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MCAT Chemistry
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Study First
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 reaction in which atoms of one element take the place of atoms of another element in a compound
Colligative properties
single displacement reaction
Decomposition reaction
Dipole
2. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
subshell
Electronegativity
Neutralization reaction
lewis base
3. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
quantum
Ionization energy
pH
4. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
d orbital
Mass number
Henderson Hasselbalch Equation
5. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 5A
Chemical Kinetics
Decomposition reaction
Group 2A
6. 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
Group 5A
ionic cmpound
Lewis definition
Nucleus
7. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
molecular weight
Proton
Ground state
Noble gases
8. 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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9. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Group 6A
Solute
Octet Rule
10. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
Octet Rule
Percent composition
Group 4A
11. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Dispersion Forces
Solute
Henderson Hasselbalch Equation
Net ionic equation
12. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Common ion effect
Group 7A
Colligative properties
atomic emission spectrum
13. 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
Percent composition
Mass number
Ionic Bond
14. 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.
Neutron
Atomic absorption Spectra
Rate law
Group 3A
15. A substance that - when dissolved in water - results in a solution that can conduct electricity
Group 7A
Octet Rule
Electrolyte
Effusion
16. Gram equivalent weight of solute per liter of solution - often denoted by N.
redox reaction
Halogens
Normality
Henry's Law
17. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
VSEPR
molecule
solvation
Effective nuclear charge
18. 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
Ionization energy
representative elements
electron configuration
quantum numbers
19. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Formal Charge
pi bonds
decomposition reaction
Molarity
20. 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
s orbital
Reaction mechanism
Acid dissociation constant
Chemical Kinetics
21. 2.18 x 10^-18 J/electron
atomic emission spectrum
Rydberg constant
bond energy
theoretical yield
22. 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.
Amphoteric
Phase diagram
atomic radius
Halogens
23. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Dipole Dipole interaction
redox reaction
gram equivalent weight
Concentration
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
actinide series
Ionization energy
pi bonds
Nonpolar covalent bond
25. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
mole
lathanide series
quanta
26. Elements in the middle of the periodic table - in groups 3-12.
actinide series
Aqueous Solution
Acid dissociation constant
transition elements
27. Chalcogens - - Oxide O
lewis base
Group 6A
Phase diagram
Molecular orbital
28. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Combination Reaction
Chemical Kinetics
empirical formula
Electronegativity
29. 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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30. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
Group 1A
Bronsted - Lowry definition
single displacement reaction
31. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
Normality
lewis base
azimuthal quantum number
polymer
32. The Percent by mass of each element in a compound.
Network covalent
electromagnetic energy of photons emmited from electrons at ground state
Period
Percent composition
33. 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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34. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
Group 5A
Raoult's Law
Spin quantum number
35. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Half equivalence point
Molarity
Group 1A
36. E=hc/?
Formula weight
electromagnetic energy of photons emmited from electrons at ground state
Solubility Product Constant
Atomic absorption Spectra
37. A base that can accept two moles of H+ per mole of itself (ex: SO4
Colligative properties
Buffer
Diprotic Base
Noble gases
38. An elementary particle with 0 charge and mass about equal to a proton
Neutron
VSEPR
Intermolecular forces
Hydrogen bonding
39. (chemistry) a substance that changes color to indicate the presence of some ion or substance
atomic emission spectrum
decomposition reaction
pH
indicator
40. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Equlibrium constant
VSEPR
Electronegativity
Triple point
41. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
atomic radius
Conjugate acids and Bases
Proton
Strong acid
42. Having characteristics of both an acid and a base and capable of reacting as either
Rate law
Reaction mechanism
Amphoteric
representative elements
43. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
Bronsted - Lowry definition
Electrolyte
Water dissociation Constant
44. A horizontal row of elements in the periodic table
Period
single displacement reaction
Hydrogen bonding
Emperical Formula
45. Named after their cation and anion
Arrhenius Definition
ionic cmpound
Avagadros number
Lyman series
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
Hydrogen bonding
transition elements
Amphoteric
single displacement reaction
47. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Ion product
d orbital
Ion
48. 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
gram equivalent weight
Intermolecular forces
lathanide series
49. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Concentration
Henderson Hasselbalch Equation
molecular weight
50. Small discrete increments of energy.
quanta
Proton
chemical reaction
molecule
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