The first five ionization energies (IE,through IE) of a Period 6 element have the following pattern: kJ/mol IE₁ IE2 IE3 IE4 IE5 Make a reasonable guess about which element this is. Enter its chemical symbol below. 0 X

Which of the following atoms and ions is (are) isoelectronic with Si: Ar, S2+, Ne, Al3+, P3−, As3+?

Consider the following set of successive ionization energies: IE1=578kJ/mol IE2=1,820kJ/mol IE3=2,750kJ/mol IE4=11,600kJ/mol To which third-period element do these ionization values belong?

Which of the following atoms is the largest? O Rb O Li OK O Cs O Na

Indicate which one statement is not true by checking the box in front of the untrue statement.     The ionic radius of a sodium ion is larger than the atomic radius of a sodium atom.     The ionic radius of a chloride ion is larger than the atomic radius of a chlorine atom.     The ionic radius of a calcium ion is smaller than the atomic radius of a bromide ion.     The ionic radius of a calcium ion is smaller than the atomic radius of a potassium ion.     The ionic radius of a nickel(II) ion is smaller than the atomic radius of a nickel atom.

An atomic cation with a charge of +1 has the following electron configuration: 1s²2s²2p5 What is the chemical symbol for the ion? How many electrons does the ion have? How many 2p electrons are in the ion? 1 1 X

Which of the following elements has the highest first ionization energy? Ве Na Li Rb K

Which of the following elements would you expect to have chemical properties most similar to those of sulfur (S)? Na Sr Se CI

Which of the following atom has the lowest ionization energy (IE1)? A Li B D C N F

Select the element that best fits. You may use elements more than once. All elements are not used.