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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 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
heisenberg uncertainty principle
percent composition
solvation
Ionic Bond
2. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Octet Rule
Aqueous Solution
quantum numbers
Redox Half Reaction
3. 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
Common ion effect
Equilibrium
redox reaction
4. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Half equivalence point
energy state
Aqueous Solution
Equilibrium
5. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
sigma bond
mole
Colligative properties
Ion
6. 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
Equivalence point
Ionic Bond
Ion
7. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Pauli exclusion principle
Henderson Hasselbalch Equation
empirical formula
atomic radius
8. Gram equivalent weight of solute per liter of solution - often denoted by N.
Water dissociation Constant
Octet Rule
Normality
Nucleus
9. 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
redox reaction
Collision theory of chemical Kinetics
percent composition
Ionization energy
10. Substance in which a solute is dissolved to form a solution
Effusion
Ion dipole interactions
ionic cmpound
Solvent
11. Rare earth element group (elements 58-71)
Dipole
indicator
lathanide series
Bronsted - Lowry definition
12. The point during a titration when the number of H+ ions and OH- ions are equal. This is at the middle of the steepest part of the titration curve.
Equivalence point
Electronegativity
mole
atomic theory
13. A definite stable energy that a physical system can have
lathanide series
energy state
Reaction mechanism
Solute
14. E=hc/?
electrolysis
Balmer series
Network covalent
electromagnetic energy of photons emmited from electrons at ground state
15. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Nucleus
VSEPR
mole
Collision theory of chemical Kinetics
16. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Nucleus
solvation
electrolysis
Ground state
17. The hypothetical equation showing only the species that is oxidized or reduced in a redox reaction and the correct number of electrons transferred between the species in the complete - balanced equation.
physical reaction
electron affinity
Redox Half Reaction
Arrhenius Definition
18. An ionic compound that resists changes in its pH
Molarity
Equilibrium
Buffer
Raoult's Law
19. 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
physical reaction
bond energy
Percent yield
pi bonds
20. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
electron affinity
Molar solubility
Formal Charge
21. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
single displacement reaction
angular momentum in the bohr model
gram equivalent weight
Reaction mechanism
22. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Dipole Dipole interaction
Redox Half Reaction
quantum
empirical formula
23. A subdivision of an energy level in an atom. They are divided into orbitals.
compound
subshell
The bohr model
Reaction mechanism
24. The percent by mass of each element in a compound
Henderson Hasselbalch Equation
Atomic absorption Spectra
percent composition
Network covalent
25. The slowest elementary step which is the limit for the rate of the other steps
Activation energy
Ionization energy
Rate determining step
crystalline solid
26. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Redox Half Reaction
Group 1A
Molality
mole
27. The energy required to break a chemical bond and form neutral isolated atoms
indicator
bond energy
Electronegativity
Acid dissociation constant
28. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
atomic radius
Net ionic equation
Group 2A
Colligative properties
29. A solid made up of particles that are not arranged in a regular pattern.
Equivalence point
und's rule
Group 2A
amorphous solid
30. An elementary particle with 0 charge and mass about equal to a proton
Neutron
theoretical yield
Ion product
Activation energy
31. The process by which one or more substances change to produce one or more different substances
chemical reaction
representative elements
Charles and Gay Lussac's Law
Electronegativity
32. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
compound
theoretical yield
Molar solubility
33. 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
ionic cmpound
The bohr model
lathanide series
atomic emission spectrum
34. A reaction in which atoms of one element take the place of atoms of another element in a compound
Neutron
atomic radius
Chemical Kinetics
single displacement reaction
35. Slightly less reactive than alkali metals - comprise group II
electron configuration
redox reaction
Water dissociation Constant
Alkaline earths
36. The lowest allowable energy state of an atom
Titration
quantum numbers
Azeotrope
Ground state
37. Defined acids as subtsances that produced H ions in water - while bases produced OH ions. When they reacted together - H and OH neutralise to make water
Equlibrium constant
Arrhenius Definition
Strong acid
Nucleus
38. 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
Proton
heisenberg uncertainty principle
Buffer
und's rule
39. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Pauli exclusion principle
indicator
Hydrogen bonding
Free radical
40. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Effusion
Electronegativity
Network covalent
Henry's Law
41. 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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42. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
compound
amorphous solid
Planck's Constant
atomic radius
43. 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
Resonance structure
Ionic Bond
percent composition
Formal Charge
44. Having characteristics of both an acid and a base and capable of reacting as either
Diprotic Base
Amphoteric
Principle quantum number
Henderson Hasselbalch Equation
45. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Dipole
energy state
Pauli exclusion principle
Lewis definition
46. Any sample of a given compound will contain the same elements in the identical mass ratio.
Group 1A
Normality
electromagnetic energy of photons emmited from electrons at ground state
law of constant composition
47. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Nonpolar covalent bond
decomposition reaction
sigma bond
48. 2.18 x 10^-18 J/electron
transition elements
effective nuclear charge
Rydberg constant
chemical reaction
49. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Ion product
Group 4A
solvation
atomic radius
50. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
quanta
Avagadros number
Combination Reaction
atomic theory