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MCAT Chemistry
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Subjects
:
mcat
,
science
Instructions:
Answer 50 questions in 15 minutes.
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.
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. 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
d orbital
angular momentum in the bohr model
Ionization energy
electron affinity
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
Group 4A
azimuthal quantum number
Effusion
3. The quantum number that has only two possible values - +1/2 and -1/2 - which indicate the two fundamental spin states of an electron in an orbital
Spin quantum number
crystalline solid
Arrhenius Definition
Group 7A
4. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Spin quantum number
Halogens
Octet Rule
Buffer
5. The weight in grams of one mole of a given elementand is expressedin tems of grams per mole.
Atomic weight
Redox Half Reaction
pi bonds
Diffusion
6. 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.
solvation
azimuthal quantum number
Atomic absorption Spectra
Formula weight
7. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Solute
The bohr model
Balmer series
8. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Reaction order
Raoult's Law
single displacement reaction
azimuthal quantum number
9. The Percent by mass of each element in a compound.
Hydrogen bonding
Equivalence point
Percent composition
Effusion
10. Acids defined as electron - pair acceptors and bases as electron - pair donors.
Lewis definition
Graham's Law
Decomposition reaction
Spin quantum number
11. Valence Shell Electron Pair Repulsion theory - stating that the three - dimensional molecular geometry about some central atom is determined by the elctronic repulsion between its bonding and nonbonding electron pairs.
Equlibrium constant
Raoult's Law
VSEPR
Water dissociation Constant
12. 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
effective nuclear charge
Electrolyte
angular momentum in the bohr model
Formal Charge
13. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
Percent composition
lewis base
theoretical yield
14. 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
transition elements
sigma bond
Avagadros number
Equlibrium constant
15. 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
redox reaction
Magnetic quantum number
quanta
heisenberg uncertainty principle
16. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
hydrogen bonding
atomic radius
Redox Half Reaction
17. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Nucleus
Bronsted Lowry
Diprotic Base
Combination Reaction
18. The vapor pressure of solution is the product of the mole fraction of the solvent and the vapor pressure of the pure solvent. P_a=X_aP_total
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19. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
decomposition reaction
Solvent
Redox Half Reaction
Aqueous Solution
20. The energy required to break a chemical bond and form neutral isolated atoms
Molality
Network covalent
lathanide series
bond energy
21. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Dispersion Forces
Redox Half Reaction
VSEPR
22. The process of decomposing a chemical compound by the passage of an electric current.
Avagadros number
electrolysis
Spin quantum number
Emperical Formula
23. States that if a stress is applied to a system at equilibrium - the system shifts in the direction that relieves the stress.
atomic theory
empirical formula
Le chateliers Principle
gram equivalent weight
24. Small discrete increments of energy.
molecular weight
Solvent
Collision theory of chemical Kinetics
quanta
25. 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
Acid dissociation constant
quanta
angular momentum in the bohr model
azimuthal quantum number
26. A reaction in which atoms of one element take the place of atoms of another element in a compound
compound
molecular weight
percent composition
single displacement reaction
27. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Lewis acid base reaction
Chemical Kinetics
Acid dissociation constant
lewis base
28. Redox reaction - in which the same species is both oxidized and reduced.
Disproportionation
London forces
Chemical Kinetics
Intermolecular forces
29. A definite stable energy that a physical system can have
heisenberg uncertainty principle
Formal Charge
energy state
Disproportionation
30. 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
Dispersion Forces
representative elements
Theoretical yield
chemical reaction
31. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
Half equivalence point
Diprotic Base
electromagnetic energy of photons emmited from electrons at ground state
32. The percent by mass of each element in a compound
Acid dissociation constant
atomic radius
amorphous solid
percent composition
33. 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
Aqueous Solution
Atomic weight
electromagnetic energy of photons emmited from electrons at ground state
34. 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
Activation energy
Theoretical yield
Decomposition reaction
Percent yield
35. 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
law of constant composition
Hydrogen bonding
Group 7A
angular momentum in the bohr model
36. An elementary particle with 0 charge and mass about equal to a proton
Buffer
Le chateliers Principle
Neutron
electron configuration
37. The average distance between the nuclei of two bonded atoms
bond length
solvation
Group 5A
Activation energy
38. 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
Lewis definition
Acid dissociation constant
Neutralization reaction
39. Any sample of a given compound will contain the same elements in the identical mass ratio.
Solute
Raoult's Law
law of constant composition
single displacement reaction
40. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
Raoult's Law
Half equivalence point
Ionic Bond
Vapor pressure
41. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Lyman series
Planck's Constant
Dispersion Forces
gram equivalent weight
42. 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.
Solubility Product Constant
Atomic absorption Spectra
compound
mole
43. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
Collision theory of chemical Kinetics
Percent yield
Dipole Dipole interaction
Group 4A
44. Expression of auto - ionization of water into H+ and OH- at a certain temperature - given by the product of the ions' molar concentrations. Denoted by Kw and equal to 10-
sigma bond
Concentration
Collision theory of chemical Kinetics
Water dissociation Constant
45. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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46. A solution in which water is the solvent
Pauli exclusion principle
Water dissociation Constant
Aqueous Solution
Strong acid
47. 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
Vapor pressure
crystalline solid
pi bonds
48. When a solute is dissolved in a solvent - it will dissociate until reaching an equilibrium point at which the rate of dissociation equals the rate of precipitation of the solute - regardless of any additional solute introduced into the mixture
Chemical Kinetics
Concentration
Solution equilibrium
actinide series
49. The lowest allowable energy state of an atom
Neutron
Ground state
d orbital
actinide series
50. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Lewis definition
Decomposition reaction
compound
Theoretical yield
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