1 / 22

Understanding Chemical Bonds: Ionic, Covalent, and Metallic Bonds Explained

Chemical bonds form when atoms gain, lose, or share electrons. This article explores three primary types of bonds: ionic, covalent, and metallic. Ionic bonds involve charged ions attracting each other, while covalent bonds form through shared electrons between atoms. Metallic bonds create a "sea of electrons" that allows metals to conduct electricity. We also discuss properties of each bond type, oxidation numbers, and how atoms achieve stability through electron transfer or sharing.

drew-bray
Télécharger la présentation

Understanding Chemical Bonds: Ionic, Covalent, and Metallic Bonds Explained

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Kinds of Bonds

  2. Chemical Bonding Chemical Bondsare formed when atoms gain, lose, or share electrons

  3. Ionic Bonding • An ion is a charged particle – it has a different number of electrons than protons • An ionic bondis the attractive force between the opposite charges of the ions

  4. Ionic Bonding

  5. Types of Ions • A cationhas a positive charge • An anion has a negative charge

  6. Ionic Bond Formation • Ionic substances form crystals because they connect to all of the neighboring opposite charges.

  7. Properties of Ionic Compounds • Hardand brittle • Solid at room temperature • Have very high melting points and boiling points

  8. Properties of Ionic Compounds • Can conduct electricity if heated to a liquid state • Can conduct electricity if dissolved in water or some other solvent

  9. Examples • NaCl (salt) • NaF (in toothpaste) • NaOH (Drano)

  10. Covalent Bonding • A covalent bond forms when atoms share electrons • A single bond contains one pair of electrons, but atoms can share multiple pairs of electrons.

  11. Covalent Bonding • Connect lone single dots of Lewis structure to show covalent bonds

  12. Covalent Properties • Some arehard and brittle but less than ionic; Others are flexible, or soft and mushy. • Can be solid, liquid or gas at room temperature. • Their boiling pointsvary from -253°C to over 4800°C.

  13. Covalent Properties • Most do not conduct electricity regardless of their state of matter. • When dissolved in a solvent, they don’t conduct electricity.

  14. Examples • C12H22O11 (Sugar) • NH3 (Ammonia) • C3H8 (Propane)

  15. Metallic Bonds • A metallic bond involves an attraction between metal atoms that loosely involves many electrons. • We call this a “Sea of Electrons”

  16. Metallic Bonds • Many electrons are moving around the metal which makes the metal highly conductive to heat andelectricity.

  17. Oxidation/“Magic” Numbers • Atoms gain / lose electrons to form an ionic bond to get to the magic number of0 or 8 • Oxidation is how many electrons you will gain or lose to get to 0 or 8. (basically it’s the charge!!!)

  18. Oxidation/“Magic” Numbers

  19. Oxidation Numbers • If an atom gains electrons, it has a negative oxidation number. • If an atom loses electrons, it has a positive oxidation number.

  20. Oxidation Numbers • For Bonding: Oxidation means CHARGE!!!!!!

  21. What is the oxidation number (charge) of: H Ba S F Na Si

  22. Polyatomic Ions A polyatomic ion is a covalently bonded groupof atoms with either a positive or negative charge We will revisit this later, but understand what it is.

More Related