Ionic bonds also show unequal charges in bonding. However, due to the strong electronegativity of one atom, the e- will be pulled away leaving ___________ on the two atoms. This creates _____________. These are often created in water in organisms to carry out metabolic functions. Give an example: ______________

Could someone help me?? The answer to this question must look similar to the example attached.   Back ground info:  Atoms of different elements combine with one another to form compounds. It is important to be able to explain how atoms actually come together to form these compounds or chemical bonds. One of the three types of bonds is an ionic bond which is a bond between a metal atom and a nonmetal atom, or a cation and an anion. The Octet Rule is the driving force behind ionic bond formation. The octet rule refers to the tendency of atoms to prefer to have eight electrons in the valence shell. When atoms have fewer than eight electrons, they tend to react and form more stable compounds. When discussing the octet rule, we do not consider d or f electrons. Only the s and p electrons are involved in the octet rule, making it useful for the main group elements (elements not in the transition metal or inner-transition metal blocks); an octet in these atoms corresponds to an electron…

1. Consider the structure shown below and then answer the following questions. a. Complete the structure by adding the missing formal charges. All atoms and lone pairs are explicitly shown. (Hint: Consider the number of bonds neutral atoms have.) :Ö: H ‚H H H b. Draw two more resonance structures of the molecule from part a by adding the missing î bonds, lone pairs, and formal charges. All atoms in both structures should possess an octet. (All atoms and o bonds are drawn for you; remember, only lone pairs and bonds move in resonance structures.) Additional guidelines are given for each structure. All atoms in this structure will be neutral (no formal charges). One oxygen atom has a +1 formal charge and one oxygen atom has a -1 formal charge. H H H H H H H H H

1 What is the total number of valence electrons in the Lewis structure of BrO4"? electrons 2 Draw a Lewis structure for BrO4 • Do not include overall ion charges or formal charges in your drawing. • If the species contains oxygen, do not draw double bonds to oxygen unless they are needed in order for the central atom to obey the octet rule. 0- Y **** O. Sn [1 2. Draw Lewis Structures (Octet and Nonoctet): This is group attempt 1 of 5

Write the electron dot structure for hydroxide ion, [OH]-a. What is the total number of available valence electrons?______Remember that hydroxide has a -1 charge, so an extra valence electron must be added to the total.b. In the space below, arrange the atomic symbols, then add bonding electron pairs. Distribute non-bonding electron pairs. Don’t forget to indicate the charge on the finished structure.

3. What type of elements form ionic bonds with metals? 4. What type of elements form ionic bonds with nonmetals? 5. Write the chemical formula that results when the following pairs of ions combine to form an ionic bond. a. Sr2+ and 02- b. Mn4+ and O2- C. Lil+ and CI- d. Cs1+ and S2-

To answer the questions, interpret the following Lewis diagram for NHF2 .     1.  For the central  nitrogen  atom:   ... The number of non-bonding electrons =    The number of bonding electrons =    The total number of electrons =  2.  The central  nitrogen  atom fill in the blank 4   ... A. obeys the octet rule.   B. has more than an octet.   C. has less than an octet.

Chemistry: Bonding 4a. Draw the Lewis structure for CH4, (methane), NH3, (ammonia), and H20 (water). b. Calculate the bond polarity for the C-H bond, N-H bond, and O-H bond. c. Classify these molecules as either polar or nonpolar. If the molecule is polar, label the partial negative and partial positive sides of the molecules you drew above.

Only one of the following Lewis dot structures for water (dihydrogen monoxide) is correct. A B H-O-H: H=O=H H-Ö-H- H-O-H C Determine which one is correct. Cite evidence and reasoning to support why it's drawn correctly. Include evidence and reasoning to support why the other three are drawn incorrectly. each structure)

rn/takeAssignment/takeCovalentActivity.do?locator=Dassignment-take [Review Topics] [References] Use the References to access important values if needed for this question. The following Lewis diagram represents the valence electron configuration of a main-group element. This element is in group According to the octet rule, this element would be expected to form an ion with a charge of| If X is in period 4, the ion formed has the same electron configuration as the noble gas The symbol for the ion is M Submit Answer Retry Entire Group 8 more group attempts remaining M) M ts 2reg pts M) 1 pts OM) Previous Next Email Instructor Save and Exit