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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. 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.
crystalline solid
Amphoteric
Buffer
Balmer series
2. 5 different orbitals shaped like clover leaves and max electrons is 10
Reaction order
Buffer
d orbital
azimuthal quantum number
3. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
hydrogen bonding
Dispersion Forces
Charles and Gay Lussac's Law
Group 1A
4. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
The bohr model
Solution equilibrium
molecule
5. 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.
Nonpolar covalent bond
Equivalence point
Proton
VSEPR
6. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
subshell
Electrolyte
Molality
Effusion
7. A definite stable energy that a physical system can have
Water dissociation Constant
Half equivalence point
energy state
Acid dissociation constant
8. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
effective nuclear charge
Chemical Kinetics
Solubility Product Constant
9. Slightly less reactive than alkali metals - comprise group II
Electrolyte
Alkaline earths
Ion
Emperical Formula
10. 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
Magnetic quantum number
Neutron
representative elements
pH
11. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
atomic emission spectrum
Formula weight
Proton
Henry's Law
12. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Free radical
Aqueous Solution
Henderson Hasselbalch Equation
actinide series
13. Two or more atoms held together by covalent bonds
molecule
Henderson Hasselbalch Equation
Rate law
redox reaction
14. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
STP
atomic emission spectrum
electron affinity
redox reaction
15. 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
VSEPR
angular momentum in the bohr model
Free radical
Dispersion Forces
16. 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
Molar solubility
Alkaline earths
Molecular orbital
Group 7A
17. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Effective nuclear charge
Acid dissociation constant
Conjugate acids and Bases
transition elements
18. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
crystalline solid
Net ionic equation
Phase diagram
19. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
London forces
Henry's Law
Triple point
Hydrogen bonding
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
Dipole
quanta
Hydrogen bonding
Effective nuclear charge
21. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
theoretical yield
gram equivalent weight
Reaction order
22. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Phase diagram
STP
atomic emission spectrum
Molality
23. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
atomic radius
Atomic absorption Spectra
Lewis acid base reaction
24. The slowest elementary step which is the limit for the rate of the other steps
Vapor pressure
atomic emission spectrum
Rate determining step
Diffusion
25. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Group 7A
Proton
Group 5A
compound
26. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
atomic emission spectrum
Formula weight
London forces
Group 2A
27. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
law of constant composition
Diprotic Base
Conjugate acids and Bases
Atomic weight
28. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Electronegativity
Magnetic quantum number
transition elements
Le chateliers Principle
29. The Percent by mass of each element in a compound.
Intermolecular forces
Diprotic Base
Mass number
Percent composition
30. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Bronsted - Lowry definition
compound
Solution equilibrium
Phase diagram
31. 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.
sigma bond
Molar solubility
percent composition
Effective nuclear charge
32. Sum of the protons and neutrons in an element often denoted by the letter A
Normality
Mass number
Octet Rule
VSEPR
33. The area of chemistry that is concerned with reaction rates and reaction mechanisms
heisenberg uncertainty principle
Rate determining step
Chemical Kinetics
electron affinity
34. 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
hydrogen bonding
Lewis definition
s orbital
Nucleus
35. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
mole
law of constant composition
Rate law
Octet Rule
36. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
London forces
Network covalent
law of constant composition
electron configuration
37. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Resonance structure
atomic radius
STP
38. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
indicator
Activation energy
und's rule
Aqueous Solution
39. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Normality
Reaction order
The bohr model
Halogens
40. 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-
Water dissociation Constant
Proton
Effective nuclear charge
empirical formula
41. A reaction in which atoms of one element take the place of atoms of another element in a compound
Nucleus
Ion
lewis base
single displacement reaction
42. Simplest whole # ration of atoms in a compound
Activation energy
Percent yield
Emperical Formula
bond energy
43. 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.
mole
electron affinity
Vapor pressure
Aqueous Solution
44. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Conjugate acids and Bases
solvation
Collision theory of chemical Kinetics
Proton
45. A base that can accept two moles of H+ per mole of itself (ex: SO4
atomic theory
Diprotic Base
Rate law
chemical reaction
46. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Common ion effect
Dispersion Forces
Halogens
Molality
47. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
electromagnetic energy of photons emmited from electrons at ground state
atomic radius
The bohr model
Solution equilibrium
48. Chalcogens - - Oxide O
Group 6A
heisenberg uncertainty principle
periodic trends
Activation energy
49. The lowest allowable energy state of an atom
Network covalent
Theoretical yield
Ground state
quanta
50. 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
Arrhenius Definition
Ion dipole interactions
Chemical Kinetics
bond length