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. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
electron affinity
Collision theory of chemical Kinetics
Pauli exclusion principle
Mass number
2. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Arrhenius Definition
Planck's Constant
Neutron
Ion dipole interactions
3. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Alkaline earths
atomic radius
decomposition reaction
4. A set of spectral lines that appear in the visible light region when a hydrogen atom undergoes a transition from energy levels n>2 to n=2.
transition elements
Balmer series
Halogens
Azeotrope
5. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
Colligative properties
Molarity
Ground state
6. A reaction where a compound does Not change its molecular structure.
Group 2A
physical reaction
Balmer series
Charles and Gay Lussac's Law
7. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
Warning
: Invalid argument supplied for foreach() in
/var/www/html/basicversity.com/show_quiz.php
on line
183
8. 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.
Effective nuclear charge
single displacement reaction
Nonpolar covalent bond
Lewis structure
9. Having characteristics of both an acid and a base and capable of reacting as either
Rate determining step
Bronsted Lowry
azimuthal quantum number
Amphoteric
10. Any sample of a given compound will contain the same elements in the identical mass ratio.
Net ionic equation
theoretical yield
lathanide series
law of constant composition
11. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Solubility Product Constant
Dipole Dipole interaction
Dipole
empirical formula
12. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
Diprotic Base
London forces
Atomic weight
13. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Titration
Le chateliers Principle
Percent composition
Electronegativity
14. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Balmer series
Octet Rule
gram equivalent weight
crystalline solid
15. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
chemical reaction
sigma bond
effective nuclear charge
Rate determining step
16. In a solution - the substance that dissolves in the solvent
Azeotrope
Ion dipole interactions
Solute
Period
17. The percent by mass of each element in a compound
lathanide series
percent composition
Electronegativity
bond energy
18. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Group 3A
Pauli exclusion principle
Henry's Law
Triple point
19. 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.
Redox Half Reaction
Theoretical yield
Rydberg constant
quantum
20. 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
Ionic Bond
Normality
Solvent
Lewis acid base reaction
21. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
sigma bond
pi bonds
Effective nuclear charge
redox reaction
22. Rare earth element group (elements 58-71)
Balmer series
Solubility Product Constant
ionic cmpound
lathanide series
23. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
atomic emission spectrum
Collision theory of chemical Kinetics
quanta
London forces
24. 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
Ion product
actinide series
gram equivalent weight
Solution equilibrium
25. 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
Dispersion Forces
Buffer
Dipole Dipole interaction
Formal Charge
26. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
molecular weight
Network covalent
percent composition
Strong acid
27. Common definition of acids as proton (H+) donors and bases as proton acceptors
representative elements
Henderson Hasselbalch Equation
atomic emission spectrum
Bronsted - Lowry definition
28. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
solvation
Covalent Bond
STP
Noble gases
29. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
periodic trends
solvation
Reaction order
Balmer series
30. An atom or group of atoms that has a positive or negative charge
bond length
Ion
Neutron
Common ion effect
31. 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.
atomic emission spectrum
Lewis structure
Spin quantum number
Atomic absorption Spectra
32. The Percent by mass of each element in a compound.
heisenberg uncertainty principle
Reaction mechanism
Percent composition
Molality
33. The energy required to break a chemical bond and form neutral isolated atoms
bond energy
Combination Reaction
subshell
Diffusion
34. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Amphoteric
Rate law
Group 1A
35. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
electrolysis
Balmer series
Dispersion Forces
36. 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
Spin quantum number
Solute
theoretical yield
representative elements
37. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Theoretical yield
STP
Network covalent
38. The average distance between the nuclei of two bonded atoms
bond length
quantum
Lewis acid base reaction
percent composition
39. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
quantum
Neutralization reaction
energy state
solvation
40. 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
quantum numbers
Free radical
subshell
Proton
41. 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
single displacement reaction
Nucleus
azimuthal quantum number
Group 5A
42. Chalcogens - - Oxide O
Group 6A
polymer
d orbital
single displacement reaction
43. An ionic compound that resists changes in its pH
Ion
Equlibrium constant
Ion
Buffer
44. 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
45. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Proton
decomposition reaction
Formal Charge
46. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
theoretical yield
Halogens
Pauli exclusion principle
quantum
47. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
pi bonds
redox reaction
Phase diagram
empirical formula
48. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
ionic cmpound
Molarity
Ion
electron configuration
49. A reaction in which atoms of one element take the place of atoms of another element in a compound
Raoult's Law
Group 7A
Planck's Constant
single displacement reaction
50. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Graham's Law
Buffer
Azeotrope
Group 2A