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MCAT Chemistry
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Study First
Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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 substance that - when dissolved in water - results in a solution that can conduct electricity
Neutralization reaction
electron affinity
quantum
Electrolyte
2. 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
Normality
Acid dissociation constant
Lewis definition
quantum numbers
3. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Mass number
Activation energy
d orbital
electron configuration
4. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
law of constant composition
Diprotic Base
Phase diagram
Lewis acid base reaction
5. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Ionic Bond
Normality
quanta
Reaction order
6. 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
Noble gases
VSEPR
sigma bond
Arrhenius Definition
7. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Half equivalence point
Molecular orbital
Electrolyte
energy state
8. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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9. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Balmer series
Group 1A
effective nuclear charge
Group 2A
10. 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
Net ionic equation
Common ion effect
Equivalence point
Titration
11. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
atomic emission spectrum
hydrogen bonding
The bohr model
12. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Intermolecular forces
Effusion
Raoult's Law
atomic theory
13. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
solvation
Rydberg constant
Common ion effect
lewis base
14. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
theoretical yield
electromagnetic energy of photons emmited from electrons at ground state
Atomic weight
Water dissociation Constant
15. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
quanta
Theoretical yield
Halogens
Redox Half Reaction
16. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
Nonpolar covalent bond
Lewis structure
lathanide series
17. 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.
Hydrogen bonding
law of constant composition
Principle quantum number
Spin quantum number
18. 5 different orbitals shaped like clover leaves and max electrons is 10
chemical reaction
Ionization energy
London forces
d orbital
19. Property of the elements that can be predicted from the arrangement of the periodic table
Water dissociation Constant
lewis base
periodic trends
The bohr model
20. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Group 7A
The bohr model
Equlibrium constant
21. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
pI
empirical formula
Neutralization reaction
22. The average distance between the nuclei of two bonded atoms
Theoretical yield
bond length
Acid dissociation constant
Effusion
23. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
subshell
Covalent Bond
Group 2A
Proton
24. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Normality
Intermolecular forces
actinide series
Magnetic quantum number
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
Vapor pressure
hydrogen bonding
Atomic weight
Avagadros number
26. Tells you how much solute is present compared to the amount of solvent
Lyman series
Concentration
Dispersion Forces
London forces
27. The percent by mass of each element in a compound
Solvent
transition elements
percent composition
Dipole Dipole interaction
28. 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
Water dissociation Constant
molecular weight
Titration
Dispersion Forces
29. An element in an 'A' group in the periodic table; as a group these elements display a wide range of physical and chemical properties. In their atoms - the s and p sublevels in the highest occupied energy level are partially filled
representative elements
decomposition reaction
Redox Half Reaction
Hydrogen bonding
30. 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
polymer
Alkaline earths
Spin quantum number
Molarity
31. Substance in which a solute is dissolved to form a solution
amorphous solid
Diffusion
Solvent
Atomic absorption Spectra
32. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Avagadros number
Group 4A
Group 6A
Principle quantum number
33. An atom or group of atoms that has a positive or negative charge
molecule
Emperical Formula
Ion dipole interactions
Ion
34. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Decomposition reaction
quantum numbers
Octet Rule
pH
35. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Diffusion
electron affinity
bond energy
36. 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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37. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
molecular weight
indicator
The bohr model
mole
38. 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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39. 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.
quantum numbers
empirical formula
Henderson Hasselbalch Equation
pH
40. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
electron affinity
Decomposition reaction
Avagadros number
representative elements
41. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
bond energy
lathanide series
Network covalent
Le chateliers Principle
42. 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.
Rate determining step
Halogens
Nonpolar covalent bond
Balmer series
43. 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
Colligative properties
pH
Principle quantum number
Theoretical yield
44. 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.
effective nuclear charge
Group 3A
decomposition reaction
Ion product
45. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
lewis base
gram equivalent weight
electrolysis
46. 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.
Period
crystalline solid
Group 7A
electrolysis
47. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Bronsted Lowry
angular momentum in the bohr model
atomic emission spectrum
48. Simplest whole # ration of atoms in a compound
Emperical Formula
Reaction order
Ion
Lyman series
49. 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
STP
lathanide series
chemical reaction
50. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Solubility Product Constant
solvation
Strong acid
Redox Half Reaction
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