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Section
           Name                                             Date


           Atomic Theory and Bonding
                                                                                            4.1
                                                                                           Summary
           Textbook pages 168–183

           Before You Read
           What do you already know about Bohr diagrams? Record your answer in the lines
           below.




                                                                              ◆
           What are atoms?
           An atom is the smallest particle of any element that retains
                                                                              ✏       Mark the Text

           the properties of the element.                                        Identify Definitions
              The particles that make up an atom are called subatomic            Highlight the definition of
           particles. Atoms are composed of three subatomic particles:           each word that appears in
           protons, neutrons, and electrons. ●
                                             ✔                                   bold type.

                                                                              ●
                                                                              ✔     Reading Check
                                                                                   Which has a positive elec-
                                                                                   tric charge, a proton, a
                                                                                   neutron, or an electron?




               Nuclear charge is the electric charge on the nucleus. This
           charge is always positive, since the protons have a positive
           charge and the neutrons are not charged. Atomic number is
           the number of protons. The nuclear charge or atomic number
           is given in the top left hand corner of the element box for
           each element in the periodic table.




           How does the periodic table provide information
           about elements?
           In the periodic table, each element is listed according to its
           atomic number. Each row is called a period. Each column

           56       MHR • Section 4.1   Atomic Theory and Bonding           © 2008 McGraw-Hill Ryerson Limited




056_080_BCSci10_U2CH04_098461.in56 56                                                      PDF Pass              7/21/08 8:11:14 PM
Section
                   Name                                                Date
                                                                                                                 4.1
                                                                                                                 Summary

                                                                                                                 continued
                                                        is called a group or family. Metals are on the left side and
                                                        in the middle of the table. Non-metals are in the upper right
                                                        corner. The metalloids form a staircase toward the right side.
                                                        The block of elements from groups 3 through 12 are the
                                                        transition metals. Elements in the same chemical group or
                                                        family have similar chemical properties. For example, group
                                                        17 contains very reactive non-metals known as halogens (i.e.,
                                                        fluorine, chlorine, bromine, etc.) Group 18 contains the
                                                        non-reactive noble gases.

                                                        How do Bohr diagrams represent atoms?
                                                        A Bohr diagram shows the arrangement of subatomic
                                                        particles in atoms and ions. Electrons are organized in
                                                        “shells”. The first shell holds a maximum of two electrons;
                                                        the second shell a maximum of eight. When this shell
                                                        is filled, it is called a stable octet. The outermost shell
                                                        containing electrons is called the valence shell. The electrons
                                                        in this shell are called valence electrons. These electrons
                                                        are involved in chemical bonding. When an atom forms a
                                                        compound, it acquires a full valence shell of electrons and
                                                        achieves a stable, low energy state. On the periodic table,
                                                        elements in Group 1 have 1 electron in their valence shell,
                                                        elements in Group 2 have 2 (a lone pair), elements in Group
                                                        3 have 3, and so on.



                                                                                  19p
                                                                                  20n




                                                                 The Bohr diagram for a potassium atom

                                                        What are ionic and covalent compounds?
                                                        There are two basic types of compounds: ionic and covalent.
                                                        1. Ionic compounds: When atoms gain or lose electrons, they
                                                           become electrically charged particles called ions. An ionic
                                                           compound contains a positive ion (usually a metal) and a
                                                           negative ion (usually a non-metal). In ionic bonding, one
                                                           or more electrons transfer from each atom of the metal

                   © 2008 McGraw-Hill Ryerson Limited                    Section 4.1    Atomic Theory and Bonding • MHR      57




056_080_BCSci10_U2CH04_098461.in57 57                                                                          PDF Pass      7/21/08 8:11:50 PM
Section
           Name                                                                Date
                                                                                                                                      4.1
                                                                                                                                      Summary

                                                                                                                                      continued
                to each atom of the non-metal. The metal atoms lose
                electrons, forming cations. For example, aluminum forms
                a 3+ cation as a result of losing three electrons. Some
                metals are multivalent and can form ions in several
                ways, depending on the chemical reaction they undergo.
                For example, iron is multivalent because it can lose two
                or three electrons to become a Fe2+ or Fe3+ ion. The non-
                metal atoms gain electrons, forming anions. Chlorine
                gains one electron and forms a 1- anion.
           The common ions are sometimes shown in the upper right-
           hand corner of the element’s box in the periodic table. For a
           multivalent metal, the most common charge is listed first.




           2. Covalent compounds: In covalent bonding, the atoms of
              a non-metal share electrons with other non-metal atoms.
              An unpaired electron from each atom will pair together,
              forming a covalent bond. These two electrons are
              sometimes called a bonding pair.
                                 ؉1                                ؊1



                    Na                         Cl                                   H             F
                                                                                                                    ●
                                                                                                                    ✔     Reading Check
                                                                                                                         What is a Lewis diagram?


                   The ionic compound sodium chloride                   The covalent compound hydrogen fluoride


           What is a Lewis diagram?
           A Lewis diagram illustrates chemical bonding by showing
           only an atom’s valence electrons and its chemical symbol.
           Lewis diagrams can be used to represent elements, ions, and
           compounds. ●✔

                                                             ؊                      2+       2؊
                                        H               Cl                     Mg        O
                              hydrogen atom         chlorine ion         magnesium oxide molecule




           58       MHR • Section 4.1         Atomic Theory and Bonding                                           © 2008 McGraw-Hill Ryerson Limited




056_080_BCSci10_U2CH04_098461.in58 58                                                                                           PDF Pass               7/21/08 8:12:46 PM
Section
                   Name                                 Date
                                                                                                 4.1
                                                                                                 Summary

                                                                                                 continued




                   © 2008 McGraw-Hill Ryerson Limited     Section 4.1   Atomic Theory and Bonding • MHR      59




056_080_BCSci10_U2CH04_098461.in59 59                                                          PDF Pass      7/21/08 8:13:26 PM
Name                                                    Date                             Comprehension
                                                                                                      Section 4.1
           Use with textbook pages 168–180.

           The atom and the subatomic particles
             1. Use the following vocabulary words to label the diagram.
            Vocabulary
            common ion charge                                        symbol
            other ion charge                                         atomic number
               ,
            name                                                     average atomic mass

                                                        (e)
           (a)
                                                        (f)
           (b)
           (c)
           (d)

             2. Examine the periodic table for the element below and complete the blanks.




                 (a) atomic number                            (b) average atomic mass
                 (c) ion charge                               (d) number of protons
                 (e) name of element                          (f) number of neutrons
             3. Complete the following table for the different atoms and ions. The first two rows have
                been completed to help you.
                   Element Name         Atomic Number     Ion Charge         Number of       Number of         Number of
                                                                              Protons        Electrons          Neutrons
                      potassium              19               1+                 19               18                20
                     phosphorus              15                0                 15               15                16
                                              3                0
                                                              2+                 20
                       nitrogen                               3–
                                              5                0
                         argon                                                                    18
                                             13                                                   10
                        chlorine                               0
                                                                                 11               10


           60       MHR • Section 4.1       Atomic Theory and Bonding                      © 2008 McGraw-Hill Ryerson Limited




056_080_BCSci10_U2CH04_098461.in60 60                                                                    PDF Pass               7/11/08 5:25:27 PM
Applying
                   Name                                                    Date                                  Knowledge
                                                                                                                 Section 4.1
                   Use with textbook pages 174–177.

                   Bohr diagrams
                    1. Define the following terms:
                        (a) Bohr diagram
                        (b) stable octet
                        (c) valence shell
                        (d) valence electrons
                    2. Complete the following table.

                          Atom/Ion         Atomic              Number of       Number of        Number of        Number of
                                           Number              Protons         Electrons        Neutrons         Electron Shells
                          neon atom

                          fluorine atom

                          fluorine ion

                          sodium atom

                          sodium ion



                    3. Use the table above to draw the Bohr model diagram for each of the following atoms
                       and ions.

                          neon atom           fluorine atom        fluorine ion             sodium atom         sodium ion




                    4. Draw the Bohr model diagram for each of the following compounds.

                          carbon dioxide (CO2)                ammonia (NH3)                       calcium chloride (CaCl2)




                   © 2008 McGraw-Hill Ryerson Limited                         Section 4.1    Atomic Theory and Bonding • MHR       61




056_080_BCSci10_U2CH04_098461.in61 61                                                                                 PDF Pass     7/11/08 5:25:30 PM
Illustrating
           Name                                                 Date                                Concepts
                                                                                                   Section 4.1
           Use with textbook pages 176–180.

           Lewis diagrams
             1. Define the following terms:
                (a) Lewis diagram
                (b) lone pair
                (c) bonding pair

             2. Draw Lewis diagrams for each of the following elements.
                (a) boron               (b) nitrogen               (c) aluminium            (d) chlorine




             3. Draw Lewis diagrams for each of the following ionic compounds.
                (a) sodium oxide                       (b) potassium chloride        (c) magnesium bromide




             4. Draw Lewis diagrams for each of the following covalent compounds.
                (a) carbon dioxide, CO2 (b) phosphorus trifluoride, PF3            (c) silicon tetrachloride, SiCl4




             5. Draw Lewis diagrams for each of the following diatomic molecules.
                (a) chlorine, Cl2                         (b) nitrogen, N2            (c) hydrogen, H2




           62       MHR • Section 4.1      Atomic Theory and Bonding                   © 2008 McGraw-Hill Ryerson Limited




056_080_BCSci10_U2CH04_098461.in62 62                                                                PDF Pass               7/11/08 5:25:31 PM
Assessment
                   Name                                                            Date
                                                                                                                        Section 4.1

                   Use with textbook pages 168–180.                                        8. Which of the following are responsible for
                                                                                              bonding?
                   Atomic theory and                                                         A. nuclei
                   bonding                                                                   B. protons
                         Match the Term on the left with the best                            C. neutrons
                      Descriptor on the right. Each Descriptor may be
                                      used only once.                                        D. electrons
                    Term                   Descriptor                                     Use the following diagram of an atom to
                    1.             shell   A. a horizontal row on the periodic            answer questions 9 to 11.
                    2.                        table
                         period            B. a vertical column on the periodic                                                    (a)
                    3.                        table
                         family            C. an area around the nucleus where
                    4.             ionic      electrons exist                                                                      (b)

                         bonding           D. chemical bonding that results from                                                   (c)
                    5.                        a sharing of valence electrons
                         covalent          E. chemical bonding that results                                                        (d)
                         bonding              when one or more electrons
                                              transfers from each atom of a                                                        (e)
                                              metal to each atom of a non-metal
                    6. Which of the following is the smallest
                       particle of an element that can exist by                            9. Which labelled part in the diagram
                       itself?                                                                represents a neutron?
                         A. ion                                                              A. (a)
                         B. atom                                                             B. (b)
                         C. molecule                                                         C. (c)
                         D. compound                                                         D. (d)
                    7. Which of the following correctly matches                           10. What is the number of subatomic particle
                       the subatomic particle with its charge and                             (c) equivalent to?
                       location in an atom?
                                                                                             A. atomic number
                                    Subatomic       Location         Charge                  B. mass number – atomic number
                                     Particle
                                                                                             C. mass number + atomic number
                          A.          proton         nucleus         neutral                 D. number of electrons + number of protons
                          B.         neutron         nucleus         positive             11. How many valence electrons are there in
                                                                                              this atom?
                          C.         electron           shell        positive                A. 2
                                                                                             B. 4
                          D.         electron           shell       negative                 C. 6
                                                                                             D. 7

                   © 2008 McGraw-Hill Ryerson Limited                                Section 4.1      Atomic Theory and Bonding • MHR    63




056_080_BCSci10_U2CH04_098461.in63 63                                                                                        PDF Pass    7/11/08 5:25:32 PM
Assessment
           Name                                                          Date
                                                                                                                  Section 4.1

           12. Which of the following describes                                 Use the following Lewis diagrams of four
               structure (e)?                                                   hypothetical elements to answer
                                                                                question 15.
                              CHARGE         SUBATOMIC PARTICLE(S)                         Ma        Di       So        Nh
                                             PRESENT
                  A.          neutral        electrons and neutrons             15. Which of the hypothetical elements shown
                                                                                    above represents a metal?
                  B.          positive       protons and neutrons
                                                                                   A. Ma
                  C.          positive       protons and electrons                 B. Di
                  D.          negative       electrons                             C. So
                                                                                   D. Nh
           13. Which of the following describes a cation?
                                                                                Use the following Bohr model of an element
                  I.                                 2+
                                examples include Ca and Al   3+                 to answer question 16.
                  II.           a metal atom that has lost electrons
                  III.          has equal numbers of electrons and                               11p
                                                                                                             2e    8e
                                protons                                                          12n

                 A. I and II only
                                                                                16. Which of the following does the Bohr
                 B. I and III only                                                  model represent?
                 C. II and III only                                                A. a neon atom
                 D. I, II, and III                                                 B. a sodium ion
           14. Which row of the table is completed                                 C. a sodium atom
               correctly for an atom of potassium?
                                                                                   D. a fluorine atom
                  Atomic           Mass      Number       Number        Number
                  Number          Number        of           of            of
                                             Protons      Neutrons     Electrons

            A.           19          39         19          20            19
            B.           19          39         39          20            20
            C.           19          39         20          20            19
            D.           39          19         19          19            20




           64           MHR • Section 4.1      Atomic Theory and Bonding                             © 2008 McGraw-Hill Ryerson Limited




056_080_BCSci10_U2CH04_098461.in64 64                                                                               PDF Pass              7/11/08 5:25:33 PM

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Chem

  • 1. Section Name Date Atomic Theory and Bonding 4.1 Summary Textbook pages 168–183 Before You Read What do you already know about Bohr diagrams? Record your answer in the lines below. ◆ What are atoms? An atom is the smallest particle of any element that retains ✏ Mark the Text the properties of the element. Identify Definitions The particles that make up an atom are called subatomic Highlight the definition of particles. Atoms are composed of three subatomic particles: each word that appears in protons, neutrons, and electrons. ● ✔ bold type. ● ✔ Reading Check Which has a positive elec- tric charge, a proton, a neutron, or an electron? Nuclear charge is the electric charge on the nucleus. This charge is always positive, since the protons have a positive charge and the neutrons are not charged. Atomic number is the number of protons. The nuclear charge or atomic number is given in the top left hand corner of the element box for each element in the periodic table. How does the periodic table provide information about elements? In the periodic table, each element is listed according to its atomic number. Each row is called a period. Each column 56 MHR • Section 4.1 Atomic Theory and Bonding © 2008 McGraw-Hill Ryerson Limited 056_080_BCSci10_U2CH04_098461.in56 56 PDF Pass 7/21/08 8:11:14 PM
  • 2. Section Name Date 4.1 Summary continued is called a group or family. Metals are on the left side and in the middle of the table. Non-metals are in the upper right corner. The metalloids form a staircase toward the right side. The block of elements from groups 3 through 12 are the transition metals. Elements in the same chemical group or family have similar chemical properties. For example, group 17 contains very reactive non-metals known as halogens (i.e., fluorine, chlorine, bromine, etc.) Group 18 contains the non-reactive noble gases. How do Bohr diagrams represent atoms? A Bohr diagram shows the arrangement of subatomic particles in atoms and ions. Electrons are organized in “shells”. The first shell holds a maximum of two electrons; the second shell a maximum of eight. When this shell is filled, it is called a stable octet. The outermost shell containing electrons is called the valence shell. The electrons in this shell are called valence electrons. These electrons are involved in chemical bonding. When an atom forms a compound, it acquires a full valence shell of electrons and achieves a stable, low energy state. On the periodic table, elements in Group 1 have 1 electron in their valence shell, elements in Group 2 have 2 (a lone pair), elements in Group 3 have 3, and so on. 19p 20n The Bohr diagram for a potassium atom What are ionic and covalent compounds? There are two basic types of compounds: ionic and covalent. 1. Ionic compounds: When atoms gain or lose electrons, they become electrically charged particles called ions. An ionic compound contains a positive ion (usually a metal) and a negative ion (usually a non-metal). In ionic bonding, one or more electrons transfer from each atom of the metal © 2008 McGraw-Hill Ryerson Limited Section 4.1 Atomic Theory and Bonding • MHR 57 056_080_BCSci10_U2CH04_098461.in57 57 PDF Pass 7/21/08 8:11:50 PM
  • 3. Section Name Date 4.1 Summary continued to each atom of the non-metal. The metal atoms lose electrons, forming cations. For example, aluminum forms a 3+ cation as a result of losing three electrons. Some metals are multivalent and can form ions in several ways, depending on the chemical reaction they undergo. For example, iron is multivalent because it can lose two or three electrons to become a Fe2+ or Fe3+ ion. The non- metal atoms gain electrons, forming anions. Chlorine gains one electron and forms a 1- anion. The common ions are sometimes shown in the upper right- hand corner of the element’s box in the periodic table. For a multivalent metal, the most common charge is listed first. 2. Covalent compounds: In covalent bonding, the atoms of a non-metal share electrons with other non-metal atoms. An unpaired electron from each atom will pair together, forming a covalent bond. These two electrons are sometimes called a bonding pair. ؉1 ؊1 Na Cl H F ● ✔ Reading Check What is a Lewis diagram? The ionic compound sodium chloride The covalent compound hydrogen fluoride What is a Lewis diagram? A Lewis diagram illustrates chemical bonding by showing only an atom’s valence electrons and its chemical symbol. Lewis diagrams can be used to represent elements, ions, and compounds. ●✔ ؊ 2+ 2؊ H Cl Mg O hydrogen atom chlorine ion magnesium oxide molecule 58 MHR • Section 4.1 Atomic Theory and Bonding © 2008 McGraw-Hill Ryerson Limited 056_080_BCSci10_U2CH04_098461.in58 58 PDF Pass 7/21/08 8:12:46 PM
  • 4. Section Name Date 4.1 Summary continued © 2008 McGraw-Hill Ryerson Limited Section 4.1 Atomic Theory and Bonding • MHR 59 056_080_BCSci10_U2CH04_098461.in59 59 PDF Pass 7/21/08 8:13:26 PM
  • 5. Name Date Comprehension Section 4.1 Use with textbook pages 168–180. The atom and the subatomic particles 1. Use the following vocabulary words to label the diagram. Vocabulary common ion charge symbol other ion charge atomic number , name average atomic mass (e) (a) (f) (b) (c) (d) 2. Examine the periodic table for the element below and complete the blanks. (a) atomic number (b) average atomic mass (c) ion charge (d) number of protons (e) name of element (f) number of neutrons 3. Complete the following table for the different atoms and ions. The first two rows have been completed to help you. Element Name Atomic Number Ion Charge Number of Number of Number of Protons Electrons Neutrons potassium 19 1+ 19 18 20 phosphorus 15 0 15 15 16 3 0 2+ 20 nitrogen 3– 5 0 argon 18 13 10 chlorine 0 11 10 60 MHR • Section 4.1 Atomic Theory and Bonding © 2008 McGraw-Hill Ryerson Limited 056_080_BCSci10_U2CH04_098461.in60 60 PDF Pass 7/11/08 5:25:27 PM
  • 6. Applying Name Date Knowledge Section 4.1 Use with textbook pages 174–177. Bohr diagrams 1. Define the following terms: (a) Bohr diagram (b) stable octet (c) valence shell (d) valence electrons 2. Complete the following table. Atom/Ion Atomic Number of Number of Number of Number of Number Protons Electrons Neutrons Electron Shells neon atom fluorine atom fluorine ion sodium atom sodium ion 3. Use the table above to draw the Bohr model diagram for each of the following atoms and ions. neon atom fluorine atom fluorine ion sodium atom sodium ion 4. Draw the Bohr model diagram for each of the following compounds. carbon dioxide (CO2) ammonia (NH3) calcium chloride (CaCl2) © 2008 McGraw-Hill Ryerson Limited Section 4.1 Atomic Theory and Bonding • MHR 61 056_080_BCSci10_U2CH04_098461.in61 61 PDF Pass 7/11/08 5:25:30 PM
  • 7. Illustrating Name Date Concepts Section 4.1 Use with textbook pages 176–180. Lewis diagrams 1. Define the following terms: (a) Lewis diagram (b) lone pair (c) bonding pair 2. Draw Lewis diagrams for each of the following elements. (a) boron (b) nitrogen (c) aluminium (d) chlorine 3. Draw Lewis diagrams for each of the following ionic compounds. (a) sodium oxide (b) potassium chloride (c) magnesium bromide 4. Draw Lewis diagrams for each of the following covalent compounds. (a) carbon dioxide, CO2 (b) phosphorus trifluoride, PF3 (c) silicon tetrachloride, SiCl4 5. Draw Lewis diagrams for each of the following diatomic molecules. (a) chlorine, Cl2 (b) nitrogen, N2 (c) hydrogen, H2 62 MHR • Section 4.1 Atomic Theory and Bonding © 2008 McGraw-Hill Ryerson Limited 056_080_BCSci10_U2CH04_098461.in62 62 PDF Pass 7/11/08 5:25:31 PM
  • 8. Assessment Name Date Section 4.1 Use with textbook pages 168–180. 8. Which of the following are responsible for bonding? Atomic theory and A. nuclei bonding B. protons Match the Term on the left with the best C. neutrons Descriptor on the right. Each Descriptor may be used only once. D. electrons Term Descriptor Use the following diagram of an atom to 1. shell A. a horizontal row on the periodic answer questions 9 to 11. 2. table period B. a vertical column on the periodic (a) 3. table family C. an area around the nucleus where 4. ionic electrons exist (b) bonding D. chemical bonding that results from (c) 5. a sharing of valence electrons covalent E. chemical bonding that results (d) bonding when one or more electrons transfers from each atom of a (e) metal to each atom of a non-metal 6. Which of the following is the smallest particle of an element that can exist by 9. Which labelled part in the diagram itself? represents a neutron? A. ion A. (a) B. atom B. (b) C. molecule C. (c) D. compound D. (d) 7. Which of the following correctly matches 10. What is the number of subatomic particle the subatomic particle with its charge and (c) equivalent to? location in an atom? A. atomic number Subatomic Location Charge B. mass number – atomic number Particle C. mass number + atomic number A. proton nucleus neutral D. number of electrons + number of protons B. neutron nucleus positive 11. How many valence electrons are there in this atom? C. electron shell positive A. 2 B. 4 D. electron shell negative C. 6 D. 7 © 2008 McGraw-Hill Ryerson Limited Section 4.1 Atomic Theory and Bonding • MHR 63 056_080_BCSci10_U2CH04_098461.in63 63 PDF Pass 7/11/08 5:25:32 PM
  • 9. Assessment Name Date Section 4.1 12. Which of the following describes Use the following Lewis diagrams of four structure (e)? hypothetical elements to answer question 15. CHARGE SUBATOMIC PARTICLE(S) Ma Di So Nh PRESENT A. neutral electrons and neutrons 15. Which of the hypothetical elements shown above represents a metal? B. positive protons and neutrons A. Ma C. positive protons and electrons B. Di D. negative electrons C. So D. Nh 13. Which of the following describes a cation? Use the following Bohr model of an element I. 2+ examples include Ca and Al 3+ to answer question 16. II. a metal atom that has lost electrons III. has equal numbers of electrons and 11p 2e 8e protons 12n A. I and II only 16. Which of the following does the Bohr B. I and III only model represent? C. II and III only A. a neon atom D. I, II, and III B. a sodium ion 14. Which row of the table is completed C. a sodium atom correctly for an atom of potassium? D. a fluorine atom Atomic Mass Number Number Number Number Number of of of Protons Neutrons Electrons A. 19 39 19 20 19 B. 19 39 39 20 20 C. 19 39 20 20 19 D. 39 19 19 19 20 64 MHR • Section 4.1 Atomic Theory and Bonding © 2008 McGraw-Hill Ryerson Limited 056_080_BCSci10_U2CH04_098461.in64 64 PDF Pass 7/11/08 5:25:33 PM