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| Have the same number of electrons (Ne and F-) |
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| The energy involved in adding an e- to the atom |
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| Provide a conductory solution when dissolved in water |
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| When dissolved in water, the solution does not conduct. |
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| amount of space that e- take up |
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| Always larger than its neutral atom because it has a lesser ENC due to the extra e- |
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| Smaller than its neutral atom because it has a greater ENC due to the lost e- |
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| The amount of energy required to remove an e- from an atom |
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Negative Electron Affinity
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| The atom releases energy to the atmosphere |
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Positive Electron Affinity
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| The atom requires an imput of energy in order for the atom to accept e- |
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attraction for the e- in a shared bond "greediness" factor |
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Held together by ionic bonds made of an anion and a cation, usually metal and non-metal |
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Atoms tend to gain, lose, or share electrons in order to achieve an octet
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Charges of Transition Metals
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Many transition metals have more than one possible charge, such as Iron (II) and Iron (III) or Copper (I) and Copper (II)
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Covalently bonded compounds "molecule" - no net charge usually between two non-metals
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Covalent Fairly equal sharing of e- Difference is ≤ 0.4
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Unequal sharing of e- 0.4 ≤ ∆ ≤ 2.0 |
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Cation : Anion Metal : Non-metal |
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Used in covalent bonds forming molecules between two non-metals Mono- = 1, di- = 2, tri- = 3, etc. H2S = dihydrogen monosulfide |
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The outermost e- occupying the s + p orbitals up two eight valence e- are possible exceptions: H and He ~ have no p orbitals |
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Shows the number of valence e-
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Compounds and elements coming together and breaking apart
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Describes chemical reactions using elemental symbols and phase subscripts
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| Phase subscript for liquid |
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Phase Subscript for solids
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| Phase subscript for aqueous |
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1. Change of state (production of a gas or solid) 2. Color Change 3. Temperature (E) change *Light may be produced, but it isn't common. |
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Energy leaves the system reactants --> products + E(heat) |
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Energy enters the system E(heat) + reactants --> products |
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Law of Conservation of Mass
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In a chemical reaction, mass is neither created nor destroyed. Mass of Reactant = Mass of Product |
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Synthesis (direct combination) Reaction
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| Two or more elements or simple compounds combine to form a single, more complex compound. |
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A single compound breaks down into elements or simpler compounds Heat or some form of energy is often needed to make these happen |
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When a substance reacts with O2
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Breaking up pf a soluable ionic compound in water into its ionic parts Ionic parts always exist in "aqueous" phase |
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Single Replacement Reactions
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A more active metal replaces a less active metal in a compound, or a more active halogen replaces a less active halogen
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Double Replacement Reaction
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Two ionic compounds exchange ions. Both must be soluble originally and at least one new compound form/precipitate |
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| Dissolves in water to form an aqueous solution |
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Doesn;t dissolve in water, stays together as a compound
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Chemist's count Used when referring to objects, like atoms, molecules, and formula units 6.02 • 1023 |
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Moles of solute
Liters of Solution Describes Concentration
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| mass of part / mass of whole • 100 |
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The amount of product that is expected based on stoichiometric principles
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| Energy that is transferedfrom one object to abother due to temperature difference |
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"ability to do work" Main types are kenetic energy (KE - energy of motion) and potential energy (PE - stored energy in bonds and in the structure itself) |
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Average KE of the particles in a sample
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Release energy to their surroundings
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Absorb energy from surroundings, which is usually stored in new bonds
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Change in the energy of a system in terms of the KE and PE of the system's parts ∆H = Hf - Hi ∆H = Hproducts - Hreactants |
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