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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 formation of one or more covalent bonds between an electron pair donor and an electron pair acceptor
electromagnetic energy of photons emmited from electrons at ground state
Lewis acid base reaction
Effective nuclear charge
Group 3A
2. A chemical formula showing the ratio of elements in a compound rather than the total number of atoms
empirical formula
Collision theory of chemical Kinetics
energy state
Lewis definition
3. An equilibrium expression used to measure weak - acid strength - given by the ratio of the product of the products' molar concentrations to the product of the reactants' molar concentrations - with each term raised to the power of its stoichiometric
Acid dissociation constant
pI
sigma bond
Network covalent
4. The pressure exerted by a vapor in equilibrium with its liquid or solid phase
crystalline solid
compound
Vapor pressure
Ion dipole interactions
5. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Molality
Chemical Kinetics
redox reaction
lathanide series
6. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
Charles and Gay Lussac's Law
bond length
Concentration
Avagadros number
7. 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.
Mass number
Effective nuclear charge
Atomic absorption Spectra
Network covalent
8. A reaction in which atoms of one element take the place of atoms of another element in a compound
Titration
electromagnetic energy of photons emmited from electrons at ground state
Combination Reaction
single displacement reaction
9. 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
Molecular orbital
Reaction mechanism
azimuthal quantum number
und's rule
10. The weak attractive forces between molecules resulting from the small - instantaneous dipoles that occur because of the varying positions of the electrons during their motion about nuclei
Bronsted Lowry
Dispersion Forces
Group 7A
London forces
11. The energy required to break a chemical bond and form neutral isolated atoms
Spin quantum number
bond energy
Covalent Bond
The bohr model
12. 5 valence electrons -3 ions - Nitride N
Decomposition reaction
chemical reaction
Group 5A
Planck's Constant
13. 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
Ionization energy
azimuthal quantum number
atomic radius
Azeotrope
14. 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.
indicator
electron affinity
molecule
Principle quantum number
15. 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
Octet Rule
STP
lathanide series
Ionic Bond
16. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Equilibrium
Molality
compound
electrolysis
17. A subdivision of an energy level in an atom. They are divided into orbitals.
subshell
Colligative properties
Electrolyte
pi bonds
18. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Group 6A
Electrolyte
Spin quantum number
19. 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
Rate determining step
Dispersion Forces
Group 1A
Noble gases
20. 5 different orbitals shaped like clover leaves and max electrons is 10
d orbital
Free radical
Water dissociation Constant
Atomic weight
21. Named after their cation and anion
ionic cmpound
theoretical yield
Avagadros number
Raoult's Law
22. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Disproportionation
atomic emission spectrum
indicator
23. Rare earth element group (elements 58-71)
Solubility Product Constant
Water dissociation Constant
lathanide series
Combination Reaction
24. E=hc/?
gram equivalent weight
Lewis structure
electromagnetic energy of photons emmited from electrons at ground state
Atomic weight
25. 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.
gram equivalent weight
hydrogen bonding
Noble gases
Equivalence point
26. A dynamic condition in which two opposing changes occur at equal rates in a closed system
bond energy
Lewis definition
quantum numbers
Equilibrium
27. Process by which molecules tend to move from an area where they are more concentrated to an area where they are less concentrated
Pauli exclusion principle
Diffusion
Dipole
solvation
28. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Group 6A
Nonpolar covalent bond
Diffusion
Triple point
29. 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
s orbital
amorphous solid
effective nuclear charge
Graham's Law
30. 1913 - Niels Bohr - said that electrons formed specific layers instead or random ones - said atoms atoms absorb and give off energy when the electrons move from one shell to another
The bohr model
Decomposition reaction
ionic cmpound
Atomic absorption Spectra
31. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
und's rule
Octet Rule
Pauli exclusion principle
mole
32. A structural formula in which electrons are represented by dots; dot pairs or dashes between two atomic symbols represent pairs in covalent bonds.
Rydberg constant
Emperical Formula
Bronsted - Lowry definition
Lewis structure
33. The amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Chemical Kinetics
pH
subshell
Activation energy
34. In a solution - the substance that dissolves in the solvent
molecule
Solute
Normality
Colligative properties
35. When polar molecules orient themselves such that the positive region of one molecule is close to the negative region of another molecule.
Group 2A
und's rule
Charles and Gay Lussac's Law
Dipole Dipole interaction
36. The average distance between the nuclei of two bonded atoms
bond length
Common ion effect
Raoult's Law
Ion product
37. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Effusion
single displacement reaction
decomposition reaction
Electrolyte
38. 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
Group 4A
Lyman series
Molality
39. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
molecule
Rydberg constant
Combination Reaction
indicator
40. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Strong acid
Lewis structure
periodic trends
Ion
41. 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
Chemical Kinetics
azimuthal quantum number
Magnetic quantum number
theoretical yield
42. (chemistry) the sum of the relative atomic masses of the constituent atoms of a molecule
Group 2A
crystalline solid
pH
molecular weight
43. The reaction of the ions that characterize acids and the ions that characterize bases to form water molecules and a salt
Henderson Hasselbalch Equation
Neutralization reaction
effective nuclear charge
electron configuration
44. 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
empirical formula
bond energy
Percent yield
Effusion
45. Where half of the acid is neutralized by the base on a titration curveAn acid dissociation constant - Ka - (also known as acidity constant - or acid - ionization constant) is a quantitative measure of the strength of an acid in solution. It is the eq
Principle quantum number
pI
ionic cmpound
Half equivalence point
46. The process of decomposing a chemical compound by the passage of an electric current.
electrolysis
Triple point
Normality
Molality
47. The process by which one or more substances change to produce one or more different substances
s orbital
chemical reaction
Avagadros number
Disproportionation
48. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
Principle quantum number
heisenberg uncertainty principle
lewis base
hydrogen bonding
49. 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
Reaction mechanism
STP
Solution equilibrium
Spin quantum number
50. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
physical reaction
Henry's Law
pi bonds
Arrhenius Definition
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