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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. Substance in which a solute is dissolved to form a solution
indicator
Balmer series
STP
Solvent
2. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
und's rule
Activation energy
gram equivalent weight
Theoretical yield
3. 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
Free radical
compound
representative elements
Resonance structure
4. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Rydberg constant
single displacement reaction
Ion product
Formula weight
5. 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 structure
Equlibrium constant
Disproportionation
quanta
6. Mixture of 2 or more substances that distills at a constant temperature and with constant composition - even though seperately the components have different boiling points
Azeotrope
empirical formula
polymer
Ground state
7. Slightly less reactive than alkali metals - comprise group II
Electronegativity
Alkaline earths
Graham's Law
Network covalent
8. 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
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9. 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
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10. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Collision theory of chemical Kinetics
Hydrogen bonding
Rate law
11. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Graham's Law
Decomposition reaction
Amphoteric
indicator
12. The percent by mass of each element in a compound
percent composition
effective nuclear charge
Lewis definition
Ionization energy
13. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Pauli exclusion principle
Octet Rule
Electronegativity
electron configuration
14. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
gram equivalent weight
Lyman series
Arrhenius Definition
compound
15. (chemistry) p(otential of) H(ydrogen)
Period
Chemical Kinetics
pH
Combination Reaction
16. A reaction where a compound does Not change its molecular structure.
law of constant composition
physical reaction
redox reaction
London forces
17. An elementary particle with 0 charge and mass about equal to a proton
Bronsted Lowry
Collision theory of chemical Kinetics
Normality
Neutron
18. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Normality
Equilibrium
Group 3A
Lewis acid base reaction
19. 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.
Ion product
Balmer series
gram equivalent weight
Rate determining step
20. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
Collision theory of chemical Kinetics
Lewis acid base reaction
Intermolecular forces
21. 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
Resonance structure
crystalline solid
Theoretical yield
22. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Formula weight
Equivalence point
Arrhenius Definition
Dipole
23. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Formal Charge
Phase diagram
empirical formula
Spin quantum number
24. Property of the elements that can be predicted from the arrangement of the periodic table
periodic trends
Principle quantum number
empirical formula
Dispersion Forces
25. 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.
Diffusion
Spin quantum number
Rydberg constant
Redox Half Reaction
26. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
pH
Water dissociation Constant
Net ionic equation
Balmer series
27. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Nucleus
Hydrogen bonding
s orbital
28. 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
ionic cmpound
Electrolyte
Group 7A
Diffusion
29. An atom or group of atoms that has a positive or negative charge
Atomic weight
Ion
VSEPR
STP
30. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
lathanide series
Dipole
Redox Half Reaction
31. 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
quantum
electromagnetic energy of photons emmited from electrons at ground state
atomic emission spectrum
azimuthal quantum number
32. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
redox reaction
theoretical yield
electromagnetic energy of photons emmited from electrons at ground state
33. 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
Avagadros number
Hydrogen bonding
Atomic absorption Spectra
Network covalent
34. 5 valence electrons -3 ions - Nitride N
Group 5A
atomic emission spectrum
Molecular orbital
Rydberg constant
35. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Equilibrium
und's rule
Chemical Kinetics
36. 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
Solvent
Lewis structure
Ionization energy
Ion
37. The Percent by mass of each element in a compound.
Collision theory of chemical Kinetics
Group 5A
Spin quantum number
Percent composition
38. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
sigma bond
mole
Atomic weight
Formal Charge
39. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Azeotrope
Group 6A
Ion dipole interactions
Molar solubility
40. A solution in which water is the solvent
Ionic Bond
mole
Acid dissociation constant
Aqueous Solution
41. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Percent composition
Combination Reaction
polymer
Equlibrium constant
42. 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
solvation
London forces
Group 1A
Spin quantum number
43. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Nonpolar covalent bond
Percent yield
Avagadros number
44. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
redox reaction
STP
Graham's Law
actinide series
45. 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
quantum
Equilibrium
Colligative properties
Equlibrium constant
46. A horizontal row of elements in the periodic table
d orbital
quantum
Raoult's Law
Period
47. 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
lewis base
Balmer series
Collision theory of chemical Kinetics
s orbital
48. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Conjugate acids and Bases
Nonpolar covalent bond
redox reaction
Azeotrope
49. 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
chemical reaction
Vapor pressure
Planck's Constant
Resonance structure
50. 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
sigma bond
London forces
Noble gases
theoretical yield