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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. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
heisenberg uncertainty principle
Colligative properties
Diffusion
empirical formula
2. 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.
Neutron
Solubility Product Constant
Lewis structure
Spin quantum number
3. 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.
VSEPR
Arrhenius Definition
Proton
Solubility Product Constant
4. Chalcogens - - Oxide O
Group 6A
Dipole
Group 7A
Group 5A
5. The average distance between the nuclei of two bonded atoms
Percent yield
Atomic weight
Formal Charge
bond length
6. The lowest allowable energy state of an atom
Effusion
ionic cmpound
bond energy
Ground state
7. 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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8. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Bronsted - Lowry definition
und's rule
Ground state
9. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Hydrogen bonding
Equivalence point
Aqueous Solution
Group 2A
10. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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11. A solution in which water is the solvent
Aqueous Solution
subshell
Theoretical yield
Bronsted Lowry
12. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
Atomic weight
Diprotic Base
Combination Reaction
13. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Group 7A
single displacement reaction
gram equivalent weight
Graham's Law
14. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points
pi bonds
Chemical Kinetics
Azeotrope
London forces
15. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
bond energy
Formula weight
theoretical yield
Nonpolar covalent bond
16. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Amphoteric
Planck's Constant
Noble gases
17. 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
Magnetic quantum number
polymer
Neutralization reaction
Diprotic Base
18. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Solubility Product Constant
amorphous solid
Electrolyte
19. 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
Noble gases
ionic cmpound
Ionization energy
Halogens
20. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Emperical Formula
pi bonds
Bronsted Lowry
Reaction mechanism
21. A reaction in which atoms of one element take the place of atoms of another element in a compound
crystalline solid
indicator
single displacement reaction
Net ionic equation
22. The energy required to break a chemical bond and form neutral isolated atoms
Equivalence point
Buffer
Alkaline earths
bond energy
23. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
d orbital
Dipole
Raoult's Law
Network covalent
24. Elements in the middle of the periodic table - in groups 3-12.
transition elements
bond length
electromagnetic energy of photons emmited from electrons at ground state
London forces
25. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Nonpolar covalent bond
Molality
Ground state
Percent composition
26. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Raoult's Law
Diffusion
Noble gases
Magnetic quantum number
27. 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
Rate determining step
bond length
d orbital
Dispersion Forces
28. 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
Formal Charge
Nucleus
s orbital
amorphous solid
29. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Nucleus
quantum
atomic emission spectrum
Lewis acid base reaction
30. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Equivalence point
Percent yield
Molar solubility
31. Simplest whole # ration of atoms in a compound
Dipole Dipole interaction
Ionization energy
Emperical Formula
Effective nuclear charge
32. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Normality
pI
Vapor pressure
Le chateliers Principle
33. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Decomposition reaction
Resonance structure
Atomic absorption Spectra
34. The process by which one or more substances change to produce one or more different substances
Normality
Half equivalence point
Group 2A
chemical reaction
35. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Formula weight
Half equivalence point
Lewis structure
Mass number
36. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Effective nuclear charge
Magnetic quantum number
Half equivalence point
electron affinity
37. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
Principle quantum number
Ionization energy
atomic radius
bond length
38. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
single displacement reaction
Ground state
Octet Rule
39. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
London forces
Lewis acid base reaction
Equivalence point
bond length
40. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Group 4A
Electrolyte
pi bonds
pH
41. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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42. Acids defined as electron - pair acceptors and bases as electron - pair donors.
atomic emission spectrum
Formal Charge
Emperical Formula
Lewis definition
43. 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.
Principle quantum number
atomic radius
Lyman series
Le chateliers Principle
44. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Molality
redox reaction
Bronsted Lowry
Solute
45. 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
heisenberg uncertainty principle
s orbital
Dispersion Forces
Rate law
46. 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
Magnetic quantum number
Net ionic equation
Resonance structure
percent composition
47. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
atomic theory
sigma bond
Half equivalence point
48. Common definition of acids as proton (H+) donors and bases as proton acceptors
chemical reaction
molecular weight
physical reaction
Bronsted - Lowry definition
49. 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
Ionic Bond
indicator
Neutron
Chemical Kinetics
50. A definite stable energy that a physical system can have
Activation energy
Octet Rule
Formal Charge
energy state