BONDING. Objectives 3.2, 3.3, 3.4, 3.5, 3.8 and 3.9. Tuesday, October 8, 13
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1 BONDING Objectives 3.2, 3.3, 3.4, 3.5, 3.8 and 3.9
2 3.2 DESCRIBE HOW AN ATOMS ELECTRON CONFIGURATION, PARTICULARLY THE VALENCE ELECTRONS, DETERMINE HOW ATOMS INTERACT WITH OTHER ATOMS Atoms will gain or lose electron to achieve a noble gas electron configuration (8 valence electrons, an octet) Ionic compounds: cations lose electrons to anions so that each atom in the compound has eight valence electrons Covalent compounds: valence electrons are shared so that each atom in the compound has 8 valence electrons
3 3.3 GIVEN ELEMENTS, PREDICT WHETHER THEY WILL FORM A COVALENT MOLECULE OR IONIC LATTICE. Ionic compounds: Formed between a cation (usually a metal) and an anion (a non-metal or a polyatomic ion) These are known as ionic lattice structures Covalent compounds: Formed between two non-metals These form covalent molecules
4 3.4 IDENTIFY PROPERTIES OF A COVALENT MOLECULE, IONIC LATTICE, AND NETWORK COVALENT STRUCTURES. Molecular (covalent) compounds Melting and boiling points: Molecular substances tend to be gases, liquids or low melting point solids Solubility in water: Most molecular substances are not soluble (or only very sparingly soluble) in water. Most are soluble in non-polar solvents such as oil Electrical conductivity:molecular substances won't conduct electricity
5 3.4 IDENTIFY PROPERTIES OF A COVALENT MOLECULE, IONIC LATTICE, AND NETWORK Ionic compounds COVALENT STRUCTURES. Melting and boiling point: Ionic compounds have a high melting and boiling point. Solubility: Ionic compounds are soluble in water (although not all). They are not soluble in non-polar solvents such as oil Electrical conductivity: Ionic compounds and other ionic substances will conduct electricity when they are dissolved in a liquid such as, water or when they are molten (liquid). They do not conduct electricity in their solid form.
6 3.5 USE ELECTRONEGATIVITY VALUES TO PREDICT WHETHER A BOND IS IONIC OR COVALENT Electronegativity - attraction of a nucleus for outside electrons. Pauling scale is used to measure A difference of 1.8 unit or more is considered an ionic bond. From 0 to 1.7 is a polar covalent bond and no difference is a covalent bond Remember electronegativity increases across a period and decreases down a group Determine if a bond between the following atoms is ionic or covalent. (pg 403) H-H, S-H, Cl-H, Na-Cl
7 3.8 GIVEN A COMPOUND IDENTIFY THE DIFFERENT TYPES OF BONDS PRESENT Ionic bonds - form between a cation and anion cations: metals and ammonium ion anions: non-metals and polyatomic ions Covalent bonds - form between two nonmetal elements Polyatomic ions are held together with covalent bonds
8 3.7 EXPLAIN THE PROPERTIES OF METALS IN TERMS OF BONDING Metallic bonding - known as the electron sea model. Electrons are free to flow amongst the metal atoms Metals... Conduct electricity very well Conduct heat very well Are malleable and ductile Mix with other metal to form alloys
9 3.9 DESCRIBE HOW CARBON BONDS WITH H, O, N, S TO FORM CHAINS, RINGS, BRANCHING NETWORKS WHICH ARE CHARACTERISTIC OF POLYMERS, FOSSIL FUELS, AND LARGE BIOMOLECULES. Carbon has unusual ability to bond strongly to itself. This results in long chains or rings of carbon atoms Carbon also forms strong bonds to non-metals such as, hydrogen, nitrogen, oxygen and sulfur
10 3.9 DESCRIBE HOW CARBON BONDS WITH H, O, N, S TO FORM CHAINS, RINGS, BRANCHING NETWORKS WHICH ARE CHARACTERISTIC OF POLYMERS, FOSSIL FUELS, AND LARGE BIOMOLECULES. Examples of carbon containing compounds Polymers: polyethylene, PVC, nylon, polyester Biomolecules: Amino acid/ proteins, DNA, triglycerides (fat), carbohydrates Fossil fuels: Coal, Petroleum
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