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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 ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
London forces
Lyman series
Molar solubility
2. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Half equivalence point
Noble gases
Henry's Law
Strong acid
3. 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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4. 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
Acid dissociation constant
Emperical Formula
Common ion effect
percent composition
5. A base that can accept two moles of H+ per mole of itself (ex: SO4
Le chateliers Principle
VSEPR
Ionic Bond
Diprotic Base
6. Property of the elements that can be predicted from the arrangement of the periodic table
Dipole
Half equivalence point
redox reaction
periodic trends
7. Elements in the middle of the periodic table - in groups 3-12.
transition elements
Theoretical yield
quanta
Activation energy
8. The average distance between the nuclei of two bonded atoms
azimuthal quantum number
bond length
Chemical Kinetics
Reaction mechanism
9. A reaction in which atoms of one element take the place of atoms of another element in a compound
single displacement reaction
Conjugate acids and Bases
Molality
Raoult's Law
10. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Dipole
Neutralization reaction
s orbital
Dipole Dipole interaction
11. The maximum amount of product that can be produced from a given amount of reactant
heisenberg uncertainty principle
mole
theoretical yield
Halogens
12. 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
quanta
Resonance structure
Principle quantum number
Dipole Dipole interaction
13. 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
Colligative properties
Phase diagram
Ground state
Proton
14. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Equilibrium
Network covalent
actinide series
Reaction mechanism
15. 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.
crystalline solid
Collision theory of chemical Kinetics
chemical reaction
atomic radius
16. 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.
VSEPR
Mass number
Colligative properties
Diffusion
17. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
und's rule
Electrolyte
Vapor pressure
redox reaction
18. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
polymer
atomic emission spectrum
Rate law
effective nuclear charge
19. 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
Group 4A
d orbital
Noble gases
20. Having characteristics of both an acid and a base and capable of reacting as either
polymer
physical reaction
Effective nuclear charge
Amphoteric
21. An elementary particle with 0 charge and mass about equal to a proton
Network covalent
Arrhenius Definition
Neutron
Solvent
22. 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
Solution equilibrium
Diffusion
polymer
23. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
heisenberg uncertainty principle
Conjugate acids and Bases
Noble gases
Lewis acid base reaction
24. Gram equivalent weight of solute per liter of solution - often denoted by N.
Ion
pi bonds
theoretical yield
Normality
25. 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
Dispersion Forces
Covalent Bond
Dipole
26. The energy required to remove an electron from a gaseous atom; generally increases in moving from left - to - right across a period and decreases in moving down a group
Ionization energy
quanta
azimuthal quantum number
Ion
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.
subshell
Emperical Formula
sigma bond
Lyman series
28. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
Octet Rule
Ion
Electrolyte
29. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Henry's Law
Group 5A
Electronegativity
polymer
30. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
und's rule
Normality
chemical reaction
sigma bond
31. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
redox reaction
Concentration
Lewis acid base reaction
Nonpolar covalent bond
32. Common definition of acids as proton (H+) donors and bases as proton acceptors
heisenberg uncertainty principle
Bronsted - Lowry definition
pH
Henderson Hasselbalch Equation
33. Slightly less reactive than alkali metals - comprise group II
Amphoteric
Group 5A
representative elements
Alkaline earths
34. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Resonance structure
Group 1A
Group 5A
Diprotic Base
35. A fundamental constant - h - that relates the energy of light quanta to their frequency: h = 6.6 X 10^-34 joule
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36. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
s orbital
Neutralization reaction
Formula weight
Combination Reaction
37. A substance that - when dissolved in water - results in a solution that can conduct electricity
actinide series
Electrolyte
quantum numbers
chemical reaction
38. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Ion product
Group 6A
Theoretical yield
molecule
39. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Lewis definition
Reaction order
Molecular orbital
electron affinity
40. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
physical reaction
Molecular orbital
theoretical yield
atomic emission spectrum
41. 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
Equilibrium
pI
physical reaction
hydrogen bonding
42. A definite stable energy that a physical system can have
Octet Rule
energy state
periodic trends
Vapor pressure
43. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
Redox Half Reaction
Free radical
atomic radius
44. A solution in which water is the solvent
Formula weight
Aqueous Solution
Combination Reaction
atomic radius
45. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
pI
empirical formula
chemical reaction
46. The percent by mass of each element in a compound
percent composition
molecular weight
Diffusion
chemical reaction
47. A subdivision of an energy level in an atom. They are divided into orbitals.
Hydrogen bonding
subshell
Theoretical yield
Diffusion
48. 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
Diprotic Base
Avagadros number
Spin quantum number
s orbital
49. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Lewis structure
quantum numbers
Molar solubility
Spin quantum number
50. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Pauli exclusion principle
Half equivalence point
pH
Henry's Law