1. Metallic Bonding
The transition metals and Lanthanide/Actinide series hold their outermost electrons loosely
This allows for metallic bonds – groups of metals held together in which their electrons are free to flow to different atoms

5. Electronegativity and Covalent bonds

6. Electronegativity An atom’s ability to attract another electron
Electronegativity increases across a period
It decreases down a group

8. Covalent bonds
A bond in which two atoms are held together due to shared electrons

9. Single bond Double bond Triple bond One pair of electrons is shared
Two pairs shared
Triple bond
Three pairs shared

10. Polarity
When one element in a covalent bond has a higher electronegativity than the other, it holds the shared pair of electrons closer to its nucleus
This side of the molecule becomes slightly negative, and the other side slightly positive
This is known as polarity

11. The slightly charged ends of a polar molecule are known as dipoles
The more electronegative side is called partially negative; the less electronegative side is called partially positive

12. Nonpolar covalent bonds
When there are no partial charges, the bond is nonpolar
Nonpolar covalent bond vs. nonpolar covalent molecule
Some molecules are nonpolar because their partial positives cancel each other out

13. Hydrogen Bonds in water

17. Cohesion: Water molecules are attracted to other water molecules
Adhesion: Water molecules are also attracted to other polar surfaces
Capillary action: water moving up a thin tube against gravity

19. Surface Tension

20. Surface Tension

21. Rain drops
Right (under ideal conditions)
Wrong

24. Hydrophobic materials