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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 ways in which electrons are arranged in various orbitals around the nuclei of atoms
Diprotic Base
electron configuration
Rydberg constant
Rate determining step
2. The slowest elementary step which is the limit for the rate of the other steps
heisenberg uncertainty principle
Colligative properties
Vapor pressure
Rate determining step
3. Chalcogens - - Oxide O
electromagnetic energy of photons emmited from electrons at ground state
solvation
Group 6A
chemical reaction
4. 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
Molar solubility
Percent yield
redox reaction
Solution equilibrium
5. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Effusion
atomic emission spectrum
Collision theory of chemical Kinetics
Group 4A
6. 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
Lyman series
Half equivalence point
quantum numbers
Network covalent
7. The process of decomposing a chemical compound by the passage of an electric current.
Concentration
atomic emission spectrum
bond length
electrolysis
8. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Arrhenius Definition
Group 4A
Group 1A
9. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Henry's Law
physical reaction
Noble gases
Vapor pressure
10. A solution in which water is the solvent
Strong acid
quantum numbers
Acid dissociation constant
Aqueous Solution
11. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
pI
Halogens
redox reaction
Solubility Product Constant
12. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
mole
Solvent
Activation energy
13. A reaction where a compound does Not change its molecular structure.
physical reaction
Reaction mechanism
single displacement reaction
Concentration
14. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
Molecular orbital
electrolysis
London forces
Covalent Bond
15. A definite stable energy that a physical system can have
Arrhenius Definition
Ion
amorphous solid
energy state
16. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Solvent
Ion
Lewis structure
Ion product
17. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Raoult's Law
Dipole
Alkaline earths
Ion dipole interactions
18. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Strong acid
Common ion effect
electron configuration
quantum
19. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Triple point
Period
sigma bond
Dispersion Forces
20. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Octet Rule
theoretical yield
Colligative properties
Phase diagram
21. 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.
Electrolyte
amorphous solid
Equivalence point
subshell
22. 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.
Net ionic equation
Ion product
Electronegativity
quantum numbers
23. 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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24. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
redox reaction
Group 1A
Theoretical yield
25. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Atomic absorption Spectra
electron affinity
Intermolecular forces
angular momentum in the bohr model
26. 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
chemical reaction
Molality
27. 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
Raoult's Law
Ion product
Spin quantum number
Diprotic Base
28. Named after their cation and anion
Alkaline earths
Combination Reaction
ionic cmpound
Titration
29. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Charles and Gay Lussac's Law
atomic radius
Concentration
decomposition reaction
30. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Nucleus
Avagadros number
Equlibrium constant
Graham's Law
31. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Normality
Bronsted Lowry
Group 3A
Network covalent
32. 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
Covalent Bond
single displacement reaction
und's rule
33. 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
Concentration
Reaction order
Hydrogen bonding
Conjugate acids and Bases
34. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
energy state
gram equivalent weight
Network covalent
Acid dissociation constant
35. 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.
chemical reaction
Period
Balmer series
Network covalent
36. 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.
bond length
Molecular orbital
Combination Reaction
Group 3A
37. Two or more atoms held together by covalent bonds
Rate law
molecule
chemical reaction
Disproportionation
38. Small discrete increments of energy.
Network covalent
Phase diagram
quanta
heisenberg uncertainty principle
39. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
transition elements
bond length
effective nuclear charge
Covalent Bond
40. 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-
Lewis acid base reaction
und's rule
effective nuclear charge
Water dissociation Constant
41. 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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42. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Formula weight
Intermolecular forces
Concentration
Vapor pressure
43. 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
Formal Charge
Group 1A
Acid dissociation constant
Equivalence point
44. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
quantum
sigma bond
transition elements
pH
45. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Period
Neutralization reaction
periodic trends
Henry's Law
46. 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
Reaction mechanism
Arrhenius Definition
hydrogen bonding
Group 6A
47. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Equlibrium constant
Balmer series
Nonpolar covalent bond
Free radical
48. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
quantum numbers
Ionization energy
Equivalence point
Net ionic equation
49. Slightly less reactive than alkali metals - comprise group II
Solubility Product Constant
Alkaline earths
d orbital
bond length
50. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Percent composition
The bohr model
Lewis acid base reaction
ionic cmpound