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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. An atom or group of atoms that has a positive or negative charge
Molarity
periodic trends
Ion
Acid dissociation constant
2. 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
lathanide series
Collision theory of chemical Kinetics
Molarity
3. 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.
polymer
crystalline solid
redox reaction
Proton
4. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Resonance structure
mole
molecule
compound
5. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Chemical Kinetics
Theoretical yield
Effective nuclear charge
Decomposition reaction
6. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
Resonance structure
pI
Spin quantum number
7. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
electrolysis
Neutralization reaction
Group 1A
Formal Charge
8. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
chemical reaction
Rate law
Activation energy
Ionic Bond
9. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Activation energy
percent composition
und's rule
Molarity
10. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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11. The lowest allowable energy state of an atom
Net ionic equation
Ground state
Group 2A
Covalent Bond
12. PH of a molecule at which it contains no net electric charge - isoelectric point.
empirical formula
Neutron
Redox Half Reaction
pI
13. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Dipole Dipole interaction
Covalent Bond
Azeotrope
Atomic weight
14. A solid made up of particles that are not arranged in a regular pattern.
Group 7A
Dispersion Forces
Atomic absorption Spectra
amorphous solid
15. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Molecular orbital
Group 3A
Equilibrium
Colligative properties
16. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
single displacement reaction
Group 2A
solvation
lewis base
17. 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.
Theoretical yield
electron affinity
Halogens
Raoult's Law
18. In a solution - the substance that dissolves in the solvent
Solute
Equilibrium
Decomposition reaction
law of constant composition
19. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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20. 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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21. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
sigma bond
periodic trends
Graham's Law
Intermolecular forces
22. 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
Acid dissociation constant
Neutron
representative elements
Raoult's Law
23. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
bond length
Phase diagram
und's rule
Reaction mechanism
24. 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
transition elements
effective nuclear charge
Equilibrium
25. Named after their cation and anion
ionic cmpound
Effusion
Dipole
Hydrogen bonding
26. 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
crystalline solid
Period
Group 1A
representative elements
27. The Percent by mass of each element in a compound.
Percent composition
Redox Half Reaction
Electrolyte
Half equivalence point
28. The average distance between the nuclei of two bonded atoms
Atomic absorption Spectra
pi bonds
Decomposition reaction
bond length
29. 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
Colligative properties
Solute
Water dissociation Constant
30. Gram equivalent weight of solute per liter of solution - often denoted by N.
Amphoteric
sigma bond
Percent composition
Normality
31. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Rate law
Group 4A
Noble gases
Strong acid
32. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Solubility Product Constant
Hydrogen bonding
electron affinity
Molality
33. 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-
Water dissociation Constant
single displacement reaction
Chemical Kinetics
Atomic weight
34. A subdivision of an energy level in an atom. They are divided into orbitals.
molecule
Noble gases
subshell
electron affinity
35. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
chemical reaction
Colligative properties
Strong acid
percent composition
36. Common definition of acids as proton (H+) donors and bases as proton acceptors
Ion dipole interactions
Electronegativity
Bronsted - Lowry definition
Dipole Dipole interaction
37. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Effective nuclear charge
physical reaction
Net ionic equation
Conjugate acids and Bases
38. 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.
indicator
Phase diagram
Equlibrium constant
Equivalence point
39. 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
Dispersion Forces
Ion
Decomposition reaction
Molarity
40. A reaction where a compound does Not change its molecular structure.
Solvent
physical reaction
Rate law
percent composition
41. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
lewis base
Atomic absorption Spectra
Acid dissociation constant
42. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Halogens
London forces
Common ion effect
Le chateliers Principle
43. 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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44. A substance that - when dissolved in water - results in a solution that can conduct electricity
Group 2A
Electrolyte
atomic emission spectrum
Half equivalence point
45. Redox reaction - in which the same species is both oxidized and reduced.
STP
Disproportionation
compound
Percent yield
46. 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
redox reaction
Redox Half Reaction
Titration
Electronegativity
47. Sum of the protons and neutrons in an element often denoted by the letter A
Covalent Bond
Graham's Law
Le chateliers Principle
Mass number
48. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Normality
Dispersion Forces
sigma bond
Dipole
49. 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
Percent yield
transition elements
decomposition reaction
Molarity
50. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Graham's Law
Octet Rule
Theoretical yield
The bohr model