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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 by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Neutron
transition elements
subshell
Effusion
2. 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
Rate determining step
Colligative properties
pH
Diprotic Base
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.
Group 7A
Lyman series
indicator
Ionization energy
4. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Avagadros number
Vapor pressure
bond length
VSEPR
5. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
solvation
decomposition reaction
Solubility Product Constant
Henderson Hasselbalch Equation
6. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
single displacement reaction
empirical formula
quanta
angular momentum in the bohr model
7. 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.
Balmer series
Noble gases
azimuthal quantum number
Le chateliers Principle
8. 5 valence electrons -3 ions - Nitride N
Group 5A
effective nuclear charge
Magnetic quantum number
Rate law
9. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Proton
Arrhenius Definition
indicator
Combination Reaction
10. A definite stable energy that a physical system can have
Atomic absorption Spectra
energy state
Henry's Law
Ionization energy
11. 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
amorphous solid
Combination Reaction
s orbital
pI
12. A reaction in which atoms of one element take the place of atoms of another element in a compound
Ionization energy
single displacement reaction
Neutralization reaction
Aqueous Solution
13. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
subshell
Charles and Gay Lussac's Law
Group 2A
14. 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
Period
Ion product
Molarity
15. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Neutralization reaction
Alkaline earths
quantum
electron configuration
16. 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.
Aqueous Solution
Triple point
Noble gases
Principle quantum number
17. Having characteristics of both an acid and a base and capable of reacting as either
Arrhenius Definition
Le chateliers Principle
Resonance structure
Amphoteric
18. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Molecular orbital
Disproportionation
angular momentum in the bohr model
atomic emission spectrum
19. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Reaction mechanism
indicator
Common ion effect
atomic emission spectrum
20. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Group 6A
ionic cmpound
theoretical yield
21. Gram equivalent weight of solute per liter of solution - often denoted by N.
molecule
Normality
quantum numbers
Molarity
22. 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
Reaction order
Magnetic quantum number
Emperical Formula
Equivalence point
23. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Common ion effect
Nonpolar covalent bond
effective nuclear charge
Mass number
24. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
lewis base
Group 2A
Group 4A
Electronegativity
25. PH of a molecule at which it contains no net electric charge - isoelectric point.
subshell
Titration
atomic emission spectrum
pI
26. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
representative elements
Covalent Bond
Molarity
Intermolecular forces
27. An atom or group of atoms that has a positive or negative charge
Lewis acid base reaction
Charles and Gay Lussac's Law
Ion
atomic emission spectrum
28. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
crystalline solid
Conjugate acids and Bases
Electrolyte
bond energy
29. Named after their cation and anion
ionic cmpound
Decomposition reaction
heisenberg uncertainty principle
electron affinity
30. E=hc/?
single displacement reaction
subshell
electromagnetic energy of photons emmited from electrons at ground state
Diprotic Base
31. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Molar solubility
atomic theory
Vapor pressure
Resonance structure
32. The slowest elementary step which is the limit for the rate of the other steps
Rate determining step
Equlibrium constant
quantum
Percent yield
33. Two or more atoms held together by covalent bonds
single displacement reaction
molecular weight
Halogens
molecule
34. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
physical reaction
compound
redox reaction
Water dissociation Constant
35. A substance that - when dissolved in water - results in a solution that can conduct electricity
Effective nuclear charge
percent composition
Reaction order
Electrolyte
36. 5 different orbitals shaped like clover leaves and max electrons is 10
Molality
d orbital
atomic radius
gram equivalent weight
37. 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
Lewis acid base reaction
Ground state
38. The process of decomposing a chemical compound by the passage of an electric current.
electromagnetic energy of photons emmited from electrons at ground state
Group 7A
electrolysis
subshell
39. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Disproportionation
electron configuration
Ion
40. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Chemical Kinetics
STP
Formula weight
Magnetic quantum number
41. 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-
heisenberg uncertainty principle
Water dissociation Constant
Solvent
Ground state
42. The lowest allowable energy state of an atom
Group 6A
Ground state
Solvent
solvation
43. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
atomic emission spectrum
STP
Colligative properties
44. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
actinide series
Group 4A
representative elements
Rate law
45. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Alkaline earths
empirical formula
Collision theory of chemical Kinetics
Rydberg constant
46. 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
Ionic Bond
Azeotrope
Nonpolar covalent bond
Equivalence point
47. 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
Common ion effect
Pauli exclusion principle
Half equivalence point
Azeotrope
48. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
quanta
Combination Reaction
Bronsted Lowry
Titration
49. The area of chemistry that is concerned with reaction rates and reaction mechanisms
indicator
Chemical Kinetics
redox reaction
Arrhenius Definition
50. An ionic compound that resists changes in its pH
Percent composition
Buffer
Avagadros number
redox reaction