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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 pair of equal and opposite electric charges or magnetic poles separated by a small distance
Arrhenius Definition
Concentration
Mass number
Dipole
2. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
molecule
Molality
Spin quantum number
Normality
3. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Intermolecular forces
single displacement reaction
actinide series
VSEPR
4. 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
Dipole Dipole interaction
s orbital
pi bonds
Titration
5. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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6. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
The bohr model
Resonance structure
Combination Reaction
Group 3A
7. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
physical reaction
Arrhenius Definition
atomic emission spectrum
Group 4A
8. An ionic compound that resists changes in its pH
pi bonds
Henderson Hasselbalch Equation
pI
Buffer
9. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
electrolysis
Lewis definition
gram equivalent weight
amorphous solid
10. (chemistry) p(otential of) H(ydrogen)
Group 2A
quantum
pH
Dispersion Forces
11. 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.
Emperical Formula
Ion product
molecule
single displacement reaction
12. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Equivalence point
Hydrogen bonding
indicator
13. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Diprotic Base
transition elements
Half equivalence point
Molar solubility
14. 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.
Molecular orbital
Henderson Hasselbalch Equation
Group 2A
polymer
15. 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
Rydberg constant
Electrolyte
Balmer series
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
Formal Charge
solvation
Chemical Kinetics
Pauli exclusion principle
17. 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
mole
Titration
Magnetic quantum number
18. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
Alkaline earths
ionic cmpound
Vapor pressure
19. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
decomposition reaction
Molality
sigma bond
Bronsted Lowry
20. 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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21. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
atomic radius
Rate law
Equilibrium
22. Named after their cation and anion
azimuthal quantum number
Electrolyte
Charles and Gay Lussac's Law
ionic cmpound
23. 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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24. 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
Percent yield
percent composition
Proton
Lewis structure
25. 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
Common ion effect
Mass number
atomic emission spectrum
26. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
sigma bond
Molarity
Group 1A
Principle quantum number
27. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
mole
Percent composition
Acid dissociation constant
Noble gases
28. 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
Proton
single displacement reaction
decomposition reaction
29. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Water dissociation Constant
Lyman series
transition elements
30. The process by which one or more substances change to produce one or more different substances
polymer
Solute
chemical reaction
Proton
31. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Electrolyte
electromagnetic energy of photons emmited from electrons at ground state
energy state
32. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
atomic emission spectrum
Atomic weight
Group 1A
33. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Equivalence point
Avagadros number
Lewis structure
crystalline solid
34. 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.
Vapor pressure
Chemical Kinetics
Theoretical yield
VSEPR
35. Substance in which a solute is dissolved to form a solution
Solvent
molecule
und's rule
Henry's Law
36. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Hydrogen bonding
ionic cmpound
Triple point
Pauli exclusion principle
37. A base that can accept two moles of H+ per mole of itself (ex: SO4
single displacement reaction
Diprotic Base
Diffusion
Phase diagram
38. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Ionic Bond
Dipole
Azeotrope
heisenberg uncertainty principle
39. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lyman series
Triple point
representative elements
bond length
40. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Vapor pressure
Dispersion Forces
Alkaline earths
Molecular orbital
41. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
empirical formula
Activation energy
Principle quantum number
Rate law
42. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
percent composition
physical reaction
Equilibrium
43. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Planck's Constant
electron configuration
Half equivalence point
Atomic weight
44. The Percent by mass of each element in a compound.
VSEPR
Percent composition
Common ion effect
Redox Half Reaction
45. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
law of constant composition
Lewis structure
electron affinity
Nucleus
46. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
Ion product
periodic trends
electron affinity
47. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
crystalline solid
Dipole
Intermolecular forces
representative elements
48. A subdivision of an energy level in an atom. They are divided into orbitals.
polymer
subshell
Formal Charge
Common ion effect
49. The percent by mass of each element in a compound
Group 1A
Neutron
bond energy
percent composition
50. Property of the elements that can be predicted from the arrangement of the periodic table
Chemical Kinetics
Dipole Dipole interaction
periodic trends
lathanide series