Ions of elements taken off of the Periodic Table that have a negative charge. In other words, ions that contain only one element. For example, the Chloride Ion (Cl-1) is the ion of Chlorine. Naming the ion goes like this:
Chlorine-"ine"=chlor+"ide"=chloride. In other words, drop the ending of the name of the element and add "ide".
It ends in -ide when they are 'made' of one anionic atom: it is for salts of negatively charged, non-metal and mono-elemental ions.
Simplier said: they are negative, single ions of non-metals
Examples:
Cl- chloride, S2- sulfide, N3- nitride, C4- carbide, and of course last but not least: oxide with O2-.
Anions derived from acids ending in -ic (and without the prefix hydro-) are given the suffix -ate.
For example, the sulfate anion in derived from sulfuric acid.
However, hydrochloric acid produces the chloride anion.
They are 'made' of one anionic atom: it is for salts of negatively charged, non-metal and mono-elemental ions.
Simplier said: they are negative, single ions of non-metals
Examples:
Cl- chloride, S2- sulfide, N3- nitride, C4- carbide, and of course last but not least: oxide with O2-.
Anions end in -ide if they are monatomic. Example: chlorine becomes "chloride." Polyatomic ions will have different suffixes.
no.
The names of most polyatomic ions end in -ite or -ate.
No. The hydroxide ion has a negative charge as do all ions ending in -ide, -ite, or -ate.
The "ite" vs. "ate" in ions refers to the number of oxygens in the ion. ex: Nitrate = NO3- Nitrite = NO2- It follows the system of: per....ate (add one oxygen to ate) ate (3 or 4 oxygens, depending on the ion, this is usually the "base") ite (subtract one oxygen from ate) hypo....ite (subract two oxygens from ate
If anion is a single atom then ending is 'ide' if it is complex and also contains oxygen then with highest no of oxygen possible, ending is 'ate' otherwise is 'ite'
Binary and Oxyacids are named by identifying the number of hydrogen Ions found in the chemical formula.
The names of most polyatomic ions end in -ite or -ate.
Polyatomic ions ending in -ate in common form contain oxygen.
There is no single ion that leads to the endings -ate or -ide, though ions with such ions can be assumed to be negative ions (anions). A few examples are given below. Monatomic anions have names ending in -ide: Hydride: H- Nitride: N3- Oxide: O2- Sulfide: S2- Chloride: Cl2- A few polyatomic ions have names ending in -ide as well Peroxide: O22- Hydroxide: OH- Cyanide; CN- Ions with names ending in -ate are polyatomic anions that contain the maximum oxygen for that atom. The prefix per- indicates an even higher number of oxygen atoms and/or a higher oxidation state: Carbonate: CO32- Acetate: C2H3O2- Nitrate: NO3- Sulfate: SO42- Cyanate: OCN- Chlorate: ClO3- Perchlorate: ClO4- A few ions ending in -ate, however, do not contain oxygen Thiocyanate: SCN- Hexafluorosilicate: SiF62- Tetrafluoroborate: BF4-
ite or ate
Bicarbonate is an anion. Ions ending in -ate, -ite, or -ide are anions.
No. The hydroxide ion has a negative charge as do all ions ending in -ide, -ite, or -ate.
It will end in -ic acid. For example perchlorate --> perchloric acid
The "ite" vs. "ate" in ions refers to the number of oxygens in the ion. ex: Nitrate = NO3- Nitrite = NO2- It follows the system of: per....ate (add one oxygen to ate) ate (3 or 4 oxygens, depending on the ion, this is usually the "base") ite (subtract one oxygen from ate) hypo....ite (subract two oxygens from ate
Gyrate
they basically ate the same things we do here in California just with different names
The -ite or -ate ending in a polyatomic ion is simply an indication of the amount of oxygen atoms present. The -are ending is used in the base form. If the polyatomic ion has one less oxygen atom than the -ate form, the -ite form applies.
The -ite or -ate ending in a polyatomic ion is simply an indication of the amount of oxygen atoms present. The -are ending is used in the base form. If the polyatomic ion has one less oxygen atom than the -ate form, the -ite form applies.