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By charge, I assume you mean oxidation number. Oxygen's oxidation number is a very dependable -2, with only a few strange exceptions. A better question would be "What is chlorine's oxidation number in ClO4-?" The answer would be +7.
ClO4 is polar.
The bond order of an ion with 8 valence electrons would depend on the specific atom and its bonding situation. For example, an oxygen atom typically forms two bonds, resulting in a bond order of 2. However, if the atom has gained or lost electrons to form an ion, the bond order can change accordingly.
The compound Ca(CLO4)2 is called calcium perchlorate. It consists of calcium ions (Ca²⁺) and perchlorate ions (ClO4⁻). In this formula, there are two perchlorate ions for each calcium ion, reflecting the need for charge balance in the compound.
The compound with the formula Ca(ClO4)2 is called calcium perchlorate. It is composed of one calcium ion (Ca²⁺) and two perchlorate ions (ClO4⁻). Calcium perchlorate is often used as a dehydrating agent and in various chemical applications.
Perchlorate ion (ClO4-) is colorless.
The symbol for the oxyanion perchlorate ion is ClO4-.
The answer is clo4- because it has the greatest bond order
ClO4- is the perchlorate ion.
The perchlorate ion has one available bond.
The formula for the perchlorate ion is ClO4-. It consists of one chlorine atom bonded to four oxygen atoms.
ClO3 has the smaller bond angle than ClO4
KClO4 has an ionic bond. In this compound, potassium (K) donates its electron to form a positive ion, while the perchlorate ion (ClO4) gains that electron to form a negative ion. The attraction between the positive and negative ions creates the ionic bond in KClO4.
1.5 for the C-O bond. and 1 for the C-H bond.
By charge, I assume you mean oxidation number. Oxygen's oxidation number is a very dependable -2, with only a few strange exceptions. A better question would be "What is chlorine's oxidation number in ClO4-?" The answer would be +7.
It is actually ClO4- which is Perchlorate ion
In ClO4-, the oxidation number of Cl is +7, and the oxidation number of each O is -2.