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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. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Percent composition
Phase diagram
Buffer
2. 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
Electrolyte
Acid dissociation constant
Pauli exclusion principle
subshell
3. An elementary particle with 0 charge and mass about equal to a proton
Atomic absorption Spectra
polymer
Neutron
Rydberg constant
4. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
atomic radius
Electronegativity
Group 7A
heisenberg uncertainty principle
5. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Reaction order
Phase diagram
decomposition reaction
pi bonds
6. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
compound
single displacement reaction
lewis base
Vapor pressure
7. PH of a molecule at which it contains no net electric charge - isoelectric point.
Arrhenius Definition
pI
solvation
The bohr model
8. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Solubility Product Constant
Avagadros number
Effusion
Solution equilibrium
9. 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.
redox reaction
Normality
Henderson Hasselbalch Equation
Hydrogen bonding
10. A solution in which water is the solvent
Activation energy
Common ion effect
Bronsted - Lowry definition
Aqueous Solution
11. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Atomic weight
effective nuclear charge
decomposition reaction
Electronegativity
12. 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
electromagnetic energy of photons emmited from electrons at ground state
Azeotrope
pH
Alkaline earths
13. 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
Octet Rule
Intermolecular forces
single displacement reaction
Titration
14. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Colligative properties
Activation energy
Molarity
bond length
15. 5 valence electrons -3 ions - Nitride N
Group 5A
Solubility Product Constant
periodic trends
Water dissociation Constant
16. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Group 5A
atomic radius
Formal Charge
subshell
17. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
percent composition
Noble gases
Solute
Diffusion
18. 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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19. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Effective nuclear charge
molecular weight
Equivalence point
Solute
20. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
redox reaction
atomic theory
Triple point
Arrhenius Definition
21. Substance in which a solute is dissolved to form a solution
Solvent
Activation energy
STP
Strong acid
22. The process of decomposing a chemical compound by the passage of an electric current.
Strong acid
Reaction order
Ionization energy
electrolysis
23. The process by which one or more substances change to produce one or more different substances
Diffusion
Group 4A
atomic theory
chemical reaction
24. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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25. 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
Ion dipole interactions
Group 1A
Free radical
26. 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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27. 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
Collision theory of chemical Kinetics
Covalent Bond
Half equivalence point
actinide series
28. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
VSEPR
crystalline solid
atomic emission spectrum
Ionic Bond
29. The Percent by mass of each element in a compound.
Percent composition
Titration
Effusion
Buffer
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
The bohr model
Balmer series
percent composition
Lewis definition
31. 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.
Le chateliers Principle
Group 7A
Group 3A
heisenberg uncertainty principle
32. 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
Group 6A
Proton
Ground state
molecule
33. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
theoretical yield
Nonpolar covalent bond
Solubility Product Constant
34. The lowest allowable energy state of an atom
Atomic weight
Ground state
Strong acid
physical reaction
35. (chemistry) a substance that changes color to indicate the presence of some ion or substance
pH
Percent composition
indicator
Electrolyte
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.
Effective nuclear charge
Atomic weight
Group 2A
VSEPR
37. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Group 1A
Ionic Bond
London forces
Molecular orbital
38. A subdivision of an energy level in an atom. They are divided into orbitals.
Lewis structure
subshell
azimuthal quantum number
Intermolecular forces
39. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Ion
redox reaction
lewis base
Solution equilibrium
40. Rare earth element group (elements 58-71)
Planck's Constant
Group 6A
Group 4A
lathanide series
41. A dynamic condition in which two opposing changes occur at equal rates in a closed system
pI
Solute
Avagadros number
Equilibrium
42. 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
Equlibrium constant
Decomposition reaction
Collision theory of chemical Kinetics
lathanide series
43. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
transition elements
Neutron
redox reaction
solvation
44. (chemistry) p(otential of) H(ydrogen)
Acid dissociation constant
pH
theoretical yield
Principle quantum number
45. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Henry's Law
Period
compound
Chemical Kinetics
46. 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.
Disproportionation
Equivalence point
Lewis definition
Dipole Dipole interaction
47. A horizontal row of elements in the periodic table
Period
periodic trends
gram equivalent weight
Molecular orbital
48. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Ground state
Reaction order
Group 6A
s orbital
49. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Electrolyte
Chemical Kinetics
empirical formula
Henderson Hasselbalch Equation
50. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
The bohr model
Effusion
Intermolecular forces
Emperical Formula