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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. 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.
Ion
Electrolyte
ionic cmpound
Balmer series
2. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
molecular weight
molecule
compound
quantum
3. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
electromagnetic energy of photons emmited from electrons at ground state
Lewis acid base reaction
Halogens
Dipole Dipole interaction
4. The lowest allowable energy state of an atom
Aqueous Solution
Ground state
sigma bond
Combination Reaction
5. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Group 2A
actinide series
quantum
Group 5A
6. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Aqueous Solution
Diprotic Base
Effective nuclear charge
pi bonds
7. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Half equivalence point
Triple point
Ionic Bond
lewis base
8. 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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9. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
electromagnetic energy of photons emmited from electrons at ground state
Aqueous Solution
Henderson Hasselbalch Equation
10. 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
Rydberg constant
Rate law
Hydrogen bonding
Principle quantum number
11. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Strong acid
Combination Reaction
Theoretical yield
Reaction mechanism
12. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
crystalline solid
Hydrogen bonding
Network covalent
Molality
13. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Effective nuclear charge
Solute
Bronsted - Lowry definition
14. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
transition elements
STP
Formula weight
15. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Dipole Dipole interaction
Strong acid
s orbital
Net ionic equation
16. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Period
angular momentum in the bohr model
Diffusion
physical reaction
17. The Percent by mass of each element in a compound.
amorphous solid
Spin quantum number
Percent composition
Phase diagram
18. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
Nucleus
Balmer series
lewis base
19. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Group 1A
atomic emission spectrum
Conjugate acids and Bases
Henderson Hasselbalch Equation
20. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
percent composition
Ion dipole interactions
Vapor pressure
azimuthal quantum number
21. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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22. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
atomic emission spectrum
Octet Rule
polymer
Henry's Law
23. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Dispersion Forces
pI
Lewis definition
redox reaction
24. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Titration
VSEPR
compound
indicator
25. The slowest elementary step which is the limit for the rate of the other steps
Period
molecular weight
Rate determining step
lathanide series
26. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Percent composition
Reaction order
Effusion
empirical formula
27. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
decomposition reaction
Ion dipole interactions
Reaction mechanism
28. Slightly less reactive than alkali metals - comprise group II
Balmer series
Neutron
Equivalence point
Alkaline earths
29. 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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30. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
lathanide series
STP
Rate law
Redox Half Reaction
31. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture
decomposition reaction
Hydrogen bonding
Solution equilibrium
transition elements
32. A reaction where a compound does Not change its molecular structure.
Aqueous Solution
Group 7A
physical reaction
Triple point
33. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
molecular weight
subshell
Molarity
34. The maximum amount of product that can be produced from a given amount of reactant
und's rule
Equilibrium
theoretical yield
energy state
35. 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.
Ion product
pH
Diprotic Base
Free radical
36. (chemistry) p(otential of) H(ydrogen)
percent composition
amorphous solid
pH
Ionic Bond
37. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
Intermolecular forces
Spin quantum number
Percent yield
empirical formula
38. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Lyman series
Lewis definition
Charles and Gay Lussac's Law
39. An elementary particle with 0 charge and mass about equal to a proton
subshell
Common ion effect
Net ionic equation
Neutron
40. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
The bohr model
theoretical yield
mole
Group 5A
41. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
electron configuration
Equilibrium
Effusion
Principle quantum number
42. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Chemical Kinetics
Ionic Bond
Intermolecular forces
Covalent Bond
43. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
lewis base
lathanide series
Half equivalence point
decomposition reaction
44. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
redox reaction
Theoretical yield
Network covalent
Electrolyte
45. The percent by mass of each element in a compound
Planck's Constant
solvation
Noble gases
percent composition
46. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
quantum
Principle quantum number
decomposition reaction
47. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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48. 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
Titration
Ion
atomic theory
The bohr model
49. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Network covalent
Decomposition reaction
Formal Charge
Reaction order
50. Common definition of acids as proton (H+) donors and bases as proton acceptors
Strong acid
Ground state
Bronsted - Lowry definition
Diffusion
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