Chapter 4 Formation of Compounds

1. Chapter 4Formation of Compounds Section 4.2 How Elements Form Compounds

2. Objectives: Model two types of compound formation- ionic and covalent, Demonstrate how and why atoms achieve chemical stability by bonding, Compare the effect of covalent and ionic bonding on the physical properties of compounds 29 min video http://www.pbslearningmedia.org/resource/7eb9615f-f534-4772-b65d-6c5117768a66/chemistry-501-introduction-to-bonding/

3. Compound formation When elements react, atoms of the elements must collide Reactions between atoms only involve their electron clouds- v.e. of colliding atoms interact

4. Noble Gases Group 18 elements Unreactive elements, extreme stability Noble gases are used in light displays, neon lights  Lack of reactivity of noble gases indicates that atoms of these elements must be stable Each noble gas has 8 valence electrons, except helium has 2

5. NOBLE GAS CONFIGURATION Achieving the same configuration of v.e.’s (a stable octet) as one of the noble gases

6. OCTET RULE Atoms can become stable by having eight electrons in their outer energy level (or 2 for H and He) If atoms collide with enough energy, their outer electrons may rearrange to achieve a stable octet of v.e.’s → the atoms will form a compound

7. Ions ION: Atom or group of combined atoms that has a charge because of the loss or gain of electrons. Ions always form when v.e.’s rearrange by electron transfer between atoms *

8. Ions If an element loses an electron it becomes a positively charged ion called a cation If an element gains an electron it becomes a negatively charged ion called an anion Where are these located on the periodic table?

9. Isoelectronic atoms/ions • Isoelectronic is a term used to describe atoms and ions that have the same number of electrons. • Practice by writing the following isoelectronic configuration for : • Na1+ • Ne • F1- • O2- • N3-

10. Lewis Dot Ions vs atoms See notes…

11. Valence electron rearrangement 2 possibilities: Transfer (ionic) - metal and nonmetal Sharing (covalent) - 2 nonmetals Video 4-3

12. Electron Transfer (Ionic Compound) • Can use Lewis dot structures to represent atoms and the rearrangement of v.e.’s. • Colliding atoms transfer electrons only when one atom has stronger attraction for valence electrons than the other atom • Electrons will move from one atom (metal) to the other (nonmetal)

13. Electron Transfer (Ionic Compound) • Example: Transfer gives both Chlorine and Sodium stable octet . . . . Na • + • Cl : → [Na] + + [ : Cl : ] - ••• • • Try these: Ca and Cl, Li and S, K and P • Atoms are no longer neutral- become ions

14. Electron Transfer (Ionic Compound) IONIC COMPOUND: A compound that is composed of ions Once the ions have formed they are strongly attracted to each other. IONIC BOND: Strong attractive force between ions of opposite charge

15. Electron Transfer (Ionic Compound) Ions in salt do not arrange themselves into isolated sodium ion/chloride ion pairs. They arrange themselves into a well-organized definite cube structure CRYSTAL: Regular repeating arrangement of atoms, ions or molecules

16. Electron Transfer (Ionic Compound) INTERPARTICLE FORCES: Forces between particles that make up a substance (strong for ionic bonds). They are key for determining state of matter of a substance at room temperature (RT) and other physical properties. Ionic attractions are strong attractive forces so it is hard to break ionic compounds giving them high melting point temperatures.

17. Properties of Ionic Compounds Generally, ionic compounds: 1) Crystalline solids at room temperature (Why?) 2) Hard, rough and brittle (Why?) 3) High temperatures in order to melt (Why? What does this look like?) 4) They tend to conduct electricity when they dissolve in water or are melted (Why? What does this look like?) http://education-portal.com/academy/lesson/ionic-compounds-formation-lattice-energy-and-properties.html ELECTROLYTE: Compound that conducts electricity when melted or dissolved in water.

18. Predict: • 1. Would NaCl dissolved in water conduct electricity? • Would this be an electrolyte? Why or why not? • 2. Would NaCl dissolved in ethanol conduct electricity? • Would this be an electrolyte? Why or why not? • 3. Would distilled water conduct electricity? • Why or Why not?

19. Polyatomic Structures http://education-portal.com/academy/lesson/lewis-dot-structures-polyatomic-ions-and-resonance-structures.html

20. Chemical Formulas Formulas of compounds tell What elements make up the compound How many atoms of each element are present in the compound Ex: Water – H2O has 2 hydrogen atoms and 1 oxygen atom Sodium Chloride- NaCl has 1 sodium and 1 chlorine atom

21. Electron Sharing/ Covalent Compounds (molecules) When atoms collide with enough energy to react, but neither attracts electrons strongly enough to take electrons from the other atom, the atoms combine by sharing v.e.’s

22. Electron Sharing/ Covalent Compounds (molecules) Ex: Sharing gives both H and O stability Hydrogen has 2 valence electrons and oxygen has an octet when they share electrons. • • • • H+ • O : → H : O : (O has 7 e-s) • • • • • • H : O : + H → H :O : • •

23. Electron Sharing/ Covalent Compounds (molecules) COVALENT BOND: Attraction of two atoms for a shared pair of electrons In a covalent bond, atoms (2 nonmetals) share electrons and neither atom has an ionic charge COVALENT COMPOUND: Compound whose atoms are held together by covalent bonds

24. Electron Sharing/ Covalent Compounds (molecules) MOLECULE: Uncharged group of two or more atoms held together by covalent bonds Covalent bonds= molecular compounds

25. Sharing More than 2 e-‘s • More than 2 electrons can be shared in some cases of electron sharing • Example: Carbon Dioxide . . . . . : O • + • C • + • O : → • • • : O : :C : :O : •• • •

26. Properties of Covalent bonds INTERPARTICLE FORCES: Forces between particles that make up a substance (weaker for covalent bonds). They are key for determining state of matter of a substance at room temperature (RT) and other physical properties Attractive force between molecules are usually weak All have very strong bonds between the atoms, but much weaker forces holding the molecules together.

27. Properties of Covalent bonds Many covalent compounds 1) Are liquids or gases at RT or are solids that melt at low temperatures 2) Do not conduct electricity 3) do not usually dissolve in water 4)In general, are usually less soluble in water than ionic compounds. http://ed.ted.com/lessons/how-atoms-bond-george-zaidan-and-charles-morton#review http://education-portal.com/academy/lesson/covalent-compounds-properties-naming-formation.html

28. Lewis Dot Structures(Structural Formulas) http://education-portal.com/academy/lesson/lewis-structures-single-double-triple-bonds.html Steps to determine the number of bonds: 1) Have -Total number of V.E. 2) Need - Total number of V.E. (Happy) 3) Subtract Need – Have 4) Divide by 2 5) Draw with that number of bonds