Charges of Ions in Periodic Table

[courtrigrad]

Hello all

Is there any good way to memorize the charges of elements in the periodic table?

Thanks?

 

[MathStudent]

Yes... the elements in the 1st column form +1 ions
" " " " 2nd " form +2 ions

The transition metals are tricky but I wouldn't expect you'd have to know those in an elementaary class

All the elements on the right side of the table form (-) ions except the noble gases
The elements in column 7 form - 1 ions (starting with Fluorine )
" " " " 6 form - 2 ions (starting with Oxygen )
" " " " 5 form - 3 ions (starting with Nitrogen )

Colum 4 (sarting with Carbon ) doesn't ionize
and for colum 3 Boron and Aluminum form +3 ions

By colums I am really reffereing to the families which are usually given in Roman Numerals

 

[DB]

Absolutely. Take your periodic table and starting on top of Hydrogen (the alkaline family) write 1+. Then for each family continue, alkali Earth metals 2+ *skip the transition metals, most people refer to a book for the charge of a specific metal because they have many different charges. So now on top of Boron you have 3+, Carbon 4+4-, Nitrogen 3-, until Helium zero. Every element downward (same family) has the same charge, but different valence number. The valence electron number is given by going downward by period. For example H, and He =1 valence electron. Soon enough, have a picture of the periodic table in your head, you begin to automatically know the charge.

 

[DB]

If I had a nickel for everytime that happened...

 

[courtrigrad]

thanks a lot guys.

so from Boron to the end it goes: $$3^+ , 4^+ 4^-, 3^-, 2^-, 1^-$$?

PS: What are the basic rules in naming inorganic compounds?

 

[DB]

thanks a lot guys.

so from Boron to the end it goes: $$3^+ , 4^+ 4^-, 3^-, 2^-, 1^-$$?

Yup

PS: What are the basic rules in naming inorganic compounds?

Organic compound? That I am not, sure usually they just give it a name like sulfuric acid or citric acid. But for binary, or radical compounds it goes as follows.
Let's say you have Mg and N:
$$Mg^{2+}N^{3-}$$
You cross the charges over and get,
$$Mg_3N_2$$
You now have Magnesium Nitride
When a metal and a non-metal react, you don't need to use prefixes, but let's say Nitogen and oxygen, once the cross is done you have
$$N_2O_3$$
Now you have dinitrogen trioxide.

*Maybe you already knew this...

 

[MathStudent]

thanks a lot guys.

so from Boron to the end it goes: $$3^+ , 4^+ 4^-, 3^-, 2^-, 1^-$$?

PS: What are the basic rules in naming inorganic compounds?

NO ... be carefull
The column containing Carbon doesn't ionize (there's no such thing as +4 or -4 ion)
The column containing Nitrogen then starts with -3
The column all the way to the right (the noble gasses) doesn't ionize they are stable => they never ever ever ionize ( at least for the sake of an elementary chemistry class which extends to first two years undergrad )

PS
for ionic compounds, just add the suffix -ide to the end of the non-metal
for covalent compounds you need to use the rules about prefixes (you can find these online, and they should be in your book )

 

[courtrigrad]

are you sure about the $$4^+, 4^-$$ ? Also is there any good device for memorizing the solubility rules?

Thanks

 

[MathStudent]

are you sure about the $$4^+, 4^-$$ ? Also is there any good device for memorizing the solubility rules?

Thanks

Positive about the +4 -4, the reason that atoms become ions is because they want to obtain an octet of valence electrons. For metals( which typically have 1,2,or 3 valence electrons as atoms) it is much easier to lose 1 or 2 electrons rather than gain 7 or 6. Thus they tend to become positive ions. For non-metals (which have 5,6,or 7 electrons in their valence shell) it is much easier to gain 1,2,or 3 electrons and so become negatively charged. For carbon which is right in the middle with 4 electrons it tends to share its electrons with other atoms rather than accept or give off any. This is due to the size of carbon as well as geometric and electromagnetic proerties which you don't need to go into.

As far as the solubility rules all the alkalines are soluble. As far as the rest,, these typically just need to be memorized, no tricks or short cuts