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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. Elements in the middle of the periodic table - in groups 3-12.
transition elements
empirical formula
Neutron
Nucleus
2. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Electronegativity
Covalent Bond
Molarity
Titration
3. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
bond energy
energy state
Charles and Gay Lussac's Law
Lewis structure
4. Property of the elements that can be predicted from the arrangement of the periodic table
quantum numbers
atomic emission spectrum
bond energy
periodic trends
5. A horizontal row of elements in the periodic table
Collision theory of chemical Kinetics
compound
The bohr model
Period
6. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
ionic cmpound
Effective nuclear charge
solvation
Balmer series
7. 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
Titration
molecular weight
atomic radius
Amphoteric
8. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Noble gases
Spin quantum number
Amphoteric
Theoretical yield
9. 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
und's rule
Nucleus
Acid dissociation constant
Lewis definition
10. Redox reaction - in which the same species is both oxidized and reduced.
actinide series
Solubility Product Constant
VSEPR
Disproportionation
11. Numbers that specify the properties of atomic orbitals and of their electrons
Spin quantum number
physical reaction
quantum numbers
Net ionic equation
12. Small discrete increments of energy.
Hydrogen bonding
quanta
quantum numbers
s orbital
13. 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
Group 6A
Proton
Common ion effect
empirical formula
14. A base that can accept two moles of H+ per mole of itself (ex: SO4
Free radical
Electronegativity
Diprotic Base
Dipole Dipole interaction
15. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Molality
Neutralization reaction
Rate determining step
Formula weight
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-
Molarity
Water dissociation Constant
Le chateliers Principle
Group 7A
17. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
theoretical yield
Rate determining step
Ionization energy
Group 4A
18. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
VSEPR
Dipole
Electrolyte
Solubility Product Constant
19. 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.
Concentration
Group 5A
Conjugate acids and Bases
Group 3A
20. Named after their cation and anion
crystalline solid
Electrolyte
ionic cmpound
electromagnetic energy of photons emmited from electrons at ground state
21. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
azimuthal quantum number
amorphous solid
Common ion effect
22. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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23. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
redox reaction
Concentration
Common ion effect
24. 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
s orbital
Nonpolar covalent bond
Collision theory of chemical Kinetics
Ionic Bond
25. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Percent yield
quantum
Diffusion
pi bonds
26. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
solvation
Lewis structure
Ion
27. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Effusion
redox reaction
Effective nuclear charge
bond energy
28. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
Azeotrope
Effusion
London forces
bond energy
29. 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.
Free radical
Ion product
lewis base
bond energy
30. Substance in which a solute is dissolved to form a solution
Reaction order
Charles and Gay Lussac's Law
polymer
Solvent
31. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Ionic Bond
Conjugate acids and Bases
subshell
bond energy
32. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Arrhenius Definition
Nonpolar covalent bond
compound
Lewis definition
33. 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
Le chateliers Principle
molecule
Colligative properties
34. 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.
Redox Half Reaction
Decomposition reaction
Proton
quanta
35. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
STP
Molecular orbital
Atomic weight
Octet Rule
36. 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.
bond length
VSEPR
Equivalence point
transition elements
37. A reaction where a compound does Not change its molecular structure.
ionic cmpound
physical reaction
Redox Half Reaction
quanta
38. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
decomposition reaction
Lyman series
Group 3A
39. 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
Network covalent
subshell
Ionic Bond
Dispersion Forces
40. A solution in which water is the solvent
decomposition reaction
Triple point
Aqueous Solution
Ion dipole interactions
41. The lowest allowable energy state of an atom
s orbital
transition elements
Water dissociation Constant
Ground state
42. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Half equivalence point
STP
decomposition reaction
pi bonds
43. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Ion dipole interactions
effective nuclear charge
electromagnetic energy of photons emmited from electrons at ground state
Triple point
44. The process of decomposing a chemical compound by the passage of an electric current.
polymer
atomic theory
electrolysis
Effective nuclear charge
45. An elementary particle with 0 charge and mass about equal to a proton
transition elements
Solvent
Neutron
Phase diagram
46. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
law of constant composition
polymer
electron configuration
Balmer series
47. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Graham's Law
Resonance structure
Raoult's Law
48. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Lyman series
Ion
indicator
Conjugate acids and Bases
49. E=hc/?
Combination Reaction
Hydrogen bonding
energy state
electromagnetic energy of photons emmited from electrons at ground state
50. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Redox Half Reaction
Rate law
Activation energy