Chemical Bonds are the glue that holds atoms together in compounds Chemical Bonds are formed by electrons

Ionic Bonds click + - + - click Magnetism

Ionic Bond – the electrical attraction between a negative ion and a positive ion.

e- Chlorine e- e- e- e- e- P+ N e- e- e- e- e- e- e- e- e- e- e-

Chlorine e- e- e- e- e- e- P+ e- e- e- e- e- e- e- e- e- e- e- e- 17 protons e- e- e- 17 neutrons e- e- 18 electrons Negative ion P+ N e- e- e- e- e- e- e- e- e- e- e- e-

Sodium e- e- e- P+ e- e- e- e- e- e- e- e- 11 protons 11 neutrons 10 electrons Positive ion P+ N e- e- e- e- e- e- e- e-

Salt Chlorine Sodium Sodium Cloride NaCl e- e- e- e- e- e- P+ e- e- e- - negative e- e- P+ N e- e- e- e- e- e- e- e- e- Salt e- Ionic bond e- e- e- e- P+ N e- e- e- e- e- Sodium e- e- + positive e-

Ionic Compound Generally from opposite sides of the periodic table. NaCl table salt

Ionic Compound Generally from opposite sides of the periodic table. KCl road salt

Ionic Compound Generally from opposite sides of the periodic table. MgSO4 Epsom salt

Ionic compounds form crystals

NaCl Type of Bond Properties Example Ionic Covalent Polar Covalent Chemical Bond Properties Type of Bond Properties Example Ionic 1) Crystalline solids (made of ions) 2) High melting and boiling points 3) Conduct electricity when melted 4) Many soluble in water 5) Generally formed from opposite sides of the periodic table (metals – nonmetals) NaCl Salt Covalent Polar Covalent Metallic

Covalent Bonds Juggling

Covalent Bond – a pair of electrons shared by two atoms.

Carbon e- P+ P+ P+ P+ e- e- e- P+ e- P+ e- wants 4 more electrons N N

Hydrogen wants 1 electron e- P+ N

e- P+ e- P+ 4 Hydrogens wants 4 electron e- P+ e- P+

Methane CH4 P+ P+ e- e- e- e- P+ P+ P+ P+ e- P+ e- P+ e- e- e- e- P+

NaCl CO2 Type of Bond Properties Example Ionic Covalent Polar Covalent Chemical Bond Properties Type of Bond Properties Example Ionic 1) Crystalline solids (made of ions) 2) High melting and boiling points 3) Conduct electricity when melted 4) Many soluble in water 5) Generally formed from opposite sides of the periodic table (metals – nonmetals) NaCl Salt Covalent 1) Gases, liquids, or solids (made of molecules) 2) Low melting and boiling points 3) Poor electrical conductors in all phases 4) Many soluble in nonpolar liquids but not in water CO2 Carbon dioxide Polar Covalent Metallic

Polar Covalent Bonds Uneven Juggling

Polar Covalent Bond – the unequal sharing of electrons between atoms that gives rise to negative and positive regions of electrical charge.

Oxygen e- P+ P+ P+ P+ P+ e- e- e- P+ P+ e- P+ e- e- e- wants 2 more electrons P+ N P+ P+ N N P+ N P+ N e- e- e- P+ N P+ N e- P+ N e- e- e-

e- P+ e- P+ 2 Hydrogens wants 2 electron

Water H2O P+ P+ e- e- e- e- P+ P+ P+ P+ P+ e- P+ P+ e- P+ e- e- e- e- N P+ P+ N N P+ N P+ N e- P+ N P+ N e- P+ N e- e- e- e-

Water H2O P+ P+ e- e- e- e- P+ P+ P+ P+ P+ e- P+ P+ e- P+ e- e- e- e- Slight positive (+) charge Slight positive (+) charge P+ P+ e- e- e- e- P+ N P+ P+ N N P+ N P+ N e- Slight negative (-) charge P+ N P+ N e- P+ N e- e- e- e-

NaCl CO2 H2O Type of Bond Properties Example Ionic Covalent Chemical Bond Properties Type of Bond Properties Example Ionic 1) Crystalline solids (made of ions) 2) High melting and boiling points 3) Conduct electricity when melted 4) Many soluble in water 5) Generally formed from opposite sides of the periodic table (metals – nonmetals) NaCl Salt Covalent 1) Gases, liquids, or solids (made of molecules) 2) Low melting and boiling points 3) Poor electrical conductors in all phases 4) Many soluble in nonpolar liquids but not in water CO2 Carbon dioxide Polar Covalent 1) Polar covalent molecules are affected by electrostatic fields 2) Have higher melting and boiling points than covalent bonds 3) Good solvent for ionic compounds H2O Water Metallic

Everyone juggling at once Metallic Bonds Mad Juggling Everyone juggling at once

Metallic Bond – a certain type of bond in which the nuclei float in a sea of electrons

Copper e- e- e- e- e- e- e- e- e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ wants 7 electrons e- e- e- e- e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- e- e- e- e- e-

e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N e- e- e- e- e- e- e- e- P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N e- e- e- e- e- e- e- e- P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e-

e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N e- e- e- e- e- e- e- e- P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N e- e- e- e- e- e- e- e- P+ N P+ N P+ N e- e- e- e- P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N P+ N e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e- e-

Another way to look at it… P+ N ND e- P+ N ND e- P+ N ND e- P+ N ND e- P+ N ND e- P+ N ND e- P+ N ND e- e- e- e- e- e- P+ N ND P+ N ND P+ N ND P+ N ND P+ N ND P+ N ND P+ N ND e- e- e- e- e- e- P+ N ND P+ N ND P+ N ND P+ N ND P+ N ND P+ N ND P+ N ND e- e- e- e- e- e- P+ N ND P+ N ND P+ N ND P+ N ND P+ N ND P+ N ND P+ N ND e- e- e- e- e- e-

NaCl CO2 H2O Al Type of Bond Properties Example Ionic Covalent Chemical Bond Properties Type of Bond Properties Example Ionic 1) Crystalline solids (made of ions) 2) High melting and boiling points 3) Conduct electricity when melted 4) Many soluble in water 5) Generally formed from opposite sides of the periodic table (metals – nonmetals) NaCl Salt Covalent 1) Gases, liquids, or solids (made of molecules) 2) Low melting and boiling points 3) Poor electrical conductors in all phases 4) Many soluble in nonpolar liquids but not in water CO2 Carbon dioxide Polar Covalent 1) Polar covalent molecules are affected by electrostatic fields 2) Have higher melting and boiling points than covalent bonds 3) Good solvent for ionic molecules H2O Water Metallic 1) Good conductors of heat and electricity 2) Bonds are not rigid - malleable and ductile 3) High boiling point 4) Shinny – electrons absorb light and re-emit at a different wavelength Al Aluminum foil

I can play music. Ionic Covalent Polar Covalent Metallic How to remember the four types of bonds. I can play music. Ionic Covalent Polar Covalent Metallic

Master Teacher Project Chemical Bonds Sean Gillette, EdD Master Teacher Project Betterlesson.com October 21, 2014