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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. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
mole
Le chateliers Principle
STP
Charles and Gay Lussac's Law
2. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Equilibrium
Titration
atomic radius
Free radical
3. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Rate determining step
electron affinity
Water dissociation Constant
heisenberg uncertainty principle
4. 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
Activation energy
Phase diagram
angular momentum in the bohr model
5. 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.
atomic radius
Group 6A
Decomposition reaction
Phase diagram
6. 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
Raoult's Law
Equivalence point
Formal Charge
angular momentum in the bohr model
7. 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-
Rydberg constant
hydrogen bonding
Chemical Kinetics
Water dissociation Constant
8. 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
percent composition
Resonance structure
Bronsted - Lowry definition
9. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Phase diagram
actinide series
Ionization energy
Decomposition reaction
10. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Rate determining step
s orbital
Solubility Product Constant
Noble gases
11. 5 different orbitals shaped like clover leaves and max electrons is 10
Noble gases
theoretical yield
Molar solubility
d orbital
12. 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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13. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Intermolecular forces
Neutron
Raoult's Law
14. A horizontal row of elements in the periodic table
Lyman series
Period
gram equivalent weight
Strong acid
15. A substance that - when dissolved in water - results in a solution that can conduct electricity
Nucleus
periodic trends
Ion dipole interactions
Electrolyte
16. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin
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17. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Balmer series
pH
Raoult's Law
18. Sum of the protons and neutrons in an element often denoted by the letter A
Combination Reaction
Collision theory of chemical Kinetics
single displacement reaction
Mass number
19. A reaction in which atoms of one element take the place of atoms of another element in a compound
Electronegativity
single displacement reaction
Dipole
Redox Half Reaction
20. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Redox Half Reaction
Nucleus
transition elements
Balmer series
21. 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
Water dissociation Constant
Group 5A
Azeotrope
Raoult's Law
22. 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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23. 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
atomic emission spectrum
und's rule
Collision theory of chemical Kinetics
24. 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
Disproportionation
Raoult's Law
Phase diagram
25. The lowest allowable energy state of an atom
Ground state
physical reaction
Ion
Dispersion Forces
26. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
molecular weight
Combination Reaction
Colligative properties
Vapor pressure
27. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
chemical reaction
Disproportionation
lewis base
28. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
compound
Disproportionation
Group 2A
Chemical Kinetics
29. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Dipole Dipole interaction
bond energy
polymer
30. Named after their cation and anion
ionic cmpound
quantum
Halogens
Effusion
31. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
crystalline solid
VSEPR
Theoretical yield
Collision theory of chemical Kinetics
32. The process by which one or more substances change to produce one or more different substances
electron configuration
Reaction order
chemical reaction
Ground state
33. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
law of constant composition
Avagadros number
Water dissociation Constant
Strong acid
34. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Electrolyte
Normality
Water dissociation Constant
STP
35. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Chemical Kinetics
indicator
hydrogen bonding
Collision theory of chemical Kinetics
36. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Solution equilibrium
Covalent Bond
Halogens
Triple point
37. Having characteristics of both an acid and a base and capable of reacting as either
Reaction mechanism
Titration
Amphoteric
Atomic weight
38. 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
pi bonds
Concentration
Diprotic Base
39. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
electron affinity
Formal Charge
VSEPR
40. 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
Octet Rule
hydrogen bonding
Henry's Law
41. (chemistry) p(otential of) H(ydrogen)
Theoretical yield
Group 7A
pH
Pauli exclusion principle
42. 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
VSEPR
The bohr model
ionic cmpound
molecular weight
43. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Theoretical yield
Henry's Law
Disproportionation
44. Tells you how much solute is present compared to the amount of solvent
Concentration
single displacement reaction
Period
Molality
45. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
physical reaction
Lewis acid base reaction
Net ionic equation
Ionic Bond
46. 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
Arrhenius Definition
Percent composition
Group 7A
Equilibrium
47. 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
Net ionic equation
decomposition reaction
Titration
molecule
48. 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
Raoult's Law
electromagnetic energy of photons emmited from electrons at ground state
Equlibrium constant
Solution equilibrium
49. 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
Normality
s orbital
Titration
Reaction mechanism
50. 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
atomic radius
Resonance structure
Ion
Network covalent