Chemistry Chapter 11 Bonding World of Chemistry Zumdahl Last revision Fall 2008

Bonding and Molecules Reaction – When an atom interacts with another atom forming a _____________. Chemical Bond – An __________ between two or more atoms that binds them together.

Types of Chemical Bonds ______________ are made from two or more atoms that share a chemical bond. 1)Found only in ____________. Examples: H 2 O, H 2 O 2 2) They can be _________ down in _________ reactions. There are two groups of compounds and types of chemical bonds: _________ and ____________

Why form chemical bonds? 1)Atoms tend to be stable when they have ____ electrons in their outer energy level. Stable Unlikely to react. Unstable Likely to react.

Rule of Octet or The Octet Rule Stable energy levels are full energy levels and allow atoms to not react. The first energy level is stable with 2 electrons and other levels with 8. This is known as the rule of Octet or Octet rule. All elements want to have the same number of electrons as the nearest noble gas!

Na Cl 11 p + 12 n o 18 n o 17 p + 1e - 8e - 2e - 7e - 8e - 2e - 8e - + _ Bohr model and the octet rule

How do atoms become stable? a) Those with 1 to 3 outer electrons tend to lose those electrons because the next energy level in has 8 e -. b) Those with 5 to 7 outer electrons tend to want to gain extra electrons until they have 8 e -. c) Those with 4 outer electrons tend to share those electrons. Valence number = family number Can’t tell share Stable

p + e - n 0 Valence # Steal/Give Charge Na Ca H C O Cl Let’s find some parts of the atom: Give 1e Give 2e Give 1e0 66 Share Steal 1e Steal 2e

Remember: _______ number tells us the Valence electrons. We diagram the valence electrons with Lewis Dot diagrams Lewis Dot diagrams – dots around the symbol represent valence electrons around the nucleus. 1. Place two electrons together if there are more than four, otherwise spread them out around the symbol. 2. Spread the rest out before pairing.

Practice drawing Lewis Dots HMgCO FAr N B

Ionic Bonds This is the force of ________ between _________ charged ions. a)Ion – an atom that gains or loses electrons.  ________ – positively charged ion = lost (gave) electrons  _________ – negatively charged ion = gained (stole) electrons

Covalent Bond In these bonds electrons are shared rather than lost or gained. Molecules – a group of atoms held together by covalent bonds. Electronegativity - This is the force of attraction that an atom has for a shared pair of electrons. This is what is responsible for the rules we looked at above. Note: Ionic compounds usually occur between a _______ and a _________ while covalent bonds occur between two nonmetals.

Chemical Formulas Chemical Formula – This is the “recipe” of a compound. It contains the ratios of the atoms combined in the compound. Sometimes information is given above the normal line of information. In the example below, 12 and +4 are written as what we call a superscript C 6 1 Sometimes the information given is below the normal line of information. In the example below, 6 and 1 are written in subscripts.

1) Write the symbol for the ___________ (determine the charge or oxidation number using your periodic table) 2) Write the symbol for the __________ (determine the charge or oxidation number using your periodic table). An oxidation number (or charge) indicates how many electrons are lost, gained or shared when bonding occurs. Writing formulas for ionic compounds:

3) Add subscripts so that the ____ of the positive and negative oxidation numbers is _____. The Crisscross Method or Swap N’ Drop Method can also work. 4) All compounds are _______ so the oxidation numbers should combine in ratios that will add up to ____. The number of ions combining in the compound will be written as subscripts in the final formula. Example: Na +1 and Cl -1 (+1) + (-1) = 0 NaCl

Try this example on your own: Ca and Br Ca +2 Br -1 (+2) + (-1) =+1 Add more negative Ca +2 Br -1 (+2) + (-2) =0 CaBr 2 1 2

Al +3 O -2 Swap and drop short cut Al and O Charges can be crisscrossed to become subscripts (remember to remove the sign) 32 Al 2 O 3 Mg +2 Cl Mg and Cl MgCl 2 A subscript of 1 is never written. The symbol stands for 1.

Polyatomic Ions – Some covalently bonded atoms function as a ion or charged particle. Two important ones are hydroxide (OH - ) and ammonium (NH 4 + ) Use parentheses to treat the group as a single unit when writing the chemical formula. Example: Al +3 OH Al OH 3 () Whenever a subscript is used to indicate more than one polyatomic ion you must use parenthesis

Naming Ionic Compounds: 1) The first ion (cation or positive ion) keeps its name. Example: NaCl Sodium 2) The second ion (anion or negative ion) keeps the first syllable or the root of the name and then ends in the suffix –ide. 3) If any of the ions are polyatomic, use the their name from the list. Example: chlor NaCl Sodiumide

Fe +3 = Iron (III) Ion Fe +2 = Iron (II) Ion Transition metals may occur in a variety of oxidation states and a roman numeral must be included in the name to tell the reader which type of ion it is. You should include a roman numeral for all transition metals (except Silver [Ag + ] and Zinc [Zn +2 ]). Transition Metals

There are two steps for determining the charge on the transition metal. 1. Un-crisscross the subscripts (remember: no subscript indicates 1 atom) 2. Check the anion (-) to see if you must adjust the numbers

Example: FeO +1 1.Un-crisscross the charges. FeO +1 2.Check the anion. Adjust as needed. x 2=-2=2 x+2 The name for the compound is Iron (II) Oxide

Naming Covalent Compounds: 1) List the least electronegative first. First atom only keeps it’s name and only uses a prefix if there is more than one 2) List the most electronegative second. Second atom ends with “ide” and always uses a prefix to tell how many atoms of each there are: mono = 1 atomhexa = 6 atoms di = 2atomshepta = 7 atoms tri = 3atomsocto = 8 atoms tetra = 4 atomsnono = 9 atoms penta= 5 atomsdeca = 10 atoms 4) There are no charges in covalent compounds so there is no crisscrossing or uncrisscrossing or roman numerals.

Properties of Ionic compounds – Ionic compounds are usually solids at room temperature Melting and Boiling Points – Ionic compounds have much higher melting points and boiling points than covalent compounds –– Ionic compounds typically melt at several hundred degrees Celsius They exist in a crystal state so we refer to the smallest ratio of ions in the crystal as their formula unit When dissolved in water, ionic compounds break into ions (charged particles) and can conduct electricity through the solution.

Properties of Covalent compounds Covalent compounds are typically formed from nonmetals Molecules – this is the single unit of compounds characterized by covalent bonding Exist as discrete molecules in the solid, liquid, and gas states. They carry no charges.