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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. Common definition of acids as proton (H+) donors and bases as proton acceptors
Phase diagram
sigma bond
Disproportionation
Bronsted - Lowry definition
2. 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
Combination Reaction
Group 5A
Acid dissociation constant
Lyman series
3. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Electrolyte
Bronsted - Lowry definition
quantum
Azeotrope
4. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Bronsted Lowry
Half equivalence point
Formula weight
indicator
5. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Resonance structure
Covalent Bond
Conjugate acids and Bases
Group 1A
6. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
Nonpolar covalent bond
Buffer
Azeotrope
Group 7A
7. 2.18 x 10^-18 J/electron
Vapor pressure
Rydberg constant
Henry's Law
Equlibrium constant
8. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Mass number
Lewis acid base reaction
Arrhenius Definition
Dipole
9. 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
Proton
bond energy
Ion dipole interactions
Period
10. 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-
redox reaction
Nucleus
Decomposition reaction
Water dissociation Constant
11. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
quantum
The bohr model
bond energy
Collision theory of chemical Kinetics
12. A solid made up of particles that are not arranged in a regular pattern.
Concentration
amorphous solid
lewis base
effective nuclear charge
13. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
quantum
solvation
compound
atomic emission spectrum
14. An ionic compound that resists changes in its pH
Avagadros number
Formal Charge
Buffer
Vapor pressure
15. Slightly less reactive than alkali metals - comprise group II
Formal Charge
Alkaline earths
Molality
lathanide series
16. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Proton
atomic radius
d orbital
Strong acid
17. 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.
Period
Conjugate acids and Bases
crystalline solid
actinide series
18. The process of decomposing a chemical compound by the passage of an electric current.
Raoult's Law
ionic cmpound
electrolysis
STP
19. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
decomposition reaction
Effusion
Amphoteric
20. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Concentration
Network covalent
Group 5A
21. 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
Triple point
Magnetic quantum number
s orbital
Intermolecular forces
22. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
lewis base
Molar solubility
Avagadros number
Nonpolar covalent bond
23. 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
24. E=hc/?
Net ionic equation
electromagnetic energy of photons emmited from electrons at ground state
Collision theory of chemical Kinetics
Molarity
25. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
subshell
Nonpolar covalent bond
The bohr model
solvation
26. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
Avagadros number
Equivalence point
London forces
27. 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.
electron configuration
Graham's Law
Formal Charge
VSEPR
28. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
pi bonds
Percent yield
Intermolecular forces
29. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
30. A reaction where a compound does Not change its molecular structure.
Activation energy
Alkaline earths
physical reaction
single displacement reaction
31. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
amorphous solid
Equilibrium
Electrolyte
sigma bond
32. The percent by mass of each element in a compound
Phase diagram
electron affinity
percent composition
Triple point
33. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Group 3A
transition elements
Rate determining step
atomic radius
34. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Formal Charge
Balmer series
Planck's Constant
35. The slowest elementary step which is the limit for the rate of the other steps
Le chateliers Principle
Rate determining step
indicator
redox reaction
36. A reaction in which atoms of one element take the place of atoms of another element in a compound
Formal Charge
Balmer series
single displacement reaction
quantum numbers
37. 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
Octet Rule
Nonpolar covalent bond
Water dissociation Constant
Ionization energy
38. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
Molality
Neutralization reaction
Charles and Gay Lussac's Law
39. Chalcogens - - Oxide O
sigma bond
Percent composition
Normality
Group 6A
40. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Proton
electron configuration
Net ionic equation
Resonance structure
41. 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
Neutron
Disproportionation
Magnetic quantum number
Collision theory of chemical Kinetics
42. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
subshell
angular momentum in the bohr model
Henry's Law
43. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
lathanide series
Solute
Lyman series
44. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Disproportionation
Ion
Octet Rule
Rydberg constant
45. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Molar solubility
Group 6A
Group 1A
46. 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.
Covalent Bond
Le chateliers Principle
Henderson Hasselbalch Equation
Bronsted Lowry
47. Named after their cation and anion
ionic cmpound
Ionic Bond
Molality
Charles and Gay Lussac's Law
48. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Phase diagram
Group 7A
atomic radius
49. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Electrolyte
Molar solubility
Resonance structure
empirical formula
50. Simplest whole # ration of atoms in a compound
Halogens
s orbital
Emperical Formula
Phase diagram