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. 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.
Strong acid
sigma bond
crystalline solid
Ion product
2. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
Percent composition
Nonpolar covalent bond
VSEPR
3. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Diffusion
Conjugate acids and Bases
Formula weight
s orbital
4. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Free radical
und's rule
transition elements
Bronsted Lowry
5. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Conjugate acids and Bases
atomic theory
Group 5A
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
bond length
Bronsted Lowry
Titration
The bohr model
7. 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
Dispersion Forces
Reaction order
pH
Equlibrium constant
8. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Solution equilibrium
redox reaction
d orbital
9. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
redox reaction
bond energy
Effusion
Concentration
10. 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
Henry's Law
energy state
Hydrogen bonding
Redox Half Reaction
11. 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
Intermolecular forces
Aqueous Solution
Formal Charge
azimuthal quantum number
12. The slowest elementary step which is the limit for the rate of the other steps
Aqueous Solution
Magnetic quantum number
Rate determining step
Ground state
13. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Molecular orbital
Hydrogen bonding
Vapor pressure
Collision theory of chemical Kinetics
14. A solution in which water is the solvent
Aqueous Solution
pH
Diffusion
Intermolecular forces
15. 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.
Theoretical yield
crystalline solid
Principle quantum number
amorphous solid
16. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Molality
Molecular orbital
Rate determining step
17. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
actinide series
electron configuration
sigma bond
Rate law
18. 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
Half equivalence point
Ionization energy
Molar solubility
Magnetic quantum number
19. A definite stable energy that a physical system can have
crystalline solid
energy state
Diffusion
Collision theory of chemical Kinetics
20. 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
Titration
Solution equilibrium
electromagnetic energy of photons emmited from electrons at ground state
chemical reaction
21. A solid made up of particles that are not arranged in a regular pattern.
Redox Half Reaction
Water dissociation Constant
amorphous solid
Group 5A
22. 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
Common ion effect
polymer
effective nuclear charge
Nucleus
23. 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
Azeotrope
solvation
transition elements
Amphoteric
24. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Graham's Law
electron affinity
compound
Nucleus
25. Property of the elements that can be predicted from the arrangement of the periodic table
azimuthal quantum number
periodic trends
Ion
STP
26. A subdivision of an energy level in an atom. They are divided into orbitals.
Octet Rule
molecular weight
subshell
Lewis acid base reaction
27. Temperature is constant; effusion and temperature are proportional to the square root of their masses
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
28. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
29. 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
Percent yield
chemical reaction
Group 3A
Raoult's Law
30. The percent by mass of each element in a compound
percent composition
Nonpolar covalent bond
Ground state
Decomposition reaction
31. 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.
Bronsted Lowry
VSEPR
Formula weight
Dispersion Forces
32. 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
Vapor pressure
heisenberg uncertainty principle
s orbital
atomic radius
33. An ionic compound that resists changes in its pH
Equilibrium
Buffer
amorphous solid
Group 7A
34. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Spin quantum number
percent composition
Network covalent
Molality
35. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Group 7A
VSEPR
Combination Reaction
Rate law
36. In a solution - the substance that dissolves in the solvent
indicator
Vapor pressure
Molecular orbital
Solute
37. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Lyman series
d orbital
Octet Rule
Spin quantum number
38. 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
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
39. Slightly less reactive than alkali metals - comprise group II
ionic cmpound
Group 3A
Effective nuclear charge
Alkaline earths
40. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
single displacement reaction
atomic radius
Rate determining step
41. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Molar solubility
electron configuration
Pauli exclusion principle
Solute
42. 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.
Alkaline earths
Phase diagram
Equivalence point
London forces
43. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Acid dissociation constant
Normality
Mass number
Triple point
44. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Half equivalence point
Water dissociation Constant
Solubility Product Constant
45. 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
Water dissociation Constant
Formal Charge
atomic emission spectrum
Disproportionation
46. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Rate law
Collision theory of chemical Kinetics
Equilibrium
Ion
47. 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.
solvation
mole
percent composition
atomic radius
48. A reaction where a compound does Not change its molecular structure.
Aqueous Solution
Percent yield
Common ion effect
physical reaction
49. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Redox Half Reaction
Lyman series
atomic radius
Theoretical yield
50. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Chemical Kinetics
Proton
atomic radius
Equilibrium