Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 2, Problem 6PE
Interpretation Introduction
Interpretation:
The number of protons and electrons in the given atoms or ions are to be determined.
Concept Introduction:
Atoms are composed of tiny particles known as protons, electrons, and neutrons.
The
Electron has negative charge, proton has positive charge and neutron has no charge.
Ions with negative charge must have gained electrons, and ions with positive charge must have lost electrons.
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
The element oxygen has three naturally occurring isotopes, with 8,9, and 10 neutrons in
the nucleus, respectively. (a) write the full chemical symbols for these three isotopes. (b)
Describe the similarities and differences between the three kinds of atoms of oxygen.
Fill in the blanks: (a) The symbol and atomic number of the heaviest alkaline earth metal are ______ and ______.
(b) The symbol and atomic number of the lightest metalloid in Group 4A(14) are ______ and ______.
(c) Group 1B(11) consists of the coinage metals. The symbol and atomic mass of the coinage metal whose atoms have the fewest electrons are ______ and ______.
(d) The symbol and atomic mass of the halogen in Period 4 are ______ and ______.
Write the symbol for each of the following ions. (Enter your answer in the form
A
X
q±
Z
.)
(a)
the ion with a 3+ charge, 28 electrons, and a mass number of 69
(b)
the ion with 36 electrons, 35 protons, and 44 neutrons
(c)
the ion with 91 electrons, 148 neutrons, and a 4+ charge
(d)
the ion with a 2+ charge, atomic number 40, and mass number 90
Chapter 2 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 2 - Practice Exercise 2.11
How many atoms of each...Ch. 2 - Prob. 2PECh. 2 - How many atoms of each clement appear on each side...Ch. 2 - Prob. 4PECh. 2 - Prob. 5PECh. 2 - Prob. 6PECh. 2 - Prob. 7PECh. 2 - Write the formulas for the compounds made from (a)...Ch. 2 - Practice Exercise 2.9 Write all the formulas for...Ch. 2 - Prob. 10PE
Ch. 2 - Prob. 11PECh. 2 - Practice Exercise 2.12
Write the formula for the...Ch. 2 - Prob. 13PECh. 2 - Prob. 14PECh. 2 - Prob. 15PECh. 2 - Prob. 16PECh. 2 - Prob. 17PECh. 2 - Write the formulas for (a) potassium chlorate, (b)...Ch. 2 - Prob. 19PECh. 2 - Prob. 20PECh. 2 - Practice Exercise 2.21
Name the following...Ch. 2 - Practice Exercise 2.22
Write formulas for the...Ch. 2 - Prob. 23PECh. 2 - Prob. 24PECh. 2 - 2.1 In the compounds formed by with chlorine, how...Ch. 2 - Prob. 2RQCh. 2 - Prob. 3RQCh. 2 - 2.4 In the refining of copper, sizable amounts of...Ch. 2 - 2.5 Why would you reasonably expect cadmium to be...Ch. 2 - 2.6 Using the symbol for nitrogen, 147N02,...Ch. 2 - Make a rough sketch of the periodic table and mark...Ch. 2 - Prob. 8RQCh. 2 - Prob. 9RQCh. 2 - Prob. 10RQCh. 2 - Which nonmetals occur as monatomic gases (i.e.,...Ch. 2 - Prob. 12RQCh. 2 - Which physical property of metalloids...Ch. 2 - Sketch the shape of the periodic table and mark...Ch. 2 - Most periodic tables have a heavy line that looks...Ch. 2 - Prob. 16RQCh. 2 - Prob. 17RQCh. 2 - Prob. 18RQCh. 2 - 2.19 What are two ways to interpret a chemical...Ch. 2 - Prob. 20RQCh. 2 - Prob. 21RQCh. 2 - 2.22 Atoms of which elements are usually...Ch. 2 - 2.23 Atoms of which elements are usually...Ch. 2 - A DNA molecule is small in actual size but...Ch. 2 - What do we mean when we say a chemical equation is...Ch. 2 - 2.26 For a chemical reaction, what do we mean by...Ch. 2 - 2.27 The combustion of a thin wire of magnesium...Ch. 2 - Describe what kind of event must occur (involving...Ch. 2 - With what kind of elements do metals react?Ch. 2 - What is an ion? How does it differ from an atom or...Ch. 2 - 2.31 Why do we use the term formula unit for ionic...Ch. 2 - Prob. 32RQCh. 2 - Prob. 33RQCh. 2 - 2.34 How many electrons has a titanium atom lost...Ch. 2 - 2.35 If an atom gains an electron to become an...Ch. 2 - 2.36 How many electrons has a nitrogen atom gained...Ch. 2 - Prob. 37RQCh. 2 - Prob. 38RQCh. 2 - Prob. 39RQCh. 2 - Prob. 40RQCh. 2 - 2.41 What are the formulas (including charges) for...Ch. 2 - Prob. 42RQCh. 2 - Prob. 43RQCh. 2 - 2.44 Write the correct formulas for the compounds...Ch. 2 - 2.45 Write the unbalanced equations for the...Ch. 2 - 2.46 Write the unbalanced equations for the...Ch. 2 - 2.47 With what kind of elements do nonmetals...Ch. 2 - Which are the only elements that exist as free,...Ch. 2 - Prob. 49RQCh. 2 - 2.50 Which kind of elements normally combine to...Ch. 2 - Prob. 51RQCh. 2 - Prob. 52RQCh. 2 - 2.53 Without referring to Table 2.6 but using the...Ch. 2 - Prob. 54RQCh. 2 - 2.55 Astatine, a member of the halogen family,...Ch. 2 - Prob. 56RQCh. 2 - Write the chemical formulas for (a) methane, (b)...Ch. 2 - Prob. 58RQCh. 2 - Prob. 59RQCh. 2 - Prob. 60RQCh. 2 - Prob. 61RQCh. 2 - What is the difference between a binary compound...Ch. 2 - Prob. 64RQCh. 2 - Prob. 65RQCh. 2 - Prob. 66RQCh. 2 - 2.67 The compound is used in the tanning of...Ch. 2 - Asbestos, a known cancer-causing agent, has a...Ch. 2 - 2.69 Epsom salts is a hydrate of magnesium...Ch. 2 - Prob. 70RQCh. 2 - Prob. 71RQCh. 2 - Prob. 72RQCh. 2 - Write the chemical formula for the molecule...Ch. 2 - Write the chemical formula for the molecule...Ch. 2 - Prob. 75RQCh. 2 - Prob. 76RQCh. 2 - 2.77 How many atoms of each element are...Ch. 2 - 2.78 How many atoms of each kind are represented...Ch. 2 - 2.79 How many atoms of each kind are represented...Ch. 2 - 2.80 How many atoms of each kind are represented...Ch. 2 - Prob. 81RQCh. 2 - How many atoms of each element are represented in...Ch. 2 - 2.83 Consider the balanced equation
(a) How many...Ch. 2 - 2.84 Consider the balanced equation for the...Ch. 2 - Prob. 85RQCh. 2 - Prob. 86RQCh. 2 - Is the following chemical equation for the...Ch. 2 - 2.88 Is the following chemical equation balanced?...Ch. 2 - 2.89 Use the periodic table, but not Table 2.2, to...Ch. 2 - 2.90 Use the periodic table, but not Table 2.2, to...Ch. 2 - Prob. 91RQCh. 2 - Prob. 92RQCh. 2 - Prob. 93RQCh. 2 - Prob. 94RQCh. 2 - Prob. 95RQCh. 2 - Prob. 96RQCh. 2 - Prob. 97RQCh. 2 - Prob. 98RQCh. 2 - Prob. 99RQCh. 2 - Prob. 100RQCh. 2 - Prob. 101RQCh. 2 - Name the following molecular compounds:...Ch. 2 - Prob. 103RQCh. 2 - Prob. 104RQCh. 2 - Prob. 105RQCh. 2 - Prob. 106RQCh. 2 - Prob. 107RQCh. 2 - Identify each of the following as molecular or...Ch. 2 - Prob. 109RQCh. 2 - Prob. 110RQCh. 2 - Prob. 111RQCh. 2 - Prob. 112RQCh. 2 - 2.113 Which of the following formulas are...Ch. 2 - Which of the following formulas are incorrect?...Ch. 2 - Prob. 115RQCh. 2 - Prob. 116RQCh. 2 - The compounds Se2S6andSe2S4 have been shown to be...Ch. 2 - Prob. 118RQCh. 2 - The following are models of molecules of two...Ch. 2 - A student obtained a sample from an experiment...Ch. 2 - 2.121 Suppose you wanted, to separate the sample...Ch. 2 - 2.122 The elements in Group 1A and Group 7A of the...Ch. 2 - Prob. 123RQCh. 2 - Prob. 124RQCh. 2 - 2.125 Write the balanced chemical equation for the...Ch. 2 - 2.126 Write the balanced gas phase chemical...Ch. 2 - Bromine is a diatomic molecule, and it has two...Ch. 2 - Prob. 128RQCh. 2 - Prob. 129RQCh. 2 - Prob. 130RQCh. 2 - Prob. 131RQCh. 2 - Explore the internet and find a reliable source of...Ch. 2 - Spreadsheet applications such as Microsoft Excel...
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Arrange the following in the order of increasing mass. (a) a potassium ion, K+ (b) a phosphorus molecule, P4 (c) a potassium atom (d) a platinum atomarrow_forwardFrom the following written description, write the balanced chemical equation for the reaction including state symbols. A diatomic gaseous molecule that contains 17 protons per atom is reacted with a solid element that has an atomic number of 19 to yield an ionic compound.arrow_forwardThe formula of water is If-O. Which of the following is indicated by this formula? Explain your answer. a. The mass of hydrogen is twice that of oxygen in each molecule. b. There are two hydrogen atoms and one oxygen atom per water molecule. c. The mass of oxygen is twice that of hydrogen in each molecule. d. There are two oxygen atoms and one hydrogen atom per water molecule.arrow_forward
- 88 and 89 pleasearrow_forwardDetermine the numbers of protons, neutrons, and electrons in each of the following species: (a) helium-4, (b) deuterium, (c) chlorine-37, and (d) carbon-13arrow_forward(b) A certain element has two naturally occurring isotopes. The mass of one of the isotopes is 106.905 amu and its natural abundance is 51.60%. The mass of the second isotope is 108.883 amu. Calculate the average atomic mass Write the chemical symbols of the isotopesarrow_forward
- Give the chemical symbol, including superscript indicating mass number, for (a) the ion with 22 protons, 26 neutrons,and 19 electrons; and (b) the ion of sulfur that has 16 neutrons and 18 electrons.arrow_forwarda)For carbon-12 and carbon-14, how many protons and neutrons are in each nucleus? Carbon-12 has protons. Carbon-12 has neutrons. Carbon-14 has protons. Carbon-14 has neutrons. (1b )Assuming neutral atoms, how many electrons are present in an atom of carbon-12 and in an atom of carbon-14? Carbon-12 has electrons. Carbon-14 has electrons.arrow_forward7. Isotopes. (a) Argon has three naturally occurring isotopes, 36Ar, 38Ar, and 40Ar. What is the mass number of each? How many protons, neutrons, and electrons are present in each? (b) Gallium has two naturally occurring isotopes, 6°Ga (isotopic mass = 68.9256 amu, abundance 60.11%) and 71Ga (isotopic mass = 70.9247 amu, abundance = 39.89%). Calculate the atomic mas of gallium.a %3D (c) Chlorine has two naturally occurring isotopes, 35CI (isotopic mass = 34.9689 amu) and 3"Cl (isotopic mass = 36.9659 amu). If chlorine has an atomic mass of 35.4527 amu, what is the percent abundance of each isotope?arrow_forward
- Estimate the percentage of the total mass of a atom that is due to (a) electrons, (b) protons, and (c) neutrons by assuming that the mass of the atom is simply the sum of the masses of the appropriate numbers of subatomic particles. The mass of an electron is 0.00054858 amu, the mass of a proton is 1.0073 amu, and the mass of a neutron is 1.0087 amu.arrow_forwardAntimony has many uses, including infrared devices and as part of an alloy in lead storage batteries. The element has two naturally occurring isotopes, one with mass 120.904 amu, the other with mass 122.904 amu.(a) Enter the notation for each isotope. antimony−121 antimony−123 (b) The atomic mass of antimony is 121.8 amu. Use this value to calculate the percent abundance of each isotope. % antimony−121 % antimony−123arrow_forwardDetermine whether each statement is true or false. If false,correct it. (a) The Fe2+ ion contains 29 protons and 26 electrons.(b) The Cs+ ion contains 55 protons and 56 electrons.(c) The Se2- ion contains 32 protons and 34 electrons.(d) The Li+ ion contains 3 protons and 2 electrons.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and ReactionsChemistryISBN:9781305079373Author:William L. Masterton, Cecile N. HurleyPublisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Principles and Reactions
Chemistry
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:Cengage Learning
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning