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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
STP
single displacement reaction
Network covalent
pI
2. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Percent yield
amorphous solid
Normality
3. The lowest allowable energy state of an atom
Equivalence point
Mass number
Ground state
Pauli exclusion principle
4. The ratio of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction
London forces
Ground state
Neutron
Percent yield
5. 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
Equlibrium constant
molecule
Combination Reaction
Disproportionation
6. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Magnetic quantum number
compound
Halogens
Proton
7. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Avagadros number
percent composition
Conjugate acids and Bases
Intermolecular forces
8. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Spin quantum number
Aqueous Solution
Common ion effect
9. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Ion dipole interactions
Activation energy
Combination Reaction
Titration
10. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Arrhenius Definition
pI
Diffusion
Concentration
11. 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
Principle quantum number
redox reaction
Spin quantum number
Molecular orbital
12. 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
single displacement reaction
Diffusion
Magnetic quantum number
STP
13. 5 valence electrons -3 ions - Nitride N
amorphous solid
Rate law
Lyman series
Group 5A
14. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Normality
Acid dissociation constant
Phase diagram
Vapor pressure
15. 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
Solute
Resonance structure
VSEPR
Dipole Dipole interaction
16. 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
Ion dipole interactions
azimuthal quantum number
Nucleus
Phase diagram
17. 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
Lewis structure
Magnetic quantum number
hydrogen bonding
Ionic Bond
18. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Lewis acid base reaction
Group 6A
electron configuration
Ion dipole interactions
19. 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
Network covalent
Lyman series
Strong acid
20. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molar solubility
Percent yield
Molecular orbital
subshell
21. 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.
Pauli exclusion principle
Water dissociation Constant
Balmer series
Network covalent
22. (chemistry) p(otential of) H(ydrogen)
pH
mole
ionic cmpound
Chemical Kinetics
23. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Network covalent
Ion dipole interactions
Noble gases
Acid dissociation constant
24. 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.
Principle quantum number
Covalent Bond
Atomic absorption Spectra
azimuthal quantum number
25. Product of the molar concentrations of dissociated ions in solution at saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted Ksp.
subshell
Decomposition reaction
Solubility Product Constant
Half equivalence point
26. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
Mass number
Reaction mechanism
atomic theory
Strong acid
27. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Atomic absorption Spectra
Hydrogen bonding
Lyman series
molecular weight
28. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Equlibrium constant
Redox Half Reaction
Lewis structure
atomic emission spectrum
29. 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
Vapor pressure
electron configuration
lewis base
London forces
30. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
quantum numbers
Graham's Law
Le chateliers Principle
31. 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
chemical reaction
Group 5A
Half equivalence point
32. 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.
s orbital
Effective nuclear charge
Graham's Law
electron affinity
33. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Intermolecular forces
Net ionic equation
heisenberg uncertainty principle
Normality
34. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
sigma bond
STP
gram equivalent weight
Pauli exclusion principle
35. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
molecular weight
Proton
pi bonds
effective nuclear charge
36. The percent by mass of each element in a compound
quanta
gram equivalent weight
percent composition
effective nuclear charge
37. Acids defined as electron - pair acceptors and bases as electron - pair donors.
single displacement reaction
Lewis definition
Percent composition
Group 1A
38. 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
Phase diagram
Combination Reaction
redox reaction
Colligative properties
39. Substance in which a solute is dissolved to form a solution
Octet Rule
electromagnetic energy of photons emmited from electrons at ground state
quantum
Solvent
40. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Reaction mechanism
Theoretical yield
actinide series
41. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Ground state
indicator
Disproportionation
quantum numbers
42. E=hc/?
Noble gases
redox reaction
electromagnetic energy of photons emmited from electrons at ground state
Activation energy
43. 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
Equlibrium constant
Hydrogen bonding
Dispersion Forces
redox reaction
44. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Nucleus
Decomposition reaction
Principle quantum number
45. 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
Lewis structure
Le chateliers Principle
Group 7A
Proton
46. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Spin quantum number
Covalent Bond
Proton
Lewis acid base reaction
47. 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
Vapor pressure
ionic cmpound
hydrogen bonding
Formal Charge
48. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Strong acid
chemical reaction
Halogens
Atomic weight
49. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
molecular weight
Raoult's Law
Buffer
quantum
50. 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
redox reaction
und's rule
electron affinity