Which of the following best helps to explain why the electron affinity of Br has a greater magnitude than that of I? Br has a lower electronegativity than I does.

Answer A: B r has a lower electronegativity than I does.
A

Br has a lower ionization energy than I does.

Answer B: B r has a lower ionization energy than I does.
B

An added electron would go into a new shell in Br but not in I.

Answer C: An added electron would go into a new shell in B r but not in I .
C

There is a greater attraction between an added electron and the nucleus in Br than in I.

"you start with 15.67 g mgco3-xh2o, when heated and all the water is removed, you are left with 7.58 g mgco3 only.

therefore, you had 15.67 - 7.58 = 8.09g h2o  

moles of each :

7.58g mgco3 = ? moles = 7.58g / 83.4g/mole = 0.09moles  

8 09g h2o = ? moles = 8.09g / 18g/mole = 0.44moles  

molar ratio between the two by dividing both numbers by the smallest number :

0.09 / 0.09 = 1  

0.44 / 0.09 = 4.8  

mgco3-5h2o"

substituting a hydrogen atom with a halogen in a hydrocarbon:

- the single bond remains single. a is wrong.

- the bond with hydrogen is as strong as with a halogen. c is wrong

- a hydrocarbon is saturated if there is no double bond. we do not know that so d is wrong.

- carbon will always have four valence electrons. e is wrong.

by elimination, the correct answer is b. the boiling point of the new compound increases.