Balmer series
Molarity
33. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Lewis structure
redox reaction
Formula weight
34. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Pauli exclusion principle
gram equivalent weight
transition elements
Common ion effect
35. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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36. 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.
Atomic absorption Spectra
law of constant composition
Redox Half Reaction
Henderson Hasselbalch Equation
37. A reaction in which atoms of one element take the place of atoms of another element in a compound
Magnetic quantum number
single displacement reaction
Rate law
Ionic Bond
38. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Triple point
Rate law
Buffer
redox reaction
39. An ionic compound that resists changes in its pH
Nucleus
Buffer
Charles and Gay Lussac's Law
quantum numbers
40. E=hc/?
London forces
Rate determining step
electromagnetic energy of photons emmited from electrons at ground state
Combination Reaction
41. 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.
Common ion effect
Ion product
percent composition
heisenberg uncertainty principle
42. 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.
Period
Equivalence point
Group 6A
single displacement reaction
43. 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
atomic radius
Dispersion Forces
Noble gases
STP
44. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
representative elements
bond energy
physical reaction
Vapor pressure
45. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
bond length
electron affinity
Colligative properties
The bohr model
46. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
lewis base
Ionic Bond
Common ion effect
47. Common definition of acids as proton (H+) donors and bases as proton acceptors
percent composition
Activation energy
Bronsted - Lowry definition
Neutron
48. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Disproportionation
Octet Rule
polymer
49. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
law of constant composition
Nonpolar covalent bond
redox reaction
Group 1A
50. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Combination Reaction
Conjugate acids and Bases
Group 2A
Collision theory of chemical Kinetics
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