6th Edition 2.71

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6th Edition 2.71

Postby 305144105 » Sun Nov 04, 2018 11:42 am

2.71 (a) What is a diagonal relationship? (b) How does it arise? (c) Give two examples to illustrate the concept.

I read the textbook but I don't quite understand. Can someone please explain this?

Emily Kennedy 4L
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Re: 6th Edition 2.71

Postby Emily Kennedy 4L » Sun Nov 04, 2018 8:58 pm

So, basically what the book is saying is that groups of atoms on the periodic table tend to show similar characteristics and react with similar compounds. The example the book gives is that both lithium and magnesium react directly with nitrogen to form nitrides.

Luc Lorain 1L
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Re: 6th Edition 2.71

Postby Luc Lorain 1L » Sun Nov 04, 2018 10:40 pm

In short, diagonal trends exist because the trends of the periodic table cancel each other out if you go down and to the right.

As one goes down a group, atomic radius increases, electron affinity decreases, and ionization energy decreases. As one goes right across a period the opposite happens: atomic radius decreases, electron affinity increases, and ionization energy increases. As such, some elements one atom down and one atom to the right on the periodic table have very similar properties, such as Li and Mg, Be and Al, and B and Si.

To explain one of the examples, Boron and Silicon are both semiconductors that have acidic oxides.

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Re: 6th Edition 2.71

Postby CaminaB_1D » Sun Nov 04, 2018 11:10 pm

Is this something we should worry for the midterm?

Layla Manoochehri
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Re: 6th Edition 2.71

Postby Layla Manoochehri » Sun Nov 04, 2018 11:13 pm

i don't think so. maybe know the concept and generally what it is, but i'd say focus on main periodic trends like trends in atomic radius, ionic radius, ionization energy, and electron affinity for the midterm.

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