Question 1 (5 points) In a same group, electronegativity decreases from bottom t

Question

Question 1 (5 points)

In a same group, electronegativity decreases from bottom to top so bromine is less electronegative than iodine.

Question 1 options:

Question 2 (5 points)

A diatomic molecule with a triple covalent bond is _____.  

Question 2 options:

N2

F2

O2

Question 3 (5 points)

Consider the molecule IF5 and PF5. How do the molecular shapes differ?

Question 3 options:

In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on phosphorus. As a result, the molecular shape of IF5 is square pyramidal and PF5 is trigonal bipyramidal.

In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on phosphorus. As a result, the molecular shape of IF5 is octahedral and PF5 is trigonal bipyramidal.

In PF5 there is a lone pair of electrons on phosphorus where as in IF5 there are no lone pairs on iodine. As a result, the molecular shape of PF5 is square pyramidal and IF5 is trigonal bipyramidal.

Question 4 (5 points)

Bond Enthalpies are always:

Question 4 options:

positive

equal to zero under STP

negative

it depends on the temperature

In an I-Br molecule, the iodine has a partial positive charge.

Question 6 options:

Explanation / Answer

Question 1 (5 points)

In a same group, electronegativity decreases from bottom to top so bromine is less electronegative than iodine.

TRUE: Electronegativity decreases, since the size of molecule increases

Question 2 (5 points)

A diatomic molecule with a triple covalent bond is _____.

The only option is Nitrogen. It is the only stable form to have N (triple) N

Question 3 (5 points)

Consider the molecule IF5 and PF5. How do the molecular shapes differ?

In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on phosphorus. As a result, the molecular shape of IF5 is octahedral and PF5 is trigonal bipyramidal.

Question 4 (5 points)

Bond Enthalpies are always:

positive, since they all require energy

In an I-Br molecule, the iodine has a partial positive charge

True, Bromine is more electronengative, therefore will take more charge (negative) and I will be slightly positive

In IF5 there is a lone pair of electrons on iodine where as in PF5 there are no lone pairs on phosphorus. As a result, the molecular shape of IF5 is octahedral and PF5 is trigonal bipyramidal.

Question 4 (5 points)

Bond Enthalpies are always:

positive, since they all require energy

In an I-Br molecule, the iodine has a partial positive charge

True, Bromine is more electronengative, therefore will take more charge (negative) and I will be slightly positive

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