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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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.
Diffusion
atomic theory
Emperical Formula
Solubility Product Constant
2. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
Aqueous Solution
ionic cmpound
Hydrogen bonding
Diprotic Base
3. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
molecular weight
atomic radius
Collision theory of chemical Kinetics
Net ionic equation
4. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
bond energy
Group 5A
Group 2A
Equivalence point
5. Tells you how much solute is present compared to the amount of solvent
energy state
heisenberg uncertainty principle
Rate law
Concentration
6. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
angular momentum in the bohr model
physical reaction
STP
single displacement reaction
7. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
quanta
Equilibrium
Concentration
Phase diagram
8. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
atomic radius
Activation energy
heisenberg uncertainty principle
Emperical Formula
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.
Henderson Hasselbalch Equation
Disproportionation
redox reaction
Ion dipole interactions
10. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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11. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
lathanide series
physical reaction
Alkaline earths
12. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
theoretical yield
molecule
Ionization energy
13. 5 valence electrons -3 ions - Nitride N
Collision theory of chemical Kinetics
Charles and Gay Lussac's Law
Group 5A
London forces
14. 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
redox reaction
d orbital
Arrhenius Definition
electromagnetic energy of photons emmited from electrons at ground state
15. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Diprotic Base
empirical formula
Net ionic equation
Lewis definition
16. The Percent by mass of each element in a compound.
Rate determining step
lathanide series
Percent composition
Effusion
17. 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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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
effective nuclear charge
Lewis structure
Octet Rule
Nucleus
19. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
lathanide series
The bohr model
Disproportionation
Halogens
20. 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
Acid dissociation constant
Intermolecular forces
Rate law
21. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture
Group 1A
Rydberg constant
Solution equilibrium
physical reaction
22. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Ion product
physical reaction
azimuthal quantum number
23. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Free radical
subshell
Formula weight
quantum
24. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Equivalence point
Bronsted Lowry
Resonance structure
molecular weight
25. 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
Azeotrope
Formal Charge
Charles and Gay Lussac's Law
angular momentum in the bohr model
26. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Solution equilibrium
Hydrogen bonding
redox reaction
27. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Effusion
lewis base
Strong acid
bond energy
28. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Group 3A
atomic radius
Azeotrope
Neutralization reaction
29. The process by which one or more substances change to produce one or more different substances
chemical reaction
Atomic absorption Spectra
Half equivalence point
Group 3A
30. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Solubility Product Constant
Rate law
polymer
Molality
31. 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
periodic trends
atomic radius
mole
32. The percent by mass of each element in a compound
Neutralization reaction
Pauli exclusion principle
electron affinity
percent composition
33. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
lathanide series
decomposition reaction
Reaction mechanism
Noble gases
34. A solution in which water is the solvent
Aqueous Solution
effective nuclear charge
energy state
atomic theory
35. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Lewis definition
gram equivalent weight
law of constant composition
Solute
36. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
mole
Molar solubility
Reaction order
azimuthal quantum number
37. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Electrolyte
atomic radius
Molarity
Group 3A
38. 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
Half equivalence point
Balmer series
Spin quantum number
Ion dipole interactions
39. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
hydrogen bonding
Rydberg constant
energy state
Conjugate acids and Bases
40. 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
Azeotrope
Intermolecular forces
Free radical
Bronsted Lowry
41. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
gram equivalent weight
electron configuration
Octet Rule
molecule
42. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
lathanide series
Combination Reaction
Alkaline earths
Proton
43. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
electrolysis
Disproportionation
effective nuclear charge
Theoretical yield
44. An ionic compound that resists changes in its pH
molecular weight
Solution equilibrium
Buffer
Nucleus
45. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Azeotrope
Water dissociation Constant
Electronegativity
Diffusion
46. The average distance between the nuclei of two bonded atoms
law of constant composition
Azeotrope
Ion product
bond length
47. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Free radical
decomposition reaction
Acid dissociation constant
48. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Solute
Redox Half Reaction
Dispersion Forces
Alkaline earths
49. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Disproportionation
Molality
pi bonds
Lewis structure
50. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Emperical Formula
redox reaction
hydrogen bonding
ionic cmpound
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