Respuesta :
These are two questions and two answers.
Question 1) The elements most likely to form more than one type of ion are the ______.
Answer: option A) transition metals.
Jusitification:
1) The elements form ions by gaining or losing electrons. By gaining electrons, theY form anions (negative iones); by losing electrons, they form cations (positive ions).
2) The valence shell of the akaly metals is the type ns¹, which means that they have one electron in the valence shell. Then, they only can form one kind of ion which has the configuration of the previous noble gas (n-1)s²(n-1)p⁶ with 1+ charge.
3) The halogens have valence shell of the type ns²np⁵. That means that easily gain 1 electron to complete the valence shell ns²np₆ (the configuration of the next noble gas), with charge 1-. Gaining 5 electrons or losing more electrons than 1 is very disfavourable, so that is the only kind of ion they form.
4) The valence shells of alkaline earth metals are of the kind ns². So, the most favourable energetic ion is formed by losing 2 electrons and so taking the configuration of the previous noble gas, with charge 2+. That is the only type of ion they form.
5) Transition metals have electrons in the orbitals d, which are very similar in energy, and so they might loose 1, 2, or 3, electrons fo form ions with charges 1+, 2+, or 3+ respectively.
Question 2) The name iron(II) indicates that a compound contains _______.
A) iron ions with an II+ charge.
B) iron ions with a 2+ charge.
C) iron ions with a negative charge.
D) two types of iron ions.
Answer: option B) iron ions with a 2+ charge.
The oxidation state may be indicated as Roman numerals, in this case II, or as a conventional number with its charge.
Iron, a transition metal, may loose 2 or 3 valence electrons. When it loses 2 electrons it forms an ion (cation) with positive charge 2. So, it is iron 2+
Question 1) The elements most likely to form more than one type of ion are the ______.
Answer: option A) transition metals.
Jusitification:
1) The elements form ions by gaining or losing electrons. By gaining electrons, theY form anions (negative iones); by losing electrons, they form cations (positive ions).
2) The valence shell of the akaly metals is the type ns¹, which means that they have one electron in the valence shell. Then, they only can form one kind of ion which has the configuration of the previous noble gas (n-1)s²(n-1)p⁶ with 1+ charge.
3) The halogens have valence shell of the type ns²np⁵. That means that easily gain 1 electron to complete the valence shell ns²np₆ (the configuration of the next noble gas), with charge 1-. Gaining 5 electrons or losing more electrons than 1 is very disfavourable, so that is the only kind of ion they form.
4) The valence shells of alkaline earth metals are of the kind ns². So, the most favourable energetic ion is formed by losing 2 electrons and so taking the configuration of the previous noble gas, with charge 2+. That is the only type of ion they form.
5) Transition metals have electrons in the orbitals d, which are very similar in energy, and so they might loose 1, 2, or 3, electrons fo form ions with charges 1+, 2+, or 3+ respectively.
Question 2) The name iron(II) indicates that a compound contains _______.
A) iron ions with an II+ charge.
B) iron ions with a 2+ charge.
C) iron ions with a negative charge.
D) two types of iron ions.
Answer: option B) iron ions with a 2+ charge.
The oxidation state may be indicated as Roman numerals, in this case II, or as a conventional number with its charge.
Iron, a transition metal, may loose 2 or 3 valence electrons. When it loses 2 electrons it forms an ion (cation) with positive charge 2. So, it is iron 2+
1. [tex]\boxed{\left( {\text{A}} \right){\text{ transition metals}}}[/tex] are most likely to form more than one type of ions.
2. The name iron (II) indicates that a compound contains [tex]\boxed{\left( {\text{B}} \right){\text{ iron ions with a 2+ charge}}}[/tex]
Further Explanation:
(1) The elements in which the valence electrons are present in d-orbitals are called d-block elements or transition metals. These have partially filled d orbitals in their ground or in one of the stable oxidation states. The general electronic configuration of transition elements is [tex]\left[ {{\mathbf{Inert gas}}} \right]\left( {{\mathbf{n - 1}}} \right){{\mathbf{d}}^{{\mathbf{1 - 10}}}}{\mathbf{n}}{{\mathbf{s}}^{{\mathbf{0 - 2}}}}[/tex]. Since all the d-orbitals are similar in energy, transition elements have the tendency to lose 1, 2 or 3 electrons, thus resulting in variable oxidation states. So these metals can form more than one type of ions.
Alkali metals are those elements that have the general electronic configuration of [tex]\left[ {{\mathbf{Inert gas}}} \right]{\mathbf{n}}{{\mathbf{s}}^{\mathbf{1}}}[/tex]. These metals lose one electron in order to achieve stable noble gas configuration. So these metals can form ions of +1 charge only.
Halogens are the group of elements that have the general configuration of [tex]\left[ {{\mathbf{Inert gas}}} \right]{\mathbf{n}}{{\mathbf{s}}^{\mathbf{2}}}{\mathbf{n}}{{\mathbf{p}}^{\mathbf{5}}}[/tex]. These metals can gain an electron in order to fulfill their outermost valence shell. So halogens can form ions of -1 charge only.
Alkaline earth metals are those elements that have the general electronic configuration of [tex]\left[ {{\mathbf{Inert gas}}} \right]{\mathbf{n}}{{\mathbf{s}}^{\mathbf{2}}}[/tex]. These metals can easily lose two electrons in order to achieve a stable noble gas configuration. So these metals can form ions of +2 charge only.
So only transition metals can form more than one type of ions.
(2) Consider an element X with an oxidation state ‘a’. Such an element is written as X(a). Here, the oxidation state of the element is written in the parenthesis, preceded by the letter symbol of the element. Oxidation state is the number of electrons gained, lost or shared during a chemical reaction and is generally written in Roman numerals. In case of simple ions, oxidation number and charge are the same things.
Iron is a transition metal. It can lose two or three electrons to form the corresponding cations. Iron(II) indicates that its oxidation state is +2, which implies that the ions of iron have a charge of +2.
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Answer details:
Grade: Senior School
Subject: Chemistry
Chapter: d-block elements
Keywords: transition metals, d-block elements, d-orbitals, oxidation state, cations, charge, iron, alkali metals, halogens, alkaline earth metals, electronic configuration, noble gas configuration, electrons, +1, +2, -1, partially filled.
