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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...
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# 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
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