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Transition metals that can form more than one type of ion are distinguished by using Roman numerals in parentheses after the metal's name in the compound's formula. For example, in iron(II) chloride (FeCl₂), the Roman numeral II indicates that iron has a +2 charge, while in iron(III) chloride (FeCl₃), the Roman numeral III indicates a +3 charge. This notation helps clarify the specific oxidation state of the metal ion in the compound.

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How are these ions distinguished from one another in writing formulas for compounds?

Ions are distinguished by their charge and ratio in chemical formulas. The charge of each ion determines how they combine to form a neutral compound through the crisscross method. The crisscross method helps ensure that the total positive charge equals the total negative charge in the compound.


How do the formulas differ from molecular and ionic compounds?

Molecular compounds are formed by sharing of electrons between atoms, resulting in covalent bonds, while ionic compounds are formed by transferring electrons from one atom to another, resulting in ionic bonds. Molecular compounds have discrete molecules with defined molecular formulas, while ionic compounds do not have discrete molecules and are represented by empirical formulas showing the ratio of ions present in the compound.


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Transition metals have multiple oxidation states due to the number of electrons that an atom loses, gains, or uses when joining another atom in compounds. It also determined the ability of an atom to reduce.


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Metals are more likely to donate electrons to form ionic compounds. However, some transition metals such as mercury and tin can form covalent bonds in which the metal shares an electron with another atom


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