7. What kind of substances form ionic bonds? Nonmetals and metal 8. What is a covalent bond? How is this different from an ionic bond? A covalent bond is a pair of electrons sharing between atoms. An ionic bond 9. What kind of substances/elements form covalent bonds? 10.Why do ions form from atoms? 11. Why do ionic compounds form from ions? Atoms, Molecules, and Ions (8:18) https://www.youtube.com/watch?v=lPuY0OHa6RA&list=PLBwHfJmqJz5h5a6UxWpMrxV- İSIMKNSIN&index=12 Video starts at 1:15 min. 1. What is a molecular compound? 2. What is an ionic compound? 3. How do you distinguish between a molecular and an ionic compound?

7. What kind of substances form ionic bonds? Nonmetals and metal 8. What is a covalent bond? How is this different from an ionic bond? A covalent bond is a pair of electrons sharing between atoms. An ionic bond 9. What kind of substances/elements form covalent bonds? 10.Why do ions form from atoms? 11. Why do ionic compounds form from ions? Atoms, Molecules, and Ions (8:18) https://www.youtube.com/watch?v=lPuY0OHa6RA&list=PLBwHfJmqJz5h5a6UxWpMrxV- İSIMKNSIN&index=12 Video starts at 1:15 min. 1. What is a molecular compound? 2. What is an ionic compound? 3. How do you distinguish between a molecular and an ionic compound?

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter12: Chemical Bonding

Section: Chapter Questions

Problem 31CR

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Think of forming an ionic compound as three steps (this is a simplification, as with all models): (I) removing an electron from the metal; (2) adding an electron to the nonmetal; and (3) allowing the metal cation and nonmetal anion to come together. a. What is the sign of the energy change for each of these three processes? b. In general, what is the sign of the sum of the first two processes? Use examples to support your answer. c. What must be the sign of the sum of the three process d. Given your answer to part c, why do ionic bonds occur? e. Given your above explanations, why is NaCl stable but not Na2Cl? NaCl2? What about MgO compared to MgO2? Mg2O?
What is resonance? Give three examples of molecules or ions that exhibit resonance, and draw Lewis structures for each of the possible resonance forms.
xplain the difference between ionic bonding and covalent bonding. How can we use the periodic table to help us determine the type of bonding between alums?
Hydrogen 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?
Element First Ionization Energy (kJImol) Second Ionization Energy (kiImol) I K 419 3050 Ca 590 1140 75. Use principles of atomic structure to answer each of the following: (a) The radius of the Ca atom is 197 pm; the radius of the Ca2+ ion is 99 pm. Account for the difference. (b) The lattice energy of CaO(s) is 3460 kJ/mol; the lattice energy of K2O is 2240 kJ/mol. Account for the difference. (c) Given these ionization values, explain the difference between Ca and K with regard to their first and second ionization energies. Element First Ionization Energy (kJ/mol) Second Ionization Energy (kJ/mol) K 419 3050 Ca 590 1140 (d) The first ionization energy of Mg is 738 kJ/mol and that of Al is 578 kJ/mol. Account for this difference.
Explain the difference between a nonpolar covalent bond, a polar covalent bond, and an ionic bond.
Compare the properties of an ionic material such as sodium chloride with a room-temperature ionic liquid. Explain this difference.
7. What kind of bond is formed when two molecules share electrons to form a molecule? a. Covalent b. Ionic c. Polar ionic d. Metallic 8. Why are transition metals special cases? a. They have two valence shells with complete octets that want to react. b. They have up to 8 electrons in their valence shell. c. They don't react with other elements because they are actually noble gases. d. They have two valence shells with an incomplete octet that want to react. 9. Name the following compound, BrF; a. Bromine pentafluoride b. Bromine fluoride c. Bromine (IV) fluoride d. Monobromine pentafluoride 10. Avron was conducting his science fair project when he came across a bottle of acid whose label read, "HSCN." What is the name of the acid that is contained within the bottle? a. Hydrocyanic acid b. Hydrothiocyanic acid c. Thiocyanic acid d. This acid does not exist 11. What is the chemical formula for copper (II) hydroxide? а. Cu,(ОН) b. CUOH с. CuOН, d. Cu(OH),
How do electrons distribute themselves in the shells of atoms? Know the maximum number of electrons in each of the first 3 shells. What is a covalent bond and what is the difference between polar and nonpolar covalent bonds? What is electronegativity? How is it important to covalent bonding? What are ions? What are cations and anions? What holds an ionic bond together? What is the difference between covalent bonds and ionic bonds? What is a hydrogen bond? Why is the study of structure and function important for molecules in the living world?
9. Which pair of atoms would form an ionic bond? a. bromine and oxygen b. chlorine and lithium c. carbon and nitrogen d. sodium and neon e. copper and chromium 15. Using only the periodic table, place the following atoms in order of increasing atomic radius: C, Ba, 0, Ca, and Ge. 21. What types of elements are bonded together to make an ionic compound? Give three examples of ionic compounds. Identify the types of elements that make up the compound in each example. 27. Describe how the physical state of a substance at room temperature depends on the strength of the intermolecular forces between the particles of the substance.
4. What does the Lewis structure explain between calcium and chlorine? çi Ca „Ċi: [ Ca ]2* 2[:Ċi:] A.calcium lose two electrons to chlorine C. chlorine gain one electron from calcium B.calcium gain two electrons to chlorine D. chlorine lose one electron from calcium 5. How many valence electrons does an atom of Silicon have? A. 2 В. 4 C.6 D. 8 6. Which of the following best describes polyatomic ions? A. always contains oxygen B. atoms with positive charge C. group of atoms with charge D. atoms with negative charge
Why does the octet rule not apply to transition metals? a. the octet rule does apply to transition metals as they are all classified as metals b. transition metals do not form cations or anions c. most transition elements form ions with more than one positive charge d. transition elements cannot be assigned with charges to form ions What do you call the process of positive and negative ions of an ionic compound separating from each other when solubilized in water? a. dissociation b. solubilization c. differentiation d. precipitation Which of the following statements is considered true? a. The size of an atom is determined by the size of the outermost occupied orbital b. Higher ionization energy means that the electron is more difficult to remove c. both are correct d. both are incorrect