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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. 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
Group 3A
Arrhenius Definition
subshell
Planck's Constant
2. The percent by mass of each element in a compound
compound
molecule
molecular weight
percent composition
3. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
redox reaction
Activation energy
electron affinity
Equivalence point
4. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
sigma bond
electromagnetic energy of photons emmited from electrons at ground state
law of constant composition
Emperical Formula
5. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
subshell
molecular weight
Group 4A
Group 2A
6. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Theoretical yield
Reaction mechanism
compound
atomic emission spectrum
7. Numbers that specify the properties of atomic orbitals and of their electrons
STP
Alkaline earths
Electronegativity
quantum numbers
8. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
electron configuration
Chemical Kinetics
Lyman series
9. The lowest allowable energy state of an atom
Hydrogen bonding
Nonpolar covalent bond
Electrolyte
Ground state
10. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Disproportionation
chemical reaction
Graham's Law
Nonpolar covalent bond
11. The Percent by mass of each element in a compound.
Amphoteric
Solvent
Dipole Dipole interaction
Percent composition
12. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
d orbital
Common ion effect
Group 6A
pi bonds
13. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Graham's Law
Solvent
Solution equilibrium
Covalent Bond
14. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Mass number
Ion
heisenberg uncertainty principle
polymer
15. A substance that - when dissolved in water - results in a solution that can conduct electricity
Electrolyte
Phase diagram
Aqueous Solution
empirical formula
16. Rare earth element group (elements 58-71)
Percent composition
Chemical Kinetics
Atomic absorption Spectra
lathanide series
17. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Rydberg constant
representative elements
Percent composition
18. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
atomic radius
quantum
Effusion
Rydberg constant
19. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
hydrogen bonding
atomic emission spectrum
angular momentum in the bohr model
Acid dissociation constant
20. 5 valence electrons -3 ions - Nitride N
Group 6A
Group 5A
STP
Phase diagram
21. 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
Lewis structure
Hydrogen bonding
pH
Group 7A
22. Simplest whole # ration of atoms in a compound
Noble gases
Emperical Formula
Free radical
Disproportionation
23. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
energy state
London forces
Percent yield
atomic radius
24. 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.
Balmer series
subshell
Dipole Dipole interaction
representative elements
25. 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
Ionization energy
Theoretical yield
crystalline solid
26. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Decomposition reaction
transition elements
Le chateliers Principle
Concentration
27. Common definition of acids as proton (H+) donors and bases as proton acceptors
London forces
Bronsted - Lowry definition
electron affinity
pi bonds
28. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
periodic trends
Aqueous Solution
Triple point
Avagadros number
29. The process by which one or more substances change to produce one or more different substances
Acid dissociation constant
chemical reaction
Half equivalence point
Formula weight
30. 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
Redox Half Reaction
angular momentum in the bohr model
electrolysis
Spin quantum number
31. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
Octet Rule
Strong acid
The bohr model
Group 5A
32. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Amphoteric
Ground state
Theoretical yield
Mass number
33. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Concentration
lewis base
Covalent Bond
Equlibrium constant
34. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
Arrhenius Definition
Henderson Hasselbalch Equation
Period
35. A reaction where a compound does Not change its molecular structure.
physical reaction
single displacement reaction
Redox Half Reaction
sigma bond
36. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Solubility Product Constant
Activation energy
effective nuclear charge
37. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Le chateliers Principle
Group 4A
Combination Reaction
actinide series
38. A reaction in which atoms of one element take the place of atoms of another element in a compound
Bronsted - Lowry definition
Molecular orbital
Effective nuclear charge
single displacement reaction
39. Substance in which a solute is dissolved to form a solution
Le chateliers Principle
s orbital
Solvent
electromagnetic energy of photons emmited from electrons at ground state
40. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
electron affinity
Strong acid
Group 7A
Conjugate acids and Bases
41. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Electrolyte
Ion product
percent composition
42. 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.
Avagadros number
Hydrogen bonding
Solution equilibrium
atomic radius
43. Named after their cation and anion
Group 1A
Molar solubility
amorphous solid
ionic cmpound
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
Neutralization reaction
energy state
Group 5A
Resonance structure
45. 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 2A
Group 3A
Solubility Product Constant
Arrhenius Definition
46. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Ionization energy
Rydberg constant
Normality
Dipole Dipole interaction
47. 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
Octet Rule
Equlibrium constant
electron configuration
48. 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 1A
Strong acid
Ionic Bond
49. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
electrolysis
Avagadros number
Period
Dipole
50. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
indicator
Neutralization reaction
Pauli exclusion principle
Net ionic equation