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Chapter 11 Chemical Bonds

Chapter 11 Chemical Bonds. Objectives. 11.1 Describe how a compound differs from the elements that compose it 11.1 Explain what a chemical formula represents 11.1 State a reason why chemical bonding occurs. Objectives. 11.2 Describe ionic and covalent bonds

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Chapter 11 Chemical Bonds

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  1. Chapter 11 Chemical Bonds

  2. Objectives • 11.1Describe how a compound differs from the elements that compose it • 11.1 Explain what a chemical formula represents • 11.1 State a reason why chemical bonding occurs

  3. Objectives • 11.2Describe ionic and covalent bonds • 11.2 Identify the particles produced by ionic bonding and by covalent bonding • 11.2 Distinguish between a polar and nonpolar covalent bond

  4. Objectives • 11.3Describe the dangers posed by hazardous compounds in the home • 11.3 Demonstrate a knowledge of a safer alternative of compounds to use • 11.4 Explain how to determine oxidation numbers

  5. Objectives • 11.4Write formulas for compounds from their names • 11.4 Name compounds from their formulas • 11.4 Describe hydrates and their formulas

  6. Introductory • Elements will have very different properties than the compounds they are in • Examples: Oxygen = Flammable, Gas at Room Temperature • Hydrogen = Flammable, Gas at Room Temperature • Water (A compound of above) = Puts out fire, liquid at room temperature • Many others, consider table salt

  7. Why do Elements come together? • To complete their outer shell • Have a noble gas configuration • Elements which have a full outer shell tend to be chemically stable (unreactive) • A full outer shell consists of 8 valence electrons • In the case of metals, losing all of their valence electrons

  8. 23 BONDING

  9. Bonds Between Atoms Polyatomic Ions Ionic Covalent Metallic Network Solids Molecular Substance Polar Coordinate Covalent Nonpolar What are we going to learn about???

  10. Important Words (Ie On Quiz) • Anion- negative ion • Cation-positive ion • Octet Rule- rule that states that atoms tend to gain, lose, or share electrons so that each atom has full outermost energy level which is typically 8 electrons. • Polyatomic Ion- charged group of covalently bound atoms • Polar-means ‘uneven’ sharing • Molecule-neutral group of atoms united by covalent bonds • Hydrate-molecule surrounded by water • Oxidation number-number of electrons lost or gained • Covalent Bond- formed between 2 nonmetals

  11. Ionic Bonds • What is an Ionic Bond? • An Ionic Bond is a chemical bond resulting from the TRANSFER of electrons from one bonding atom to another • It is composed of positive and negative atoms or particles • When is an ionic bond formed? - An ionic bond is formed when a Metal and Non-Metal come together

  12. What are some characteristics of an ionic bond? • Crystalline at room temperatures • Have higher melting points and boiling points compared to covalent compounds • Composed of Positive and Negative Charges, but do NOT conduct electricity • Corrosion stops batteries

  13. Covalent Bonds • What is an Covalent Bond? • - A covalent bond is a chemical bond resulting from SHARING of electrons between 2 bonding atoms. • What forms a covalent bond? - A covalent bond is formed between two nonmetals.

  14. What are some characteristics of a covalent bond? • Covalent bonds have definite and predicable shapes. • Low melting and boiling points • Is a molecule

  15. Molecules • Composed of COVALENT Bonds • Electrons are shared • Not all elements share equally though • Polar Molecules: Uneven sharing • Have a Positive and Negative side • If you have different elements, will have a Polar Bond • IE If Carbon and Oxygen make a bond, it will be polar • Non-Polar Molecules: Even Sharing • Same element, IE Oxygen

  16. Chemical Formulas • Chemical Formulas tell us how many of each element are in a compound • A ratio for salts (ionic compounds) and an actual number for molecules. • NaOH = 1 Na, 1 O, 1 H • H2O = 2 H, 1 O • Mg(NO3)2 = 1 Mg, 2 N, 6 O • 2 CO2 = 2 C, 4 O

  17. +1 +2 Ionic Charges -3 -2 -1

  18. Formulas of Ionic Compounds Formulas of ionic compounds are determined from the charges on the ions atoms ions  – Na  +  F :  Na+ : F :  NaF  sodium + fluorine sodium fluoride formula Charge balance: 1+ 1- = 0

  19. Writing a Formula Write the formula for the ionic compound that will form between Ba2+ and Cl. Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba2+ Cl Cl 3. Write the number of ions needed as subscriptsBaCl2

  20. Ionic Nomenclature • What is the formula of the following? • Potassium Oxide • K2O • Strontium Chloride • SrCl2 • Magnesium Nitride • Mg3N2

  21. Ionic Nomenclature • Potassium Phosphide • K3P • Magnesium Sulfide • MgS • Radium Flouride • RaF2

  22. Ionic Nomenclature • Binary Compounds of Metals with Fixed Charges: Given Formula, Write the Name • The order for names in a binary compound is first the cation (Metal), then the anion (Non-Metal). • Use the name of cation with a fixed oxidation state directly from the periodic table. • The name of the anion will be made from the root of the element's name plus the suffix "-ide."

  23. Practice Naming • What is the name of the following? • MgO • Magnesium Oxide • NaF • Sodium Flouride • CaS • Calcium Sulfide

  24. Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu+,Cu2+ Fe2+, Fe3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion

  25. Variable Charges • Formula to Name • 1) Find the charge of the cation by • Finding total charge of anion and dividing by number of cations • Example: FeCl3 • We have 3 Chlorines, each has a -1 charge • The Fe needs to be +3 to balance it out • 2) Say the cation with its Roman Numeral • Iron (III) Chloride

  26. Variable Charges • What is the name? • AuF3 • Gold (III) Flouride • AgF • Silver (I) Flouride • PbO2 • Lead (IV) Oxide

  27. Variable Charges • SnF2 • Tin (II) Flouride • MnO2 • Manganese (IV) Oxide • CrN • Chromium (III) Nitride • Sn3N4 • Tin (IV) Nitride

  28. Variable Charges • Name to Formula • The Roman Numeral tells you the charge • Balance the formula • Iron (III) Oxide • Fe has a +3 charge as denoted by the III • Oxygen always has a -2 charge • Cross them (Balance) • Fe2O3

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