Be sure you can predict ion formation from the previous module. (In other words--what is the charge expected when an atom forms an ion). Remember an ion is a charged particle that results from the loss or gain of 1 or more electrons. The number of electrons that an atom will lose or gain is based on its group number from the periodic table. Ca N Li Br S Al

Be sure you can predict ion formation from the previous module. (In other words--what is the charge expected when an atom forms an ion). Remember an ion is a charged particle that results from the loss or gain of 1 or more electrons. The number of electrons that an atom will lose or gain is based on its group number from the periodic table. Ca N Li Br S Al

Living By Chemistry: First Edition Textbook

1st Edition

ISBN:9781559539418

Author:Angelica Stacy

Publisher:Angelica Stacy

ChapterU1: Alchemy: Matter, Atomic Structure, And Bonding

SectionU1.18: Life On The Edge: Valence And Core Electrons

Problem 6E

See similar textbooks

Similar questions

1. Hydrogen is a Group I element and each hydrogen will contribute I valence electron. Carbon is a Group (Roman numeral) element and each carbon will contribute ___ (number) electrons. Every oxygen atom in a compound will contribute valence electrons. Chloromethane has the molecular formula . Its skeleton is and the number of valence electrons may be determined as follows. There are three hydrogen atoms, each of which contributes 1 valence electron; the single carbon contributes 4 electrons; and the single chlorine atom contributes 7 electrons, making a total of 14 . A convenient tabular form of this calculation is
Complete the following statements: Metals have ____, ____ or ____ electrons in their valence shell and need to __________ these electrons to achieve a full outer shell and become stable. Metals form _____________charged ions as they end up with ________protons than electrons.
A particular atom, in its neutral form, has 90 electrons; how many electrons will a corresponding negative ion have?
Complete the following statement: Non metals have ____, ____ or ____ electrons in their outer shell and need to __________ these electrons to achieve a full outer shell and become stable. Non metals form _____________charged ions as they end up with ________ protons than electrons.
how many electrons would an sr atom lose or gain to become an ion
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
Briefly explain the various scientists involved in the creation of the atomic model and what their view of the atom was Explain what the Quantum Mechanical model of the atom proposes Identify the number of protons/neutrons/electrons in a neutral element and in an ion Describe the different types of radioactive decay Calculate the average atomic mass of an element Define electronegativity, electron affinity, reactivity, atomic and ionic radius, ionization energy explain how each trend increases along a group and a column compare various elements to answer questions regarding C periodic trends Explain WHY a trend increases the way it does in a period or O group Interpret data of ionization energies Define the following: shielding effect, effective nuclear charge, the periodic law, cation, valence electrons, atomic mass, anion, energy levels(orbital), element, isotope, radioisotope
Based on its outer shell, the atom in figure 2.5 would be characterized as ___.
The maximum number of valence electrons that any element in the periodic table may have is eight. True or False?
Does an increase in the number of electrons around the nucleus of an atom ALWAYS increase the size of the atom? Use CER, claim, evidence, reasoning. Your claim is your answer to the question. Evidence should be pulled from the periodic table. Include reasoning this should come after your evidence. Notes: Across a period: Even though there are more electrons, there also more protons. This results in more electrostatic attraction which pulls all the orbitals in tighter. Down a group: At the beginning of each new period, atoms have an additional orbital to provide room for additional electrons. The edditional orbital results in a much larger atom. Atoms get smaller across a period. Atoms get bigger down a group. When atoms absorb energy from their environment, the electrons move to higher energy orbitals farther from the nucleus. When atoms release energy to their environment in the form of visible-light, the elctrons move to lower energy orbitals closer to the nucleus. Period=number of…
If you were to add an electron to the atom in the image below, what would they be added to?
Sara suggests that when electrons change in number within atoms, an ion is formed. Therefore, if the atom loses electrons, it turns into a positive ion (cation), on the other hand, if an atom receives electrons, it turns into a negative ion (anion). True or False?