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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. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Percent yield
Free radical
Neutron
Effusion
2. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
Azeotrope
Triple point
Chemical Kinetics
3. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Intermolecular forces
Group 4A
Decomposition reaction
4. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
indicator
molecular weight
lewis base
heisenberg uncertainty principle
5. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Common ion effect
Henderson Hasselbalch Equation
Diprotic Base
Charles and Gay Lussac's Law
6. A definite stable energy that a physical system can have
sigma bond
energy state
Formula weight
Charles and Gay Lussac's Law
7. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
effective nuclear charge
Period
VSEPR
electrolysis
8. The Percent by mass of each element in a compound.
Group 5A
mole
Combination Reaction
Percent composition
9. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Covalent Bond
sigma bond
Strong acid
periodic trends
10. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Amphoteric
actinide series
pi bonds
11. Small discrete increments of energy.
quanta
Common ion effect
Formula weight
Rate determining step
12. 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.
pi bonds
The bohr model
Redox Half Reaction
Group 7A
13. 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.
Charles and Gay Lussac's Law
periodic trends
Electronegativity
crystalline solid
14. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
pH
Nonpolar covalent bond
Formula weight
hydrogen bonding
15. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Balmer series
molecular weight
pi bonds
heisenberg uncertainty principle
16. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
indicator
Resonance structure
Colligative properties
Diprotic Base
17. (chemistry) p(otential of) H(ydrogen)
pH
Spin quantum number
Proton
Pauli exclusion principle
18. 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.
gram equivalent weight
Dipole Dipole interaction
Principle quantum number
chemical reaction
19. 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
s orbital
subshell
Planck's Constant
Electronegativity
20. 5 valence electrons -3 ions - Nitride N
Group 5A
Azeotrope
Decomposition reaction
Halogens
21. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
Principle quantum number
Equivalence point
indicator
22. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Neutron
Molecular orbital
solvation
Concentration
23. 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.
atomic radius
percent composition
Effective nuclear charge
Lewis structure
24. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
crystalline solid
hydrogen bonding
Net ionic equation
Avagadros number
25. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
quantum numbers
Balmer series
Nucleus
Conjugate acids and Bases
26. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Bronsted - Lowry definition
Graham's Law
Nonpolar covalent bond
Diffusion
27. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
ionic cmpound
Normality
sigma bond
pi bonds
28. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Neutralization reaction
Diprotic Base
Common ion effect
electromagnetic energy of photons emmited from electrons at ground state
29. 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
Lewis acid base reaction
Rate law
molecule
Equlibrium constant
30. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
atomic radius
Group 3A
Noble gases
bond length
31. 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
solvation
Solute
representative elements
Diprotic Base
32. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Lyman series
Nucleus
empirical formula
redox reaction
33. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Rate determining step
Ion
Bronsted - Lowry definition
34. Rare earth element group (elements 58-71)
solvation
Water dissociation Constant
lathanide series
Atomic weight
35. 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.
Balmer series
Mass number
Atomic absorption Spectra
Half equivalence point
36. The area of chemistry that is concerned with reaction rates and reaction mechanisms
atomic theory
Percent composition
Molarity
Chemical Kinetics
37. The slowest elementary step which is the limit for the rate of the other steps
und's rule
Dispersion Forces
gram equivalent weight
Rate determining step
38. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Molecular orbital
Ion dipole interactions
angular momentum in the bohr model
Common ion effect
39. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Effective nuclear charge
Formula weight
crystalline solid
Group 2A
40. Tells you how much solute is present compared to the amount of solvent
mole
Formal Charge
Concentration
Neutron
41. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
VSEPR
Magnetic quantum number
Group 4A
Raoult's Law
42. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
redox reaction
Network covalent
Charles and Gay Lussac's Law
Balmer series
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.
representative elements
electron affinity
Water dissociation Constant
amorphous solid
44. 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
London forces
Mass number
Group 3A
Titration
45. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
electron configuration
Colligative properties
sigma bond
46. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Theoretical yield
Arrhenius Definition
electron affinity
47. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
polymer
Halogens
d orbital
molecular weight
48. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
mole
redox reaction
lathanide series
Lyman series
49. 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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50. The process by which one or more substances change to produce one or more different substances
chemical reaction
molecule
Atomic absorption Spectra
Formula weight