G11-W4-T1 Chemistry PDF

CHEMISTR Y High Performance Learning Model - HPL  AY 2024-2025 chemistry Grade 11 Week 4–Session -1 McGraw Hill Inspire Chemistry Unit 6 & 7 – Chemical Bonding 2: Ionic bonds and ionic compounds McGraw Hill Inspire Chemistry Unit 6 & 7 – Chemical Bonding 2: Ionic bonds and ionic compounds Su...

CHEMISTR Y High Performance Learning Model - HPL  AY 2024-2025 chemistry Grade 11 Week 4–Session -1 McGraw Hill Inspire Chemistry Unit 6 & 7 – Chemical Bonding 2: Ionic bonds and ionic compounds McGraw Hill Inspire Chemistry Unit 6 & 7 – Chemical Bonding 2: Ionic bonds and ionic compounds Success Criteria ACPC: We can interpret the formation of ionic bonds. (Power Thinking) VAA’S We caN investigate the effects of electronegativity differences in the formation of chemical bonds.(Power Hardworking). McGraw Hill Inspire Chemistry Unit 6 & 7 – Chemical Bonding 2: Ionic bonds and ionic compounds Learning Objective: Students will can analyse the formation of ionic bonds.. McGraw Hill Inspire Chemistry Unit 6 & 7 – Chemical Bonding 2: Ionic bonds and ionic compounds McGraw Hill Inspire Chemistry Unit 6 & 7 – Chemical Bonding 2: Ionic bonds and ionic compounds Vocabulary; 1-Ionic bond; 2-Ionic compound 3-Crystal lattice;  Ionic Bonding An introductory presentation + - Li F  Learning Points Describe what State which types of Explain some key happens to electrons elements ionic bonds properties of ionic when an ionic bond can exist between. compounds. is formed.  Elements Metals Ionic bonds form between Metals can be found in the metals and non-metals. middle and on the left hand side of the periodic table. Non-metals Non-metals can be found on the right hand side of the periodic table.  Li F What are ionic bonds? An ionic bond is formed when a metal and non-metal react. Metal atoms become positively charged ions by losing electrons. Non-metal atoms become negatively charged ions by gaining electrons. The oppositely charged ions are very strongly attracted to each other. This is known as an electrostatic attraction.  Forming Forming positive ions negative ions Metal atoms lose electrons to form Non-metal atoms gain electrons to positively charged ions with a full form negatively charged ions with a outer shell of electrons. full outer shell of electrons. + - Li Li F F  2+ 2- Mg Handy O tips For elements in groups 1,2 and 3, For elements in groups 6 and 7, the the number of electrons lost is the number of electrons gained is 8 same as the group number (e.g. subtract the group number (e.g. magnesium is in group 2 and forms oxygen is in group 6 and forms a a 2+ ion). 2- ion).  Sodium chloride Na Cl Chlorine gains an electron from sodium to become a negative ion (-1). Sodium loses an electron to become a positive ion (+1). Both + - ions now have a full outer shell of electrons and the ionic Na Cl compound sodium chloride is formed.  Li O Li Lithium oxide Each lithium atom loses an electron to become a positively charged ion (1+). The oxygen + 2- atom gains two electrons to become a negatively charged ion 2 Li O (2-).  Ionic lattice + - + An ionic compound is a regular repeating structure of ions known as - + - a giant ionic lattice. The lattice is composed of a repeating pattern of oppositely charged ions held together + - + by strong electrostatic attractions.  Conduction Ionic compounds can conduct electricity when they are either melted or dissolved in water to form an aqueous solution. In these states, the ions are free to move from place to place. Ionic compounds cannot conduct electricity when solid as their ions are in fixed positions.  Melting and boiling points Ionic compounds consist of oppositely charged ions held together by strong electrostatic attractions. A lot of energy is required to overcome these strong attractions, hence the high melting and boiling points.  Ionic Bonding The end of the presentation + - Li F