For Calcium atom answer the following questions: 1) How many protons does it have? 20 protons 2) How many electrons does it have? 20 electrons 3) How many valence electrons does it have? 2 valence electrons 4) Show full electron configuration (use format similar to this example: 1s2 252 2p6 3s2 ) 4 s2 5) The number of dots on the Lewis structure o 6) How many electrons does it need to lose or gain to achieve the stable octet? 2 (lose/gain) electrons 7) What is the net charge after losing/gaining some electrons? 2 8) Did it become a cation or an anion? cation 9) Show electron configuration after transformation to cation or anion? (use format similar to this example: 1s2 2s2 2p6 3s2) 4 s2 10) Now which noble gas has an electron configuration identical to electron configuration this lon? Argon

For Calcium atom answer the following questions: 1) How many protons does it have? 20 protons 2) How many electrons does it have? 20 electrons 3) How many valence electrons does it have? 2 valence electrons 4) Show full electron configuration (use format similar to this example: 1s2 252 2p6 3s2 ) 4 s2 5) The number of dots on the Lewis structure o 6) How many electrons does it need to lose or gain to achieve the stable octet? 2 (lose/gain) electrons 7) What is the net charge after losing/gaining some electrons? 2 8) Did it become a cation or an anion? cation 9) Show electron configuration after transformation to cation or anion? (use format similar to this example: 1s2 2s2 2p6 3s2) 4 s2 10) Now which noble gas has an electron configuration identical to electron configuration this lon? Argon

Introductory Chemistry For Today

8th Edition

ISBN:9781285644561

Author:Seager

Publisher:Seager

Chapter4: Forces Between Particles

Section: Chapter Questions

Problem 4.100E

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Answer the following questions List three elements that have 2 electrons in their valence shell. List three elements that have filled valence shells. List three elements that are one electron short of having a filled valence shell. As you work your way across the periodic table from left to right in any given row, what it happening to the electronic structure of the atoms? What property of an element is described by its electronegativity? How does electronegativity typically changes going across the periodic table? Why is that? How does electronegativity typically change going down the periodic table? Why is that? On a scale that goes from nonpolar bond to increasingly polar bond to ionic bond, how would you expect these bonds to be ranked? Why? NaCl, CO, OO, CaO, HCl, SiC If the bonds in a molecule are, in fact, polar, would the molecule as a whole also be polar for each of the following shapes? Why?…
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 configuration ending with s2p6. One way an atom can satisfy the Octet Rule is by transferring valence…
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?
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State true or false for the following: Within a period, elements with higher atomic numbers require more energy to remove an electron from the atom, because the atoms have higher effective nuclear charge. Within a family, elements with higher atomic numbers require more energy to remove an electron from the atom, because the valance electrons are in lower principal energy levels. Within a family, elements with lower atomic numbers have higher electronegativity because the atoms have higher effective nuclear charge.
1, The bonds in the compound OF2 are characterized as Group of answer choices coordinate covalent A, ionic B, polar covalent C, non-polar covalent 2,What is the "general" formula for the compound that forms between an element in Group IA ( M) and Group VIA (N)? Group of answer choices A, MN B, MN6 C, M2N D, MN2 E, M6N
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Be sure to answer all parts. Identify the correct Lewis electron-dot symbol for the ion formed from each of the following atoms: Br    −    3−    2−    − Li    LI3+    Li2+    Li2−    Li+ Predict the formula of their compound:
Draw the Lewis structure for OSiS before answering the following questions (You do NOT submit a picture just answer the questions). Silicon is the central atom and all atoms obey the octet rule. WARNING:  Do NOT USE the internet or other sources to find the structures. Use ONLY the rules taught in class. ALL atoms obey the octet rule Answer the following questions for the Lewis structure for OSiS , given that silicon is the central atom and all atoms obey the octet rule. Give answers as numbers (1,2,3 ...etc.) NOT words (one, two three etc.) How many double bonds exist in this structure How many electrons surround the silicon atom How many lone pairs are around the silicon atom How many lone pairs are around the sulfur atom How many lone pairs are around the oxygen atom How many electrons surround the Sulfur atom