1 / 28

Bonding The way things are joined together

Bonding The way things are joined together. 24 12. Mg. Metal and non-metal. Non-metals only. Metals only. Atoms can be joined together in 3 possible ways. Ionic Bonding. Covalent Bonding. Metallic Bonding.

baskink
Download Presentation

Bonding The way things are joined together

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. Bonding The way things are joined together

  2. 24 12 Mg

  3. Metal and non-metal Non-metals only Metals only Atoms can be joined together in 3 possible ways Ionic Bonding Covalent Bonding Metallic Bonding All three types involve changes in the electrons in the outermost electron shells of the atoms

  4. Ionic bonds + and - charges

  5. n+ Lose 1 or more electrons Neutral atom Positive ion n- Gain 1 or more electrons Neutral atom Negative ion Most ionic compounds contain a metal and a non-metal. When metals react they lose outer shell electrons to leave a full electron shell. This produces a charged atom (ion) with a + charge. When non-metals react with a metal they gain electrons to achieve a full electron shell.

  6. 19 9 F Has ? Electrons in outer shell Does it need to pick up or lose electrons to make the outer shell full

  7. 19 9 F Gains 1 electron Now has more negative electrons than positive protons = a negative charge

  8. 24 12 Mg Loses 2 electrons Now has more positive protons than negative electrons = a positive charge

  9. Loses 1 electron Na+ Na Cl Gains1 electron (from sodium) Cl Sodium atom (2.8.1) Sodium 1+ ion (2.8.0) Chlorine atom (2.8.7) Chlorine I - ion (2.8.8)

  10. + + - + + + opposites attract + - + + + - - - - - - - + - + The oppositely charged ions are attracted into a lattice that gets bigger and bigger until it consists of millions of ions

  11. + + + + + + - - - - - - - - - - - - + + + + + + + + + + + + - - - - - - - - - - + + + + - - - - + + + + + + - - - - - - + + + + + + + + + + - - - - + + + + - - - - + + + + - - - - • We have shown ions attracting and building into a 2 dimensional sheet. In fact the whole process will be going on in three dimensions to build up a giant 3-D lattice.

  12. + + + + - - - - - - - - + + + + + + + + - - - - - + - + + + + - - - - + + + + + - + - + - • Ionic compounds are very brittle. • Opposite charges attract, so neighbouring ions are pulled together. • When something hits the substance a layer of ions will be pushed so that they are next to ions with the same charge. • Attraction becomes: repulsion! Blow

  13. + + - - - - + + + + + + - - - - + - - + - + + - - + + + - + Molten – mobile Does conduct Solid – not free to move Doesn’t conduct - + - • Ionic substances do not conduct electricity as solids. • When molten or dissolved they will conduct (and also undergo electrolysis). • This is because the electricity is carried through the solution by the ions which are free to move when the ionic compound is molten or in solution.

  14. The ionic bonds are very strong. Will that make ionic compounds have a high or low boiling point? High

  15. Covalent bonding Sharing.

  16. Covalent compounds are formed when non-metal atoms react together. • The atoms share electrons

  17. - Figure 1 Figure 2 F F X X F F • Covalent compounds are held together by this sharing of electrons. • A pair of electrons shared in this way is known as a covalent bond. • It is sometimes represented in full bonding diagrams (see figure 1). Often these bonds are just shown as a pair of electrons (xx) or even just a line (see figure 2).

  18. There can be small covalent molecules and large covalent molecules

  19. Cl Cl Cl (2,8,7) (2,8,7) Cl (2,8,8) (2,8,8) Chlorine (2.8.7) needs 1 more electron to attain a full electron shell. Cl-Cl

  20. O O H H H H H H O Hydrogen (1) needs 1 more electron but oxygen (2.6) needs 2 more. Therefore, we need 2 hydrogens.

  21. The bonds between ATOMS that share electrons are STRONG The bonds between molecules that don’t share electrons are WEAK What effect will this have on the melting and boiling points? Will they be high or low? Low

  22. Do these covalent molecules conduct electricity? Will they dissolve in water and spread out like ionic solids? No No

  23. Metallic bond

  24. The protons sit in a sea of electrons Metallic bonding is the attraction of + metal ions for the “sea of electrons.”

  25. Metals are not brittle. • The metal atoms are the same and exist in simple structures. • If something hits the substance, it simply moves to the next layer along. Blow

  26. Like ionic bonds the metallic bonds are strong. Will melting points be high or low? High If the sea of electrons can flow, will metals conduct electricity? yes

More Related