SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Ion
indicator
Alkaline earths
redox reaction
2. 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
Ion
Half equivalence point
single displacement reaction
Balmer series
3. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
theoretical yield
Molarity
Common ion effect
Planck's Constant
4. 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
azimuthal quantum number
Nucleus
Magnetic quantum number
Atomic absorption Spectra
5. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
redox reaction
Covalent Bond
pi bonds
subshell
6. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
azimuthal quantum number
Vapor pressure
Henderson Hasselbalch Equation
molecular weight
7. A horizontal row of elements in the periodic table
Period
sigma bond
Nonpolar covalent bond
Activation energy
8. 2.18 x 10^-18 J/electron
STP
Group 7A
Rydberg constant
pI
9. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Network covalent
Group 4A
heisenberg uncertainty principle
Dipole
10. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Atomic absorption Spectra
Common ion effect
Ionic Bond
Ion
11. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Planck's Constant
effective nuclear charge
physical reaction
12. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
compound
Diffusion
Mass number
Ion product
13. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Intermolecular forces
Triple point
Period
Mass number
14. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Equlibrium constant
compound
Molecular orbital
atomic theory
15. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Atomic absorption Spectra
Octet Rule
Normality
decomposition reaction
16. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Amphoteric
Reaction mechanism
representative elements
Dipole Dipole interaction
17. 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
Dispersion Forces
Octet Rule
Dipole
Graham's Law
18. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Decomposition reaction
single displacement reaction
indicator
Mass number
19. A subdivision of an energy level in an atom. They are divided into orbitals.
compound
subshell
electromagnetic energy of photons emmited from electrons at ground state
electron affinity
20. A definite stable energy that a physical system can have
atomic radius
Acid dissociation constant
energy state
Strong acid
21. 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
Percent yield
bond energy
Avagadros number
decomposition reaction
22. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
Hydrogen bonding
Group 2A
Charles and Gay Lussac's Law
23. An elementary particle with 0 charge and mass about equal to a proton
atomic emission spectrum
bond length
quantum
Neutron
24. 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
Graham's Law
representative elements
Resonance structure
Ground state
25. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
bond length
Equilibrium
crystalline solid
redox reaction
26. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
crystalline solid
bond length
Atomic weight
empirical formula
27. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Ion product
Electrolyte
ionic cmpound
Phase diagram
28. 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
Triple point
Ionization energy
indicator
Titration
29. Named after their cation and anion
s orbital
Decomposition reaction
Azeotrope
ionic cmpound
30. The process of decomposing a chemical compound by the passage of an electric current.
angular momentum in the bohr model
Graham's Law
Rate law
electrolysis
31. In a solution - the substance that dissolves in the solvent
Decomposition reaction
effective nuclear charge
Network covalent
Solute
32. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
subshell
Molality
Molar solubility
Electronegativity
33. 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.
ionic cmpound
solvation
Group 3A
Equivalence point
34. 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.
periodic trends
atomic radius
Conjugate acids and Bases
Phase diagram
35. Having characteristics of both an acid and a base and capable of reacting as either
pi bonds
Amphoteric
Net ionic equation
atomic radius
36. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
molecule
pi bonds
energy state
37. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
pH
Formal Charge
Molality
quantum
38. (chemistry) p(otential of) H(ydrogen)
Henry's Law
Spin quantum number
pH
Period
39. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Equlibrium constant
Acid dissociation constant
atomic radius
Reaction order
40. Gram equivalent weight of solute per liter of solution - often denoted by N.
STP
The bohr model
Collision theory of chemical Kinetics
Normality
41. 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.
Emperical Formula
Group 3A
molecular weight
Principle quantum number
42. Common definition of acids as proton (H+) donors and bases as proton acceptors
Titration
Bronsted - Lowry definition
Avagadros number
solvation
43. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
law of constant composition
Magnetic quantum number
Ionization energy
sigma bond
44. Simplest whole # ration of atoms in a compound
Pauli exclusion principle
redox reaction
Emperical Formula
Neutralization reaction
45. Substance in which a solute is dissolved to form a solution
Emperical Formula
Graham's Law
Rate determining step
Solvent
46. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Normality
Disproportionation
Henry's Law
Molecular orbital
47. 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
indicator
Colligative properties
Bronsted - Lowry definition
Electronegativity
48. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
actinide series
Ion
Group 6A
49. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Group 1A
Octet Rule
Lewis structure
Electronegativity
50. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
Proton
Arrhenius Definition
gram equivalent weight
Percent composition