What happens to electrons in a covalent bond? Compare and contrast ionic and covalent bonds in terms of electron movement. In an ionic bond, metals tend to become electron (donors/acceptors), and non-metals tend to become electron (donors/acceptors). What happens to electrons in a covalent bond?

Covalent & Ionic Name two types of chemical bonds. Compare and contrast ionic and covalent bonds in terms of electron movement. Name two types of chemical bonds. Covalent & Ionic What happens to electrons in an ionic bond?

What is an ion? An ion is a charged atom. It is formed when an atom gains or loses electrons. What information is shown in a Lewis/Dot Diagram?

IONIC BONDING

Ionic Compounds When electrons are transferred from a metal to a non-metal, ionic bonds form from the attractions between oppositely charged ions. Metal + Nonmetal Metals tend to lose electrons to become positively charged (cations) Nonmetals tend to gain electrons to become negatively charged (anions)

Example F K Lewis Dot Structures (show valence electrons)

K F

Ions + _ K F Stable ionic bonds have the same number of positive and negative charges.

K F _ This ionic bond is the attraction between the positive K+ ion and the negative F- ion

KF Put the symbols together and you have the chemical formula

Naming Ionic Compounds KF For the first element, use the full element name Potassium For the second element, change the ending to “-ide” Fluoride Potassium Fluoride

Mg2+ Oxidation Number Shows the charge of an ion Write the oxidation numbers across the top of your periodic table Mg2+

Periodic Table Ion Trend +1 +2 +3 +/-4 -3 -2 -1

More Practice Sodium and Chlorine Calcium and Fluorine Magnesium and oxygen

BR: What is an ion? An ion is a charged atom. It is formed when an atom gains or loses electrons. EQ: What information is shown in a Lewis/Dot Diagram? Lewis/Dot Diagrams are used to show the number of valence electrons for a given element.

BR: What is an ion? An ion is a charged atom. It is formed when an atom gains or loses electrons. What information is shown in a Lewis/Dot Diagram? Lewis/Dot Diagrams are used to show the number of valence electrons for a given element.

What happens to electrons when an ionic bond is formed? Valence electrons are transferred from a metal to a non-metal. How can you check/be sure that your ionic formula is stable? In a stable ionic compound, there are equal numbers of positive and negative charges.

When should you use the “-ide” ending? Use “-ide” as the ending for a non-metal.

Ionic Compounds Cation (positive ion) TRANSITION METALS Many of these metals form more than one monoatomic ion Give the element name Use roman numerals to denote charge Cr chromium Cr2+ chromium (II) Cr3+ chromium (III) MAIN GROUP Give the element name Li lithium Li+ lithium

How would you name the following? Ag +2 Ba +2 Mg +2 Fe +3 Na+1 Zn +4 Al +3 Co +3 Silver (II) Barium Magnesium Iron (III) Sodium Zinc (IV) Aluminum Cobalt (III)

Ionic Compounds Anions (negative ion) Give the element name but drop the ending Add the “-ide” ending F fluorine F- fluoride ion

How would you name the following? P -3 Cl -1 S -2 N -3 Br -1 Oxide Phosphide Chloride Sulfide Nitride Bromide

Binary Ionic Compounds Binary compound: compounds composed of two different atoms Write the name of the cation first Write the name of the anion last MgO Magnesium Oxide

How would you name the following? AgO Ba3P2 MgCl2 FeS Fe2S Na3N ZnBr4 Al 2O3 CuBr2 CuBr Silver (II) oxide Barium phosphide Magnesium Chloride Iron (II) sulfide Iron (I) sulfide Sodium nitride Zinc (IV) bromide Aluminum oxide Copper (II) bromide Copper (I) bromide

What does the roman numeral in iron (III) oxide tell you? Roman numerals show the charge of a transition metal. Iron has a +3 What is the formula for iron (III) oxide? Fe2O3

Bond With Your Classmates Part I

Ionic Compound Grid Determine the charge of each ion. Make a stable ionic compounds. Determine the number of total electrons transferred to form each compound. Oxide Bromide Sulfide nitride Sodium Copper II Potassium Iron III Calcium Gallium Iron II

Ionic Compound Grid Oxide Bromide Sulfide nitride Iodide phosphide Sodium Na O Na Br Na S Na N Na I Na P Copper II Cu O Cu Br Cu S Cu N Cu I Cu P Potassium K O K Br K S K N K I K P Iron III Fe O Fe Br Fe S Fe N Fe I Fe P Calcium Ca O Ca Br Ca S Ca N Ca I Ca P Gallium Ga O Ga Br Ga S Ga N Ga I Ga P Iron II

Chemistry CAT Joke

1. What is the name for NaCl? A. sodium chloride B. sodium chlorine C. sodium I chloride

2. What is the correct formula for Aluminum chloride? A. AlCl B. Al3Cl C. AlCl3

3. What is the correct formula for Ba+2 and Cl-1? A. Cl2Ba B. BaCl C. BaCl2

4. What is the name for CaF? A. calcium fluoride B. calcium fluorine C. calcium II fluoride

5. What is the correct formula for a compound formed when a sodium ion combines with a fluoride ion? A. NaF2 B. NaF C. Na2F

6. What is the correct formula for Magnesium chloride? A. MgCl B. Mg2Cl C. MgCl2

7. What is the correct formula for calcium oxide ? A. CaO2 B. CaO C. Ca2O

8. What is the name for MgS? A. magnesium II sulfide B. magnesium sulfur C. magnesium sulfide

9. What is the correct formula for Ag+1 Cl -1? A. SiCl B. AgCl C. AgCl3

10. What is the formula formed by a potassium ion and a sulfur ion? A. K2S B. KS C. KS2

11. What is the compound formed from Ca +2 and I-1? A. CaI2 B. I2Ca C. CaI

12. What is the formula formed by Li +1 and O-2? A. Li2O B. LiO C. LiO2

Mock Quiz Potassium & sulfur Name  Formula Sodium chloride Valence Electrons Ions Formula & Name Potassium & sulfur Name  Formula Sodium chloride Aluminum sulfide MgI2 Na2O

Mock Quiz Potassium & sulfur Name  Formula Sodium chloride Valence Electrons Ions Formula & Name Potassium & sulfur Name  Formula Sodium chloride Aluminum sulfide MgI2 Na2O

What does the roman numeral in iron (IV) oxide tell you? Roman numerals show the charge of a transition metal. Iron has a +4 What is the formula for iron (IV) oxide? FeO2

How do ionic compounds form? When electrons are transferred from a metal to a non-metal, oppositely charged ions attract to form an ionic bond.

BONDING PART II

Covalent Compounds

Covalent Compounds In covalent bonding, atoms still want to achieve stability by having a full outer energy level. Atoms SHARE electrons rather than lose or gain Nonmetal—Nonmetal

EXAMPLE: Chlorine forms a Covalent bond with itself Cl2

How will these two chlorine atoms become stable? Cl Cl

Cl Cl Each chlorine atom wants to gain one electron to achieve 8.

Cl Cl do to achieve an octet? What’s the solution – what can they Neither atom will give up an electron … What’s the solution – what can they do to achieve an octet?

Cl Cl

Cl Cl Octet: contains 8 electrons

Cl Cl octet circle the electrons for each atom that completes their octets

Cl Cl The octet is achieved by each atom sharing the electron pair in the middle circle the electrons for each atom that completes their octets

Cl Cl This is the bonding pair circle the electrons for each atom that completes their octets

Cl Cl It is a single bonding pair circle the electrons for each atom that completes their octets

Single bonds are abbreviated Cl Cl Single bonds are abbreviated with a dash circle the electrons for each atom that completes their octets

Chlorine is a single bond written as Cl2 circle the electrons for each atom that completes their octets

O How will these two oxygen atoms bond?

O Oxygen atoms are highly electronegative. So both atoms want to gain two electrons.

Both electron pairs are shared.

O O 6 valence electrons plus 2 shared electrons = full octet

O O 6 valence electrons plus 2 shared electrons = full octet

O O two bonding pairs, making a DOUBLE BOND

O O = For convenience, the double bond can be shown as two dashes.

Oxygen is a double bond written as = Oxygen is a double bond written as O2

Naming Covalent Compounds (for compounds made with more than one element) Use “–ide” on the end of the second element Use numerical prefixes on both element names to show how many there are of each

Number of Atoms Prefix 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-

Examples of compounds of N and O: NO nitrogen oxide NO2 nitrogen dioxide N2O dinitrogen oxide N2O4 dinitrogen tetroxide N2O5 dinitrogen pentoxide In most cases, “mono” is understood

Select the correct name for each compound. A. SiCl4 1) silicon chloride 2) tetrasilicon chloride 3) silicon tetrachloride B. P2O5 1) phosphorus oxide 2) phosphorus pentoxide 3) diphosphorus pentoxide C. Cl2O7 1) dichlorine heptoxide 2) dichlorine oxide 3) chlorine heptoxide

Name these compounds CO2 N2O3 BF3 SiO2 SiI4 As2O5 Carbon dioxide Dinitrogen trioxide Boron trifluoride Silicon dioxide Silicon tetriodide Diarsenic pentoxide

Write the Formulas phosphorus pentachloride dinitrogen trioxide sulfur hexafluoride PCl5 N2O3 SF6

QUIZ TIME Only use numeric prefixes for covalent compounds. When is it appropriate to use numeric prefixes in a compound name? Only use numeric prefixes for covalent compounds. Nonmetal + Nonmetal

What does the numerical prefix in a covalent compound tell you? The numerical prefix determines the number of each nonmetal present in the covalent compound. Carbon and Oxygen combine in many different ways to make covalent compounds. How are the formulas of the following different? carbon monoxide carbon dioxide dicarbon trioxide CO CO2 C2O3

Review: Valence Electrons Transferred Aluminum and Chlorine Dot diagrams Charges

Review: Name to Formula Potassium oxide Lead I sulfide Boron phosphide

Review: Formula to Name BeS Fe2O3 CaF2

Review: Valence Electrons Transferred Sulfur and Chlorine Sulfur and Oxygen Dot diagrams Dash structure

Review: Name to Formula Iodine pentafluoride Dinitrogen tetroxide Phosphorous triiodide

Review: Formula to Name CCl4 Si2Br6 CO

Timed Challenge Naming Binary Compounds (Ionic) One – Ten 6 minutes Eleven – Twenty 4 1/2 minutes Naming Binary Compounds (Covalent) One – Seven 4 minutes Eight – Fifteen 3 minutes

Timed Challenge Naming Binary Compounds (Ionic) One – Ten 6 minutes Eleven – Twenty 4 1/2 minutes Naming Binary Compounds (Covalent) One – Seven 4 minutes Eight – Fifteen 3 minutes

Number of Atoms Prefix 1 mono- 2 di- 3 tri- 4 tetra- 5 penta- 6 hexa- 7 hepta- 8 octa- 9 nona- 10 deca-