CHEMICAL BONDS

I. Chemical Compounds Compounds Are made from more than one type of atom (element) Are made during a chemical chg Have properties different from the elements they are made of Have constant compositions

Fe2O3 I. Chemical Compounds Chemical Formulas Use symbols to represent the ratios of elements in a particular compound. Element symbols Subscripts Fe2O3

3. Practice Interpreting Formulas B. Chemical Formulas 3. Practice Interpreting Formulas NaCl 1 sodium atom; 1 chlorine atom H2O 2 hydrogen atoms; 1 oxygen atom Al2(SO4)3 2 aluminum atoms 3 sulfur atoms 12 oxygen atoms

Your Turn! Fe2O3 Pb(C2H3O2)2 Interpret each of the following 2 iron atoms 3 oxygen atoms 1 lead atom 4 carbon atoms 6 hydrogen atoms 4 oxygen atoms

I. Chemical Compounds C. Atoms Combine To become Stable Atoms are stable when they have a full valence energy level Octet rule: Usually 8 e- Exception: He is stable w/ 2 e- Atoms gain, lose or share e- to achieve a full valence level c. Atoms are held together by a chemical bond

I. Chemical Compounds C. Atoms Combine Noble gases Are inert do not react because they already have a full valence energy level (stable octet)

II. Ions A. Ions are atoms which 1. Have gained or lost e- ELements to the Left of the Line Lose eLectrons Neither LOSE GAIN

II. Ions A. Ions are atoms which 1. Have gained or lost e-

II. Ions A. Ions are atoms which 1. Have gained or lost e- You can predict the # of e- which will be gained or lost by looking at the family

Gains 3 e- Lose 1 e- Varies Lose 2 e- Gain 3 e- Gain 2 e- Gain 1 e- Will P gain or lose electrons when forming an ion? How many? Gains 3 e-

A. Ions are atoms which Formula= Na1+ Formula= Cl1- Another name for charge is oxidation number The formula for an ion includes its charge (oxidation number) Na ion Lost 1 e- Formula= Na1+ Cl ion Gained 1 e- Formula= Cl1-

Review it Now! Ions have a charge, atoms do not What is the difference between an atom and an ion? What is an oxidation number? Write the oxidation number for each of the following ions: a.  Li f. Al b. K g. S c. Mg h. Cl d.  P i. Ne e. B j. N The charge on an ion 1+ 3+ 1+ 2- 2+ 1- 3- 3+ 3-

III.Compounds with Ionic Bonds 1.Are formed a.between (+) and (-) ions b.When one atom gains e- while the other loses e- 2.Compounds with ionic bonds are called ionic compounds

III.Compounds with Ionic Bonds 3. Ionic bonds are formed between a metal and a nonmetal!

Check Your Understanding! Which of the following are ionic compounds? 1. KCl 2. CO2 3. LiF 4. CaCl2 Ionic Not ionic Ionic Ionic

B. Formulas for Binary Cmpds Step 1:Write the symbol of the (+) ion first, followed by the symbol of the (-) ion Step 2: Determine the ox.# for each ion and write it above the symbols. Step 3: Crisscross the charges and write them as subscripts. Step 4: If the charges can be reduced, do so.

B. Formulas for Ionic Cmpds Example #1: Ba and Cl

B. Formulas for Ionic Cmpds Example #2: Be and P Be3P2

BaS Ba2S2 B. Formulas for Ionic Cmpds Example #3: Ba and S note subscripts can be reduced; do so!

Write the formula for each of the following compounds Your Turn! Write the formula for each of the following compounds 1. calcium with chlorine 2. potassium with bromine 3. lithium with sulfur 4. magnesium with phosphorus 5. aluminum with nitrogen CaCl2 KBr Li2S Mg3P2 AlN

C. Naming Binary Cmpds Step 1:Write the name of the positive element 1st. Step 2:Write the name of the negative element 2nd. Step 3:Add the ending -ide to the root of the second element.

calcium chloride C. Naming Binary Cmpds Example #1: What is the formula name for CaCl2? Step 1: calcium Step 2: calcium chlorine Step 3: calcium chloride calcium chloride

Magnesium phosphide C. Naming Binary Cmpds Example #2: What is the formula name for Mg3P2? Step 1: magnesium Step 2: magnesium phosphorus Step 3: magnesium phosphide Magnesium phosphide

Name each of the following Your Turn! Name each of the following 1. Li2S 2. KBr 3. BaS 4. Al2O3 5. Na3N Lithium sulfide Potassium bromide Barium sulfide Aluminum oxide Sodium nitride

D. Formulas for Polyatomic Ionic Cmpds Binary compounds are made of two kinds of elements. Example: BaCl2 Polyatomic (ternary) compounds are made of three or more elements. Examples: K2SO4 Mg(ClO3)2

D. Formulas for Polyatomic Ionic Cmpds Polyatomic ions are a group of covalently bonded atoms that act as one atom with a charge.

D. Formulas for Polyatomic Ionic Cmpds Rules for Writing Formulas Step 1:Write the symbol and ox. # Step 2: Crisscross the charges and write them as subscripts. Step 3: Make sure you put polyatomic ions in parentheses (if you need more than one). Step 4: Make sure the subscripts are reduced.

Ca(NO3)2 D. Formulas for Ionic Cmpds Example #1: Calcium Nitrate Ca2+ and NO31- Ca2+ and NO31- 2 Ca2+ and (NO3) 2 Ca(NO3)2

Ca3(PO4)2 D. Formulas for Polyatomic Ionic Cmpds Example #2: Calcium Phosphate Ca2+ and PO43- Ca2+ and PO43- 3 2 Ca3 and (PO4)2 Ca3(PO4)2

Your Turn! Write the formula for each of the following compounds 1. Sodium sulfate 2. Calcium hydroxide 3. Beryllium phosphate 4. Aluminum nitrate Na2SO4 Ca(OH)2 Be3(PO4)2 Al(NO3)3

E. Naming Polyatomic Ionic Compounds Rules for Naming Polyatomic Compounds Step 1:Write the name of the positive ion. Step 2: Write the name of the negative ion .

Calcium nitrate E. Naming Polyatomic Ionic Cmpds Example #1: Ca(NO3)2

Aluminum phosphate E. Naming Polyatomic Ionic Cmpds Example #2: AlPO4

Your Turn! Name each of the following compounds Potassium sulfate 1. K2SO4 2. CaCO3 3. NaOH 4. NH4C2H3O2 Potassium sulfate Calcium carbonate Sodium hydroxide Ammonium acetate

G. Special case ionic bonds: ACIDS Acids are easy to recognize as compounds as they begin with the element hydrogen. As with other ionic bonds, acids fall into 2 categories, binary and ternary.

G. Special case ionic bonds: ACIDS Examples of binary acids would include things like: HF, HI, H2S and HCl Examples of ternary acids would include things like: H2SO4 and HNO3

G. Special case ionic bonds: ACIDS Naming of binary acids Step 1:Name the anion, changing the ending to “-ic” Step 2: Add the prefix “hydro-” Step 3: Slap acid on the end

G. Special case ionic bonds: ACIDS Example #1: HF

G. Special case ionic bonds: ACIDS Example #1: HF “flourine” becomes

G. Special case ionic bonds: ACIDS Example #2: HF “flourine” becomes “flouric” becomes

G. Special case ionic bonds: ACIDS Example #1: HF “flourine” becomes “flouric” becomes “hydroflouric” becomes

“hydroflouric acid” G. Special case ionic bonds: ACIDS Example #1: HF “chlorine” becomes “chloric” becomes “hydrochloric” becomes “hydroflouric acid”

G. Special case ionic bonds: ACIDS Example #2: HCl

G. Special case ionic bonds: ACIDS Example #2: HCl “chlorine” becomes

G. Special case ionic bonds: ACIDS Example #2: HCl “chlorine” becomes “chloric” becomes

G. Special case ionic bonds: ACIDS Example #2: HCl “chlorine” becomes “chloric” becomes “hydrochloric” becomes

“hydrochloric acid” G. Special case ionic bonds: ACIDS Example #2: HCl “chlorine” becomes “chloric” becomes “hydrochloric” becomes “hydrochloric acid”

Naming of ternary acids G. Special case ionic bonds: ACIDS Naming of ternary acids Step 1:Name the polyatomic Step 2: Change “-ate” to “-ic” or “-ite” to “-ous” Step 3: Slap acid on the end

“sulfuric acid” G. Special case ionic bonds: ACIDS Example #1: H2SO4 “sulfate” becomes “sulfuric” becomes “sulfuric acid”

G. Special case ionic bonds: ACIDS Example #1: H2SO4

G. Special case ionic bonds: ACIDS Example #1: H2SO4 “sulfate” becomes

G. Special case ionic bonds: ACIDS Example #1: H2SO4 “sulfate” becomes “sulfuric” becomes

“sulfuric acid” G. Special case ionic bonds: ACIDS Example #1: H2SO4 “sulfate” becomes “sulfuric” becomes “sulfuric acid”

G. Special case ionic bonds: ACIDS Example #1: HNO2

G. Special case ionic bonds: ACIDS Example #1: HNO2 “nitrite” becomes

G. Special case ionic bonds: ACIDS Example #1: HNO2 “nitrite” becomes “nitrous” becomes

“nitrous acid” G. Special case ionic bonds: ACIDS Example #1: HNO2 “nitrite” becomes “nitrous” becomes “nitrous acid”

Rules for Writing Formulas for binary acids G. Special case ionic bonds: ACIDS Rules for Writing Formulas for binary acids Step 1: Does the name begin with “hydro-”? If yes, then… Step 2:Write the symbol for the hydrogen ion followed by the symbol for the second element Step 3: Crisscross the charges and write them as subscripts.

G. Special case ionic bonds: ACIDS Rules for Writing Formulas for binary acids Example: hydrosulfuric acid

G. Special case ionic bonds: ACIDS Rules for Writing Formulas for binary acids Example: hydrosulfuric acid H+1 S-2

G. Special case ionic bonds: ACIDS Rules for Writing Formulas for binary acids Example: hydrosulfuric acid H+1 S-2

H2S G. Special case ionic bonds: ACIDS Example: hydrosulfuric acid Rules for Writing Formulas for binary acids Example: hydrosulfuric acid H+1 S-2 H2S

Rules for Writing Formulas for ternary acids G. Special case ionic bonds: ACIDS Rules for Writing Formulas for ternary acids Step 1: Does the name begin with “hydro-”? If no, then… Step 2:Write the symbol for the hydrogen ion followed by the appropriate polyatomic ion Step 3: Crisscross the charges and write them as subscripts.

Rules for Writing Formulas for binary acids Example: sulfuric acid G. Special case ionic bonds: ACIDS Rules for Writing Formulas for binary acids Example: sulfuric acid

Rules for Writing Formulas for binary acids Example: sulfuric acid G. Special case ionic bonds: ACIDS Rules for Writing Formulas for binary acids Example: sulfuric acid H+1 SO4-2

Rules for Writing Formulas for binary acids Example: sulfuric acid G. Special case ionic bonds: ACIDS Rules for Writing Formulas for binary acids Example: sulfuric acid H+1 SO4-2 H+1 SO4-2

Rules for Writing Formulas for binary acids Example: sulfuric acid G. Special case ionic bonds: ACIDS Rules for Writing Formulas for binary acids Example: sulfuric acid H+1 SO4-2 H+1 SO4-2 H2SO4

G. Special case ionic bonds: ACIDS Name the chemical or write the symbol 1. HI 2. phosphoric acid 3. hydrobromic acid 4. H2SO3

G. Special case ionic bonds: ACIDS Name the chemical or write the symbol hydroiodic acid 1. 2. phosphoric acid 3. hydrobromic acid 4. H2SO3

G. Special case ionic bonds: ACIDS Name the chemical or write the symbol hydroiodic acid 1. 2. 3. hydrobromic acid 4. H2SO3 H3PO4

G. Special case ionic bonds: ACIDS Name the chemical or write the symbol hydroiodic acid 1. 2. 3. 4. H2SO3 H3PO4 HBr

G. Special case ionic bonds: ACIDS Name the chemical or write the symbol hydroiodic acid 1. 2. 3. 4. H3PO4 HBr sulfurous acid

IV.Compounds with Covalent Bonds 1.Are formed when atoms share e-

IV.Cmpds with Covalent Bonds 2.Are formed Between two nonmetals

Your Turn! State if each of the following compounds is ionic or covalent 1. CO2 2. MgS 3. Na2O 4. PI3

Your Turn! State if each of the following compounds is ionic or covalent 1. CO2 2. MgS 3. Na2O 4. PI3 covalent

Your Turn! State if each of the following compounds is ionic or covalent 1. CO2 2. MgS 3. Na2O 4. PI3 covalent ionic

Your Turn! State if each of the following compounds is ionic or covalent 1. CO2 2. MgS 3. Na2O 4. PI3 covalent ionic ionic

Your Turn! State if each of the following compounds is ionic or covalent 1. CO2 2. MgS 3. Na2O 4. PI3 covalent ionic ionic covalent

IV.Cmpds with Covalent Bonds Writing Covalent Formulas Greek Prefixes mono- one di- two tri- three tetra- four penta- five hexa- six hepta- seven octa- eight nona- nine deca- ten

B. Writing Covalent Formulas 2.Rules Step 1: Write the symbol of the first nonmetal. Step 2: Use the nonmetal’s prefix as a subscript

B. Writing Covalent Formulas 2.Rules Step 3: Write the symbol of the second nonmetal. Step 4: Use the nonmetal’s prefix as a subscript. Note: If there is no prefix, there is no subscript.

C B. Writing Covalent Formulas 3.Practice problem #1 Write the formula for carbon dioxide C

C O B. Writing Covalent Formulas 3.Practice problem #1 Write the formula for carbon dioxide C O

C O B. Writing Covalent Formulas 2 3.Practice problem #1 Write the formula for carbon dioxide C O 2

No Prefix = No Subscript B. Writing Covalent Formulas 3.Practice problem #1 Write the formula for carbon dioxide C O 2 No Prefix = No Subscript

B. Writing Covalent Formulas 3.Practice problem #2 Write the formula for dinitrogen trioxide

N B. Writing Covalent Formulas 3.Practice problem #2 Write the formula for dinitrogen trioxide N

N O B. Writing Covalent Formulas 3.Practice problem #2 Write the formula for dinitrogen trioxide N O

N O B. Writing Covalent Formulas 2 3 3.Practice problem #2 Write the formula for dinitrogen trioxide N O 2 3

B. Writing Covalent Formulas 3.Practice problem #3 Write the formula for dichlorine hexabromide

Cl B. Writing Covalent Formulas 3.Practice problem #3 Write the formula for dichlorine hexabromide Cl

Cl Br B. Writing Covalent Formulas 3.Practice problem #3 Write the formula for dichlorine hexabromide Cl Br

Cl Br B. Writing Covalent Formulas 2 6 3.Practice problem #3 Write the formula for dichlorine hexabromide Cl Br 2 6

Cl Br B. Writing Covalent Formulas 2 6 3.Practice problem #3 Write the formula for dichlorine hexabromide Cl Br 2 6 Note: Do Not Reduce subscripts!

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide CCl4

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide CCl4 Cl3Br7

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide CCl4 Cl3Br7 N2O

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide CCl4 Cl3Br7 N2O CO

IV.Cmpds with Covalent Bonds Naming Covalent Cmpds Step 1: Name each element. Step 2: Change the ending of the 2nd element to -ide Step 3: Add Greek prefixes to indicate the # ofatoms of each element Note: Do not use mono on the first element!

C. Naming Covalent Cmpds 2.Practice problem #1 Write the name for CO

C. Naming Covalent Cmpds 2.Practice problem #1 Write the name for CO Carbon

C. Naming Covalent Cmpds 2.Practice problem #1 Write the name for CO Carbon Monoxide oxygen

C. Naming Covalent Cmpds 2.Practice problem #1 Write the name for CO Carbon oxide oxygen

C. Naming Covalent Cmpds 2.Practice problem #1 Write the name for CO Carbon Monoxide

C. Naming Covalent Cmpds 2.Practice problem #1 Write the name for CO Carbon Monoxide Carbon Monoxide

C. Naming Covalent Cmpds 2.Practice problem #2 Write the name for Cl2O3 Dichlorine trioxide trioxide oxide Dichlorine trioxide

C. Naming Covalent Cmpds 2.Practice problem #2 Write the name for Cl2O3 chlorine

C. Naming Covalent Cmpds 2.Practice problem #2 Write the name for Cl2O3 chlorine oxygen

C. Naming Covalent Cmpds 2.Practice problem #2 Write the name for Cl2O3 chlorine oxide

C. Naming Covalent Cmpds 2.Practice problem #2 Write the name for Cl2O3 Dichlorine chlorine trioxide trioxide oxygen oxide

C. Naming Covalent Cmpds 2.Practice problem #2 Write the name for Cl2O3 Dichlorine chlorine trioxide trioxide oxygen oxide Dichlorine trioxide

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide CCl4

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide CCl4 Cl3Br7

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide CCl4 Cl3Br7 N2O

Write formulas for the following compounds Your Turn! Write formulas for the following compounds 1. Carbon tetrachloride 2. Trichlorine heptabromide 3. Dinitrogen monoxide 4. Carbon monoxide CCl4 Cl3Br7 N2O CO

Name the following compounds Your Turn! Name the following compounds 1. PBr5 2. NO 3. S2I3

Name the following compounds Your Turn! Name the following compounds 1. phosphorus pentabromide 2. NO 3. S2I3

Name the following compounds Your Turn! Name the following compounds 1. phosphorus pentabromide 2. nitrogen monoxide 3. S2I3

Name the following compounds Your Turn! Name the following compounds 1. PBr5 2. nitrogen monoxide 3. disulfur triiodide phosphorus pentabromide

THAT’S ALL FOLKS!!! Now you can name not only covalent bonds but binary and ternary ionic bonds, including acids. That being said, now… GO DO!!!