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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 subdivision of an energy level in an atom. They are divided into orbitals.
pH
Noble gases
subshell
Lewis structure
2. An atom or group of atoms that has a positive or negative charge
Solute
Aqueous Solution
Ion
Covalent Bond
3. 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
Molecular orbital
electron affinity
Group 5A
Acid dissociation constant
4. The process by which one or more substances change to produce one or more different substances
Combination Reaction
Equivalence point
Magnetic quantum number
chemical reaction
5. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
Electronegativity
Free radical
chemical reaction
6. 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
Nucleus
Covalent Bond
Formal Charge
Reaction order
7. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Group 5A
heisenberg uncertainty principle
Activation energy
Octet Rule
8. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Effective nuclear charge
Solute
Atomic weight
Nonpolar covalent bond
9. Any sample of a given compound will contain the same elements in the identical mass ratio.
redox reaction
law of constant composition
Group 2A
Group 6A
10. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
s orbital
quantum
Colligative properties
STP
11. 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
Dispersion Forces
Group 7A
Intermolecular forces
quantum
12. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
indicator
Period
Neutralization reaction
13. 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 emission spectrum
Balmer series
Molecular orbital
mole
14. Common definition of acids as proton (H+) donors and bases as proton acceptors
polymer
Half equivalence point
Bronsted - Lowry definition
Molarity
15. The solubility of a gas in a liquid is directly proportional to the partial pressure of that gas on the surface of the liquid
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16. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Graham's Law
Equilibrium
Diprotic Base
energy state
17. Have the shape of a sphere - with the center of the sphere at the nucleus; completely symmetrical along all axes; 1s orbital is spherically symmetric and has no nodes; 2s orbital is also spherical but contains a node and is higher in energy
Mass number
Equlibrium constant
Activation energy
s orbital
18. Small discrete increments of energy.
quanta
representative elements
Atomic weight
heisenberg uncertainty principle
19. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Vapor pressure
Solution equilibrium
Bronsted - Lowry definition
Free radical
20. Rare earth element group (elements 58-71)
quanta
Group 2A
lathanide series
Rate determining step
21. 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
Disproportionation
Rydberg constant
azimuthal quantum number
VSEPR
22. 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
d orbital
Graham's Law
Equlibrium constant
Disproportionation
23. 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.
Decomposition reaction
Neutralization reaction
und's rule
Principle quantum number
24. Acids defined as electron - pair acceptors and bases as electron - pair donors.
atomic emission spectrum
Lewis definition
Common ion effect
Chemical Kinetics
25. Having characteristics of both an acid and a base and capable of reacting as either
Acid dissociation constant
atomic radius
Amphoteric
Balmer series
26. E=hc/?
Amphoteric
Ion product
electromagnetic energy of photons emmited from electrons at ground state
subshell
27. 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.
atomic radius
Conjugate acids and Bases
Planck's Constant
Effective nuclear charge
28. Two or more atoms held together by covalent bonds
Equivalence point
Henry's Law
chemical reaction
molecule
29. 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
Common ion effect
subshell
Neutron
30. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Neutralization reaction
Normality
Ion dipole interactions
s orbital
31. Numbers that specify the properties of atomic orbitals and of their electrons
quantum numbers
Rate law
Effective nuclear charge
Colligative properties
32. A reaction in which atoms of one element take the place of atoms of another element in a compound
Mass number
Molality
Solubility Product Constant
single displacement reaction
33. A horizontal row of elements in the periodic table
lathanide series
Ion
atomic theory
Period
34. A definite stable energy that a physical system can have
Group 4A
Halogens
Group 1A
energy state
35. 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
actinide series
Colligative properties
Normality
electromagnetic energy of photons emmited from electrons at ground state
36. 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.
Chemical Kinetics
crystalline solid
quanta
d orbital
37. Sum of the protons and neutrons in an element often denoted by the letter A
und's rule
Mass number
Resonance structure
Atomic weight
38. 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
Effusion
Formal Charge
Solubility Product Constant
Proton
39. An ionic compound that resists changes in its pH
Colligative properties
Buffer
Disproportionation
Dispersion Forces
40. Specifies the specific orbital in which the electron is most likely to be found. - Third quantum number - designated as ml. Describes a particular orbital within a subshell where an electron is very likely to be found. Possible values are integers in
The bohr model
Solubility Product Constant
Phase diagram
Magnetic quantum number
41. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
representative elements
Arrhenius Definition
Conjugate acids and Bases
Theoretical yield
42. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Vapor pressure
Electrolyte
Chemical Kinetics
Lewis definition
43. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Lyman series
Principle quantum number
Le chateliers Principle
Molality
44. 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
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45. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
Group 2A
azimuthal quantum number
Ion
Chemical Kinetics
46. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Solubility Product Constant
Network covalent
subshell
molecular weight
47. The process of decomposing a chemical compound by the passage of an electric current.
s orbital
electrolysis
Reaction mechanism
Network covalent
48. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole Dipole interaction
Lewis structure
atomic radius
Combination Reaction
49. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Lewis acid base reaction
chemical reaction
single displacement reaction
heisenberg uncertainty principle
50. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Phase diagram
Electrolyte
theoretical yield
Amphoteric