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Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

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BuyFindarrow_forward

Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

Write balanced chemical equations for the reactions forming the following compounds from the elements.

  1. (a) NaBr
  2. (b) CaSe
  3. (c) PbO
  4. (d) AlCl3

(a)

Interpretation Introduction

Interpretation: To write the balanced chemical equation for the formation of NaBr

Concept introduction: Main group elements are categorised as s-block and p-block elements. The s-block elements includes metals belonging to group 1 and group 2 and elements from group 13 to 18 are referred to as p-block elements.The reaction of themetals of main group elements with the non metals forms ionic compounds.

Ionic compounds are formed by the loss of electrons from the metal which are gained by the non metals. The metal gets positively charge and the non metal attains a negative charge thus forming cations and anions respectively. They do so to attain a noble gas configuration or to attain stability.

  MMn++ne

Here, by losing electrons metal M achieve the noble gas configuration. These electrons are gained by the non-metals X as shown below.

    X+neXn

The metals of group 1A form +1 ions because the highest oxidation number is always equal to the group number of that element. Thus, the charge on group 1A elements is +1. Similarly, group 2A elements form +2 ions by losing two electrons and have an oxidation number of +2. The non-metal gains these electrons to form anions with 1 and 2 charge.

The stoichometric coefficents are multiplied with the compounds or species in the chemical equation to have equal number of atoms on both side of the equation. The equation is known as a balanced chemical equation  if there are equal number of atoms of each element in both the product and reactant side.

For the naming of an ionic compound, the cation is always named first followed by the anion and the anion ends with the “-ide”.

Explanation

Sodium belongs to group 1A of periodic table and has oxidation number of +1. Thus, it loses one electron to attain noble gas configuration.

    NaNa++e

This electron is gained by bromine to form anion with one negative charge. Bromine belongs to halogen family and it has the oxidation number of 1.

    Br2+e_2Br

The number of electrons in both the equations are same. Thus an ionic compound is formed in which Sodium has +1 charge and bromine bears 1 charge

(b)

Interpretation Introduction

Interpretation: The balanced chemical equation for the formation of CaSe should be written. 

Concept introduction: Main group elements are categorised as s-block and p-block elements. The s-block elements includes metals belonging to group 1 and group 2 and elements from group 13 to 18 are referred to as p-block elements.The reaction of themetals of main group elements with the non metals forms ionic compounds.

Ionic compounds are formed by the loss of electrons from the metal which are gained by the non metals. The metal gets positively charge and the non metal attains a negative charge thus forming cations and anions respectively. They do so to attain a noble gas configuration or to attain stability.

  MMn++ne

Here, by losing electrons metal M achieve the noble gas configuration. These electrons are gained by the non-metals X as shown below.

    X+neXn

The metals of group 1A form +1 ions because the highest oxidation number is always equal to the group number of that element. Thus, the charge on group 1A elements is +1. Similarly, group 2A elements form +2 ions by losing two electrons and have an oxidation number of +2. The non-metal gains these electrons to form anions with 1 and 2 charge.

The stoichometric coefficents are multiplied with the compounds or species in the chemical equation to have equal number of atoms on both side of the equation. The equation is known as a balanced chemical equation  if there are equal number of atoms of each element in both the product and reactant side.

For the naming of an ionic compound, the cation is always named first followed by the anion and the anion ends with the “-ide”.

(c)

Interpretation Introduction

Interpretation: The balanced chemical equation for the formation of PbO should be written. 

Concept introduction: Main group elements are categorised as s-block and p-block elements. The s-block elements includes metals belonging to group 1 and group 2 and elements from group 13 to 18 are referred to as p-block elements.The reaction of themetals of main group elements with the non metals forms ionic compounds.

Ionic compounds are formed by the loss of electrons from the metal which are gained by the non metals. The metal gets positively charge and the non metal attains a negative charge thus forming cations and anions respectively. They do so to attain a noble gas configuration or to attain stability.

  MMn++ne

Here, by losing electrons metal M achieve the noble gas configuration. These electrons are gained by the non-metals X as shown below.

    X+neXn

The metals of group 1A form +1 ions because the highest oxidation number is always equal to the group number of that element. Thus, the charge on group 1A elements is +1. Similarly, group 2A elements form +2 ions by losing two electrons and have an oxidation number of +2. The non-metal gains these electrons to form anions with 1 and 2 charge.

The stoichometric coefficents are multiplied with the compounds or species in the chemical equation to have equal number of atoms on both side of the equation. The equation is known as a balanced chemical equation  if there are equal number of atoms of each element in both the product and reactant side.

For the naming of an ionic compound, the cation is always named first followed by the anion and the anion ends with the “-ide”.

(d)

Interpretation Introduction

Interpretation: The balanced chemical equation for the formation of AlCl3 should be written. 

Concept introduction: Main group elements are categorised as s-block and p-block elements. The s-block elements includes metals belonging to group 1 and group 2 and elements from group 13 to 18 are referred to as p-block elements.The reaction of themetals of main group elements with the non metals forms ionic compounds.

Ionic compounds are formed by the loss of electrons from the metal which are gained by the non metals. The metal gets positively charge and the non metal attains a negative charge thus forming cations and anions respectively. They do so to attain a noble gas configuration or to attain stability.

  MMn++ne

Here, by losing electrons metal M achieve the noble gas configuration. These electrons are gained by the non-metals X as shown below.

    X+neXn

The metals of group 1A form +1 ions because the highest oxidation number is always equal to the group number of that element. Thus, the charge on group 1A elements is +1. Similarly, group 2A elements form +2 ions by losing two electrons and have an oxidation number of +2. The non-metal gains these electrons to form anions with 1 and 2 charge.

The stoichometric coefficents are multiplied with the compounds or species in the chemical equation to have equal number of atoms on both side of the equation. The equation is known as a balanced chemical equation  if there are equal number of atoms of each element in both the product and reactant side.

For the naming of an ionic compound, the cation is always named first followed by the anion and the anion ends with the “-ide”.

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Chapter 21 Solutions

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Sect-21.11 P-2.4ACPSect-21.11 P-2.5ACPCh-21 P-1PSCh-21 P-2PSCh-21 P-3PSCh-21 P-4PSCh-21 P-5PSCh-21 P-6PSCh-21 P-7PSCh-21 P-8PSCh-21 P-9PSCh-21 P-10PSCh-21 P-11PSCh-21 P-12PSCh-21 P-13PSCh-21 P-14PSCh-21 P-15PSCh-21 P-16PSCh-21 P-17PSCh-21 P-18PSCh-21 P-19PSCh-21 P-20PSCh-21 P-21PSCh-21 P-22PSCh-21 P-23PSCh-21 P-24PSCh-21 P-25PSCh-21 P-26PSCh-21 P-27PSCh-21 P-28PSCh-21 P-29PSCh-21 P-30PSCh-21 P-31PSCh-21 P-32PSCh-21 P-33PSCh-21 P-34PSCh-21 P-35PSCh-21 P-36PSCh-21 P-37PSCh-21 P-38PSCh-21 P-39PSCh-21 P-40PSCh-21 P-41PSCh-21 P-42PSCh-21 P-43PSCh-21 P-44PSCh-21 P-45PSCh-21 P-46PSCh-21 P-47PSCh-21 P-48PSCh-21 P-49PSCh-21 P-50PSCh-21 P-51PSCh-21 P-52PSCh-21 P-53PSCh-21 P-54PSCh-21 P-55PSCh-21 P-56PSCh-21 P-57PSCh-21 P-58PSCh-21 P-59PSCh-21 P-60PSCh-21 P-61PSCh-21 P-62PSCh-21 P-63PSCh-21 P-64PSCh-21 P-65PSCh-21 P-66PSCh-21 P-67PSCh-21 P-68PSCh-21 P-69PSCh-21 P-70PSCh-21 P-71PSCh-21 P-72PSCh-21 P-73PSCh-21 P-74PSCh-21 P-75PSCh-21 P-76PSCh-21 P-77PSCh-21 P-78PSCh-21 P-79PSCh-21 P-80PSCh-21 P-81PSCh-21 P-82PSCh-21 P-83PSCh-21 P-84PSCh-21 P-85PSCh-21 P-86PSCh-21 P-87PSCh-21 P-88PSCh-21 P-89GQCh-21 P-90GQCh-21 P-91GQCh-21 P-92GQCh-21 P-93GQCh-21 P-94GQCh-21 P-95GQCh-21 P-96GQCh-21 P-97GQCh-21 P-98GQCh-21 P-99GQCh-21 P-100GQCh-21 P-101GQCh-21 P-102GQCh-21 P-103GQCh-21 P-105GQCh-21 P-106GQCh-21 P-107GQCh-21 P-108GQCh-21 P-110GQCh-21 P-111GQCh-21 P-112GQCh-21 P-113GQCh-21 P-114GQCh-21 P-115ILCh-21 P-116ILCh-21 P-117ILCh-21 P-118ILCh-21 P-119ILCh-21 P-120ILCh-21 P-121SCQCh-21 P-122SCQCh-21 P-123SCQCh-21 P-124SCQCh-21 P-125SCQCh-21 P-126SCQCh-21 P-127SCQCh-21 P-128SCQCh-21 P-129SCQCh-21 P-130SCQCh-21 P-131SCQ

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