WARM UP DAY 1 Take out your notebook

WARM UP – DAY 1 Take out your notebook. Write the Unit topic (Bonding & Nomenclature) on the next page. Copy down these topic objectives. UNIT 3 OBJECTIVES: At the end of this unit I will be able to: � Compare (qualitatively) the relative strengths of ionic, covalent and metallic bonds. � Infer the type of bond and chemical formula formed between atoms. � Compare intra- and inter-particle forces � Interpret the name and formula of compounds using IUPAC Convention. � Compare the properties of ionic, metallic, and network compounds.

UNIT 3 BONDING & NOMENCLATURE

AGENDA ESSENTIAL QUESTION: � How do single atoms come together to form new substances? Warm Up Announcements Bonding Vocabulary Valence Electrons Lewis Dot Structures � Atoms � Ions Exit Ticket

ANNOUNCEMENTS Next Tuesday is the last opportunity to retest for Unit 2. Nuclear Radiation Research is due this Friday!!! Tutoring after school Tuesdays & Thursdays 2: 30 -3: 30. Check Powerschool regularly for updated grades, and to see any work you are missing. Absent? Go to the class website to view

Unit 3 – Subtopic 1: INTRODUCTION TO BONDING - Vocabulary - Valence Electrons - Lewis Dot Structures *** Remember NOTES are in blue!***

INTRODUCTION TO BONDING Create a Frayer chart, crossword, word map, song or other product to describe each of the words on the vocabulary list. � Bond � Network � Ion compoun d � Valence shell � Electron � Cation � Anion � Covalent Make sure you have: • Vocabulary terms (8) • Definition • Example

Introduction to Bonding: Valence Electrons Valence electrons are the electrons found in the outermost shell of the atom. Valence electrons are important because they are the electrons that will react to form bonds with other atoms. For the elements of groups 1 A, 2 A, 3 A, 4 A, 5 A, 6 A, 7 A and 8 A their valence electrons are the same as their group number. � For example: All elements in group 3 A have 3 valence electrons. All elements in group 6 A have 6 valence electrons.

Introduction to Bonding: Lewis Dot Structures Lewis Dot diagrams are a simplified way of representing atomic structure. Lewis Dot diagrams have the element symbol surrounded by dots representing their valence electrons. For example, Chlorine (Cl) is in group 7 A. It has 7 valence electrons so its Lewis Dot diagram looks like this:

Introduction to Bonding: Let’s Practice For the first 20 elements of the periodic table, complete a table with their valence electrons and their Lewis Dot Structures. 2 examples are done for you below: ELEMENT VALENCE LEWIS DOT ELECTRON STRUCTUR S E 1 HYDROGEN 1 … (FILL IN THE OTHER ELEMENTS BETWEEN 1 AND 20) … 20 CALCIUM 2

Introduction to bonding: Ions It’s easy to figure out the charge on atoms – they will gain or lose the number of electrons that make them have a stable valence shell. All elements in Group 1 A have 1 valence electron, so they will lose that 1 electron and have a +1 charge. Fill out these charges on your periodic table: � Grp 1 A: +1 Grp 2 A: +2 Grp 3 A: +3 � Grp 4 A: +/-4 Grp 5 A: -3 Grp 6 A: -2 � Grp 7 A: -1 Grp 8 A: 0 � Grp B elements have ions with variable charges.

Introduction to Bonding: Lewis Dot Structures of Ions Remember: Ions are atoms that have lost or gained electrons. They do this to become stable. All ions have a full valence shell. The Lewis Dot diagram of cations will normally have no electrons (no dots), the symbol and the charge The Lewis dot diagram of anions will always have the symbol, valence shell and charge of the ion.

Introduction to Bonding: Let’s Practice For the following ions, write the number of valence electrons they have, and the Lewis Dot structures. ION Ca 2+ P 3 Mg 2+ H+ At- VALENCE LEWIS DOT ELECTRONS STRUCTURE

EXIT QUIZ Answer these questions about the element Francium: 1. 2. 3. 4. What group number is it? How many valence electrons does it have? Draw the Lewis Dot structure of its atom. What is the formula of the ion it will form?

WARM UP Complete the Chemistry class and teacher report card you got on the way in to class today. DO NOT WRITE YOUR NAME ON THE PAPER. When you are done, turn in your paper so I can give you a warm up grade for this week. TURN IN VOCABULARY ACTIVITIES FROM YESTERDAY!!!

UNIT 3 BONDING & NOMENCLATURE

AGENDA ESSENTIAL QUESTION: � How do single atoms come together to form new substances? Warm Up Announcements Ahmed Mohammed Lewis Dot Structures � Atoms � Ions Ionic Bonding Class Discussion Exit Ticket

ANNOUNCEMENTS Next Tuesday is the last opportunity to retest for Unit 2. Nuclear Radiation Research is due today!!! (Blocks 1 & 3 have until Monday to turn work in). Tutoring after school Tuesdays & Thursdays 2: 30 -3: 30. Check Powerschool regularly for updated grades, and to see any work you are missing. Absent? Go to the class website to view

Introduction to bonding: Ions It’s easy to figure out the charge on atoms – they will gain or lose the number of electrons that make them have a stable valence shell. All elements in Group 1 A have 1 valence electron, so they will lose that 1 electron and have a +1 charge. Fill out these charges on your periodic table: � Grp 1 A: +1 Grp 2 A: +2 Grp 3 A: +3 � Grp 4 A: +/-4 Grp 5 A: -3 Grp 6 A: -2 � Grp 7 A: -1 Grp 8 A: 0 � Grp B elements have ions with variable charges.

Introduction to Bonding: Lewis Dot Structures of Ions Remember: Ions are atoms that have lost or gained electrons. They do this to become stable. All ions have a full valence shell. The Lewis Dot diagram of cations will normally have no electrons (no dots), the symbol and the charge The Lewis dot diagram of anions will always have the symbol, valence shell and charge of the ion.

Introduction to Bonding: Let’s Practice For the following ions, write the number of valence electrons they have, and the Lewis Dot structures. ION Ca 2+ P 3 Mg 2+ H+ At- VALENCE LEWIS DOT ELECTRONS STRUCTURE

Covalent vs Ionic Compounds In this lab, we observe the conductivity, and structure of covalent and ionic compounds. Complete this table as you visit the station: IONIC COMPOUNDS COVALENT COMPOUNDS Example Conductivity as a solid Conductivity when dissolved Appearance under microscope

Unit 3 – Subtopic 2: IONIC BONDING - What is ionic bonding? - Swap, Drop & Chop - Nomenclature of Ionic Compounds *** Remember NOTES are in blue!***

IONIC BONDING Ionic bonds occur to make the atom more stable. They may happen between: �A metal and a non-metal � A polyatomic ion and a metal or non-metal Ionic bonds involve electrons being transferred from one atom to another.

Ionic Bonding: Properties of Ionic Compounds Electronegativity difference ( EN) is above 1. 7 High melting points High boiling points Brittle, crystalline solids at room temperature High electrical conductivity when melted or dissolved in water

Ionic Bonding For example: � Na is a metal with 1 valence electron. It needs to lose that electron to become stable. � Cl is a non-metal with 7 valence electrons. It needs 1 more electron to achieve stability. � Na will transfer its 1 electron to Cl forming Na. Cl.

Ionic Bonding: Let’s Practice Use Lewis Dot diagrams to show the ionic bonds formed between: � Potassium & Fluorine � Magnesium and Oxygen � Lithium and Sulfur � Aluminum & Bromine � Calcium and Phosphorus

Ionic Bonding: Swap, Drop & Chop There is an easier way to determine formula than using Lewis Dot Diagrams. It is called Swap, Drop and Chop. Swap the charges of the two ions Drop the signs. Chop (divide) the numbers to their smallest ratio.

Ionic Bonding: Swap, Drop and Chop On your index card you have the formula of either a cation or an anion. Find at least three other people to bond with. Remember – cations can only bond with anions and anions can only bond with cations. Write out the swap, drop and chop steps for each person you bond with on the back of your index cards. Turn this in to me for a grade when you are done.

Ionic Bonding: Nomenclature To Name Ionic Compounds: Separate the two ions that form the compound. Name the cation first – give it the name of the element. (Transition elements ** Name the anion second. For elements, write the name of the element then replace the ending with -ide. **Polyatomic ions use their own names (as listed in your reference table).

Unit 3 – Subtopic 3: COVALENT BONDING - What is covalent bonding? - Nomenclature of Covalent Compounds *** Remember NOTES are in blue!***

COVALENT BONDING Covalent bonds occur to make the atom more stable. They happen between 2 or more nonmetals. Ionic bonds involve electrons being shared between atoms.

Covalent Bonding: Properties of Covalent Compounds Electronegativity difference ( EN) is below 1. 7 Low melting points Low boiling points Polar substances Poor electrical conductivity

Covalent Bonding For example: � Cl is a non-metal with 7 valence electrons. It needs 1 more electron to achieve stability. � Two Cl atoms can share one electron, each ending up with a full outer shell and forming Cl 2.

Covalent Bonding: Let’s Practice Use Lewis Dot diagrams to show the ionic bonds formed between: � Oxygen & Oxygen � Sulfur and Oxygen � Phosphorus and Sulfur � Bromine & Bromine

Covalent Bonding – Bond Strength and Length Single bonds are formed when one pair (2) of electrons is shared between atoms. They are the longest type of bond, but they are also the weakest type of bond. Double bonds are formed when two pairs (4) of electrons are shared between atoms. They are shorter and stronger than single bonds. Triple bonds are formed when three pairs (6) of electrons are shared between atoms. They are the shortest type of bond. They are also the strongest type of bond.

Covalent Bonding: Nomenclature Use a prefix to represent the subscript of the 1 st element written. Name the first element. Use a prefix to represent the subscript of the 2 nd element written. Name the second element as if it were an anion (with an –ide ending). NUMBER PREFIX 1 Mono- 2 Di- 3 Tri- 4 Tetra- 5 Penta- 6 Hexa- 7 Hepta- 8 Octa- 9 Nona- 10 Deca-

Unit 3 – Subtopic 4: METALLIC BONDING - Structure of Metallic Compounds *** Remember NOTES are in blue!***

METALLIC BONDING Metallic bonds occur between metals. Metallic bonds are often described as metal ions surrounded by a sea of mobile electrons.

Metallic Bonding: Properties of Metallic Compounds High melting points High boiling points High conductivity Malleable and ductile Lustrous (shiny)

Metallic Bonding Instead of transferring or sharing electrons, metal atoms will lose electrons which can then move around to other atoms. The electrons can then easily carry energy in the form of heat or electricity around the sample.

Unit 3 – Subtopic 5: INTERMOLECULAR BONDING - Strength of bonds - Bond Length & Bond energy - *** Remember NOTES are in blue!***

INTERMOLECULAR BONDING Intermolecular bonding is the type of bond that holds similar particles together. There are three main types that we will focus on: � Hydrogen bonds � London Dispersion forces (van der Waals Forces) � Dipole forces

Unit 3 – Subtopic 5: BONDING – MOLECULE SHAPES - Polarity - VSEPR Theory - *** Remember NOTES are in blue!***

MOLECULE SHAPES – VSEPR Theory

Bonding Shapes: Polarity