As elements of Group 1 of the Periodic Table are considered in order from top to bottom, the ionization energy of each successive element decreases. This decrease is due to __. increasing radius and increasing shielding effect high ionization energy and high electronegativity first ionization energy because they have the same number of valence electrons On the Periodic Table of the Elements, all the elements within group 16 have the same number of __ neutrons electronegativity valence electrons protons Which statement best describes Group 2 elements as they are considered in order from top to bottom of the Periodic Table? Be, Mg, Ca increases the number of principal energy levels increases, and the number of valence electrons remains the same O Which properties are most common in nonmetals? first ionization energy increasing radius and increasing shielding effect less than that of nitrogen and oxygen high ionization energy and high electronegativity Which element in Group 16 has the greatest tendency to gain electrons? Ba the number of principal energy levels increases, and the number of valence electrons remains the same I O Which sequence of elements is arranged in order of decreasing atomic radii? Be, Mg, Ca Al, Si, P N, C, B Cl, Br, I The strength of an atom's attraction for the electrons in a chemical bond is the atom's __ electronegativity valence electrons polar covalent bond first ionization energy Which Group 17 element has the lest attraction for electrons? I Ba O flurine Why do elements in the same family generally have similar properties? the average mass of one atom of the element because they have the same number of valence electrons that there is a hidden pattern in the elements increasing radius and increasing shielding effect Which sequence correctly places the elements in order of increasing ionization energy? O-s-se-te H-li-na-k H-be-al-ga I-Br-Cl-F As the elements Li to F in Period 2 of the Periodic Table are considered in succession, how do the relative electronegativity and the covalent radius of each successive element compare? because they have the same number of valence electrons valence electrons first ionization energy the relative electronegativity increases, and the atomic radius increases The Group 17 element with the highest electronegativity is __ adenine cytosine flurine fluoride The elements calcium and strontium have similar chemical properties because they both have the same __ atomic number number of valence electrons first ionization energy electronegativity Which of these elements has the least attraction for electrons in a chemical bond? carbon nitrogen helium oxygen What is the total number of valence electrons in an atom of xenon, Xe? I 8 K 3 Which element is a member of the halogen family? helium high ionization energy and high electronegativity K I Which of the following atoms has the largest atomic radium? nitrogen [Ar]3d⁵4s² helium K Which noble gas has the highest first ionization energy? helium hydrogen nitrogen oxygen Why does fluorine have a higher ionization energy than iodine? a larger nuclear charge a transition metal it is higher up on the periodic table valence electrons Rank the following elements by increasing electronegativity: sulfur, oxygen, neon, aluminium oxygen, carbon, aluminium, potassium aluminium, sulfur, oxygen, neon al, si, p number of valence electrons