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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. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
transition elements
Noble gases
Pauli exclusion principle
Redox Half Reaction
2. 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
Network covalent
bond length
transition elements
Ionic Bond
3. 2.18 x 10^-18 J/electron
Activation energy
Percent yield
Rydberg constant
chemical reaction
4. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
Molecular orbital
redox reaction
electron configuration
5. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
Activation energy
Group 5A
azimuthal quantum number
6. 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.
Rate determining step
Group 7A
VSEPR
Electrolyte
7. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Pauli exclusion principle
Emperical Formula
Ion dipole interactions
Activation energy
8. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
9. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Neutralization reaction
Collision theory of chemical Kinetics
d orbital
Phase diagram
10. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Halogens
Ionic Bond
Bronsted Lowry
chemical reaction
11. 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
12. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
13. 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.
Equilibrium
Proton
Redox Half Reaction
Azeotrope
14. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Percent composition
Dipole
Raoult's Law
amorphous solid
15. 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
16. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
Balmer series
Strong acid
s orbital
atomic theory
17. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Hydrogen bonding
heisenberg uncertainty principle
Group 1A
bond length
18. 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
Ion
Redox Half Reaction
Magnetic quantum number
Equilibrium
19. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Le chateliers Principle
Vapor pressure
Group 1A
mole
20. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
angular momentum in the bohr model
Water dissociation Constant
Reaction mechanism
21. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Charles and Gay Lussac's Law
Atomic weight
electromagnetic energy of photons emmited from electrons at ground state
Halogens
22. 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
hydrogen bonding
Charles and Gay Lussac's Law
Azeotrope
sigma bond
23. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
mole
Triple point
Disproportionation
molecular weight
24. PH of a molecule at which it contains no net electric charge - isoelectric point.
Water dissociation Constant
pI
Lewis definition
Group 7A
25. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Proton
pi bonds
redox reaction
Reaction order
26. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Nucleus
bond length
Electronegativity
Molecular orbital
27. The slowest elementary step which is the limit for the rate of the other steps
Normality
Equilibrium
Group 2A
Rate determining step
28. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Henry's Law
Effective nuclear charge
Free radical
Strong acid
29. 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
Raoult's Law
Mass number
Henderson Hasselbalch Equation
30. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Acid dissociation constant
angular momentum in the bohr model
quantum numbers
31. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
atomic radius
redox reaction
Equilibrium
32. 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.
Effective nuclear charge
Henderson Hasselbalch Equation
electrolysis
VSEPR
33. 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
Henry's Law
Hydrogen bonding
Bronsted Lowry
Ionization energy
34. 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.
crystalline solid
ionic cmpound
Equilibrium
pH
35. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
electromagnetic energy of photons emmited from electrons at ground state
Henderson Hasselbalch Equation
subshell
Aqueous Solution
36. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Balmer series
Equlibrium constant
Electronegativity
Atomic absorption Spectra
37. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Dipole
Decomposition reaction
Concentration
electron configuration
38. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Formula weight
Solution equilibrium
Ion
pH
39. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Henry's Law
Equivalence point
Lewis structure
40. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Amphoteric
Raoult's Law
physical reaction
Avagadros number
41. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Octet Rule
redox reaction
Neutron
Pauli exclusion principle
42. A solid made up of particles that are not arranged in a regular pattern.
Disproportionation
Activation energy
Common ion effect
amorphous solid
43. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Electronegativity
lewis base
Electrolyte
subshell
44. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Ionic Bond
Rate determining step
electron configuration
quantum
45. A solution in which water is the solvent
Henry's Law
Solvent
Aqueous Solution
Acid dissociation constant
46. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
electrolysis
Acid dissociation constant
Percent yield
Lewis acid base reaction
47. A definite stable energy that a physical system can have
Ion product
energy state
Lewis definition
bond energy
48. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
solvation
Covalent Bond
Combination Reaction
lathanide series
49. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Ground state
Rate determining step
Network covalent
Charles and Gay Lussac's Law
50. 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
Molality
Free radical
Proton
Noble gases