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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 measured amount of a solution of unknown concentration is added to a known volume of a second solution until the reaction between them is just complete
Titration
Redox Half Reaction
Ground state
atomic radius
2. 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
quanta
Resonance structure
Ionic Bond
Concentration
3. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
Group 6A
Aqueous Solution
Bronsted Lowry
Noble gases
4. 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
Molality
Azeotrope
electrolysis
representative elements
5. Property of the elements that can be predicted from the arrangement of the periodic table
Solution equilibrium
periodic trends
Principle quantum number
Neutralization reaction
6. 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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7. In a solution - the substance that dissolves in the solvent
pH
Solute
Collision theory of chemical Kinetics
Nonpolar covalent bond
8. Small discrete increments of energy.
Lewis definition
Equilibrium
quanta
Combination Reaction
9. A solid made up of particles that are not arranged in a regular pattern.
Henry's Law
Buffer
amorphous solid
Equivalence point
10. 5 valence electrons -3 ions - Nitride N
lathanide series
Atomic weight
Group 5A
d orbital
11. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Covalent Bond
Raoult's Law
quanta
Common ion effect
12. 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
Reaction order
Hydrogen bonding
VSEPR
Spin quantum number
13. 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
Nucleus
Le chateliers Principle
Group 5A
Collision theory of chemical Kinetics
14. 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
lewis base
percent composition
Neutralization reaction
15. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
STP
Lewis definition
Nucleus
theoretical yield
16. Redox reaction - in which the same species is both oxidized and reduced.
Disproportionation
Raoult's Law
Net ionic equation
Ion dipole interactions
17. 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
empirical formula
Proton
Planck's Constant
pi bonds
18. The formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
Resonance structure
Lewis acid base reaction
Colligative properties
Network covalent
19. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Nucleus
Chemical Kinetics
Lewis acid base reaction
Neutralization reaction
20. Contains nonmetals - 7 valence electrons in it's outermost energy level. Very reactive
Lewis acid base reaction
s orbital
Halogens
law of constant composition
21. Sum of the protons and neutrons in an element often denoted by the letter A
Mass number
Diffusion
Solvent
Noble gases
22. 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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23. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
Reaction order
Lewis acid base reaction
Charles and Gay Lussac's Law
Ion dipole interactions
24. The percent by mass of each element in a compound
Dipole Dipole interaction
Buffer
Formula weight
percent composition
25. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
amorphous solid
Covalent Bond
London forces
electron configuration
26. 5 different orbitals shaped like clover leaves and max electrons is 10
energy state
d orbital
molecule
Phase diagram
27. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Emperical Formula
solvation
quantum
Dipole
28. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Solute
solvation
Avagadros number
Magnetic quantum number
29. 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.
pi bonds
actinide series
atomic radius
London forces
30. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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31. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
energy state
Henry's Law
gram equivalent weight
Atomic weight
32. E=hc/?
Bronsted Lowry
azimuthal quantum number
Redox Half Reaction
electromagnetic energy of photons emmited from electrons at ground state
33. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
sigma bond
pi bonds
Avagadros number
bond energy
34. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
s orbital
Lewis structure
Lewis definition
Theoretical yield
35. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Rydberg constant
Reaction mechanism
Nonpolar covalent bond
Acid dissociation constant
36. An uncharged molecule with a single unpaitred electron in its outer ring - very unstable - exists for only about 10 seconds
Free radical
Strong acid
bond energy
Combination Reaction
37. 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
Halogens
Solute
Lyman series
azimuthal quantum number
38. An elementary particle with 0 charge and mass about equal to a proton
Neutron
Aqueous Solution
und's rule
Colligative properties
39. 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
electron affinity
atomic radius
Ionic Bond
Concentration
40. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Group 3A
Equilibrium
gram equivalent weight
Net ionic equation
41. The nuclear charge experienced by the outermost electrons of an atom (actual charge minus the shielding caused by inner shells: Z- eff)
lewis base
effective nuclear charge
Titration
electrolysis
42. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Acid dissociation constant
Rate determining step
Pauli exclusion principle
Molality
43. 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
azimuthal quantum number
Neutron
Arrhenius Definition
Aqueous Solution
44. A reaction in which atoms of one element take the place of atoms of another element in a compound
Colligative properties
single displacement reaction
pi bonds
ionic cmpound
45. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Combination Reaction
atomic radius
crystalline solid
lewis base
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
Formal Charge
Solvent
hydrogen bonding
Resonance structure
47. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Colligative properties
Conjugate acids and Bases
electron affinity
Planck's Constant
48. A horizontal row of elements in the periodic table
Group 7A
amorphous solid
Period
Hydrogen bonding
49. Numbers that specify the properties of atomic orbitals and of their electrons
Acid dissociation constant
quantum numbers
quanta
Vapor pressure
50. Having characteristics of both an acid and a base and capable of reacting as either
molecular weight
Amphoteric
Percent composition
single displacement reaction