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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. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
Avagadros number
mole
Bronsted Lowry
2. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
electron affinity
Octet Rule
Chemical Kinetics
Mass number
3. 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.
Normality
periodic trends
Nonpolar covalent bond
atomic radius
4. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Triple point
Rate law
polymer
Lewis acid base reaction
5. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Alkaline earths
Water dissociation Constant
Lewis structure
solvation
6. Elements in the middle of the periodic table - in groups 3-12.
Electrolyte
The bohr model
Diprotic Base
transition elements
7. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Colligative properties
Amphoteric
d orbital
8. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Group 4A
Alkaline earths
single displacement reaction
9. 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-
Water dissociation Constant
atomic theory
Halogens
Aqueous Solution
10. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Atomic weight
decomposition reaction
Normality
London forces
11. A reaction where a compound does Not change its molecular structure.
physical reaction
Ion
bond energy
Ionization energy
12. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
electromagnetic energy of photons emmited from electrons at ground state
pH
pI
13. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Conjugate acids and Bases
atomic emission spectrum
Equlibrium constant
14. An ionic compound that resists changes in its pH
Solvent
Disproportionation
Buffer
Lewis acid base reaction
15. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Raoult's Law
gram equivalent weight
compound
heisenberg uncertainty principle
16. 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
Arrhenius Definition
Bronsted Lowry
bond energy
redox reaction
17. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
quanta
lathanide series
Ground state
Triple point
18. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
pi bonds
Solubility Product Constant
Dispersion Forces
Group 1A
19. The average distance between the nuclei of two bonded atoms
Covalent Bond
bond length
Dispersion Forces
Group 5A
20. Tells you how much solute is present compared to the amount of solvent
Charles and Gay Lussac's Law
Concentration
Percent composition
Henry's Law
21. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Neutron
STP
Concentration
Hydrogen bonding
22. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Reaction mechanism
Acid dissociation constant
Balmer series
23. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
periodic trends
Reaction order
Network covalent
24. 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
Amphoteric
Vapor pressure
Nucleus
Ion
25. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
gram equivalent weight
periodic trends
chemical reaction
effective nuclear charge
26. 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.
Equlibrium constant
Principle quantum number
Solubility Product Constant
Effusion
27. 2.18 x 10^-18 J/electron
electron configuration
Graham's Law
Rydberg constant
Group 6A
28. 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.
Network covalent
Azeotrope
Redox Half Reaction
Reaction order
29. The percent by mass of each element in a compound
percent composition
hydrogen bonding
redox reaction
Halogens
30. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Balmer series
azimuthal quantum number
atomic theory
31. (chemistry) a substance that changes color to indicate the presence of some ion or substance
atomic emission spectrum
VSEPR
indicator
amorphous solid
32. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Avagadros number
representative elements
redox reaction
Strong acid
33. 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
Phase diagram
Magnetic quantum number
Dispersion Forces
electron affinity
34. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
Solvent
crystalline solid
Phase diagram
mole
35. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
s orbital
transition elements
solvation
Proton
36. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
VSEPR
Group 3A
Lewis acid base reaction
Dipole Dipole interaction
37. 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
Effusion
Dipole
Decomposition reaction
Percent yield
38. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Hydrogen bonding
ionic cmpound
Chemical Kinetics
Water dissociation Constant
39. 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.
Amphoteric
Net ionic equation
Effective nuclear charge
Halogens
40. Chalcogens - - Oxide O
angular momentum in the bohr model
Dipole
Group 6A
chemical reaction
41. 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
und's rule
s orbital
Hydrogen bonding
Network covalent
42. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Molality
Rate determining step
Dipole
STP
43. Simplest whole # ration of atoms in a compound
Atomic absorption Spectra
physical reaction
Emperical Formula
Amphoteric
44. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Net ionic equation
Group 4A
atomic theory
Ion dipole interactions
45. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
STP
angular momentum in the bohr model
Theoretical yield
Azeotrope
46. PH of a molecule at which it contains no net electric charge - isoelectric point.
Group 1A
Acid dissociation constant
pI
Charles and Gay Lussac's Law
47. 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.
sigma bond
physical reaction
Ion product
Formal Charge
48. Named after their cation and anion
ionic cmpound
Group 2A
Bronsted - Lowry definition
Molar solubility
49. The process of decomposing a chemical compound by the passage of an electric current.
angular momentum in the bohr model
electrolysis
Triple point
Molality
50. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Graham's Law
Magnetic quantum number
Effective nuclear charge