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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. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
Redox Half Reaction
Intermolecular forces
mole
azimuthal quantum number
2. An ionic compound that resists changes in its pH
Disproportionation
Buffer
Acid dissociation constant
redox reaction
3. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Ground state
Solute
heisenberg uncertainty principle
4. 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
London forces
Covalent Bond
Colligative properties
5. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Pauli exclusion principle
law of constant composition
Dipole
crystalline solid
6. 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.
Planck's Constant
Rate determining step
sigma bond
atomic radius
7. Keq describes the ratio of product concentration to reactant concentration - with each raised to the power corresponding ot its coefficient ion in the balanced equation
Bronsted Lowry
s orbital
Equlibrium constant
Phase diagram
8. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Molar solubility
sigma bond
Group 5A
Diprotic Base
9. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin
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10. 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
Le chateliers Principle
Titration
Avagadros number
single displacement reaction
11. Any sample of a given compound will contain the same elements in the identical mass ratio.
sigma bond
Group 7A
Alkaline earths
law of constant composition
12. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Atomic weight
Ion dipole interactions
mole
13. 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
Dispersion Forces
Molecular orbital
quantum numbers
London forces
14. 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
empirical formula
The bohr model
Percent composition
Emperical Formula
15. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Dipole Dipole interaction
atomic emission spectrum
Group 4A
ionic cmpound
16. 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 7A
Dipole Dipole interaction
Henry's Law
Formula weight
17. A base that can accept two moles of H+ per mole of itself (ex: SO4
indicator
Diprotic Base
Molality
Nucleus
18. 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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19. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
atomic radius
redox reaction
Solubility Product Constant
Theoretical yield
20. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
atomic emission spectrum
empirical formula
effective nuclear charge
21. 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
Atomic absorption Spectra
Arrhenius Definition
Hydrogen bonding
Disproportionation
22. The lowest allowable energy state of an atom
Principle quantum number
Proton
Ground state
Period
23. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Reaction mechanism
Lyman series
Molecular orbital
molecular weight
24. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Solute
atomic radius
quantum numbers
Lewis definition
25. Redox reaction - in which the same species is both oxidized and reduced.
Octet Rule
Solution equilibrium
Disproportionation
gram equivalent weight
26. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
bond energy
Concentration
amorphous solid
27. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Charles and Gay Lussac's Law
compound
indicator
Theoretical yield
28. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Magnetic quantum number
Concentration
electrolysis
Collision theory of chemical Kinetics
29. 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
Period
Rate determining step
Spin quantum number
sigma bond
30. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
crystalline solid
Group 1A
quanta
31. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Neutralization reaction
Molecular orbital
Henry's Law
redox reaction
32. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
Reaction order
Hydrogen bonding
Combination Reaction
Colligative properties
33. The percent by mass of each element in a compound
Molality
Group 4A
percent composition
Phase diagram
34. 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
Triple point
Planck's Constant
Activation energy
Ionic Bond
35. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Decomposition reaction
Redox Half Reaction
Ionization energy
Resonance structure
36. 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.
hydrogen bonding
Atomic absorption Spectra
redox reaction
Effective nuclear charge
37. Sum of the protons and neutrons in an element often denoted by the letter A
lathanide series
Mass number
angular momentum in the bohr model
single displacement reaction
38. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
Group 1A
Nonpolar covalent bond
Equivalence point
Ground state
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.
Lewis structure
Effective nuclear charge
Network covalent
chemical reaction
40. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
atomic emission spectrum
heisenberg uncertainty principle
ionic cmpound
Effusion
41. A reaction in which atoms of one element take the place of atoms of another element in a compound
Planck's Constant
atomic radius
single displacement reaction
Ionization energy
42. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Noble gases
percent composition
subshell
polymer
43. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
Lewis definition
Raoult's Law
Water dissociation Constant
44. 2.18 x 10^-18 J/electron
Lewis acid base reaction
Group 3A
Octet Rule
Rydberg constant
45. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Solubility Product Constant
Theoretical yield
Molality
Percent yield
46. A horizontal row of elements in the periodic table
Effusion
Formal Charge
Period
Solute
47. Rare earth element group (elements 58-71)
Vapor pressure
solvation
Diffusion
lathanide series
48. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
lathanide series
polymer
Noble gases
mole
49. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Common ion effect
Lyman series
law of constant composition
single displacement reaction
50. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
Henderson Hasselbalch Equation
lewis base
Intermolecular forces