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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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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. 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
atomic radius
bond length
Formal Charge
Water dissociation Constant
2. 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.
redox reaction
molecule
VSEPR
Mass number
3. 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
Molar solubility
atomic radius
Acid dissociation constant
4. 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
Arrhenius Definition
Dispersion Forces
Water dissociation Constant
Magnetic quantum number
5. 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
Solute
representative elements
Network covalent
The bohr model
6. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
s orbital
Vapor pressure
Le chateliers Principle
7. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Phase diagram
pi bonds
Lewis structure
Group 7A
8. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Group 7A
Electronegativity
Balmer series
angular momentum in the bohr model
9. 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
Theoretical yield
Halogens
Equivalence point
Group 7A
10. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
compound
ionic cmpound
Effective nuclear charge
atomic theory
11. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
redox reaction
Ground state
Pauli exclusion principle
representative elements
12. 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
Group 6A
Vapor pressure
Ion
13. Substance in which a solute is dissolved to form a solution
Charles and Gay Lussac's Law
Solvent
atomic radius
pI
14. The slowest elementary step which is the limit for the rate of the other steps
energy state
Reaction mechanism
Rate determining step
Equivalence point
15. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Group 3A
sigma bond
Equilibrium
Dipole
16. A subdivision of an energy level in an atom. They are divided into orbitals.
Rate law
Disproportionation
Triple point
subshell
17. The Percent by mass of each element in a compound.
Group 7A
subshell
Percent composition
molecule
18. 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
Principle quantum number
lewis base
ionic cmpound
Ionic Bond
19. An ionic compound that resists changes in its pH
Group 2A
Formula weight
Buffer
lewis base
20. 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.
Ionization energy
Azeotrope
Le chateliers Principle
electron affinity
21. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Rate determining step
effective nuclear charge
Water dissociation Constant
Equilibrium
22. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Arrhenius Definition
Percent yield
Azeotrope
23. 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
Spin quantum number
bond energy
Nucleus
Common ion effect
24. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
pi bonds
Water dissociation Constant
Molality
25. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
subshell
solvation
Octet Rule
Group 5A
26. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
molecular weight
subshell
Common ion effect
Dipole
27. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Common ion effect
empirical formula
Atomic weight
28. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Charles and Gay Lussac's Law
Group 5A
Chemical Kinetics
29. Rare earth element group (elements 58-71)
Avagadros number
lathanide series
Group 3A
Ionic Bond
30. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
molecular weight
Electronegativity
lewis base
redox reaction
31. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Henderson Hasselbalch Equation
Rate law
compound
und's rule
32. Gram equivalent weight of solute per liter of solution - often denoted by N.
Decomposition reaction
Normality
Group 3A
Hydrogen bonding
33. Elements in the middle of the periodic table - in groups 3-12.
pi bonds
transition elements
Ionic Bond
Aqueous Solution
34. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Le chateliers Principle
electron affinity
Equivalence point
Chemical Kinetics
35. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Resonance structure
Aqueous Solution
decomposition reaction
Redox Half Reaction
36. 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
Group 7A
Alkaline earths
Electrolyte
Dispersion Forces
37. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Group 4A
Dipole Dipole interaction
electron affinity
Theoretical yield
38. Structure that occurs when it is possible to draw two or more valid electron dot structures that have the same number of electron pairs for a molecule or ion
bond length
Resonance structure
Vapor pressure
Nonpolar covalent bond
39. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Noble gases
Nonpolar covalent bond
Octet Rule
Dispersion Forces
40. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Emperical Formula
atomic emission spectrum
Covalent Bond
percent composition
41. Sum of the protons and neutrons in an element often denoted by the letter A
quantum
Ion product
Mass number
lewis base
42. Chalcogens - - Oxide O
Avagadros number
compound
lewis base
Group 6A
43. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
redox reaction
electromagnetic energy of photons emmited from electrons at ground state
polymer
Nonpolar covalent bond
44. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
Intermolecular forces
gram equivalent weight
Electronegativity
45. 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
Water dissociation Constant
bond length
Amphoteric
46. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
VSEPR
Vapor pressure
Reaction order
solvation
47. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Free radical
energy state
Ground state
Covalent Bond
48. Simplest whole # ration of atoms in a compound
Emperical Formula
Molarity
atomic radius
Arrhenius Definition
49. 5 valence electrons -3 ions - Nitride N
bond energy
Group 1A
transition elements
Group 5A
50. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
Rate law
electrolysis
Theoretical yield
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