St. George's College Subject: 8th CHEMISTRY
Teacher's notes
Objectives
Class: Inorganic Compounds
Vocabulary Link and Learn
Date:
In‐Class Survey
November 2nd
Prepared by
2009 1
___ C5H10 + ___ O2 ___ CO2 + ___ H2O
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8th Milton A ‐ Inorganic Compounds Name
Oral Intervention
Blackmark
Sergio María Fernanda Alejandra Almendra Anna Paula Sandra E‐C Maia María Belén Alfredo Kinley Arianne Sandra M. Fiorella Cristina Giulia Jaime Stefano Bruno
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8th Milton Alpha ‐ Inorganic Compounds Name
Oral Intervention
Blackmark
Marcelo Antonella Paulo Alejandro Brenda Diego Gabriel Valeria Giuliana Joshua María Gracia Gonzalo N. Rodrigo Paolo Gonzalo R. Giorgio Nicolás María Claudia
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Let's remember previous learned concepts...
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What are two main types of Chemistry?
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New knowledge beginning......
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Classification I • Inorganic compounds can be classified in different ways. • A common method is based on the constant presence of certain specific elements. For example: • Oxides, always contain one or more Oxygen atoms. • Hydrides, contain one or more atoms of Hydrogen. • Halogens, contain one or more Halogen atoms (group VIIA).
http://bit.ly/4xs9of
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Classification II • Another way to classify inorganic compounds is based on the types of chemical bonds that are present in the compound. • Ionic compounds contain ions are bonded by the electrostatic forces of opposite charges in the compound's ions. For example: Table Salt (Na+Cl‐). • Molecular compounds, contain elements formed by sharing electrons. For example: Water (H20).
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http://bit.ly/FEKdp
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Classification III • A third type of classification considers the possible specific reactivity of inorganic compounds depending on the type of chemical reactions they can go through. • Acids are compounds that produce H+ ions (protons) when dissolved in aqueous solutions. Example: HCl (Chlorhydric Acid), H2SO4 (Sulphuric Acid). • Bases, on the other side, are proton acceptors. Example: NaOH (Sodium hydroxide).
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Chemical Functions • This type of classification referring to an atom, or group of atoms called functional group. They're common for a group of chemical compounds. • The functional group determines the chemical properties common to the group of compounds.
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INORGANIC COMPOUNDS
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Inorganic Compounds • Inorganic compounds can be: Binary, when they're made up of two different elements: CuO, NaO; Ternary, if they're formed by three different elements: Ba(OH)2; Cuaternary, if they're formed by four different elements: NaHSO4.
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NOMENCLATURE
SYSTEMATIC NOMENCLATURE • To name chemical compounds using this technique, you must use number prefixes: MONO_ (1), DI_ (2), TRI_ (3), TETRA_ (4), PENTA_ (5), HEXA_ (6), HEPTA_ (7), OCTA‐ (8), NONA_ (9), DECA_ (10), etc... Examples: Cl2O3 Dichloric trioxide I2O Diiodine monoxide CO2 Carbon dioxide
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NOMENCLATURE
STOCK NOMENCLATURE • In this type of nomenclature, when the element forming the compound has more than one valence, it is indicated at the end of the name with roman numbers in parenthesis. Examples: Fe(OH)2 Iron hydroxide (II) Fe(OH)3 Iron hydroxide (III)
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NOMENCLATURE
TRADITIONAL NOMENCLATURE • In this nomenclature, prefixes and suffixes must be used to distinguish the valence the chemical compound is using: Examples:
ENGLISH
SPANISH
3 Valences 4 Valences hypo‐ ‐ous hipo‐ ‐oso 2 Valences
1 Valence
‐ous ‐oso ‐ic ‐ico (hy)per‐ ‐ic (hi)per‐ ‐ico
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OXIDES
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OXIDES • These are the compounds where Oxygen is combined with other element. • Almost all elements form oxides (except noble gases and halogens), and their properties vary from the place in the periodic table of the element combined with Oxygen. • Oxides are classified in: Basic or Metallic Oxides, and Acid Oxides.
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http://bit.ly/AOCta
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OXIDES • These are the compounds where Oxygen is combined with other element. • Almost all elements form oxides (except noble gases and halogens), and their properties vary from the place in the periodic table of the element combined with Oxygen. • Oxides are classified in: Basic or Metallic Oxides, and Acid Oxides.
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BASIC OXIDES • Also called Metallic Oxides, they are binary ionic compounds that result from combining a metal and Oxygen. • They're crystalline solids formed by a metallic cation and an oxide anion (O2‐). • These oxides typically react with water to form Bases or Hydroxides. • When the metal combined is farther to the left in the periodic table, the oxide will have a stronger ionic bond.
http://bit.ly/nObOs
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EXERCISES Pb + O2 → PbO2 Name: Na + O2 → Na2O Name: 2Fe + O2 → 2FeO Name: Fe + O2 → Fe2O3 Name:
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ACID OXIDES • Also called Nonmetal Oxides. • Are binary covalent compounds resulting from the combination of Oxygen and Non‐Metals. • These oxides are from elements located at the right side of the periodic table, and with more covalent character for those elements located in the upper part of the groups. • Their aqueous solutions form acids.
C + O2 → CO2 Name:
S + O2 → SO3 Name: 25
HYDROXIDES
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HYDROXIDES • Are compounds that result from the combination of a basic oxide and water. • The hydroxides from alkaline metals (Lithium, Sodium, Potassium, Radius and Cesium) are the stronger and more stable ones. • The hydroxides from metals such as: Magnesium, Iron, Bismuth, Nickel and Copper, are less soluble in water, but can still neutralize acids. CaO + H2O → Ca(OH)2 Name: Na2O + H2O → Na(OH) Name: Fe2O3 + H2O → Fe(OH)3 Name: 27
ACIDS
• Their characteristics are opposed to those of hydroxides. • According to Arrhenius, an acid is a substance that releases protons in an aqueous solution (H+); and a base releases hydroxide ions (OH‐). • According to Bronsted‐Lowry, an acid is a substance that releases protons (H+), and a base is an acceptor of protons. ARRHENIUS: H2O(l) + H2O(l) is in equilibrium with H3O+(aq) + OH‐(aq)
BRONSTED‐LOWRY:
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OXOACIDS • Are the substances that result from the combination of an acid oxide and water. • It's a type of acid that contains Oxygen, hence the name.
SO2 + H2O → H2SO3 Name: N2O5 + H2O → HNO3 Name:
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HYDRACIDS • Are binary compounds that result from the combination of Hydrogen with a Halogen from group VIIA or from group VIA.
HF HCl HI
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SALTS
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SALTS • Salts are ionic compounds, which result from the combination of an acid and a base. • They're formed by cations from bases or anions from acids, in these reactions water is always produced.
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OXOACID SALTS • Are the compounds that result from the combination of an oxoacid with a base, where the substitution can be total as in neutral oxosalts; or partial as acid and basic oxosalts. • Are ionic compounds, that have ionic bond between cations and radicals. • Their important property es conducting electricity in solutions.
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HYDRIDES
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HYDRIDES • They're binary compounds that result from combining Hydrogen with other element. • Almost all elements are capable of forming hydrides. • Metals have a positive valence (+), and Hydrogen works with a negative valence (‐1). • The combinations of hydrogen with no metals have a predominantly covalent bond, therefore are covalent bonds. • The combinations of alkaline metals and alkaline earth metals have predominantly an ionic bond.
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METALES
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NON足METALS
HYDROGEN 37
Objectives • Identify the types of Inorganic Compounds. • Identify metal and non‐metal oxides. • Remember and apply the Valences of Elements. • Perform chemical reactions involving: Hydrogen, Oxygen, Water, Metals, Non‐Metals, Acids and Bases.
Note: All, or most, of the objectives will be covered during class time, however the student must be responsible for those objectives not covered or concluded.
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Vocabulary • • • • • •
Reactant Product Reversible Decomposition Synthesis Balancing
Note: Most of the vocabulary words will be covered during class time, however the student must be responsible for those words not covered or concluded.
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Prepared by
Gerardo LAZARO Science Lead Teacher Email: glazaro@sanjorge.edu.pe Wiki: http://science‐learning2009.wikispaces.com Blog: http://learningandscience.blogspot.com Twitter: http://twitter.com/glazaro
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Link and Learn You can visit the following websites to improve your understanding on the present topic: • • • • • • •
http://bit.ly/rGJuh http://bit.ly/1FkjYu http://goldbook.iupac.org/index.html http://bit.ly/SJXue http://science‐learning2009.wikispaces.com http://learningandscience.blogspot.com http://libraryatstgeorge.blogspot.com
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