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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. 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
Equivalence point
Atomic absorption Spectra
Spin quantum number
empirical formula
2. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Solution equilibrium
Formal Charge
bond energy
redox reaction
3. The lowest allowable energy state of an atom
Ground state
Ion
Noble gases
Combination Reaction
4. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
The bohr model
Common ion effect
Dispersion Forces
Aqueous Solution
5. 5 different orbitals shaped like clover leaves and max electrons is 10
Spin quantum number
energy state
d orbital
Common ion effect
6. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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7. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
pi bonds
Formula weight
Collision theory of chemical Kinetics
indicator
8. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Diffusion
Period
single displacement reaction
9. A definite stable energy that a physical system can have
und's rule
energy state
Rate law
d orbital
10. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Free radical
Alkaline earths
bond length
11. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Decomposition reaction
Spin quantum number
Net ionic equation
lathanide series
12. 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
polymer
Combination Reaction
Aqueous Solution
13. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
actinide series
sigma bond
Lewis structure
atomic theory
14. 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.
Principle quantum number
Neutron
Henderson Hasselbalch Equation
Equilibrium
15. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Reaction mechanism
Electronegativity
transition elements
Vapor pressure
16. Two or more atoms held together by covalent bonds
Effective nuclear charge
Normality
molecule
decomposition reaction
17. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
percent composition
Molecular orbital
theoretical yield
18. 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
Reaction mechanism
Henderson Hasselbalch Equation
Planck's Constant
19. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
angular momentum in the bohr model
Solubility Product Constant
azimuthal quantum number
The bohr model
20. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
empirical formula
Phase diagram
Group 5A
21. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Pauli exclusion principle
Ion product
Colligative properties
Lewis acid base reaction
22. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
lewis base
Nucleus
Solute
Concentration
23. 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
Charles and Gay Lussac's Law
Bronsted - Lowry definition
Equlibrium constant
redox reaction
24. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Azeotrope
atomic theory
Henderson Hasselbalch Equation
Formula weight
25. In a solution - the substance that dissolves in the solvent
quanta
Solute
Percent composition
Atomic absorption Spectra
26. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points
Azeotrope
Intermolecular forces
Ground state
Mass number
27. 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
Group 2A
Halogens
chemical reaction
28. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
Nonpolar covalent bond
crystalline solid
Half equivalence point
Magnetic quantum number
29. 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
Equivalence point
subshell
Half equivalence point
30. A reaction in which atoms of one element take the place of atoms of another element in a compound
atomic emission spectrum
crystalline solid
pi bonds
single displacement reaction
31. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
subshell
Buffer
Le chateliers Principle
Electronegativity
32. Elements in the middle of the periodic table - in groups 3-12.
Activation energy
electromagnetic energy of photons emmited from electrons at ground state
transition elements
Decomposition reaction
33. Named after their cation and anion
ionic cmpound
quanta
compound
redox reaction
34. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Covalent Bond
Bronsted Lowry
Dipole Dipole interaction
Acid dissociation constant
35. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Avagadros number
Proton
STP
gram equivalent weight
36. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Collision theory of chemical Kinetics
electron configuration
Molality
pi bonds
37. Rare earth element group (elements 58-71)
amorphous solid
heisenberg uncertainty principle
lathanide series
Equlibrium constant
38. 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.
Lewis structure
Atomic absorption Spectra
Pauli exclusion principle
Ion product
39. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Group 3A
electromagnetic energy of photons emmited from electrons at ground state
Lyman series
40. Small discrete increments of energy.
quanta
Solution equilibrium
Combination Reaction
electrolysis
41. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
Molarity
Rate law
lathanide series
42. 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
pi bonds
lathanide series
electron configuration
Ionic Bond
43. Tells you how much solute is present compared to the amount of solvent
pi bonds
Henderson Hasselbalch Equation
molecule
Concentration
44. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Lewis definition
Molecular orbital
Avagadros number
heisenberg uncertainty principle
45. 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
Acid dissociation constant
ionic cmpound
Bronsted Lowry
azimuthal quantum number
46. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Ground state
Free radical
Water dissociation Constant
theoretical yield
47. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
theoretical yield
energy state
Nonpolar covalent bond
48. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Aqueous Solution
Solution equilibrium
Conjugate acids and Bases
Half equivalence point
49. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Electronegativity
Covalent Bond
energy state
50. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Activation energy
Theoretical yield
energy state
Ion