The valence of an element is the number of covalent bonds its atoms form or the charge on the ion it forms in ionic compounds. For the following questions, use the position of an element in the periodic table to deduce its valence. (1) What is the valence of nitrogen? 8 (2) What is the valence of sodium? (3) What is the valence of calcium? e

The valence of an element is the number of covalent bonds its atoms form or the charge on the ion it forms in ionic compounds. For the following questions, use the position of an element in the periodic table to deduce its valence. (1) What is the valence of nitrogen? 8 (2) What is the valence of sodium? (3) What is the valence of calcium? e

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter2: Atoms

Section: Chapter Questions

Problem 2.98P: 2-98 Explain how the ionization energy of atoms changes when proceeding down a group of the Periodic...

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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.
The valence of an element is the number of covalent bonds its atoms form or the charge on the ion it forms in ionic compounds. For the following questions, use the position of an element in the periodic table to deduce its valence. (1) What is the valence of strontium? (2) What is the valence of arsenic? (3) What is the valence of hydrogen?
Consider the following elements in their stable forms: Chlorine Fluorine Bromine Carbon Then for each of the following questions, enter the number listed (1-4) before the element, for elements that satisfy the criterion. Enter the number(s) in order with no separators. If none, type "none" or leave blank. (a) Which of these elements have allotropes? fill in the blank 2d8840092ffc02e_1 (b) Which of these elements exist as diatomic molecules? fill in the blank 2d8840092ffc02e_2 (c) Which of these elements exist as a metallic lattice?
Answer true or false. (a) The octet rule refers to the chemical bonding patterns of the first eight elements of the Periodic Table. (b) The octet rule refers to the tendency of certain elements to react in such a way that they achieve an outer shell of eight valence electrons. (c) In gaining electrons, an atom becomes a positively charged ion called a cation. (d) When an atom forms an ion, only the number of valence electrons changes; the number of protons and neutrons in the nucleus does not change. (e) In forming ions, Group 2A elements typically lose two electrons to become cations with a charge of 12. (f) In forming an ion, a sodium atom (1s22s22p63s1) completes its valence shell by adding one electron to fill its 3s shell (1s22s22p63s2). (g) The elements of Group 6A typically react by ac- cepting two electrons to become anions with a charge of 22. (h) With the exception of hydrogen, the octet rule applies to all elements in periods 1, 2, and 3. (i) Atoms and the ions derived from…
Illustrated are four ions — A, B, X, and Y— showing their relative ionic radii. The ions shown in red carry positive charges: a 2+ charge for A and a 1+ charge for B. Ions shown in blue carry negative charges: a 1- charge for X and a 2- charge for Y. (a) Which combinations of these ions produce ionic compounds where there is a 1:1 ratio of cations and anions?(b) Among the combinations in part (a), which leads to the ionic compound having the largest lattice energy? Why?
A fluorine atom has 9 electrons - 7 in its outer shell and 2 in its inner shell. How many electrons would be in the outer shell if it were to become a fluoride ion?
2 (S 18 PERIMENT D Flame Tests: Which lon Causes the Color? Part A: Laboratory Results Summarize your laboratory results in the following data table after examining the color of the flame. Complete the table by filling in the flame test color and the missing chemical formulas, and ions (cation and/or anion). MATERIAL/COMPOUND TESTED Sodium Chloride NaCl Sodium Carbonate Strontium Acetate Copper (II) Sulfate Lithium Carbonate Potassium Sulfate Sodium Phosphate Barium Nitrate CATION PRESENT ANION PRESENT Na¹+ Na¹+ Sr2+ ㅎ CIT- CO3²- C₂H30₂¹- SO4²- CO3²- SO4²- PO4³- NO 3¹- Data detailed FLAME TEST COLOR orange greenish with a spark of crange Orange with a sparn в purple oraine outler spergi be sparvo of crange red with crant with still be due fame affranks ready bottarg Orange that arany -sparks up on greenish reatly no change oranze purple, at first a little thi turned back blue notice green crange Purple, peach red at top bright arany blue at botter Blue, Crans green Jumped different Did…
As seen in the table, compounds containing an integer ratio of elements depend on how many cations combine with how many anions to form a stable compound. For example, in table 1, to form a NaCl compound, first Na ionizes from the Na+ cation which is having +1 positive charge, which will lose 1 electron, it is having +1 charge, this electron then goes to Cl and it will change to Cl- anion by gaining the electron, so here 1:1 ratio charge which means 1 Na+ combines with 1 Cl-1 to form NaCl. So here integer ratio is 1:1 for this sodium chloride compound. As listed in table 2, Mg(OH)2, the integer ratio is 1:2 which means, Mg is a neutral atom that loses 2 electrons and forms an Mg+2 cation, which combines with OH which gains 1 electron to form OH- anion, So here Mg2+ can combine with 2 OH- anion, so they both combine to form Mg(OH)2 which has integer ratio as 1:2 . Thus, atom forms as ions by losing or gaining electrons and combines together in whole number ratio to form stable…
39. How many grams are in 2.3 x 104 formula units of KNO,? (A) 38.6 grams (B) 102.3 grams (C) 140 gramsS (D) 386 grams 40. Which statement describes the general trends in electronegativity and first ionization energy as the elements in Period 3 are considered in order from Na to Cl? (A) Electronegativity increases, and first ionization energy decreases (B) Electronegativity decreases, and first ionization energy decreases (C) Electronegativity and first ionization energy both increase (D) Electronegativity and first ionization energy both decrease 2020 Illuminate Education TM, Inc. 9.
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