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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. Property of the elements that can be predicted from the arrangement of the periodic table
Half equivalence point
electron configuration
ionic cmpound
periodic trends
2. An atom or group of atoms that has a positive or negative charge
Molar solubility
Ion
Group 7A
Aqueous Solution
3. 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.
Ion dipole interactions
Concentration
crystalline solid
Atomic weight
4. The percent by mass of each element in a compound
Common ion effect
gram equivalent weight
Solution equilibrium
percent composition
5. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
crystalline solid
Formula weight
Strong acid
Combination Reaction
6. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
amorphous solid
lewis base
redox reaction
7. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Neutralization reaction
atomic emission spectrum
subshell
Water dissociation Constant
8. Substance in which a solute is dissolved to form a solution
Lewis definition
Solvent
Effusion
und's rule
9. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Group 4A
Solute
crystalline solid
mole
10. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
11. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
Equilibrium
Buffer
Spin quantum number
representative elements
12. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
13. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Ion dipole interactions
decomposition reaction
Molar solubility
Net ionic equation
14. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
d orbital
quantum
London forces
Ion dipole interactions
15. The area of chemistry that is concerned with reaction rates and reaction mechanisms
ionic cmpound
effective nuclear charge
Chemical Kinetics
Dipole
16. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
Group 7A
Henry's Law
decomposition reaction
Hydrogen bonding
17. 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
electromagnetic energy of photons emmited from electrons at ground state
subshell
The bohr model
Formula weight
18. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Lewis structure
Principle quantum number
Concentration
19. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Redox Half Reaction
molecular weight
Intermolecular forces
atomic radius
20. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
transition elements
Atomic absorption Spectra
Period
21. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
electron configuration
Formula weight
percent composition
Henry's Law
22. 5 different orbitals shaped like clover leaves and max electrons is 10
STP
d orbital
single displacement reaction
Redox Half Reaction
23. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
amorphous solid
pi bonds
molecular weight
quanta
24. The intermolecular force in which a hydrogen atom that is bonded to a highly electronegative atom is attracted to an unshared pair of electrons of an electronegative atom in a nearby molecule
hydrogen bonding
Neutron
representative elements
Solute
25. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
amorphous solid
indicator
Le chateliers Principle
Percent yield
26. A base that can accept two moles of H+ per mole of itself (ex: SO4
Chemical Kinetics
Diprotic Base
Ionic Bond
Lewis acid base reaction
27. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Ionic Bond
polymer
Equlibrium constant
28. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Concentration
Solubility Product Constant
Molar solubility
Molality
29. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
electromagnetic energy of photons emmited from electrons at ground state
Noble gases
Molality
Half equivalence point
30. A solution in which water is the solvent
Activation energy
d orbital
Phase diagram
Aqueous Solution
31. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
32. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Ground state
Octet Rule
Bronsted - Lowry definition
redox reaction
33. 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
Spin quantum number
s orbital
Avagadros number
atomic radius
34. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Effective nuclear charge
Formal Charge
Equivalence point
35. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital
Spin quantum number
Electronegativity
Emperical Formula
Lewis structure
36. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Ion dipole interactions
Halogens
Avagadros number
37. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Lewis structure
Dipole Dipole interaction
Noble gases
Henderson Hasselbalch Equation
38. An elementary particle with 0 charge and mass about equal to a proton
Activation energy
Octet Rule
gram equivalent weight
Neutron
39. Elements in the middle of the periodic table - in groups 3-12.
Raoult's Law
Group 5A
ionic cmpound
transition elements
40. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
s orbital
Vapor pressure
law of constant composition
Network covalent
41. 2.18 x 10^-18 J/electron
Dispersion Forces
Charles and Gay Lussac's Law
Rydberg constant
electrolysis
42. 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
VSEPR
Dipole Dipole interaction
Acid dissociation constant
Group 3A
43. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Rate determining step
Proton
Dipole Dipole interaction
44. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Theoretical yield
redox reaction
Molecular orbital
electrolysis
45. Redox reaction - in which the same species is both oxidized and reduced.
ionic cmpound
Lewis acid base reaction
Henry's Law
Disproportionation
46. 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
crystalline solid
atomic radius
Solvent
47. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Triple point
Noble gases
Rydberg constant
Effusion
48. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Chemical Kinetics
atomic radius
Molecular orbital
Solution equilibrium
49. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Disproportionation
angular momentum in the bohr model
Phase diagram
polymer
50. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
atomic radius
redox reaction
hydrogen bonding