Chemistry Fall and Winter – Flashcards
Unlock all answers in this set
Unlock answers| Anion |
| negatively charged ion |
| Cation |
| positively charged ion |
| Isoelectronic Ions |
| Have the same number of electrons (Ne and F-) |
| Electron Affinity |
| The energy involved in adding an e- to the atom |
| Ionic Compounds |
| Provide a conductory solution when dissolved in water |
| Molecular Compounds |
| When dissolved in water, the solution does not conduct. |
| Atomic Size |
| amount of space that e- take up |
| Anion Size |
| Always larger than its neutral atom because it has a lesser ENC due to the extra e- |
| Cation Size |
| Smaller than its neutral atom because it has a greater ENC due to the lost e- |
| Ionization Energy |
| The amount of energy required to remove an e- from an atom |
| Negative Electron Affinity |
| The atom releases energy to the atmosphere |
| Positive Electron Affinity |
| The atom requires an imput of energy in order for the atom to accept e- |
| Electronegativity |
attraction for the e- in a shared bond
"greediness" factor |
| Ionic Compounds |
Held together by ionic bonds
made of an anion and a cation, usually metal and non-metal
|
| Octet Rule |
| Atoms tend to gain, lose, or share electrons in order to achieve an octet |
| Charges of Transition Metals |
| Many transition metals have more than one possible charge, such as Iron (II) and Iron (III) or Copper (I) and Copper (II) |
| Sulfate |
| SO42- |
| Ammonium |
| NH4+ |
| Acetate |
| C2H3O2- |
| Carbonate |
| CO32- |
| Hydroxide |
| OH- |
| Nitrate |
| NO3- |
| Phosphate |
PO43- |
| Molecular Compounds |
Covalently bonded compounds
"molecule" - no net charge
usually between two non-metals |
| Non-polar bonds |
Covalent
Fairly equal sharing of e-
Difference is ≤ 0.4 |
| Polar Covalent Bonds |
Unequal sharing of e-
0.4 ≤ ∆ ≤ 2.0 |
| Ionic Compounds |
Cation : Anion
Metal : Non-metal |
| Prefixes Denoting Count |
Used in covalent bonds forming molecules between two non-metals
Mono- = 1, di- = 2, tri- = 3, etc.
H2S = dihydrogen monosulfide |
| Valence e- |
The outermost e- occupying the s + p orbitals
up two eight valence e- are possible
exceptions: H and He ~ have no p orbitals |
| Lewis Dot Structure |
| Shows the number of valence e- |
| Ethanol |
| C2H5OH |
| Chemical Reactions |
| Compounds and elements coming together and breaking apart |
| Chemical Equation |
| Describes chemical reactions using elemental symbols and phase subscripts |
| (l) |
| Phase subscript for liquid |
| (s) |
| Phase Subscript for solids |
| (g) |
| Phase subscript for gas |
| (aq) |
| Phase subscript for aqueous |
| Aqueous |
| Dissolved in water |
| Signs of a Reaction |
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.; |
| Exothermic Reaction |
Energy leaves the system ; reactants --> products + E(heat) |
| Endothermic |
Energy enters the system
E(heat) + reactants --> products |
| Law of Conservation of Mass |
In a chemical reaction, mass is neither created nor destroyed.
Mass of Reactant = Mass of Product |
| Synthesis (direct combination) Reaction |
| Two or more elements or simple compounds combine to form a single, more complex compound. |
| Decomposistion Reactions |
A single compound breaks down into elements or simpler compounds
Heat or some form of energy is often needed to make these happen |
| Combustion Reaction |
| When a substance reacts with O2 |
| Dissociation Reactions |
Breaking up pf a soluable ionic compound in water into its ionic parts
Ionic parts always exist in "aqueous" phase |
| Single Replacement Reactions |
| A more active metal replaces a less active metal in a compound, or a more active halogen replaces a less active halogen |
| Double Replacement Reaction |
Two ionic compounds exchange ions.
Both must be soluble originally and at least one new compound form/precipitate |
| Soluable |
| Dissolves in water to form an aqueous solution |
| Insoluable |
| Doesn;t dissolve in water, stays together as a compound |
| Mole |
Chemist's count
Used when referring to objects, like atoms, molecules, and formula units
6.02 • 1023 |
| Molarity, M |
Moles of solute Liters of Solution Describes Concentration
|
| Percent by Mass |
| mass of part / mass of whole • 100 |
| Theoretical Yield |
| The amount of product that is expected based on stoichiometric principles |
| Heat |
| Energy that is transferedfrom one object to abother due to temperature difference |
| Energy |
"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) |
| Temperature |
| Average KE of the particles in a sample |
| Exothermic Reactions |
| Release energy to their surroundings |
| Endothermic Reactions |
| Absorb energy from surroundings, which is usually stored in new bonds |
| ∆H, Enthalpy |
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 |
