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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. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
mole
Equlibrium constant
Molarity
2. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Ion dipole interactions
Molality
mole
Molecular orbital
3. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Henderson Hasselbalch Equation
Decomposition reaction
Redox Half Reaction
Combination Reaction
4. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
electromagnetic energy of photons emmited from electrons at ground state
Diprotic Base
quantum
5. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
hydrogen bonding
electrolysis
Lewis acid base reaction
atomic emission spectrum
6. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Activation energy
Spin quantum number
atomic radius
Collision theory of chemical Kinetics
7. 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
crystalline solid
Charles and Gay Lussac's Law
Percent yield
transition elements
8. 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.
Balmer series
Henderson Hasselbalch Equation
effective nuclear charge
Pauli exclusion principle
9. 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
Hydrogen bonding
quantum
Disproportionation
s orbital
10. Rare earth element group (elements 58-71)
Charles and Gay Lussac's Law
Concentration
Redox Half Reaction
lathanide series
11. 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
Ionic Bond
pH
Phase diagram
Arrhenius Definition
12. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
Equilibrium
Solute
Lewis definition
13. 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.
Arrhenius Definition
chemical reaction
Strong acid
Henderson Hasselbalch Equation
14. 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
Diprotic Base
Water dissociation Constant
bond energy
15. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Le chateliers Principle
Group 1A
atomic radius
solvation
16. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Redox Half Reaction
Network covalent
The bohr model
Bronsted Lowry
17. Numbers that specify the properties of atomic orbitals and of their electrons
Halogens
Collision theory of chemical Kinetics
solvation
quantum numbers
18. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Half equivalence point
redox reaction
STP
pH
19. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Group 7A
Strong acid
Common ion effect
Solution equilibrium
20. An atom or group of atoms that has a positive or negative charge
Percent composition
Ion
Magnetic quantum number
Colligative properties
21. 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
Ionization energy
Resonance structure
Reaction mechanism
Titration
22. 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
Ionization energy
Rate law
Group 3A
Molar solubility
23. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
azimuthal quantum number
sigma bond
chemical reaction
Molarity
24. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
Atomic absorption Spectra
atomic radius
lathanide series
25. Substance in which a solute is dissolved to form a solution
Titration
Noble gases
Solvent
Emperical Formula
26. 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
Group 3A
Formal Charge
mole
Half equivalence point
27. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
gram equivalent weight
bond length
Effusion
angular momentum in the bohr model
28. An elementary particle with 0 charge and mass about equal to a proton
molecular weight
Neutron
Group 4A
Lewis acid base reaction
29. The percent by mass of each element in a compound
Collision theory of chemical Kinetics
azimuthal quantum number
percent composition
redox reaction
30. 5 valence electrons -3 ions - Nitride N
Reaction mechanism
Electronegativity
Group 5A
Ion product
31. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Molarity
gram equivalent weight
Reaction order
Covalent Bond
32. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Combination Reaction
Lewis definition
Collision theory of chemical Kinetics
33. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Amphoteric
Concentration
Spin quantum number
34. 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
Acid dissociation constant
representative elements
Le chateliers Principle
quantum
35. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Solvent
Decomposition reaction
Chemical Kinetics
Ion dipole interactions
36. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
atomic theory
lewis base
Solubility Product Constant
Electronegativity
37. 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
Neutralization reaction
Dispersion Forces
quantum numbers
38. Named after their cation and anion
molecular weight
Ion dipole interactions
ionic cmpound
Electrolyte
39. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Activation energy
und's rule
Lewis definition
pi bonds
40. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Mass number
Spin quantum number
atomic radius
Nonpolar covalent bond
41. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Group 4A
Reaction mechanism
compound
Lewis acid base reaction
42. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
compound
Raoult's Law
Group 7A
Chemical Kinetics
43. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
redox reaction
Octet Rule
polymer
molecular weight
44. 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.
VSEPR
Ionization energy
Magnetic quantum number
electromagnetic energy of photons emmited from electrons at ground state
45. 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.
Equivalence point
atomic emission spectrum
amorphous solid
effective nuclear charge
46. A subdivision of an energy level in an atom. They are divided into orbitals.
Acid dissociation constant
Aqueous Solution
subshell
Emperical Formula
47. 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
Atomic weight
Nonpolar covalent bond
molecular weight
48. The slowest elementary step which is the limit for the rate of the other steps
Lewis definition
azimuthal quantum number
Rate determining step
The bohr model
49. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
mole
Rydberg constant
Dipole Dipole interaction
50. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutralization reaction
Percent yield
Molarity
percent composition