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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
Solute
Period
transition elements
periodic trends
2. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
single displacement reaction
Triple point
compound
theoretical yield
3. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
molecular weight
pH
effective nuclear charge
Diffusion
4. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic theory
azimuthal quantum number
atomic radius
pH
5. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Principle quantum number
pI
Formula weight
Net ionic equation
6. A dynamic condition in which two opposing changes occur at equal rates in a closed system
VSEPR
amorphous solid
Equilibrium
Colligative properties
7. 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
Raoult's Law
Magnetic quantum number
redox reaction
redox reaction
8. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
energy state
theoretical yield
chemical reaction
9. 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
Arrhenius Definition
Henry's Law
atomic emission spectrum
Disproportionation
10. 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.
atomic emission spectrum
Group 2A
Principle quantum number
Solute
11. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
und's rule
Planck's Constant
percent composition
12. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Octet Rule
lathanide series
Aqueous Solution
Lewis definition
13. A substance that - when dissolved in water - results in a solution that can conduct electricity
Avagadros number
Group 2A
Equivalence point
Electrolyte
14. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Decomposition reaction
Magnetic quantum number
Formula weight
molecular weight
15. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Net ionic equation
transition elements
Planck's Constant
16. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Lewis acid base reaction
Phase diagram
quanta
17. PH of a molecule at which it contains no net electric charge - isoelectric point.
physical reaction
Buffer
pI
STP
18. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
theoretical yield
Vapor pressure
physical reaction
Atomic weight
19. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
electron affinity
Decomposition reaction
Solution equilibrium
20. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
subshell
Common ion effect
atomic radius
Molarity
21. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
Water dissociation Constant
pH
Ground state
22. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
energy state
Percent yield
Reaction mechanism
Free radical
23. 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.
Ground state
VSEPR
periodic trends
Le chateliers Principle
24. 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
Rydberg constant
Resonance structure
Normality
Formal Charge
25. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Effective nuclear charge
Lewis definition
Dipole Dipole interaction
26. The percent by mass of each element in a compound
Neutralization reaction
Avagadros number
Solubility Product Constant
percent composition
27. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
atomic theory
Acid dissociation constant
London forces
molecular weight
28. 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
Solution equilibrium
Nucleus
The bohr model
Half equivalence point
29. Charge assigned to an atom in a molecule or polyatmic ion - calculated by (# valence electrons) - (# 1/2 bonding electrons) - (# nonbonding electrons). Molecules containing atoms with lower formal charges tend to be more stable than those with higher
Aqueous Solution
percent composition
Formal Charge
s orbital
30. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Activation energy
d orbital
mole
31. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Chemical Kinetics
mole
Lewis acid base reaction
Concentration
32. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Balmer series
representative elements
Lewis definition
33. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Principle quantum number
bond length
Combination Reaction
34. 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
Aqueous Solution
lewis base
und's rule
azimuthal quantum number
35. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
Electronegativity
redox reaction
Combination Reaction
36. 5 different orbitals shaped like clover leaves and max electrons is 10
Ion dipole interactions
Bronsted Lowry
d orbital
Solvent
37. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Strong acid
STP
Rate determining step
Collision theory of chemical Kinetics
38. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Chemical Kinetics
Lewis structure
redox reaction
Ion
39. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Net ionic equation
Aqueous Solution
Titration
40. A reaction in which atoms of one element take the place of atoms of another element in a compound
Redox Half Reaction
Concentration
single displacement reaction
pH
41. Slightly less reactive than alkali metals - comprise group II
Covalent Bond
Neutron
Alkaline earths
Noble gases
42. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Acid dissociation constant
Noble gases
STP
Colligative properties
43. 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.
Formula weight
actinide series
Rate determining step
crystalline solid
44. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Group 7A
Ionization energy
Water dissociation Constant
45. 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
Raoult's Law
theoretical yield
Nucleus
Azeotrope
46. Two or more atoms held together by covalent bonds
Spin quantum number
angular momentum in the bohr model
electrolysis
molecule
47. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
Combination Reaction
Azeotrope
Alkaline earths
48. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
mole
actinide series
Combination Reaction
Nucleus
49. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
electron configuration
Equilibrium
Principle quantum number
Molality
50. A solid made up of particles that are not arranged in a regular pattern.
theoretical yield
Theoretical yield
amorphous solid
hydrogen bonding