Slide 1 / 130 Slide 2 / 130 Ionic Compounds and Ionic Bonding Slide 3 / 130 Slide 4 / 130 Table of Contents: Ionic Compounds and Ionic Bonding Click on the topic to go to that section Periodic Table Review · Valence Electrons and the Octet Rule · Periodic Table Review Ions · Ionic Bonding · Properties of Ionic Compounds · Predicting an Ionic Compound's Formula · Naming Ionic Compounds · Formulas and Names of Ionic Compounds with Transition Metals · Polyatomic ions · Formula and Names of Compounds with Polyatomic ions · (Ternary Ionic Compounds) Return to Table Polyatomic Patterns · of Contents Slide 5 / 130 Slide 6 / 130 The Periodic Table of the Elements Periodic Table - Review The periodic table can be divided into three large classifications of elements. The periodic table is "periodic" because of certain trends that are seen in the elements. What type of elements are highlighted in blue, in yellow and in pink? What is unique about the elements that are highlighted in Some of these trends can be seen in the properties of atoms we pink? covered in the last unit: atomic size, ionization energy, electronegativity and metallic character. B Si Ge As Would you predict that elements from the same family/group Sb Te would have similar physical and chemical properties? ?
Slide 7 / 130 Slide 8 / 130 Metallic Character of the Elements 1 In the periodic table, the elements are arranged in __________. What the relationship between metallic character and effective nuclear charge? Are they directly or inversely related? Is it accurate to say "Element A is more A alphabetical order metallic than element B" even if element B is a non-metal? B order of increasing atomic number C order of increasing metallic properties More metallic Less metallic Non-metallic D order of increasing neutron content E reverse alphabetical order B Si F I don't know how to answer this. Ge As Sb Te ? Most metallic Slide 9 / 130 Slide 10 / 130 2 Elements __________ exhibit similar physical 3 Which pair of elements would you expect to and chemical properties. exhibit the greatest similarity in their physical and chemical properties? A with similar chemical symbols A Li, Na B with similar atomic masses B Cs, Ba C in the same period of the periodic table C Ca, Si D on opposite sides of the periodic table D Ga, Ge E C, O E in the same group of the periodic table Slide 11 / 130 Slide 12 / 130 4 Which one of the following is a nonmetal? 5 Potassium is a __________ and chlorine is a __________. A W B Sr A metal, nonmetal C Os B metal, metal D Ir C metal, metalloid E S D metalloid, nonmetal E nonmetal, metal
Slide 13 / 130 Slide 14 / 130 Review: Octet Rule Atoms tend towards having complete outer shells of electrons (remember stability). Valence Electrons and the A full outer shell will have: 2 electrons in the s subshell and Octet Rule 6 electrons in the p subshell ( s 2 p 6 configuration) Octet rule: atoms tend towards having a total of 8 electrons 8 valence electrons make an octet Which elements on the periodic table have a complete outer shell? What is true about these elements relative chemical reactivity? Return to Table of Contents Slide 15 / 130 Slide 16 / 130 Valence Electrons Valence Electrons Number of valence Valence electrons are the electrons in the 1 2 3 4 5 6 7 8 electrons in neutral atoms: highest occupied energy level of an Valence element’s atoms. electron 1 - 4 The valence electrons determine the chemical properties of an element. Why do you think this would be true? To find the number of valence electrons in an atom of a representative element (elements found in the s and p blocks), simply look at its group number. Atoms in group 3 have 3 valence electrons, There is one exception: atoms in group 17 have 7 valence electrons, etc. helium has only 2 valence electrons. Slide 17 / 130 Slide 18 / 130 6 How many valence electrons does potassium have? 7 How many valence electrons does Aluminum have? A 3 A 5 B 1 B 7 C 19 C 3 D 4 D 27 E 8 E 13
Slide 19 / 130 Slide 20 / 130 9 Arsenic (As) has 6 valence electrons. 8 How many valence electrons does Barium have? True A 1 B 2 False C 52 3 D E 6 Slide 21 / 130 Slide 22 / 130 Ions Ions are atoms or groups of atoms that have become charged by either gaining or losing electrons . Ions Anions are negative and Cations are positive and are are formed by elements on formed by elements on the the right side of the periodic left side of the periodic chart chart (nonmetals). (metals). Return to Table of Contents Slide 23 / 130 Slide 24 / 130 The Formation of Cations The Formation of Cations Metals usually give up/lose valence electrons to become more stable. Na atom Na+ ion This often results in a noble gas (8 electron) outer shell. loses e- Ne atom Na : 1s 2 2s 2 2p 6 3s 1 Na +1 : 1s 2 2s 2 2p 6 3s 2p 2s Loss of valence electrons 11p 1s 11p 10e - 11e- How many electrons does the Na + ion have? The Na + ion is smaller than the Na atom. Do you remember what factors cause this reduction in size?
Slide 25 / 130 Slide 26 / 130 The Formation of Anions The Formation of Cations Nonmetals usually gain valence electrons. Cations of Group 1A elements always have a charge of 1+. This results in a noble gas (8 electrons) outer shell Cations of Group 2A elements always have a charge of 2+. Ar atom Cl: 1s2 2s2 2p6 3s2 3p5 Cl - 1s2, 2s2, 2p6, 3s2, 3p6 3p 3s Mg Mg 2+ 2e - + 2p Magnesium atom Magnesium ion (2 in front of e - (electrically 2s (+2 indicates 2 indicates 2 units of neutral, units of positive negative charge) charge = 0) charge) How many electrons does the Cl - have? Slide 27 / 130 Slide 28 / 130 The Formation of Anions The Formation of Anions Anions of Group 15 (5A) elements always Cl - ion Cl atom have a charge of 3 - Anions of Group 16 (6A) elements always have a charge of 2 - Anions of Group 17 (7A) elements always Gains an e- have a charge of 1 - 17P 17p 17e - 18e - Consider Group 14 (4A) elements, what common charge(s) would you predict The Cl - ion is larger than the Cl atom. Do you remember what for these elements? factors cause this increase in size? Slide 29 / 130 Slide 30 / 130 10 Metals tend to __________ electrons and 11 Anions tend to be __________ and cations nonmetals tend to __________ electrons. tend to be __________. A metals, metals A gain, gain B nonmetals, nonmetals B lose, lose C gain, lose C metals, nonmetals D lose, gain D nonmetals, metals E neither, they keep their electrons E metalloids, metalloids
Slide 31 / 130 Slide 32 / 130 12 Metals lose electrons to form cations 13 Anions are formed from nonmetals True True False False Slide 33 / 130 Slide 34 / 130 14 Nonmetals tend to lose electrons forming ions 15 This is the ion formed from a calcium atom True A Ca + False B Ca 2+ C Ca - D Ca 2- Slide 35 / 130 Slide 36 / 130 16 Phosphorous forms an ion with a charge of 17 Aluminum forms an ion with a charge of __________. __________. A 1+ A 2+ B 2- B 1- C 3+ C 3+ D 3- E 2+ D 2- E 0
Slide 37 / 130 Slide 38 / 130 18 Of the following, __________ contains the 19 Oxygen forms an ion with a charge of __________. greatest number of electrons. A 2- A P 3+ B 2+ B P C 3- C P 2- D 3+ D P 3- E 6+ E P 2+ Slide 39 / 130 Slide 40 / 130 20 Iodine forms an ion with a charge of __________. 21 This is the ion formed from nitrogen A N - A 7- B N 2- B 1+ C 2- C N 3+ D 2+ D N 3- E 1- Slide 41 / 130 Slide 42 / 130 23 What would be the expected charge on the gallium 22 Predict the charge of the most stable ion of S? (Ga) ion? A 3+ A +1 B 1- B +2 C 6+ C +3 2+ D D +13 E 2- E -5
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