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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. 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.
Nucleus
electron affinity
law of constant composition
electron configuration
2. 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.
London forces
Colligative properties
Disproportionation
Effective nuclear charge
3. A substance that - when dissolved in water - results in a solution that can conduct electricity
The bohr model
Acid dissociation constant
Noble gases
Electrolyte
4. Small discrete increments of energy.
energy state
Group 6A
Dispersion Forces
quanta
5. Chalcogens - - Oxide O
Effective nuclear charge
Rate law
Group 6A
Half equivalence point
6. Any sample of a given compound will contain the same elements in the identical mass ratio.
Chemical Kinetics
law of constant composition
Colligative properties
Nucleus
7. A definite stable energy that a physical system can have
Solubility Product Constant
Group 3A
STP
energy state
8. States that it is impossible to determine simultaneously both the position and momentum of an electron or any other particle
Formula weight
sigma bond
heisenberg uncertainty principle
chemical reaction
9. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Diffusion
Dipole Dipole interaction
physical reaction
effective nuclear charge
10. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
electron configuration
atomic emission spectrum
polymer
Nonpolar covalent bond
11. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
electron configuration
Effusion
Common ion effect
Ionic Bond
12. A solution in which water is the solvent
Aqueous Solution
Triple point
Azeotrope
Rydberg constant
13. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Phase diagram
Electrolyte
Effusion
Theoretical yield
14. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
The bohr model
quanta
Common ion effect
sigma bond
15. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
Lyman series
Graham's Law
Decomposition reaction
solvation
16. 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
Neutron
Dipole Dipole interaction
physical reaction
Ionization energy
17. 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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18. 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
Arrhenius Definition
Strong acid
indicator
Bronsted Lowry
19. 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
Ionic Bond
pH
transition elements
subshell
20. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
Water dissociation Constant
Ion
Aqueous Solution
Group 3A
21. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Equivalence point
pI
periodic trends
22. 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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23. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Bronsted - Lowry definition
chemical reaction
Molality
Concentration
24. 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
Free radical
s orbital
compound
Emperical Formula
25. 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
Ion
Rydberg constant
Proton
Water dissociation Constant
26. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Network covalent
Decomposition reaction
solvation
Dipole Dipole interaction
27. (chemistry) p(otential of) H(ydrogen)
Group 4A
Atomic weight
Ion
pH
28. 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 emission spectrum
Lewis structure
Atomic absorption Spectra
Conjugate acids and Bases
29. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
London forces
physical reaction
Avagadros number
law of constant composition
30. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
ionic cmpound
Common ion effect
electrolysis
Atomic weight
31. Tells you how much solute is present compared to the amount of solvent
Concentration
Hydrogen bonding
Chemical Kinetics
Percent composition
32. Substance in which a solute is dissolved to form a solution
Solvent
Dispersion Forces
Raoult's Law
bond energy
33. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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34. 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.
Formula weight
Proton
solvation
Principle quantum number
35. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Atomic weight
Reaction order
Octet Rule
Group 4A
36. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
Aqueous Solution
Henry's Law
angular momentum in the bohr model
Period
37. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Equilibrium
quantum
Ionization energy
Covalent Bond
38. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Planck's Constant
theoretical yield
Bronsted Lowry
Triple point
39. An ionic compound that resists changes in its pH
redox reaction
heisenberg uncertainty principle
Percent yield
Buffer
40. 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
Molecular orbital
Effusion
Dispersion Forces
polymer
41. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Group 3A
Strong acid
azimuthal quantum number
Planck's Constant
42. (chemistry) a substance that changes color to indicate the presence of some ion or substance
indicator
Collision theory of chemical Kinetics
Group 1A
Octet Rule
43. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
Formal Charge
actinide series
lewis base
mole
44. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
single displacement reaction
Decomposition reaction
Effective nuclear charge
atomic theory
45. Product of the molar concentrations of dissociated ions in solution at any point in the reaction other than equilibrium or saturation - where each ion is raised to the power of its stoichiometric coefficient. Denoted IP.
Vapor pressure
Dipole
London forces
Ion product
46. 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
Molality
Bronsted Lowry
Intermolecular forces
hydrogen bonding
47. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
Group 2A
Group 5A
electron configuration
Chemical Kinetics
48. The tendency for an atom to attract electrons to itself when it is chemically combined with another element
Electronegativity
Rydberg constant
atomic emission spectrum
Chemical Kinetics
49. 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
quanta
Planck's Constant
Nucleus
atomic radius
50. 2.18 x 10^-18 J/electron
Planck's Constant
Rydberg constant
Conjugate acids and Bases
Group 5A