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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. An ionic compound that resists changes in its pH
Formal Charge
Nonpolar covalent bond
Ion dipole interactions
Buffer
2. 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.
crystalline solid
s orbital
Strong acid
Resonance structure
3. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Atomic absorption Spectra
Avagadros number
ionic cmpound
compound
4. The energy required to break a chemical bond and form neutral isolated atoms
Common ion effect
Network covalent
bond energy
Henry's Law
5. A reaction where a compound does Not change its molecular structure.
Decomposition reaction
physical reaction
lathanide series
Ion product
6. A horizontal row of elements in the periodic table
redox reaction
Solute
Period
Atomic weight
7. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Molarity
Neutron
Rydberg constant
Lyman series
8. Having characteristics of both an acid and a base and capable of reacting as either
representative elements
Amphoteric
Titration
heisenberg uncertainty principle
9. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Intermolecular forces
Group 6A
Ground state
Combination Reaction
10. 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
Nonpolar covalent bond
atomic radius
quantum
11. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
indicator
Proton
quantum numbers
electrolysis
12. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Emperical Formula
Octet Rule
atomic radius
Network covalent
13. 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
amorphous solid
Henderson Hasselbalch Equation
Normality
Spin quantum number
14. The percent by mass of each element in a compound
percent composition
Atomic weight
Group 6A
Balmer series
15. Common definition of acids as proton (H+) donors and bases as proton acceptors
Diffusion
lathanide series
Bronsted - Lowry definition
Group 2A
16. 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.
Principle quantum number
Alkaline earths
Titration
Halogens
17. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
lewis base
Octet Rule
Alkaline earths
redox reaction
18. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
electron configuration
Atomic absorption Spectra
bond length
gram equivalent weight
19. A substance that - when dissolved in water - results in a solution that can conduct electricity
Ion
Electrolyte
Halogens
Buffer
20. Redox reaction - in which the same species is both oxidized and reduced.
Lewis structure
molecular weight
atomic theory
Disproportionation
21. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
decomposition reaction
Group 5A
Rate law
STP
22. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Rydberg constant
crystalline solid
effective nuclear charge
23. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Group 5A
Nonpolar covalent bond
Dispersion Forces
atomic emission spectrum
24. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Common ion effect
Ion dipole interactions
Formula weight
Half equivalence point
25. 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
Equlibrium constant
mole
Ionic Bond
Strong acid
26. Two or more atoms held together by covalent bonds
energy state
molecule
Graham's Law
redox reaction
27. 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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28. 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
gram equivalent weight
single displacement reaction
Equivalence point
29. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Alkaline earths
Theoretical yield
Octet Rule
single displacement reaction
30. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
redox reaction
Vapor pressure
subshell
percent composition
31. One - half of the distance between the center of identical atoms that are not bonded together. Since effective nuclear charge increases when moving from left to right each additional electron is pulled more strogly toward the nucleus.
Group 1A
Chemical Kinetics
d orbital
atomic radius
32. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
VSEPR
Ion dipole interactions
Solute
33. 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.
actinide series
Ion product
Bronsted Lowry
Group 2A
34. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
bond energy
Group 2A
Rate law
35. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
percent composition
Nucleus
molecular weight
Molecular orbital
36. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
electron affinity
Principle quantum number
Effusion
theoretical yield
37. 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.
heisenberg uncertainty principle
electron affinity
VSEPR
Dipole
38. 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
Formula weight
Nucleus
Group 6A
ionic cmpound
39. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Group 1A
Normality
electron affinity
Molality
40. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Formula weight
Reaction mechanism
lewis base
Ion
41. An elementary particle with 0 charge and mass about equal to a proton
electron configuration
gram equivalent weight
solvation
Neutron
42. The process by which one or more substances change to produce one or more different substances
single displacement reaction
Acid dissociation constant
chemical reaction
Triple point
43. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
single displacement reaction
d orbital
molecule
44. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Principle quantum number
Ion
Theoretical yield
Half equivalence point
45. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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46. 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
Collision theory of chemical Kinetics
azimuthal quantum number
STP
Noble gases
47. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Bronsted Lowry
Vapor pressure
polymer
Pauli exclusion principle
48. Sum of the protons and neutrons in an element often denoted by the letter A
Half equivalence point
Mass number
Reaction mechanism
electrolysis
49. 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
pI
Principle quantum number
Arrhenius Definition
Half equivalence point
50. 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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