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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. Simplest whole # ration of atoms in a compound
Proton
polymer
Emperical Formula
bond length
2. 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
Nucleus
bond length
Pauli exclusion principle
Reaction mechanism
3. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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4. 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
Molecular orbital
Hydrogen bonding
Atomic weight
solvation
5. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Emperical Formula
Dipole
Ion
Collision theory of chemical Kinetics
6. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Lyman series
atomic theory
Halogens
7. 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
Formula weight
Effusion
Disproportionation
8. An elementary particle with 0 charge and mass about equal to a proton
Henderson Hasselbalch Equation
Neutron
Molecular orbital
Alkaline earths
9. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molecular orbital
Ion
Noble gases
Lewis definition
10. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
gram equivalent weight
STP
ionic cmpound
Group 6A
11. Having characteristics of both an acid and a base and capable of reacting as either
heisenberg uncertainty principle
Amphoteric
sigma bond
Period
12. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Neutralization reaction
Amphoteric
indicator
13. 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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14. 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
transition elements
hydrogen bonding
Magnetic quantum number
Ionization energy
15. 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
d orbital
Molarity
Percent yield
16. 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
Molar solubility
Equlibrium constant
Noble gases
Balmer series
17. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
single displacement reaction
VSEPR
sigma bond
molecule
18. 5 different orbitals shaped like clover leaves and max electrons is 10
Dipole Dipole interaction
d orbital
und's rule
Alkaline earths
19. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Effusion
polymer
Solution equilibrium
Group 4A
20. A solid made up of particles that are not arranged in a regular pattern.
Ion product
Formula weight
indicator
amorphous solid
21. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Combination Reaction
Acid dissociation constant
ionic cmpound
Lewis structure
22. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Magnetic quantum number
Proton
Rate law
23. The process by which one or more substances change to produce one or more different substances
chemical reaction
Group 2A
crystalline solid
Decomposition reaction
24. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Bronsted - Lowry definition
Conjugate acids and Bases
Theoretical yield
Colligative properties
25. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Effusion
Group 1A
decomposition reaction
Effective nuclear charge
26. 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
electron configuration
Avagadros number
Titration
chemical reaction
27. Rare earth element group (elements 58-71)
lathanide series
Redox Half Reaction
Pauli exclusion principle
Disproportionation
28. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
ionic cmpound
empirical formula
physical reaction
indicator
29. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
hydrogen bonding
Half equivalence point
Diprotic Base
Electronegativity
30. The average distance between the nuclei of two bonded atoms
Emperical Formula
Titration
indicator
bond length
31. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Activation energy
subshell
atomic radius
Molar solubility
32. Redox reaction - in which the same species is both oxidized and reduced.
Disproportionation
Molecular orbital
quantum numbers
Nonpolar covalent bond
33. An ionic compound that resists changes in its pH
Redox Half Reaction
Solvent
Buffer
Molecular orbital
34. E=hc/?
und's rule
Alkaline earths
electromagnetic energy of photons emmited from electrons at ground state
Rydberg constant
35. 2.18 x 10^-18 J/electron
Group 3A
Rydberg constant
Molar solubility
Formula weight
36. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Aqueous Solution
decomposition reaction
Octet Rule
Atomic weight
37. An atom or group of atoms that has a positive or negative charge
Ion
Percent yield
Spin quantum number
Conjugate acids and Bases
38. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Common ion effect
Ion
Lyman series
39. Sum of the protons and neutrons in an element often denoted by the letter A
Redox Half Reaction
Formula weight
Mass number
heisenberg uncertainty principle
40. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Rydberg constant
Titration
Atomic weight
Lyman series
41. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
Solubility Product Constant
London forces
decomposition reaction
percent composition
42. 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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43. A definite stable energy that a physical system can have
Diprotic Base
heisenberg uncertainty principle
energy state
Molality
44. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Electronegativity
Amphoteric
Activation energy
Common ion effect
45. A base that can accept two moles of H+ per mole of itself (ex: SO4
Buffer
Network covalent
Diprotic Base
physical reaction
46. A reaction where a compound does Not change its molecular structure.
Percent yield
physical reaction
atomic radius
Lewis structure
47. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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48. Tells you how much solute is present compared to the amount of solvent
pI
Concentration
Net ionic equation
quantum
49. 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
und's rule
Spin quantum number
Diprotic Base
actinide series
50. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis structure
Lewis definition
Colligative properties
polymer