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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. (chemistry) a substance that changes color to indicate the presence of some ion or substance
representative elements
Noble gases
indicator
Decomposition reaction
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
hydrogen bonding
pI
Redox Half Reaction
Nonpolar covalent bond
3. In a solution - the substance that dissolves in the solvent
Solute
Acid dissociation constant
Covalent Bond
VSEPR
4. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
Solute
Aqueous Solution
Reaction order
5. 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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6. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Dispersion Forces
Group 2A
lewis base
Azeotrope
7. 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.
Normality
Network covalent
Balmer series
Group 3A
8. 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.
Neutron
Effective nuclear charge
chemical reaction
Atomic weight
9. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
molecular weight
pi bonds
Molality
London forces
10. 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
atomic radius
Rate determining step
Half equivalence point
Mass number
11. 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
Ionization energy
Molality
Diprotic Base
12. 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.
mole
sigma bond
law of constant composition
atomic radius
13. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Group 1A
solvation
sigma bond
14. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
Atomic absorption Spectra
Electronegativity
Group 7A
molecular weight
15. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Equivalence point
crystalline solid
Hydrogen bonding
Lewis definition
16. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Equlibrium constant
Strong acid
Decomposition reaction
Nonpolar covalent bond
17. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
Ion product
Henderson Hasselbalch Equation
pH
heisenberg uncertainty principle
18. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Chemical Kinetics
Ion
Solvent
percent composition
19. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
electrolysis
subshell
decomposition reaction
Noble gases
20. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Lewis structure
Molality
The bohr model
21. The average distance between the nuclei of two bonded atoms
Reaction order
bond length
Rate law
electron affinity
22. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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23. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
decomposition reaction
Net ionic equation
law of constant composition
Strong acid
24. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
London forces
Ionization energy
Atomic weight
Solute
25. 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.
Neutralization reaction
Henderson Hasselbalch Equation
Pauli exclusion principle
Common ion effect
26. The Percent by mass of each element in a compound.
atomic radius
Percent composition
Octet Rule
Equlibrium constant
27. (chemistry) p(otential of) H(ydrogen)
pH
effective nuclear charge
electromagnetic energy of photons emmited from electrons at ground state
decomposition reaction
28. 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
azimuthal quantum number
s orbital
Combination Reaction
decomposition reaction
29. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
pi bonds
Atomic weight
azimuthal quantum number
30. 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
representative elements
und's rule
Molecular orbital
31. A reaction where a compound does Not change its molecular structure.
chemical reaction
Vapor pressure
physical reaction
Ionic Bond
32. 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
Lyman series
Nucleus
Half equivalence point
Group 4A
33. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Vapor pressure
periodic trends
Acid dissociation constant
34. 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.
atomic emission spectrum
Spin quantum number
Strong acid
Solubility Product Constant
35. A dynamic condition in which two opposing changes occur at equal rates in a closed system
lewis base
d orbital
Equilibrium
representative elements
36. An atom or group of atoms that has a positive or negative charge
Alkaline earths
Ion
Neutralization reaction
Water dissociation Constant
37. Common definition of acids as proton (H+) donors and bases as proton acceptors
Covalent Bond
solvation
periodic trends
Bronsted - Lowry definition
38. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Conjugate acids and Bases
Molality
Atomic weight
Solvent
39. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Bronsted Lowry
Theoretical yield
electron affinity
law of constant composition
40. 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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41. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
redox reaction
gram equivalent weight
Percent composition
Theoretical yield
42. The process by which one or more substances change to produce one or more different substances
chemical reaction
Ion
Solvent
Dipole Dipole interaction
43. 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-
Ion product
theoretical yield
Ionization energy
Water dissociation Constant
44. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
London forces
Henderson Hasselbalch Equation
Activation energy
Emperical Formula
45. 2.18 x 10^-18 J/electron
Dispersion Forces
Rydberg constant
Free radical
Group 2A
46. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Resonance structure
Ion product
Planck's Constant
47. 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
Diffusion
Percent yield
Triple point
Azeotrope
48. 5 valence electrons -3 ions - Nitride N
redox reaction
Emperical Formula
Group 5A
electromagnetic energy of photons emmited from electrons at ground state
49. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
redox reaction
electron configuration
electromagnetic energy of photons emmited from electrons at ground state
Effusion
50. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Redox Half Reaction
Solvent
gram equivalent weight
polymer