Ions and Ionic Bonding Cornell Doodle Notes PDF

# IONS AND IONIC BONDING ## Cornell Doodle Notes ### Essential Question: How do atoms form bonds by lending and borrowing electrons? # VOCABULARY - **Charge:** An uneven number of protons and electrons in an atom; can cause an overall positive or negative charge - **Valence Electrons:** Electron...

# IONS AND IONIC BONDING ## Cornell Doodle Notes ### Essential Question: How do atoms form bonds by lending and borrowing electrons? # VOCABULARY - **Charge:** An uneven number of protons and electrons in an atom; can cause an overall positive or negative charge - **Valence Electrons:** Electrons that orbit furthest from an atom's nucleus # TOPIC QUESTION # 1 ## What is an ion? - An ion is an atom that has lost or gained electrons and now has an electric charge. - An ion is charged while an atom is neutral. - A **lithium atom** has 3 protons and 3 electrons. It is neutral (not charged). - If the atom gives away its **valence electron**, it becomes more stable. It will then have 3 protons and only 2 electrons. - This **lithium ion** has lost a negative particle and now has a charge of 1+. # TOPIC QUESTION # 2 ## Why would an atom give away or receive electrons? - An atom feels stable when its outermost shell is full with 8 electrons (except for Helium, which feels stable with 2). - When atoms form ions, they are trying to obtain the electron arrangement of the Noble Gas nearest to them on the Periodic Table. - The Noble Gases already have 8 valence electrons. You can think of them as “The Snobs” because they don’t like to interact with other atoms. # TOPIC QUESTION # 3 ## What are the two types of ions? - **Positively-charged ions** are called **cations** (pronounced cat-ions). Cations have given away some electrons (negatively-charged particles), so they have become more positive. - **Negatively-charged ions** are called **anions** (pronounced an-ions). Anions have taken some electrons (negatively-charged particles) from other atoms, so they have become more negative. # TOPIC QUESTION # 4 ## Which atoms give electrons and which ones take them? - **Metals** act as cations and **nonmetals** act as anions. - The cations are like the “hippies” of the periodic table because they will give away their electrons. - The anions are the “greedy” atoms because they want to go around and take valence electrons from others. - **Noble gases** do not form ions, along with some other elements. # TOPIC QUESTION # 5 ## What is an ionic bond? - An ionic bond forms when one atom gives up one or more electrons to another atom. Both atoms become charged ions. - It’s a very strong bond because an electrostatic attraction ends up linking ions with opposite charges. - In **lithium fluoride**, lithium gives up its valence electron to fluorine. This makes lithium a 1+ cation (3 p+ and 2 e-) and fluorine a 1- anion (7 p+ and 8 e-). # TOPIC QUESTION # 6 ## What types of ions do the different elements form? - This table shows the most common ions that atoms form when they give up or take electrons. The ion’s charge can be written to the top right of the element symbol. - Some atoms can form ions of different charges. For example, iron can form **Fe3+** or **Fe2+**. - The metals form positive ions, the nonmetals form negative ions, and the noble gases do not form ions. - **Beryllium** doesn’t form an ion. - All of the elements in groups 1, 2, 15, 16, and 17 have the same charge as one another. | Element | # Protons | # Electrons | # Valence e- | Metal/Nonmetal | For Full Valence Shell | New # of Electrons | New Charge | Ion that Forms | |---|---|---|---|---|---|---|---|---| | **Sodium Na** | 11 | 11 | 1 | M | Give 1 | 11 - 1 = 10 | 1+ | Na1+ | | **Chlorine Cl** | | | | | | | | | | **Magnesium Mg** | | | | | | | | | | **Oxygen O** | | | | | | | | | | **Nitrogen N** | | | | | | | | | # TOPIC QUESTION # 7 ## How can we represent an ionic bond? - Using **potassium** and **fluorine** as an example: * Write the metal and draw its Lewis Dot Diagram. * Write the nonmetal and draw its Lewis Dot Diagram. * Draw arrow(s) to show the electron transfer(s). The cation will lend to the anion. * Write the two ions that have formed (element symbol and charge to its top right). * “Criss-cross” the charge numbers (NOT the plus/minus signs) to make them into subscripts. * Write the new compound’s complete formula. - Using **calcium** and **chlorine** as an example: * In this case, you start by writing just one of each atom, but you must add another chlorine atom in order for the calcium to be able to give away both of its valence electrons. * Draw arrow(s) to show the electron transfer(s). The cation will lend to the anion. * Write the two ions that have formed (element symbol and charge to its top right). * “Criss-cross” the charge numbers (NOT the plus/minus signs) to make them into subscripts. * Write the new compound’s complete formula. * Be Careful! Even though you have drawn two anions, you only use ONE of them for the formula writing part. # QUICK WATCH FuseSchool: What are lonic Bonds? https://tinyurl.com/pjfzpkv # SUM IT UP! Practice what you’ve learned by answering the Let’s Try lonic Bonding questions!