1. Ionic Bonding and Nomenclature

2. Ionic Bonding and Nomenclature
Ionic Bonding Comparing the Properties of Ionic and Covalent Compounds Naming and Writing Formulas for Ions Naming and Writing Formulas for Ionic Compounds Metallic Bonding Naming and Writing Formulas for Acids and Bases

3. Ionic Bonding
Ionic bonding involves the transfer of valence electrons. One atom loses one or more valence electrons to become a cation (positive ion). The other atom gains one or more valence electrons to become an anion (negative ion). Ionic compounds are electrically neutral. This means the total number of negative charges is equal to the total number of positive charges.
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4. Ionic Bonding
Ionic bonding usually results from the bonding of a metal with a nonmetal. For example, the alkali metals typically bond with the halogens to form an ionic compound commonly referred to as a salt. The chemical formula for an ionic compound is referred to as a formula unit and not a molecule.
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5. Ionic Bonding
At room temperature, crystals of ionic compounds exist as regular, three-dimensional arrangements of cations and anions held together by electrostatic attractions. The arrangements are called crystal lattices.
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6. Here is an example of the crystal lattice for sodium chloride.
Ionic Bonding
Here is an example of the crystal lattice for sodium chloride.
(Note: The lines between the ions are not bonds; they are reference lines showing the relative positions of Na+ and Cl-.)
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7. Using Lewis Dot Diagrams to Predict Formulas for Ionic Compounds
Lewis dot diagrams can be used to illustrate the transfer of valence electrons that occurs and to predict the chemical formula for an ionic compound.
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8. Example 1. Use Lewis dot diagrams to predict the formula for the ionic compound formed from sodium and chlorine.
First draw the Lewis dot diagrams for sodium and for chlorine. Next use arrows to illustrate the transfer of valence electrons. The resulting chemical formula is NaCl. The compound formed is called sodium chloride.
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9. First draw the Lewis dot diagrams for calcium and for iodine.
Example 2. Use Lewis dot diagrams to predict the formula for the ionic compound formed from calcium and iodine.
First draw the Lewis dot diagrams for calcium and for iodine.
Next use arrows to illustrate the transfer of valence electrons.
The resulting chemical formula is CaI2. The compound formed is called calcium iodide.
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10. First draw the Lewis dot diagrams for barium and for sulfur.
Example 3. Use Lewis dot diagrams to predict the formula for the ionic compound formed from barium and sulfur.
First draw the Lewis dot diagrams for barium and for sulfur.
Next use arrows to illustrate the transfer of valence electrons.
The resulting chemical formula is BaS. The compound formed is called barium sulfide.
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11. You Try It
Use Lewis dot diagrams to predict the formula for the ionic compound formed from lithium and oxygen.
Chemical Formula
Li2O
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12. You Try It
Use Lewis dot diagrams to predict the formula for the ionic compound formed from aluminum and nitrogen.
Chemical Formula
AlN
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13. You Try It
Use Lewis dot diagrams to predict the formula for the ionic compound formed from magnesium and nitrogen.
Chemical Formula
Mg3N2
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14. Comparing the Properties of Ionic and Covalent Compounds
Characteristics of Ionic and Covalent Compounds
Characteristic
Ionic Compound
Nonpolar Covalent Compound
Polar Covalent Compound
Representative Unit (smallest particle that has all of the properties)
Bond Formation
Type of Elements forming compounds
Physical State
Melting Point
Solubility in H2O
Electrical Conductivity of Aqueous Solution
formula unit
molecule
transfer of one or more valence electrons between atoms
sharing of electron pairs between atoms
Metal with a nonmetal
nonmetals
solid, liquid, or gas
Solid
low
high
soluble
insoluble
soluble
poor to
nonelectrolyte (usually nonelectrolytes)
good electrolyte
nonelectrolyte
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15. Daily Starter (12/3 & 12/4) A C B
The table below represents a student’s experimental results. Use the information to answer the questions below.
Compound
Solubility in Water
Conductivity in Water
Melting Point A
Soluble
Weak Electrolyte
Low B
Strong Electrolyte
High C
Insoluble
Non Electrolyte
1. Which compound is polar covalent?
2. Which compound is nonpolar covalent?
3. Which compound is ionic? A C B

16. Predicting Charges for Ions
The periodic table can be used to help predict the charge on an ion. Remember: Cations are formed when an loses one or more valence electrons. This is typical of metals. Anions are formed when a metal gains one or more valence electrons. This is typical of nonmetals.

17. Symbols of Ions for Cations
The metals in groups 1, 2 and 13 lose electrons when they form ions. Group 1 forms +1 ions. Group 2 forms +2 ions Group 13 forms +3 ions.
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18. Naming and Writing Symbols for Cations
You Try It. Write the symbol and name for each of the following ions.
Element
Symbol of Ion
Name of Ion
Calcium
Sodium
Aluminum
Ca2+
Calcium ion
Na+
Sodium ion
Al3+
Aluminum ion
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19. Metals with More than One Common Oxidation Number
The metals in groups 3-12 are called transition metals. They often have more than one common oxidation number (ionic charge).
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20. Metals with More than One Common Oxidation Number
Here are some of the more commonly used transition metals and their oxidation numbers. Notice that a Roman numeral is used to indicate the charge on the ion when naming the ions formed.
Fe2+ Iron(II) ion Fe3+ Iron(III) ion
Cu+ Copper(I) ion Cu2+ Copper(II) ion
Hg22+ Mercury(I) ion Hg2+ Mercury(II) ion
Pb2+ Lead(II) ion Pb4+ Lead(IV) ion
Sn2+ Tin(II) ion Sn4+ Tin(IV) ion
Cr2+ Chromium(II) ion Cr3+ Chromium(III) ion
Cr6+ Chromium(VI) ion
Mn2+ Manganese(II) ion Mn3+ Manganese(III) ion
Co2+ Cobalt(II) ion Co3+ Cobalt(III) ion
Ni2+ Nickel(II) ion Ni3+ Nickel(III) ion
Ag+ Silver ion
Zn2+ Zinc ion
Cd2+ Cadmium ion
Note: Silver, Zinc and Cadmium do not have more than one common oxidation number. Do not use a Roman numeral when naming them.
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21. Symbols of Ions for Anions
An anion is an atom or group of atoms with a negative charge. An anion has more electrons than a neutral atom of the element. Group 17 forms -1 ions. Group 16 forms -2 ions. Group 15 forms -3 ions. The names of monatomic anions end in ide.
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22. Naming and Writing Formulas for Anions
You Try It. Write the symbol and name for each of the following ions.
Element
Symbol of Ion
Name of Ion
Chlorine
Nitrogen
Oxygen
Cl-
Chloride ion
N3-
Nitride ion
O2-
Oxide ion
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23. Number of Electrons Lost or Gained
You Try It
Complete the following table.
Symbol of Ion
Name of Ion
Number of Electrons Lost or Gained
Sulfide ion
Cu+
Barium ion
Al3+
Iron(III) ion
Li+
Phosphide ion
S2-
2 e- gained
Copper(I) ion
1 e- lost
Ba2+
2 e- lost
Aluminum ion
3 e- lost
Fe3+
3 e- lost
Lithium ion
1 e- lost
P3-
3 e- gained
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24. Naming and Predicting Formulas for Binary Ionic Compounds
Binary ionic compounds usually consist of a metal, such as an alkali metal, bonded to a nonmetal, such as a halogen. They are electrically neutral. This means that the total positive charge is equal to the total negative charge. Empirical formulas are used to represent ionic compounds. An empirical formula is the simplest ratio in which the atoms combine to form a compound. They are named by naming the cation followed by the anion. ex. LiCl is lithium chloride, FeCl2 is iron(II) chloride
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25. a. K+, Cl- KCl Mg2+, S2- MgS Na+, N3- Na3N Al3+, S2- Al2S3 Sn4+, O2-
Examples: Write the formulas for the compounds formed between the following pairs of ions and then name the compound.
a. K+, Cl-
Mg2+, S2-
Na+, N3-
Al3+, S2-
Sn4+, O2-
KCl
MgS
Na3N
Al2S3
SnO2
potassium chloride
magnesium sulfide
sodium nitride
aluminum sulfide
tin(IV) oxide
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26. You Try It Sodium bromide Magnesium sulfide c. Copper(I) chloride
Write the formulas for the following binary ionic compounds. Hint: First determine the symbols for the ions involved. Always write the cation first. The first one has been done for you as an example.
Sodium bromide
Magnesium sulfide
c. Copper(I) chloride
d. Calcium bromide
e. Strontium fluoride
Na+, Br-
Mg2+, S2-
Cu+, Cl-
Ca2+, Br-
Sr2+, F-
NaBr
MgS
CuCl
CaBr2
SrF2
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27. j. Chromium(VI) nitride Na+, O2- Pb2+, Br- Zn2+, S2- Al3+, O2-
You Try It
Write the formulas for the following binary ionic compounds. Hint: First determine the symbols for the ions involved. Always write the cation first. The first one has been done for you as an example.
f. Sodium oxide
g. Lead(II) bromide
h. Zinc sulfide
i. Aluminum oxide
j. Chromium(VI) nitride
Na+, O2-
Pb2+, Br-
Zn2+, S2-
Al3+, O2-
Cr6+, N3-
Na2O
PbBr2
ZnS
Al2O3
CrN2
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28. Roman Numerals
So far, you have been given examples where the Roman numeral has been indicated either by the name of the compound or by the symbol of the cation. But how do you determine the charge of the Roman numeral if it is not given to you?
To determine the charge of the Roman numeral you have to first identify the ions making up the compound.
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29. Roman Numerals Examples. Iron(III) oxide Fe2O3 Cu2S Copper(I) sulfide
Ions
Chemical Formula
Name of Compound
Fe3+, O2-
Cu+, S2-
CoI2
Tin(IV) oxide
FeS
Cu3N
Fe2O3
Iron(III) oxide
Cu2S
Copper(I) sulfide
Co2+, I-
Cobalt(II) iodide
Sn4+, O2-
SnO2
Fe2+, S2-
Iron(II) sulfide
Cu+, N3-
Copper(I) nitride
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30. You Try It Li+, O2- Li2O SnS2 Sn4+, S2- Ba2+, N3- Ba3N2 Na+, F- NaF
Write formulas for the following compounds. Remember to determine the ions involved first.
Name of Compound
Ions
Formula of Compound
Lithium oxide
Tin(IV) sulfide
Barium nitride
Sodium fluoride
Li+, O2-
Li2O
SnS2
Sn4+, S2-
Ba2+, N3-
Ba3N2
Na+, F-
NaF
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31. You Try It Name the following compounds. a. CaS b. FeN c. K2O d. PbO
Calcium sulfide
Iron(III) nitride
Potassium oxide
Lead(II) oxide
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32. Naming and Writing Formulas for Ternary Ionic Compounds
Ternary ionic compounds contain more than two elements. They usually contain one or more polyatomic ions.
POLYATOMIC IONS
Name of Ion
Symbol
Acetate
C2H3O2-, CH3COO-
Hyroxide
OH-
Ammonium
NH4+
Hypochlorite
ClO-
Carbonate
CO32-
Nitrate
NO3-
Chlorate
ClO3-
Nitrite
NO2-
Chlorite
ClO2-
Perchlorate
ClO4-
Chromate
CrO42-
Permanganate
MnO4-
Cyanide
CN-
Phosphate
PO43-
Dichromate
Cr2O72-
Sulfate
SO42-
Hydrogen Carbonate
HCO3-
Sulfite
SO32-
Note: You are expected to be able to use this list to help you determine the names/symbols of polyatomic ions not given in the list.
Predict the symbol for each of the following polyatomic ions.
Bromate ion
Phosphite ion
BrO3-
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PO33-

33. Writing the Formulas and Naming Ternary Ionic Compounds
Writing the formulas and naming ternary ionic compounds is just like writing the formula and naming binary ionic compounds. To write the formula, you write the symbol and charge of the ions involved and then balance the charges. To name the compound, you name the ions.
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34. Naming and Writing Formulas for Ternary Ionic Compounds
Examples:
a. K+, NO3-
b. Ba2+, PO43-
KNO3
Ba3(PO4)2
Potassium nitrate
Barium phosphate
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35. You Try It
1. Write the formulas for the following ternary ionic compounds, given the ions involved then name the compounds.
a. Ca2+, SO42-
b. K+, PO43-
c. NH4+, N3-
d. Fe3+, SO42-
CaSO4
K3PO4
(NH4)3N
Fe2(SO4)3
Calcium Sulfate
Potassium Phosphate
Ammonium nitride
Iron(III) sulfate
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36. You Try It
2. Write the formulas for the following ternary ionic compounds given their names.
Lithium hypochlorite
Sodium sulfite
Calcium acetate
Barium phosphate
Copper(II) nitrite
Li+, ClO-
Na+, SO32-
Ca2+, C2H3O2-
Ba2+, PO43-
Cu2+, NO2-
LiClO
Na2SO3
Ca(C2H3O2)2
Ba3(PO4)2
Cu(NO2)2
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37. You Try It 3. Name the following compounds. a. Ca(NO3)2 b. K2SO4
c. PbSO3
d. NaC2H3O2
e. (NH4)2S
Calcium nitrate
Potassium sulfate
Lead(II) sulfite
Sodium Acetate
Ammonium sulfide
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38. Daily Starter (12/5 & 12/6)
Lithium chloride
Magnesium sulfide
1. Name the following compounds.
a. LiCl
b. MgS
c. Cu2O
d. BaCO3
e. Fe(NO3)3
Copper(I) oxide
Barium carbonate
Iron(III) nitrate

39. Daily Starter (12/5 & 12/6) Na3N Li3PO4 Sn(CO3)2 CaS Pb(NO3)2
Write the chemical formula for each of the following compounds.
a. Sodium nitride
b. Lithium phosphate
c. Tin(IV) carbonate
d. Calcium sulfide
e. Lead(II) nitrate
Na3N
Li3PO4
Sn(CO3)2
CaS
Pb(NO3)2

40. Metallic Bonding
Metals have some characteristics that distinguish them from nonmetals. Name some properties of metals. Good conductors of heat and electricity Ductile: Capable of being drawn into fine wires Malleable: Capable of being shaped (hammered) without breaking
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41. Metallic Bonding and Sea of Electrons
Metals have these properties because metal atoms form a special type of bond with each other called a metallic bond. In metallic bonding, metal atoms don’t lose their valence electrons. The metal atoms release their valence electrons into a “sea of electrons” shared by all of the metal atoms.
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42. Metallic Bonding and Sea of Electrons
The electrons are said to be delocalized because they are not held in one “locality” as part of a specific ion or covalent bond.
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43. Metallic Bonding and Sea of Electrons
Metallic bonding between different metals results in the formation of solutions, also called alloys.
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44. Explaining Metallic Properties - Hardness
The hardness of a metal is determined by the number of delocalized valence electrons. The alkali metals are very soft metals which can be easily cut by a knife. This is due to the fact that the alkali metals only have one valence electron per atom.
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45. Explaining Metallic Properties - Luster
The delocalized valence electrons interact readily with light, creating the luster of metals.
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46. Explaining Metallic Properties Malleability and Ductility
The delocalized valence electrons of a metal are spread more or less uniformly throughout the metal. When a piece of metal is subjected to pressure, the positive cores of the atoms slide past each other but are still held together by the delocalized sea of electrons.
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47. Why aren’t ionic compounds malleable?
If an ionic compound is struck with a hammer, the blow tends to push ions of like charge together. they repel, and the crystal shatters.
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48. Explaining Metallic Properties Conductivity of Metals
Because the valence electrons of all metal atoms are not attached to any one metal atom, they can move easily through the metal when an external force, such as that provided by a battery, is applied.
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49. Why aren’t molecular or ionic compounds good conductors?
In molecular compounds, the valence electrons are localized in electron pair bonds between neutral atoms. In ionic compounds, the electrons are bound to individual ions that are held in place in crystal structures. Since the electrons are not free to move throughout the solid, ionic and molecular compounds are not good conductors of heat and electricity.
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50. Naming Bases
Bases are compounds that produce hydroxide ions (OH-) in water. Bases are named by naming the metallic ion and adding the word hydroxide. Example: LiOH Lithium hydroxide
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51. Write names for the following bases.
You Try It
Write names for the following bases.
NaOH
KOH
Mg(OH)2
CuOH
Sodium hydroxide
Potassium hydroxide
Magnesium hydroxide
Copper(I) hydroxide
An exception is NH3.
This is ammonia.
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52. Writing Formulas for Bases
Balance the charges as you would other ionic compounds. Example: Strontium hydroxide Sr2+, OH- Sr(OH)2
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53. Write the formulas for the following bases.
You Try It
Write the formulas for the following bases.
Tin(II) hydroxide
Lithium hydroxide
Barium hydroxide
Tin(IV) hydroxide
Sn2+, OH-
Li+, OH-
Ba2+, OH-
Sn4+, OH-
Sn(OH)2
LiOH
Ba(OH)2
Sn(OH)4
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54. Naming Binary Acids (H + Nonmetal)
Acids are compounds that produce hydrogen ions (H+) in water. Binary acids contain hydrogen and a nonmetal – they do not contain oxygen. Binary acids are named by using the prefix hydro, then the root followed by the ic suffix. Example: HBr hydrobromic acid
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55. Write names for the following binary acids.
You Try It
Write names for the following binary acids.
HCl HI
H2S
Hydrochloric acid
Hydroiodic acid
Hydrosulfuric acid
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56. Writing Formulas for Binary Acids
Balance the charges just as you did for ionic compounds. Example: Hydrophosphoric acid H+, P3- H3P
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57. Write the formulas for the following binary acids.
You Try It
Write the formulas for the following binary acids.
Hydrofluoric acid
Hydroselenic acid
H+, F-
H+, Se2- HF
H2Se
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58. Naming Oxyacids (H + Polyatomic Ion)
Oxyacids contain polyatomic ions. The name indicates the number of oxygen atoms in each molecule and the nonmetallic element present. Suffixes and prefixes are used to indicate the number of oxygen atoms present.
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59. Naming Oxyacids
In order to name oxyacids, it is important to known the name of the polyatomic ion from which the acid is formed.
Note: Not all forms of a polyatomic ion are given on your state formula chart.
Note: The common polyatomic ions for bromine and iodine, follow the same pattern as chlorine.
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60. Example – Naming the Acids of Chlorine
Ion
Name of Ion
Formula of Acid
Name of Acid
ClO3-
chlorate
ClO2-
chlorite
ClO-
hypochlorite
ClO4-
perchlorate
Cl-
chloride
HClO3
chloric acid
HClO2
chlorous acid
HClO2
hypochlorous acid
HClO4
perchloric acid
HCl
hydrochloric acid
(This is a binary acid)

61. Examples to be Worked Together
a. HNO3 b. H3PO3
nitric acid (-ate ion)
phosphorous acid (-ite ion)
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62. Name the following acids.
You Try It
Name the following acids.
sulfurous acid
nitrous acid
phosphoric acid
Iodous acid
a. H2SO3 b. HNO2 c. H3PO4 d. HIO2
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63. Writing Formulas for Oxyacids
Identify the polyatomic ion
Balance the charges just as you did for ionic compounds.
Example: Carbonic Acid
-ic comes from ate
Carbonate is CO32-
H+, CO H2CO3
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64. Write the formulas for the following acids.
You Try It
Write the formulas for the following acids.
Bromous acid
Periodic acid
Carbonous acid
Acetic Acid
H+, BrO2-
H+, IO4-
H+, CO22-
H+, C2H3O2-
HBrO2
HIO4
H2CO2
HC2H3O2
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