Chemistry
4th Edition
ISBN: 9780078021527
Author: Julia Burdge
Publisher: McGraw-Hill Education
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Chapter 2, Problem 100AP
Interpretation Introduction
Interpretation:
The elements that are more likely to form ionic compounds and the metallic elements that are likely to form cations with different charges are to be discussed.
Concept introduction:
An ionic bond is the
When an atom loses electrons, it forms a cation and when the atom accepts electrons, it forms an anion.
The oxidation state describes the degree of oxidation of an atom in a chemical compound.
There are some metals that exhibit variable oxidation states, like
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Write formulas for ionic compounds.
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Cation formula
Anion formula
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Answer true or false.
(a) The name of a binary ionic compound consists of the name of the positive ion followed by the name of the negative ion.
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(c) The formula of aluminum oxide is Al2 O3 .
(d) Both copper(II) oxide and cupric oxide are acceptable names for CuO.
(e) The systematic name for Fe2 O3 is iron(II) oxide.
(f) The systematic name for FeCO3 is iron carbonate.
(g) The systematic name for NaH2PO4 is sodium di- hydrogen phosphate.
(h) The systematic name for K2HPO4 is dipotassium hydrogen phosphate.
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(j) The systematic name for PCl3 is potassium chloride.
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39.
(a) A covalent bond is formed between two atoms whose difference in electronegativity is less than 1.9.
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Chapter 2 Solutions
Chemistry
Ch. 2.1 - Practice Problem ATTEMPT
In each case, calculate...Ch. 2.1 - Practice Problem BUILD
(a) Two of the simplest...Ch. 2.1 - Practice Problem CONCEPTUALIZE
Which of the...Ch. 2.1 - For the two compounds pictured, evaluate the...Ch. 2.1 - Prob. 2CPCh. 2.2 - Practice ProblemATTEMPT How many protons,...Ch. 2.2 - Practice ProblemBUILD Give the correct symbols to...Ch. 2.2 - Prob. 1PPCCh. 2.3 - 2.3.1 How many neutrons are there in an atom of
Ch. 2.3 - Prob. 2CP
Ch. 2.3 - Practice ProblemATTEMPT The atomic masses of the...Ch. 2.3 - Practice ProblemBUILD The average atomic mass of...Ch. 2.3 - Practice Problem CONCEPTUALIZE
The following...Ch. 2.4 - Which of the following series of elemental symbols...Ch. 2.4 - 2.4.2 Which of the following elements would you...Ch. 2.4 - Practice Problem ATTEMPT
Name the following ionic...Ch. 2.4 - Practice Problem BUILD
Name the following ionic...Ch. 2.4 - Practice ProblemCONCEPTUALIZE The diagram...Ch. 2.5 - Boron has two naturally occurring isotopes, which...Ch. 2.5 - 2.5.2 The two naturally occurring isotopes of...Ch. 2.5 - Practice Problem ATTEMPT
Deduce the formulas of...Ch. 2.5 - Practice ProblemBUILD Deduce the formulas of the...Ch. 2.5 - Practice Problem CONCEPTUALIZE
The diagram...Ch. 2.6 - Prob. 1PPACh. 2.6 - Practice ProblemBUILD Name the following species:...Ch. 2.6 - Prob. 1PPCCh. 2.6 - Prob. 1CPCh. 2.6 - Prob. 2CPCh. 2.6 - Prob. 3CPCh. 2.6 - 2.6.4 What is the formula of nickel(II) nitrate...Ch. 2.6 - Prob. 5CPCh. 2.6 - Prob. 6CPCh. 2.7 - Practice ProblemATTEMPT Chloroform was used as an...Ch. 2.7 - Practice ProblemBUILD Write the molecular formula...Ch. 2.7 - Prob. 1PPCCh. 2.7 - Prob. 1CPCh. 2.7 - 2.7.2 What is the name of the compound...Ch. 2.7 - What is the correct formula for the compound...Ch. 2.7 - 2.7.4 What is the empirical formula of the...Ch. 2.8 - Practice Problem ATTEMPT
Name the following...Ch. 2.8 - Practice ProblemBUILD Name the following binary...Ch. 2.8 - Practice Problem CONCEPTUALIZE
Name the binary...Ch. 2.9 - Practice ProblemATTEMPT Give the molecular formula...Ch. 2.9 - Practice ProblemBUILD Give the molecular formula...Ch. 2.9 - Prob. 1PPCCh. 2.10 - Practice ProblemATTEMPT Determine the formula of...Ch. 2.10 - Practice ProblemBUILD Determine the formula of...Ch. 2.10 - Practice ProblemCONCEPTUALIZE Referring to the...Ch. 2.11 - Practice Problem ATTEMPT
Write empirical formulas...Ch. 2.11 - Practice ProblemBUILD For which of the following...Ch. 2.11 - Practice ProblemCONCEPTUALIZE Which of the...Ch. 2 - Prob. 1KSPCh. 2 - Prob. 2KSPCh. 2 - Prob. 3KSPCh. 2 - What is the correct formula for phosphorus...Ch. 2 - What are the hypotheses on which Dalton's atomic...Ch. 2 - State the laws of definite proportions and...Ch. 2 - Prob. 3QPCh. 2 - Prob. 4QPCh. 2 - 2.5 Sulfur reacts with fluorine to produce three...Ch. 2 - 2.6 Both and contain only iron and oxygen. The...Ch. 2 - For the two compounds pictured, evaluate the...Ch. 2 - 2.8 For the two compounds pictured, evaluate the...Ch. 2 - Prob. 9QPCh. 2 - Prob. 10QPCh. 2 - Prob. 11QPCh. 2 - Describe the contributions of the following...Ch. 2 - 2.13 Describe the experimental basis for believing...Ch. 2 - The diameter of a neutral helium atom is about 1 ×...Ch. 2 - Prob. 15QPCh. 2 - Prob. 16QPCh. 2 - Prob. 17QPCh. 2 - Prob. 18QPCh. 2 - Prob. 19QPCh. 2 - 2.20 What is the mass number of an iron atom that...Ch. 2 - Prob. 21QPCh. 2 - 2.22 For each of the following species, determine...Ch. 2 - 2.23 Indicate the number of protons, neutrons, and...Ch. 2 - Prob. 24QPCh. 2 - Prob. 25QPCh. 2 - 2.26 Determine the mass number of (a) a boron atom...Ch. 2 - Prob. 27QPCh. 2 - Prob. 28QPCh. 2 - What is the periodic table, and what is its...Ch. 2 - 2.30 State two differences between a metal and a...Ch. 2 - Prob. 31QPCh. 2 - Give two examples of each of the following: (a)...Ch. 2 - Prob. 33QPCh. 2 - Prob. 34QPCh. 2 - Prob. 35QPCh. 2 - Prob. 36QPCh. 2 - Prob. 37QPCh. 2 - Prob. 38QPCh. 2 - Prob. 39QPCh. 2 - Prob. 40QPCh. 2 - Prob. 41QPCh. 2 - Prob. 42QPCh. 2 - Prob. 43QPCh. 2 - Prob. 44QPCh. 2 - The atomic masses of 204 Pb ( 1 .4 percent ) . 206...Ch. 2 - Prob. 46QPCh. 2 - Prob. 47QPCh. 2 - 2.48 What is the mass in grams of 13.2 amu?
Ch. 2 - Prob. 49QPCh. 2 - Prob. 50QPCh. 2 - Prob. 51QPCh. 2 - Prob. 52QPCh. 2 - Prob. 53QPCh. 2 - Prob. 54QPCh. 2 - Prob. 55QPCh. 2 - Prob. 56QPCh. 2 - Prob. 57QPCh. 2 - Prob. 58QPCh. 2 - Prob. 59QPCh. 2 - Prob. 60QPCh. 2 - 2.61 Name the following compounds:
Ch. 2 - Prob. 62QPCh. 2 - Prob. 63QPCh. 2 - Prob. 64QPCh. 2 - Prob. 65QPCh. 2 - Prob. 66QPCh. 2 - Prob. 67QPCh. 2 - Prob. 68QPCh. 2 - Prob. 69QPCh. 2 - Prob. 70QPCh. 2 - Prob. 71QPCh. 2 - Prob. 72QPCh. 2 - Prob. 73QPCh. 2 - Prob. 74QPCh. 2 - Prob. 75QPCh. 2 - Prob. 76QPCh. 2 - Prob. 77QPCh. 2 - Prob. 78QPCh. 2 - Prob. 79QPCh. 2 - Prob. 80QPCh. 2 - Prob. 81QPCh. 2 - Prob. 82QPCh. 2 - Prob. 83QPCh. 2 - Prob. 84QPCh. 2 - Prob. 85QPCh. 2 - Prob. 86QPCh. 2 - Prob. 87APCh. 2 - Prob. 88APCh. 2 - Prob. 89APCh. 2 - One isotope of a metallic element has mass number...Ch. 2 - Prob. 91APCh. 2 - Prob. 92APCh. 2 - 2.93 What is wrong with or ambiguous about the...Ch. 2 - Prob. 94APCh. 2 - Prob. 95APCh. 2 - Prob. 96APCh. 2 - Prob. 97APCh. 2 - Prob. 98APCh. 2 - Prob. 99APCh. 2 - Prob. 100APCh. 2 - Prob. 101APCh. 2 - Prob. 102APCh. 2 - Prob. 103APCh. 2 - Determine the molecular and empirical formulas of...Ch. 2 - Prob. 105APCh. 2 - Prob. 106APCh. 2 - The Group 1B metals . Cu, Ag, and Au, are called...Ch. 2 - Prob. 108APCh. 2 - Prob. 109APCh. 2 - Prob. 110APCh. 2 - Two elements form a compound that can be...Ch. 2 - Which of the diagrams can be used to illustrate...Ch. 2 - Prob. 113APCh. 2 - Prob. 114APCh. 2 - Prob. 115APCh. 2 - 2.116 Show the locations of (a) alkali metals, (b)...Ch. 2 - Prob. 117APCh. 2 - Prob. 118APCh. 2 - Prob. 119APCh. 2 - 2.120 (a) Describe Rutherford’s experiment and how...Ch. 2 - Prob. 121APCh. 2 - Prob. 122APCh. 2 - Prob. 123APCh. 2 - A cube made of platinum (Pt) has an edge length of...Ch. 2 - Prob. 125APCh. 2 - Prob. 126APCh. 2 - Prob. 1SEPPCh. 2 - Prob. 2SEPPCh. 2 - Prob. 3SEPPCh. 2 - Prob. 4SEPP
Knowledge Booster
Similar questions
- Answer true or false. (a) For Group 1A and Group 2A elements, the name of the ion each form is simply the name of the element followed by the word ion; for example, Mg21 is named magnesium ion. (b) H2 is named hydride ion. (c) The nucleus of H1 consists of one proton and one neutron. (d) Many transition and inner transition elements form more than one positively charged ion. (e) In naming metal cations with two different charges, the suffix -ous refers to the ion with a charge of 11 and -ic refers to the ion with a charge of 12. (f) Fe31 may be named either iron (III) ion or ferric ion. (g) The anion derived from a bromine atom is named bromine ion. (h) The anion derived from an oxygen atom is named oxide ion. (i) HCO3 2 is named hydrogen carbonate ion. (j) The prefix bi- in the name “bicarbonate” ion indicates that this ion has a charge of 22. (k) The hydrogen phosphate ion has a charge of 11, and the dihydrogen phosphate ion has a charge of 12. (l) The phosphate ion is PO3 42. (m)…arrow_forwardName the following binary ionic compounds. (a) MgF2 (b) Bal2 (c) FeCl2arrow_forwardMany chemical names are similar at first glance. Give the for-mulas of the species in each set: (a) ammonium ion and ammo-nia; (b) magnesium sulfide, magnesium sulfite, and magnesiumsulfate; (c) hydrochloric acid, chloric acid, and chlorous acid; (d) cuprous bromide and cupric bromidearrow_forward
- Which of the following sets contains an ionic compound, a molecular compound, and an acid, in that order? (A) Al2O3, B2O3, CH3OH; (B) CaCl2, NH4Cl, HCl; (C) CH3F, COCl2, HOCl; (D) CoCl2, COCl2, HClO2.arrow_forwardWhich of the following pairs react to form ioniccom-pounds: (a) Cl and Br; (b) Na and Br; (c) P and Se; (d) H and Ba?.arrow_forwardIllustrated 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?arrow_forward
- Many chemical names are similar at first glance. Give the formulas of the species in each set: (a) Ammonium ion and ammonia (b) Magnesium sulfide, magnesium sulfite, and magnesium sulfate (c) Hydrochloric acid, chloric acid, and chlorous acid (d) Cuprous bromide and cupric bromidearrow_forwardBased on Linus Pauling's electronegativity scale, would H2S be considered a polar molecule? Pick the best answer. (a) No. It would technically be considered a non-polar molecule. (b) No. Even though it contains polar bonds they are symmetrical and therefore H2S is non-polar. (c) No. The electronegativity difference between H and S is so great that it would be considered an ionic compound. (d) H2S violates the octet rule and therefore would not even existarrow_forwardWhat are the chemical formulas for ( a ) disulfur dioxide and ( b ) iodine pentafluoride ?arrow_forward
- The compound SiO2 does not exist as a discrete molecule while CO2 does. This is because ________. (A) CO2 is a molecular compound, whereas SiO2 is an ionic compound. (B) The SiO2 is solid while CO2 is a gas. (C) The sigma bond between Si and O atoms is very weak. (D) The Si atom does not form a stable pi-bond with the O atom.arrow_forwardWrite the formula of the compound that will be formed between these elements: (a) H and F (b) Cs and P (c) Al and Clarrow_forwardElements in the same group of the periodic table often form oxyanions with the same general formula. The anions are also named in a similar fashion. Based on these observations, suggest a chemical formula or name, as appropriate, for each of the following ions: (a) BrO4 -, (b) SeO3 2-, (c) arsenate ion, (d) hydrogen tellurate ion.arrow_forward
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