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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 structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
pI
actinide series
amorphous solid
Lewis structure
2. Substance in which a solute is dissolved to form a solution
pH
Free radical
Solvent
Azeotrope
3. 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
Solvent
Effusion
atomic radius
4. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Principle quantum number
Period
Collision theory of chemical Kinetics
empirical formula
5. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
bond length
Nucleus
Group 3A
Resonance structure
6. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Lewis acid base reaction
angular momentum in the bohr model
atomic radius
7. A reaction in which atoms of one element take the place of atoms of another element in a compound
quantum
single displacement reaction
bond energy
Colligative properties
8. Common definition of acids as proton (H+) donors and bases as proton acceptors
Molecular orbital
Titration
Bronsted - Lowry definition
und's rule
9. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Collision theory of chemical Kinetics
Lewis acid base reaction
angular momentum in the bohr model
Network covalent
10. 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
compound
Solute
Spin quantum number
Formal Charge
11. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Formal Charge
Reaction mechanism
Amphoteric
Formula weight
12. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
pi bonds
Reaction mechanism
hydrogen bonding
decomposition reaction
13. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Nucleus
Equlibrium constant
Ionic Bond
law of constant composition
14. 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 dipole interactions
Rydberg constant
Nucleus
15. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
amorphous solid
Ion
Triple point
16. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Resonance structure
Net ionic equation
gram equivalent weight
Halogens
17. 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.
Activation energy
Avagadros number
Balmer series
Raoult's Law
18. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
The bohr model
Octet Rule
electron affinity
Electronegativity
19. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Lyman series
Ion
gram equivalent weight
Solution equilibrium
20. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Nucleus
Ion
Group 2A
actinide series
21. Rare earth element group (elements 58-71)
Equilibrium
Solute
The bohr model
lathanide series
22. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Colligative properties
Molarity
Conjugate acids and Bases
und's rule
23. 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
Group 5A
Half equivalence point
Buffer
Henry's Law
24. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
quantum
Free radical
Noble gases
sigma bond
25. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Theoretical yield
electron configuration
energy state
redox reaction
26. 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.
Theoretical yield
Group 2A
Ion product
Reaction mechanism
27. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Nonpolar covalent bond
molecule
angular momentum in the bohr model
Principle quantum number
28. 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
polymer
Azeotrope
Alkaline earths
Hydrogen bonding
29. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Solubility Product Constant
periodic trends
Solvent
30. Property of the elements that can be predicted from the arrangement of the periodic table
Normality
atomic theory
Nucleus
periodic trends
31. 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
Ion
Acid dissociation constant
Mass number
quanta
32. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
lewis base
solvation
quantum
Theoretical yield
33. A subdivision of an energy level in an atom. They are divided into orbitals.
Lewis definition
subshell
Acid dissociation constant
Henry's Law
34. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Charles and Gay Lussac's Law
London forces
Bronsted Lowry
35. 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.
Rate determining step
Effective nuclear charge
Emperical Formula
Covalent Bond
36. 2.18 x 10^-18 J/electron
quantum
Rydberg constant
ionic cmpound
Activation energy
37. A base that can accept two moles of H+ per mole of itself (ex: SO4
Dipole
Solution equilibrium
Diprotic Base
Magnetic quantum number
38. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Combination Reaction
Resonance structure
Bronsted Lowry
39. Sum of the protons and neutrons in an element often denoted by the letter A
theoretical yield
Mass number
Balmer series
molecule
40. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Equilibrium
STP
Strong acid
Group 5A
41. Named after their cation and anion
molecular weight
quanta
ionic cmpound
Mass number
42. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Disproportionation
Vapor pressure
Equivalence point
43. 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
Lewis acid base reaction
electron configuration
Equlibrium constant
atomic radius
44. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Magnetic quantum number
Combination Reaction
electromagnetic energy of photons emmited from electrons at ground state
molecular weight
45. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Vapor pressure
Diprotic Base
Common ion effect
compound
46. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
compound
Group 6A
Halogens
atomic emission spectrum
47. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
Common ion effect
Reaction mechanism
Raoult's Law
48. 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.
Balmer series
Ion product
heisenberg uncertainty principle
atomic radius
49. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Network covalent
Nucleus
Percent yield
Formula weight
50. 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
Avagadros number
Normality
Nucleus
pI