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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 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
Strong acid
Proton
molecule
Ground state
2. 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
indicator
lewis base
Intermolecular forces
Formal Charge
3. 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
azimuthal quantum number
Henderson Hasselbalch Equation
Molar solubility
Solution equilibrium
4. 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
Resonance structure
London forces
atomic radius
Strong acid
5. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Balmer series
Common ion effect
Arrhenius Definition
Decomposition reaction
6. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
physical reaction
Dipole
Molality
Avagadros number
7. 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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8. 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
Colligative properties
Atomic absorption Spectra
Halogens
Period
9. 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
Electronegativity
electromagnetic energy of photons emmited from electrons at ground state
The bohr model
Le chateliers Principle
10. Simplest whole # ration of atoms in a compound
Group 6A
percent composition
Emperical Formula
Reaction order
11. 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.
Molar solubility
crystalline solid
Electrolyte
compound
12. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
molecule
Aqueous Solution
Group 6A
actinide series
13. A reaction where a compound does Not change its molecular structure.
physical reaction
pi bonds
electron affinity
Collision theory of chemical Kinetics
14. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
angular momentum in the bohr model
Group 2A
Nucleus
Le chateliers Principle
15. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Rate law
Bronsted - Lowry definition
representative elements
16. 5 different orbitals shaped like clover leaves and max electrons is 10
Aqueous Solution
d orbital
Arrhenius Definition
Formula weight
17. 5 valence electrons -3 ions - Nitride N
London forces
Activation energy
Group 5A
empirical formula
18. Halogens; ns2np5 - - 2nd most reactive group - The Halogens; very active because of need to fill; form -1 ions; 7 electrons in valence shell; tend to form salts with elements from groups 1A and 2A
percent composition
Group 7A
Ion product
Molecular orbital
19. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Group 7A
Conjugate acids and Bases
angular momentum in the bohr model
Rate law
20. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
Dipole
Molar solubility
Titration
Effective nuclear charge
21. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Ion dipole interactions
Magnetic quantum number
Dipole
Ion
22. E=hc/?
Theoretical yield
Diprotic Base
electromagnetic energy of photons emmited from electrons at ground state
Chemical Kinetics
23. 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
quantum
Normality
Formula weight
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.
Emperical Formula
Le chateliers Principle
Principle quantum number
energy state
25. 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
Solution equilibrium
Lewis definition
Solute
Ionic Bond
26. Property of the elements that can be predicted from the arrangement of the periodic table
Solvent
Dipole Dipole interaction
Group 4A
periodic trends
27. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
bond length
atomic theory
STP
Amphoteric
28. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Molar solubility
Collision theory of chemical Kinetics
Aqueous Solution
Half equivalence point
29. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
transition elements
electrolysis
Graham's Law
Octet Rule
30. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
quantum
VSEPR
molecular weight
Titration
31. Named after their cation and anion
Redox Half Reaction
quanta
effective nuclear charge
ionic cmpound
32. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Arrhenius Definition
azimuthal quantum number
Balmer series
33. 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
Nucleus
Azeotrope
Hydrogen bonding
Equilibrium
34. 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
The bohr model
Activation energy
Hydrogen bonding
Halogens
35. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Avagadros number
Ionic Bond
Dipole Dipole interaction
molecule
36. A horizontal row of elements in the periodic table
Buffer
electron affinity
Period
Molecular orbital
37. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
ionic cmpound
redox reaction
Principle quantum number
effective nuclear charge
38. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Lewis structure
Colligative properties
bond length
sigma bond
39. Resulting positive nuclear charge an outer electron senses after accounting for the shielding effect of inner core electrons. Abbreviated as Z(eff). Increases from left to right - and bottom to top on the Periodic Table.
bond length
redox reaction
Effective nuclear charge
Acid dissociation constant
40. 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
Triple point
Equlibrium constant
percent composition
Ion
41. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
chemical reaction
pi bonds
Electronegativity
Molar solubility
42. The process of decomposing a chemical compound by the passage of an electric current.
quantum numbers
electrolysis
Amphoteric
redox reaction
43. A subdivision of an energy level in an atom. They are divided into orbitals.
Ionization energy
quantum
Titration
subshell
44. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
Rate determining step
pH
electron affinity
45. 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
Lewis definition
electron configuration
Lewis structure
46. The energy required to break a chemical bond and form neutral isolated atoms
STP
bond energy
Magnetic quantum number
Activation energy
47. 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.
Ion
single displacement reaction
Ground state
Solubility Product Constant
48. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Neutralization reaction
Effusion
lathanide series
Hydrogen bonding
49. 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
Planck's Constant
Emperical Formula
Molarity
Dispersion Forces
50. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
Network covalent
Solution equilibrium
Electrolyte
Covalent Bond