Study Guide with Student Solutions Manual for Seager/Slabaugh/Hansen's Chemistry for Today: General, Organic, and Biochemistry, 9th Edition
Study Guide with Student Solutions Manual for Seager/Slabaugh/Hansen's Chemistry for Today: General, Organic, and Biochemistry, 9th Edition
9th Edition
ISBN: 9781305968608
Author: Spencer L. Seager, Michael R. Slabaugh, Maren S. Hansen
Publisher: Cengage Learning
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Chapter 2, Problem 2.10E
Interpretation Introduction

(a)

Interpretation:

The charge and mass (in u) of nucleus made up of 4 protons and 5 neutrons are to be calculated

Concept introduction:

The three subatomic particles are electrons, neutrons and protons. Out of these three, neutrons and protons are located inside the nucleus of an atom. The electron carries a charge of 1, proton carries a charge of +1 and neutron does not carry any charge.

Expert Solution
Check Mark

Answer to Problem 2.10E

The charge and mass (in u) of nucleus made up of 4 protons and 5 neutrons are +4 and 9u respectively.

Explanation of Solution

In a nucleus having 4 protons and 5 neutrons, the charge is only due to the protons as the neutron does not carry any charge. Thus, the charge for such a nucleus is equal to charge of protons which is equal to +4. The mass of nucleus is calculated by the formula given below.

Mnucleus=Mproton+Mneutron

Where,

Mnucleus is the mass of nucleus

Mproton is the mass of protons

Mneutron is the mass of neutrons

Mass of neutron and mass of proton in terms of atomic unit is 1u each.

Substitute the values in the above equation as follows.

Mnucleus=Mproton+Mneutron=(4×1u)+(5×1u)=9u

Thus, the mass of nucleus having 4 protons and 5 neutrons is 9u.

Conclusion

The charge and mass (in u) of nucleus made up of 4 protons and 5 neutrons are calculated +4 and 9u respectively.

Interpretation Introduction

(b)

Interpretation:

The charge and mass (in u) of nucleus made up of 9 protons and 10 neutrons are to becalculated

Concept introduction:

The three subatomic particles are electrons, neutrons and protons. Out of these three, neutrons and protons are located inside the nucleus of an atom. The electron carries a charge of 1, proton carries a charge of +1 and neutron does not carry any charge.

Expert Solution
Check Mark

Answer to Problem 2.10E

The charge and mass (in u) of nucleus made up of 9 protons and 10 neutrons are +9 and 19u respectively.

Explanation of Solution

In a nucleus having 9 protons and 10 neutrons, the charge is only due to the protons as the neutron does not carry any charge. Thus, the charge for such a nucleus is equal to charge of protons which is equal to +9. The mass of nucleus is calculated by the formula given below.

Mnucleus=Mproton+Mneutron

Where,

Mnucleus is the mass of nucleus

Mproton is the mass of protons

Mneutron is the mass of neutrons

Mass of neutron and mass of proton in terms of atomic unit is 1u each.

Substitute the values in the above equation as follows.

Mnucleus=Mproton+Mneutron=(9×1u)+(10×1u)=19u

Thus, the mass of nucleus having 9 protons and 10 neutrons is 19u.

Conclusion

The charge and mass (in u) of nucleus made up of 9 protons and 10 neutrons are calculated as +9 and 19u respectively.

Interpretation Introduction

(c)

Interpretation:

The charge and mass (in u) of nucleus made up of 20 protons and 23 neutrons are to be calculated

Concept introduction:

The three subatomic particles are electrons, neutrons and protons. Out of these three, neutrons and protons are located inside the nucleus of an atom. The electron carries a charge of 1, proton carries a charge of +1 and neutron does not carry any charge.

Expert Solution
Check Mark

Answer to Problem 2.10E

The charge and mass (in u) of nucleus made up of 20 protons and 23 neutrons are +20 and 43u respectively.

Explanation of Solution

In a nucleus having 20 protons and 23 neutrons, the charge is only due to the protons as the neutron does not carry any charge. Thus, the charge for such a nucleus is equal to charge of protons which is equal to +20. The mass of nucleus is calculated by the formula given below.

Mnucleus=Mproton+Mneutron

Where,

Mnucleus is the mass of nucleus

Mproton is the mass of protons

Mneutron is the mass of neutrons

Mass of neutron and mass of proton in terms of atomic unit is 1u each.

Substitute the values in the above equation as follows.

Mnucleus=Mproton+Mneutron=(20×1u)+(23×1u)=43u

Thus, the mass of nucleus having 20 protons and 23 neutrons is 43u.

Conclusion

The charge and mass (in u) of nucleus made up of 20 protons and 23 neutrons are calculated as +20 and 43u respectively.

Interpretation Introduction

(d)

Interpretation:

The charge and mass (in u) of nucleus made up of 47 protons and 60 neutrons are to be calculated

Concept introduction:

The three subatomic particles are electrons, neutrons and protons. Out of these three, neutrons and protons are located inside the nucleus of an atom. The electron carries a charge of 1, proton carries a charge of +1 and neutron does not carry any charge.

Expert Solution
Check Mark

Answer to Problem 2.10E

The charge and mass (in u) of nucleus made up of 47 protons and 60 neutrons are +47 and 107u respectively.

Explanation of Solution

In a nucleus having 47 protons and 60 neutrons, the charge is only due to the protons as the neutron does not carry any charge. Thus, the charge for such a nucleus is equal to charge of protons which is equal to +47. The mass of nucleus is calculated by the formula given below.

Mnucleus=Mproton+Mneutron

Where,

Mnucleus is the mass of nucleus

Mproton is the mass of protons

Mneutron is the mass of neutrons

Mass of neutron and mass of proton in terms of atomic unit is 1u each.

Substitute the values in the above equation as follows.

Mnucleus=Mproton+Mneutron=(47×1u)+(60×1u)=107u

Thus, the mass of nucleus having 47 protons and 60 neutrons is 107u.

Conclusion

The charge and mass (in u) of nucleus made up of 47 protons and 60 neutrons are calculated as +47 and 107u respectively.

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Chapter 2 Solutions

Study Guide with Student Solutions Manual for Seager/Slabaugh/Hansen's Chemistry for Today: General, Organic, and Biochemistry, 9th Edition

Ch. 2 - Determine the number of electrons that would have...Ch. 2 - Determine the number of electrons that would have...Ch. 2 - Determine the number of electrons and protons...Ch. 2 - Determine the number of electrons and protons...Ch. 2 - Prob. 2.15ECh. 2 - Prob. 2.16ECh. 2 - Write symbols like those given in Exercises 2.15...Ch. 2 - Write symbols like those given in Exercises 2.15...Ch. 2 - Prob. 2.19ECh. 2 - Prob. 2.20ECh. 2 - Write isotope symbols for neutral atoms with the...Ch. 2 - Write isotope symbols for neutral atoms with the...Ch. 2 - Write the symbols and names for two elements whose...Ch. 2 - Round atomic weights to the nearest whole number,...Ch. 2 - Round atomic weights to the nearest whole number,...Ch. 2 - What are the symbol and name for an element whose...Ch. 2 - In the first 36 elements, 6 elements have atoms...Ch. 2 - What are the symbol and name of the element whose...Ch. 2 - Prob. 2.29ECh. 2 - Prob. 2.30ECh. 2 - The molecular weight was determined for a gas that...Ch. 2 - A flammable gas is known to contain only carbon...Ch. 2 - Glycine, an amino acid found in proteins, has a...Ch. 2 - Serine, an amino acid found in proteins, has a...Ch. 2 - Naturally occurring sodium has a single isotope....Ch. 2 - Naturally occurring aluminum has a single isotope....Ch. 2 - Calculate the atomic weight of lithium on the...Ch. 2 - Calculate the atomic weight of boron on the basis...Ch. 2 - Calculate the atomic weight of silicon on the...Ch. 2 - Calculate the atomic weight of copper on the basis...Ch. 2 - Refer to the periodic table and determine how many...Ch. 2 - Refer to the periodic table and determine how many...Ch. 2 - Write three relationships equalities based on the...Ch. 2 - Write three relationships equalities based on the...Ch. 2 - Use a factor derived from the relationships...Ch. 2 - Use a factor derived from the relationships...Ch. 2 - Prob. 2.47ECh. 2 - Refer to the periodic table and calculate the...Ch. 2 - Prob. 2.49ECh. 2 - Prob. 2.50ECh. 2 - Answer the following questions based on the...Ch. 2 - Answer the following questions based on...Ch. 2 - How many moles of N2O5 contain the same number of...Ch. 2 - How many grams of C2H6O contain the same number of...Ch. 2 - Prob. 2.55ECh. 2 - Determine the mass percentage of hydrogen in CH4...Ch. 2 - Prob. 2.57ECh. 2 - Prob. 2.58ECh. 2 - Urea (CH4N2O) and ammonium sulfate (N2H8SO4) are...Ch. 2 - Prob. 2.60ECh. 2 - Prob. 2.61ECh. 2 - Prob. 2.62ECh. 2 - Prob. 2.63ECh. 2 - The mass of a single carbon 12 atom is 1.991023g....Ch. 2 - Prob. 2.65ECh. 2 - Prob. 2.66ECh. 2 - a. Explain how atoms of different elements differ...Ch. 2 - The atomic weight of aluminum is 26.98u and the...Ch. 2 - Answer the question in the caption of Figure 2.3...Ch. 2 - Answer the question in the caption of Figure 2.5...Ch. 2 - Prob. 2.71ECh. 2 - Prob. 2.72ECh. 2 - Prob. 2.73ECh. 2 - Prob. 2.74ECh. 2 - Prob. 2.75ECh. 2 - Which one of the following substances is a...Ch. 2 - Which of the following is true about compounds?...Ch. 2 - C1734l has a.17 protons, 17 electrons, and 17...Ch. 2 - If two atoms are isotopes, they will a.have same...Ch. 2 - Copper (Cu) has an atomic number of 29 and a mass...Ch. 2 - Atoms are electrically neutral. This means that an...Ch. 2 - The negative charged particle found within the...Ch. 2 - Prob. 2.83ECh. 2 - Prob. 2.84ECh. 2 - The mass of an atom is almost entirely contributed...Ch. 2 - Which of the following is the chemical symbol for...Ch. 2 - Prob. 2.87ECh. 2 - What is the mass number of an atom with 60...Ch. 2 - Which of the following represents Avogadros...Ch. 2 - Which of the following has the greatest number of...Ch. 2 - The formula of carbon dioxide is CO2. Its...Ch. 2 - What is the molar mass of calcium oxide, CaO? a....Ch. 2 - How many grams are contained in 0.200mol of...Ch. 2 - How many moles are contained in a 54.0g sample of...
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