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Test your basic knowledge |
MCAT Chemistry
Start Test
Study First
Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
Period
pH
Solubility Product Constant
quantum numbers
2. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Molality
redox reaction
Electronegativity
representative elements
3. Common definition of acids as proton (H+) donors and bases as proton acceptors
heisenberg uncertainty principle
Molar solubility
Theoretical yield
Bronsted - Lowry definition
4. 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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5. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Bronsted - Lowry definition
chemical reaction
Nonpolar covalent bond
Emperical Formula
6. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Spin quantum number
energy state
Atomic absorption Spectra
Neutralization reaction
7. 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
Normality
Ion dipole interactions
lewis base
8. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Ion
Buffer
Common ion effect
Decomposition reaction
9. 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
electrolysis
Electrolyte
Period
representative elements
10. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
atomic emission spectrum
Nonpolar covalent bond
quantum
percent composition
11. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
mole
Halogens
Pauli exclusion principle
ionic cmpound
12. Named after their cation and anion
Graham's Law
Period
ionic cmpound
Strong acid
13. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
Theoretical yield
Avagadros number
Dispersion Forces
14. 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
Reaction mechanism
electron configuration
transition elements
15. A solution in which water is the solvent
Aqueous Solution
chemical reaction
Emperical Formula
atomic theory
16. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
Colligative properties
Formal Charge
hydrogen bonding
Arrhenius Definition
17. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Graham's Law
Arrhenius Definition
Halogens
18. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities
Nucleus
physical reaction
Normality
empirical formula
19. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
azimuthal quantum number
single displacement reaction
lewis base
Percent composition
20. 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
Solution equilibrium
Aqueous Solution
Group 7A
Group 5A
21. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
effective nuclear charge
Solvent
Proton
Le chateliers Principle
22. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
amorphous solid
Network covalent
Diprotic Base
Concentration
23. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Diffusion
polymer
Ion product
amorphous solid
24. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Theoretical yield
Ion
Effective nuclear charge
25. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Chemical Kinetics
Arrhenius Definition
Combination Reaction
Solute
26. The energy required to break a chemical bond and form neutral isolated atoms
Amphoteric
Formal Charge
polymer
bond energy
27. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ionization energy
Ion
electron affinity
Octet Rule
28. 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.
Ionic Bond
electron affinity
Colligative properties
Alkaline earths
29. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Effective nuclear charge
Covalent Bond
Ionic Bond
Graham's Law
30. 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
Ground state
quantum numbers
The bohr model
Vapor pressure
31. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Neutron
Colligative properties
Ionization energy
32. A definite stable energy that a physical system can have
Molar solubility
energy state
Acid dissociation constant
polymer
33. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Effective nuclear charge
Dispersion Forces
Principle quantum number
Combination Reaction
34. 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
Formula weight
bond energy
Percent yield
Ion dipole interactions
35. 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
lewis base
Ionization energy
Triple point
Dispersion Forces
36. 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.
Triple point
Activation energy
Effective nuclear charge
London forces
37. Slightly less reactive than alkali metals - comprise group II
Emperical Formula
s orbital
Diprotic Base
Alkaline earths
38. Gram equivalent weight of solute per liter of solution - often denoted by N.
Free radical
Normality
Formula weight
compound
39. An atom or group of atoms that has a positive or negative charge
Acid dissociation constant
Triple point
Ion
Dipole Dipole interaction
40. The Percent by mass of each element in a compound.
Ion
Percent composition
Molecular orbital
Electronegativity
41. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Ion product
Half equivalence point
Formal Charge
42. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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43. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Pauli exclusion principle
Formula weight
redox reaction
quanta
44. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
lewis base
Aqueous Solution
Electrolyte
45. 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
Spin quantum number
Titration
Common ion effect
angular momentum in the bohr model
46. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Equlibrium constant
Water dissociation Constant
Redox Half Reaction
47. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Chemical Kinetics
electron configuration
Molecular orbital
STP
48. An elementary particle with 0 charge and mass about equal to a proton
Acid dissociation constant
Triple point
Neutralization reaction
Neutron
49. Property of the elements that can be predicted from the arrangement of the periodic table
Network covalent
Octet Rule
periodic trends
electromagnetic energy of photons emmited from electrons at ground state
50. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Half equivalence point
Group 6A
Atomic weight
Nucleus