The ion has a noble gas electron configuration. O 02+ O F2-

Is K2S ionic and held together by opposite charge or shared electrons in

Arrange the single covalent bonds within each set in order of INCREASING polarity. If: • most polar is b • medium polarity is c • least polar is a this leads to the following input: acb (To answer this question you may consult the table of electronegativity values in the table below.) 1A 2A Li Be 1.0 1.5 Na Mg 0.9 1.2 3B 4B 5B 6B 7B K Ca Sc Ti V 0.8 1.0 1.3 1.5 Rb Sr 0.8 1.0 1.2 Y Zr 1.4 <1.0 1.0-1.4 Cr Mn 1.5 1.6 1.6 Nb Mo 1.6 1.8 Cs Ba La Hf Ta 0.7 0.9 1.1 W 1.3 1.5 1.7 1.5-1.9 2.0-2.4 Fe 1.8 H 2.1 Re Os 1.9 2.2 8B Co Ni 1.8 1.8 1B 2B Cu Zn 1.9 1.6 Ir Pt Au 2.2 2.2 2.4 2.5-2.9 3.0-4.0 Te Ru Rh Pd Ag Cd In 1.9 2.2 2.2 2.2 1.9 1.7 1.7 3 A 4A 5A 6A 7A B N 0 F C 2.5 3.0 3.5 2.0 4.0 Hg 1.9 Al 1.5 Si P S CI 1.8 2.1 2.5 3.0 Ga Ge 1.6 As Se 1.8 2.0 2.4 Br 2.8 Sn Sb Te I 1.9 2.1 2.5 1.8 TI Pb Bi Po 1.8 1.8 At 1.9 2.0 2.2

Give the VSEPR and molecular shape for each element

How many valence electrons does phosphorus contain? O 10 O 15 O 5 3 2

Which of the following answer choices explains how Lewis-Dot structures are used in Chemistry? O Lewis-Dot Structures are used to illustrate the valence electrons of an atom. Valence electrons are represented as dots around the element symbol of the atom. O Lewis-Dot Structures are used to illustrate the core electrons of an atom. Core electrons are represented as dots around the element symbol of the atom. O Lewis-Dot Structures are used to illustrate the protons of an atom. Protons are represented as dots around the element symbol of the atom. O Lewis-Dot Structures are used to illustrate the neutrons of an isotope. Neutrons are represented as dots around the element symbol of the atom.

Starting with 1s2draw out the complete electron configuration for the most stable ion of selenium. Explain how you used the Octet Rule to determine your answer.

Predict the most stable ion of mercury O 2- O 3+ 1+ It is a Type II metal and would have more than one charge 2+

question 4