Chapter 6 Chemical Bonds Warmup Question 1 What

Chapter 6 Chemical Bonds Warm-up Question: 1. What are valence electrons? 2. List the number of valence electrons for the following elements: Na ____K ____ Cl _____Al _____ ***Hint: You need your periodic table***

Chemical Bonds… n Chemical Bond – force that holds atoms together q q q Bonding occurs between the valence electrons These chemical bonds are constantly being made and broken down in our environment. Your body breaks the chemical bonds in the food we eat to get energy so our body can do work. n Chemical bonding forms COMPOUNDS n Reading a Chemical compound formula C 6 H 12 O 6

Chemical Bonds… (cont) n There are two types of chemical bonds. q q q The difference is what they do with their valence electrons. 1. Ionic Bonds - One atom steals electrons from another atom. n Ionic is always a metal with a nonmetal 2. Covalent Bonds – Electrons are shared between the atoms. n Covalent is always two nonmetals

Representing Valence Electrons Lewis Dot Structure – model of an atom in which each dot represents a valence electron C= S= He = * symbol in the center is the nucleus and all the inner electrons in the atom

IONIC COMPOUNDS n Ion - an atom that has a charge. (+ or -) q 2 types of ions 1. anion – negatively charged ion (must gain electrons) ex: Cl-1 O-2 N-3 2. cation - positively charged ion (must lose electrons) ex: Ca+2 K+1 Al+3 ***You can determine charge by where they are located on the periodic table.

Stable Electron Configurations When the highest energy level is filled with electrons, the atom is stable and not likely to react. Octet Rule – the tendency of atoms to gain or lose electrons in order to fill the outer most electron shell. (a full outer shell has 8 valence electrons) What group on the periodic table already has a full outer most shell?

Drawing Lewis Dot Structures of Ions n Cations – they are + charge so they must have ____ electrons. q n Examples: Anions – They are – charge so they must have _______ electrons. q Examples:

Dot Structures for Ionic Compounds n Examples: q Ba. O q Ca. Cl 2 q Mg 3 N 2 q Al. Br 3 n *** Now for the homework assignment***

II. Ionic Bonds 1. ion – an atom that has a positive or negative charge a. When an atom gains or loses an electron, the # of protons no longer = the # of electrons b. 2 types of ions 1. anion – negatively charged ion (gains a electron) 2. cation - positively charged ion (loses a electron) → Na+Cl→ Mg+2 S-2

2. Ionic Bond – Form between metals and nonmetal (transfer of electrons) ex. Na. Cl, Mg. O, Ca. Br 2 3. Chemical Bond – force that holds atoms together 4. Ionization energy – amount of energy used to remove an electron q q a. Lower the ionization energy, the easier it is to remove an electron from an atom b. Ionization energies increase from left to right in a period Ex. More energy is required to remove an electron from a nonmetal than a metal. c. Energy increases from the bottom of a group to the top § Ex. Easier to remove an electron from K than Na

III. Covalent Bonds – form between two nonelectrons) metals (sharing of a. Molecule – neutral group of atoms that are joined together by one or more covalent bonds IV. Metallic bonds 1. Metal in a sea of electrons Ex. Cu, Al, Fe

V. Unequal Sharing of Electrons 1. Electronegativity – ability of an atom attract electrons to itself, greater this number the greater its ability to attract electrons a. Non-Polar Covalent Bonding- an equal sharing of electrons ex. F 2 b. Polar Covalent Bonding - an unequal sharing of electrons ex. HF attraction between polar molecules are stronger

VI. Naming Compounds and Writing Formulas a. The subscripts on H 2 = 2 atoms in 1 molecule of hydrogen b. determining the number of atoms Ex. P 2 F 4 = 2 phosphorus atoms 4 fluorine atoms Ex. (Na. SO 4)3 = 3 sodium 3 sulfate 12 oxygen

1. Writing Formulas for ionic compounds a. list the symbols and charges for the cation and anion b. use the criss cross method ex. = Ca. Cl 2 2. Naming Ionic Compounds (TYPE 1) A. Cations (metals) and Anion (nonmetal) q q 1 st cation before the anion (or metal before the nonmetal) 2 nd drop the end of the second element and add “ide” Ex. Na. Cl = Sodium Chloride BP = Boron Phosphide

3. Naming TYPE (2) A. If the metal is a transition metal Roman Numerals in parentheses are used 1 = (I) 2 = (II) 3 = (III) 4 = (IV) 5 = (V) ex. Cu+2 = copper (II) ion Fe+3 = iron (III) ion Cu. Cl 2 = Copper (II) Chloride Iron (III) oxide = Fe 2 O 3

3. Naming Covalent Compounds (TYPE 3) A. Name between two nonmetals 1 st – most metallic element first (element farthest to the left) 2 nd – then add “ide” on the end of the second element 3 rd – then add a prefix (mono is never used with the 1 st element) Ex. N 2 O = Di. Nitrogen Monoxide Ex. diphosphorus tetraflouride = P 2 F 4