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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. Numbers that specify the properties of atomic orbitals and of their electrons
representative elements
Electrolyte
d orbital
quantum numbers
2. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
Dipole
Formula weight
Balmer series
Decomposition reaction
3. 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
Dipole
Lewis acid base reaction
azimuthal quantum number
actinide series
4. 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
electromagnetic energy of photons emmited from electrons at ground state
Proton
indicator
und's rule
5. 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
Collision theory of chemical Kinetics
Dispersion Forces
crystalline solid
Equivalence point
6. 2.18 x 10^-18 J/electron
Conjugate acids and Bases
Phase diagram
electrolysis
Rydberg constant
7. 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.
Period
Half equivalence point
Solubility Product Constant
Diprotic Base
8. The energy required to break a chemical bond and form neutral isolated atoms
Formal Charge
bond energy
London forces
Le chateliers Principle
9. 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.
Effective nuclear charge
Solution equilibrium
Redox Half Reaction
molecular weight
10. Alkaline Earth Metals - 2 valence electrons +2 ions - Magnesium Mg
quantum
Molarity
Group 2A
Half equivalence point
11. 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
Equlibrium constant
Molality
crystalline solid
Emperical Formula
12. Atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas - usually eight valence electrons
Vapor pressure
Electrolyte
Atomic absorption Spectra
Octet Rule
13. Sum of the protons and neutrons in an element often denoted by the letter A
d orbital
Molecular orbital
representative elements
Mass number
14. A reaction in which two or more substances combine to form a single substance A+B>>>>>>>C
Group 1A
Neutron
Lyman series
Combination Reaction
15. A representation of a displacement reaction showing only the reactive species and omitting the spectator ions.
Net ionic equation
redox reaction
Lewis structure
pI
16. 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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17. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
empirical formula
Collision theory of chemical Kinetics
Rydberg constant
18. A bond formed when two atomic orbitals combine to form a molecular orbital that is symmetrical around the axis connecting the two atomic nuclei
molecular weight
sigma bond
Normality
Network covalent
19. A set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors
Emperical Formula
quanta
Triple point
atomic emission spectrum
20. A reaction where a compound does Not change its molecular structure.
Common ion effect
Electronegativity
heisenberg uncertainty principle
physical reaction
21. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
quantum numbers
Proton
Pauli exclusion principle
Neutralization reaction
22. The area of chemistry that is concerned with reaction rates and reaction mechanisms
Principle quantum number
Chemical Kinetics
Group 2A
Lewis acid base reaction
23. (chemistry) p(otential of) H(ydrogen)
Effective nuclear charge
pH
atomic emission spectrum
Solubility Product Constant
24. A covalent bond in which the bonding electrons are shared equally by the bonded atoms - resulting in a balanced distribution of electrical charge
Nonpolar covalent bond
Reaction order
Rate determining step
Formula weight
25. A subdivision of an energy level in an atom. They are divided into orbitals.
Concentration
Common ion effect
representative elements
subshell
26. PH=pka+log[base/acid] Used in titration based problems that relates the pH or pOH of a solution to the pK and the ratio of the dissociated species.
Henderson Hasselbalch Equation
Chemical Kinetics
Emperical Formula
electrolysis
27. A substance that - when dissolved in water - results in a solution that can conduct electricity
molecular weight
Electrolyte
angular momentum in the bohr model
representative elements
28. 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
Combination Reaction
heisenberg uncertainty principle
Magnetic quantum number
periodic trends
29. PH of a molecule at which it contains no net electric charge - isoelectric point.
Neutralization reaction
Avagadros number
Intermolecular forces
pI
30. 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
Atomic weight
Formal Charge
s orbital
Vapor pressure
31. 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
electron affinity
atomic theory
Noble gases
s orbital
32. The average distance between the nuclei of two bonded atoms
bond length
Percent composition
gram equivalent weight
sigma bond
33. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
Alkaline earths
Magnetic quantum number
Common ion effect
34. The process of decomposing a chemical compound by the passage of an electric current.
electromagnetic energy of photons emmited from electrons at ground state
theoretical yield
electrolysis
Half equivalence point
35. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Nucleus
Common ion effect
Free radical
Reaction order
36. Rare earth element group (elements 58-71)
STP
Dipole Dipole interaction
electron configuration
lathanide series
37. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Rydberg constant
decomposition reaction
Ionization energy
Lewis acid base reaction
38. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
molecule
Group 3A
quantum
Group 7A
39. A chemical bond that involves sharing a pair of electrons between atoms in a molecule
decomposition reaction
und's rule
Diffusion
Covalent Bond
40. 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.
Buffer
lewis base
Atomic absorption Spectra
electromagnetic energy of photons emmited from electrons at ground state
41. 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
sigma bond
physical reaction
Formal Charge
Half equivalence point
42. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Pauli exclusion principle
Group 4A
Effusion
subshell
43. An emperimentally determined mathmatical expression showing the rate of a reaction as a function of the concentration of its reactants
Collision theory of chemical Kinetics
Rate law
Amphoteric
Planck's Constant
44. A base that can accept two moles of H+ per mole of itself (ex: SO4
Diprotic Base
Henry's Law
London forces
Dispersion Forces
45. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Reaction mechanism
Ionization energy
Vapor pressure
Intermolecular forces
46. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance C>>>>A+B
Effusion
Decomposition reaction
azimuthal quantum number
Free radical
47. The ways in which electrons are arranged in various orbitals around the nuclei of atoms
VSEPR
electron configuration
atomic radius
lewis base
48. Two or more atoms held together by covalent bonds
molecule
Halogens
Concentration
Rate law
49. A model of acids and bases which an acid is hydrogen ion donor and base is a hydrogen ion acceptor.
lewis base
Bronsted Lowry
Disproportionation
London forces
50. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
mole
Resonance structure
bond energy
electromagnetic energy of photons emmited from electrons at ground state