Order the following five elements by size where 1 is the smallest sizeand 5 is the largest size. You may find a periodic table helpful.Ga, Si, Rb, Ar, Cs1ArSiRb5GaWhich of the following statements are not true about nonmetals? Selectall that apply. Incorrect selections will deduct credit.Nonmetals never react with metalsNonmetal oxides are basicNonmetals generally have large negative electron affinity valuesNonmetals do not conduct electricityNonmetals as a class have a wide variety of properties234

When we go from left to right throughout a period, electrons are added to the existing…

Answered: Order the following five elements by…

Order the following five elements by size where 1 is the smallest size and 5 is the largest size. You may find a periodic table helpful. Ga, Si, Rb, Ar, Cs

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter2: Atomic Structure And Periodicity

Section: Chapter Questions

Problem 158CWP

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Similar questions

Arrange the following in order of increasing ionic radius: I, Cs+, and Te2+. Explain this order. (You may use a periodic table.)
Account for the fact that the line that separates the metals from the nonmetals on the periodic table is diagonal downward to the right instead of horizontal or vertical.
Cerium, as noted in Applying Chemical Principles: 22.3 The Rare Earths, is a relatively abundant lanthanide element that has some important uses. Cerium(IV) oxide. CeO2, is widely used as a polishing agent for glass. Cerium(III) sulfide, Ce2S3, is becoming more widely used as a red pigment to replace cadmium pigments, which are environmentally less desirable. (a) Give the electron configurations (using the noble gas notation) for Ce, Ce3+, and Ce4+. (b) Is either Ce3+ or Ce4+ paramagnetic? If so, how many unpaired electrons does each have? (c) The solid state structure for CeO2 is shown below. Describe the unit cell of the compound. How is this structure related to the formula?
Periodic Properties I A hypothetical element, X, has the following ionization energy values: First ionization energy: 900 kJ/mol Second ionization energy: 1750 kJ/mol Third ionization energy: 14,900 kJ/mol Fourth ionization energy: 21,000 kJ/mol Another element, Y, has the following ionization energy values: First ionization energy: 1200 kJ/mol Second ionization energy: 2500 kJ/mol Third ionization energy : 19,900 kJ/mol Fourth ionization energy: 26,000 kJ/mol a To what family of the periodic table would element X be most likely to belong? Explain? b What charge would you expect dement X to have when it forms an ion? c If you were to place elements X and Y into the periodic table, would element Y be in the same period as element X? If not in the same period, where might they be relative to each other in the periodic table? d Would an atom of Y be smaller or larger than an atom of X? Explain your reasoning.
It is possible to define metallic character as we do in this bookand base it on the reactivity of the element and the ease withwhich it loses electrons. Alternatively, one could measure how well electricity is conducted by each of the elements todetermine how “metallic” the elements are. On the basis ofconductivity, there is not much of a trend in the periodic table:Silver is the most conductive metal, and manganese theleast. Look up the first ionization energies of silver and manganese;which of these two elements would you call moremetallic based on the way we define it in this book?
Sulfur, B, element 16, tends to form a 2- ion. Write the electron configuration of neutral S and ofthis ion.S: S^2- Explain why the 2- ion is the one that tends typically to form? In what group of the periodie table is S located? What ions would the other elements in thisgroup tend to form? Why?
Yttrium (Y), niobium (Nb), and antimony (Sb) are elements in the fifth period of the Periodic Table. All three elements form 3+ cations. Y3+ has a radius of 104 pm, Nb3+ has a radius of 86 pm, and Sb3+ has a radius of 90 pm. a) Write the electron configuration for Nb3+ and for Sb3+ using the condensed noble gas notation. Identify which orbitals lose electrons to yield the 3+ cation. b) Explain the radius size trend for these three ions.
The electron affinities, in kJ>mol, for the group 1B and group2B metals are as follows: (a) Why are the electron affinities of the group 2B elementsgreater than zero? (b) Why do the electron affinities of thegroup 1B elements become more negative as we move downthe group? [Hint: Examine the trends in the electron affinitiesof other groups as we proceed down the periodic table.]
A) Which of the halogen elements has the highest density in its standard state? B) Which of the elements of the third period should have the highest 2nd ionization energy? C) For which of Al, Si or P is the absolute value of the Electron Affinity greatest? D) Which of the ions Mg2+, Sr2+, Ca2+, Be2+, Ba2+, or Ra2+ is the smallest? E) For the elements: X = Br, I, Cl, or H, which has the the smallest average X-C bond energy?
Arrange the following in order of increasing radius: Cl^-, P^3-, Ar, Ca^2+, Mg^2+, K^+, As^5+, Ga^3+, Ge^4-
You read the following statement about two elements X andY: One of the elements is a good conductor of electricity, andthe other is a semiconductor. Experiments show that the firstionization energy of X is twice as great as that of Y. Whichelement has the greater metallic character?
Consider the following ionization energies for aluminum : Al (g) → Al+ (g) + e- I1 = 580 kJ/mol Al+(g) → Al2+ (g) + e- I2 = 1815 kJ/mol Al2+(g) → Al 3+ (g) + e- I3 = 2740 kJ/mol Al3+(g) → Al 4+ (g) + e- I4 = 11, 600kJ/mol a. Account for the trend in the values of the ionization energies. b. Explain the large increase between I3 and I4

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