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Chemistry Elements, Compounds, subscript, superscript, coefficientPeriodic Table o o Periods, groups, etc.Metals o o Non-metalsMetalloids The patterns are related to the chemical properties of the element.Patterns in the periodic table describe how substance behave during a chemical reaction.Why do elements in the same group have similar chemical properties? What is it about metals and non-metals that allows you to predict the kinds ofcompounds they are likely to form? Electron Shells
Notice theKnowing the number of electrons helps you predict the formation of compounds, shells and valence electrons. name the compounds, and write their chemical formulas.A chemical bond forms between two atoms when electrons in the outer shell of each atom from a stable arrangement together.Outer shell is called the valence shell , the electrons in the outer shell are the ^ valence Chemical properties are related to the energy changes that take place when their^ electrons. atoms lose, gain, or share electrons to obtain a filled valence shell.Elements that easily gain or lose electrons are very reactive.
Cations: o Energy is added to the atom, which then (collides) releases an electron. – o Write out symbol.Reactivity increases down the group – farther from nucleus. o o Want to have valence shell like that of a noble gas.Group two not as reactive as group one, why is that? Anions: o Electron joins the atom releasing energy. – Write out symbol. o o Atoms gain electrons to have the valence shell of a noble gas.Chemical reactivity decreases as you move down the group – why is that?
Writing Names of Formulas of Binary Ionic Compounds Binary compound consist of only two elements. Anions are named by changing their ending to “ide” o F–^ Fluoride o O^2 –^ Oxide o CO 2 carbon dioxide o Cl–^ The subscript in a formula is determined by the charges of the ions (are the valence shells filled? Does each element have a noble gas electron configuration?) Are the following correct formulas? If not, write the correct formula. o LiO o MgO o K 2 S o KN 3 o AlBr 3
o Copper Oxide: Cu 2 O Cu+^ O^2 – Use the reverse cross–over method to find the charge on the cation in the following compounds o Cu 2 S o PbO 2 o NiCl 2 o CrN o HgO o Cu 3 P 2
The Stock Naming System: For use with transition metals. o The charge on the cation is written, in parenthesis, as Roman numeral after the name of the metal. o Transition metals can bond with different amounts of electrons (can have a different ionic charge), but remember that the anions will always gain the same number of electrons no matter what the compound is. o FeCl 3 Fe3+^ Cl–^ iron (III) chloride o FeO Fe2+^ O^2 –^ o Cu 2 S Cu+^ S^2 –^ o PbO 2 Write the chemical formulas for each of the following compounds:
o Copper(I) oxide o Lead(IV) bromide o Iron(III) sulfide o Nickel(III) fluoride o Manganese(IV) sulfide Writing Names of Formulas of Binary Molecular Compounds
Binary molecular compounds consist of covalent bonds of two different non-metals. Three rules to writing names and formulas: o The name of the compound ends in “ide” (like that for the ionic compounds). o Name and formula (usually) begins with the element that is more to the left on the periodic table. o Use a prefix to specify the number of atoms of each element that are present in the molecule. (Pg. 162) Prefix Number it Represents mono 1 di 2 tri 3 tetra 4 penta 5 hexa 6
Except for the hydroxide ion, many polyatomic ions end in the suffix “ate” rather than “ide”. Other than that the procedure for writing the names and formulas is the same as that for ionic compounds. Writing the formulas follow the same technique, but the polyatomic ion is written in parentheses (when there is more than one of them). Name Chemical Formula Ammonium ion NH 4 + Hydroxide ion OH– Carbonate CO 32 – Nitrate NO^3 – Sulfate SO 42 – Hydrogen Carbonate HCO^3 – Hydrogen Sulfate HSO 4 – Phosphate PO 43 –
Iron (III) hydroxide Fe3+^ OH– Fe(OH) 3 What is the formula for ammonium phosphide? o NH 4 +^ and P^3 –^ (NH 4 ) 3 P What is the name of Ag(PO 4 )?
o Ag(PO 4 ) Ag+^ and PO 4 –^ Ag3+ and PO 43 –^ Silver(III) Phosphate Ferrum = Iron(I), Ferrous = Iron(II), Ferric = Iron(III) Writing and Balancing Chemical Equations In a chemical reaction mass is conserved (except a nuclear reaction in which energy is conserved). The simplest form of a chemical equation is a word equation. o Sodium + Chlorine Sodium chloride o + means reacts with, means produces o left: reactants; right: products Writing the chemical formulas in place of the names creates a skeleton equation. o Na + Cl 2 NaCl The equation contains more atoms of reactants than products, so as is, mass is not conserved. We will use coefficients to balance the equation so that there are the same number of atoms on both sides. This produces a balanced equation. o 2Na + Cl 2 2NaCl
o Al + H 3 PO 4 H 2 + AlPO 4 there is an odd number of hydrogen atoms on one side and an even number on the other, so write ½H 2 o Al + H 3 PO 4 ½H 2 + AlPO 4 now there is 3 on the left and one on the right, so multiply the ½H 2 by
o Al + H 3 PO 4 23 H 2 + AlPO 4 the equation is balanced, but we don’t want fractions in our answer. Multiply every term by 2. o 2Al + 2H 3 PO 4 3H 2 + 2AlPO 4 Equations Where Polyatomic Ions are Conserved The general rule is to treat the polyatomic ions as if they are one element. Example 1: KI + Pb(NO 3 ) 2 PbI 2 + KNO 3 o To start, we’ll balance the iodine. o 2KI + Pb(NO 3 ) 2 PbI 2 + KNO 3 o The lead (Pb) is balanced, but there are 2 nitrate ions on the left and only one on the right. Since the nitrate ion did not change we can balance it the
same way as a single atom. 2KNO 3 balances the equation. o KI + Pb(NO 3 ) 2 PbI 2 + 2KNO 3 Example 2: Al + H 2 SO 4 Al 2 (SO 4 ) 3 + H 2 o Balance the Al: 2Al + H 2 SO 4 Al 2 (SO 4 ) 3 + H 2 o Now the sulfate groups: with 3H 2 SO 4 2Al + 3H 2 SO 4 Al 2 (SO 4 ) 3 + H 2 o Balance the hydrogen atoms with 3H 2 2Al + 3H 2 SO 4 Al 2 (SO 4 ) 3 + 3H 2 Example 3: Cu(NO 3 ) 2 + NH 4 OH Cu(OH) 2 + NH 4 NO 3
o There are three polyatomic ions: NO 3 – , OH–,
and NH 4 +. All of the ions are conserved, so
we balance the equation like the polyatomic
ions are single atoms.
o Two nitrates on the left and one on the right:
Cu(NO 3 ) 2 + NH 4 OH Cu(OH) 2 + 2NH 4 NO 3 o Balance the ammonium ions, which will also balance the hydroxide ions: Cu(NO 3 ) 2 + 2NH 4 OH Cu(OH) 2 + 2NH 4 NO 3
More difficult to identify by their names; but any containing the hydroxide ion, or that react with water to form hydroxide ions are bases. o NaOH sodium hydroxide o KOH potassium hydroxide o HCO 3 -^ forms an OH- in water.
The pH Scale Compares the concentration of hydrogen ions in various solutions. used to represent how acidic or basic a solution is. Ranges from 0 to 14, with 7 (pure water) being neutral. Bases have a high pH (above 7), acids are lower in pH (below 7). Logarithmic scale o A change of 1 on the scale means one substance is 10 times more acid/basic. o An acid of pH = 2 is ten times more acidic than an acid of pH = 3. o A base of pH = 13 is ten times more basic than an acid of pH = 12.
Examples: o How many times more acidic is an acid of pH = 3 than water (pH = 7)? o Which is the stronger base: pH = 9 or pH = 14? How many times stronger (basic) is it? o Be careful: pH = 2, and a pH = 2.5; logarithms are not linear, a difference of 0.5 in pH does not mean 5 times as powerful. Problems 1 – 7, 9, and 10. Neutralization Reactions Mixing an acid and a base results in a neutralization reaction. The products are a salt and (often) water. There may also be other products (like a gas, CO 2 ). Water is formed by combining the H+^ from the acid and the OH–^ from the base: HOH, or H 2 O. Acid – base reactions are used all the time: o Many cleaners use this property. o Baking soda as an ingredient in food. o Antacids to settle a stomach that is too acidic or reacting with the stomach or esophagus lining.
