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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 amount of energy that reactants must absorb before a chemical reaction will start; also called free energy of activation.
Amphoteric
polymer
Activation energy
Ion
2. Redox reaction - in which the same species is both oxidized and reduced.
Proton
Equivalence point
energy state
Disproportionation
3. Side - to side parallel orbitals overlap to share electrons - the 2nd/3rd covalent bond between two atoms - cannot rotate and maintain the bond.
pi bonds
Proton
Amphoteric
Octet Rule
4. 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
Charles and Gay Lussac's Law
quantum
single displacement reaction
5. 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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6. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
Noble gases
Molarity
Buffer
compound
7. The molar solubility of one salt is reduced when another salt - having a common ion is brought into the same solution
Common ion effect
azimuthal quantum number
Principle quantum number
subshell
8. An atom - radical - or molecule that has gained or lost one or more electrons and has a negative or positive charge
London forces
Atomic absorption Spectra
Network covalent
Ion
9. The amount of product that can be made in a chemical reaction based on the amount of limiting reactant
Theoretical yield
transition elements
Molality
Lewis acid base reaction
10. The process by which a gas escapes from one container to another at lower pressure through a tiny hole in the container.
Phase diagram
Mass number
Effusion
Molar solubility
11. Standard Temperature and Pressure. 273 Kelvin (0 Celsius) - 1 atmosphere (760 torr - 760 kPA).
pi bonds
Ion
Conjugate acids and Bases
STP
12. (physics) the smallest discrete quantity of some physical property that a system can possess (according to quantum theory) E=hf
Rydberg constant
polymer
Net ionic equation
quantum
13. A solid made up of particles that are not arranged in a regular pattern.
amorphous solid
Solution equilibrium
Lewis structure
chemical reaction
14. (chemistry) separation of a substance into two or more substances that may differ from each other and from the original substance
Normality
electron configuration
pi bonds
decomposition reaction
15. 2.18 x 10^-18 J/electron
Rate determining step
Solubility Product Constant
Concentration
Rydberg constant
16. The amount of a substance that contains as many particles as there are atoms in exactly 12g of carbon -12
Group 3A
mole
Water dissociation Constant
lathanide series
17. The maximum amount of product that can be produced from a given amount of reactant
theoretical yield
Proton
Colligative properties
Ion
18. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
Equlibrium constant
Phase diagram
heisenberg uncertainty principle
Dipole
19. Two or more atoms held together by covalent bonds
molecule
Nucleus
amorphous solid
Strong acid
20. The sum of the exponents in a rate law - where each exponent provides the reaction order with respect to its reactants
Lewis structure
Reaction order
Bronsted Lowry
law of constant composition
21. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Proton
Molarity
subshell
Formula weight
22. 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
Group 3A
azimuthal quantum number
Solubility Product Constant
Percent composition
23. Substance in which a solute is dissolved to form a solution
Percent yield
Bronsted - Lowry definition
Concentration
Solvent
24. The number of atoms in exactly 12 g of pure 12c and equal to 6.022 x 10^23 is called
molecular weight
Strong acid
Reaction order
Avagadros number
25. 5 valence electrons -3 ions - Nitride N
Reaction order
Lyman series
Equilibrium
Group 5A
26. 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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27. The process of decomposing a chemical compound by the passage of an electric current.
London forces
Acid dissociation constant
electrolysis
Group 6A
28. 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
heisenberg uncertainty principle
Molecular orbital
Ionic Bond
Reaction order
29. 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
amorphous solid
Collision theory of chemical Kinetics
Diffusion
30. E=hc/?
atomic emission spectrum
electromagnetic energy of photons emmited from electrons at ground state
Triple point
Lewis structure
31. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
actinide series
Henry's Law
transition elements
32. The weight in grams of compound that can be substituted by 1 atom of Hydrogen. GEW = MW / # of acidic Hyrdogens
Combination Reaction
Electronegativity
single displacement reaction
gram equivalent weight
33. Tells you how much solute is present compared to the amount of solvent
Concentration
Decomposition reaction
Aqueous Solution
Dipole Dipole interaction
34. 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
Dispersion Forces
Intermolecular forces
polymer
35. At a constant pressure - the volume of an ideal gas is directly proportinal to its temperature: V (a) T
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36. 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
Titration
Acid dissociation constant
Neutralization reaction
lewis base
37. 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.
Network covalent
Atomic absorption Spectra
Nonpolar covalent bond
Redox Half Reaction
38. 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.
Avagadros number
Redox Half Reaction
Dipole
Azeotrope
39. 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
Azeotrope
Half equivalence point
Ionization energy
Ground state
40. 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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41. A physical property of a solution that depends on the number - but not the identity - of the disswolved solute particles; example properties include vapor pressure lowering - boiling point elevation - osmotic pressure - and frezzing point depression
energy state
ionic cmpound
Colligative properties
Arrhenius Definition
42. The slowest elementary step which is the limit for the rate of the other steps
azimuthal quantum number
Nonpolar covalent bond
Rate determining step
quantum numbers
43. Region in a molecule where atomic orbitals overlap - resulting in either a stable low - energy bonding orbital or an unstable high - energy antibonding orbital.
Collision theory of chemical Kinetics
Molarity
Molecular orbital
The bohr model
44. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Phase diagram
Molality
Solute
molecule
45. Solids in which the particles are arranged in a repeating - 3- D pattern - has a specific melting point - classified as ionic network covalent - metallic or molecular.
Le chateliers Principle
empirical formula
Nucleus
crystalline solid
46. 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
Henry's Law
Arrhenius Definition
Effusion
Bronsted Lowry
47. Large molecular structures - strong covalent bonding - share qualities of IONIC And COVALENT
electromagnetic energy of photons emmited from electrons at ground state
Molarity
Network covalent
compound
48. Property of the elements that can be predicted from the arrangement of the periodic table
Nonpolar covalent bond
periodic trends
London forces
Molar solubility
49. 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
Graham's Law
Magnetic quantum number
Dipole
Formal Charge
50. 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.
pI
Conjugate acids and Bases
VSEPR
heisenberg uncertainty principle
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