Using Lewis electron-dot symbols to depict the monatomic ions formed from each of the following reactants, predict the formula of the compound the ions produce.(Type your answer using the format CO2 for CO2.) (a) O and Ca (b) N and Mg (c) Br and Li (d) K and P
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- 3-58 In Section 2-3B, we saw that there are seven diatomic elements. (a) Draw Lewis structures for each of these diatomic elements. (b) Which diatomic elements are gases at room temperature? Which are liquids? Which are solids?Which of the following pairs react to form ioniccom-pounds: (a) Cl and Br; (b) Na and Br; (c) P and Se; (d) H and Ba?.Write formulas for ionic compounds. (a) What is the formula of the ionic compound expected to form between the elements sodium and fluorine? (b) What is the formula of the compound formed between the ions Co²+ and SO₂²? (c) What ions make up the ionic compound Zn(CN)₂? Cation formula Anion formula
- Answer true or false. (a) The octet rule refers to the chemical bonding patterns of the first eight elements of the Periodic Table. (b) The octet rule refers to the tendency of certain elements to react in such a way that they achieve an outer shell of eight valence electrons. (c) In gaining electrons, an atom becomes a positively charged ion called a cation. (d) When an atom forms an ion, only the number of valence electrons changes; the number of protons and neutrons in the nucleus does not change. (e) In forming ions, Group 2A elements typically lose two electrons to become cations with a charge of 12. (f) In forming an ion, a sodium atom (1s22s22p63s1) completes its valence shell by adding one electron to fill its 3s shell (1s22s22p63s2). (g) The elements of Group 6A typically react by ac- cepting two electrons to become anions with a charge of 22. (h) With the exception of hydrogen, the octet rule applies to all elements in periods 1, 2, and 3. (i) Atoms and the ions derived from…Assume that you encounter the following phrases in your reading. What is the chemical formula for each substance mentioned? (a) Sodium Hydrogen carbonate is used as a deodorant. (b) Calcium hypochlorite is used in some bleaching solutions. (c) Hydrogen cyanide is a very poisonous gas. (d) Magnesium hydroxide is used as a cathartic. (e) Tin (II) fluoride has been used as a fluoride additive in toothpastes. (f) When cadmium sulfide is treated with sulfuric acid, fumes of hydrogen sulfide are given off.Write the formulas of the following covalent compounds. (Type your answer using the format CO2 for CO2.) (a) silicon tetrachloride(b) carbon tetrachloride(c) dinitrogen tetroxide(d) dinitrogen oxide
- An element X reacts with oxygen to form XO2 and with chlorineto form XCl4. XO2 is a white solid that melts at high temperatures(above 1000 °C). Under usual conditions, XCl4 is acolorless liquid with a boiling point of 58 °C. (a) XCl4 reactswith water to form XO2 and another product. What is thelikely identity of the other product? (b) Do you think thatelement X is a metal, nonmetal, or metalloid?An element X reacts with oxygen to form XO2 and with chlorineto form XCl4. XO2 is a white solid that melts at high temperatures(above 1000 °C). Under usual conditions, XCl4 is acolorless liquid with a boiling point of 58 °C. (a) XCl4 reactswith water to form XO2 and another product. What is thelikely identity of the other product? (b) Do you think thatelement X is a metal, nonmetal, or metalloid? (c) By using asourcebook such as the CRC Handbook of Chemistry and Physics,try to determine the identity of element X.Chlorine reacts with oxygen to form Cl2O7. (a) What is the name of this product (see Table 2.6)? (b) Write a balanced equation for the formation of Cl2O7(l) from the elements. (c) Under usual conditions, Cl2O7 is a colorless liquid with a boiling point of 81℃. Is this boiling point expected or surprising? (d) Would you expect Cl2O7 to be more reactive toward H+(aq) or OH− (aq)? Explain. (e) If the oxygen in Cl2O7 is considered to have the -2 oxidation state, what is the oxidation state of the Cl? What is the electron configuration of Cl in this oxidation state?
- A gaseous binary compound has a vapor density that is 1.94 times that of oxygen at the same temperature and pressure. When 1.39 g of the gas is burned in an excess of oxygen, 1.21 g water is formed, removing all the hydrogen originally present.(a) Estimate the molecular mass of the gaseous compound.(b) How many hydrogen atoms are there in a molecule ofthe compound?(c) What is the maximum possible value of the atomicmass of the second element in the compound?(d) Are other values possible for the atomic mass of thesecond element? Use a table of atomic masses to identify the element that best fits the data.(e) What is the molecular formula of the compound?Answer true or false. (a) For Group 1A and Group 2A elements, the name of the ion each form is simply the name of the element followed by the word ion; for example, Mg21 is named magnesium ion. (b) H2 is named hydride ion. (c) The nucleus of H1 consists of one proton and one neutron. (d) Many transition and inner transition elements form more than one positively charged ion. (e) In naming metal cations with two different charges, the suffix -ous refers to the ion with a charge of 11 and -ic refers to the ion with a charge of 12. (f) Fe31 may be named either iron (III) ion or ferric ion. (g) The anion derived from a bromine atom is named bromine ion. (h) The anion derived from an oxygen atom is named oxide ion. (i) HCO3 2 is named hydrogen carbonate ion. (j) The prefix bi- in the name “bicarbonate” ion indicates that this ion has a charge of 22. (k) The hydrogen phosphate ion has a charge of 11, and the dihydrogen phosphate ion has a charge of 12. (l) The phosphate ion is PO3 42. (m)…Write the chemical formulas for the following compounds:(a) aluminum hydroxide(b) potassium sulfate(c) copper(I) oxide(d) zinc nitrate(e) mercury(II) bromide