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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. A horizontal row of elements in the periodic table
Theoretical yield
periodic trends
Period
Electronegativity
2. The lowest allowable energy state of an atom
subshell
Triple point
Dipole
Ground state
3. 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
Electrolyte
atomic radius
Ionization energy
Effective nuclear charge
4. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Normality
Redox Half Reaction
Group 2A
hydrogen bonding
5. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
energy state
Atomic weight
Octet Rule
6. 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
representative elements
Azeotrope
Le chateliers Principle
Water dissociation Constant
7. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
s orbital
Halogens
Molar solubility
electron affinity
8. E=hc/?
electromagnetic energy of photons emmited from electrons at ground state
Avagadros number
Molecular orbital
Graham's Law
9. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Strong acid
Spin quantum number
Principle quantum number
Network covalent
10. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Diprotic Base
und's rule
Dipole
Normality
11. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Azeotrope
lathanide series
polymer
Chemical Kinetics
12. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
gram equivalent weight
Le chateliers Principle
Resonance structure
Ion
13. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Solution equilibrium
Pauli exclusion principle
Reaction order
Electronegativity
14. Slightly less reactive than alkali metals - comprise group II
Rydberg constant
redox reaction
Group 2A
Alkaline earths
15. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Equlibrium constant
Hydrogen bonding
Ion
Intermolecular forces
16. A definite stable energy that a physical system can have
effective nuclear charge
energy state
Pauli exclusion principle
mole
17. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Neutralization reaction
Solute
Molality
18. In a solution - the substance that dissolves in the solvent
Nucleus
s orbital
Solvent
Solute
19. 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
heisenberg uncertainty principle
Equlibrium constant
Molar solubility
Ground state
20. An ionic compound that resists changes in its pH
amorphous solid
Henry's Law
Buffer
Net ionic equation
21. Named after their cation and anion
Group 5A
Lyman series
Equivalence point
ionic cmpound
22. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Disproportionation
quantum numbers
Diffusion
23. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Ionic Bond
Azeotrope
molecule
24. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
atomic radius
Net ionic equation
Molar solubility
mole
25. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Phase diagram
Collision theory of chemical Kinetics
electron configuration
Network covalent
26. (chemistry) p(otential of) H(ydrogen)
compound
Percent yield
pH
Reaction order
27. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Magnetic quantum number
Network covalent
Titration
28. 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
Ion product
Hydrogen bonding
Group 2A
29. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Resonance structure
Group 4A
single displacement reaction
Network covalent
30. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Equilibrium
physical reaction
Formula weight
Group 5A
31. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
atomic radius
Ion dipole interactions
Neutralization reaction
mole
32. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Intermolecular forces
Free radical
Redox Half Reaction
azimuthal quantum number
33. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Emperical Formula
Bronsted - Lowry definition
Phase diagram
amorphous solid
34. A dynamic condition in which two opposing changes occur at equal rates in a closed system
und's rule
Equilibrium
physical reaction
energy state
35. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Rydberg constant
Activation energy
atomic emission spectrum
Amphoteric
36. A solid made up of particles that are not arranged in a regular pattern.
heisenberg uncertainty principle
Titration
Dipole
amorphous solid
37. 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
38. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
Group 6A
Bronsted - Lowry definition
indicator
39. 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.
VSEPR
Group 6A
quanta
heisenberg uncertainty principle
40. (chemistry) a substance that changes color to indicate the presence of some ion or substance
law of constant composition
Chemical Kinetics
atomic theory
indicator
41. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Equlibrium constant
redox reaction
Ion
energy state
42. 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.
Avagadros number
Nucleus
Principle quantum number
Diprotic Base
43. 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.
Ion
Group 3A
The bohr model
electrolysis
44. Small discrete increments of energy.
Lyman series
The bohr model
Nucleus
quanta
45. A solution in which water is the solvent
polymer
crystalline solid
Aqueous Solution
Amphoteric
46. 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
Strong acid
percent composition
Colligative properties
Amphoteric
47. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
48. The Percent by mass of each element in a compound.
Colligative properties
Percent composition
Dispersion Forces
Octet Rule
49. 5 valence electrons -3 ions - Nitride N
Colligative properties
Lewis definition
Lyman series
Group 5A
50. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
Triple point
Phase diagram
transition elements