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4 years ago

Explain why most metals are malleable and ductile but ionic crystals are not

2 answers:

7 0

Throughout the metallic structure allowing the atoms to slide past each other. This sliding is why metals are ductile and malleable. Ioniccompound must break bonds to slide past one another, which causes the ionic material to split and crack.

Yuki888 [10]4 years ago

6 0

Answer:

Metals are malleable due to the layers of atoms which can move over each other. Ionic crystals are made of rigid lattice structures

Explanation:

The molecular structure of metals consists of metallic ions in a sea of de-localized electrons. The ions are closely packed in a regular arrangement. The layers of ions are held together due to the electrostatic forces between the ions and electrons. The layers of ions are not bonded to each other directly, which allows them to move when force is applied. This is why metals are malleable

Ionic crystals are strongly bonded lattice structures with oppositely charged ions strongly attracted to each other. As the ions are bonded directly to each other, the application of a force has the potential to break existing bonds, making the structure brittle.

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PLS HELP!

Nadya [2.5K]

Question 1

Fe(III) forms a chelate complex with salicylic acid which has purple color. therefore, when a solution is made either with salicylic acid or with aspirin having trae amount of salicylic acid in it, we see color formation in solution due to the resulting complex formed.

Question 2

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2 years ago

6 Fe2+ (aq) + Cr2O72− (aq) + 14 H+ (aq) → 6 Fe3+ (aq) + 2 Cr3+ (aq) + 7 H2O (aq) If the titration of 23 mL of an iron(II) soluti

ratelena [41]

Answer:

1.047 M

Explanation:

The given reaction:

$6Fe^{2+}_{(aq)}+Cr_2O_7^{2-}_{(aq)}+14H^+_{(aq)}\rightarrow 6Fe^{3+}_{(aq)}+2Cr^{3+}_{(aq)}+7H_2O_{(aq)}$

For dichromate :

Molarity = 0.254 M

Volume = 15.8 mL

The conversion of mL to L is shown below:

1 mL = 10⁻³ L

Thus, volume = 15.8 ×10⁻³ L

Thus, moles of dichromate :

$Moles=0.254 \times {15.8\times 10^{-3}}\ moles$

Moles of dichromate = 0.0040132 moles

1 mole of dichromate react with 6 moles of iron(II) solution

Thus,

0.0040132 moles of dichromate react with 6 × 0.0040132 moles of iron(II) solution

Moles of iron(II) solution = 0.02408 moles

Volume = 23 mL = 0.023 L

Considering:

$Molarity=\frac{Moles\ of\ solute}{Volume\ of\ the\ solution}$

<u>Molarity = 0.02408 / 0.023 = 1.047 M</u>

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3 years ago