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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. Having characteristics of both an acid and a base and capable of reacting as either
pI
Molar solubility
Reaction order
Amphoteric
2. 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
Effusion
Ionization energy
Spin quantum number
Molecular orbital
3. E=hc/?
Combination Reaction
electromagnetic energy of photons emmited from electrons at ground state
Ion dipole interactions
Formula weight
4. PH of a molecule at which it contains no net electric charge - isoelectric point.
Ion product
Group 5A
Charles and Gay Lussac's Law
pI
5. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Pauli exclusion principle
Disproportionation
Atomic absorption Spectra
Theoretical yield
6. A horizontal row of elements in the periodic table
Period
Group 2A
Collision theory of chemical Kinetics
mole
7. An elementary particle with 0 charge and mass about equal to a proton
Chemical Kinetics
Equivalence point
Neutron
Group 5A
8. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
atomic emission spectrum
Dispersion Forces
Ion product
9. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Lewis definition
Combination Reaction
Halogens
law of constant composition
10. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Activation energy
quantum
Lewis structure
11. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Solute
bond energy
indicator
Dipole Dipole interaction
12. Common definition of acids as proton (H+) donors and bases as proton acceptors
electromagnetic energy of photons emmited from electrons at ground state
Bronsted - Lowry definition
hydrogen bonding
Half equivalence point
13. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
compound
Dipole
Planck's Constant
14. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Percent composition
Percent yield
Conjugate acids and Bases
Group 4A
15. 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
Electrolyte
Lewis acid base reaction
Intermolecular forces
Percent yield
16. The percent by mass of each element in a compound
atomic theory
Effective nuclear charge
percent composition
Spin quantum number
17. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
periodic trends
Group 7A
Formula weight
Hydrogen bonding
18. 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
Resonance structure
Effusion
Balmer series
atomic radius
19. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
decomposition reaction
Proton
atomic emission spectrum
Molar solubility
20. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Normality
Triple point
empirical formula
Collision theory of chemical Kinetics
21. Chalcogens - - Oxide O
Group 6A
Le chateliers Principle
crystalline solid
Noble gases
22. 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.
Electronegativity
Effective nuclear charge
Colligative properties
Solute
23. A reaction where a compound does Not change its molecular structure.
Half equivalence point
Period
physical reaction
chemical reaction
24. Orbitals of equal energy are each occupied by one electron before any orbital is occupied by a second electron - and all electrons in singly occupied orbitals must have the same spin
25. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
crystalline solid
quantum numbers
Lewis acid base reaction
London forces
26. Small discrete increments of energy.
Principle quantum number
transition elements
quanta
Rydberg constant
27. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Aqueous Solution
Acid dissociation constant
transition elements
28. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
29. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
percent composition
decomposition reaction
lewis base
30. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Diprotic Base
Mass number
Activation energy
Ion
31. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
pI
Phase diagram
molecule
Percent yield
32. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
energy state
Spin quantum number
Ion dipole interactions
33. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Diffusion
Ionization energy
single displacement reaction
34. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Principle quantum number
Concentration
Lyman series
Common ion effect
35. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 4A
polymer
percent composition
Balmer series
36. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Le chateliers Principle
Spin quantum number
Effusion
angular momentum in the bohr model
37. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Resonance structure
Ionic Bond
crystalline solid
38. 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
Percent composition
Bronsted Lowry
Spin quantum number
Solute
39. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Bronsted Lowry
Molarity
pI
Electronegativity
40. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
41. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Balmer series
pI
Octet Rule
Mass number
42. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Henderson Hasselbalch Equation
Aqueous Solution
actinide series
Common ion effect
43. Simplest whole # ration of atoms in a compound
Effusion
Network covalent
Rate law
Emperical Formula
44. 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
compound
Percent yield
Equlibrium constant
Group 2A
45. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
Group 4A
gram equivalent weight
pi bonds
46. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
Neutralization reaction
Ion product
empirical formula
Decomposition reaction
47. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Effective nuclear charge
Azeotrope
mole
48. 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
Ion product
quantum numbers
London forces
Solute
49. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Ion dipole interactions
Rate law
Magnetic quantum number
Conjugate acids and Bases
50. Gram equivalent weight of solute per liter of solution - often denoted by N.
Alkaline earths
Nucleus
Azeotrope
Normality