Question

Answer the questions below based on your observations. DATA Symbol Name Atomic Number Mass Number Number of Protons Number of Neutrons Number of Electrons H He Li Be B C N O F Ne Questions: Which particles contribute to the mass number and which do not? Why? Which particle(s) contributed to the atomic number and why? Which particles contribute to the net charge and how does each change the net charge? How are the number of protons and electrons in an atom important to determining the unique nature of each element? Use 3 elements from the table above and describe the unique properties of each. Be sure to discuss the importance of proton numbers, electron numbers, and mass numbers in your explanation. Isotopes Background: For all elements, the number of neutrons can make the nucleus stable or unstable. The Nuclear Strong Interaction (also called the nuclear strong force or nuclear force) is what holds the nucleus together. Neutrons help hold the protons the right distance apart from each other to maintain nuclear stability. Different isotopes of the same element are written in words and symbols to show the mass number. (Recall that the mass number is the number of protons and neutrons). For example, two isotopes of Carbon are carbon-12 and carbon-14. The symbolic notation for these two isotopes would be: for carbon 12 with an atomic number of 6 and a mass number of 12. for carbon 14 with an atomic number of 6 and a mass number of 14 Activity: Start by creating the isotope oxygen-16. This will have 8 protons, 8 neutrons, and 8 electrons. What is the symbolic notation for this isotope? . Is this isotope stable or unstable? . Add a neutron to the atom. What element is this now? . What is the name of this isotope? . What is the symbolic notation for this isotope? _. Add another neutron to the atom. You should have 8 protons, 10 neutrons, and 8 electrons. What element is this now? ______. What is the name of this isotope? . What is the symbolic notation for this isotope? _. Is this isotope stable or unstable? __________________. If the three isotopes of oxygen have a percent abundance and masses shown below, compute the atomic mass of this element. Multiply the Mass of each isotope times the Percent Abundance to get the Mass Contribution. Add the Mass Contributions of each isotope to get the atomic mass of oxygen. Mass X Percent Abundance = Mass Contribution Oxygen-16 16 95% Oxygen-17 17 2.5% Oxygen-18 18 2.5% Oxygen Research two examples of isotopes from the elements listed in the table. Discuss how these isotopes are used in medicine, ecology, or environmental research. Be sure to explain whether it is a stable or unstable isotope. How do you know if an element is stable or unstable?

Answer the questions below based on your observations.

DATA
Symbol
Name
Atomic Number
Mass Number
Number of Protons
Number of Neutrons
Number of Electrons
H
He
Li
Be
B
C
N
O
F
Ne

Questions:
Which particles contribute to the mass number and which do not? Why?
Which particle(s) contributed to the atomic number and why?
Which particles contribute to the net charge and how does each change the net charge?
How are the number of protons and electrons in an atom important to determining the unique nature of each element? Use 3 elements from the table above and describe the unique properties of each. Be sure to discuss the importance of proton numbers, electron numbers, and mass numbers in your explanation.

Isotopes
Background:
For all elements, the number of neutrons can make the nucleus stable or unstable. The Nuclear Strong Interaction (also called the nuclear strong force or nuclear force) is what holds the nucleus together. Neutrons help hold the protons the right distance apart from each other to maintain nuclear stability.

Different isotopes of the same element are written in words and symbols to show the mass number. (Recall that the mass number is the number of protons and neutrons). For example, two isotopes of Carbon are carbon-12 and carbon-14. The symbolic notation for these two isotopes would be:
for carbon 12 with an atomic number of 6 and a mass number of 12.
for carbon 14 with an atomic number of 6 and a mass number of 14

Activity:
Start by creating the isotope oxygen-16. This will have 8 protons, 8 neutrons, and 8 electrons.
What is the symbolic notation for this isotope? ____________.
Is this isotope stable or unstable? ________________________.
Add a neutron to the atom.
What element is this now? ______________________________.
What is the name of this isotope? ________________________.
What is the symbolic notation for this isotope? _____________.
Add another neutron to the atom. You should have 8 protons, 10 neutrons, and 8 electrons.
What element is this now? ______________________________.
What is the name of this isotope? ________________________.
What is the symbolic notation for this isotope? _____________.
Is this isotope stable or unstable? ________________________.

If the three isotopes of oxygen have a percent abundance and masses shown below, compute the atomic mass of this element. Multiply the Mass of each isotope times the Percent Abundance to get the Mass Contribution. Add the Mass Contributions of each isotope to get the atomic mass of oxygen.

Mass X Percent Abundance = Mass Contribution
Oxygen-16 16 95%
Oxygen-17 17 2.5%
Oxygen-18 18 2.5%

Oxygen

Research two examples of isotopes from the elements listed in the table. Discuss how these isotopes are used in medicine, ecology, or environmental research. Be sure to explain whether it is a stable or unstable isotope. How do you know if an element is stable or unstable?

Added by Mary T.

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