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. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
redox reaction
VSEPR
Atomic weight
Half equivalence point
2. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Amphoteric
Group 5A
Reaction mechanism
Avagadros number
3. Rare earth element group (elements 58-71)
Equivalence point
Ionization energy
Ion
lathanide series
4. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Phase diagram
Halogens
Neutralization reaction
Le chateliers Principle
5. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Half equivalence point
d orbital
Collision theory of chemical Kinetics
molecular weight
6. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Colligative properties
Conjugate acids and Bases
Raoult's Law
energy state
7. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Rate determining step
Graham's Law
Decomposition reaction
Hydrogen bonding
8. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
crystalline solid
und's rule
Molecular orbital
STP
9. 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
Molecular orbital
Mass number
Half equivalence point
10. In a solution - the substance that dissolves in the solvent
gram equivalent weight
hydrogen bonding
atomic radius
Solute
11. Property of the elements that can be predicted from the arrangement of the periodic table
polymer
Reaction order
periodic trends
atomic emission spectrum
12. (chemistry) p(otential of) H(ydrogen)
Arrhenius Definition
Diprotic Base
pH
heisenberg uncertainty principle
13. 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
indicator
Molar solubility
Common ion effect
Ionic Bond
14. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
Collision theory of chemical Kinetics
Conjugate acids and Bases
Ionization energy
15. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Arrhenius Definition
Phase diagram
Concentration
Octet Rule
16. The process of decomposing a chemical compound by the passage of an electric current.
Dipole Dipole interaction
Mass number
Acid dissociation constant
electrolysis
17. An ionic compound that resists changes in its pH
Buffer
atomic emission spectrum
decomposition reaction
Electrolyte
18. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
transition elements
Emperical Formula
molecular weight
19. 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
Azeotrope
Rate determining step
Covalent Bond
20. 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
Diprotic Base
gram equivalent weight
Solution equilibrium
atomic radius
21. The percent by mass of each element in a compound
Nucleus
Theoretical yield
Avagadros number
percent composition
22. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Group 6A
law of constant composition
solvation
Raoult's Law
23. An elementary particle with 0 charge and mass about equal to a proton
s orbital
und's rule
Neutron
Molality
24. A reaction in which atoms of one element take the place of atoms of another element in a compound
Group 6A
single displacement reaction
Combination Reaction
Spin quantum number
25. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
electromagnetic energy of photons emmited from electrons at ground state
Noble gases
Theoretical yield
Diffusion
26. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
angular momentum in the bohr model
Lyman series
indicator
effective nuclear charge
27. 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.
crystalline solid
lathanide series
Reaction order
Le chateliers Principle
28. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
Rate law
hydrogen bonding
Strong acid
29. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Group 1A
quantum
Dipole
gram equivalent weight
30. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
percent composition
Le chateliers Principle
The bohr model
Normality
31. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Equilibrium
Bronsted - Lowry definition
Phase diagram
Molality
32. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Effusion
electron configuration
electron affinity
Ionic Bond
33. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
electron configuration
Ionization energy
electron affinity
Lewis acid base reaction
34. Substance in which a solute is dissolved to form a solution
Ion dipole interactions
Solvent
Decomposition reaction
Rate determining step
35. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Raoult's Law
und's rule
Bronsted - Lowry definition
mole
36. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
bond length
Group 7A
Triple point
Atomic absorption Spectra
37. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Nonpolar covalent bond
Formula weight
Amphoteric
Effective nuclear charge
38. 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
STP
VSEPR
s orbital
azimuthal quantum number
39. 2.18 x 10^-18 J/electron
heisenberg uncertainty principle
Rydberg constant
lathanide series
Dispersion Forces
40. Chalcogens - - Oxide O
Planck's Constant
Percent composition
Group 6A
Phase diagram
41. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Group 2A
Balmer series
Group 4A
Molality
42. 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
Ion product
Azeotrope
Atomic weight
Lewis acid base reaction
43. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
bond length
Group 7A
Henderson Hasselbalch Equation
Spin quantum number
44. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole Dipole interaction
Aqueous Solution
Activation energy
Titration
45. 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
Charles and Gay Lussac's Law
mole
representative elements
energy state
46. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
und's rule
Collision theory of chemical Kinetics
atomic radius
47. Slightly less reactive than alkali metals - comprise group II
Equilibrium
Dipole
Alkaline earths
Molality
48. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion
Formula weight
molecule
Dipole Dipole interaction
49. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
chemical reaction
Ionization energy
molecular weight
50. 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
Graham's Law
Equlibrium constant
Avagadros number
angular momentum in the bohr model