1) Atoms in their normal state have a charge, because their number of charged protons equals their number of charged electrons.

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1 Page1 What is an ion Unit packet 3 An ion is a charged atom or molecule. It is charged because the number of electrons does not equal the number of protons in the atom or molecule. An atom can acquire a positive charge or a negative charge depending on whether the number of electrons in an atom is greater or less then the number of protons in the atom. If the atom has more electrons than protons, it is a negative ion, or ANION. If it has more protons than electrons, it is a positive ion, or CATION. Protons Neutrons Anion CaTion Protons Neutrons Protons Neutrons Protons Neutrons 1) Atoms in their normal state have a charge, because their number of charged protons equals their number of charged electrons. 2) An atom becomes a negative ion, called a(n), when it gains one or more electrons. This makes sense, because by adding electrons you are adding more negative charges then there are positive charges from the protons, so the overall charge is. 3) An atom becomes a positive ion, called a, when it loses one or more electrons. If an atom loses electrons it now has more positively charged, than it does negatively charged and therefore has an overall positive charge. 4) A (two or more atoms) may also become an ion by gaining or losing electrons from a shared group of electrons, but we will learn more about them in the next unit. 5) is the process by which an electrically neutral atom or molecule loses or gains one or more electrons and becomes an ion. Ionization can occur in gases, liquids, or solids. 6) tend to form positive ions because they have few valence electrons that are easier to lose. WORD BANK: Ionization Protons Negative Neutral Electrons Cation Positively Anion Molecule Metals Nonmetals Negatively Little Angel/Devil Analogy: Often consciousness is represented as an angel on one shoulder and a devil on the other each attempting to lead you to make positive or negative choices. As long as there are one of each they are supposed to have a neutral influence. However, imagine if you gain a devil, you now have more negative than positive influences and therefore will make negative choices. Oppositely, if you lose a devil you now have more positive than negative influences and therefore will make more positive choices. This situation is directly analogous gaining and losing electrons and the resulting positive or negative charge. 7) How does the little angel/devil analogy correlate to the gaining and losing of electrons and the formation of ions? Give examples. Chemical Symbols For Ions: The chemical symbol for an ion consists of: (1) the symbol or symbols for elements it contains (2) a sign showing the overall charge of the atom(s) For example, the hydrogen ion is written: H + This + charge means the atom has one more positive charge (proton) than negative charges (electrons) Considering a neutral Hydrogen only has 1 proton and 1 electron in order for this ion to have a + charge the atom must have lost one electron.

2 Page2 If an atom is neutral, does it mean it is stable? NOT NECESSARILY (1.) is used to describe balanced charges (equal number of positives and negatives). (2.) is used to describe the likelihood that an atom will react. Atoms are stable when they have a full outer shell of electrons. The lower the charge on the ion the more stable the ion. Therefore only 1 family of atoms is both stable and neutral. The (3.) Family. Also, the more full shells an atom has the more stable it is. Therefore the most stable atom from the most stable family is (4.) (not in word bank, mwahaha) WORD BANK: Stability Neutral Halogen Noble Gas Alkali Metal It is this lack of stability, or lack of a full valence shell that leads to the creation of ions. Unstable atoms, those without a full outer shell will react with other atoms in an attempt to either: a) Gain electrons to fill their outer shell b) Lose the few electrons they have in their outer shell, so the previous (full) outer shell becomes their valence shell. The Reactivity of Metals with water Note: Some metals react with water. When they react they give off hydrogen gas, a flammable gas. Name of metal What happens when it is added to water? 1. copper, zinc, iron and aluminium 2. magnesium Conclusion List the Metals in order of most reactive to least reactive: 3. calcium 4. lithium 5. sodium

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4 Page4 1. What charge do each of these atoms go to when they become stable ions? A. Potassium, K B. Sulfur, S C. Phosphorous, P D. Neon, Ne E. Aluminum, Al 2. What are the stable numbers of electrons? 3. What is the octet rule? 4. What charges do metals tend to go to, positive or negative? 5. What charges do non-metals tend to go to, positive or negative? 8

5 Page5 1. According to the periodic table, which of these elements will form an ion with a -2 charge? A)Sulfur C)Magnesium B)Fluorine D)Rubidium A 2. Elements in which of the following shaded area undergo the fewest chemical reactions? Select and Explain B C D 3. Which of these elements is most likely to donate one electron? A)Be B)Cs C)Rn D)He 4. According to the periodic table, which element most readily accepts electrons? A) Fluorine B) Nitrogen C) Arsenic D) Aluminum 5. An unidentified element has many of the same physical and chemical properties as magnesium and strontium but has a lower atomic mass than either of these elements. What is the most likely identity of this element? A) Sodium B) Beryllium C) Calcium D) Rubidium Isotopes Vs Ions *Ions are positively or negatively charged atoms while isotopes are atoms with different neutrons and therefore different masses. *Ions exist when there is a deficiency or excess of electrons in an atom while isotopes exist when there is a deficiency or excess of neutrons in an atom. Decide if each of the following is an ion, isotope, both, or neither 6. Carbon-12 7.Neon Cl 9. Na Cl Mg Use the pictures to the right to answer the following: 12. Which pictures would be considered ions? Explain: 13. Which one(s) is a cation? Explain: 14. Which one(s) is an anion? Explain: 15. Are any of them atoms (or neutral)? Which ones? How do you know? 16. Which ones are isotopes? Give the name and mass and compare the mass number to atomic masses to explain how you identified it.

6 Page6 1) Determine the correct items that belong in the blank atomic symbol to the right (mass number, atomic number, charge, symbol) 2) How do you write the name of any element s isotope? 20 9 F 1-3) How can you determine the atomic number of any element? 4) How do you calculate the mass number of an isotope? 5) How can you determine the charge of an atom? 6) How can you determine the number of protons in an atom? 7) How can you determine the number of neutrons in an atom? 8) How can you calculate the number of electrons in an atom that is NOT neutral? 9) How can you determine the number of particles in an atom s nucleus? 10) Fill in the following chart using a periodic table Review: Atomic mass, atomic number, and mass number can get very confusing. Check the correct boxes Atomic Atomic Mass Mass Number Number Potassium Is equal to protons + neutrons Is always equal to the number of protons in an atom Can be found on the periodic table Is always a whole number Describes the mass of an isotope Can always be used to identify an element Is equal to the number of electrons in a neutral atom 1- Can be different for the same element

7 Page7 Naming Ions Cations (Positive ions) are written with the name of the element and the word ion o Ex: K + is named a potassium ion o When you see the word ion after an element name it is a cation. 1) Name each of the following ions a) O 2- b) Mg 2+ c) Br 1- d) N 3- e) S 2- f) Ca 2+ Anions (Negative ions) are written with the name of the element, but the suffix is replaced with ide o Ex: Cl - is named chloride o When you -ide at the end of an element name is an anion. g) Cs + h) P 3-2) Write the Lewis electron-dot symbol for each of the following. a. Carbon ion d. Potassium ion g. Fluoride b. Sodium c. Aluminum ion e. Boron f. Magnesium ion h. Boron ion i. Neon 3) Show the electron configuration of the following. a) oxygen e. sodium ion j. Hydride k. Hydrogen ion b) boron f. bromide c) aluminum g. magnesium ion d) calcium h. sulfide Isoelectronic Configurations We already know that elements with similar electronic configurations tend to have similar chemical and physical properties. It is possible, in fact common, for elemental ions to have not only similar but exactly the same electronic configurations as other elements or ions. When two elements and/or ions have the same electronic configurations it is said that they are "isoelectronic" with one another. When two chemical species are isolectronic they again tend to have similar chemical properties. Element or ion pair Electronic configuration Li +, He 1s 2 Be +2, He 1s 2 F -, Ne 1s 2 2s 2 2p 6 S -2, Ar 1s 2 2s 2 2s 6 3s 2 3p 6 Mg +2, Na + 1s 2 2s 2 2p 6 Ca +, K [Ne]4s 1 P -3, S -2 1s 2 2s 2 2p 6 3s 2 3p 6 Ion Name Ion Symbol # of Protons # of Electrons Electrons Lost or Gained fluoride F Gained 1 Neon Gained 2 6. potassium ion Lost 1 7. Ca Sr H + none Gained Lost aluminum ion H lithium ion Lost Rb Lost 1 Argon Isoelectronic with which Noble Gas?

8 Page8 Electronegativity: measure of the of an atom to attract or an electron from atom Negatively charged ions, called, have an ionic radius that is than the atomic radius because the addition of electrons the positive pull of the nucleus. Positively charged ions, called, have an ionic radius that is than the atomic radius because the loss of electrons the positive pull of the nucleus.

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10 Page10 Periodic Trends Questions: In your own words what is ionization energy? 2. What is the general trend of ionization energy as you go from left to right across the periodic table? 3. What is the general trend of ionization energy as you go down a group on the periodic table? 4. Which of these elements has the highest first ionization energy: Sn, As, or S? 5. When an atom becomes an anion, what happens to its radius? In your own words explain why. 6. When an atom becomes a cation, what happens to its radius? In your own words explain why. 7. For each of the following pairs, circle the atom or ion having the larger radius. a. S or O c. Na 1+ or K 1+ e. S 2 or O 2 b. Ca or Ca 2+ d. Na or K f. F or F 1 8. For each of the following pairs, circle the smaller ion. a. K 1+ or Ca 2+ c. C 4+ or C 4 e. O 2 or F 1 b. F 1 or Cl 1 d. S 2 or F 1 f. Fe 2+ or Fe In your own words what is electronegativity? 8. List the following atoms in order of increasing electronegativity: O, Al, Ca 9. List the following atoms in order of decreasing electronegativity: Cl, K, Cu 10. What is the general trend of electronegativity as you go down the periodic table? 11. What is the general trend of electronegativity as you go left to right across the periodic table? 12. What is the name given to the group of elements that have the following valence shell electron configurations? a. s 2 b. s 2 p 6 c. s 2 p 5 d. s Given the electronic configuration, tell the element name as well as the group and period where these elements are located. a) 1s 2 2s 2 2p 6 3s 1 b) [Ar] 4s 2 3d 10 4p 4 c) 1s 2 2s 2 2p 6 3s 2 3p Group the following elements, in pairs, by similar chemical properties: Ga S Cl Ca Fe O B I Be Os 17. Which corner is the highest electronegativity generally found?. 18. A cation is ( larger / smaller ) than its parent atom. 19. Rank these in order from smallest to largest: H, H 1-, H Rank these elements from largest to smallest atomic radius: a) F, Mg, K, N b) Al, In, B, Ga c) Cl, Mn, Sr, Si 21. Arrange the elements listed in order of decreasing ionization energies: Li, O, C, K, Ne, and F. 22. Which element is more electronegative? a) K, As b) N, Sb c) Sr, Be 23. Identify each of the following as an alkali metal, alkaline earth metal, transition metal, lanthanide, or actinide and write their Noble Gas Electron Configuration a) cesium c) gold e) uranium b) zirconium d) ytterbium f) francium

11 Page11 Electronegativity and ions: Electronegativity is the basis for bonding, the process that forms compounds and molecules. Remember all matter is made of atoms of elements, but rarely do we find atoms of elements in their pure form. Mostly we find atoms of elements bonded to atoms of other elements. For instance table salt is made by the bonding of atoms from 2 elements: sodium and chlorine. How they come to be bonded is from their differences in electronegativity. Look back to the Periodic Table representing electronegativity (page 15). 1. What is the electronegativity of sodium? 2. What is the electronegativity of chlorine? 3. What is the difference in electronegativity? 4. Is the difference in electronegativity greater than 1.7? Remember electronegativity is the measure of the (5) of an atom to attract or (6) an electron from (7) atom. When atoms interact they each have their own electronegativity. The atoms with a higher electronegativity pull on the electrons of the atoms with lower electronegativity. 1.7 Rule: If the difference in electronegativity between two atoms is greater than 1.7, then the atom with the higher electronegativity is able to steal 1 or more electrons from the atom with the lower electronegativity. Thus ions are formed. The atom with their higher electronegativity gains 1 or more electrons becoming an Anion with a (8) charge. The atom with the lower electronegativity loses an electron becoming a Cation with a (9) charge. Positives and Negatives are attracted; therefore the new positive and negative ions stick together once the electrons have been transferred. This new molecule of two atoms is called a compound and the positive/negative attraction holding them together is called an Ionic bond. 1. What happens when two atoms interact which have an electronegativity difference greater than 1.7? (2 sentences) 2. What is a compound? Ionic bonds are the bonds formed between two ions once they have transfered electrons becoming anions and cations. Since elements have different electronegativity they can bond with other elements. These chemical bonds are an attempt to fill electron shells. - Metals have few electrons on their outer shell and a low electronegativity, therefore they easily give up electrons becoming cations. Group 1(1A) metals form 1+ cations Group 2 (2A) metals form 2+ cations Group 13(3A) metals form 3+ cations Non-Metals have many electrons on their outer shell and high electronegativity, therefore they easily take electrons becoming anions. Group 15(5A) non-metals form 3- anions Group 16(6A) non-metals form 2- anions Group 17(7A) non-metals form 1- anions Characteristics of ionic bonds: Between atoms of metals and nonmetals Elements have very different electronegativities Bond formed by transfer of electrons Conductors and have high melting point.

12 Ionic bonding (7:19) What kinds of elements form ionic bonds? 2. Why are the sodium and chlorine atoms bonded? 3. What does the sodium atom give the chlorine atom? 4. How does this change the chlorine atom? 5. After the sodium gives an electron to the chlorine atom, how does it change? 6. What is the difference between chlorine and chloride? 7. Using what you just learned, describe how an ionic bond forms between magnesium and oxygen. Ionic Bonding, Part 2 (10:19) What is every atom s goal in life? 14. Write the formula for Potassium nitride. 15. Write the formula for sodium chloride. 9. Write a definition of an ion in your own words. 10. Describe how an ion is formed. Ionic Bonding, Part 3 (7:56,) What is electronegativity? 12. What kind of atoms are electron givers? Takers? 13. Why are lattice structures formed? Writing Ionic Formulas (11:44)- Step 1: Find the charge -Li O Step 2: Balance the charges. Step 3: Count the atoms and write the formula. 16. Write the formula for aluminum oxide. 17. What are common mistakes when formula writing? Ionic Compounds Formulas and Naming An ionic compound is a compound that is formed between a metal and a non-metal. (Metalloids can also be used in ionic compounds, sometimes as cations and sometimes as anions, depending on the properties of the specific element). In ionic compounds the metal will always be a cation and the non-metal will always be the anion. When forming ionic compounds the goal is to balance the number of positive charges with the number of negative charges. More specifically, you want to ensure that the number of electrons that the cations are giving up is equal to the number of electrons the anions need so that both have full outer energy levels. Part 1: How to Write an Ionic Compound Formulas i. Cation: Write the cation symbol first, then anion (metal then non-metal just like the periodic table) ii. Charge: Look at the periodic table to find the charge of the ions iii. Subscripts: Figure out the subscripts, Never write 1 as a subscript, it is understood. Option A: Logic- write the number of each ion needed to cancel the charges. Option B: Cross and reduce- cross the charge number of each ion as the subscripts (ignore the positive and negative). Reduce if possible. For Example: Write the formula for the compound of barium and sulfur i. Cation: barium is Ba and sulfur is S, so Ba_S_ ii. Charge: Ba 2+ S 2- iii. Subscripts Option A: Logic- since they both have a 2 charge the charges cancel with 1 of each. The subscripts are 1 which are never written. The formula is: BaS ption B: Cross and reduce- The charge numbers cross Ba 2+ S 2- becomes Ba 2S 2 which reduces to: BaS The formula is the same with either option; choose the one you prefer and practice! 18. potassium and fluoride 20. strontium and phosphorus 22. selenium and calcium 19. bromine and magnesium 21. cesium and sulfur 23. rubidium and nitrogen 12

13 Part 2: How to Name an Ionic Compound IMPORTANT: On your periodic table, cross out the suffixes for the nonmetals and metalloids that form anions. For each of the halogens, cross out ine; for selenium and tellurium, cross out ium; for carbon, arsenic, and sulfur, cross out the last two letters of each name; and for oxygen, nitrogen, and phosphorous, cross out the last four letters of each element s name. What remains will be referred to as the anion s root name. We will use this root name and the new suffix ide when naming ionic compounds. i. Cation: Write the name of the cation first- No change ii. Anion -ide : write the root name of the anion and end it in -ide For our example, we will name the compound we made earlier using barium and sulfur, BaS. i. Cation: Ba is barium ii. Anion -ide : S root name is sulf- end it in -ide = sulfide Compound name: barium sulfide Important: Lower case lettering should be used when naming an ionic compound. Also note that our answer is two separate words. The first is the cation and the second is the root of the anion and the suffix ide. Part 1: Write the formula of each binary ionic compound named below. 1. strontium fluoride 2. sodium phosphide 3. beryllium iodide 4. calcium bromide 5. aluminum astatide 6. lithium telluride 7. magnesium arsenide 8. potassium nitride 10. hydrogen chloride 11. cesium sulfide 12. calcium selenide 13. gallium oxide 14. strontium selenide 15. francium nitride 16. aluminum chloride 17. When writing a chemical formula which comes first? Anion or cation Part 2: Name each of the following below. 18. CaCl Mg 2 C 20. RbAt 21. RaI LiF 23. K 2 Se 24. NaBr 26. H 3 N 27. In 2 S Fr 3 P 29. SrTe 30. AlF HI 32. CsI 9. rubidium carbide 25. Be 3 As 2 Ionic Compounds Formulas and Naming with Polyatomic Ions Polyatomic Ions Write the definition of a polyatomic ion in your own words: Writing Ionic Formulas with Polyatomic Ions(11:20) What two items do you need in order to write a chemical formula for an ionic compound with a polyatomic ion? 35. How is writing a formula with a polyatomic different from others you have written? 36. How do you avoid getting the polyatomic ions confused with the anions? 37. Write the formula for: a) sodium carbonate b) ammonium phosphate c) magnesium phosphate 13

14 Ionic Compounds Using Polyatomic Ions Polyatomic ions are a group of two or more elements that have an overall ionic charge. Most times the polyatomic will function as an anion, but there are a few polyatomic ions that are cations. Part 1: How to write a formula for an ionic compound that has a polyatomic ion. The only new information is highlighted, everything else is the same. i. Cation: Write the cation symbol(s) first, then anion(s) ii. iii. Charge: Look at the periodic table or Polyatomic List to find the charge Subscripts: Figure out the subscripts, Never write 1 as a subscript, it is understood. If you need to add a subscript to a polyatomic ion, put the polyatomic ion in parenthesis and the subscript outside the parenthesis. NEVER CHANGE THE SUBSCRIPTS OF A POLYATOMIC ION. Option A: Logic- write the number of each ion needed to cancel the charges. Option B: Cross and reduce- cross the charge number of each ion as the subscripts (ignore the positive and negative). Reduce if possible. For Example: Write the formula for the compound of barium and nitrate i. Cation: barium is Ba and nitrate is NO 3, so Ba_NO 3_ ii. Charge: Ba 2+ NO 3 1- iii. Subscripts Option A: Logic- since Ba has a 2 charge, and nitrate a 1 charge; 1 barium and 2 nitrates are needed to cancel the charges. The subscript 1 won t be written and parentheses must be used for the subscript on nitrate. The formula is: Ba(NO 3) 2 Option B: Cross and reduce- The charge numbers cross Ba 2+ NO3 1- Use Parenthesis for Polyatomic Ion becomes Ba(NO 3)2 which doesn t reduce. The formula is the same with either option; choose the one you prefer and practice! 1. potassium and chromate 3. strontium and phosphate 5. calcium and selenite 2. magnesium and oxalate 4. cesium and sulfite 6. rubidium and iodate Part 2: Naming ionic compounds that have polyatomic ions. i. Cation: Write the name of the cation first, doesn t matter if monatomic or polyatomic- No change ii. Anion: -if monatomic (directly from periodic table) write the root name of the anion and end it in -ide -if polyatomic write the name of the polyatomic ion- No change For our example, we will name the compound we made earlier using barium and nitrate, Ba(NO 3) 2. iii. Cation: Ba is barium iv. Anion: NO 3 is the polyatomic ion nitrate Compound name: barium nitrate Part 1: write the correct formula. 7. calcium and selenite More Practice: Ionic Compounds Using Polyatomic Ions Part 2: Name each of the 19. Ga 2 (SiO 3 ) 3 following ionic compounds. 13. NaHCO AlAsO calcium hydroxide 25. gallium permanganate 8. magnesium and nitrite 14. Be(CHO 2 ) (NH 4 ) 3 PO aluminum hydrogen sulfate 9. rubidium and dichromate 10. ammonium and hydroxide 11. lithium and periodate 12. potassium and sulfate 15. H 2 O In(HSO 4 ) Fr 3 PO Sr(N 3 ) 2 Part 3: Write the formula for each ionic compound named. 22. sodium sulfate 23. cesium nitrate 27. lithium perchlorate 28. magnesium thiocyanate 29. potassium tellurite 30. rubidium borate 14

15 Page15 Ionic Compounds Using Multivalent Cations Multivalent means multiple valence electron arrangements. If there are multiple valence electron arrangements, then there are multiple possible charges. Most of the transition metals and other metals are multivalent cations. You need to memorize the 4 univalent (one charge) transition/other metals and their charge: Aluminum, Al 3+, Zinc, Zn 2+, Cadmium, Cd 2+, and Silver, Ag +. ALL OTHER TRANSITION METALS & OTHER METALS have a special addition to the naming/formula writing system to identify the charge, they use roman numerals. Part 1: How to Write an Ionic Compound Formula with Multivalent Cations. The only new information is highlighted, everything else is the same. i. Cation: Write the cation symbol first, then anion (metal then non-metal just like the periodic table) ii. Charge: The charge of the multivalent cation will be given to you as a Roman Numeral in parenthesis. Look at the periodic table or polyatomic list to find the charge of the anion. iii. Subscripts: Figure out the subscripts, Never write 1 as a subscript, it is understood. Option A: Logic- write the number of each ion needed to cancel the charges. Option B: Cross and reduce- cross the charge number of each ion as the subscripts (ignore the positive and negative). Reduce if possible. For Example: Write the formula for the compound of iron(iii)oxide i. Cation: iron is Fe and oxide is the oxygen anion, so Fe_O_ ii. Charge: the charge of the multivalent ion is given in roman numeral Fe 3+ O 2- iii. Subscripts Option A: Logic- since iron has a 3 charge and oxygen a 2, 2 irons and 3 oxygens are needed to cancel the charges. The formula is: Fe 2O 3 Option B: Cross and reduce- The charge numbers cross Fe 3+ O 2-- becomes Fe 2O 3 which doesn t reduce. Part 2: How to Name an Ionic Compound with Multivalent Cations i. Cation: Write the name of the cation first, and then in parenthesis write the charge as a roman numeral. Option A: Logic -To find the charge use the known charge of the anion to find the equal charge of the cation that cancels it out. For example: If the subscripts are 1:1, the charges are equal. Ex. FeO, iron (II) oxide If the subscripts are 1:2 the cation has twice the charge of the anion (twice as many anions to cancel) PbO 2 lead (IV) oxide If the subscripts are 2:1 the cation has half the charge of the anion (twice as many cations to cancel) Fe 2O, Iron (I) oxide Option B: Reverse cross. Reverse cross subscripts back to the charge position, check to ensure the anion has the correct charge. If it does not, multiply both charges until the anion does have the correct charge ii. Anion -if monatomic (directly from periodic table) write the root name of the anion and end it in -ide -if polyatomic write the name of the polyatomic ion- No change For our example, we will name the compound we made earlier using iron and oxygen, Fe 2O 3. i. Cation: Fe is iron, to find the charge to go in the parenthesis as a roman numeral: Option A: Logic-write the the charge on this Fe must be 3 + because each oxygen has a 2- charge and three are required to cancel the charge of 2. iron(iii) Option B: Reverse cross- The formula has not been reduced because the subscript on Fe is 2 from oxygen s charge. Reverse cross the charges and Fe must have a charge of 3 +. iron(iii) ii. Anion: oxygen s root name is ox- end it in -ide = oxide Compound name: iron(iii)oxide 1. HgF 2 2. NaCl 3. Ca(MnO 4 ) 2 Naming Ionic Compounds with Multivalent Cations 7. ZnO 13. ZnCl 2 8. Mg(HCO 3 ) Ba 3 (PO 3 ) Fe(NO 2 ) K 2 SO 4 9. B(OH) AgH 2 PO Ba(HSO 4 ) 2 4. FeHPO Sn 3 (PO 3 ) Fe 2 O Sn(HCO 3 ) 4 5. RbClO NH 4 IO 17. HgCl 23. NaMnO 4 6. BeCO SrCO CoF Ag 2 O 15

16 Page16 Names & Formulas for Ionic Compounds Give the name or formula of the following ionic compounds: Name 1) Na 2 CO 3 2) NaOH 3) MgBr 2 4) KCl 5) FeCl 2 6) FeCl 3 7) Zn(OH) 2 8) Be 2 SO 4 9) CrF 2 10) Al 2 S 3 11) PbO 12) Li 3 PO 4 13) TiI 4 14) Co 3 N 2 15) Mg 3 P 2 16) Ga(NO 2 ) 3 17) Ag 2 SO 3 18) NH 4 OH 19) Al(CN) 3 20) Be(CH 3 COO) 2 Formula 21) sodium phosphide 22) magnesium nitrate 23) lead (II) sulfite 24) calcium phosphate 25) ammonium sulfate 26) silver cyanide 27) aluminum sulfide 28) beryllium chloride 29) copper (I) arsenide 30) iron (III) oxide 31) gallium nitride 32) iron (II) bromide 33) vanadium (V) phosphate 34) calcium oxide 35) magnesium acetate 36) aluminum sulfate 37) copper (I) carbonate 38) barium oxide 39) ammonium sulfite 40) silver bromide 16

17 Page17 Lewis Dot Practice Ionic Bond Practice 1. Fill in the missing information on the chart. 2. For each of the following ionic bonds: Write the Formula for the compound to find out how many of each elements are in the compound. Write the symbol for each element. Draw a Lewis Dot structure for the valence shell of each element. Draw an arrow (or more if needed) to show the transfer of electrons Write the name of the compound a) Sodium + Chlorine Formula: Lewis Dots of each element (with arrows showing transferred electrons: Element Sodium Chlorine Magnesium Fluorine Lithium # of Protons # of Electrons # of Valence Electrons # of electrons needed to fill outer Oxygen Phosphorus Iodine Compound Name: Calcium b) Magnesium + Iodine Formula: Lewis Dots of each element (with arrows showing transferred electrons: Lewis Dots of each element( with arrows showing transferred electrons: Compound Name: Compound Name: c) Sodium + Oxygen Formula: Lewis Dots of each element (with arrows showing transferred electrons: f) Lithium + Nitrogen Formula: Lewis Dots of each element( with arrows showing transferred electrons: Compound Name: Compound Name: g) Aluminum + Oxygen Formula: Lewis Dots of each element( with arrows showing transferred electrons: d) Calcium + Chlorine Formula: Lewis Dots of each element( with arrows showing transferred electrons: Compound Name: Compound Name: e) Aluminum + Chlorine Formula: 17