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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. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Theoretical yield
Octet Rule
theoretical yield
Period
2. Small discrete increments of energy.
Halogens
electron affinity
Diprotic Base
quanta
3. A horizontal row of elements in the periodic table
Period
Ground state
Diprotic Base
Emperical Formula
4. The process of decomposing a chemical compound by the passage of an electric current.
Electrolyte
electrolysis
Rydberg constant
Group 5A
5. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Electrolyte
Molarity
Dipole Dipole interaction
decomposition reaction
6. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Raoult's Law
Molality
Diprotic Base
Effusion
7. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Bronsted - Lowry definition
Network covalent
Lewis acid base reaction
Group 4A
8. 2.18 x 10^-18 J/electron
atomic theory
atomic radius
Rydberg constant
Decomposition reaction
9. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Period
Henderson Hasselbalch Equation
pi bonds
10. A subdivision of an energy level in an atom. They are divided into orbitals.
chemical reaction
Avagadros number
subshell
hydrogen bonding
11. 5 valence electrons -3 ions - Nitride N
Theoretical yield
Group 5A
Magnetic quantum number
physical reaction
12. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
pH
Diffusion
Group 1A
13. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Resonance structure
transition elements
Diffusion
14. Two or more atoms held together by covalent bonds
subshell
gram equivalent weight
molecule
Octet Rule
15. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
theoretical yield
Graham's Law
Free radical
16. 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-
Buffer
Water dissociation Constant
Electrolyte
Solubility Product Constant
17. The Percent by mass of each element in a compound.
Network covalent
Percent composition
bond length
Lewis acid base reaction
18. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
Balmer series
electron affinity
atomic radius
Decomposition reaction
19. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Concentration
polymer
Azeotrope
20. 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.
Ion product
Aqueous Solution
Group 7A
Solvent
21. 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.
electron affinity
Effective nuclear charge
gram equivalent weight
Free radical
22. 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
23. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Percent composition
Equlibrium constant
Neutralization reaction
Titration
24. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
Group 4A
molecule
Electrolyte
25. 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
Resonance structure
Avagadros number
s orbital
redox reaction
26. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
hydrogen bonding
polymer
Ground state
mole
27. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Ion
Bronsted - Lowry definition
Activation energy
28. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Bronsted Lowry
Group 3A
actinide series
quantum
29. The lowest allowable energy state of an atom
Solution equilibrium
molecule
Equlibrium constant
Ground state
30. An ionic compound that resists changes in its pH
Buffer
ionic cmpound
quanta
Proton
31. 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
Net ionic equation
Group 6A
Noble gases
32. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Titration
Avagadros number
Phase diagram
und's rule
33. Sum of the protons and neutrons in an element often denoted by the letter A
Alkaline earths
Mass number
decomposition reaction
Reaction order
34. The slowest elementary step which is the limit for the rate of the other steps
s orbital
Rate determining step
Group 4A
Ionic Bond
35. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Aqueous Solution
Intermolecular forces
heisenberg uncertainty principle
redox reaction
36. 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
Decomposition reaction
The bohr model
Group 3A
crystalline solid
37. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
Atomic absorption Spectra
Colligative properties
Nonpolar covalent bond
Le chateliers Principle
38. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
hydrogen bonding
Ionic Bond
Conjugate acids and Bases
Molar solubility
39. An atom or group of atoms that has a positive or negative charge
effective nuclear charge
Ion
Titration
hydrogen bonding
40. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Acid dissociation constant
Electronegativity
Neutralization reaction
Henry's Law
41. 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.
Solute
crystalline solid
Network covalent
Solution equilibrium
42. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Buffer
Formal Charge
Triple point
representative elements
43. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Strong acid
Free radical
atomic radius
Reaction mechanism
44. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Balmer series
Resonance structure
bond length
Half equivalence point
45. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Hydrogen bonding
Henderson Hasselbalch Equation
Activation energy
Spin quantum number
46. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
azimuthal quantum number
redox reaction
Group 1A
subshell
47. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Electrolyte
angular momentum in the bohr model
Atomic weight
electromagnetic energy of photons emmited from electrons at ground state
48. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
electrolysis
Ion
Dipole
49. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Molarity
und's rule
Effusion
Raoult's Law
50. 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.
law of constant composition
Principle quantum number
Halogens
Reaction mechanism