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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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Match each statement with the correct term.
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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. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Group 7A
Collision theory of chemical Kinetics
Effusion
electrolysis
2. Simplest whole # ration of atoms in a compound
Combination Reaction
Redox Half Reaction
Phase diagram
Emperical Formula
3. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum numbers
ionic cmpound
quantum
Strong acid
4. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
empirical formula
angular momentum in the bohr model
amorphous solid
Vapor pressure
5. 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.
Half equivalence point
polymer
Equivalence point
Titration
6. 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.
Redox Half Reaction
Bronsted - Lowry definition
crystalline solid
Acid dissociation constant
7. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole Dipole interaction
atomic radius
Effusion
Ionic Bond
8. A dynamic condition in which two opposing changes occur at equal rates in a closed system
redox reaction
electrolysis
pi bonds
Equilibrium
9. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
atomic emission spectrum
transition elements
Ion dipole interactions
10. In a solution - the substance that dissolves in the solvent
Electrolyte
Solute
Electronegativity
atomic theory
11. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Solubility Product Constant
Dipole Dipole interaction
Mass number
12. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Group 7A
Magnetic quantum number
Ion dipole interactions
und's rule
13. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
lewis base
Charles and Gay Lussac's Law
Net ionic equation
Strong acid
14. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
redox reaction
Triple point
STP
Rydberg constant
15. 2.18 x 10^-18 J/electron
Group 1A
Rydberg constant
electromagnetic energy of photons emmited from electrons at ground state
bond energy
16. 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
electron configuration
Alkaline earths
Formal Charge
solvation
17. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Nonpolar covalent bond
Avagadros number
redox reaction
18. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Lewis acid base reaction
Ion
d orbital
lewis base
19. 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
Arrhenius Definition
Balmer series
Dispersion Forces
Henry's Law
20. 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.
Henderson Hasselbalch Equation
Ground state
Percent composition
Atomic weight
21. 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
Lewis acid base reaction
molecular weight
Spin quantum number
Octet Rule
22. 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
Magnetic quantum number
Ion dipole interactions
Planck's Constant
Bronsted - Lowry definition
23. 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
lewis base
Ionic Bond
Molarity
Ion
24. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Bronsted Lowry
Molarity
Molality
Titration
25. 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
Bronsted Lowry
Hydrogen bonding
Noble gases
percent composition
26. 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
law of constant composition
Equlibrium constant
Percent yield
Chemical Kinetics
27. 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
Azeotrope
Percent composition
representative elements
hydrogen bonding
28. Named after their cation and anion
Bronsted Lowry
Normality
angular momentum in the bohr model
ionic cmpound
29. 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
Group 6A
Group 5A
Noble gases
30. 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
Nucleus
Rate law
Group 4A
31. 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
Strong acid
Colligative properties
Ion dipole interactions
Ionic Bond
32. Any sample of a given compound will contain the same elements in the identical mass ratio.
Triple point
Effusion
law of constant composition
Molality
33. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
Dipole Dipole interaction
Redox Half Reaction
Dipole
34. 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
Hydrogen bonding
Le chateliers Principle
Nucleus
pI
35. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Net ionic equation
gram equivalent weight
Dipole Dipole interaction
36. 5 valence electrons -3 ions - Nitride N
redox reaction
VSEPR
Group 2A
Group 5A
37. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
Acid dissociation constant
Octet Rule
Mass number
38. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture
Combination Reaction
redox reaction
Solution equilibrium
Balmer series
39. Two or more atoms held together by covalent bonds
single displacement reaction
Atomic absorption Spectra
molecule
Rate law
40. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
molecule
Formula weight
bond length
Neutralization reaction
41. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Molar solubility
Acid dissociation constant
Atomic weight
quantum
42. The lowest allowable energy state of an atom
chemical reaction
Group 7A
Half equivalence point
Ground state
43. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
ionic cmpound
Solute
Electronegativity
Combination Reaction
44. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Hydrogen bonding
Magnetic quantum number
Theoretical yield
45. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
law of constant composition
Ion
Percent yield
Strong acid
46. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
amorphous solid
Rate law
s orbital
Nucleus
47. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Ion
Reaction order
Emperical Formula
48. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Nucleus
Lewis definition
Formal Charge
pH
49. The energy required to break a chemical bond and form neutral isolated atoms
Graham's Law
mole
bond energy
Lewis definition
50. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Reaction mechanism
Aqueous Solution
Lewis definition
polymer
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