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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. 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
Group 7A
Normality
Atomic absorption Spectra
Resonance structure
2. Small discrete increments of energy.
Le chateliers Principle
quanta
solvation
Amphoteric
3. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Dispersion Forces
Half equivalence point
quanta
atomic radius
4. 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.
Concentration
Redox Half Reaction
Strong acid
s orbital
5. The Percent by mass of each element in a compound.
Electronegativity
Chemical Kinetics
pH
Percent composition
6. A solution in which water is the solvent
Mass number
Ionic Bond
Aqueous Solution
chemical reaction
7. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
gram equivalent weight
quantum
Effusion
Diffusion
8. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Percent yield
atomic emission spectrum
Period
9. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Le chateliers Principle
gram equivalent weight
atomic radius
10. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
Alkaline earths
Redox Half Reaction
empirical formula
Neutralization reaction
11. 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.
Azeotrope
Diprotic Base
Effective nuclear charge
Group 6A
12. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Group 3A
Ion
Henry's Law
amorphous solid
13. 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
ionic cmpound
transition elements
Octet Rule
14. An atom or group of atoms that has a positive or negative charge
Ion
Emperical Formula
Diprotic Base
bond length
15. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
lewis base
Percent composition
Bronsted Lowry
Alkaline earths
16. Simplest whole # ration of atoms in a compound
Neutron
Emperical Formula
heisenberg uncertainty principle
Charles and Gay Lussac's Law
17. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
gram equivalent weight
Solvent
decomposition reaction
physical reaction
18. 5 different orbitals shaped like clover leaves and max electrons is 10
actinide series
d orbital
molecule
Water dissociation Constant
19. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Group 1A
Molality
effective nuclear charge
Nucleus
20. 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.
electron affinity
pi bonds
Spin quantum number
Rate law
21. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Solubility Product Constant
Principle quantum number
electromagnetic energy of photons emmited from electrons at ground state
Lewis structure
22. 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
s orbital
decomposition reaction
Collision theory of chemical Kinetics
Azeotrope
23. A reaction in which atoms of one element take the place of atoms of another element in a compound
Molarity
Lewis acid base reaction
single displacement reaction
Ion
24. 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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25. 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.
Concentration
sigma bond
Balmer series
s orbital
26. 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
sigma bond
Aqueous Solution
representative elements
27. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
single displacement reaction
The bohr model
electron configuration
Diffusion
28. 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.
Planck's Constant
Avagadros number
lathanide series
Equivalence point
29. 4 valence electrons +4 - -4 ions. - Carbon Group can form covalent bonds with nonmetals. Only carbon forms strong pi bonds
Equivalence point
bond energy
bond length
Group 4A
30. E=hc/?
subshell
representative elements
electromagnetic energy of photons emmited from electrons at ground state
Bronsted - Lowry definition
31. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Molecular orbital
Henderson Hasselbalch Equation
Group 2A
Covalent Bond
32. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
Neutron
Group 1A
lewis base
pi bonds
33. 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
percent composition
Ion
Resonance structure
34. Have three valance electrons. In certain instances - some elements will loose three electrons - but they will also share electrons with another element to attain stability.
Group 3A
Phase diagram
Diffusion
Rate determining step
35. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
representative elements
Diffusion
Lewis structure
Octet Rule
36. A reaction in which atoms of one element take the place of atoms of another element in a compound
Group 3A
Chemical Kinetics
single displacement reaction
Electronegativity
37. Gram equivalent weight of solute per liter of solution - often denoted by N.
atomic theory
actinide series
Normality
Aqueous Solution
38. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Lewis acid base reaction
Pauli exclusion principle
theoretical yield
single displacement reaction
39. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Water dissociation Constant
molecular weight
Atomic weight
Henry's Law
40. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Diffusion
Effusion
Henry's Law
compound
41. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
actinide series
STP
Theoretical yield
VSEPR
42. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Concentration
STP
Nonpolar covalent bond
d orbital
43. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
Molar solubility
Molality
pH
Le chateliers Principle
44. Any sample of a given compound will contain the same elements in the identical mass ratio.
law of constant composition
Decomposition reaction
The bohr model
Chemical Kinetics
45. A dynamic condition in which two opposing changes occur at equal rates in a closed system
Pauli exclusion principle
Equilibrium
Ion
Buffer
46. The maximum amount of product that can be produced from a given amount of reactant
hydrogen bonding
Raoult's Law
theoretical yield
Lyman series
47. 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
Magnetic quantum number
Lyman series
Henderson Hasselbalch Equation
Rate law
48. Named after their cation and anion
Electrolyte
Pauli exclusion principle
molecule
ionic cmpound
49. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Ion dipole interactions
Neutralization reaction
redox reaction
Lewis acid base reaction
50. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Molarity
electromagnetic energy of photons emmited from electrons at ground state
Planck's Constant