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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 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
VSEPR
Equilibrium
atomic radius
2. Simplest whole # ration of atoms in a compound
subshell
Equivalence point
Emperical Formula
atomic emission spectrum
3. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
periodic trends
Group 3A
Lyman series
Percent yield
4. An atom or group of atoms that has a positive or negative charge
percent composition
und's rule
Ion
periodic trends
5. A definite stable energy that a physical system can have
energy state
bond length
crystalline solid
electron configuration
6. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
theoretical yield
solvation
Common ion effect
Henry's Law
7. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
azimuthal quantum number
Diffusion
Rate law
Group 1A
8. Any sample of a given compound will contain the same elements in the identical mass ratio.
Net ionic equation
law of constant composition
compound
Formula weight
9. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
bond length
Strong acid
Atomic weight
percent composition
10. 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.
Network covalent
electromagnetic energy of photons emmited from electrons at ground state
Effective nuclear charge
d orbital
11. A reaction where a compound does Not change its molecular structure.
Lyman series
energy state
physical reaction
empirical formula
12. Numbers that specify the properties of atomic orbitals and of their electrons
Equivalence point
Titration
Balmer series
quantum numbers
13. 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
atomic radius
decomposition reaction
Effective nuclear charge
Resonance structure
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
representative elements
Colligative properties
Balmer series
Decomposition reaction
15. 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
Group 7A
Mass number
Neutralization reaction
Group 2A
16. Gram equivalent weight of solute per liter of solution - often denoted by N.
Vapor pressure
Graham's Law
pI
Normality
17. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Neutron
Neutralization reaction
Dipole Dipole interaction
STP
18. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Ion dipole interactions
theoretical yield
subshell
Halogens
19. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
d orbital
Nonpolar covalent bond
atomic theory
Disproportionation
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
Arrhenius Definition
s orbital
hydrogen bonding
Amphoteric
21. Tells you how much solute is present compared to the amount of solvent
Effective nuclear charge
d orbital
Concentration
Rate determining step
22. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Azeotrope
Group 1A
Group 2A
periodic trends
23. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Effusion
Planck's Constant
Phase diagram
Dipole
24. 5 different orbitals shaped like clover leaves and max electrons is 10
The bohr model
Group 3A
d orbital
physical reaction
25. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Rate determining step
Molecular orbital
electromagnetic energy of photons emmited from electrons at ground state
26. Substance in which a solute is dissolved to form a solution
Solvent
Le chateliers Principle
Spin quantum number
Emperical Formula
27. 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.
Rate determining step
Balmer series
Half equivalence point
Covalent Bond
28. (chemistry) p(otential of) H(ydrogen)
Buffer
Atomic weight
pi bonds
pH
29. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Solution equilibrium
Rate determining step
quanta
30. The energy required to break a chemical bond and form neutral isolated atoms
Titration
Nonpolar covalent bond
bond energy
ionic cmpound
31. 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
Azeotrope
Dispersion Forces
Lyman series
Ionization energy
32. 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
hydrogen bonding
Halogens
Water dissociation Constant
Group 5A
33. 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
azimuthal quantum number
Magnetic quantum number
Nucleus
Common ion effect
34. The maximum amount of product that can be produced from a given amount of reactant
Combination Reaction
theoretical yield
Halogens
Diffusion
35. An elementary particle with 0 charge and mass about equal to a proton
Equivalence point
Ionic Bond
Neutron
physical reaction
36. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Proton
electron affinity
Mass number
quantum
37. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted - Lowry definition
quantum numbers
Solvent
percent composition
38. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Rate law
Ion product
Network covalent
Lewis definition
39. Having characteristics of both an acid and a base and capable of reacting as either
Amphoteric
Planck's Constant
Henderson Hasselbalch Equation
solvation
40. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Ion product
Effusion
electron configuration
pH
41. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Combination Reaction
mole
atomic emission spectrum
Effusion
42. The Percent by mass of each element in a compound.
theoretical yield
Percent composition
London forces
single displacement reaction
43. A reaction in which atoms of one element take the place of atoms of another element in a compound
atomic radius
single displacement reaction
Solvent
atomic theory
44. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Net ionic equation
Halogens
Electrolyte
Bronsted Lowry
45. 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 radius
Octet Rule
atomic emission spectrum
Lyman series
46. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
decomposition reaction
pi bonds
polymer
Bronsted Lowry
47. The lowest allowable energy state of an atom
Proton
Group 4A
Ground state
Alkaline earths
48. 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
representative elements
Arrhenius Definition
Intermolecular forces
Solute
49. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Lewis acid base reaction
atomic radius
Graham's Law
Nucleus
50. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
Ion product
molecular weight
STP
Ionic Bond