17. a) How many valence electrons are there in an atom of each of these elements? neon; bromine; sulfur; strontium; sodium; chlorine; tin; magnesium; silicon. b) Draw the Lewis structure for the elements in a) above. c) Without consulting a periodic table, classify each element from a) above as metal, non-metal or metalloid.

17. a) How many valence electrons are there in an atom of each of these elements? neon; bromine; sulfur; strontium; sodium; chlorine; tin; magnesium; silicon. b) Draw the Lewis structure for the elements in a) above. c) Without consulting a periodic table, classify each element from a) above as metal, non-metal or metalloid.

Living by Chemistry

2nd Edition

ISBN:9781464142314

Author:Angelica M. Stacy

Publisher:Angelica M. Stacy

ChapterU2: Smells: Molecular Structure And Properties

Section: Chapter Questions

Problem 6STP

See similar textbooks

Similar questions

What is the difference between sulfuric acid and hydrosulfuric acid?
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?
2.26 In what region of the periodic table are you likely to find elements that form more than one stable ion?
2-98 Explain how the ionization energy of atoms changes when proceeding down a group of the Periodic Table and explain why this change occurs.
What are the chemical formulas for ( a ) disulfur dioxide and ( b ) iodine pentafluoride ?
Hello, sorry I think I was a bit bland with the question. In the periodic descriptions attached below, how did you come to the conclusion that the letters equalled the elements in the chart?- Which clue helped you figure that out for each element. (Provide a small explanation of how you came to the conclusion using the given properties.) Also, how does the Hydride, Chloride, and Oxide tell about the element? How is that helping us when finding the element? Alphabet Element Name Alphabet Element Name Alphabet Element Name A C Carbon J Ca Calcium S Ar Argon B F Fluorine K Ne Neon T Mg Magnesium C I Iodine L Be Beryllium U Rb Rubidium D Li Lithium M K Potassium V Ba Barium E He Helium N Ba Barium W Cl Chlorine F Fr Francium P Kr Krypton X Sn Tin G Xe Xenon Q Ge Germanium Y Pb Lead I Si Silicon R Br Bromine Z Na Sodium
Which one in each pair has the larger radius ? Explain. (a) a magnesium ion or an aluminum ion (b) a sodium atom or a silicon atom (c) a potassium ion or bromide ion
What information do you need to write a correct chemicalformula to represent an ionic compound?
How many electrons does each of the following elements have in its outermost electron shell? Draw the Lewis Dot Structure.(a) Potassium (b) Calcium (c) Aluminum
Illustrate the sharing of electrons of each covalent compound using the Bohr Model. Apply the octet rule if possible. (A) A molecule composed of two chlorine atoms. (b) A molecule composed of a hydrogen atom and a bromine atom. (c) A molecule composed of 2 hydrogen atoms. (d) A molecule composed of a hydrogen atom and a chlorine atom.
Section 1. Answer the following questions about magnesium: a) Write the longhand and shorthand configuration: b) How many of the electrons are valence electrons? c) If magnesium were to form a positive ion by losing valence electrons, what charge would result? d) Would you expect the ion to be larger or smaller in volume than the neutral atom? Why?
[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. •X• 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 5, the ion formed has the same electron configuration as the noble gas The symbol for the ion is Submit Answer Retry Entire Group 8 more group attempts remaining Cengage LearningI Cengage Technical Support 96 F Sunny