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Test your basic knowledge |
MCAT Chemistry
Start Test
Study First
Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
sigma bond
Noble gases
atomic theory
Effective nuclear charge
2. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutralization reaction
Electronegativity
angular momentum in the bohr model
Equivalence point
3. An ionic compound that resists changes in its pH
Buffer
bond length
d orbital
STP
4. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Rate determining step
Normality
indicator
mole
5. Sum of the protons and neutrons in an element often denoted by the letter A
Magnetic quantum number
hydrogen bonding
molecular weight
Mass number
6. Rare earth element group (elements 58-71)
Electrolyte
Atomic absorption Spectra
lathanide series
hydrogen bonding
7. PH of a molecule at which it contains no net electric charge - isoelectric point.
atomic theory
Resonance structure
pI
single displacement reaction
8. The process of decomposing a chemical compound by the passage of an electric current.
STP
Vapor pressure
representative elements
electrolysis
9. 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.
Spin quantum number
Equlibrium constant
bond length
Effective nuclear charge
10. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
London forces
redox reaction
Atomic weight
atomic theory
11. The lowest allowable energy state of an atom
Charles and Gay Lussac's Law
Chemical Kinetics
Ground state
und's rule
12. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Arrhenius Definition
Neutron
Chemical Kinetics
Group 6A
13. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Ionic Bond
Emperical Formula
effective nuclear charge
Atomic weight
14. Any sample of a given compound will contain the same elements in the identical mass ratio.
Ionic Bond
redox reaction
Percent yield
law of constant composition
15. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
VSEPR
periodic trends
indicator
Dipole Dipole interaction
16. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
chemical reaction
Half equivalence point
STP
Formal Charge
17. Slightly less reactive than alkali metals - comprise group II
mole
Net ionic equation
Rydberg constant
Alkaline earths
18. Property of the elements that can be predicted from the arrangement of the periodic table
Nucleus
periodic trends
Intermolecular forces
Group 2A
19. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
atomic radius
Chemical Kinetics
Bronsted Lowry
Group 2A
20. Common definition of acids as proton (H+) donors and bases as proton acceptors
Charles and Gay Lussac's Law
Raoult's Law
s orbital
Bronsted - Lowry definition
21. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Group 5A
Reaction mechanism
theoretical yield
Network covalent
22. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Effusion
compound
pI
Avagadros number
23. 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.
Decomposition reaction
Octet Rule
Group 3A
Graham's Law
24. A reaction where a compound does Not change its molecular structure.
quantum numbers
Atomic absorption Spectra
physical reaction
Rate determining step
25. 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
theoretical yield
Raoult's Law
Percent yield
Lyman series
26. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
chemical reaction
Ion dipole interactions
Aqueous Solution
Activation energy
27. Gram equivalent weight of solute per liter of solution - often denoted by N.
heisenberg uncertainty principle
Formula weight
Spin quantum number
Normality
28. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Titration
Rate determining step
Henderson Hasselbalch Equation
29. The average distance between the nuclei of two bonded atoms
representative elements
bond length
Effusion
Rate law
30. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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31. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Solution equilibrium
Combination Reaction
Molar solubility
Rydberg constant
32. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Conjugate acids and Bases
VSEPR
Charles and Gay Lussac's Law
Group 4A
33. A reaction in which atoms of one element take the place of atoms of another element in a compound
redox reaction
Equilibrium
single displacement reaction
mole
34. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Azeotrope
Collision theory of chemical Kinetics
pi bonds
Rydberg constant
35. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Principle quantum number
Diprotic Base
actinide series
36. Redox reaction - in which the same species is both oxidized and reduced.
mole
Disproportionation
Lewis definition
Activation energy
37. The percent by mass of each element in a compound
percent composition
Group 7A
Group 2A
d orbital
38. Chalcogens - - Oxide O
azimuthal quantum number
Effusion
Conjugate acids and Bases
Group 6A
39. Substance in which a solute is dissolved to form a solution
Rate determining step
Rate law
Activation energy
Solvent
40. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
electron affinity
Equilibrium
Group 1A
41. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
ionic cmpound
Group 7A
Ion
42. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
STP
Atomic absorption Spectra
Colligative properties
Graham's Law
43. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Vapor pressure
Lyman series
Group 2A
44. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Combination Reaction
Titration
Intermolecular forces
Reaction mechanism
45. 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
Covalent Bond
Group 7A
Ionization energy
Graham's Law
46. A definite stable energy that a physical system can have
Combination Reaction
Emperical Formula
Concentration
energy state
47. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
theoretical yield
redox reaction
compound
Combination Reaction
48. Simplest whole # ration of atoms in a compound
Solubility Product Constant
single displacement reaction
Emperical Formula
mole
49. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
STP
Phase diagram
single displacement reaction
Charles and Gay Lussac's Law
50. 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
VSEPR
Half equivalence point
Reaction mechanism
Proton