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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 reaction in which atoms of one element take the place of atoms of another element in a compound
electron configuration
Ionic Bond
electromagnetic energy of photons emmited from electrons at ground state
single displacement reaction
2. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Lewis structure
Molecular orbital
Effusion
effective nuclear charge
3. A solid made up of particles that are not arranged in a regular pattern.
und's rule
amorphous solid
periodic trends
heisenberg uncertainty principle
4. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
gram equivalent weight
Half equivalence point
Dispersion Forces
Ion product
5. 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
Group 1A
The bohr model
atomic radius
Ionization energy
6. Rare earth element group (elements 58-71)
empirical formula
lathanide series
Lyman series
decomposition reaction
7. PH of a molecule at which it contains no net electric charge - isoelectric point.
Aqueous Solution
Reaction order
pI
redox reaction
8. Common definition of acids as proton (H+) donors and bases as proton acceptors
Electronegativity
gram equivalent weight
Bronsted - Lowry definition
Normality
9. Acids defined as electron - pair acceptors and bases as electron - pair donors.
amorphous solid
Emperical Formula
Neutron
Lewis definition
10. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
lathanide series
Rydberg constant
effective nuclear charge
Le chateliers Principle
11. 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
Equlibrium constant
Network covalent
Reaction mechanism
Group 3A
12. 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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13. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
STP
molecular weight
Octet Rule
Molecular orbital
14. 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
angular momentum in the bohr model
Atomic absorption Spectra
physical reaction
hydrogen bonding
15. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Le chateliers Principle
Titration
Graham's Law
Diffusion
16. A substance that - when dissolved in water - results in a solution that can conduct electricity
redox reaction
Electrolyte
Pauli exclusion principle
Molality
17. 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
single displacement reaction
Ionic Bond
Percent composition
Triple point
18. 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.
Effective nuclear charge
Balmer series
Le chateliers Principle
Proton
19. 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
s orbital
Formal Charge
Group 7A
chemical reaction
20. A horizontal row of elements in the periodic table
Period
Mass number
quantum
s orbital
21. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Group 4A
Rate law
Neutralization reaction
atomic radius
22. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Spin quantum number
s orbital
Group 1A
Theoretical yield
23. Elements in the middle of the periodic table - in groups 3-12.
Raoult's Law
Equlibrium constant
Group 1A
transition elements
24. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Acid dissociation constant
electron configuration
Group 2A
Planck's Constant
25. 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.
Atomic weight
Alkaline earths
Principle quantum number
atomic radius
26. 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
Neutralization reaction
Collision theory of chemical Kinetics
Dispersion Forces
Rydberg constant
27. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Avagadros number
Group 3A
Charles and Gay Lussac's Law
Covalent Bond
28. The process by which one or more substances change to produce one or more different substances
chemical reaction
Acid dissociation constant
Normality
Collision theory of chemical Kinetics
29. (chemistry) a substance that changes color to indicate the presence of some ion or substance
compound
Neutron
indicator
Disproportionation
30. 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
crystalline solid
Octet Rule
Collision theory of chemical Kinetics
azimuthal quantum number
31. 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
Dipole
Concentration
Phase diagram
32. Any sample of a given compound will contain the same elements in the identical mass ratio.
Dipole Dipole interaction
Lyman series
law of constant composition
electrolysis
33. Substance in which a solute is dissolved to form a solution
Solubility Product Constant
Arrhenius Definition
energy state
Solvent
34. Chalcogens - - Oxide O
Group 6A
Nucleus
solvation
chemical reaction
35. 5 valence electrons -3 ions - Nitride N
Group 5A
Charles and Gay Lussac's Law
law of constant composition
Graham's Law
36. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
quanta
Vapor pressure
Conjugate acids and Bases
37. 2.18 x 10^-18 J/electron
Rydberg constant
Ion product
Ionization energy
Network covalent
38. Spectrum of certain absorbed wavelengths of light corresponding to an atom's spectrum of emitted frequencies of light. Unique to each element. AAS can be used to indentify an element.
Atomic absorption Spectra
Noble gases
Nucleus
Ionic Bond
39. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
Theoretical yield
hydrogen bonding
electron affinity
STP
40. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
crystalline solid
atomic theory
Ion
single displacement reaction
41. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Molality
Nonpolar covalent bond
Solution equilibrium
pi bonds
42. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Electrolyte
single displacement reaction
Resonance structure
43. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Ground state
Ionization energy
s orbital
angular momentum in the bohr model
44. Having characteristics of both an acid and a base and capable of reacting as either
Lewis structure
Amphoteric
azimuthal quantum number
indicator
45. 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
Equivalence point
Rydberg constant
Balmer series
46. 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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47. A base that can accept two moles of H+ per mole of itself (ex: SO4
atomic emission spectrum
Diprotic Base
pi bonds
Molar solubility
48. The lowest allowable energy state of an atom
electron affinity
Group 1A
Ground state
electromagnetic energy of photons emmited from electrons at ground state
49. 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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50. 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 acid base reaction
compound
Emperical Formula