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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. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
bond energy
redox reaction
Ion dipole interactions
2. 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
und's rule
Reaction mechanism
Formula weight
representative elements
3. 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
Disproportionation
s orbital
periodic trends
Equlibrium constant
4. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Reaction mechanism
d orbital
Molality
Group 6A
5. 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
Formal Charge
decomposition reaction
STP
hydrogen bonding
6. A substance that - when dissolved in water - results in a solution that can conduct electricity
ionic cmpound
Electrolyte
Triple point
Electronegativity
7. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Conjugate acids and Bases
Combination Reaction
Strong acid
gram equivalent weight
8. An ionic compound that resists changes in its pH
s orbital
Buffer
electron affinity
Emperical Formula
9. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Half equivalence point
Solvent
Chemical Kinetics
compound
10. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Conjugate acids and Bases
solvation
single displacement reaction
Dispersion Forces
11. 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.
Lewis acid base reaction
Proton
percent composition
atomic radius
12. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Henry's Law
Diffusion
redox reaction
compound
13. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Pauli exclusion principle
Buffer
Bronsted - Lowry definition
Strong acid
14. The Percent by mass of each element in a compound.
Group 1A
Percent composition
Equilibrium
Water dissociation Constant
15. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Normality
Group 4A
Formal Charge
Resonance structure
16. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Conjugate acids and Bases
pi bonds
London forces
Spin quantum number
17. 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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18. Small discrete increments of energy.
Formula weight
quanta
law of constant composition
single displacement reaction
19. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Ion product
Ground state
Effusion
bond energy
20. 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.
Electrolyte
electron affinity
Collision theory of chemical Kinetics
Bronsted Lowry
21. 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
Triple point
Neutralization reaction
Resonance structure
Bronsted Lowry
22. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Triple point
atomic theory
mole
Combination Reaction
23. 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
single displacement reaction
Electrolyte
azimuthal quantum number
Arrhenius Definition
24. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
pi bonds
azimuthal quantum number
Bronsted - Lowry definition
25. 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
Aqueous Solution
s orbital
Buffer
decomposition reaction
26. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Group 2A
energy state
indicator
Formal Charge
27. 2.18 x 10^-18 J/electron
Rydberg constant
Ground state
Intermolecular forces
Dispersion Forces
28. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lyman series
redox reaction
electrolysis
Colligative properties
29. 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
Nonpolar covalent bond
Percent yield
Reaction mechanism
Dipole Dipole interaction
30. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Bronsted Lowry
Percent yield
redox reaction
electron configuration
31. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Normality
redox reaction
Reaction order
atomic radius
32. A solution in which water is the solvent
atomic emission spectrum
Aqueous Solution
Mass number
Group 7A
33. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Combination Reaction
Percent composition
Theoretical yield
Acid dissociation constant
34. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Ground state
gram equivalent weight
Concentration
Atomic weight
35. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Henry's Law
Proton
quantum
Diffusion
36. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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37. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Planck's Constant
Charles and Gay Lussac's Law
Alkaline earths
STP
38. An atom or group of atoms that has a positive or negative charge
Atomic weight
Ion
polymer
VSEPR
39. 5 valence electrons -3 ions - Nitride N
Diprotic Base
Group 5A
indicator
quantum numbers
40. 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.
Ground state
pI
Arrhenius Definition
crystalline solid
41. 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
Planck's Constant
crystalline solid
bond length
42. (chemistry) p(otential of) H(ydrogen)
atomic radius
Magnetic quantum number
pH
electrolysis
43. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Halogens
Noble gases
periodic trends
Principle quantum number
44. A dynamic condition in which two opposing changes occur at equal rates in a closed system
crystalline solid
molecular weight
Equilibrium
Electrolyte
45. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Titration
molecule
Neutralization reaction
Reaction mechanism
46. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Colligative properties
Decomposition reaction
Avagadros number
Ionic Bond
47. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Dipole Dipole interaction
Magnetic quantum number
empirical formula
Conjugate acids and Bases
48. 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.
Covalent Bond
Effective nuclear charge
Halogens
redox reaction
49. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Net ionic equation
decomposition reaction
Nonpolar covalent bond
single displacement reaction
50. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Buffer
Group 2A
Free radical
Balmer series