SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. Any sample of a given compound will contain the same elements in the identical mass ratio.
Solute
Avagadros number
law of constant composition
atomic radius
2. 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
lewis base
pH
VSEPR
3. Chalcogens - - Oxide O
Octet Rule
Activation energy
Group 6A
Spin quantum number
4. 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
Rate law
Alkaline earths
Equilibrium
representative elements
5. 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
atomic theory
azimuthal quantum number
Equilibrium
Molarity
6. Redox reaction - in which the same species is both oxidized and reduced.
Normality
STP
Disproportionation
gram equivalent weight
7. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Free radical
Pauli exclusion principle
Half equivalence point
law of constant composition
8. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Solute
Group 2A
Molar solubility
Diprotic Base
9. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
solvation
Aqueous Solution
Concentration
10. Rare earth element group (elements 58-71)
lathanide series
und's rule
Nucleus
Concentration
11. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Ionization energy
Ionic Bond
atomic radius
Bronsted Lowry
12. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
representative elements
electron configuration
atomic emission spectrum
13. A horizontal row of elements in the periodic table
Azeotrope
actinide series
Period
Henderson Hasselbalch Equation
14. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
Formal Charge
STP
Neutralization reaction
15. 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
gram equivalent weight
Ion
London forces
Effusion
16. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Period
STP
Theoretical yield
17. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Diprotic Base
Octet Rule
Water dissociation Constant
Phase diagram
18. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Lewis structure
single displacement reaction
Octet Rule
sigma bond
19. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
Magnetic quantum number
Ionic Bond
Ion
20. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Reaction order
Octet Rule
Vapor pressure
Effusion
21. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Magnetic quantum number
molecule
electron configuration
Raoult's Law
22. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
bond energy
Avagadros number
Rydberg constant
Colligative properties
23. Numbers that specify the properties of atomic orbitals and of their electrons
Lewis acid base reaction
quantum numbers
redox reaction
Molecular orbital
24. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy
Group 5A
Conjugate acids and Bases
s orbital
Proton
25. Two or more atoms held together by covalent bonds
energy state
Noble gases
molecule
mole
26. 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.
electron affinity
bond length
crystalline solid
sigma bond
27. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
28. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Electronegativity
chemical reaction
Equivalence point
29. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
Planck's Constant
quantum numbers
Ionization energy
30. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Ionization energy
Lewis structure
Resonance structure
Group 5A
31. A solution in which water is the solvent
Aqueous Solution
Rate law
Conjugate acids and Bases
Pauli exclusion principle
32. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Strong acid
Chemical Kinetics
pH
33. Gram equivalent weight of solute per liter of solution - often denoted by N.
Decomposition reaction
compound
Normality
Formula weight
34. Elements in the middle of the periodic table - in groups 3-12.
Henry's Law
Acid dissociation constant
transition elements
quantum
35. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Group 4A
Triple point
und's rule
36. 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.
Reaction order
electron affinity
und's rule
Rate law
37. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Solution equilibrium
Spin quantum number
Dipole
Equilibrium
38. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
Avagadros number
Solubility Product Constant
Percent yield
atomic theory
39. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
electron configuration
Network covalent
Conjugate acids and Bases
Combination Reaction
40. A reaction in which atoms of one element take the place of atoms of another element in a compound
Disproportionation
single displacement reaction
Rate determining step
Buffer
41. In a solution - the substance that dissolves in the solvent
Solute
London forces
atomic theory
Lewis definition
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
Rate determining step
Spin quantum number
Acid dissociation constant
Normality
43. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Resonance structure
Nonpolar covalent bond
periodic trends
Ion
44. The maximum amount of product that can be produced from a given amount of reactant
single displacement reaction
representative elements
theoretical yield
Group 1A
45. The Percent by mass of each element in a compound.
Spin quantum number
Solvent
Molarity
Percent composition
46. 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-
Water dissociation Constant
Net ionic equation
Rate law
heisenberg uncertainty principle
47. 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
Group 3A
theoretical yield
representative elements
48. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
electrolysis
Group 4A
Chemical Kinetics
Combination Reaction
49. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Covalent Bond
actinide series
Molecular orbital
bond length
50. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
lewis base
Colligative properties
mole
Lewis structure