SUBJECTS
|
BROWSE
|
CAREER CENTER
|
POPULAR
|
JOIN
|
LOGIN
Business Skills
|
Soft Skills
|
Basic Literacy
|
Certifications
About
|
Help
|
Privacy
|
Terms
|
Email
Search
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. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Reaction mechanism
Effective nuclear charge
Group 4A
actinide series
2. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Lyman series
Molarity
Strong acid
Theoretical yield
3. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
Neutron
Group 5A
heisenberg uncertainty principle
4. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
percent composition
electron affinity
Magnetic quantum number
redox reaction
5. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Equivalence point
Bronsted - Lowry definition
redox reaction
Atomic weight
6. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Rydberg constant
Amphoteric
azimuthal quantum number
Strong acid
7. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Titration
Proton
Dipole
8. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
Solubility Product Constant
chemical reaction
Charles and Gay Lussac's Law
atomic emission spectrum
9. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
und's rule
electron affinity
heisenberg uncertainty principle
Vapor pressure
10. 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
single displacement reaction
Group 7A
Diprotic Base
Reaction order
11. 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
azimuthal quantum number
molecule
Network covalent
atomic theory
12. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
molecule
Group 1A
atomic radius
13. The quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
Principle quantum number
Group 2A
Ground state
mole
14. Common definition of acids as proton (H+) donors and bases as proton acceptors
angular momentum in the bohr model
Solution equilibrium
Net ionic equation
Bronsted - Lowry definition
15. 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
Diffusion
transition elements
Formal Charge
single displacement reaction
16. Tells you how much solute is present compared to the amount of solvent
ionic cmpound
redox reaction
Normality
Concentration
17. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Henderson Hasselbalch Equation
Henry's Law
Halogens
Reaction order
18. A definite stable energy that a physical system can have
quanta
energy state
redox reaction
effective nuclear charge
19. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
20. An atom or group of atoms that has a positive or negative charge
Ion
bond energy
ionic cmpound
pi bonds
21. 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 radius
crystalline solid
Period
22. 2.18 x 10^-18 J/electron
Electronegativity
Rydberg constant
Concentration
physical reaction
23. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
Activation energy
decomposition reaction
Redox Half Reaction
hydrogen bonding
24. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
crystalline solid
Avagadros number
Ground state
Group 3A
25. A base that can accept two moles of H+ per mole of itself (ex: SO4
decomposition reaction
Diprotic Base
quantum numbers
Ion
26. 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.
Reaction order
Effective nuclear charge
Arrhenius Definition
VSEPR
27. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
pi bonds
Solution equilibrium
bond length
Dipole
28. Elements in the middle of the periodic table - in groups 3-12.
quantum
law of constant composition
Group 7A
transition elements
29. Slightly less reactive than alkali metals - comprise group II
Ionization energy
Alkaline earths
theoretical yield
pi bonds
30. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Equlibrium constant
Effusion
electrolysis
Ionization energy
31. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Formal Charge
Mass number
Period
32. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Formula weight
pI
Ion
33. A chemical bond in which one atom loses an electron to form a positive ion and the other atom gains to electron to form a negative ion
Ionic Bond
Period
VSEPR
heisenberg uncertainty principle
34. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Noble gases
Ion
s orbital
Group 7A
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
Vapor pressure
Arrhenius Definition
Neutron
Lewis acid base reaction
36. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
Theoretical yield
electron configuration
Lewis acid base reaction
37. 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
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
38. 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
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
39. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
40. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Effective nuclear charge
Dispersion Forces
Decomposition reaction
Ion dipole interactions
41. 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
Phase diagram
The bohr model
polymer
Titration
42. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Bronsted Lowry
Alkaline earths
crystalline solid
Solute
43. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Nonpolar covalent bond
atomic theory
Net ionic equation
redox reaction
44. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
und's rule
Triple point
Combination Reaction
Acid dissociation constant
45. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Percent yield
Magnetic quantum number
sigma bond
Conjugate acids and Bases
46. 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
Group 1A
d orbital
Buffer
London forces
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
The bohr model
Amphoteric
Diffusion
decomposition reaction
48. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Formula weight
electromagnetic energy of photons emmited from electrons at ground state
Neutralization reaction
49. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Atomic absorption Spectra
Alkaline earths
Reaction order
50. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Lyman series
Planck's Constant
Period
empirical formula