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Chapter 2: Problem 73

Would you expect each of the following atoms to gain or lose electrons when forming ions? What ion is the most likely in each case? a. Ra b. In c. P d. Te e. Br f. Rb

Short Answer

Expert verified
Ra will likely form a Ra^(2+) ion, In will form an In^(3+) ion, P will form a P^(3-) ion, Te will form a Te^(2-) ion, Br will form a Br^(-) ion, and Rb will form an Rb^(1+) ion.

Step by step solution

01

a. Ra (Radium)

Radium is in group 2 of the periodic table, belonging to the alkaline earth metals. Elements in group 2 have a general electron configuration of [noble gas] ns^2. They tend to lose two electrons to achieve a stable electron configuration, forming ions with a 2+ charge. So, Ra will most likely form a Ra^(2+) ion.
02

b. In (Indium)

Indium is in group 13 of the periodic table. Elements in group 13 have a general electron configuration of [noble gas] ns^2 np^1. These elements tend to lose three electrons to achieve a stable electron configuration, forming ions with a 3+ charge. So, In will most likely form an In^(3+) ion.
03

c. P (Phosphorus)

Phosphorus is in group 15 of the periodic table. Elements in this group have a general electron configuration of [noble gas] ns^2 np^3. They tend to gain three electrons to achieve a stable electron configuration, forming ions with a 3- charge. So, P will most likely form a P^(3-) ion.
04

d. Te (Tellurium)

Tellurium is in group 16 of the periodic table, which includes the chalcogens. Elements in this group have a general electron configuration of [noble gas] ns^2 np^4. They tend to gain two electrons to achieve a stable electron configuration, forming ions with a 2- charge. So, Te will most likely form a Te^(2-) ion.
05

e. Br (Bromine)

Bromine is in group 17 of the periodic table, which includes the halogens. Elements in this group have a general electron configuration of [noble gas] ns^2 np^5. They tend to gain one electron to achieve a stable electron configuration, forming ions with a 1- charge. So, Br will most likely form a Br^(-) ion.
06

f. Rb (Rubidium)

Rubidium is in group 1 of the periodic table, belonging to the alkali metals. Elements in group 1 have a general electron configuration of [noble gas] ns^1. They tend to lose one electron to achieve a stable electron configuration, forming ions with a 1+ charge. So, Rb will most likely form an Rb^(1+) ion.

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Most popular questions from this chapter

Dalton assumed that all atoms of the same element were identical in all their properties. Explain why this assumption is not valid.

For each of the following sets of elements, label each as either noble gases, halogens, alkali metals, alkaline earth metals, or transition metals. a. Ti, Fe, Ag b. Mg, Sr, Ba c. Li, K, Rb d. Ne, Kr, Xe e. F, Br, I

You have gone back in time and are working with Dalton on a table of relative masses. Following are his data. 0.602 g gas A reacts with 0.295 g gas \(\mathrm{B}\) 0.172 \(\mathrm{g}\) gas \(\mathrm{B}\) reacts with 0.401 \(\mathrm{g}\) gas \(\mathrm{C}\) 0.320 \(\mathrm{g}\) gas A reacts with 0.374 \(\mathrm{g}\) gas \(\mathrm{C}\) a. Assuming simplest formulas (AB, BC, and AC), construct a table of relative masses for Dalton. b. Knowing some history of chemistry, you tell Dalton that if he determines the volumes of the gases reacted at constant temperature and pressure, he need not assume simplest formulas. You collect the following data: 6 volumes gas \(\mathrm{A}+1\) volume gas \(\mathrm{B} \rightarrow\) 4 volumes product 1 volume gas \(\mathrm{B}+4\) volumes gas \(\mathrm{C} \rightarrow\) 4 volumes product 3 volumes gas \(\mathrm{A}+2\) volumes gas \(\mathrm{C} \rightarrow\) 6 volumes product Write the simplest balanced equations, and find the actual relative masses of the elements. Explain your reasoning.

What are the symbols of the following nonmetals: fluorine, chlorine, bromine, sulfur, oxygen,phosphorus?

Write the formula for each of the following compounds: a. ammonium hydrogen phosphate b. mercury(I) sulfide c. silicon dioxide d. sodium sulfite e. aluminum hydrogen sulfate f. nitrogen trichloride g. hydrobromic acid h. bromous acid i. perbromic acid j. potassium hydrogen sulfide k. calcium iodide l. cesium perchlorate
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