The ionic charge for the given element Sulfur ( S ) .

Question

Want to see more full solutions like this?

Answer 1

Question

Chapter 12, Problem 13E

(a)

To determine

The ionic charge for the given element Sulfur (S) .

(a)

Expert Solution

Answer to Problem 13E

The ionic charge for sulfur (S) is 2− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Sulfur belongs to the group 6A. The elements of group 6A have two electrons less than the noble configuration thus tends to gain two electrons and complete their octet.

The elements of group 6A gain two electrons and form an anion with charge 2− .

Conclusion:

Therefore, the ionic charge for sulfur (S) is 2− .

(b)

To determine

The ionic charge for the given element potassium (K) .

(b)

Expert Solution

Answer to Problem 13E

The ionic charge for potassium (K) is 1+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Potassium belongs to the group 1A. The elements of group 1A have one electron more than the noble configuration thus tends to lose one electron and complete their octet.

The elements of group 1A lose one electron and form a cation with charge 1+ .

Conclusion:

Therefore, the ionic charge for potassium (K) is 1+ .

(c)

To determine

The ionic charge for the given element bromine (Br) .

(c)

Expert Solution

Answer to Problem 13E

The ionic charge for bromine (Br) is 1− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Bromine belongs to the group 7A. The elements of group 7A have one electron less than the noble configuration thus tends to gain one electron and complete their octet.

The elements of group 7A gain one electron and form an anion with charge 1− .

Conclusion:

Therefore, the ionic charge for bromine (Br) is 1− .

(d)

To determine

The ionic charge for the given element nitrogen (N) .

(d)

Expert Solution

Answer to Problem 13E

The ionic charge for nitrogen (N) is 3− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Nitrogen belongs to the group 5A. The elements of group 5A have three electrons less than the noble configuration thus tends to gain 3 electrons and complete their octet.

The elements of group 5A gain 3 electrons and form an anion with charge 3− .

Conclusion:

Therefore, the ionic charge for nitrogen (N) is 3− .

(e)

To determine

The ionic charge for the given element magnesium (Mg) .

(e)

Expert Solution

Answer to Problem 13E

The ionic charge for magnesium (Mg) is 2+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Magnesium belongs to the group 2A. The elements of group 2A have two electrons more than the noble configuration thus tends to lose two electrons and complete their octet.

The elements of group 2A lose two electrons and form a cation with charge 2+ .

Conclusion:

Therefore, the ionic charge for magnesium (Mg) is 2+ .

(f)

To determine

The ionic charge for the given element neon (Ne) .

(f)

Expert Solution

Answer to Problem 13E

The ionic charge for neon (Ne) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Neon belongs to the group 8A. The elements of group 8A are called noble gas elements. They have completely filled octet and are very stable. They do not gain or lose electrons because they are already very stable.

Thus, the elements of group 8A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for neon (Ne) is 0 .

(g)

To determine

The ionic charge for the given element carbon (C) .

(g)

Expert Solution

Answer to Problem 13E

The ionic charge for carbon (C) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Carbon belongs to the group 4A. Elements of group 4A have 4 valence electrons and 4 electrons less than noble configuration. Elements of group 4A do not form ions generally because it is very difficult to gain or lose 4 electrons to complete the octet.

Thus, the elements of group 4A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for carbon (C) is 0 .

(h)

To determine

The ionic charge for the given element aluminium (Al) .

(h)

Expert Solution

Answer to Problem 13E

The ionic charge for aluminium (Al) is 3+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Aluminium belongs to the group 3A. The elements of group 3A have three electrons more than the noble configuration thus tends to lose three electrons and complete their octet. The elements of group 3A lose three electrons and form a cation with charge 3+ .

Conclusion:

Therefore, the ionic charge for aluminium (Al) is 3+ .

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Students have asked these similar questions

For each of the actions depicted below, a magnet and/or metal loop moves with velocity v→ (v→ is constant and has the same magnitude in all parts). Determine whether a current is induced in the metal loop. If so, indicate the direction of the current in the loop, either clockwise or counterclockwise when seen from the right of the loop. The axis of the magnet is lined up with the center of the loop. For the action depicted in (Figure 5), indicate the direction of the induced current in the loop (clockwise, counterclockwise or zero, when seen from the right of the loop). I know that the current is clockwise, I just dont understand why. Please fully explain why it's clockwise, Thank you

A planar double pendulum consists of two point masses \[m_1 = 1.00~\mathrm{kg}, \qquad m_2 = 1.00~\mathrm{kg}\]connected by massless, rigid rods of lengths \[L_1 = 1.00~\mathrm{m}, \qquad L_2 = 1.20~\mathrm{m}.\]The upper rod is hinged to a fixed pivot; gravity acts vertically downward with\[g = 9.81~\mathrm{m\,s^{-2}}.\]Define the generalized coordinates \(\theta_1,\theta_2\) as the angles each rod makes with thedownward vertical (positive anticlockwise, measured in radians unless stated otherwise).At \(t=0\) the system is released from rest with \[\theta_1(0)=120^{\circ}, \qquad\theta_2(0)=-10^{\circ}, \qquad\dot{\theta}_1(0)=\dot{\theta}_2(0)=0 .\]Using the exact nonlinear equations of motion (no small-angle or planar-pendulumapproximations) and assuming the rods never stretch or slip, determine the angle\(\theta_2\) at the instant\[t = 10.0~\mathrm{s}.\]Give the result in degrees, in the interval \((-180^{\circ},180^{\circ}]\).

What are the expected readings of the ammeter and voltmeter for the circuit in the figure below? (R = 5.60 Ω, ΔV = 6.30 V) ammeter I =

Answer 2

Question

Chapter 12, Problem 13E

(a)

To determine

The ionic charge for the given element Sulfur (S) .

(a)

Expert Solution

Answer to Problem 13E

The ionic charge for sulfur (S) is 2− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Sulfur belongs to the group 6A. The elements of group 6A have two electrons less than the noble configuration thus tends to gain two electrons and complete their octet.

The elements of group 6A gain two electrons and form an anion with charge 2− .

Conclusion:

Therefore, the ionic charge for sulfur (S) is 2− .

(b)

To determine

The ionic charge for the given element potassium (K) .

(b)

Expert Solution

Answer to Problem 13E

The ionic charge for potassium (K) is 1+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Potassium belongs to the group 1A. The elements of group 1A have one electron more than the noble configuration thus tends to lose one electron and complete their octet.

The elements of group 1A lose one electron and form a cation with charge 1+ .

Conclusion:

Therefore, the ionic charge for potassium (K) is 1+ .

(c)

To determine

The ionic charge for the given element bromine (Br) .

(c)

Expert Solution

Answer to Problem 13E

The ionic charge for bromine (Br) is 1− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Bromine belongs to the group 7A. The elements of group 7A have one electron less than the noble configuration thus tends to gain one electron and complete their octet.

The elements of group 7A gain one electron and form an anion with charge 1− .

Conclusion:

Therefore, the ionic charge for bromine (Br) is 1− .

(d)

To determine

The ionic charge for the given element nitrogen (N) .

(d)

Expert Solution

Answer to Problem 13E

The ionic charge for nitrogen (N) is 3− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Nitrogen belongs to the group 5A. The elements of group 5A have three electrons less than the noble configuration thus tends to gain 3 electrons and complete their octet.

The elements of group 5A gain 3 electrons and form an anion with charge 3− .

Conclusion:

Therefore, the ionic charge for nitrogen (N) is 3− .

(e)

To determine

The ionic charge for the given element magnesium (Mg) .

(e)

Expert Solution

Answer to Problem 13E

The ionic charge for magnesium (Mg) is 2+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Magnesium belongs to the group 2A. The elements of group 2A have two electrons more than the noble configuration thus tends to lose two electrons and complete their octet.

The elements of group 2A lose two electrons and form a cation with charge 2+ .

Conclusion:

Therefore, the ionic charge for magnesium (Mg) is 2+ .

(f)

To determine

The ionic charge for the given element neon (Ne) .

(f)

Expert Solution

Answer to Problem 13E

The ionic charge for neon (Ne) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Neon belongs to the group 8A. The elements of group 8A are called noble gas elements. They have completely filled octet and are very stable. They do not gain or lose electrons because they are already very stable.

Thus, the elements of group 8A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for neon (Ne) is 0 .

(g)

To determine

The ionic charge for the given element carbon (C) .

(g)

Expert Solution

Answer to Problem 13E

The ionic charge for carbon (C) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Carbon belongs to the group 4A. Elements of group 4A have 4 valence electrons and 4 electrons less than noble configuration. Elements of group 4A do not form ions generally because it is very difficult to gain or lose 4 electrons to complete the octet.

Thus, the elements of group 4A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for carbon (C) is 0 .

(h)

To determine

The ionic charge for the given element aluminium (Al) .

(h)

Expert Solution

Answer to Problem 13E

The ionic charge for aluminium (Al) is 3+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Aluminium belongs to the group 3A. The elements of group 3A have three electrons more than the noble configuration thus tends to lose three electrons and complete their octet. The elements of group 3A lose three electrons and form a cation with charge 3+ .

Conclusion:

Therefore, the ionic charge for aluminium (Al) is 3+ .

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Question

Chapter 12, Problem 13E

(a)

To determine

The ionic charge for the given element Sulfur (S) .

(a)

Expert Solution

Answer to Problem 13E

The ionic charge for sulfur (S) is 2− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Sulfur belongs to the group 6A. The elements of group 6A have two electrons less than the noble configuration thus tends to gain two electrons and complete their octet.

The elements of group 6A gain two electrons and form an anion with charge 2− .

Conclusion:

Therefore, the ionic charge for sulfur (S) is 2− .

(b)

To determine

The ionic charge for the given element potassium (K) .

(b)

Expert Solution

Answer to Problem 13E

The ionic charge for potassium (K) is 1+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Potassium belongs to the group 1A. The elements of group 1A have one electron more than the noble configuration thus tends to lose one electron and complete their octet.

The elements of group 1A lose one electron and form a cation with charge 1+ .

Conclusion:

Therefore, the ionic charge for potassium (K) is 1+ .

(c)

To determine

The ionic charge for the given element bromine (Br) .

(c)

Expert Solution

Answer to Problem 13E

The ionic charge for bromine (Br) is 1− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Bromine belongs to the group 7A. The elements of group 7A have one electron less than the noble configuration thus tends to gain one electron and complete their octet.

The elements of group 7A gain one electron and form an anion with charge 1− .

Conclusion:

Therefore, the ionic charge for bromine (Br) is 1− .

(d)

To determine

The ionic charge for the given element nitrogen (N) .

(d)

Expert Solution

Answer to Problem 13E

The ionic charge for nitrogen (N) is 3− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Nitrogen belongs to the group 5A. The elements of group 5A have three electrons less than the noble configuration thus tends to gain 3 electrons and complete their octet.

The elements of group 5A gain 3 electrons and form an anion with charge 3− .

Conclusion:

Therefore, the ionic charge for nitrogen (N) is 3− .

(e)

To determine

The ionic charge for the given element magnesium (Mg) .

(e)

Expert Solution

Answer to Problem 13E

The ionic charge for magnesium (Mg) is 2+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Magnesium belongs to the group 2A. The elements of group 2A have two electrons more than the noble configuration thus tends to lose two electrons and complete their octet.

The elements of group 2A lose two electrons and form a cation with charge 2+ .

Conclusion:

Therefore, the ionic charge for magnesium (Mg) is 2+ .

(f)

To determine

The ionic charge for the given element neon (Ne) .

(f)

Expert Solution

Answer to Problem 13E

The ionic charge for neon (Ne) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Neon belongs to the group 8A. The elements of group 8A are called noble gas elements. They have completely filled octet and are very stable. They do not gain or lose electrons because they are already very stable.

Thus, the elements of group 8A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for neon (Ne) is 0 .

(g)

To determine

The ionic charge for the given element carbon (C) .

(g)

Expert Solution

Answer to Problem 13E

The ionic charge for carbon (C) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Carbon belongs to the group 4A. Elements of group 4A have 4 valence electrons and 4 electrons less than noble configuration. Elements of group 4A do not form ions generally because it is very difficult to gain or lose 4 electrons to complete the octet.

Thus, the elements of group 4A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for carbon (C) is 0 .

(h)

To determine

The ionic charge for the given element aluminium (Al) .

(h)

Expert Solution

Answer to Problem 13E

The ionic charge for aluminium (Al) is 3+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Aluminium belongs to the group 3A. The elements of group 3A have three electrons more than the noble configuration thus tends to lose three electrons and complete their octet. The elements of group 3A lose three electrons and form a cation with charge 3+ .

Conclusion:

Therefore, the ionic charge for aluminium (Al) is 3+ .

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 12, Problem 13E

(a)

To determine

The ionic charge for the given element Sulfur (S) .

(a)

Expert Solution

Answer to Problem 13E

The ionic charge for sulfur (S) is 2− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Sulfur belongs to the group 6A. The elements of group 6A have two electrons less than the noble configuration thus tends to gain two electrons and complete their octet.

The elements of group 6A gain two electrons and form an anion with charge 2− .

Conclusion:

Therefore, the ionic charge for sulfur (S) is 2− .

(b)

To determine

The ionic charge for the given element potassium (K) .

(b)

Expert Solution

Answer to Problem 13E

The ionic charge for potassium (K) is 1+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Potassium belongs to the group 1A. The elements of group 1A have one electron more than the noble configuration thus tends to lose one electron and complete their octet.

The elements of group 1A lose one electron and form a cation with charge 1+ .

Conclusion:

Therefore, the ionic charge for potassium (K) is 1+ .

(c)

To determine

The ionic charge for the given element bromine (Br) .

(c)

Expert Solution

Answer to Problem 13E

The ionic charge for bromine (Br) is 1− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Bromine belongs to the group 7A. The elements of group 7A have one electron less than the noble configuration thus tends to gain one electron and complete their octet.

The elements of group 7A gain one electron and form an anion with charge 1− .

Conclusion:

Therefore, the ionic charge for bromine (Br) is 1− .

(d)

To determine

The ionic charge for the given element nitrogen (N) .

(d)

Expert Solution

Answer to Problem 13E

The ionic charge for nitrogen (N) is 3− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Nitrogen belongs to the group 5A. The elements of group 5A have three electrons less than the noble configuration thus tends to gain 3 electrons and complete their octet.

The elements of group 5A gain 3 electrons and form an anion with charge 3− .

Conclusion:

Therefore, the ionic charge for nitrogen (N) is 3− .

(e)

To determine

The ionic charge for the given element magnesium (Mg) .

(e)

Expert Solution

Answer to Problem 13E

The ionic charge for magnesium (Mg) is 2+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Magnesium belongs to the group 2A. The elements of group 2A have two electrons more than the noble configuration thus tends to lose two electrons and complete their octet.

The elements of group 2A lose two electrons and form a cation with charge 2+ .

Conclusion:

Therefore, the ionic charge for magnesium (Mg) is 2+ .

(f)

To determine

The ionic charge for the given element neon (Ne) .

(f)

Expert Solution

Answer to Problem 13E

The ionic charge for neon (Ne) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Neon belongs to the group 8A. The elements of group 8A are called noble gas elements. They have completely filled octet and are very stable. They do not gain or lose electrons because they are already very stable.

Thus, the elements of group 8A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for neon (Ne) is 0 .

(g)

To determine

The ionic charge for the given element carbon (C) .

(g)

Expert Solution

Answer to Problem 13E

The ionic charge for carbon (C) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Carbon belongs to the group 4A. Elements of group 4A have 4 valence electrons and 4 electrons less than noble configuration. Elements of group 4A do not form ions generally because it is very difficult to gain or lose 4 electrons to complete the octet.

Thus, the elements of group 4A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for carbon (C) is 0 .

(h)

To determine

The ionic charge for the given element aluminium (Al) .

(h)

Expert Solution

Answer to Problem 13E

The ionic charge for aluminium (Al) is 3+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Aluminium belongs to the group 3A. The elements of group 3A have three electrons more than the noble configuration thus tends to lose three electrons and complete their octet. The elements of group 3A lose three electrons and form a cation with charge 3+ .

Conclusion:

Therefore, the ionic charge for aluminium (Al) is 3+ .

Want to see more full solutions like this?

Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 12, Problem 13E

(a)

To determine

The ionic charge for the given element Sulfur (S) .

(a)

Expert Solution

Answer to Problem 13E

The ionic charge for sulfur (S) is 2− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Sulfur belongs to the group 6A. The elements of group 6A have two electrons less than the noble configuration thus tends to gain two electrons and complete their octet.

The elements of group 6A gain two electrons and form an anion with charge 2− .

Conclusion:

Therefore, the ionic charge for sulfur (S) is 2− .

(b)

To determine

The ionic charge for the given element potassium (K) .

(b)

Expert Solution

Answer to Problem 13E

The ionic charge for potassium (K) is 1+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Potassium belongs to the group 1A. The elements of group 1A have one electron more than the noble configuration thus tends to lose one electron and complete their octet.

The elements of group 1A lose one electron and form a cation with charge 1+ .

Conclusion:

Therefore, the ionic charge for potassium (K) is 1+ .

(c)

To determine

The ionic charge for the given element bromine (Br) .

(c)

Expert Solution

Answer to Problem 13E

The ionic charge for bromine (Br) is 1− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Bromine belongs to the group 7A. The elements of group 7A have one electron less than the noble configuration thus tends to gain one electron and complete their octet.

The elements of group 7A gain one electron and form an anion with charge 1− .

Conclusion:

Therefore, the ionic charge for bromine (Br) is 1− .

(d)

To determine

The ionic charge for the given element nitrogen (N) .

(d)

Expert Solution

Answer to Problem 13E

The ionic charge for nitrogen (N) is 3− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Nitrogen belongs to the group 5A. The elements of group 5A have three electrons less than the noble configuration thus tends to gain 3 electrons and complete their octet.

The elements of group 5A gain 3 electrons and form an anion with charge 3− .

Conclusion:

Therefore, the ionic charge for nitrogen (N) is 3− .

(e)

To determine

The ionic charge for the given element magnesium (Mg) .

(e)

Expert Solution

Answer to Problem 13E

The ionic charge for magnesium (Mg) is 2+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Magnesium belongs to the group 2A. The elements of group 2A have two electrons more than the noble configuration thus tends to lose two electrons and complete their octet.

The elements of group 2A lose two electrons and form a cation with charge 2+ .

Conclusion:

Therefore, the ionic charge for magnesium (Mg) is 2+ .

(f)

To determine

The ionic charge for the given element neon (Ne) .

(f)

Expert Solution

Answer to Problem 13E

The ionic charge for neon (Ne) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Neon belongs to the group 8A. The elements of group 8A are called noble gas elements. They have completely filled octet and are very stable. They do not gain or lose electrons because they are already very stable.

Thus, the elements of group 8A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for neon (Ne) is 0 .

(g)

To determine

The ionic charge for the given element carbon (C) .

(g)

Expert Solution

Answer to Problem 13E

The ionic charge for carbon (C) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Carbon belongs to the group 4A. Elements of group 4A have 4 valence electrons and 4 electrons less than noble configuration. Elements of group 4A do not form ions generally because it is very difficult to gain or lose 4 electrons to complete the octet.

Thus, the elements of group 4A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for carbon (C) is 0 .

(h)

To determine

The ionic charge for the given element aluminium (Al) .

(h)

Expert Solution

Answer to Problem 13E

The ionic charge for aluminium (Al) is 3+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Aluminium belongs to the group 3A. The elements of group 3A have three electrons more than the noble configuration thus tends to lose three electrons and complete their octet. The elements of group 3A lose three electrons and form a cation with charge 3+ .

Conclusion:

Therefore, the ionic charge for aluminium (Al) is 3+ .

Answer 6

Chapter 12, Problem 13E

(a)

To determine

The ionic charge for the given element Sulfur (S) .

(a)

Expert Solution

Answer to Problem 13E

The ionic charge for sulfur (S) is 2− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Sulfur belongs to the group 6A. The elements of group 6A have two electrons less than the noble configuration thus tends to gain two electrons and complete their octet.

The elements of group 6A gain two electrons and form an anion with charge 2− .

Conclusion:

Therefore, the ionic charge for sulfur (S) is 2− .

Answer 7

Chapter 12, Problem 13E

(a)

To determine

The ionic charge for the given element Sulfur (S) .

Answer 8

(a)

Expert Solution

Answer to Problem 13E

The ionic charge for sulfur (S) is 2− .

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Sulfur belongs to the group 6A. The elements of group 6A have two electrons less than the noble configuration thus tends to gain two electrons and complete their octet.

The elements of group 6A gain two electrons and form an anion with charge 2− .

Conclusion:

Therefore, the ionic charge for sulfur (S) is 2− .

Answer 13

(b)

To determine

The ionic charge for the given element potassium (K) .

(b)

Expert Solution

Answer to Problem 13E

The ionic charge for potassium (K) is 1+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Potassium belongs to the group 1A. The elements of group 1A have one electron more than the noble configuration thus tends to lose one electron and complete their octet.

The elements of group 1A lose one electron and form a cation with charge 1+ .

Conclusion:

Therefore, the ionic charge for potassium (K) is 1+ .

Answer 14

(b)

To determine

The ionic charge for the given element potassium (K) .

Answer 15

(b)

Expert Solution

Answer to Problem 13E

The ionic charge for potassium (K) is 1+ .

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Potassium belongs to the group 1A. The elements of group 1A have one electron more than the noble configuration thus tends to lose one electron and complete their octet.

The elements of group 1A lose one electron and form a cation with charge 1+ .

Conclusion:

Therefore, the ionic charge for potassium (K) is 1+ .

Answer 20

(c)

To determine

The ionic charge for the given element bromine (Br) .

(c)

Expert Solution

Answer to Problem 13E

The ionic charge for bromine (Br) is 1− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Bromine belongs to the group 7A. The elements of group 7A have one electron less than the noble configuration thus tends to gain one electron and complete their octet.

The elements of group 7A gain one electron and form an anion with charge 1− .

Conclusion:

Therefore, the ionic charge for bromine (Br) is 1− .

Answer 21

(c)

To determine

The ionic charge for the given element bromine (Br) .

Answer 22

(c)

Expert Solution

Answer to Problem 13E

The ionic charge for bromine (Br) is 1− .

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Bromine belongs to the group 7A. The elements of group 7A have one electron less than the noble configuration thus tends to gain one electron and complete their octet.

The elements of group 7A gain one electron and form an anion with charge 1− .

Conclusion:

Therefore, the ionic charge for bromine (Br) is 1− .

Answer 27

(d)

To determine

The ionic charge for the given element nitrogen (N) .

(d)

Expert Solution

Answer to Problem 13E

The ionic charge for nitrogen (N) is 3− .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Nitrogen belongs to the group 5A. The elements of group 5A have three electrons less than the noble configuration thus tends to gain 3 electrons and complete their octet.

The elements of group 5A gain 3 electrons and form an anion with charge 3− .

Conclusion:

Therefore, the ionic charge for nitrogen (N) is 3− .

Answer 28

(d)

To determine

The ionic charge for the given element nitrogen (N) .

Answer 29

(d)

Expert Solution

Answer to Problem 13E

The ionic charge for nitrogen (N) is 3− .

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Nitrogen belongs to the group 5A. The elements of group 5A have three electrons less than the noble configuration thus tends to gain 3 electrons and complete their octet.

The elements of group 5A gain 3 electrons and form an anion with charge 3− .

Conclusion:

Therefore, the ionic charge for nitrogen (N) is 3− .

Answer 34

(e)

To determine

The ionic charge for the given element magnesium (Mg) .

(e)

Expert Solution

Answer to Problem 13E

The ionic charge for magnesium (Mg) is 2+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Magnesium belongs to the group 2A. The elements of group 2A have two electrons more than the noble configuration thus tends to lose two electrons and complete their octet.

The elements of group 2A lose two electrons and form a cation with charge 2+ .

Conclusion:

Therefore, the ionic charge for magnesium (Mg) is 2+ .

Answer 35

(e)

To determine

The ionic charge for the given element magnesium (Mg) .

Answer 36

(e)

Expert Solution

Answer to Problem 13E

The ionic charge for magnesium (Mg) is 2+ .

Answer 37

(e)

Expert Solution

Answer 38

(e)

Expert Solution

Answer 39

Expert Solution

Answer 40

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Magnesium belongs to the group 2A. The elements of group 2A have two electrons more than the noble configuration thus tends to lose two electrons and complete their octet.

The elements of group 2A lose two electrons and form a cation with charge 2+ .

Conclusion:

Therefore, the ionic charge for magnesium (Mg) is 2+ .

Answer 41

(f)

To determine

The ionic charge for the given element neon (Ne) .

(f)

Expert Solution

Answer to Problem 13E

The ionic charge for neon (Ne) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Neon belongs to the group 8A. The elements of group 8A are called noble gas elements. They have completely filled octet and are very stable. They do not gain or lose electrons because they are already very stable.

Thus, the elements of group 8A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for neon (Ne) is 0 .

Answer 42

(f)

To determine

The ionic charge for the given element neon (Ne) .

Answer 43

(f)

Expert Solution

Answer to Problem 13E

The ionic charge for neon (Ne) is 0 .

Answer 44

(f)

Expert Solution

Answer 45

(f)

Expert Solution

Answer 46

Expert Solution

Answer 47

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Neon belongs to the group 8A. The elements of group 8A are called noble gas elements. They have completely filled octet and are very stable. They do not gain or lose electrons because they are already very stable.

Thus, the elements of group 8A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for neon (Ne) is 0 .

Answer 48

(g)

To determine

The ionic charge for the given element carbon (C) .

(g)

Expert Solution

Answer to Problem 13E

The ionic charge for carbon (C) is 0 .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Carbon belongs to the group 4A. Elements of group 4A have 4 valence electrons and 4 electrons less than noble configuration. Elements of group 4A do not form ions generally because it is very difficult to gain or lose 4 electrons to complete the octet.

Thus, the elements of group 4A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for carbon (C) is 0 .

Answer 49

(g)

To determine

The ionic charge for the given element carbon (C) .

Answer 50

(g)

Expert Solution

Answer to Problem 13E

The ionic charge for carbon (C) is 0 .

Answer 51

(g)

Expert Solution

Answer 52

(g)

Expert Solution

Answer 53

Expert Solution

Answer 54

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Carbon belongs to the group 4A. Elements of group 4A have 4 valence electrons and 4 electrons less than noble configuration. Elements of group 4A do not form ions generally because it is very difficult to gain or lose 4 electrons to complete the octet.

Thus, the elements of group 4A have an ionic charge of 0 .

Conclusion:

Therefore, the ionic charge for carbon (C) is 0 .

Answer 55

(h)

To determine

The ionic charge for the given element aluminium (Al) .

(h)

Expert Solution

Answer to Problem 13E

The ionic charge for aluminium (Al) is 3+ .

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Aluminium belongs to the group 3A. The elements of group 3A have three electrons more than the noble configuration thus tends to lose three electrons and complete their octet. The elements of group 3A lose three electrons and form a cation with charge 3+ .

Conclusion:

Therefore, the ionic charge for aluminium (Al) is 3+ .

Answer 56

(h)

To determine

The ionic charge for the given element aluminium (Al) .

Answer 57

(h)

Expert Solution

Answer to Problem 13E

The ionic charge for aluminium (Al) is 3+ .

Answer 58

(h)

Expert Solution

Answer 59

(h)

Expert Solution

Answer 60

Expert Solution

Answer 61

Explanation of Solution

Given Info: Refer to the periodic table figure 11.24.

Explanation:

Aluminium belongs to the group 3A. The elements of group 3A have three electrons more than the noble configuration thus tends to lose three electrons and complete their octet. The elements of group 3A lose three electrons and form a cation with charge 3+ .

Conclusion:

Therefore, the ionic charge for aluminium (Al) is 3+ .