**Atomic Structure Assignment**---**Be sure to answer all parts.****Give the following information for the atom: [1] the atomic number; [2] the mass number; [3] the number of protons; [4] the number of neutrons; [5] the number of electrons.****\( ^{55}_{26}\text{Fe} \)**1. **Atomic Number: \_\_\_\_**2. **Mass Number: \_\_\_\_**3. **Number of Protons: \_\_\_\_**4. **Number of Neutrons: \_\_\_\_**5. **Number of Electrons: \_\_\_\_**---**Instructions:**- To determine the atomic number, look at the subscript (lower number) next to the element symbol. This represents the number of protons in the nucleus.- The mass number is the superscript (upper number) next to the element symbol. It represents the total number of protons and neutrons in the atom's nucleus.- Number of protons is given directly by the atomic number.- Number of neutrons can be found by subtracting the atomic number from the mass number.- In a neutral atom, the number of electrons is equal to the number of protons.**Hint:**For the given atom \( ^{55}_{26}\text{Fe} \):- The atomic number is \(26\).- The mass number is \(55\).- The number of protons = atomic number (\(26\)).- The number of neutrons = mass number (\(55\)) - atomic number (\(26\)) = \(29\).- The number of electrons in a neutral atom = number of protons (\(26\)).Please fill in the blanks accordingly.

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3 attempts left Check my work Be sure to answer all parts. Give the following information for the atom: [1] the atomic number; [2] the mass number; [3] the number of protons; [4] the number of neutrons; [5] the number of electrons. 55Fe Atomic Number: Mass Number: Number of Protons: Number of Neutrons: Number of Electrons:

3 attempts left Check my work Be sure to answer all parts. Give the following information for the atom: [1] the atomic number; [2] the mass number; [3] the number of protons; [4] the number of neutrons; [5] the number of electrons. 55Fe Atomic Number: Mass Number: Number of Protons: Number of Neutrons: Number of Electrons:

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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1. Describe briefly, indicating the scientist responsible, experiments that gave the following evida,riee7RT¬the model of an atom:a) The atom consists of a very tiny, thickly dense positively charged nucleus, surrounded by a negatively charged electron cloud.b) The nucleus contains a specific number of protons, positively charged particles that gives the atomic number.c) Neutrons together with the protons in the nucleus account for the atomic weight.
11) To calculate the number of neutrons in an atom, you would subtract A) mass number from atomic number B) atomic number from electron number C) atomic number from mass number 12) What is the correct notation for a particle which has 17 protons, 18 neturals and 18 electrons? A) ECi- B) Ci- 1
Please don't provide handwritten solution ...
1- For each of the following atoms, calculate the number of protons and neutrons in the nucleus and the number of electrons outside the nucleus (assume neutral atoms). element number of number of number of electrons mass number (A) symbol 126C protons (Z) neutrons 12 10 12 10 14 27 10 23,1Na 11 17 18 2- Calculate the atomic mass to four significant figures for carbon, given the following data: Isotope Exact Atomic Mass (amu) 12.00000 13.00335 Abundance in Nature (%) 98.89 1.110 12C 13C
True or False...and why? a.) If you change number of protons, you have isotopes of an element b.) If you change number of neutrons, ions are created c.) If you change number of electrons, you have a different element
I'm sturggling on the last question part c. I submitted what I though was correct (36 on top and 78 on bottom with the symbol Kr) if that makes sense. I was wondering if you could help me. Thank you. I have 10 attemps and already used 3 because I miss read the question at first and only submitted symbols instead of the atomic number and mass number as well like you see on a periodic table.
8) Complete the table Isotope Neon-20 Mass (amu) 19.992 Relative Abundance (%) 90.51 Neon-21 20.994 Neon-22 Avg. Atomic Mass= 9.23 Total %:
Naturally occurring neon (Ne) has three isotopes with the following data neon-20, 90.92% (19.99 amu) neon-21, 0.257% (20.99 amu) neon-22, 8.82% (? amu) The atomic mass for Ne is 20.183 amu. What is the mass in amu for neon-22? Report 2 decimal places in your final answer. No need to include unit.