Introductory Chemistry: An Active Learning Approach
6th Edition
ISBN: 9781305079250
Author: Mark S. Cracolice, Ed Peters
Publisher: Cengage Learning
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Textbook Question
Chapter 12, Problem 9E
When potassium and chlorine react and form an ionic compound, why is there only one chlorine atom for each potassium atom instead of two?
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Which of these elements would bond with Fluorine to create an Ionic Compound m? Give me the correct Ionic formula for each one that can bond.
Potassium
Nitrogen
Sulfur
Beryllium
Chlorine
Aluminum
Which of the following statements about the ionic bond in ammonium chloride is correct?
It is formed by the transfer of electrons from metal atoms to non-metal atoms.
It is the electrostatic attraction between ammonium ions and chloride ions.
It is formed by the sharing of electrons between the nitrogen atom and chlorine atom.
There is actually no ionic bond in ammonium chloride.
Draw the Lewis structures of the neutral atom of Calcium and the ion of Calcium. Determine the number of electrons gained or lost in forming an ion.
Chapter 12 Solutions
Introductory Chemistry: An Active Learning Approach
Ch. 12 - Write the electronic configuration for the ions of...Ch. 12 - A monoatomic ion with a charge of 1 has an...Ch. 12 - Identify by symbol two positively charged...Ch. 12 - Considering only ions with charges of 1+,2+,1, and...Ch. 12 - Write the symbols of two ions that are...Ch. 12 - Considering only ions with charges of 1+,2+,1, and...Ch. 12 - Prob. 7ECh. 12 - Prob. 8ECh. 12 - When potassium and chlorine react and form an...Ch. 12 - Fill in the blanks with the smallest integers...
Ch. 12 - Prob. 11ECh. 12 - Prob. 12ECh. 12 - Prob. 13ECh. 12 - Prob. 14ECh. 12 - Prob. 15ECh. 12 - Prob. 16ECh. 12 - Prob. 17ECh. 12 - Prob. 18ECh. 12 - Prob. 19ECh. 12 - Prob. 20ECh. 12 - Prob. 21ECh. 12 - Consider the following bonds: GeSe, BrSe, BrGe....Ch. 12 - Prob. 23ECh. 12 - Consider the following bonds: TeSe, OTe, OSe....Ch. 12 - Prob. 25ECh. 12 - Prob. 26ECh. 12 - Prob. 27ECh. 12 - Prob. 28ECh. 12 - Prob. 29ECh. 12 - What is the maximum number of atoms to which a...Ch. 12 - Prob. 31ECh. 12 - Prob. 32ECh. 12 - Prob. 33ECh. 12 - Prob. 34ECh. 12 - Prob. 35ECh. 12 - Prob. 36ECh. 12 - Prob. 37ECh. 12 - Prob. 38ECh. 12 - Prob. 39ECh. 12 - Prob. 40ECh. 12 - Prob. 41ECh. 12 - Prob. 42ECh. 12 - Prob. 43ECh. 12 - Prob. 44ECh. 12 - Prob. 45ECh. 12 - Prob. 46ECh. 12 - Prob. 47ECh. 12 - Prob. 48ECh. 12 - Which orbitals of each atom overlap in forming a...Ch. 12 - Prob. 50ECh. 12 - Prob. 51ECh. 12 - A monatomic ion with a 2 charge has the electron...Ch. 12 - Prob. 53ECh. 12 - Prob. 54ECh. 12 - Prob. 55ECh. 12 - Prob. 56ECh. 12 - Prob. 57ECh. 12 - Prob. 58ECh. 12 - Prob. 59ECh. 12 - Prob. 60ECh. 12 - Prob. 61ECh. 12 - Which ions among the following are isoelectronic...Ch. 12 - Prob. 12.2TCCh. 12 - Prob. 12.3TCCh. 12 - Prob. 12.4TCCh. 12 - Prob. 12.5TCCh. 12 - Prob. 1CLECh. 12 - Prob. 2CLECh. 12 - Prob. 3CLECh. 12 - Prob. 4CLECh. 12 - Prob. 5CLECh. 12 - Prob. 6CLECh. 12 - Write the electron configurations for the oxide...Ch. 12 - Arrange the following bonds in order of decreasing...
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- What main factors control the magnitude of lattice energies? Give a specific example of a compound that should have a high lattice energy, and explain why its lattice energy is high.arrow_forwardUsing Lewis Structures to Determine the Correct Chemical Formula for Ionic Compounds Use Lewis structures to determine the correct chemical formula for the compound formed between LiandO.arrow_forwardHydrogen gas and oxygen gas react violently to form water. When this occurs, a very loud noise is heard. Draw the Lewis structures for hydrogen gas, oxygen gas, and water. State whether each molecule is polar or nonpolar and why. Explain how the polarity of these molecules is related to hydrogen and oxygen existing in the gas phase at room temperature and water existing in the liquid phase at room temperature. Which is lower in energy for this reaction a mixture of hydrogen and oxygen gases or water? How do you know this is true?arrow_forward
- Draw the Lewis structures of the neutral atom of Aluminum and the ion of Aluminum. Determine the number of electrons gained or lost in forming an ion.arrow_forwardIndicate and explain with examples and diagrams the following interatomic chemical bonds. Metallic bond Ionic bond Covalent bondarrow_forwardProvide one example of molecule with correct chemical name and one example of ionic compound with correct chemical name.arrow_forward
- What does “polar” means, in the case of an ionized molecules and how is this related to “charged” of a moleculearrow_forwardThe following Lewis diagram represents the valence electron configuration of a main-group element. This element is in what group in the periodic table? According to the octet rule, this element would be expected to form an ion with a charge of? If X is in period 5, the ion formed has the same electron configuration as the noble gas? What is the symbol for the ion?arrow_forwardFor each row in the table below, decide whether the pair of elements will form a molecular compound held together by covalent chemical bonds. If the elements will form a molecular compound, check the box and enter the chemical formula and name of the compound. (If the elements will form more than one molecular compound, use the compound with the fewest total number of atoms.) You may assume all chemical bonds are single bonds, not double or triple bonds. molecular compound element #1 element #2 element pair will form a molecular compound chemical name formula magnesium chlorine ☐ ☐ carbon chlorine ☐ ☐ hydrogen iodine ☐ ☐arrow_forward
- Now, we will investigate diatomic molecules, those that are made up of two of the same type of atom. Select 2 fluorine atoms. How many valence electrons are in each fluorine atom? Is a fluorine atom a metal or a non-metal? Did the combination of these atoms create a covalent or ionic bond? How are the valence electrons organized to form a bond between these atoms? How is this different from the ionic bonds formed in the previous part of the activity?arrow_forward+1 +2 Type I Binary Ionic Compounds Type I binary ionic compounds contain a metal and a nonmetal AND the metal that is present only forms one type of cation. Metals with only one cation (shaded below with charges). Both the metal and the nonmetal form ions, which is why it is called an ionic compound. From the following list, cross out those compounds that do NOT belong in the category for Type I binary ionic compounds. 1) KS NaCl FeCl2 CaCl2 TiO2 MgO AIBR3 KCI Cu2O3 AgCl Zna Formula and name examples for Type I binary ionic compounds: KI = potassium iodide Ag3N = silver nitride BaO = barium oxide ZnF2 = zinc fluoride Nazs = sodium sulf BeCl2 = beryllium chloride Metal What type of element is always listed first (metal or nonmetal)? 2) 3) Is the name of the first element in the compound different from the element? (yes/no 4) What is the common ending for all the names? 5) In zinc fluoride, there are 2 fluoride atoms, are they indicated in the name? (yesy no) 6) What is the charge on…arrow_forwardA polar covalent bond would form in which of the following pairs of atoms? (Refer to a periodic table with electronegativity values) Ca-CI b Cr-Br P-CI d CI-CIarrow_forward
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