2. General Chemistry Faculty of Allied Medical Sciences (MGGC-101)

3. Supervision: Prof.Dr.Shehata El-Sewedy Dr.Fatma Ahmed Chemical bonds & chemical reactions

4. Outcomes By the end of this lecture, the students will be able to 1-Understand the meaning of chemical bond 2-learn to type of chemical bond 3-To differentiate between solute, solvent and solution 4-Recognize the meaning of electrolyte 5-To know types of chemical reactions 6-To differentiate between acids and bases

5. Chemical bonds

6. CHEMICAL BONDS: THE OCTET RULE Why do atoms bond together? More stable (has less energy) Octet Rule Atoms form bonds to produce the electron configuration of a noble gas because the electronic configuration of noble gases is particularly ) stable) For most atoms of interest this means achieving a valence shell configuraon of 8 electrons corresponding to that of the nearest noble gas Atoms close to helium achieve a valence shell configuraon of 2 electrons Atoms can form either ionic or covalent bonds to satisfy the octet rule How to describe bonding? The ionic bond : formed by the transfer of one or more electrons from one atom to another to create ions The covalent bond : results when atoms share electrons Atoms without the electronic configuration of a noble gas generally react to produce such a configuration

7. 1) Ionic Bonds Results from transfer of electrons from one atom to another such as NaCl, NaBr and so on. Electronegativity measures the ability of an atom to attract electrons

9. Ionic Bonds: One Big Greedy Thief Dog!

10. Electronegativities of Some of Elements The electronegativity increases across a horizontal row of the periodic table from left to right The electronegativity decreases go down a vertical column

11. F>O>N>C fluorine is the most electronegative atom. Ionic substances, because of their strong internal electrostatic forces, are usually very high melting solids, often having melting points above 1000 °C

12. 2 )Covalent Bonds Results from sharing of electrons by two atoms such as H-H, Cl-Cl, H-Cl and so on. Polar covalent bond ( between two atoms different in electronegativity)

14. Polar Covalent Bonds: Unevenly matched, but willing to share.

15. Chemical reactions

16. Reaction without electron transfer Reaction with electron transfer 1-Combination 1-Oxidation (loss of electrons) 2-Substitution 2-Reduction (gain of electrons) 3-Addition 3-Redox reaction (oxidation-reduction) 4-Combustion

17. A solution is a homogenous mixture of 2 or more substances The solute is(are) the substance(s) present in the smaller amount(s) The solvent is the substance present in the larger amount SolutionSolventSolute Soft drink (l) H2OH2O Sugar

18. An electrolyte is a substance that, when dissolved in water, results in a solution that can conduct electricity. A nonelectrolyte is a substance that, when dissolved, results in a solution that does not conduct electricity. nonelectrolyte weak electrolyte strong electrolyte

19. Acid–base reactions

20. Acids : Is the substance that produces H + ions when it dissolved in Water strong acid ; it is a strong electrolyte. weak acid: it is a weak electrolyte. Acids can be divided into two classes Strong Acids : Completely dissociate into its ions eg: HCl, HBr, HNO 3 and H 2 SO 4 HCl (aq) → H + (qa) + Cl - (aq) 100% dissociation Weak acids : is the one dissociate incompletely into its ions eg: CH3COOH. CH3COOH ↔ H + (aq) + CH 3 COO - (aq) 1% dissociation

21. Base : Is the substance that produces OH - ions when it dissolved in water strong base ; it is a strong electrolyte. weak base: it is a weak electrolyte. Bases: can be divided into two classes Strong Bases : Completely dissociate into its ions eg: NaOH and KOH NaOH (aq) → Na + (qa) +OH - (aq) 100% dissociation Weak Base : is the one dissociate incompletely into its ions eg: ammonia. NH 3 (aq) + H 2 O(l) ↔ NH 4 + (aq) + OH - (aq) 1% dissociation

22. Examples of the acid-base reactions: Reaction of Sodium hydroxide and Nitric acid & reaction of Potassium hydroxide and Sulfuric acid. The Brønsted - Lowry theory of acids and bases. A Brønsted – Lowry acid: is a species which donates a proton (H + ion) to another species. A Brønsted – Lowry base: is a species which accepts a proton from another species. You must have a reaction in order to name a species as a Brønsted - Lowry acid (B-L acid) or base.

23. Example HCl (aq) + H 2 O (l)  H 3 O + (aq) + Cl - (aq) HCl is the B-L acid, it donates the proton to the H 2 O which is the B-L base since it accepts the proton (H + ion) Example NH 3(g) + H 2 O (l) NH 4 + (aq) + OH - (aq) H 2 O is the B-L acid, it donates the proton to the NH 3 which is the B-L base since it accepts the proton (H + ion).

24. Quiz time

25. Mention Brønsted - Lowry theory of acids and bases for the fowlloing reaction NH 3(g) + H 2 O (l) NH 4 + (aq) + OH - (aq) HCl (aq) + H 2 O (l)  H 3 O + (aq) + Cl - (aq) NH 3 (aq) + H 2 O(l) ↔ NH 4 + (aq) + OH - (aq) What is type of base for NH3? HCl (aq) → H + (qa) + Cl - (aq) What is type of acid for HCl? N,C, F,O, Order according for electronegativity ?

26. Mention types of reaction?

27. Student Question

28. Mention types of reaction? Base Acids solute electrolyte Define and give example

29. Mention Brønsted - Lowry theory of acids and bases for the fowlloing reaction NH 3(g) + H 2 O (l) NH 4 + (aq) + OH - (aq) HCl (aq) + H 2 O (l)  H 3 O + (aq) + Cl - (aq) NH 3 (aq) + H 2 O(l) ↔ NH 4 + (aq) + OH - (aq) What is type of base for NH3? HCl (aq) → H + (qa) + Cl - (aq) What is type of acid for HCl? N,C, F,O, Order according for electronegativity ?

30. Assignments Group A and Group B Noor El-Din Adel Mohamad Abd El Fatah Ali Mahmoud Ahmad Combustion reaction Naamat Hafez Mana Allah Mostafa Passant Ahmad Hamza Substitution reaction in industry Ashraf Moahamad El Amir Said Tawfik Ibrahim Shahaat Ahmad Mahmoud Raafat AbdAllah Application of redox reaction Abeer El Said -Haidy Adel- Ali Hassan Hossam Hassan- Yehia Hamdy Youssef Ali Physical properties of matter

31. R ECOMMENDED TEXTBOOKS : 1-Raymond Chang. Chemistry. 10th ed. 2009 2-Zumdehl. International edition. 2009