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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. 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
Ionic Bond
s orbital
subshell
Strong acid
2. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Group 1A
Intermolecular forces
Emperical Formula
Bronsted - Lowry definition
3. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Ion dipole interactions
Reaction mechanism
Titration
Conjugate acids and Bases
4. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Group 7A
Dipole
Theoretical yield
Half equivalence point
5. 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
Lewis structure
molecule
Hydrogen bonding
Disproportionation
6. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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7. The slowest elementary step which is the limit for the rate of the other steps
energy state
Lyman series
Ion product
Rate determining step
8. A reaction where a compound does Not change its molecular structure.
Azeotrope
lewis base
Electrolyte
physical reaction
9. 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
Formal Charge
Dipole
chemical reaction
Group 5A
10. An ionic compound that resists changes in its pH
Buffer
Solution equilibrium
Covalent Bond
Lewis structure
11. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Equilibrium
Diprotic Base
Diffusion
12. 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.
amorphous solid
hydrogen bonding
electron affinity
Octet Rule
13. Two or more atoms held together by covalent bonds
molecule
Noble gases
quantum
empirical formula
14. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Reaction order
Lyman series
Equilibrium
STP
15. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
STP
Triple point
Magnetic quantum number
pi bonds
16. PH of a molecule at which it contains no net electric charge - isoelectric point.
Network covalent
pI
Strong acid
Group 3A
17. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Ion
Formal Charge
single displacement reaction
18. 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
Disproportionation
Lyman series
Ion
Equlibrium constant
19. The energy required to break a chemical bond and form neutral isolated atoms
theoretical yield
angular momentum in the bohr model
Bronsted Lowry
bond energy
20. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Charles and Gay Lussac's Law
Octet Rule
Solution equilibrium
d orbital
21. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
quantum numbers
Buffer
Neutron
22. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Equivalence point
hydrogen bonding
azimuthal quantum number
Proton
23. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Vapor pressure
Noble gases
Halogens
Emperical Formula
24. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
polymer
Magnetic quantum number
lewis base
Conjugate acids and Bases
25. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
electrolysis
Conjugate acids and Bases
Lewis definition
26. Tells you how much solute is present compared to the amount of solvent
quantum
physical reaction
Solution equilibrium
Concentration
27. 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
Solubility Product Constant
Disproportionation
solvation
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
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29. 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
Emperical Formula
Effusion
Ionization energy
Bronsted - Lowry definition
30. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Nonpolar covalent bond
Azeotrope
Net ionic equation
31. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
indicator
Common ion effect
Bronsted - Lowry definition
Atomic weight
32. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
redox reaction
sigma bond
Equlibrium constant
Solute
33. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
heisenberg uncertainty principle
Reaction mechanism
Molarity
Period
34. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Effusion
Colligative properties
Formal Charge
solvation
35. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Reaction mechanism
London forces
Water dissociation Constant
mole
36. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
molecular weight
Dipole Dipole interaction
Group 3A
37. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Equivalence point
lathanide series
Balmer series
Combination Reaction
38. The process by which one or more substances change to produce one or more different substances
Percent yield
single displacement reaction
Phase diagram
chemical reaction
39. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
gram equivalent weight
Rate law
VSEPR
quantum
40. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Reaction mechanism
Molar solubility
Neutralization reaction
41. Chalcogens - - Oxide O
pH
Charles and Gay Lussac's Law
Planck's Constant
Group 6A
42. Any sample of a given compound will contain the same elements in the identical mass ratio.
electrolysis
Effusion
law of constant composition
Charles and Gay Lussac's Law
43. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
Reaction mechanism
Intermolecular forces
Ion dipole interactions
Water dissociation Constant
44. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Aqueous Solution
Lyman series
Formal Charge
Group 4A
45. An atom or group of atoms that has a positive or negative charge
Noble gases
chemical reaction
Ion
angular momentum in the bohr model
46. 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.
redox reaction
Principle quantum number
Halogens
Balmer series
47. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Ground state
Equilibrium
Percent yield
decomposition reaction
48. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Group 4A
Group 3A
Chemical Kinetics
Rate determining step
49. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Ion dipole interactions
Vapor pressure
Dispersion Forces
50. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Formula weight
VSEPR
Electronegativity
Redox Half Reaction
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