Ionic Solids Characteristics Ionic Solids Rigid crystalline structure Hard, brittle solids In the...
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![Page 1: Ionic Solids Characteristics Ionic Solids Rigid crystalline structure Hard, brittle solids In the molten or aqueous phase Conductivity In the solid phase.](https://reader036.fdocuments.in/reader036/viewer/2022082820/56649ef15503460f94c02c88/html5/thumbnails/1.jpg)
Ionic Solids Characteristics
Ionic Solids
Rigid crystallinestructure
Hard, brittle solids
In the molten or aqueous
phase
Conductivity
In the solid
phase
NoYes
Formed from a bond
between a metal
and nonmetal
Relatively High Melting Point
Strong Electrostatic Attractions
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The First Couple
• # 1) Energy is released when bonds are formed. Energy is absorbed when bonds are broken.
• #2) As a bond forms the PE decreases.
• #3) Energy is released -> stability increases
• #4) Two atoms combine to form a molecule, bond formed, energy is released
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#5 Which electron-dot diagram represents H2?
H H
H H
Both hydrogen’s will equally share their valence
electron
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#9) In which compound do the atoms have the greatest difference in electronegativity?
(1) NaBr |0.9 – 3.0| = 2.1
(3) KF |0.8 – 4.0| = 3.2
(2) AlCl3 |1.6 – 3.2| = 1.6
(4) LiI |1.0 – 2.7| = 1.7
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#13) Given the reaction:
M + 2H2O -> M(OH)2 + H2
The metal represented by M is most likely a metal from Group
M(OH)2
The subscript of 2 on the hydroxide came from the charge on
the metal (M).
M+2(OH)-1
So the Metal (M) must be from Group 2 because of its +2 oxidation state!
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3 Valence e-’s means that is will have an
oxidation state of +3
#16) Element X has an electron configuration of 2-8-3. This element will combine with the
phosphate ion to form a compound with the formula
X+3(PO4)-3 From Table
E: phosphate has a -3
X3(PO4)3Reduce
to Lowest
Ratio
Criss Cross w/out
charges
3 3
X (PO4)
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#33a.
b.
c.
H H
H HH2 is nonpolar and H2O is polar, like dissolves like, therefore H2 will not dissolve in H2O.
1 Mg + 1 H2SO4 1 H2 + 1 MgSO4
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#34
a. b.
HH HN
HH HN
H+
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#35
a.
b.
c. H-Cl is polar, water is polar; like dissolves like
H Cl
H Cl
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#36a.
OR
b. N2 is very stable, unreactive because of triple bond (a lot of energy was released when this bond was formed).
N NN N
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#6) Group 1 metals are highly reactive and form stable compounds.
#7) Na 1s22s22p63s1 1s22s22p6 Ne
Cl 1s22s22p63s23p5 1s22s22p63s23p6 Ar
Will become
Will become
ClCl
Na [Na]+1
-1
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#8. Radon is a group 2 (metal), it wants to lose its 2 valence electrons to a nonmetal.
1) Iodine – nonmetal, wants to gain 1 e-
2) Fluorine – nonmetal, wants to gain 1 e-
3) sodium – metal, wants to lose 1 e-
4) calcium – metal, wants to lose 2 e-
Of the 2 choices that want electrons choice 2 is more reactive, larger electronegativity, than choice 1. Fluorine is the answer (choice 2).
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#10) Which compound would most likely have the greatest ionic character?
(1) CO |2.6 – 3.5| = 0.9
(3) CaO |1.0 – 3.5| = 2.5
(2) KF |0.8 – 4.0| = 3.2
(4) LiH |1.0 – 2.1| = 1.1
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#11) Given the reaction H2 + Cl2 → 2HCl• Bond Breaking requires/absorbs energy.• Bond Formation releases/emits energy.
The H2 and Cl2 bonds are broken – requires energy!
The HCl bond is formed- releases energy!
The answer is choice (4) the forming of the HCl bond releases energy
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#12) Noble gases have the most stable electron configuration, choice 1 (Ne).
#14) In order for the electrons to have been transferred to Oxygen, the oxygen will have to be the most electronegative element and the ionic character of the compound would be 1.7 or greater.(1) CO2
|2.6 – 3.5| = 0.9
(2) N2O
|3.0 – 3.5| = 0.5
(2) NO2
|3.0 – 3.5| = 0.5
(4) Na2O
|0.9 – 3.5| = 2.6
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15) Compounds including polyatomic ions have covalent bonding within and ionic bonding to the
metal outside the parenthesis (brackets).
S
2-
OO O
OCa2+