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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. The process of decomposing a chemical compound by the passage of an electric current.
atomic emission spectrum
Group 4A
electrolysis
Electrolyte
2. 5 different orbitals shaped like clover leaves and max electrons is 10
quanta
Molality
d orbital
Percent yield
3. Energy released when an atom or ion in the gaseous state gains an electron. Increases from left to right and from bottom to top on the Periodic Table.
decomposition reaction
VSEPR
electron affinity
Reaction order
4. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Group 1A
Group 4A
Rate law
periodic trends
5. 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
Group 2A
Ionic Bond
theoretical yield
Solution equilibrium
6. The percent by mass of each element in a compound
Nonpolar covalent bond
percent composition
theoretical yield
Phase diagram
7. The Percent by mass of each element in a compound.
Percent composition
Concentration
single displacement reaction
empirical formula
8. Two or more atoms held together by covalent bonds
Bronsted - Lowry definition
amorphous solid
Solute
molecule
9. Small discrete increments of energy.
Group 5A
energy state
actinide series
quanta
10. A solution in which water is the solvent
Pauli exclusion principle
Solubility Product Constant
mole
Aqueous Solution
11. 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
Acid dissociation constant
electrolysis
s orbital
Azeotrope
12. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Lewis acid base reaction
angular momentum in the bohr model
Hydrogen bonding
d orbital
13. Attractions between molecules caused by the electron motion on one molecule affecting the electron motion on the other through electrical forces; these are the weakest interactions between molecules
Graham's Law
Free radical
Neutralization reaction
Dispersion Forces
14. 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
Ionization energy
Colligative properties
Chemical Kinetics
Group 4A
15. Simplest whole # ration of atoms in a compound
Ion product
Colligative properties
Formal Charge
Emperical Formula
16. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Combination Reaction
Activation energy
Effusion
Free radical
17. Having characteristics of both an acid and a base and capable of reacting as either
Diprotic Base
Amphoteric
decomposition reaction
Graham's Law
18. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Normality
empirical formula
Alkaline earths
Bronsted Lowry
19. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Diffusion
Dispersion Forces
atomic radius
Solubility Product Constant
20. 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
Bronsted - Lowry definition
Percent composition
Arrhenius Definition
Halogens
21. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Rydberg constant
actinide series
Effective nuclear charge
Resonance structure
22. 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
actinide series
Proton
Colligative properties
sigma bond
23. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Effusion
Intermolecular forces
Buffer
Half equivalence point
24. A reaction in which atoms of one element take the place of atoms of another element in a compound
Group 4A
Ion product
single displacement reaction
decomposition reaction
25. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Ion
physical reaction
Reaction order
26. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
quanta
single displacement reaction
bond length
Water dissociation Constant
27. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
molecular weight
s orbital
Ion
28. The maximum amount of product that can be produced from a given amount of reactant
Molarity
Effusion
theoretical yield
STP
29. 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
atomic theory
Group 7A
pi bonds
representative elements
30. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
compound
Group 6A
percent composition
31. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Half equivalence point
Concentration
Titration
Phase diagram
32. 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
mole
Spin quantum number
Raoult's Law
Colligative properties
33. 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
d orbital
Hydrogen bonding
azimuthal quantum number
Common ion effect
34. 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
s orbital
Solvent
Graham's Law
The bohr model
35. 5 valence electrons -3 ions - Nitride N
Neutron
Bronsted Lowry
law of constant composition
Group 5A
36. Sum of the protons and neutrons in an element often denoted by the letter A
Arrhenius Definition
The bohr model
Mass number
Percent yield
37. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Graham's Law
Hydrogen bonding
Halogens
Avagadros number
38. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
Solute
Le chateliers Principle
bond energy
39. A horizontal row of elements in the periodic table
Equilibrium
law of constant composition
Period
Azeotrope
40. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Conjugate acids and Bases
Covalent Bond
Reaction order
Electronegativity
41. A measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
quantum
Lewis structure
Titration
quanta
42. 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
Solute
Octet Rule
amorphous solid
43. Redox reaction - in which the same species is both oxidized and reduced.
Disproportionation
Half equivalence point
pi bonds
atomic radius
44. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
heisenberg uncertainty principle
quantum
Azeotrope
bond energy
45. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
quantum
molecular weight
representative elements
46. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Neutron
bond energy
Triple point
Free radical
47. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Half equivalence point
Rydberg constant
Solubility Product Constant
effective nuclear charge
48. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Equlibrium constant
molecular weight
Equilibrium
Percent yield
49. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
STP
pH
electron configuration
quantum
50. Substance in which a solute is dissolved to form a solution
Solvent
Noble gases
percent composition
Pauli exclusion principle