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Chapter 2: Q14E (page 118)

Open theBuild an Atom simulation (http://openstaxcollege.org/l/16PhetAtomBld)(a) Drag protons, neutrons, and electrons onto the atom template to make a neutral atom of Oxygen-16 and give theisotope symbol for this atom.(b) Now add two more electrons to make an ion and give the symbol for the ion you have created.

Short Answer

Expert verified

The structure and symbol of an oxygen atom or isotope and oxide ion is shown below.

Step by step solution

01

Structure of Oxygen - 16 atoms and symbol of the isotope of oxygen - 16

The atomic mass number of oxygen is 16 and the atomic number is 8. There are eight protons and eight neutrons in the nucleus of the O -16 isotope. This is the most abundant isotope of oxygen found in nature.

One atomic mass unit is defined as the 1/16 mass of a 16Oatom, the standard form where atomic mass and nuclide were described.

02

Drawing the structure and symbol of the oxygen ion

Two electrons are added to make an ion. The oxide ion has two negativecharges. There are 10 electrons in the atom. The structure and symbol of oxide ion are shown as follows

Number of protons = 8

Number of neutrons = 8

Number of electrons = 10

Charge = -2

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Most popular questions from this chapter

Use the periodic table to give the name and symbol for each of the following elements:

(a) The Nobel gas in the same period as Germanium.

(b) The Alkaline earth metal in the same period as selenium.

(c) The Halogen in the same period as lithium.

(d) The Chalcogen in the same period as cadmium.

Open theBuild an Atom simulation (http://openstaxcollege.org/l/16PhetAtomBld)and click on the

Atom icon.

a. Pick any one of the first 10 elements that you would like to build and state its symbol.

b. Drag protons, neutrons, and electrons onto the atom template to make an atom of your element.

State the numbers of protons, neutrons, and electrons in your atom, as well as the net charge and mass number.

c. Click on “Net Charge” and “Mass Number,” check your answers to (b), and correct, if needed.

d. Predict whether your atom will be stable or unstable. State your reasoning.

e. Check the “Stable/Unstable” box. Was your answer to (d) correct? If not, first predict what you can do to make a Stable atom of your element, and then do it and see if it works. Explain your reasoning.

Question: Write the formulas of the following compounds:

(a) rubidium bromide

(b) magnesium selenide

(c) sodium oxide

(d) calcium chloride

(e) hydrogen fluoride

(f) gallium phosphide

(g) aluminum bromide

(h) ammonium sulfate

Repeat Exercise 2.20 using an element that has three naturally occurring isotopes.

Each of the following compounds contains a metal that can exhibit more than one ionic charge. Name these compounds:

a. NiCO3

b. MoO3

c.Co(NO3)2

d. V2O5

e. MnO2

f. Fe2O3
See all solutions

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