Mechel Golenberke: My First Website
Chapter 6 Chemical Bonds
http://www.nclark.net/Compounds
Chapter 6 Vocabulary Worksheet & Chapter 6 Word Search (day 1)
Chapter 6 Summary (day 1)
Chapter 6 Pre-Test
6.1 Ionic Bonding
6.1.1 Recognize stable electron configurations
6.1.2 Predict an element’s chemical properties using number of valence electrons and electron dot diagrams
6.1.3 Describe how an ionic bond forms and how ionization energy affects the process
6.1.4 Predict the composition of an ionic compound from its chemical formula
6.1.5 Relate the properties of ionic compounds to the structure of crystal lattices
- When the highest occupied energy level of an atom is filled with electrons, the atom is stable and not likely to react.
- Some elements achieve stable electron configurations through the transfer of electrons between atoms. An ionic bond forms when electrons are transferred from one atom to another.
- The properties of an ionic compound can be explained by the strong attraction s among ions within a crystal lattice.
electron dot diagram – a diagram of an atom, ion or molecule in which each dot represents a valence electron
ion – an atom or group of atoms that has a positive or negative charge
anion – an ion with a negative charge
cation – an ion with a positive charge
chemical bond – the force that holds atoms or ions together as a unit
ionic bond – the force that holds cations and anions together
chemical formula – notation that shows what elements a compound contains and the ratio of the atoms or ions of these elements in the compound
Stephen C Murray Notes: 19:1 Metal vs. Non-metals, Dot Diagrams, Ions
6.1 Interest Grabber (day 1)
Review models of electrons:
- First review chart from 4.3
- Then http://hyperphysics.phy-astr.gsu.edu/hbase/pertab/perlewis.html
(Electron Distributions Into Shells for the First Three Periods)
The chemical elements represented by their electron shell diagrams, which are sorted by atomic number. Note: these images are extremely simplified from reality and should only be used to illustrate the number of electrons in their shells.
- Then virtual periodic table: http://chemicalelements.com/
6.1 PowerPoint (64 slides) & Note Guide (begin day 2 & finish day 3)
6.1 Reading & Study Workbook (due day 4, go over day 5)
Brightstorm: Chemical Bonds Ionic Bond (5:11)
In an ionic bond, two ions are held together by electrostatic force. These two atoms are trying to attain full valence shells of eight electrons. One atom has too many electrons and another has too few so one atom donates electrons and the other accepts them. The donor atom forms a cation, or positively charged ion and the other forms an anion, a negatively charged ion. The two are held together by the electrostatic attraction between opposite charges.
Brightstorm: Chemical Bonds Ionic Compound Properties (5:05)
Ionic compound properties stem from their structure. Ionic compounds are found in lattice structures, making them extremely brittle. Ionic compounds have high melting points and form electrolytic solutions, which conduct electricity. Covalent compounds, on the other hand, are comparatively soft and round, have relatively low melting and boiling points and form non-electrolytic solutions.
Prentice Hall Worksheets – do together (day 5)
- Charting Oxidation Number – correlates well with Brightstorm Ionic Bond video
- Bonding & Chemical Formulas – correlates well with Brightstorm Ionic Bond video
*Need to review polyatomic ions: "Learning Chemical Formulas" PowerPoint presentation. (slides 1-5) – especially if doing worksheet below:
Writing Formulas for Ionic Compounds (Chapter 6 Math Skills) (day 4) – includes polyatomic ions – find better worksheet from nclark
A worksheet on writing formulas for ionic compounds
Section 6.1 Ionic Bonding (6.1 Math Skills & Problem Solving) (day 4)
A good worksheet for writing chemical formulas with rules for writing them
Have students play "Formulas Poker"
6.2 Covalent Bonding
6.2.1 Describe how covalent bonds form and the attractions that keep atoms together in molecules
6.2.2 Compare polar and nonpolar bonds, and demonstrate how polar bonds affect the polarity of a molecule
6.2.3 Compare the attractions between polar and nonpolar molecules
- The attractions between the shared electrons and the protons in each nucleus hold the atoms together in a covalent bond.
- When atoms form a polar covalent bond, the atom with the greater attraction for electrons has a partial negative charge. The other atom has a partial positive charge.
- The type of atoms in a molecule and its shape are factors that determine whether a molecule is polar or nonpolar.
- Attractions between polar molecules are stronger than attractions between nonpolar molecules.
covalent bond – a chemical bond in which two atoms share a pair of valence electrons
molecule – a neutral group of atoms that are joined together by one or more covalent bonds
polar covalent bond – a covalent bond in which electrons are not shared equally
Stephen C Murray Notes: 19:2 Bonding, 19:3 More Chemical Bonding
6.2 PowerPoint (30 slides) & Note Guide
Nice Ionic & Covalent Animation/Tutorial (about 15 minutes to go through) - do instead of Brightstorm
Brightstorm: Chemical Bonds Lewis Electron Dot Diagram (8:38)
Lewis Electron Dot Diagrams are used to visually depict bonding by representing valence electrons as dots surrounding an elemental symbol. These dots can be on any of the four sides of the symbol, each side representing a different orbital (1 s orbital and 3 p orbitals).
Brightstorm: Chemical Bonds Covalent Bonds (2:35)
Molecules are bound by covalent bonds in which two atoms with unfilled valence shells share electrons so that they each have a full octet. If one atom is more electronegative than the other, it holds onto the shared electrons more tightly, pulling the negatively charged electron cloud towards itself and resulting in an imbalance of charges called polarity. If a single covalent bond isn’t enough for two atoms to fill their octets, they may share two or more pairs of electrons.
Brightstorm: Chemical Bonds Polarity (5:12)
The eletronegativity of the atoms involved in bonding determines the polarity of the bond. Electronegativity is a quantitative measure of how tightly an atom holds onto its electrons. Polarity has a great effect on solubility and other chemical interactions because polar and non-polar molecules do not like to interact.
Prentice Hall Worksheets together:
More Worksheets together:
"Bonding Basics - Ionic Bonds"
"Bonding Basics - Covalent Bonds"
On Own:
"Bonding Basics Practice Page"
Website: Ionic & Covalent Bonding Tutorial
"Polar Bears and Penguins" activity
Investigation 6B Comparing Ionic & Molecular Compounds
6.3 Naming Compounds and Writing Formulas
6.3.1 Recognize and describe binary ionic compounds, metals with multiple ions, and polyatomic ions
6.3.2 Name and determine chemical formulas for ionic and molecular compounds
- The name of an ionic compound must distinguish the compound from other ionic compounds containing the same elements. The formula of an ionic compound describes the ratio of the ions in the compound.
- The name and formula of a molecular compound describe the type and number of atoms in a molecule of the compound.
polyatomic ion – a covalently bonded group of atoms that has a positive or negative charge and acts as a unit
6.3 PowerPoint (44 slides) & Note Guide
Prentice Hall Worksheet
C Stephen Murray Review Sheets
19.1 Metals vs. Nonmetals; Dot Diagrams; Ions
19.2 Bonding
19.3 More Chemical Bonding
19.4 Naming Compounds
19.5 More Making & Naming
19.6 Even More Making & Naming
Investigation 6A Playing the Ionic Compound Card Game
Brightstorm: Chemical Bonds Naming Covalent Compounds (2:25)
In naming covalent compounds, each element in a covalent compounds needs a prefix to denote the number of atoms of that element. These prefixes are Greek (mon-, di-, tri-, etc) and the last element in the formula also gets the suffix "-ide."
Brightstorm: Chemical Bonds Naming Ionic Compounds (6:51)
When naming ionic compounds, we always name the cation first with its full scientific name. Then, we name the anion, cutting off the last syllable and adding the suffix “-ide”. Sodium chloride, for instance, is an ionic compound containing sodium and chlorine.
6.4 The Structure of Metals
6.4.1 Describe the structure and strength of bonds in metals
6.4.2 Relate the properties of metals to their structure
6.4.3 Define an alloy and demonstrate how the composition of the alloy affects its properties
- The cations in a metal form a lattice that is held in place by strong metallic bonds between the cations and the surrounding valence electrons.
- The mobility of electrons within a metal lattice explains some of the properties of metals.
- Scientists can design alloys with specific properties by varying the types and amounts of elements in the alloy.
metallic bond – the attraction between a metal cation and the shared electrons that surround it
alloy – a mixture of two or more elements, at least one of which is a metal, that has the characteristic properties of a metal
6.4 PowerPoint (25 slides) & Note Guide
Brightstorm: Chemical Bonds Metallic Bond (2:30)
A metallic bond shares electrons but unlike ionic bonds, it does not fill the valence shell octets of the bonding atoms. All of the electrons involved form one huge electron cloud which all the nuclei share. The attraction of the nuclei to the electrons keeps them together. Metallic solids are very conductive because of this electron cloud and are malleable.
**Review Bonds: Hippocampus/Kahn Academy – Chemistry: Ionic, Covalent & Metallic Bonds
More Brightstorm:
Brightstorm: Chemical Bonds Hydrates (2:33)
Hydrates are solid compounds which contain water. This water is included with the chemical formula of the compound because there is a set ratio of water to compound.
Brightstorm: Chemical Bonds Hybridization (6:14)
Hybridization occurs when an atom bonds using electrons from both the s and p orbitals, creating an imbalance in the energy levels of the electrons. To equalize these energy levels, the s and p orbitals involved are combined to create hybrid orbitals. Hybridization is a key concept in valence bond theory, but alternate models are proposed in molecular orbital theory.
Brightstorm: Chemical Bonds Intermolecular Forces (5:39)
Intermolecular forces are forces that hold two molecules together. Dispersion forces (also called Van der Waals Forces) act on all molecules and are the only forces between two non-polar molecules. Two polar molecules are held together by the electrostatic attraction between their dipoles in dipole - dipole force. The strongest type of intermolecular force is hydrogen bonding.
Brightstorm: Chemical Bonds VSPER Model (5:37)
The VSEPR model stands for Valence Shell Electron Pair Repulsion model. The VSEPR model is a model which predicts the geometrical shapes of molecules based on the repulsion between their lone pairs. Types of VSEPR structures include linear, trigonal planar and tetrahedral.
