Questions47). When do chemical bonds form? 48). Why do positive and negative ions form? 49). Why are halogens and alkali metals likely to form ions? Explain 50). Discuss the importance of electron affinity and ionization energy in the formation of ions. 51). Discuss the formation of ionic bonds. 52). Briefly discuss three physical properties of ionic solids that are linked to ionic bonds. 53). What does the term 'electrically neutral' mean when discussing ionic compounds? 54). What information is needed to write a correct chemical formula to represent an ionic compound? 55). When are subscripts used in formulas for ionic compounds? 56). Discuss how an ionic compound is made. 57). Describe a metallic bond. 58). Briefly explain how malleability and ductility of metals are explained by metallic bonds. 59). Compare and contrast the two types of metal alloys. 60). Explain why nobel gasses are not likely to form chemical bonds. 61). Give the number of valence electrons for the following: a. cesium b. rubidium c. gallium d. zinc e. strontium 62). Discuss the formation of the barium ion. 63). Explain how an anion of nitrogen forms. 64). Which atom would have more potential energy Fluorine or Neon? Why? 65). Predict the reactivity of the following: a. Potassium b. Fluorine c. Neon 66). Discuss the formation of the iron ion that has a 3+ oxidation number. | Answers47). A chemical bond forms when a positive nucleus bonds twits negative electrons.
48). Positive and negative ions form because the atoms need a full outer layer of electrons. 49). Halogens are very attracted to the negative electrons that the alkali metals give away. 50). The number of electrons lost must equal the number of electrons gained for each atom to be happy. 51). Ionic bonds are the electrostatic force that holds oppositely charged atoms together. It occurs when atoms lose, gain, or share electrons. 52). Melting point, boiling point, and hardness in a solid show how strong the bond is. If melting and boiling points are high, then the bond is strong. 53). It means that there is an equal number of positive ions to negative ions. 54). You need to know the symbols of the atoms, their charge, and how many there are in the compound. 55). Subscripts are used when there is more then 1 atom of a curtain element in the compound. 56). An ionic compound is created when several ionic bonds join together. 57). A metallic bonds happens when a metal is attracted to delocalized electrons. 58). The more malleable and ductal a solid metal is, the stronger the bond. 59). The 2 types of alloys are Substitutional and Interstitial. Substitutional alloys have some metal atoms replaced by metalloid atoms. Interstitial alloys are made when small holes in the crystal are filled with smaller atoms. 60). They have all of their outer electron layers filled so they won't be likely to mix with anyone else because they have all they need already. 61). a. 37 b. 19 c. 13 d. 12 e. 20 62). Barium wants its configuration to be that of a nobel gas. The closest one is Krypton. To accomplish its goal, Barium loses to electrons, causing it to be a positive ion. 63). Nitrogen gains three electrons to match Neon, causing it to become an anion. 64). Fluorine would have more energy because it's more reactive then Neon. 65). a. slightly reactive b. reactive c. not reactive 66). |