Exam 2 – Chemistry Flashcard
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| Substances which dissolve in water to produce conduction solutions of ions |
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| Electrolytes |
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| Molecular covalent compounds and non-electrolytes are |
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| Mostly neutral in water |
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| Substances which do not produce ions in aqueous solutions |
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| Non-electrolytes |
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| Compounds that dissociate to a large extent into ions when dissolved in water |
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| Strong electrolytes |
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| Compounds that dissociate to a small extent into ions when dissolved in water |
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| Weak electrolytes |
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| All substance in the chemical equation are written using their complete formulas as if they were molecules |
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| Molecular equation |
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| All of the strong electrolytes are written as ions |
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| Ionic equation |
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| The ionic equation is reduced to the ______ by removing the spectator ions which appear on each side |
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| Net ionic equation |
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| Ions that undergo no change during the reaction and appear on both sides of the reaction arrow |
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| Spectator ions |
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| A substance that dissociates in water to produce hydrogen ions, H+1 |
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| Acid |
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| A substance that dissociates in water to produce hydroxide ions, OH-1 |
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| Base |
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| Strong acids and strong bases are _______ electrolytes |
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| Strong |
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| Weak acids and weak bases are _______ |
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| electrolytes |
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| Acids (H+) and bases (OH-) react to produced a |
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| Neutral water and a salt |
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| Double-replacement reactions just like the precipitation reactions |
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| Acid-base neutralization reactions |
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| Neutralization reactions are |
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| Ionic |
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| A value which indicates whether an atom is neutral, electron-rich, or electron-poor |
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| Oxidation Number |
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| A monoatomic ion has an oxidation number _____ to its charge |
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| Identical |
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| An atom in a polyatomic ion or in a molecular compound usually has the _____ oxidation number it would have if it were a monoatomic ion |
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| Same |
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| Halogens usually have an oxidation number of |
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| -1 |
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| The sum of the oxidation numbers is ____ for a neutral compound and is _____ to the net charge for a polyatomic ion |
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| 0, equal |
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| Causes reduction, loses one or more electrons, undergoes oxidation, oxidation number of atom increases |
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| Reducing agent |
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| causes oxidation, gains one or more electrons, undergoes reduction, oxidation number of atom decreases |
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| Oxidizing agent |
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| The periodic table is organized into groups and families because of the organization of _____ in atoms |
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| Electrons |
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| Atomic size ________ across a period and ______ down a group |
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| Decreases, increases |
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| A wave that is characterized by wavelength, frequency, and amplitude |
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| Electromagnetic energy |
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| Frequency and wavelength are ______ related since their product is a constant, the speed of light |
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| Inversely |
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| High energy electromagnetic radiation has _____ frequency and ______ wavelength |
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| High, short |
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| Einstein recognized the threshold energy (energy required)as the quanta needed to release and electron from _______ |
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| A nucleus |
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| It is impossible to know precisely where an electron is and what path it follows |
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| Heisenberg uncertainty principle |
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| Describes the size and energy level of the orbital, Commonly called the shell, positive integer (n = 1, 2, 3, 4, ...), as the value increases: the energy increases and the average distance of the electron from the nucleus increases |
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| Principal quantum number (n) |
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| Defines the three-dimensional shaped of the orbital, commonly called the subshell |
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| Angular-momentum quantum number (l) |
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| Defines the spatial orientation of the orbital, there are 2l + 1 values of ___, and they can have any integral value from -l to +l |
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| Magnetic quantum number (ml) |
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| Spherical about the nucleus and increase in size with increasing nodes (area of zero probability (wave behavior)) |
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| S orbitals |
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| Dumbbell shapes about 1 axis. The x-axis represents l = -1 , the y-axis for l = 0 and z-axis for l = +1 |
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| P orbital |
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| The nuclear charge actually felt by an electron |
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| Effective nuclear charge (Zeff) |
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| A description of which orbitals are occupied by electrons |
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| Electron configuration |
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| Orbitals that have the same energy level. For examples, the three p orbitals in a given subshell |
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| Degenerate orbitals |
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| The lowest-energy configuration |
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| Ground-state electron configuration |
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| A guide for determining the filling order of orbitals |
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| Aufbau principle |
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| Lower-energy orbitals fill before higher-energy orbitals; and orbital can only hold two electrons, which must have opposite signs; if two or more degenerate orbitals are available, follow Hund's rule |
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| Rules of the aufbau principles |
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| If two or more orbitals with the same energy are available, one electron goes into each until all are half-full. The electrons in the half-filled orbitals all have the same spin |
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| Hund's rule |
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| The group 1A atoms are largest in a period because of the ____ effective nuclear charge |
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| Low |
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| Halogens are smallest in a period because of their ______ effective nuclear charge |
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| High |
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| The main group non-metals _____ electrons to reach nearest noble gas electron configurations |
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| Gain |
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| The main group metals ____ electrons to reach the nearest noble gas electron configuration |
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| Lose |
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| Because metals lose electrons, the ions are ______ than the element, the degree of change depends on the number of electrons lost |
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| Smaller |
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| A gain of electrons by non-metals decreases the effective nuclear charge, so the anions are _____ than the element |
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| Larger |
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| The amount of energy necessary to remove the highest-energy electron from an isolated neutral atom in the gaseous state |
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| Ionization energy (Ei) |
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| Ionization energy _______ with a low effective nuclear charge and large size |
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| Decreases |
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| Noble gases have the ______ ionization energy and order _____ from Li>Ba>K>Rb, etc. |
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| Highest |
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| 1A metals have the ______ ionization energy |
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| Lowest |
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| The energy released when a neutral atom gains an electron to form an anion |
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| Electron affinity |
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| The amount of energy that must be supplied to break up an ionic solid into individual gaseous ions. Determines solubility. |
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| Lattice energy (U) |
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| Main-group elements tend to undergo reactions that leave them with eight outer-shell electrons |
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| Octet rule |
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| Metals tend to have _____ ionization energy and ____ electron affinity. they tend to lose one or more electrons. |
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| Low, low |
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| Non-metals tend to have ____ ionization energy and ____ electron affinity. They tend to gain one or more electrons. |
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| High, high |
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| Transition metals, lanthanide metals, and actinide metals do not follow the |
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| Octet rule |
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| Powerful reducing agents, metallic, bright and silvery, malleable, good conductors of electricity, relatively soft, very reactive, and occur only in salts, ionization energy decreases down the group |
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| Group 1A elements: alkali metals |
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| Elements are made from the cations by _______ that uses electrical energy to supply electrons |
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| Electrolysis |
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| Powerful reducing agents, metallic, bright and silvery, relatively soft, not as reactive, occur only in salts, higher melting point and ionization energy |
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| Group 2A elements: Alkaline earth metals |
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| Metallic, bright and silvery, good conductors of electricity, reacts well with oxygen (forms an oxide coating), does not react well with water due to the oxide coating, found in many minerals |
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| Group 3A elements |
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| Powerful oxidizing agents, non-metals, exist as diatomics in elemental form, very reactive occur only in salts and minerals, low melting points, high electron affinity |
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| Group 7A: Halogens |
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| Colorless and odorless, non-metals, very unreactive, occur naturally as atomic gases |
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| Group 8A: Noble gases |
