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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. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Molality
Percent composition
Alkaline earths
crystalline solid
2. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Strong acid
Balmer series
Effusion
Group 1A
3. 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
Equivalence point
Ion
Solution equilibrium
transition elements
4. Contains nonmetals that are non - reactive. Full outermost energy level except helium which has 2.
Noble gases
energy state
theoretical yield
Solvent
5. 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
Avagadros number
Proton
The bohr model
Common ion effect
6. 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
Common ion effect
Reaction order
s orbital
Group 6A
7. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Half equivalence point
Aqueous Solution
Neutron
8. Common definition of acids as proton (H+) donors and bases as proton acceptors
Bronsted Lowry
Molecular orbital
Percent composition
Bronsted - Lowry definition
9. (chemistry) p(otential of) H(ydrogen)
effective nuclear charge
amorphous solid
pH
crystalline solid
10. Rare earth element group (elements 58-71)
Le chateliers Principle
Group 1A
lathanide series
Halogens
11. Having characteristics of both an acid and a base and capable of reacting as either
Reaction mechanism
Amphoteric
Strong acid
Group 2A
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. 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
Effective nuclear charge
Activation energy
Group 3A
14. The Percent by mass of each element in a compound.
bond length
Azeotrope
Percent composition
electron affinity
15. 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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16. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Spin quantum number
energy state
Phase diagram
Molar solubility
17. Temperature is constant; effusion and temperature are proportional to the square root of their masses
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18. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
solvation
Group 2A
Effective nuclear charge
Chemical Kinetics
19. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Half equivalence point
pH
lewis base
compound
20. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
lathanide series
Vapor pressure
s orbital
Molar solubility
21. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
STP
Free radical
Lewis structure
molecule
22. Sol - a chemical process in which solvent molecules and molecules or ions of the solute combine to form a compound
solvation
Azeotrope
pi bonds
London forces
23. 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
Le chateliers Principle
Formal Charge
Percent yield
pI
24. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
Group 4A
Covalent Bond
periodic trends
transition elements
25. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
Effusion
Bronsted - Lowry definition
Combination Reaction
atomic radius
26. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Chemical Kinetics
pi bonds
redox reaction
Henderson Hasselbalch Equation
27. Chalcogens - - Oxide O
Emperical Formula
Group 6A
pI
Raoult's Law
28. 5 valence electrons -3 ions - Nitride N
Group 5A
Redox Half Reaction
Network covalent
molecule
29. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Lyman series
gram equivalent weight
Dipole Dipole interaction
redox reaction
30. 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
Percent composition
Water dissociation Constant
Azeotrope
Bronsted Lowry
31. The process by which one or more substances change to produce one or more different substances
Strong acid
Raoult's Law
chemical reaction
Water dissociation Constant
32. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Atomic weight
Triple point
Molarity
transition elements
33. 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.
Colligative properties
Solution equilibrium
Lyman series
Balmer series
34. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Activation energy
Concentration
Electronegativity
London forces
35. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Group 2A
Percent yield
Lewis definition
mole
36. A definite stable energy that a physical system can have
Electronegativity
energy state
Molality
Group 1A
37. 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.
ionic cmpound
empirical formula
Principle quantum number
Lyman series
38. Theory stating that the rate of a reaction is directly proportional to the number of collisions that take place between reactants per second.
angular momentum in the bohr model
Concentration
Collision theory of chemical Kinetics
compound
39. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Ion
Reaction order
crystalline solid
Equilibrium
40. 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.
Activation energy
Nucleus
Strong acid
Equivalence point
41. Two or more atoms held together by covalent bonds
molecule
heisenberg uncertainty principle
Azeotrope
Group 1A
42. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Neutron
Dipole
Theoretical yield
Lewis definition
43. In a solution - the substance that dissolves in the solvent
Rate determining step
atomic radius
Spin quantum number
Solute
44. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
Group 2A
Buffer
effective nuclear charge
Disproportionation
45. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Conjugate acids and Bases
effective nuclear charge
Ionic Bond
Intermolecular forces
46. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
Solution equilibrium
sigma bond
Intermolecular forces
Equivalence point
47. The point on a phase diagram that represents the only set of conditions at which all three phases exist in equilibrium with one another
Triple point
Ionic Bond
azimuthal quantum number
bond length
48. 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.
Redox Half Reaction
Ionic Bond
London forces
STP
49. 5 different orbitals shaped like clover leaves and max electrons is 10
Reaction mechanism
Ground state
d orbital
mole
50. Named after their cation and anion
Group 4A
ionic cmpound
Percent composition
pi bonds