Question 2 Which of the following is correct for the 15t ionization energies of S, Se, F S>P> Se

< Question 15 of 18 Arrange these elements according to first ionization energy. Highest ionization energy Lowest ionization energy Answer Bank As K Se Ga Kr Ge Са Br

Which element would have the least favorable favorable (least negative) electron affinity?  S, Si, Al, Cl     Which equation below illustrates the first electron affinity for sulfur?

Put the following in order of decreasing ionization energy: Fe, Ba, O, Zn

Which of the following pairs is isoelectronic I Al^ 3+ and B^ 3+; S^ 2- and Ne; Li and K^ + ;Na * and Ne

The number in parentheses after the symbol is the element's atomic number Choose the element with the smallest radius Select ] Choose the neutral atom or ion with the smallest radius [Select ] Choose the element with the smallest ionization energy [ Select ] Choose the element with the smallest electron affinity (magnitude) [Select] a %23 99+ hp 立

Type the element in each list with the largest atomic radius: Na, Al, Mg - Rb, F, N Ca, Sr, Ba Fr, Be, K ↑ ↑ ? ? ? ? TYPE

Which of the options below provides a reason why the covalent radius of hafnium (1.44 Å) is less than that of zirconium (1.45 Å), even though the element above it in the periodic table? A. Between Zr and Hf lies the 4d10 configuration due to the transition metals. This leads to much greater Z* because the d electrons are so poor at shielding. Thus Hf is smaller than expected for an element in a higher shell than Zr, called the Scandide contraction. B. Hf being below Zr suggests that it will have a smaller atomic radius because the trend shows a decrease going down a group. C. Hf is below Zr and has a smaller ionisation energy, electron affinity and electronegativity compared to Zr. This reduces its atomic radius, thus leading to it having a smaller atomic radius compared to that of Zr. D. Between Zr and Hf lies the 4f14 configuration due to the Lanthanides. This leads to much greater Z* because the f electrons are so poor at shielding. Thus Hf is smaller than expected for an element in…

Rank the following species in terms of increasing size:F, H, Te, N, O, Br-, I-.

element X has an electron affinity of 295.3 kJ/mol and the following ionization energies (in kJ/mol): IE1 = 1.008e3, IE2 = 1.846e3, IE3 = 3.20e3. In what column of the periodic table is this element probably found?