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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 reaction in which atoms of one element take the place of atoms of another element in a compound
Nucleus
single displacement reaction
Effusion
Percent composition
2. Small discrete increments of energy.
Concentration
redox reaction
energy state
quanta
3. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
electron configuration
indicator
Net ionic equation
4. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
heisenberg uncertainty principle
Lyman series
Phase diagram
bond energy
5. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
periodic trends
Noble gases
Pauli exclusion principle
6. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
gram equivalent weight
pi bonds
crystalline solid
Dipole
7. 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-
Group 6A
Rate law
Water dissociation Constant
empirical formula
8. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
The bohr model
Resonance structure
Network covalent
Solubility Product Constant
9. Elements in the middle of the periodic table - in groups 3-12.
transition elements
electromagnetic energy of photons emmited from electrons at ground state
Bronsted - Lowry definition
d orbital
10. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Conjugate acids and Bases
periodic trends
Effusion
mole
11. The energy required to break a chemical bond and form neutral isolated atoms
physical reaction
Principle quantum number
Henderson Hasselbalch Equation
bond energy
12. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Combination Reaction
Solubility Product Constant
Le chateliers Principle
electron affinity
13. 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.
Group 1A
Molar solubility
Intermolecular forces
Equivalence point
14. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Emperical Formula
crystalline solid
Lewis structure
percent composition
15. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Group 2A
periodic trends
Activation energy
Lyman series
16. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital
Atomic weight
Azeotrope
Neutron
Spin quantum number
17. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Group 3A
Lewis structure
Lewis definition
Solubility Product Constant
18. The process by which one or more substances change to produce one or more different substances
molecular weight
chemical reaction
Titration
Free radical
19. A solution in which water is the solvent
Electrolyte
Equlibrium constant
pH
Aqueous Solution
20. 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
periodic trends
Hydrogen bonding
polymer
Diffusion
21. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
compound
Formal Charge
Halogens
Alkaline earths
22. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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23. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
sigma bond
Solubility Product Constant
Electrolyte
Conjugate acids and Bases
24. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
solvation
Effective nuclear charge
Lewis structure
25. 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
Network covalent
Reaction mechanism
Disproportionation
Formal Charge
26. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Ion dipole interactions
Percent yield
Neutron
27. 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
Normality
Titration
Molarity
Ion
28. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
actinide series
Phase diagram
energy state
Intermolecular forces
29. Redox reaction - in which the same species is both oxidized and reduced.
Disproportionation
Resonance structure
Triple point
Magnetic quantum number
30. Rare earth element group (elements 58-71)
Diprotic Base
heisenberg uncertainty principle
lathanide series
Lewis acid base reaction
31. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
Atomic absorption Spectra
Percent yield
Strong acid
Ion dipole interactions
32. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Halogens
Formula weight
Group 6A
Emperical Formula
33. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
sigma bond
d orbital
redox reaction
Decomposition reaction
34. 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.
decomposition reaction
percent composition
Group 3A
Collision theory of chemical Kinetics
35. 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
Electronegativity
Arrhenius Definition
Reaction mechanism
STP
36. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Ion product
Equivalence point
Collision theory of chemical Kinetics
37. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
heisenberg uncertainty principle
Reaction mechanism
sigma bond
Spin quantum number
38. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
polymer
electron configuration
Covalent Bond
Disproportionation
39. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
gram equivalent weight
representative elements
pH
40. Property of the elements that can be predicted from the arrangement of the periodic table
lewis base
Neutron
Disproportionation
periodic trends
41. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
gram equivalent weight
Atomic weight
Electrolyte
Bronsted Lowry
42. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Avagadros number
Formula weight
Molarity
Neutron
43. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
STP
Equlibrium constant
Charles and Gay Lussac's Law
44. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Atomic absorption Spectra
Group 4A
law of constant composition
lathanide series
45. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Effusion
Theoretical yield
crystalline solid
Dipole Dipole interaction
46. The average distance between the nuclei of two bonded atoms
Network covalent
amorphous solid
bond length
Group 3A
47. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Reaction order
bond length
Rate determining step
48. 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
Ion
Atomic absorption Spectra
Octet Rule
Percent yield
49. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
London forces
Intermolecular forces
Charles and Gay Lussac's Law
50. Second quantum number - designated by the letter 'l.' This 'angular momentum' refers to the subshells within each principle quantum energy level. It can take on the value of an integer in the 0 to (n -1) range. The four subshellscorresponding to l=0
Decomposition reaction
Solubility Product Constant
azimuthal quantum number
Ionization energy