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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 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
Ion
redox reaction
Hydrogen bonding
Equivalence point
2. 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
Buffer
Group 3A
Ion product
3. One - half the distance between the nuclei of two atoms of the same element when the atoms are joined
quantum
s orbital
angular momentum in the bohr model
atomic radius
4. 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
redox reaction
Effusion
Ionic Bond
Group 5A
5. A concentration unit of a solution expressed as moles of solute dissolved per liter of solution
Molarity
Resonance structure
Electrolyte
Dipole
6. No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers
Buffer
Rydberg constant
Pauli exclusion principle
Atomic absorption Spectra
7. 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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8. An ionic compound that resists changes in its pH
Concentration
Rate law
Buffer
Titration
9. 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.
Atomic weight
Bronsted Lowry
Intermolecular forces
VSEPR
10. 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
Proton
Nucleus
empirical formula
The bohr model
11. Play- by- play showing the individual steps of a reaction - including the formation and destruction of any reaction intermediates that may occur.
Reaction mechanism
Raoult's Law
Electrolyte
Equilibrium
12. (chemistry) any theory in which all matter is composed of tiny discrete finite indivisible indestructible particles
atomic theory
Theoretical yield
redox reaction
Triple point
13. (chemistry) a substance that changes color to indicate the presence of some ion or substance
Lewis acid base reaction
indicator
Ionization energy
Concentration
14. Substance in which a solute is dissolved to form a solution
Diprotic Base
d orbital
Solvent
Dispersion Forces
15. 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
law of constant composition
hydrogen bonding
Dispersion Forces
Ionization energy
16. Systematic pairing of a deprotonated species (base) with its protonated form (conjugate acid). Conjugates appear on opposite sides of a chemical equation.
Conjugate acids and Bases
Solubility Product Constant
redox reaction
decomposition reaction
17. (chemistry) a substance formed by chemical union of two or more elements or ingredients in definite proportion by weight
atomic theory
Half equivalence point
compound
Charles and Gay Lussac's Law
18. 5 different orbitals shaped like clover leaves and max electrons is 10
Colligative properties
Lewis acid base reaction
d orbital
Rate determining step
19. When dipoles are dissolved in a solution where ions are present ions wil arrange themselves with the opposite charged end of the dipole.
s orbital
Ion dipole interactions
Avagadros number
Collision theory of chemical Kinetics
20. 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.
Diffusion
Colligative properties
Balmer series
Period
21. (chemistry) a series from actinium to lawrencium of 15 radioactive elements with increasing atomic numbers
actinide series
Chemical Kinetics
Nucleus
theoretical yield
22. Gram equivalent weight of solute per liter of solution - often denoted by N.
Normality
Molar solubility
Atomic absorption Spectra
Proton
23. The molar amount of a solute that can dissolve in 1L of solvent until equilibrium - saturation - is reached
atomic radius
Acid dissociation constant
Molar solubility
redox reaction
24. An acid that will completely dissociate in aqueous solution - like HCl - HI - HClO4 HBr.
Common ion effect
Ion product
Strong acid
Group 1A
25. Set of spectral lines appearing in the UV region when a hydrogen atom undergoes a transition from energy levels n>1 to n=1.
Halogens
Lyman series
Henderson Hasselbalch Equation
Octet Rule
26. 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.
Covalent Bond
crystalline solid
Noble gases
electron affinity
27. A pair of equal and opposite electric charges or magnetic poles separated by a small distance
atomic emission spectrum
Dipole
compound
indicator
28. The process by which one or more substances change to produce one or more different substances
Henderson Hasselbalch Equation
Molecular orbital
chemical reaction
single displacement reaction
29. Two or more atoms held together by covalent bonds
Strong acid
molecule
Solubility Product Constant
Formal Charge
30. A naturally occurring or synthetic compound consisting of large molecules made up of a linked series of repeated simple monomers
Octet Rule
polymer
decomposition reaction
d orbital
31. A graph of pressure versus temperature that shows the conditions under which the phases of a substance exist
decomposition reaction
pi bonds
d orbital
Phase diagram
32. A chemical reaction involving the transfer of one or more electrons from one reactant to another; also called oxidation - reduction reaction.
Half equivalence point
Arrhenius Definition
Intermolecular forces
redox reaction
33. Slightly less reactive than alkali metals - comprise group II
Alkaline earths
Reaction order
Group 6A
Solvent
34. Attractive and repulsive forces between molecules that are weaker than forces within molecules.
Intermolecular forces
gram equivalent weight
angular momentum in the bohr model
Rate determining step
35. Alkali metals: highly reactive - therefore always compounds. - 1 valence electron +1 ion - Hydrogen H? - Lithium Li? - Sodium Na? - Potassium K? - Rubidium Rb? - Cesium Cs?
Planck's Constant
Spin quantum number
Group 1A
Bronsted Lowry
36. 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.
Arrhenius Definition
Formal Charge
Solubility Product Constant
atomic radius
37. 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
Group 3A
Acid dissociation constant
polymer
Arrhenius Definition
38. Nh/2p The angular momentum changes only in discete amounts with respect to the quantum number. Also E=- R_h/n^2
angular momentum in the bohr model
Strong acid
Solution equilibrium
Ionic Bond
39. The ratio of the number of moles of solute dissolved in one kilogram of solvent. molality (M = moles solute/kg of solution)
Atomic absorption Spectra
sigma bond
Acid dissociation constant
Molality
40. Simplest whole # ration of atoms in a compound
Emperical Formula
Diprotic Base
Common ion effect
Neutron
41. 5 valence electrons -3 ions - Nitride N
Graham's Law
Raoult's Law
Intermolecular forces
Group 5A
42. 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
Molality
Spin quantum number
azimuthal quantum number
polymer
43. An atom - ion - or molecule that donates an electron pair to form a covalent bond.
lewis base
physical reaction
Equlibrium constant
Percent composition
44. The maximum amount of product that can be produced from a given amount of reactant
hydrogen bonding
Magnetic quantum number
theoretical yield
Reaction order
45. 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
Solution equilibrium
Reaction order
Colligative properties
empirical formula
46. 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
Planck's Constant
Formal Charge
Combination Reaction
Lyman series
47. Tells you how much solute is present compared to the amount of solvent
Reaction order
Concentration
Solution equilibrium
pH
48. 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
molecule
Ion
Spin quantum number
Formal Charge
49. Property of the elements that can be predicted from the arrangement of the periodic table
atomic emission spectrum
Free radical
Chemical Kinetics
periodic trends
50. Sum of all the masses - in AMU - present in one molecule of a molecular compound.
Neutralization reaction
Hydrogen bonding
Formula weight
single displacement reaction