Chemical Reactions Packet 2 Bonding-REG.

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1 Chemical Reactions Packet 2 Bonding-REG. Ms. Rabenda Name: Period: 1

2 Lewis Dot Diagram Notes Illustrates the number of valence electrons. Valence electrons = Placed around the symbol of the element Helps us determine how compounds are formed / how elements bond The group # gives you the number of valence electrons Drawing Valence Electrons How many valence electrons does Fluorine have? Start at 12:00 with your first dot F Add dots at 3:00, 6:00, and 9:00 moving clockwise until you reach the correct number of valence electrons. F F F You need one dot at each location before you start adding your second dots F F F Lewis Dot Diagram Practice Draw the Lewis Dot Diagram for Phosphorus Phosphorus Symbol: Atomic Number: Atomic Mass: Protons: Neutrons: Electrons: Valance Electrons: P 2

3 Lewis Dot Diagram Worksheet Determine the number of valance electrons. Once you have found the number of valance electrons, place them around the elements symbol. Element Atomic # Atomic Mass Protons Neutrons Electrons Valence Electrons Lewis Dot 1. Carbon dots around the symbol 2. Lithium Li 3. Magnesium Mg 4. Boron B 5. Oxygen O 6. Fluorine F 7. Nitrogen N 3

4 Element Atomic # Atomic Mass Protons Neutrons Electrons Lewis Dot 8. Helium He 9. Potassium K 10.Aluminum 13 Al 10. Beryellium Be 11. Silicon Si 12. Iodine 52 I 13. Chlorine Cl 14. Neon Ne 4

5 Why do Elements Bond? Element # of Valence Electrons Type of Element What happens to the electrons Number of Electrons Gained or Lost Lithium 1 Metal Lose 1 electron Chlorine Sodium Carbon Calcium Beryllium Boron Nitrogen Oxygen Fluorine Hydrogen Magnesium Phosphorous Iodine Lead Sulfur Aluminum Neon Cesium Silicon 5

6 Come Together - A Bonding Experience Purpose: The objective of this activity is to combine the pieces of the paper plate to make a whole plate. You may allow the centers of the plates to sit on top of each other but the outside edges cannot overlap. Each piece can be identified by the letter written in the center of the plate s circle. Questions: 1. What do you observe about the pieces before you begin? BE SPECIFIC! What do you see? 2. How can these pieces come together? Make sure you are discussing what the outer edge looks like. 3. How many combinations can you make? 4. Does it matter which plate combines with which? Why? 5. How many full paper plates were you able to create? Name them by letters What do the dots on the plates represent? 7. What does each of the paper plates represent? 8. What do the combined paper plates represent? 9. If you had a full paper plate, what type of element would that represent? 10. Think about the place each of these plates have on the periodic tables. What does this tell you about certain groups? 6

Bonding Notes Elements Goal = Elements want to be stable In order to be stable they need to fill their outermost energy level completely (oct meaning 8) When outer level is filled No Charge = - When

7 Bonding Notes Elements Goal = Elements want to be stable In order to be stable they need to fill their outermost energy level completely (oct meaning 8) When outer level is filled No Charge = - When outer level is not filled Charge = - How do we figure out and elements charge? Charge is determined by how many electrons they need to gain or lose to complete their outer level Every element in the group has the same charge Example: All Halogens are -1 Logical Order Group Charge 7

8 How can elements complete their octet? Bonds Bonds Forms between and a Forms between a and a Electrons are Electrons are Strong Bonds Weak bonds Hard / Brittle Relatively Soft Soluble in Water Insoluble in water High melting and boiling points Low melting and boiling points Conducts electricity Does not conduct electricity Solid at room temperature Liquids and gases at room temperature Bonds Bond in which one or more electrons from one atom are removed and attached to another atom. It is when atoms electrons One element gives an electron One element takes an electron How does ionic bonding work? Bonds occur between and Opposite charges are going to attract Their charges will cancel out and become 0 0 = Stable Example: = Does NOT equal 0 so you would need another -1 atom (of the same element) 8

9 How does the sharing work? Na has the 1 lone electron to share in its outermost level Cl needs 1 to complete its octet Na will give 1 electron to Cl Bonding Steps Step 1: to determine the number of atoms that are needed Step 2: Write Lewis dot diagrams with showing electron movement Step 3: Write Final Compound Bonding Problem: Sodium and Sulfur Step 1: Write charges to determine the number of atoms that are needed Step 2: Write Lewis dot diagrams with arrow showing electron movement Step 3: Write Final Compound 9

10 Bond Worksheet Using the correct steps, complete each of the ionic bonds below. Elements Lithium and Fluorine Lithium and Oxygen Step 1: Write charges to determine the number of atoms that are needed Step 2: Write Lewis Dot diagrams with arrow showing electron movement Step 3: Write Final Compound Elements Magnesium and Chlorine Calcium and Sulfur Step 1: Write charges to determine the number of atoms that are needed Step 2: Write Lewis Dot diagrams with arrow showing electron movement Step 3: Write Final Compound Elements Cesium and Iodine Potassium and Sullfur Step 1: Write charges to determine the number of atoms that are needed Step 2: Write Lewis Dot diagrams with arrow showing electron movement Step 3: Write Final Compound 10

11 Bond Notes Why do atoms bond? Each atom wants a outermost energy level How do they do this? By gaining, losing, or sharing valence electrons to achieve the duet or octet rule aka: Gives each atom an electron configuration similar to that of a noble gas Ex. Group 18: He, Ne, Ar Types of Bonding Bonds Bonds Forms between a and a Forms between a and a Electrons are Electrons are Strong Bonds Weak bonds Hard / Brittle Relatively Soft Soluble in Water Insoluble in water High melting and boiling points Low melting and boiling points Conducts electricity Does not conduct electricity Solid at room temperature Liquids and gases at room temperature Bonds Definition A chemical bond in which two atoms a pair of valence electrons Always formed between and How to Draw Bonds Step 1: Draw the Lewis Dot structures and circle the electrons that are being shared Step 2: Rewrite the elements with a line representing each shared pair (it replaces the circle) Step 3: Write the final compound Practice: Chlorine and Chlorine Step 1: Draw the Lewis Dot structures and circle the electrons that are being shared 11

12 Step 2: Rewrite the elements with a line representing each shared pair (it replaces the circle) Step 3: Write the final compound 12

13 Bond Worksheet Using the correct steps, complete each of the covalent bonds below. Elements Hydrogen and Chlorine Fluorine and Chlorine Step 1: Write Lewis Dot structures with circle showing the shared electrons Step 2: Rewrite elements with a line(s) representing electron(s) being shared Step 3: Write Final Compound Elements Hydrogen and Oxygen Oxygen and Oxygen Step 1: Write Lewis Dot structures with circle showing the shared electrons Step 2: Rewrite elements with a line(s) representing electron(s) being shared Step 3: Write Final Compound Elements Hydrogen and Nitrogen Hydrogen and Carbon Step 1: Write Lewis Dot structures with circle showing the shared electrons Step 2: Rewrite elements with a line(s) representing electron(s) being shared Step 3: Write Final Compound 13

14 or Electron Dot Structure Review Directions: Complete the boxes below. Remember: bonds happen between metals and non-metals. bonds happen between non-metals and non-metals. Elements or? (circle one) Draw Bond Compound with charges (ionic)/ redrawn with line (covalent) Final Compound Na and F (EXAMPLE) Na +1 F -1 NaF Br and Br Br 2 Mg and O C and H Mg and F N and H 14

15 Elements or? (circle one) Draw Bond Compound with charges (ionic)/ redrawn with line (covalent) Final Compound I and Br K and Br Na and Cl K and N Cl and O N and F 15

Carbon Dioxide - CO 2 Ozone cannot be an example because there aren t two different elements Water - H 2 O All compound are molecules but not all molecules are compounds Simple Molecule Complex

16 Types of Molecules What is the difference between a molecule and a compound? Molecule - When two or more atoms are joined together chemically Examples Carbon Dioxide - CO 2 Ozone - O 3 Water - H 2 O Compound - When two or more elements are joined together chemically Examples Carbon Dioxide - CO 2 Ozone cannot be an example because there aren t two different elements Water - H 2 O All compound are molecules but not all molecules are compounds Simple Molecule Complex Molecule Only a few atoms bonded together Hundreds or thousands of atoms bonded together, in a repeating pattern to form a polymer Possible because carbon atoms form very stable bonds with other carbon atoms Examples: Water molecules (H 2 0) Ammonia (NH 3 ) Methanol (CH 4 O). Examples: Crystals Diamonds Graphite (pencil leads) Counting simple and complex molecules You write each element (elements only have one capital letter) and count how many of them there are 16

17 Types of Molecules Worksheet Molecule Simple/Complex Number of Elements C = O = H = 17

18 Elements of the week Week Clues Element

19 19

Chapter 5 TEST: The Periodic Table name

Chapter 5 TEST: The Periodic Table name HPS # date: Multiple Choice Identify the choice that best completes the statement or answers the question. 1. The order of elements in the periodic table is based