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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 quantum number that indicates the main energy level occupied by the electron. Can theoretically take on any positive interger. Denoted by the letter n.
percent composition
Principle quantum number
Hydrogen bonding
Octet Rule
2. Property of the elements that can be predicted from the arrangement of the periodic table
hydrogen bonding
Lyman series
Neutralization reaction
periodic trends
3. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Lyman series
Combination Reaction
electromagnetic energy of photons emmited from electrons at ground state
compound
4. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
crystalline solid
Amphoteric
Arrhenius Definition
5. 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.
Hydrogen bonding
Atomic absorption Spectra
pH
atomic emission spectrum
6. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
Collision theory of chemical Kinetics
Ion
subshell
7. The Percent by mass of each element in a compound.
Percent composition
London forces
Graham's Law
quantum numbers
8. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
9. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture
Common ion effect
Intermolecular forces
Solution equilibrium
Buffer
10. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
hydrogen bonding
Covalent Bond
Period
11. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Solute
Henry's Law
STP
Covalent Bond
12. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 3A
Group 2A
Molar solubility
d orbital
13. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
crystalline solid
Network covalent
Molar solubility
effective nuclear charge
14. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Henderson Hasselbalch Equation
single displacement reaction
mole
15. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
electron affinity
transition elements
Intermolecular forces
Molality
16. 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
Percent yield
effective nuclear charge
azimuthal quantum number
Lewis acid base reaction
17. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Diprotic Base
Buffer
Strong acid
empirical formula
18. A base that can accept two moles of H+ per mole of itself (ex: SO4
Reaction order
Diprotic Base
angular momentum in the bohr model
Acid dissociation constant
19. Having characteristics of both an acid and a base and capable of reacting as either
Dipole
Amphoteric
electrolysis
Electrolyte
20. 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
redox reaction
representative elements
Emperical Formula
Normality
21. E=hc/?
s orbital
polymer
electromagnetic energy of photons emmited from electrons at ground state
Group 2A
22. 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
23. A solid made up of particles that are not arranged in a regular pattern.
Group 1A
Conjugate acids and Bases
energy state
amorphous solid
24. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
electron affinity
Ion dipole interactions
Triple point
25. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
Group 5A
Le chateliers Principle
s orbital
26. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Ionization energy
transition elements
Triple point
atomic radius
27. 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.
Nonpolar covalent bond
Group 4A
Redox Half Reaction
electron configuration
28. Numbers that specify the properties of atomic orbitals and of their electrons
Effusion
quantum numbers
Ionic Bond
Formula weight
29. 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
Spin quantum number
Ionic Bond
Equivalence point
bond length
30. A subatomic particle that has a positive charge and that is found in the nucleus of an atom Charge of +1 and mass of 1.0073 amu
Dispersion Forces
Group 5A
Formula weight
Proton
31. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
quantum numbers
Nonpolar covalent bond
Intermolecular forces
Equilibrium
32. 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
Equlibrium constant
subshell
Emperical Formula
Group 1A
33. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
STP
Group 1A
compound
Group 5A
34. Two or more atoms held together by covalent bonds
molecule
Group 1A
physical reaction
subshell
35. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
quantum
Resonance structure
Water dissociation Constant
Group 1A
36. Substance in which a solute is dissolved to form a solution
Formula weight
Dipole Dipole interaction
Conjugate acids and Bases
Solvent
37. An elementary particle with 0 charge and mass about equal to a proton
Solubility Product Constant
Ionization energy
Chemical Kinetics
Neutron
38. 5 valence electrons -3 ions - Nitride N
Group 5A
azimuthal quantum number
Solution equilibrium
Diffusion
39. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
representative elements
mole
pi bonds
Rate determining step
40. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
representative elements
Henry's Law
Group 6A
Molar solubility
41. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
electron configuration
Octet Rule
compound
crystalline solid
42. 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
London forces
Solute
Solubility Product Constant
43. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
sigma bond
Group 7A
Lewis acid base reaction
Molecular orbital
44. 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 Kinetics
Dipole
Dipole Dipole interaction
Resonance structure
45. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
und's rule
Activation energy
Disproportionation
VSEPR
46. (chemistry) p(otential of) H(ydrogen)
pH
amorphous solid
Strong acid
Lyman series
47. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Aqueous Solution
Henderson Hasselbalch Equation
VSEPR
48. Elements in the middle of the periodic table - in groups 3-12.
Group 2A
transition elements
Balmer series
Ground state
49. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Buffer
decomposition reaction
Henry's Law
indicator
50. Temperature is constant; effusion and temperature are proportional to the square root of their masses