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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 maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Formal Charge
Common ion effect
molecule
2. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Colligative properties
electromagnetic energy of photons emmited from electrons at ground state
Noble gases
Vapor pressure
3. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Vapor pressure
pi bonds
Halogens
periodic trends
4. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Group 3A
mole
Diffusion
electromagnetic energy of photons emmited from electrons at ground state
5. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
representative elements
decomposition reaction
Redox Half Reaction
Principle quantum number
6. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Net ionic equation
Effusion
Ion
Vapor pressure
7. 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.
Conjugate acids and Bases
Spin quantum number
Bronsted Lowry
crystalline solid
8. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
gram equivalent weight
periodic trends
molecule
quantum
9. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Diffusion
Noble gases
Equlibrium constant
10. 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.
Half equivalence point
Molarity
Group 6A
Group 3A
11. 2.18 x 10^-18 J/electron
Rydberg constant
Ion product
Lewis structure
Ionic Bond
12. 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.
theoretical yield
Redox Half Reaction
actinide series
Amphoteric
13. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Titration
gram equivalent weight
energy state
14. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
representative elements
atomic theory
Chemical Kinetics
15. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Titration
Buffer
Alkaline earths
16. 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
Water dissociation Constant
Equlibrium constant
Activation energy
Formula weight
17. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
quantum
Combination Reaction
physical reaction
Neutralization reaction
18. 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
Lewis acid base reaction
Acid dissociation constant
Atomic weight
19. An elementary particle with 0 charge and mass about equal to a proton
Electrolyte
Magnetic quantum number
Neutron
redox reaction
20. 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
Solution equilibrium
crystalline solid
Mass number
Rate law
21. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
lathanide series
chemical reaction
gram equivalent weight
22. 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
quantum numbers
Proton
Atomic weight
atomic radius
23. 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
polymer
Acid dissociation constant
Nucleus
lathanide series
24. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Reaction mechanism
Group 3A
transition elements
25. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Solute
Normality
Group 7A
compound
26. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
Alkaline earths
Noble gases
physical reaction
27. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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28. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Activation energy
Dipole Dipole interaction
Electronegativity
Percent yield
29. 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
Emperical Formula
Strong acid
Half equivalence point
Magnetic quantum number
30. 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
quanta
Equivalence point
Dispersion Forces
Group 4A
31. 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
Spin quantum number
Mass number
Charles and Gay Lussac's Law
electron configuration
32. Property of the elements that can be predicted from the arrangement of the periodic table
Bronsted Lowry
mole
periodic trends
Half equivalence point
33. The average distance between the nuclei of two bonded atoms
The bohr model
Aqueous Solution
energy state
bond length
34. Having characteristics of both an acid and a base and capable of reacting as either
Avagadros number
Group 7A
Conjugate acids and Bases
Amphoteric
35. 5 different orbitals shaped like clover leaves and max electrons is 10
Rydberg constant
Equlibrium constant
d orbital
Ionization energy
36. A reaction where a compound does Not change its molecular structure.
redox reaction
physical reaction
Molar solubility
Diprotic Base
37. Redox reaction - in which the same species is both oxidized and reduced.
Magnetic quantum number
Disproportionation
Half equivalence point
Titration
38. Small discrete increments of energy.
Normality
quanta
indicator
bond length
39. The slowest elementary step which is the limit for the rate of the other steps
Disproportionation
Rate determining step
Triple point
Nonpolar covalent bond
40. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Raoult's Law
solvation
Effective nuclear charge
Intermolecular forces
41. Gram equivalent weight of solute per liter of solution - often denoted by N.
Redox Half Reaction
Ion
Emperical Formula
Normality
42. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Resonance structure
effective nuclear charge
Triple point
heisenberg uncertainty principle
43. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Neutron
decomposition reaction
hydrogen bonding
transition elements
44. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Conjugate acids and Bases
Ionic Bond
Group 4A
Magnetic quantum number
45. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
sigma bond
redox reaction
Ionic Bond
chemical reaction
46. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
Conjugate acids and Bases
Triple point
Percent yield
47. 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
Hydrogen bonding
Ground state
redox reaction
48. E=hc/?
Equivalence point
Vapor pressure
Water dissociation Constant
electromagnetic energy of photons emmited from electrons at ground state
49. 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.
Henderson Hasselbalch Equation
Period
Nonpolar covalent bond
Normality
50. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
crystalline solid
polymer
lewis base
single displacement reaction