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Which one has the most covalent character?
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How would you work out:
Which one of the following has the most covalent character?
A MgF2
B MgBr2
C AlF3
D AlBr3
It's on the synoptic paper in chemistry, but i don't know how i would do it in the exam without knowing the electronegativities of the elements.
Which one of the following has the most covalent character?
A MgF2
B MgBr2
C AlF3
D AlBr3
It's on the synoptic paper in chemistry, but i don't know how i would do it in the exam without knowing the electronegativities of the elements.
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#2
Look at where they are in the Periodic table, the ones nearest each other, group-wise, are the most covalent.
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#3
You know that electronegativity increases from left to right and from down to up...
I would say it was MgBr2
I would say it was MgBr2
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#4
Magnesium Fluoride is ionic as well as Magnesium Bromide, so those two are out,
AlF3 and AlBr3, well Fluorine has the greater electronegativity hence I would guess D then? right?
In general Electronegativities decrease down the group and increase across (left to right) a period...
AlF3 and AlBr3, well Fluorine has the greater electronegativity hence I would guess D then? right?
In general Electronegativities decrease down the group and increase across (left to right) a period...
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#9
(Original post by modini)
Sorry come to think of it they're not
Sorry come to think of it they're not
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#10
AlBr3
Al3+ is more polarising than Mg2+ and the Br- (higher charge + smaller ionic radius), the anion is large and polarisable.
Al3+ is more polarising than Mg2+ and the Br- (higher charge + smaller ionic radius), the anion is large and polarisable.
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(Original post by xinolisss)
Try to work it out mate, it ain't that difficult
Magnesium Fluoride is ionic as well as Magnesium Bromide, so those two are out,
AlF3 and AlBr3, well Fluorine has the greater electronegativity hence I would guess C then? right?
In general Electronegativities decrease down the group and increase across (left to right) a period...
Try to work it out mate, it ain't that difficult
Magnesium Fluoride is ionic as well as Magnesium Bromide, so those two are out,
AlF3 and AlBr3, well Fluorine has the greater electronegativity hence I would guess C then? right?
In general Electronegativities decrease down the group and increase across (left to right) a period...
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#14
It is AlBr3...I dont think you need electronegativities, just FAJAN'S RULES..
Al^3+ is a smaller molecule and has higher positive charge then Mg^2+
Br- is a bigger molecule then F-
Therefore more covalent as the electron cloud of Br is attracted more and its more negative...
Al^3+ is a smaller molecule and has higher positive charge then Mg^2+
Br- is a bigger molecule then F-
Therefore more covalent as the electron cloud of Br is attracted more and its more negative...
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#16
This question can be solved by Fajan's Rule. According to the rule, smaller size of cation and larger size of anion favours more of covalent character. The opposite will result in more of ionic character
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#17
(Original post by ArinSom)
This question can be solved by Fajan's Rule. According to the rule, smaller size of cation and larger size of anion favours more of covalent character. The opposite will result in more of ionic character
This question can be solved by Fajan's Rule. According to the rule, smaller size of cation and larger size of anion favours more of covalent character. The opposite will result in more of ionic character
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