Which of the two elements (Ag and Cu) is higher and which is lower in the series knowing that the reduced form of the element will react spontaneously. Explain your answer.   lower: higher:

(a) Rank elements: Na, Mg, Al, and K, in increasing order of: (i) atomic size; (ii) ionization energy, and (iii) reactivity. (b) Explain why atomic size decreases from left to right, but increases from top to bottom; (c) Explain why ionization energy increases from left to right, but decreases from top to bottom; (d) Explain why the reactivity of alkali metals (Group-1) increases from top to bottom, where as the reactivity of halogen (Group-17) decreases from top to bottom.

Briefly explain the following trends and derive a reason for the following observations: a) ionization energy (include the definition & equation) - how does the second ionization energy of sodium compare to the first ionization energy of magnesium? Is it higher or lower and why? b) electron affinity (include the definition & equation) - why is the electron affinity of carbon larger (more negative) than that of nitrogen when oxygen and fluorine are more negative than carbon? c) electronegativity - why do beryllium and aluminum exhibit similar electronegativities? The electronegativities are 1.57 (Be) and 1.61 (AI). d) electron configurations why is the electron configuration of chromium [Ar] 3d54s¹ and not [Ar]3d¹4s²? Why is the electron configuration of ytterbium [Xe] 4f¹46s² and not [Ar] 4f135d¹6d²? -

The electron configuration of an element describes how electrons are distributed in its atomic orbitals. (a) Explain the applications of the Aufbau principle, Hund's rule and the Pauli exclusion principle in relation to electronic configuration of oxygen atom. Explain how these principles determine the stability and reactivity of atoms oxygen.

Why are the electron configurations for Cu and Cr (and elements with similar valence electron configurations) different than the expected configurations? Support your answer with electron configuration(s)

I think the answer is chlorine, but why is bromine not a valid answer?? Please explain, thanks.

Which has a greater ionization energy, K or Ca and why

(a) Identify the following neutral elements by their condensed electron configurations. (Enter the chemical symbol or name of the element.) (i)    [Ar] 4s2 3d3 (ii)    [Kr] 5s2 4d10 5p3 (iii)    [Ar] 4s2 3d10 4p4

Write condensed electron configurations for the following atoms and ions, using appropriate noble-gas core abbreviations. Put superscripted electron count numbers in parentheses. Examples: Fe = [Ar]4s(2)3d(6), Sn2+ = [Kr]4d(10)5s(2), s2- = [Ar]. (a) Te2- = [Kr]4d(10)

2.(a) Write the full electron configuration for each of Ge and Ge3-2.(b) Write the noble gas configuration, and valence configuration of Ge 2.(c) Write the orbital diagram for the Ge3-2.(d) For the unpaired electron in the orbital diagram for the Ge3-ion, give its four quantum numbersn,l,ml,ms 2.(e) Is Ge3+ diamagnetic or paramagnetic?