Homework Help is Here – Start Your Trial Now!
Science
Chemistry
Determine the isotope symbol that fits each description. Ag 76 a. 68 neutrons, 47 electrons b. mass number = 197, 79 electrons Au 78 Er 79 Os 86 d. atomic number = 76, mass number = 192 C. atomic number = 86, 136 neutrons Pt 115 Rn 192 47 197 68 222 < Prev 19 of 20 Next > T... search (26 hp

Determine the isotope symbol that fits each description. Ag 76 a. 68 neutrons, 47 electrons b. mass number = 197, 79 electrons Au 78 Er 79 Os 86 d. atomic number = 76, mass number = 192 C. atomic number = 86, 136 neutrons Pt 115 Rn 192 47 197 68 222 < Prev 19 of 20 Next > T... search (26 hp

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
See similar textbooks
icon
Related questions
Question
18)
# Isotope Symbols and Their Determination ### Instructions: Determine the isotope symbol that fits each description. --- ### a. 68 neutrons, 47 electrons ``` ❑ ❑ ❑ ``` ### b. Mass number = 197, 79 electrons ``` ❑ ❑ ❑ ``` Options: - Ag, 76 - Au, 78 - Er, 79 - Os, 86 --- ### c. Atomic number = 86, 136 neutrons ``` ❑ ❑ ❑ ``` ### d. Atomic number = 76, mass number = 192 ``` ❑ ❑ ❑ ``` Options: - Pt, 115 - Rn, 192 - 47, 197 - 68, 222 --- ## Explanation: In each blank box, place the appropriate subscript and superscript values that indicate the isotope symbol. For example: - The first (vertical) box indicates the __mass number__ (total number of protons and neutrons). - The second (horizontal) box indicates the __atomic number__ (number of protons). - The third (box on the right) denotes the __element symbol__. These values can be determined based on the descriptions provided and matched against the options given in the problem. For educational purposes, it is essential to understand: - The **atomic number** is equal to the number of protons in an element and can also be derived from the number of electrons for neutral atoms. - The **mass number** is the sum of protons and neutrons in the nucleus. - The number of **neutrons** can be derived from the difference between the mass number and the atomic number. The isotope symbol is commonly written in the form: $$ \frac{Mass \: Number}{Atomic \: Number} \: Element \: Symbol $$
Transcribed Image Text:# Isotope Symbols and Their Determination ### Instructions: Determine the isotope symbol that fits each description. --- ### a. 68 neutrons, 47 electrons ``` ❑ ❑ ❑ ``` ### b. Mass number = 197, 79 electrons ``` ❑ ❑ ❑ ``` Options: - Ag, 76 - Au, 78 - Er, 79 - Os, 86 --- ### c. Atomic number = 86, 136 neutrons ``` ❑ ❑ ❑ ``` ### d. Atomic number = 76, mass number = 192 ``` ❑ ❑ ❑ ``` Options: - Pt, 115 - Rn, 192 - 47, 197 - 68, 222 --- ## Explanation: In each blank box, place the appropriate subscript and superscript values that indicate the isotope symbol. For example: - The first (vertical) box indicates the __mass number__ (total number of protons and neutrons). - The second (horizontal) box indicates the __atomic number__ (number of protons). - The third (box on the right) denotes the __element symbol__. These values can be determined based on the descriptions provided and matched against the options given in the problem. For educational purposes, it is essential to understand: - The **atomic number** is equal to the number of protons in an element and can also be derived from the number of electrons for neutral atoms. - The **mass number** is the sum of protons and neutrons in the nucleus. - The number of **neutrons** can be derived from the difference between the mass number and the atomic number. The isotope symbol is commonly written in the form: $$ \frac{Mass \: Number}{Atomic \: Number} \: Element \: Symbol $$
### Subatomic Particles: Key Characteristics #### Complete the following table for the three key subatomic particles: | Name | Symbol | Charge | Mass | Location in the Atom | |---------|--------|-------------------|---------------------|--------------------------| | | | Relative | Absolute (C) | Relative (amu) | Absolute (g) | | | Proton | \( p^+ \) | +1 | \( +1.6 \times 10^{-19} \) | 1.00727 | \( 1.67 \times 10^{-24} \) | Inside the nucleus | | Neutron | \( n^0 \) | 0 | 0 | 1.00866 | \( 1.67 \times 10^{-24} \) | Inside the nucleus | | Electron| \( e^- \) | -1 | \( -1.6 \times 10^{-19} \) | 0.00054858 | \( 9.1 \times 10^{-28} \) | Outside the nucleus | #### Details: 1. **Proton (\( p^+ \))**: - **Charge**: - Relative: +1 - Absolute: \( +1.6 \times 10^{-19} \) Coulombs - **Mass**: - Relative: 1.00727 atomic mass units (amu) - Absolute: \( 1.67 \times 10^{-24} \) grams - **Location in the Atom**: Inside the nucleus 2. **Neutron (\( n^0 \))**: - **Charge**: - Relative: 0 - Absolute: 0 Coulombs - **Mass**: - Relative: 1.00866 atomic mass units (amu) - Absolute: \( 1.67 \times 10^{-24} \) grams - **Location in the Atom**: Inside the nucleus 3. **Electron (\( e^- \))**: - **Charge**: - Relative: -1 - Absolute: \( -1.6 \times 10^{-19} \) Coulombs - **Mass**: - Relative: 0.00054858 atomic
Transcribed Image Text:### Subatomic Particles: Key Characteristics #### Complete the following table for the three key subatomic particles: | Name | Symbol | Charge | Mass | Location in the Atom | |---------|--------|-------------------|---------------------|--------------------------| | | | Relative | Absolute (C) | Relative (amu) | Absolute (g) | | | Proton | \( p^+ \) | +1 | \( +1.6 \times 10^{-19} \) | 1.00727 | \( 1.67 \times 10^{-24} \) | Inside the nucleus | | Neutron | \( n^0 \) | 0 | 0 | 1.00866 | \( 1.67 \times 10^{-24} \) | Inside the nucleus | | Electron| \( e^- \) | -1 | \( -1.6 \times 10^{-19} \) | 0.00054858 | \( 9.1 \times 10^{-28} \) | Outside the nucleus | #### Details: 1. **Proton (\( p^+ \))**: - **Charge**: - Relative: +1 - Absolute: \( +1.6 \times 10^{-19} \) Coulombs - **Mass**: - Relative: 1.00727 atomic mass units (amu) - Absolute: \( 1.67 \times 10^{-24} \) grams - **Location in the Atom**: Inside the nucleus 2. **Neutron (\( n^0 \))**: - **Charge**: - Relative: 0 - Absolute: 0 Coulombs - **Mass**: - Relative: 1.00866 atomic mass units (amu) - Absolute: \( 1.67 \times 10^{-24} \) grams - **Location in the Atom**: Inside the nucleus 3. **Electron (\( e^- \))**: - **Charge**: - Relative: -1 - Absolute: \( -1.6 \times 10^{-19} \) Coulombs - **Mass**: - Relative: 0.00054858 atomic
Expert Solution
trending now

Trending now

This is a popular solution!

steps

Step by step

Solved in 6 steps

SEE SOLUTIONCheck out a sample Q&A here
Blurred answer
Knowledge Booster
Matter
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
Recommended textbooks for you
Chemistry
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning
Chemistry
Chemistry
Chemistry
ISBN:
9781259911156
Author:
Raymond Chang Dr., Jason Overby Professor
Publisher:
McGraw-Hill Education
Principles of Instrumental Analysis
Principles of Instrumental Analysis
Chemistry
ISBN:
9781305577213
Author:
Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher:
Cengage Learning
Organic Chemistry
Organic Chemistry
Chemistry
ISBN:
9780078021558
Author:
Janice Gorzynski Smith Dr.
Publisher:
McGraw-Hill Education
Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Elementary Principles of Chemical Processes, Bind…
Elementary Principles of Chemical Processes, Bind…
Chemistry
ISBN:
9781118431221
Author:
Richard M. Felder, Ronald W. Rousseau, Lisa G. Bullard
Publisher:
WILEY
SEE MORE TEXTBOOKS