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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 reaction in which atoms of one element take the place of atoms of another element in a compound
Electrolyte
Rate law
sigma bond
single displacement reaction
2. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Nucleus
atomic radius
Magnetic quantum number
Triple point
3. 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
Raoult's Law
representative elements
Rate determining step
d orbital
4. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
pi bonds
Hydrogen bonding
Theoretical yield
effective nuclear charge
5. Tells you how much solute is present compared to the amount of solvent
Concentration
azimuthal quantum number
Raoult's Law
Spin quantum number
6. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Planck's Constant
Group 3A
redox reaction
7. The process by which one or more substances change to produce one or more different substances
Intermolecular forces
Equivalence point
Resonance structure
chemical reaction
8. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
amorphous solid
Intermolecular forces
Nonpolar covalent bond
Percent composition
9. A reaction where a compound does Not change its molecular structure.
Disproportionation
amorphous solid
electromagnetic energy of photons emmited from electrons at ground state
physical reaction
10. 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
Intermolecular forces
Acid dissociation constant
lewis base
Reaction order
11. 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
Colligative properties
Buffer
quantum numbers
12. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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13. Small discrete increments of energy.
Network covalent
Activation energy
quanta
amorphous solid
14. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
heisenberg uncertainty principle
Electrolyte
redox reaction
Redox Half Reaction
15. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Diprotic Base
hydrogen bonding
gram equivalent weight
pi bonds
16. (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
Chemical Kinetics
Effusion
Arrhenius Definition
17. The maximum amount of product that can be produced from a given amount of reactant
Triple point
Pauli exclusion principle
theoretical yield
actinide series
18. 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.
Emperical Formula
Activation energy
Dispersion Forces
Group 3A
19. 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
electrolysis
single displacement reaction
hydrogen bonding
20. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Octet Rule
molecule
Effective nuclear charge
21. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
gram equivalent weight
Water dissociation Constant
Chemical Kinetics
22. 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
Effective nuclear charge
Common ion effect
Alkaline earths
azimuthal quantum number
23. 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
Henry's Law
Halogens
gram equivalent weight
Resonance structure
24. 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.
Common ion effect
crystalline solid
Nonpolar covalent bond
Noble gases
25. 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.
Equilibrium
pi bonds
VSEPR
Combination Reaction
26. A horizontal row of elements in the periodic table
Period
physical reaction
Ion
amorphous solid
27. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
Half equivalence point
polymer
quantum
28. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Noble gases
decomposition reaction
Molarity
Bronsted - Lowry definition
29. 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
Lyman series
Percent yield
Group 1A
Ionic Bond
30. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Free radical
Diprotic Base
The bohr model
quantum
31. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Reaction mechanism
lathanide series
Chemical Kinetics
solvation
32. Rare earth element group (elements 58-71)
Ionization energy
empirical formula
Theoretical yield
lathanide series
33. An elementary particle with 0 charge and mass about equal to a proton
Solute
Group 7A
law of constant composition
Neutron
34. 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
amorphous solid
s orbital
VSEPR
35. 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.
electrolysis
periodic trends
bond energy
Balmer series
36. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Free radical
Molality
Aqueous Solution
37. A solution in which water is the solvent
electron configuration
Diprotic Base
Emperical Formula
Aqueous Solution
38. 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
The bohr model
Dispersion Forces
Chemical Kinetics
Conjugate acids and Bases
39. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Phase diagram
Group 7A
Rate determining step
Halogens
40. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
chemical reaction
azimuthal quantum number
Reaction order
atomic emission spectrum
41. Common definition of acids as proton (H+) donors and bases as proton acceptors
Formula weight
Bronsted - Lowry definition
redox reaction
redox reaction
42. The center of the atom which contains the protons and neutrons; in cells - structure that contains the cell's genetic material (DNA) and controls the cell's activities
Buffer
Dipole Dipole interaction
Lewis acid base reaction
Nucleus
43. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
empirical formula
ionic cmpound
pH
Group 4A
44. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Electrolyte
Period
electromagnetic energy of photons emmited from electrons at ground state
Group 1A
45. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Disproportionation
The bohr model
Avagadros number
Theoretical yield
46. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Formula weight
Principle quantum number
Conjugate acids and Bases
Neutralization reaction
47. 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
single displacement reaction
Half equivalence point
Ground state
Titration
48. 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
theoretical yield
Le chateliers Principle
Diprotic Base
Azeotrope
49. Sum of the protons and neutrons in an element often denoted by the letter A
Principle quantum number
Mass number
Free radical
hydrogen bonding
50. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Half equivalence point
Molar solubility
Dipole Dipole interaction
Effusion