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Oct 23, 2014 · The Expanded Octet: In many of the compound in the third period of the periodic table, the 3d orbital is also available for bonding. Compounds of such elements show an expanded octet. For example: PF 6, SF 6, H 2 SO 4.


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Therefore, the d orbitals participate in bonding with other atoms and an expanded octet is produced. Examples of molecules in which a third period central atom contains an expanded octet are the phosphorus pentahalides and sulfur hexafluoride.

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How many of the following elements can form compounds with an expanded octet?S Kr Xe Ba. 0b. 1c. 2d. 3e. 4 Solved • Oct 11, 2019 Octet Rule

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the octet rule is not satisfied for all the atoms. Expanded octet: Elements belonging to groups 15, 16 and 17 have more than four electrons in their valence (outermost) shell. The elements of these groups form stable compounds in which there are more than eight electrons around the central atom. Examples: PF 5, PCl 5, IF 6, SF 6

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Feb 08, 2014 · The octet rule is the understanding that most atoms seek to gain stability in their outer most energy level by filling the s and p orbitals of the highest energy level with eight electrons. Carbon has an electron configuration of 1s^2 2s^2 2p^2 this means that carbon has four valence electrons 2s^2 2p^4. Carbon seeks out four additional electrons to fill the p orbital and gain the stability of ...

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Nov 19, 2016 - Ionic bonds, covalent bonds, nomenclature, reactions, acids and bases. See more ideas about teaching chemistry, chemistry, teaching science.

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When atoms form compounds, the octet rule is not always satisfied for all atoms at all times, but it is a very good rule of thumb for understanding the kinds of bonding arrangements that atoms can make. It is not impossible to violate the octet rule. Consider sodium: in its elemental form, it has one valence electron and is stable.

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SKILL LEVEL Elementary, Middle School, High School TRY IT! There are many ways that elements can join together to form compounds, depending on the nature of the chemical bonds that form between them. For example, when a nonmetal (elements in the upper right of the periodic table, such as nitrogen or oxygen) combines with another …

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Q. Write a Lewis structure for each of the following molecules that are exceptions to the octet rule.BBr3 NO ClO2 Q. Draw a Lewis structure for SiCl4 and answer the following questions based on your drawing.1.

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Periodic Table. The Periodic Table of the Elements is the chemist’s friend. It is an extremely useful tool. Based upon its trends, we can make many predictions in regard to element behavior and to some extent physical properties.

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A) C B) Br C) F D) Be E) None of the above can form compounds with an expanded octet.
The use of term ‘Zero Group’ to refer to this group of chemical elements can be traced to the initial assumption that these gases had a valence of zero, owing to which they were not able to form compounds.
38) How many of the following elements can form compounds with an expanded octet? I O Cl Xe A) 2 B) 0 C) 3 D) 1 E) 4 Answer: C 39) How many of the following elements can form compounds with an expanded octet? Pb Kr Si B A) 0 B) 1 C) 2 D) 3 E) 4 Answer: D 40) Choose the bond below that is the strongest. A) C-F B) C=O C) C-I D) I-I E) C≡N
For example, group 17 elements (one group left of the noble gases) form 1− ions; group 16 elements (two groups left) form 2− ions, and so on. This trend can be used as a guide in many cases, but its predictive value decreases when moving toward the center of the periodic table. is a platform for academics to share research papers.

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The names of the elements can be cumbersome to write in full, especially when combined to form the names of compounds. Therefore, each element name is abbreviated as a one- or two-letter chemical symbol1. By convention, the first letter of a chemical symbol is a capital letter, while the second letter (if there is one) is a lowercase letter.
To decide if a binary compound has ionic or covalent bonding, first locate the two elements concerned in the Periodic Table and decide if they are metals (shown in blue) or non-metals (shown in pink). If they are both non-metals (such as carbon and oxygen) they will form a covalent compound (such as carbon dioxide, CO 2).