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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. An elementary particle with 0 charge and mass about equal to a proton
quantum numbers
Rate law
energy state
Neutron
2. 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
hydrogen bonding
The bohr model
Chemical Kinetics
percent composition
3. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
atomic emission spectrum
Molarity
sigma bond
Net ionic equation
4. 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
Proton
Solvent
lewis base
Solute
5. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
Equlibrium constant
polymer
Magnetic quantum number
6. Rare earth element group (elements 58-71)
actinide series
lathanide series
Henry's Law
Combination Reaction
7. The process of decomposing a chemical compound by the passage of an electric current.
Henderson Hasselbalch Equation
polymer
electrolysis
Rydberg constant
8. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Normality
periodic trends
bond length
9. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
energy state
Common ion effect
Net ionic equation
10. Temperature is constant; effusion and temperature are proportional to the square root of their masses
11. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Proton
Chemical Kinetics
Effusion
Pauli exclusion principle
12. A reaction in which atoms of one element take the place of atoms of another element in a compound
Equivalence point
single displacement reaction
law of constant composition
transition elements
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
Collision theory of chemical Kinetics
Molar solubility
Equilibrium
14. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Titration
gram equivalent weight
Normality
15. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Molecular orbital
Ion dipole interactions
Phase diagram
Intermolecular forces
16. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Atomic weight
Formal Charge
Conjugate acids and Bases
angular momentum in the bohr model
17. Common definition of acids as proton (H+) donors and bases as proton acceptors
physical reaction
quanta
Bronsted - Lowry definition
Intermolecular forces
18. The percent by mass of each element in a compound
Ion dipole interactions
percent composition
Redox Half Reaction
bond energy
19. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Dipole Dipole interaction
Bronsted - Lowry definition
Avagadros number
20. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
empirical formula
Vapor pressure
atomic theory
amorphous solid
21. Simplest whole # ration of atoms in a compound
Halogens
Emperical Formula
Effusion
Intermolecular forces
22. A horizontal row of elements in the periodic table
Triple point
Net ionic equation
transition elements
Period
23. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Triple point
Emperical Formula
Percent composition
24. Having characteristics of both an acid and a base and capable of reacting as either
Solution equilibrium
Amphoteric
Water dissociation Constant
polymer
25. A subdivision of an energy level in an atom. They are divided into orbitals.
Ionic Bond
Net ionic equation
subshell
Group 5A
26. Redox reaction - in which the same species is both oxidized and reduced.
Resonance structure
Concentration
theoretical yield
Disproportionation
27. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
periodic trends
Halogens
Colligative properties
sigma bond
28. E=hc/?
Le chateliers Principle
und's rule
electromagnetic energy of photons emmited from electrons at ground state
Disproportionation
29. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
30. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Diprotic Base
Lewis definition
electron configuration
Colligative properties
31. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
subshell
Colligative properties
Ion dipole interactions
Solute
32. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
periodic trends
Noble gases
Titration
actinide series
33. Elements in the middle of the periodic table - in groups 3-12.
Rate determining step
Spin quantum number
Chemical Kinetics
transition elements
34. The lowest allowable energy state of an atom
Resonance structure
Ground state
Rate law
Effective nuclear charge
35. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Molecular orbital
Percent yield
Nonpolar covalent bond
crystalline solid
36. Chalcogens - - Oxide O
Group 6A
Solvent
pi bonds
Normality
37. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Net ionic equation
Bronsted - Lowry definition
law of constant composition
38. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
indicator
subshell
Aqueous Solution
atomic theory
39. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
und's rule
Rate law
Lewis structure
Decomposition reaction
40. 5 different orbitals shaped like clover leaves and max electrons is 10
s orbital
Phase diagram
d orbital
electron affinity
41. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Decomposition reaction
pH
Half equivalence point
42. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
lathanide series
Neutron
Halogens
43. 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
Electronegativity
Resonance structure
Solute
amorphous solid
44. Named after their cation and anion
Decomposition reaction
Effusion
Henderson Hasselbalch Equation
ionic cmpound
45. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
indicator
Neutralization reaction
effective nuclear charge
Decomposition reaction
46. 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
47. 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.
Molarity
atomic radius
Ground state
lathanide series
48. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Formal Charge
Effective nuclear charge
Disproportionation
atomic emission spectrum
49. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
Principle quantum number
compound
hydrogen bonding
chemical reaction
50. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
atomic radius
Dispersion Forces
pH
Collision theory of chemical Kinetics