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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. 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
angular momentum in the bohr model
lewis base
Spin quantum number
transition elements
2. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
transition elements
quanta
atomic radius
3. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Group 3A
compound
heisenberg uncertainty principle
atomic radius
4. 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
Ion
The bohr model
Group 4A
Raoult's Law
5. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Henderson Hasselbalch Equation
polymer
und's rule
Water dissociation Constant
6. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Reaction order
Phase diagram
Emperical Formula
indicator
7. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
pi bonds
Phase diagram
gram equivalent weight
polymer
8. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Normality
Nonpolar covalent bond
Diffusion
Group 3A
9. 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.
Formula weight
pi bonds
atomic radius
electron affinity
10. A definite stable energy that a physical system can have
energy state
Raoult's Law
azimuthal quantum number
Water dissociation Constant
11. Simplest whole # ration of atoms in a compound
Noble gases
Bronsted - Lowry definition
Emperical Formula
Diffusion
12. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Ion
actinide series
Effusion
13. 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.
Covalent Bond
crystalline solid
Diffusion
Concentration
14. The average distance between the nuclei of two bonded atoms
pH
Buffer
bond length
Rate determining step
15. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Azeotrope
Neutralization reaction
Group 2A
Intermolecular forces
16. A substance that - when dissolved in water - results in a solution that can conduct electricity
Reaction order
Intermolecular forces
Electrolyte
Percent yield
17. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
physical reaction
lewis base
sigma bond
Combination Reaction
18. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Equivalence point
redox reaction
Hydrogen bonding
molecular weight
19. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
d orbital
STP
Network covalent
20. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Lyman series
Nonpolar covalent bond
Chemical Kinetics
Emperical Formula
21. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
mole
Free radical
Ion
molecular weight
22. 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.
effective nuclear charge
ionic cmpound
gram equivalent weight
Henderson Hasselbalch Equation
23. 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.
Electronegativity
Effective nuclear charge
Lewis acid base reaction
Strong acid
24. 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.
Avagadros number
periodic trends
Redox Half Reaction
VSEPR
25. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
periodic trends
Ion product
London forces
Pauli exclusion principle
26. 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
decomposition reaction
Resonance structure
Diffusion
Formal Charge
27. In a solution - the substance that dissolves in the solvent
Solute
percent composition
periodic trends
Solvent
28. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Solubility Product Constant
indicator
decomposition reaction
Titration
29. 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
Azeotrope
Ionization energy
Lewis acid base reaction
Acid dissociation constant
30. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Redox Half Reaction
physical reaction
Ion
Intermolecular forces
31. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Aqueous Solution
Molality
Period
Halogens
32. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
redox reaction
Ion dipole interactions
mole
Conjugate acids and Bases
33. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Acid dissociation constant
Group 7A
quanta
34. E=hc/?
Octet Rule
Spin quantum number
Group 1A
electromagnetic energy of photons emmited from electrons at ground state
35. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Ground state
polymer
actinide series
36. Slightly less reactive than alkali metals - comprise group II
Reaction mechanism
Collision theory of chemical Kinetics
solvation
Alkaline earths
37. 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
Titration
Solubility Product Constant
Combination Reaction
single displacement reaction
38. 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
Equilibrium
Reaction mechanism
Percent yield
Normality
39. Temperature is constant; effusion and temperature are proportional to the square root of their masses
40. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
angular momentum in the bohr model
Lyman series
Henderson Hasselbalch Equation
Rate law
41. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
und's rule
pi bonds
Group 5A
42. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
pH
Alkaline earths
Electronegativity
43. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Mass number
solvation
Equilibrium
Covalent Bond
44. A horizontal row of elements in the periodic table
law of constant composition
Period
Titration
hydrogen bonding
45. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Free radical
energy state
quantum numbers
46. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
Theoretical yield
Le chateliers Principle
atomic radius
47. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
decomposition reaction
Molecular orbital
Noble gases
48. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher
ionic cmpound
Ground state
Formal Charge
Mass number
49. The Percent by mass of each element in a compound.
electron affinity
Solubility Product Constant
Percent composition
Henry's Law
50. A reaction in which atoms of one element take the place of atoms of another element in a compound
Normality
pH
Electronegativity
single displacement reaction