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Chapter 2: Q40E (page 124)

Using the periodic table, identify the heaviest member of each of the following groups:

(a) Alkali metals

(b) Chalcogens

(c) Noble gases

(d) Alkaline earth metals

Short Answer

Expert verified

(a) The heaviest member of the alkali metal group is francium (223Fr87)

(b) The heaviest member of the chalcogens group is polonium (209Po84)

(c) The heaviest member of the Nobel gas group is radon (222Rn86)

(d) The heaviest member of the alkaline earth metal is radium (224Ra88).

Step by step solution

01

Explanation

(a) The last member of alkali group is Fr, so it has most number of protons and neutrons, and hence, it is heaviest.

(b) The last member of chalcogens is Po, so it is heaviest.

(c) The last member of noble gases is Rn, so it is heaviest.

(d) The last member of alkaline earth metal is Ra, so it is heaviest.

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Most popular questions from this chapter

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.

The following compounds are found in common household products. Write the formulas for each compound:

a. Potassium Phosphate

b. Copper (II) sulfate

c. Calcium Chloride

d. Titanium (IV) Dioxide

e. Ammonium nitrate

f. Sodium bisulfate (thecommon name for sodium hydrogen sulfate)

Average atomic masses listed by IUPAC are based on a study of experimental results. Bromine has two isotopes 79Br and 81Br, whose masses (78.9183 and 80.9163 amu) and abundance (50.69% and 49.31%) were determined in earlier experiments. Calculate the average atomic mass of bromine based on these experiments.

Give the number of protons, electrons, and neutrons in neutral atoms of each of the following isotopes:

\(\begin{aligned}{}\begin{aligned}{{}{}}{\left( a \right){\rm{ }}{}_5^{10}B}\\{\left( b \right){\rm{ }}{}_{80}^{199}Hg}\\{\left( c \right){\rm{ }}{}_{29}^{63}Cu}\\{\left( d \right){\rm{ }}{}_6^{13}C}\end{aligned}\\\left( e \right){\rm{ }}{}_{34}^{77}Se\end{aligned}\)

Question : Name the following compounds:

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