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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 structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Emperical Formula
energy state
Lewis structure
Covalent Bond
2. 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.
Ion product
heisenberg uncertainty principle
Effusion
decomposition reaction
3. Two or more atoms held together by covalent bonds
Half equivalence point
London forces
Group 4A
molecule
4. Any sample of a given compound will contain the same elements in the identical mass ratio.
Collision theory of chemical Kinetics
law of constant composition
Equlibrium constant
Network covalent
5. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
theoretical yield
Reaction order
Solvent
6. 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
Vapor pressure
The bohr model
Strong acid
atomic radius
7. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Rate determining step
Water dissociation Constant
Spin quantum number
Dipole Dipole interaction
8. 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
Electrolyte
Group 6A
London forces
Azeotrope
9. 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
azimuthal quantum number
Octet Rule
Avagadros number
electron configuration
10. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Ionization energy
The bohr model
Ground state
STP
11. PH of a molecule at which it contains no net electric charge - isoelectric point.
Titration
Aqueous Solution
Network covalent
pI
12. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Network covalent
pi bonds
quantum
13. 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
Amphoteric
Net ionic equation
VSEPR
14. Acids defined as electron - pair acceptors and bases as electron - pair donors.
VSEPR
Collision theory of chemical Kinetics
Lewis definition
Neutron
15. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Lewis structure
Ion
heisenberg uncertainty principle
Covalent Bond
16. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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17. The Percent by mass of each element in a compound.
periodic trends
Percent yield
Period
Percent composition
18. The percent by mass of each element in a compound
single displacement reaction
percent composition
Alkaline earths
Amphoteric
19. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
redox reaction
Intermolecular forces
Percent composition
Free radical
20. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Arrhenius Definition
quantum
Alkaline earths
Ion
21. A horizontal row of elements in the periodic table
lathanide series
Azeotrope
Period
transition elements
22. The energy required to break a chemical bond and form neutral isolated atoms
Ion dipole interactions
chemical reaction
bond energy
quanta
23. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
single displacement reaction
ionic cmpound
empirical formula
Noble gases
24. 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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25. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
heisenberg uncertainty principle
Network covalent
Ionic Bond
Disproportionation
26. Sum of the protons and neutrons in an element often denoted by the letter A
Reaction mechanism
Raoult's Law
Mass number
Electronegativity
27. 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
Electrolyte
Percent yield
Solution equilibrium
Proton
28. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
sigma bond
Molecular orbital
Strong acid
Electrolyte
29. Common definition of acids as proton (H+) donors and bases as proton acceptors
Water dissociation Constant
compound
Bronsted - Lowry definition
Neutralization reaction
30. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Group 7A
Reaction mechanism
Concentration
Electrolyte
31. Simplest whole # ration of atoms in a compound
Octet Rule
Graham's Law
Redox Half Reaction
Emperical Formula
32. An ionic compound that resists changes in its pH
bond length
Buffer
solvation
electron configuration
33. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Lewis structure
law of constant composition
quantum
mole
34. 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
Percent yield
Ionization energy
Triple point
Spin quantum number
35. Property of the elements that can be predicted from the arrangement of the periodic table
Theoretical yield
Rate determining step
redox reaction
periodic trends
36. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Rate law
empirical formula
effective nuclear charge
Ionization energy
37. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Raoult's Law
Ion product
Le chateliers Principle
Molar solubility
38. Small discrete increments of energy.
quanta
Electrolyte
Water dissociation Constant
atomic theory
39. 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
atomic radius
Ionic Bond
Neutron
Nucleus
40. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
Network covalent
Lewis structure
quantum
41. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Reaction order
atomic radius
Molarity
Ground state
42. 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
Raoult's Law
Acid dissociation constant
Dipole Dipole interaction
Le chateliers Principle
43. Gram equivalent weight of solute per liter of solution - often denoted by N.
theoretical yield
Period
lewis base
Normality
44. 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.
hydrogen bonding
Octet Rule
Equivalence point
Planck's Constant
45. 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.
Avagadros number
single displacement reaction
crystalline solid
Planck's Constant
46. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Group 6A
Equlibrium constant
Chemical Kinetics
lewis base
47. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Reaction mechanism
Neutralization reaction
Atomic weight
Ion dipole interactions
48. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Balmer series
quantum
Electrolyte
Halogens
49. Named after their cation and anion
Rate determining step
Emperical Formula
ionic cmpound
electron configuration
50. A definite stable energy that a physical system can have
energy state
Buffer
atomic radius
Le chateliers Principle