Many common ionic compounds contain ions that are themselves composed of a group of covalently bonded atoms with an overall charge. True or false? Give some examples?

1. Compare cations, anions, and polyatomic ions. What do they all have in common? How are they different? 2. How can the periodic table help to remember the charges on the simple ions of the representative elements? 3. Is there more than one chemical name that can be used for baking soda?

There was a part missing from the first one. This activity is structured as a game, wherein your challenge is to create correct ionic compound formulas by combining individual ions based on their charges. Once you correctly connect the atoms in the interactive website, a common use for that compound will be revealed. In the chart,  record both the correct formula for each of seven ionic compounds and their common uses as revealed by the interactive program.

Please answer all questions.

Read: An Ion is a charged atom, # protons ≠ # electrons. On page three, paragraph one states, “The prefix poly- means many and atomic refers to atoms, so a polyatomic ion is an ion that contains more than one atom. This differentiates polyatomic ions from monatomic ions, which contain only one atom.” Ions that contain only one atom are called monoatomic ions. Ions that contain more than one atom are called polyatomic ions. A monatomic ion is a single charged atom, with the number of protons not equal to the number of electrons. A polyatomic ion is a group of covalently-bonded atoms, with the total number of protons not equal to the total number of electrons. Using the image attached how could you further elaborate this answer? Cite evidence from the image.

Ionic Compounds, Covalent Compounds, and Chemical Equations a. Define the terms "ianic compound" and "covalent compound". Use all of the following terms correctly in at least one of the two definitions cation, anion metal, nonmetol, electrons are shared, and electrons are transferred. Write your answers in complete sentences. b. Complete the following chart using the information given. Correctly write the name or formula of each compound and identify it as lo covalent Formula AlO₂ K₂5 PC1₂ OF Name Magnesium iodide Tetrasulfur tetranitide Iron (III) sulfide Ammonium nitrate Tonico Covalent? CUCO Dinitrogen tetroxide c. Write o balanced chemical equation for the reaction that takes place between magnesium iodide and iron (III) sulfide ond identify the reaction type

Write the formulas of the following covalent compounds. (Type your answer using the format CO2 for CO2.) 1. dinitrogen tetroxide 2. silicon tetrachloride 3. dinitrogen oxide 4. carbon tetrachloride

Predict the formula for each ionic compound. (Recall the polyatomic ions in the table below.) Some Common Polyatomic Ions Name Formula Acetate C2H3O2− Hydrogen carbonate HCO3− Hydroxide OH− Nitrate NO3− Carbonate CO32− Sulfate SO42− Phosphate PO43− Ammonium NH4+ Note: The names of positive polyatomic ions end in -ium. Many negative polyatomic ions have names ending in -ate. Another name for the hydrogen carbonate ion is bicarbonate. (a) radium nitrate   chemPad Help                   (b) barium phosphate   chemPad Help                   (c) cesium iodide   chemPad Help                   (d) gallium phosphide   chemPad Help                   (e) aluminum nitride   chemPad Help                   (f) lithium sulfate   chemPad Help

What kind of substances do not dissociate into ions? O lonic compounds with no polyatomic ions O lonic compounds with polyatomic ions O Acid and bases Molecular (covalent) compounds

Read: On page three, paragraph one reads, "As the prefix, poly means many and atomic is related to atoms. An ion with more than one atom is a polyatomic ion. This differentiates polyatomic ions from monoatomic ions, which contain only one atom." A polyatomic ion is a group of covalently bonded atoms, with the total number of protons not equal to the total number of electrons. Atoms become ions when they gain or lose electrons, resulting in a net charge. On page one paragraph two it says. "The Octet rule describes the tendency of atoms to prefer valence shells with eight electrons. Atoms react and tend to create more stable compounds since they have fewer electrons. When discussing the octet rule, d or f electrons are not considered." According to the octet rule, atoms typically have eight electrons in their valence shell. Elements in the S block and P-block follow the Octet rule. On page two, paragraph one, "To draw a Lewis Structure, start with the atomic symbol in the middle, then…