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KOH

KOH. AlPO 4. NH 4 C 2 H 3 O 2. Fe 2 (SO 3 ) 3. Cu 3 P. Mg(MnO 4 ) 2. LiF. Cu 3 P 2. CrO. CsNO 3. NH 4 Br. Co 2 (CrO 4 ) 3. NiCl 3. (NH 4 ) 2 SO 4. V 2 S 5. Ammonium Acetate. Aluminum Phosphate. Potassium Hydroxide. Magnesium Permanganate. Copper (I) Phosphide.

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KOH

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  1. KOH AlPO4 NH4C2H3O2 Fe2(SO3)3 Cu3P Mg(MnO4)2 LiF Cu3P2 CrO CsNO3 NH4Br Co2(CrO4)3 NiCl3 (NH4)2SO4 V2S5

  2. Ammonium Acetate Aluminum Phosphate Potassium Hydroxide Magnesium Permanganate Copper (I) Phosphide Iron (III) Sulfite Chromium (II) Oxide Copper (II) Phosphide Lithium Fluoride Cobalt (III) Chromate Ammonium Bromide Cesium Nitrate Vanadium (V) Sulfide Ammonium Sulfate Nickel (III) Chloride

  3. WI3 FrHSO4 Zn(C2H3O2)2 LiCN RbHCO3 Cu(MnO4)2 Ti(ClO4)2 Sr(NO2)2 Ba(NO3)2 PbC2O4 NaSCN Ag2Se Pb(C2O4)2 Mo2O3 AuF3

  4. Zinc Acetate Francium Hydrogen Sulfate Tungsten (III) Iodide Copper (II) Permanganate Rubidium Hydrogen Carbonate Lithium Cyanide Barium Nitrite Strontium Nitrite Titanium (II) Perchlorate Silver Selenide Sodium Thiocyanate Lead (II) Oxalate Gold (III) Fluoride Molybdenum (III) Oxide Lead (IV) Oxalate

  5. SeCl6 SiO2 NO SeO2 XeF6 N2O CO XeCl4 N4O3 OF2 XeBr2 P2O5 S5O8 IF4 BF3

  6. Nitrogen Monoxide Silicon Dioxide Selenium Hexachloride Dinitrogen Monoxide Xenon Hexafluoride Selenium Dioxide Tetranitrogen Trioxide Xenon Tetrachloride Carbon Monoxide Diphosphorus Pentoxide Xenon Dibromide Oxygen Difluoride Boron Trifluoride Iodine Tetrafluoride Pentasulfur Octoxide

  7. NF3 N2F4 P4O10 B2O3 CO2 SiCl4 SF6 PF5 TeO PI3 S3N2 P3S9 XeO3 NH3 SO

  8. Tetraphosphorus Decoxide Dinitrogen Tetrafluoride Nitrogen Trifluoride Silicon Tetrachloride Carbon Dioxide Diboron Trioxide Tellurium Monoxide Phosphorus Pentafluoride Sulfur Hexafluoride Triphosphorus Nonasulfide Trisulfur Dinitride Phosphorus Triiodide Sulfur Monoxide Nitrogen Trihydride Xenon Trioxide

  9. Ion Reactants Ionic Liquid Products Covalent Aqueous Precipitate Coefficient Binary Compound Octet Rule Subscript Formula Unit Law of Conservation of Matter Chemical Symbol

  10. Ions bonded together, usually a M + NM The atoms and/or compounds that start a chemical reactions An element that has either lost or gained electrons All Nonmetals bonded together. The atoms and/or compounds that are produced in a chemical reaction. A pure substance in rotational motion. Number placed in front of a compound to show how many there are total. A solid produced from 2 aqueous solutions. A salt dissolved in water, so it is a mixture. Number placed after a chemical symbol to show how many atoms of the specific element. All elements want 8 valence electrons. A compound made up of only 2 types of elements. 1 to 2 letter abbreviation to represent an element Matter can never be created nor destroyed. A list of elements in the compound using subscripts to show the least whole number ratio of atoms.

  11. Alkali Charge Nitrogen Family Charge Reason why Boron Family has a +3 charge. Alkaline Earth Charge Oxygen Family Charge Reason why Nitrogen Family has a -3 charge. Transition Metal Charge Halogen Charge Reason why Alkali Metals have a +1 charge. Boron Family Charge Noble Gas Charge Reason why Roman Numerals must be used for Transition Metals. Carbon Family Charge Reason Noble Gases don’t have a charge or make bonds (easily). Why are very small atoms often an exception to the octet rule?

  12. Easier to lose 3 electrons than gain 5 electron. -3 +1 Easier to take 3 electrons than give 5 electrons. -2 +2 Easier to give 1 electron, then gain 7 electrons. -1 Can change its charge based on what it is combined with in a given situation. Only way we can know how to write the formula because multiple charges are possible. 0 +3 Energy level 1 is complete and stable with only 2 valence electrons. Already have a stable octet +4

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