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. 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
Colligative properties
Group 7A
mole
2. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
Balmer series
Ion
Planck's Constant
Equivalence point
3. 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
Atomic weight
Percent yield
Colligative properties
s orbital
4. A reaction in which atoms of one element take the place of atoms of another element in a compound
Principle quantum number
Octet Rule
single displacement reaction
Molecular orbital
5. 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
Le chateliers Principle
Activation energy
hydrogen bonding
Ionization energy
6. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Percent composition
Amphoteric
Charles and Gay Lussac's Law
7. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Net ionic equation
STP
Nucleus
Pauli exclusion principle
8. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Percent composition
molecular weight
bond length
Colligative properties
9. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
atomic emission spectrum
Solution equilibrium
Solute
10. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Rate law
Intermolecular forces
Group 3A
Bronsted Lowry
11. 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
Group 7A
Avagadros number
Molecular orbital
angular momentum in the bohr model
12. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Spin quantum number
bond energy
Rate determining step
Effusion
13. 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
amorphous solid
Arrhenius Definition
Resonance structure
Group 6A
14. 5 valence electrons -3 ions - Nitride N
Group 5A
Molality
quantum
und's rule
15. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molecular orbital
gram equivalent weight
London forces
s orbital
16. Temperature is constant; effusion and temperature are proportional to the square root of their masses
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
17. 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
Collision theory of chemical Kinetics
Emperical Formula
Resonance structure
Noble gases
18. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Half equivalence point
atomic radius
Ionic Bond
Octet Rule
19. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Electrolyte
Avagadros number
solvation
quantum numbers
20. The Percent by mass of each element in a compound.
Electrolyte
Rate determining step
Percent composition
Formal Charge
21. 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
22. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Redox Half Reaction
Nonpolar covalent bond
s orbital
23. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Halogens
electron affinity
subshell
24. Slightly less reactive than alkali metals - comprise group II
Lewis structure
Dispersion Forces
Alkaline earths
Rate determining step
25. 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
Hydrogen bonding
quantum
Acid dissociation constant
26. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
solvation
energy state
Vapor pressure
27. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Ion
Dispersion Forces
Chemical Kinetics
Ionic Bond
28. 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.
law of constant composition
atomic radius
Concentration
bond length
29. A base that can accept two moles of H+ per mole of itself (ex: SO4
molecule
Diprotic Base
Ion
periodic trends
30. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Conjugate acids and Bases
sigma bond
VSEPR
Octet Rule
31. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Chemical Kinetics
Rate determining step
Nonpolar covalent bond
Bronsted Lowry
32. E=hc/?
Ionic Bond
electromagnetic energy of photons emmited from electrons at ground state
pi bonds
quantum numbers
33. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Aqueous Solution
Covalent Bond
Ground state
gram equivalent weight
34. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
lewis base
Diprotic Base
redox reaction
Halogens
35. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Effusion
Common ion effect
effective nuclear charge
Charles and Gay Lussac's Law
36. The process of decomposing a chemical compound by the passage of an electric current.
Nonpolar covalent bond
Vapor pressure
electrolysis
Titration
37. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Equilibrium
electron configuration
Vapor pressure
Rydberg constant
38. 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
Hydrogen bonding
Ion
Redox Half Reaction
representative elements
39. A reaction in which atoms of one element take the place of atoms of another element in a compound
Disproportionation
Diffusion
single displacement reaction
indicator
40. 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
representative elements
atomic theory
Redox Half Reaction
41. Rare earth element group (elements 58-71)
Phase diagram
energy state
Molarity
lathanide series
42. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Period
Group 6A
Spin quantum number
Net ionic equation
43. 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
Ion
s orbital
Network covalent
Concentration
44. A reaction where a compound does Not change its molecular structure.
physical reaction
pH
Halogens
percent composition
45. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
crystalline solid
decomposition reaction
Collision theory of chemical Kinetics
46. 5 different orbitals shaped like clover leaves and max electrons is 10
Group 4A
d orbital
Raoult's Law
Common ion effect
47. Simplest whole # ration of atoms in a compound
effective nuclear charge
law of constant composition
Emperical Formula
Ion dipole interactions
48. A subdivision of an energy level in an atom. They are divided into orbitals.
Group 4A
Solution equilibrium
subshell
The bohr model
49. Elements in the middle of the periodic table - in groups 3-12.
electron configuration
bond length
lewis base
transition elements
50. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Triple point
redox reaction
Conjugate acids and Bases
physical reaction