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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.
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 chemical bond that involves sharing a pair of electrons between atoms in a molecule
Group 4A
Covalent Bond
Buffer
Conjugate acids and Bases
2. The lowest allowable energy state of an atom
Ground state
Lewis structure
Octet Rule
Half equivalence point
3. 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.
Equivalence point
Raoult's Law
Decomposition reaction
Bronsted Lowry
4. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Dispersion Forces
Neutron
Group 2A
Equlibrium constant
5. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
amorphous solid
Free radical
electromagnetic energy of photons emmited from electrons at ground state
6. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Graham's Law
Alkaline earths
Ionic Bond
Conjugate acids and Bases
7. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
VSEPR
Common ion effect
Equlibrium constant
representative elements
8. Having characteristics of both an acid and a base and capable of reacting as either
Half equivalence point
Solute
Amphoteric
Solubility Product Constant
9. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Group 7A
Neutralization reaction
electromagnetic energy of photons emmited from electrons at ground state
Theoretical yield
10. 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
Electronegativity
Ion dipole interactions
Disproportionation
11. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Equilibrium
Hydrogen bonding
atomic radius
Halogens
12. 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
Rydberg constant
actinide series
Ion dipole interactions
13. 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
actinide series
empirical formula
Ionization energy
Solution equilibrium
14. 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
s orbital
subshell
Noble gases
Magnetic quantum number
15. 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
periodic trends
Hydrogen bonding
Phase diagram
amorphous solid
16. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
periodic trends
Conjugate acids and Bases
Lewis structure
Acid dissociation constant
17. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Electrolyte
Molar solubility
crystalline solid
bond energy
18. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Arrhenius Definition
Group 6A
s orbital
19. Any sample of a given compound will contain the same elements in the identical mass ratio.
Formula weight
Common ion effect
law of constant composition
Titration
20. 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-
Buffer
Atomic weight
Water dissociation Constant
Principle quantum number
21. 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
Solute
Combination Reaction
hydrogen bonding
Reaction order
22. PH of a molecule at which it contains no net electric charge - isoelectric point.
quanta
Ionic Bond
Molecular orbital
pI
23. 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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24. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
pI
Bronsted Lowry
STP
Group 5A
25. 5 different orbitals shaped like clover leaves and max electrons is 10
ionic cmpound
Period
Balmer series
d orbital
26. 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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27. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Solubility Product Constant
Lewis definition
quantum
Solute
28. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Electrolyte
Dipole Dipole interaction
Network covalent
sigma bond
29. Named after their cation and anion
periodic trends
representative elements
ionic cmpound
Water dissociation Constant
30. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
atomic theory
Equilibrium
Noble gases
Azeotrope
31. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
atomic radius
Noble gases
Charles and Gay Lussac's Law
Molality
32. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Diffusion
ionic cmpound
Octet Rule
STP
33. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Graham's Law
Collision theory of chemical Kinetics
Reaction mechanism
molecule
34. A solution in which water is the solvent
Vapor pressure
Buffer
Aqueous Solution
Pauli exclusion principle
35. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
compound
Free radical
Rydberg constant
36. 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.
Solubility Product Constant
Acid dissociation constant
Nonpolar covalent bond
atomic radius
37. 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
Intermolecular forces
Principle quantum number
Dispersion Forces
Group 2A
38. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Decomposition reaction
Common ion effect
heisenberg uncertainty principle
pi bonds
39. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Concentration
Percent composition
London forces
40. Redox reaction - in which the same species is both oxidized and reduced.
Avagadros number
Disproportionation
Pauli exclusion principle
Amphoteric
41. Gram equivalent weight of solute per liter of solution - often denoted by N.
electron configuration
Normality
Nonpolar covalent bond
Group 7A
42. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Resonance structure
Phase diagram
atomic emission spectrum
43. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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44. A horizontal row of elements in the periodic table
Period
Neutron
Equilibrium
Lewis acid base reaction
45. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Dipole
Redox Half Reaction
Pauli exclusion principle
Half equivalence point
46. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Reaction order
single displacement reaction
heisenberg uncertainty principle
Diprotic Base
47. Two or more atoms held together by covalent bonds
Graham's Law
Normality
molecule
heisenberg uncertainty principle
48. A substance that - when dissolved in water - results in a solution that can conduct electricity
Principle quantum number
single displacement reaction
Electrolyte
Avagadros number
49. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Network covalent
Henderson Hasselbalch Equation
Bronsted - Lowry definition
Dipole
50. The process by which one or more substances change to produce one or more different substances
atomic radius
Group 4A
chemical reaction
Solvent
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