Basic Chemistry Copyright © 2011 Pearson Education, Inc. Chemistry Chapter 6 Key Vocabulary: 1.octet 2.Octet rule 3.Duet 4.Ionic bond 5.Covalent bond 6.cation.

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Chemistry Chapter 6 Key Vocabulary: 1.octet 2.Octet rule 3.Duet 4.Ionic bond 5.Covalent bond 6.cation 7.anion 8.Ionic compound 9.Transition metals 10. Polyatomic ions 11. Diatomic molecule 12. Organic compound 13. Hydrocarbon 14. Saturated hydrocarbon 15. Tetrahedral 16. Alkane 17. Expanded formula 18. Condensed formula

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Chapter 6 -Inorganic and Organic Compounds: Names and Formulas Chapter 6 -Inorganic and Organic Compounds: Names and Formulas 2 Basic Chemistry Copyright © 2011 Pearson Education, Inc.

6.1 Octet Rule and Ions 6.1 Octet Rule and Ions I.Octet rules A. octet- 8 valence electrons associated with the stability of the noble gases 1.does not occur with He, which is stable with two valence electrons (duet) Valence electrons He 1 s 2 2 Ne 1 s 2 2 s 2 2 p 6 8 Ar 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 8 Kr 1 s 2 2 s 2 2 p 6 3 s 2 3 p 6 4 s 2 3 d 10 4 p 6 8 3

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Ionic and Covalent Bonds C. ionic bonds involve loss of electrons by a metal gain of electrons by a nonmetal D. Covalent bonds involve a sharing of electrons by nonmetals 5

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Metals Form Positive Ions E. Metals form positive ions (cations) 1.by a loss of their valence electrons 2.with the electron configuration of their previous noble gas 3.that have fewer electrons than protons. Group 1A (1) metals  ion + Group 2A (2) metals  ion 2+ Group 3A (13) metals  ion 3+ 6

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Charge of Sodium Ion, Na + With the loss of its valence electron, the sodium ion has a 1+ charge. Sodium atom Sodium ion 11 p + 11 e  10 e  0 1+ 8

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Charge of Magnesium Ion, Mg 2+ With the loss of two valence electrons, magnesium forms a positive ion with a 2+ charge. Mg atomMg 2+ ion 12 p + 12 p + 12 e  10 e  0 2+ 10

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Formation of Negative Ions F. In ionic compounds, nonmetals 1.achieve an octet arrangement 2.gain electrons with the electron configuration of their next noble gas 3.form negatively charged ions (anions) with 3 , 2 , or 1  charges 11

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Charge of a Chloride Ion, Cl - A chloride ion forms when Cl gains one electron so it has a 1  charge Chlorine atom Chloride ion 17 p + 17 p + 17 e  18 e  0 1  13

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Ionic Charge from Group Numbers G. The charge of an atom can be figured out by using their group numbers 1. ions achieve the electron configuration of their nearest noble gas 2. 13 metals in Group 1A (1), Group 2A (2), or Group 3A have positive 1+. 2+, or 3+ charges 3. nonmetals in Groups 5A (15), 6A (16), or 7A (17) have negative 3 , 2 , or 1  charges 4. The charge of an ion is obtained by subtracting 8 from its Group number. Example: Group 6A = 6  8 = 2  15

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 17 II. Ionic compounds consist of positive and negative ions & have attractions called ionic bonds between positively and negatively charged ions A. ionic compounds have high melting and boiling points & are solids at room temperature 1. Sodium chloride (table salt) is an example of an ionic compound. 6.2 Ionic Compounds

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 18 B. An ionic formula consists of positively and negatively charged ions & is electrically neutral 1. it has a net charge of zero (total positive charge = total negative charge) 2. it uses subscripts to indicate the number of ions needed to give charge balance Ionic Formulas

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 19 Ex. Charge Balance for NaCl, “Salt” 3. In NaCl, a.a Na atom loses its valence electron b.a Cl atom gains an electron c.the symbol of the metal (cation) is written first followed by the symbol of the nonmetal (anion) d.the charges of the ions in the compound are not shown

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 20 4. The formulas of ionic compounds are determined from the charges on the ions. atoms ions      Na  +  F :  Na + : F :  NaF     sodium fluorine sodium fluoride a. The overall charge of NaF is zero (0). Na + F  = NaF 1(1+ ) + 1(1  ) = 0 Ex. Charge Balance in NaF

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 21 Ex. Charge Balance In MgCl 2 5. In MgCl 2, a Mg atom loses two valence electrons a.two Cl atoms each gain one electron b.subscripts indicate the number of ions needed to balance the charge

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 22 Ex. Charge Balance In Na 2 S 6. In Na 2 S, two Na atoms lose one valence electron each a.one S atom gains two electrons b.subscripts show the number of ions needed to balance the charge

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 23 Writing Ionic Formulas from Charges C. Charge balance is used to write the formula for sodium nitride, a compound containing Na + and N 3−. Na + 3Na + + N 3− = Na 3 N Na + 3(+1) + 1(3  ) = 0

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 24 Ex. Write the ionic formula of the compound containing Ba 2+ and Cl . Write the symbols of the ions. Ba 2+ Cl  Balance the charges. Ba 2+ Cl  two Cl  needed Cl  Write the ionic formula using a subscript 2 for two chloride ions that give charge balance. BaCl 2 Formula from Ionic Charges

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 25 6.3 Naming and Writing Ionic Formulas III. Naming ionic compounds A. In the name of an ionic compound, 1.the positive ion (first ion-cation) is named as the element 2.the negative ion (second ion- anion) is named by changing the end of the element name to – ide

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 26 Formula IonsName Cation Anion NaClNa + Cl  sodium chloride K 2 SK + S 2  potassium sulfide MgOMg 2+ O 2  magnesium oxide CaI 2 Ca 2+ I  calcium iodide Al 2 O 3 Al 3+ O 2  aluminum oxide Examples of Ionic Compounds with Two Elements

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 28 Transition Metals That Form Two or More Positive Ions B. Most transition metals and Group 4 (14) metals form two or more positive ions 1. Zn 2+, Ag +, and Cd 2+ form only one ion Examples: Copper forms Cu + and Cu 2+ Iron forms Fe 2+ and Fe 3+ Gold forms Au + and Au 3+

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 31 Examples of Names of Compounds with Variable Charge Metals C. Transition metals with two different ions use a Roman numeral after the name of the metal to indicate the ionic charge 1. only zinc, silver, and cadmium do not use a Roman numeral because they form only one ion (Zn 2+, Ag +, and Cd 2+ )

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 33 Ex. Naming FeCl 2 STEP1 Determine the charge of the cation from the anion. 2Cl  2(1  ) = 0 Fe = 2+ = Fe 2+ STEP 2 Name the cation by its element name and use a Roman numeral in parentheses for the charge. Fe 2+ = iron(II)

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 34 Naming FeCl 2 (continued) STEP 3 Name the anion by using the first syllable of its element name followed by - ide. ex. chloride STEP 4 Write the name of the cation first and the name of the anion second. ex. iron(II) chloride = FeCl 2

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 35 Naming Cr 2 O 3 STEP1 Determine the charge of the cation from the anion. 2Cr(?) + 3O 2  = 2Cr (?) + 3(2  ) = 0 2Cr(?) = 6+ Cr(?) = 3+ = Cr 3+ STEP 2 Name the cation by its element name and use a Roman numeral in parentheses for the charge. Cr 3+ = chromium(III)

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 36 STEP 3 Name the anion by using the first syllable of its element name followed by - ide. ex. oxide STEP 4 Write the name of the cation first and the name of the anion second. ex. chromium(III) oxide Naming Cr 2 O 3

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 37 Ex. Writing Formulas Write the formula of potassium sulfide. STEP1 Identify the cation and anion. potassium = K + sulfide = S 2− STEP 2 Balance the charges. K + S 2− K + 2(1+) + 1(2  ) = 0 STEP 3 Write the formula, cation first, using the subscripts from the charge balance. 2 K + and 1 S 2− = K 2 S

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 38 Ex. Writing Formulas Write the formula of cobalt(III) chloride. STEP1 Identify the cation and anion. cobalt (III) = Co 3+ (III = charge of 3+) chloride = Cl − STEP 2 Balance the charges. Co 3+ and 3Cl − = (3+) + 3(1-) = 0 STEP 3 Write the formula, cation first, using the subscripts from the charge balance. 1 Co 3+ and 3 Cl − = CoCl 3

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 39 IV. A polyatomic ion - a group of covalently bonded atoms (non-metals) that has an overall ionic charge A. an ionic compound may have a polyatomic ion as one of it’s cations or anions B. almost all are anions with the exception of NH 4 + Examples: NH 4 + ammoniumOH − hydroxide NO 3 − nitrateNO 2 − nitrite CO 3 2− carbonatePO 4 3− phosphate HCO 3 − hydrogen carbonate (bicarbonate) 6.4 Polyatomic Ions Basic Chemistry Copyright © 2011 Pearson Education, Inc.

41 C. The names of the common polyatomic anions end in ate NO 3 − nitratePO 4 3− phosphate D. The same groups with one oxygen less end in ite NO 2 − nitritePO 3 3− phosphite E. with hydrogen use prefix hydrogen (or bi) HCO 3 − hydrogen carbonate (bicarbonate) HSO 3 − hydrogen sulfite (bisulfite) More Names of Polyatomic Ions

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 45 G. Some polyatomic ions of the halogens require prefixes, and they all have the same charge. ClO 4 − perchlorateper + syllable of element + ate –one oxygen more (most) ClO 3 − chlorate syllable of element + ate- (usually most common form) ClO 2 − chlorite syllable of element + ite- one oxygen less (smaller) ClO − hypochlorite hypo + syllable of element - two oxygens less (least) Prefixes for Names of Polyatomic Ions of Halogens

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 47 H. In a compound with a negatively charged polyatomic, the positive ion is named first followed by the name of the polyatomic ion NaNO 3 sodium nitrate K 2 SO 4 potassium sulfate Fe(HCO 3 ) 3 iron(III) bicarbonate or iron(III) hydrogen carbonate (NH 4 ) 3 PO 3 ammonium phosphite Examples of Naming Compounds with Polyatomic Ions

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 48 Writing Formulas with Polyatomic Ions I. The formula of an ionic compound containing a polyatomic ion must have a charge balance that equals zero(0) Na + and NO 3 − →NaNO 3 1. with two or more polyatomic ions encloses the polyatomic ions in parentheses Mg 2+ and 2NO 3 − → Mg(NO 3 ) 2 subscript 2 for charge balance

Basic Chemistry Copyright © 2011 Pearson Education, Inc. When to use Roman Numerals Use Roman numerals if: 1.There is a metal and nonmetal & 2.The metal is a transition metal (including Sn & Pb)& 3.The metal has more than one ion & 4.The metal is NOT Ag, Zn, or Cd Do not use Roman numerals if: 1.There are two non metals (use prefixes) 2.If the metal is not a transition metal 3.If the metal is Ag, Zn, or Cd 49

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 53 V. Naming covalent compounds A. In a hydrogen (H 2 ) molecule, two hydrogen atoms share electrons to form a covalent single bond 1. each H atom acquires two (2) electrons 2. each H becomes stable like helium (He) B. These elements share electrons to form diatomic, covalent molecules. Basic Chemistry Copyright © 2011 Pearson Education, Inc.

54 Electron-Dot Formulas C. Electron-dot formulas show 1. the order of bonded atoms in a covalent compound 2. the bonding pairs of electrons between atoms 3. the unshared (lone) valence electrons 4. a central atom with an octet Basic Chemistry Copyright © 2011 Pearson Education, Inc.

56 Names of Covalent Compounds D. In the naming of covalent compounds, prefixes are used because two nonmetals can form two or more different compounds Examples of compounds of N and O: NO nitrogen oxide NO 2 nitrogen dioxide N 2 O dinitrogen oxide N 2 O 4 dinitrogen tetroxide N 2 O 5 dinitrogen pentoxide Basic Chemistry Copyright © 2011 Pearson Education, Inc.

58 To name the covalent compound SO 3, STEP 1 Name the first nonmetal by its element name. The element S is sulfur. STEP 2 Name the second nonmetal by using the first syllable of its element name followed by ide. O is named oxide. STEP 3 Add prefixes to indicate the number of atoms (subscripts). The subscript 3 of O is shown as the prefix tri. SO 3 → sulfur trioxide The subscript 1(for S) or mono is understood. Ex. Naming Covalent Compounds Basic Chemistry Copyright © 2011 Pearson Education, Inc.

Chemistry Chapter 10 Key Vocabulary: 1.Electron dot symbols 2.Electron dot formulas 3.single bond 4.double bond 5.Triple bond 6.Resonance structures 7.electronegativity 8.polar covalent bond 9.Non-polar covalent bond 10. Ionic bond 11. Polar molecules 12. non-polar molecules

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 10.1 Electron-Dot Formulas I.Electron-dot symbols show the valence electrons (electrons in the outermost energy level) of an atom - one to four valence electrons as single dots on the sides of an atomic symbol Five to eight valence electrons with one or more pairs of dots on the sides of an atomic symbol

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 66 A. Electron-dot formulas –show the sequence of bonded atoms in a molecule or polyatomic ion 1. it shows the bonding pairs of electrons shared between atoms 2. the nonbonding or unshared (lone pairs) of valence electrons 3. atoms with octets except H, which needs two electrons

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 68 Example of Writing an Electron-Dot Formula for SF 2 Write the electron-dot formula for SF 2. STEP 1 Determine the arrangement of atoms. S is the central atom. F S F STEP 2 Determine the total number of valence electrons. 1 S(6 e  ) + 2 F(7 e  ) = 6 e  + 14 e  = 20 e 

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 69 Electron-Dot Formula for SF 2 STEP 3 Attach each bonded atom to the central atom with a pair of electrons. F : S : F STEP 4 Place the remaining electrons using single or multiple bonds to complete octets. Calculate the remaining electrons: 20 valence e  - 4 bonding e  = 16 e  remaining             : F : S : F : or : F─S─F :            

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 70 B. Multiple Bonds 1. single bond -one pair of electrons is shared 2. double bond -two pairs of electrons are shared 3. triple bond -three pairs of electrons are shared Ex. In nitrogen, N 2, octets are achieved by sharing three pairs of electrons, which is a triple bond

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 71 Example of Writing the Electron-Dot Formula of CS 2 Write the electron-dot formula for CS 2. STEP 1 Determine the arrangement of atoms. The C atom is the central atom. S C S STEP 2 Determine the total number of valence electrons. 1 C(4 e  ) + 2 S(6 e  ) = 4 e  + 12 e = 16 e 

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 73 Electron-Dot Formula of CS 2 STEP 4 Place the remaining electrons using single or multiple bonds to complete octets. Calculate the remaining electrons. 16 valence e  - 4 bonding e  = 12 e  remaining.... : S : C : S :.... To complete octets, move two lone pairs between C and each S atom to give two double bonds......... : S : : C : : S : or : S = C = S :

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 74 Exceptions to the octet rule 1.Usually non-metals form octets but some elements don’t follow the standard filling rule 2.Boron compounds have 6 valence electrons on the central Boron and form 3 bonds 3.P, S, Cl, Br, I with octets may also share more valence electrons

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 75 C. Resonance structures - consist of two or more electron-dot formulas for the same arrangement of atoms 1.may be written for molecules or polyatomic ions with multiple bonds 2.are shown with a double-headed arrow 3.are written by changing location of a double bond from the central atom to a different attached atom 4.Resonance can occur only in molecules with double bonds or charges

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 76 D. It is a resonance structure if it has: 1) the same molecular formulas. 2) the same total number of electrons (same overall charge). 3) the same atoms connected together. Although, they can differ in whether the connections are single, double or triple bonds.

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 78 Cyanate ion NCO − has three resonance structures. STEP 1 Determine the arrangement of atoms. N C O − STEP 2 Determine the total number of valence electrons. 1 N(5 e  ) + 1 C(4 e  ) + 1 O(6 e  ) + charge (1e − ) 5 e  + 4 e  + 6 e  + 1 e  = 16 e  Writing Resonance Structures

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 79 STEP 3 Attach each bonded atom to the central atom with a pair of electrons. N : C : O − STEP 4 Place the remaining electrons using single or multiple bonds to complete octets. Determine the remaining electrons. 16 valence e  - 4 bonding e  = 12 e  remaining Writing Resonance Structures (continued)

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 80 Add 12 remaining electrons as 6 lone pairs     − : N─C─O :     Form double or triple bonds to make octets     −   −   − : N=C=O : : N─C  O : : N  C─O :     Writing Resonance Structures (continued)

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 81 III. Electronegativity - https://www.youtube.com/watch?v=PVL24HAesnc A. Electronegativity - the relative ability of atoms to attract shared electrons 1.is higher for nonmetals, with fluorine as the highest with a value of 4.0 2.is lower for metals, with cesium and francium as the lowest with a value of 0.7 3.increases from left to right going across a period on the periodic table 4.decreases going down a group on the periodic table

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 84 https://www.youtube.com/watch?v=QXT4OVM4vXI B. nonpolar covalent bond - occurs between nonmetal atoms and consists of an equal (or almost equal) sharing of electrons 1.has a zero (or close to zero) electronegativity difference of 0.0 to 0.4 Examples: Atoms Electronegativity Type of Bond Difference N  N 3.0 - 3.0 = 0.0 Nonpolar covalent Cl  Br 3.0 - 2.8 = 0.2 Nonpolar covalent H  Si2.1 - 1.8 = 0.3 Nonpolar covalent

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 85 C. polar covalent bond - occurs between nonmetal atoms and consists of atoms that share electrons unequally 1.has an electronegativity difference range of 0.5 to 1.8 Examples: Atoms ElectronegativityType of Bond Difference O  Cl 3.5 - 3.0 = 0.5Polar covalent Cl  C 3.0 - 2.5 = 0.5Polar covalent O  S 3.5 - 2.5 = 1.0Polar covalent

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 87 D. ionic bond - occurs between metal and nonmetal ions and is a result of electron transfer 1.has a large electronegativity difference (1.8 or more) Examples: Atoms Electronegativity Type of Bond Difference Cl  K 3.0 – 0.8 = 2.2 Ionic N  Na 3.0 – 0.9 = 2.1 Ionic S  Cs2.5 – 0.7= 1.8 Ionic

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 89 Polar Molecules E. polar molecules - contains polar bonds 1.has a separation of positive and negative charge called a dipole indicated by a dipole arrow 2.has dipoles that do not cancel 3.It has a positive end and a negative end 4.The bigger number gets the negative, smaller gets positive sign

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 90 6.6 Organic Compounds VI. organic compound - a compound with one or more C atoms, many H atoms & may also contain O, S, N, P, and halogens (more in Chap 17) A. Properties of some organic compounds 1. Propane, C 3 H 8, is an organic compound used as a fuel. 2. NaCl, salt, is an inorganic compound (doesn’t contain Carbon) composed of Na + and Cl  ions.

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 91 Organic Compounds B. Typical organic compounds 1.contain carbon 2.have covalent bonds 3.have low melting points 4.have low boiling points 5.are flammable 6.are not usually soluble in water 7.If an organic compound only contains carbons and hydrogens, it is called a hydrocarbon.

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 94 Organic Molecules D. In organic molecules with more than one carbon atom: 1.valence electrons are shared 2.covalent bonds form between C atoms 3.covalent bonds form between C and H atoms H H H H H  C  C  H H C CH H H H H Ethane, CH 3 ─CH 3 4. Each carbon in ethane has a tetrahedral shape

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 95 6.7 Structural Formulas of Alkanes VII. Alkanes (always end in ane) – type of hydrocarbon that have single bonds between the carbons & are written with structural formulas that are expanded to show each bond or condensed to show each carbon atom and its attached hydrogen atoms

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 97 A. Drawing Structures for Butane 1. In the expanded structure formula, each bond from the C atom to the attached H atoms is shown. 2. In the condensed structural formula, each C atom is combined with its attached H atoms. 3. In the skeletal formula, a carbon skeleton in which carbon atoms are represented as the end of each line or as corners in a zigzag pattern Skeletal formula

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 98 B. Alkanes 1.are nonpolar (equal sharing of electrons) 2.are less dense than water (float) 3.with 1-4 carbon atoms are gases & used as heating fuel 4.with 5-8 carbon atoms are liquids at room temperature (very volatile – used in gasoline)

Basic Chemistry Copyright © 2011 Pearson Education, Inc. 99 C. Alkanes 5.with 9-17 carbon atoms are liquids such as kerosene, diesel, and jet fuel 6.with 18 or more carbon atoms are waxy solids (paraffins) 7.More than 25 – used in ointments 8.They are saturated hydrocarbons – have only single bonds between the carbons and every carbon has the maximum # of hydrogen attached

Basic Chemistry Copyright © 2011 Pearson Education, Inc. Chemistry Chapter 6 Key Vocabulary: 1.octet 2.Octet rule 3.Duet 4.Ionic bond 5.Covalent bond 6.cation.

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Basic Chemistry Copyright © 2011 Pearson Education, Inc. Chemistry Chapter 6 Key Vocabulary: 1.octet 2.Octet rule 3.Duet 4.Ionic bond 5.Covalent bond 6.cation.

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Presentation on theme: "Basic Chemistry Copyright © 2011 Pearson Education, Inc. Chemistry Chapter 6 Key Vocabulary: 1.octet 2.Octet rule 3.Duet 4.Ionic bond 5.Covalent bond 6.cation."— Presentation transcript:

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