Atomic Theory and Bonding
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1 Atomic Theory and Bonding Textbook pages Section 4.1 Summary 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 the properties of the element. The particles that make up an atom are called subatomic particles. Atoms are composed of three subatomic particles: protons, neutrons, and electrons. Mark the Text Identify Definitions Highlight the definition of each word that appears in bold type. Reading Check Which has a positive electric 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 Atomic Theory and Bonding 2008 McGraw-Hill Ryerson Limited
2 Section 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 Atomic Theory and Bonding MHR 57
3 Section 4.1 Summary 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 Fe 2+ or Fe 3+ ion. The nonmetal atoms gain electrons, forming anions. Chlorine gains one electron and forms a 1 - anion. The common ions are sometimes shown in the upper righthand corner of the element s box in the periodic table. For a multivalent metal, the most common charge is listed first. continued 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 Na Cl H F 1 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. H hydrogen atom Cl chlorine ion Mg 2+ O 2 magnesium oxide molecule 58 MHR Atomic Theory and Bonding 2008 McGraw-Hill Ryerson Limited
4 Section 4.1 Summary continued 2008 McGraw-Hill Ryerson Limited Atomic Theory and Bonding MHR 59
5 Comprehension Use with textbook pages The atom and the subatomic particles 1. Use the following vocabulary words to label the diagram. Vocabulary common ion charge other ion charge name, symbol atomic number average atomic mass (a) (b) (c) (d) (e) (f) 2. Examine the periodic table for the element below and complete the blanks. (a) atomic number (c) ion charge (e) name of element (b) average atomic mass (d) number of protons (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 Ion Charge Protons Electrons Neutrons potassium phosphorus nitrogen argon chlorine MHR Atomic Theory and Bonding 2008 McGraw-Hill Ryerson Limited
6 Use with textbook pages Bohr diagrams 1. Define the following terms: (a) Bohr diagram (b) stable octet (c) valence shell (d) valence electrons 2. Complete the following table. Applying Knowledge Atom/Ion neon atom Atomic Protons Electrons Neutrons Electron Shells 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 (CO 2 ) ammonia (NH 3 ) calcium chloride (CaCl 2 ) 2008 McGraw-Hill Ryerson Limited Atomic Theory and Bonding MHR 61
7 Use with textbook pages Lewis diagrams 1. Define the following terms: (a) Lewis diagram (b) lone pair (c) bonding pair Illustrating Concepts 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, CO 2 (b) phosphorus trifluoride, PF 3 (c) silicon tetrachloride, SiCl 4 5. Draw Lewis diagrams for each of the following diatomic molecules. (a) chlorine, Cl 2 (b) nitrogen, N 2 (c) hydrogen, H 2 62 MHR Atomic Theory and Bonding 2008 McGraw-Hill Ryerson Limited
8 Assessment Use with textbook pages Atomic theory and bonding Match the Term on the left with the best Descriptor on the right. Each Descriptor may be used only once. Term Descriptor 1. shell 2. period 3. family 4. ionic bonding 5. covalent bonding A. a horizontal row on the periodic table B. a vertical column on the periodic table C. an area around the nucleus where electrons exist D. chemical bonding that results from a sharing of valence electrons E. chemical bonding that results when one or more electrons transfers from each atom of a metal to each atom of a non-metal 6. Which of the following is the smallest particle of an element that can exist by itself? A. ion B. atom C. molecule D. compound 7. Which of the following correctly matches the subatomic particle with its charge and location in an atom? Subatomic Particle Location Charge A. proton nucleus neutral B. neutron nucleus positive C. electron shell positive D. electron shell negative 8. Which of the following are responsible for bonding? A. nuclei B. protons C. neutrons D. electrons Use the following diagram of an atom to answer questions 9 to Which labelled part in the diagram represents a neutron? A. (a) B. (b) C. (c) D. (d) 10. What is the number of subatomic particle (c) equivalent to? A. atomic number B. mass number atomic number C. mass number + atomic number D. number of electrons + number of protons 11. How many valence electrons are there in this atom? A. 2 B. 4 C. 6 D. 7 (a) (b) (c) (d) (e) 2008 McGraw-Hill Ryerson Limited Atomic Theory and Bonding MHR 63
9 Assessment 12. Which of the following describes structure (e)? CHARGE SUBATOMIC PARTICLE(S) PRESENT A. neutral electrons and neutrons B. positive protons and neutrons C. positive protons and electrons D. negative electrons 13. Which of the following describes a cation? I. examples include Ca 2+ and Al 3+ II. III. A. I and II only B. I and III only C. II and III only D. I, II, and III a metal atom that has lost electrons has equal numbers of electrons and protons 14. Which row of the table is completed correctly for an atom of potassium? Use the following Lewis diagrams of four hypothetical elements to answer question 15. Ma Di So Nh 15. Which of the hypothetical elements shown above represents a metal? A. Ma B. Di C. So D. Nh Use the following Bohr model of an element to answer question p 12n 16. Which of the following does the Bohr model represent? A. a neon atom B. a sodium ion C. a sodium atom D. a fluorine atom 2e 8e Atomic Mass of Protons of Neutrons of Electrons A B C D MHR Atomic Theory and Bonding 2008 McGraw-Hill Ryerson Limited
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