Can you answer part B

The usual oxidation state of boron and aluminum is +3, whereas the heavier elements in group 13 have an increasing tendency to form compounds in the +1 oxidation state. Given that all group 13 elements have an ns2np1 electron configuration, how do you explain this difference between the lighter and heavier group 13 elements?

stion 18 of 19 Write a chemical equation representing the second ionization energy for lithium. Use e as the symbol for an electron. chemical equation:

A hypothetical element A has these properties: first ionization energy= 850 kJ/mol second ionization energy= 1700 kJ/mol third ionization energy= 13,999 kJ/mol a) if you were to react element A with oxygen, what would be the chemical formula of the resulting compound? b) write the balanced chemical equation of a reacting with oxygen to give the product from part a. c) would you expect the product of the chemical reaction of a with auction gym to be a basic, acidic or an amphoteric oxid?

which of these elements have the smallest atomic radius? silicon sodium cholrine sulfur phosphorus

1. Which halogen has the highest ionization energy? Explain why. 2. Explain why, at room temperature, fluorine and chlorine are gases, bromine is a liquid, and iodine is a solid.

What is the element with the smallest atomic radius in period 4?   Give this element’s ground state noble gas orbital diagram and its electron configuration.

Which of the following pnictogens (N, P, or As) has the atomic radius?  This chalcogen has the smallest atomic radius because, compared to the other chalcogens, it has___  number of electron shells and___  effective nuclear charge. Which of the following third-period elements (Na, Si, or S) has the smallest atomic radius?  This third-period element has the smallest atomic radius because, compared to the other third-period elements, it has___  number of electron shells and___  effective nuclear charge. options to pick from:  - the largest, the smallest, about the same

Why is chlorine a halogen