Naming Anions (know table 2.6 pg 55)Names and Formulas of Ionic CompoundsHydrated Ionic CompoundsCHEM 1465 1st Edition Lecture 3Chapter 2 – Atoms and Molecules (continued)Chemical Nomenclature In order to correctly name a compound, you must first determine if the compound is ionic or molecular. Molecular Compounds:2 nonmetal binary elements that form a covalent bond (use number prefixes)Ionic Compounds: one metal and one nonmetal binary compound that forms ionic bonds (don’t use prefixes)Important: Metals tend to lose electrons and become cations. Nonmetals tend to gain electrons and become anions. Naming Cations ( Know Table 2.5 pg 55) 1. Monatomic Cations from the Main Groups – the name is the same as the name of the element Na _Sodium___ Na+_Sodium____ Charge of Group 1 __+1___Ca _Calcium___ Ca2+_Calcium___ Charge of Group 2 _+2____ Al _Aluminum__ Al3+_Aluminum_ Charge of Aluminum __+3__In addition to Groups 1, 2, and Aluminum, you should know the charge of the silver ion and the zinc ion: Ag+ and Zn2+2. Some transition metals form more than one cation: Two ways to name: Fe2+_ferrous______ or _iron (II)____Fe3+_ferric_______ or _iron (III)____Cu+_cuprous_____ or _copper (I)___These notes represent a detailed interpretation of the professor’s lecture. GradeBuddy is best used as a supplement to your own notes, not as a substitute.Cu2+_cupric______ or _copper (II)___3. Know two polyatomic cations: Ammonium__NH4___ (easy to remember because the formula for ammonia is _NH3__) Hydronium_H3O + ___Naming Anions (know table 2.6 pg 55) 1. Monoatomic Anions – change the element ending to “-ide” Cl _chlorine____ Cl–_chloride____ Charge of Group 17 anions: _-1______ O _oxygen_____ O2–_oxide______ Charge of Group 16 anions: _-2_______N _nitrogen____ N3–_nitrite______ Charge of Group 15 anions: _-3_______2. two polyatomic anions ending in “-ide”: hydroxide __OH - ________ cyanide __CN - ________3. Eight important oxoanions: acetate C2H3O2- _or_CH3COO - _permanganate __MnO42- _____ carbonate __CO32- _________ phosphate __PO43- _______ chlorate __ClO3- _________ sulfate __SO42- _______nitrate __NO3- _________ chromate __CrO42- ______4. If you memorize nitrate and sulfate, then you also know nitrite and sulfite. (One less oxygen, but thesame charge.) sulfate __SO42- _________sulfite __SO32- _________nitrate __NO3- _________nitrite __NO2- _________5. If you memorize chlorate, then you know 12 polyatomic anions in all: ClO4–_perchlorate__ _BRO4______ _perbromate_ _IO4- _______ _periodate___ ClO3–_chlorate_____ _BRO3- ______ _bromate____ _IO3- _______ _iodate_____ClO2–_chlorite_____ _BRO2- ______ _bromite____ _IO2- ______ _iodite______ ClO–_hypochlorite__ _BRO - _______ _hypobromite_ _IO - _______ _hypoidite____Names and Formulas of Ionic Compounds Two important principles: 1. To name an ionic compound, name the _cation_ and then name the _anion_. Do not use _number prefixes__ such as _di, tri, tetra______. For example, MgCl2 is _magnesium chloride___ not __magnesium dichloride_____. 2. The overall formula for an ionic compound must be __electronicallyneutral______. That is, the number of positive charges __must equal_ the number of negative charges. Only use parentheses if you have _more than one___ of a __polyatomic ion___. Examples: Give the formulas of the following ionic compounds: magnesium chloride __MgCl2____ sodium nitrate __NaNO3____ iron(III) bromide __FeBr3_____ calcium hydroxide __Ca(OH)2____ magnesium sulfide __MgS______Hydrated Ionic Compounds Some ionic compounds, called __hydrates__, contain a specific number of __water molecules__associated with each __formula unit___. Know the common hydrate prefixes: # of water molecules prefix # of water molecules prefix ½ _hemi_____ 1 _mono_____ 5 _penta_____2 _di_______ 6 _hexa_____ 3 _tri_______ 7 _hepta_____4 _tetra_____ 8 _octa______CoCl2 · 6 H2O _cobalt (II) chloride hexahydrate__ BeCl2 · 2 H2O _beryllium chloride dihydrate___Cobalt (II) phosphate octahydrate _CO3(PO -1)_x_8H2O_ magnesium bromite hexahydrate __Mg(BRO2)2_x 6H2O_Chapter 3 – Molecules, Moles and Chemical EquationsChemical Equations: Reactants → products Na + H2O → H2 + NaOH +heat Physical states: have symbols to indicate physical states- Solid (s) - Liquid (l)- Gas (g)- Aqueous (aq)Nas + H2Ol → H2(g) + NaOHsBalancing Chemical EquationsThe Law of Conservation of Matter: matter is not created or destroyedIn practice: add or subtract atoms Nas + 2H2Ol → 2H2(g) + 2 NaOH Stoichiometry: the quantitative description of the proportions by moles of the substances in a chemical reactionStoichiometric coefficients: numbers used to balance an equation General rules for a chemist approach:1. Start with the most complex compound or molecule2. Save elements and simple molecules for last3. Clear any fractions (balanced equations have no fractions)Examples 1. C3H8 + 5O2 → 3CO2 + 4H2O2. Fe2O3 + 3 Cs → 2Fes + 3COgAqueous solutionHow are solutions made? Solute must dissolve in solvent- Solute: minor component- Solvent: major component- Water as a solvent: means an aqueous solution- Example: salt water where NaCl is a solute and H2O is the solvent (commonly called brine)The Mole and interpreting equations The Mole:“the SI unit for amount of substance; the quantity of a substance that contains the same number of entities as the number of atoms in exactly 12 g of carbon-12” 1. “Mole” is a __number__ word. 1 dozen eggs = 12 eggsA couple of tacos = 2 tacos1 gross of pencils = 144 pencils1 mol of particle = 6.022 X 1023 particles1 mol of atoms = 6.022 X 10 23 atoms1 mol of electrons = 6.022 X 1023 electrons1 mol of molecules = 6.022 X 1023 moleculesExample: How many moles of atoms are present in 9.5 x 1015 atoms? 9.5 x 1015 atoms (1 mol6.022 x1023¿= 1.6 x 10-8 molesExample: How many molecules are present in 2.35 mol of molecules? 2.35 mol (6.022 x10231 mol¿ = 1.42 x 1024