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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 horizontal row of elements in the periodic table
Phase diagram
Period
decomposition reaction
pH
2. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Equlibrium constant
Disproportionation
Free radical
3. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
Group 2A
Redox Half Reaction
Le chateliers Principle
Group 7A
4. A definite stable energy that a physical system can have
law of constant composition
energy state
Solubility Product Constant
Covalent Bond
5. 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
The bohr model
Reaction order
theoretical yield
Ionic Bond
6. Any sample of a given compound will contain the same elements in the identical mass ratio.
Concentration
Solute
law of constant composition
Ground state
7. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
quantum numbers
Lewis acid base reaction
Resonance structure
8. 2.18 x 10^-18 J/electron
Rydberg constant
Rate determining step
Octet Rule
polymer
9. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Magnetic quantum number
Atomic weight
Dipole
Molar solubility
10. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Phase diagram
Neutralization reaction
Network covalent
Effusion
11. A dynamic condition in which two opposing changes occur at equal rates in a closed system
decomposition reaction
bond energy
Lyman series
Equilibrium
12. 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.
periodic trends
quanta
Free radical
Ion product
13. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
gram equivalent weight
Ion
heisenberg uncertainty principle
solvation
14. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Redox Half Reaction
polymer
Raoult's Law
Bronsted Lowry
15. 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
redox reaction
Collision theory of chemical Kinetics
Noble gases
16. An ionic compound that resists changes in its pH
atomic radius
atomic emission spectrum
Avagadros number
Buffer
17. Common definition of acids as proton (H+) donors and bases as proton acceptors
Resonance structure
Bronsted - Lowry definition
theoretical yield
Group 3A
18. 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.
chemical reaction
Equlibrium constant
Effective nuclear charge
azimuthal quantum number
19. 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
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20. 5 different orbitals shaped like clover leaves and max electrons is 10
Common ion effect
d orbital
Half equivalence point
Group 4A
21. Having characteristics of both an acid and a base and capable of reacting as either
redox reaction
STP
Raoult's Law
Amphoteric
22. A solid made up of particles that are not arranged in a regular pattern.
Proton
amorphous solid
quanta
Conjugate acids and Bases
23. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Intermolecular forces
Equilibrium
Strong acid
Diprotic Base
24. 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.
Collision theory of chemical Kinetics
Alkaline earths
Redox Half Reaction
Bronsted Lowry
25. 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
Le chateliers Principle
percent composition
Arrhenius Definition
molecule
26. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Ionic Bond
redox reaction
percent composition
molecular weight
27. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Diprotic Base
energy state
Chemical Kinetics
Colligative properties
28. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Group 2A
Electrolyte
Solute
Octet Rule
29. Substance in which a solute is dissolved to form a solution
Pauli exclusion principle
representative elements
molecule
Solvent
30. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
quantum
representative elements
VSEPR
31. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
Group 7A
Bronsted - Lowry definition
Ion
32. Rare earth element group (elements 58-71)
Solute
electromagnetic energy of photons emmited from electrons at ground state
Neutralization reaction
lathanide series
33. A solution in which water is the solvent
Molality
Aqueous Solution
Net ionic equation
Network covalent
34. A reaction in which atoms of one element take the place of atoms of another element in a compound
percent composition
Henderson Hasselbalch Equation
Solvent
single displacement reaction
35. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Aqueous Solution
Halogens
actinide series
Lewis structure
36. (chemistry) p(otential of) H(ydrogen)
Net ionic equation
Network covalent
Ground state
pH
37. 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
pH
representative elements
Hydrogen bonding
Concentration
38. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
bond energy
Rate law
Magnetic quantum number
Principle quantum number
39. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
electromagnetic energy of photons emmited from electrons at ground state
Bronsted Lowry
decomposition reaction
Diffusion
40. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
polymer
Dispersion Forces
single displacement reaction
41. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
Solvent
Redox Half Reaction
Acid dissociation constant
42. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 3A
Balmer series
lewis base
Group 4A
43. A subdivision of an energy level in an atom. They are divided into orbitals.
Molar solubility
effective nuclear charge
subshell
bond length
44. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
electrolysis
Planck's Constant
quantum
electron affinity
45. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
transition elements
Group 3A
Molar solubility
percent composition
46. The process of decomposing a chemical compound by the passage of an electric current.
bond length
electrolysis
Normality
Nucleus
47. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Group 4A
effective nuclear charge
Mass number
solvation
48. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
Equivalence point
STP
Strong acid
49. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
Nucleus
molecular weight
Covalent Bond
50. 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
Raoult's Law
Equilibrium
Water dissociation Constant