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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.
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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 physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
Strong acid
Common ion effect
Colligative properties
Titration
2. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
decomposition reaction
Octet Rule
Free radical
gram equivalent weight
3. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
single displacement reaction
mole
actinide series
Group 4A
4. Named after their cation and anion
Lyman series
pH
periodic trends
ionic cmpound
5. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Ground state
Percent yield
Percent composition
Lewis acid base reaction
6. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Neutralization reaction
Formal Charge
Strong acid
Magnetic quantum number
7. The Percent by mass of each element in a compound.
quantum numbers
Percent composition
Water dissociation Constant
single displacement reaction
8. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
sigma bond
STP
single displacement reaction
9. 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
Theoretical yield
Hydrogen bonding
Resonance structure
Atomic absorption Spectra
10. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Period
The bohr model
Combination Reaction
molecular weight
11. A definite stable energy that a physical system can have
energy state
Group 1A
Pauli exclusion principle
Chemical Kinetics
12. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Intermolecular forces
Balmer series
Principle quantum number
13. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
theoretical yield
Diprotic Base
Formula weight
Solubility Product Constant
14. 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
Group 7A
atomic radius
d orbital
Acid dissociation constant
15. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Lyman series
Raoult's Law
empirical formula
16. 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
angular momentum in the bohr model
Ion
Bronsted - Lowry definition
Formal Charge
17. 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
Acid dissociation constant
physical reaction
Common ion effect
Hydrogen bonding
18. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Aqueous Solution
Intermolecular forces
Collision theory of chemical Kinetics
Raoult's Law
19. The average distance between the nuclei of two bonded atoms
bond length
Octet Rule
polymer
mole
20. Tells you how much solute is present compared to the amount of solvent
Concentration
Azeotrope
Electrolyte
single displacement reaction
21. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
mole
Molarity
Le chateliers Principle
Alkaline earths
22. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
Solvent
Bronsted - Lowry definition
heisenberg uncertainty principle
23. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Dipole Dipole interaction
Activation energy
Nonpolar covalent bond
electromagnetic energy of photons emmited from electrons at ground state
24. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
atomic radius
atomic emission spectrum
Intermolecular forces
Emperical Formula
25. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
quantum
Colligative properties
Lewis definition
Molecular orbital
26. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Group 5A
Conjugate acids and Bases
electron affinity
Group 1A
27. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Henry's Law
pH
Half equivalence point
empirical formula
28. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
London forces
Formula weight
solvation
29. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Ion
Group 7A
gram equivalent weight
Phase diagram
30. 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.
Group 3A
Nucleus
Reaction mechanism
angular momentum in the bohr model
31. Property of the elements that can be predicted from the arrangement of the periodic table
Ion
periodic trends
Percent yield
single displacement reaction
32. 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
Phase diagram
Net ionic equation
Buffer
33. A subdivision of an energy level in an atom. They are divided into orbitals.
Noble gases
quantum
Principle quantum number
subshell
34. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Nucleus
Molality
polymer
Henderson Hasselbalch Equation
35. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Half equivalence point
Ion dipole interactions
compound
Pauli exclusion principle
36. 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
Mass number
Activation energy
Molarity
37. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Solvent
Nucleus
Halogens
Free radical
38. An elementary particle with 0 charge and mass about equal to a proton
Neutron
pI
Group 6A
indicator
39. PH of a molecule at which it contains no net electric charge - isoelectric point.
Formal Charge
Formula weight
gram equivalent weight
pI
40. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Molality
Hydrogen bonding
Dipole Dipole interaction
redox reaction
41. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
theoretical yield
Effective nuclear charge
Neutralization reaction
42. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Chemical Kinetics
crystalline solid
Free radical
Group 4A
43. The lowest allowable energy state of an atom
Net ionic equation
Ground state
representative elements
Electrolyte
44. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
physical reaction
sigma bond
amorphous solid
lathanide series
45. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Conjugate acids and Bases
Neutralization reaction
Group 5A
Phase diagram
46. 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.
Electronegativity
atomic theory
Acid dissociation constant
atomic radius
47. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Group 2A
Lyman series
actinide series
Reaction order
48. A base that can accept two moles of H+ per mole of itself (ex: SO4
London forces
STP
Diprotic Base
Neutron
49. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Diffusion
molecular weight
Titration
50. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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