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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. 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.
Redox Half Reaction
pi bonds
Lewis definition
Triple point
2. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
Ionization energy
angular momentum in the bohr model
atomic emission spectrum
Resonance structure
3. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Magnetic quantum number
Graham's Law
redox reaction
Group 6A
4. 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.
Strong acid
Lewis structure
Balmer series
Azeotrope
5. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
lewis base
effective nuclear charge
Acid dissociation constant
6. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Normality
Effusion
Rate determining step
Lewis definition
7. (chemistry) p(otential of) H(ydrogen)
Lewis structure
pH
ionic cmpound
bond energy
8. 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
Equilibrium
Activation energy
representative elements
sigma bond
9. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Half equivalence point
Equlibrium constant
energy state
Conjugate acids and Bases
10. 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
quantum
Ion dipole interactions
crystalline solid
11. 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
molecular weight
Neutralization reaction
amorphous solid
hydrogen bonding
12. Elements in the middle of the periodic table - in groups 3-12.
Reaction mechanism
transition elements
Percent yield
quantum numbers
13. Any sample of a given compound will contain the same elements in the identical mass ratio.
Group 7A
gram equivalent weight
law of constant composition
Strong acid
14. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Nonpolar covalent bond
The bohr model
Acid dissociation constant
Molecular orbital
15. 5 different orbitals shaped like clover leaves and max electrons is 10
Electrolyte
Decomposition reaction
d orbital
crystalline solid
16. 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
Normality
Decomposition reaction
Acid dissociation constant
Group 4A
17. The process of decomposing a chemical compound by the passage of an electric current.
Group 3A
electrolysis
Electrolyte
bond length
18. Slightly less reactive than alkali metals - comprise group II
Network covalent
Covalent Bond
Ion
Alkaline earths
19. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Free radical
Emperical Formula
Neutralization reaction
Reaction order
20. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Hydrogen bonding
The bohr model
Spin quantum number
Avagadros number
21. Small discrete increments of energy.
Normality
quanta
Halogens
Lewis acid base reaction
22. 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
Nucleus
Principle quantum number
Acid dissociation constant
lewis base
23. 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.
Solution equilibrium
Free radical
atomic radius
Triple point
24. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
single displacement reaction
law of constant composition
Water dissociation Constant
25. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Mass number
Period
Intermolecular forces
Network covalent
26. The maximum amount of product that can be produced from a given amount of reactant
VSEPR
Decomposition reaction
theoretical yield
Effusion
27. 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.
Molar solubility
Nucleus
gram equivalent weight
Henderson Hasselbalch Equation
28. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Henderson Hasselbalch Equation
Group 3A
compound
Alkaline earths
29. A base that can accept two moles of H+ per mole of itself (ex: SO4
Vapor pressure
Diprotic Base
Amphoteric
polymer
30. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
bond length
Intermolecular forces
und's rule
electron configuration
31. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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32. 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
compound
Percent yield
Half equivalence point
Network covalent
33. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
pH
redox reaction
Vapor pressure
lathanide series
34. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Water dissociation Constant
Molarity
Triple point
Percent composition
35. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
Conjugate acids and Bases
Graham's Law
Bronsted Lowry
36. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
quantum numbers
s orbital
Nonpolar covalent bond
Emperical Formula
37. A reaction in which atoms of one element take the place of atoms of another element in a compound
Octet Rule
Net ionic equation
single displacement reaction
Rydberg constant
38. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Solvent
Network covalent
angular momentum in the bohr model
amorphous solid
39. 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
Mass number
Spin quantum number
theoretical yield
Bronsted Lowry
40. Substance in which a solute is dissolved to form a solution
Solvent
Aqueous Solution
Pauli exclusion principle
Group 2A
41. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Titration
Dipole
angular momentum in the bohr model
Resonance structure
42. 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
effective nuclear charge
The bohr model
Henderson Hasselbalch Equation
energy state
43. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
redox reaction
atomic radius
empirical formula
Group 2A
44. Chalcogens - - Oxide O
Group 6A
Net ionic equation
d orbital
Avagadros number
45. The percent by mass of each element in a compound
Rate determining step
lewis base
molecular weight
percent composition
46. 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
Half equivalence point
s orbital
Decomposition reaction
Combination Reaction
47. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
solvation
Nucleus
Lewis structure
48. Simplest whole # ration of atoms in a compound
Net ionic equation
Dipole Dipole interaction
Emperical Formula
Alkaline earths
49. 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
Solution equilibrium
Free radical
50. 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.
Group 5A
Group 7A
London forces
Effective nuclear charge