QQuestionChemistry
QuestionChemistry
# The atomic number of fluorine is 9. How many electrons does an ion of fluorine have if it is represented by the symbol shown below?
19 \mathrm{~F}^{1 -}
A. 8 electrons
B. 9 electrons
C. 10 electrons
D. 20 electrons
12 months agoReport content
Answer
Full Solution Locked
Sign in to view the complete step-by-step solution and unlock all study resources.
Step 1:Let's solve this step by step:
Step 2:: Understand the atomic number
- The atomic number represents the number of protons in an atom's nucleus - For fluorine, the atomic number is 9, which means a neutral fluorine atom has 9 protons and 9 electrons
Step 3:: Analyze the ion symbol ^{1 -}
- The superscript $$^{1-}$$ indicates a charge of -1
- A negative charge means the atom has gained electrons
Step 4:: Calculate the number of electrons
- With a $$^{1-}$$ charge, the atom gains 1 additional electron
- Neutral fluorine has 9 electrons - Total electrons = 9 + 1 = 10 electrons
Step 5:: Verify the calculation
- Protons remain 9 - Electrons are now 10 - Charge is - 1
Final Answer
Explanation: When fluorine forms a ^{1 -} ion, it gains one electron, bringing its total electron count to 10 while maintaining 9 protons in its nucleus.
Need Help with Homework?
Stuck on a difficult problem? We've got you covered:
- Post your question or upload an image
- Get instant step-by-step solutions
- Learn from our AI and community of students