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3 years ago

Hi:) why covalent substances don’t have free moving ions / electrons?

Chemistry

2 answers:

Igoryamba3 years ago

6 0

Answer:

Covalent compounds don't contain ions because they make bonds by sharing electrons. In addition, they don't have any charge carries that are free to move so they can't carry electric current

Explanation:

blagie [28]3 years ago

6 0

Answer:

im confused

Explanation:

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EXPERIMENT 1: Identify the oxidation and reduction half-reactions that occur in

Hoochie [10]

Answer:

Cathode: Mn → Mn²⁺ + 2e⁻ (Oxidation)

Anode: Zn²⁺ + 2e⁻ → Zn (Reduction)

Mn | Mn²⁺ || Zn²⁺ | Zn

Explanation:

To identify the half reaction we need to see the oxidation states.

Mn(s) → Ground state → Oxidation state = 0

Mn(NO₃)₂ → Mn²⁺ → The oxidation state has increased.

This is the oxidation reaction. It has released two electrons:

Mn → Mn²⁺ + 2e⁻

Zn(NO₃)₂ → Zn²⁺

Zn → Ground state → The oxidation state was decreased.

This is the reduction reaction. It has gained two electrons:

Zn²⁺ + 2e⁻ → Zn

Cathode: Mn → Mn²⁺ + 2e⁻

Anode: Zn²⁺ + 2e⁻ → Zn

Mn | Mn²⁺ || Zn²⁺ | Zn

4 0

3 years ago

Many computer chips are manufactured from silicon, which occurs in nature as SiO2 . When SiO2 is heated to melting, it reacts wi

Ierofanga [76]

Answer:

a. Theoretical yield of Si = 72.58 kg

b. Percent Yield = 91.2 %

Explanation:

The chemical reaction involved is: SiO₂ (l) + 2C (s) → Si (l) + 2CO (g)

The stoichiometric ratio = 1 mol SiO₂ ÷ 2 mol C = 0.5 mol SiO₂ ÷ 1 mol C

Given: mass of SiO₂: w₁ = 155.3kg = 155.3 × 10³g, mass of C: w₂ = 79.3kg = 79.3 × 10³g, mass of Si: w₃ = 66.2kg = 66.2 × 10³g (∵ 1 kg =1000g)

Molar mass of SiO₂: m₁ = 60.08 g/mol, atomic mass of C: m₂ = 12.01 g/mol, atomic mass of Si: m₃ = 28.08 g/mol

Number of moles of SiO₂ taken: n₁ = w₁ ÷ m₁ = 155300 g ÷ 60.08 g/mol = 2584.88 mol

Number of moles of C taken: n₂ = w₂ ÷ m₂ = 79300 g ÷ 12.01 g/mol = 6602.83 mol

Actual ratio = n₁ ÷ n₂ = 2584.88 mol SiO₂ ÷ 6602.83 mol C = 0.39 mol SiO₂ ÷ 1 mol C

Since the stoichiometric ratio > actual ratio

Therefore, SiO₂ is the limiting reagent.

Now, the mass of SiO₂ in 1 mol = number of moles × molar mass = 1 mol × 60.08 g/mol = 60.08 g

the mass of Si in 1 mol = number of moles × molar mass = 1 mol × 28.08 g/mol = 28.08 g

So 28.08 g of Si is produced from 60.08 g SiO₂

Therefore, the amount of Si produced from 155300 g SiO₂ = 155300 g × 28.08 g ÷ 60.08 g = 72583.62 g = 72.58 kg

Therefore, the theoretical yield of Si = 72.58 kg

Actual yield of Si = 66.2 kg

Therefore, Percent Yield = Actual yield ÷ Theoretical yield × 100 = 66.2 kg ÷ 72.58 kg × 100 = 91.2 %

3 0

3 years ago

1. we used __________ to represent an element.

scoundrel [369]

$▪▪▪▪▪▪▪▪▪▪▪▪▪ {\huge\mathfrak{Answer}}▪▪▪▪▪▪▪▪▪▪▪▪▪▪$

1. we used Symbol to represent an element.

2. The chemical formula of a molecule shows the number and kind of atoms contained in the molecule.

3. K (potassium) is the atom among the given choices.

4. CO (carbon - monoxide) is the molecule among given choices.

6 0

3 years ago

Read 2 more answers

5. Hydrogen & oxygen react chemically to form water. How much water

stepladder [879]

39.25 g of water (H₂O)

Explanation:

We have the following chemical reaction:

2 H₂ + O₂ → 2 H₂O

Now we calculate the number of moles of each reactant:

number of moles = mass / molar weight

number of moles of H₂ = 14.8 / 2 = 7.4 moles

number of moles of O₂ = 34.8 / 32 = 1.09 moles

We see from the chemical reaction that 2 moles of H₂ will react with 1 mole of O₂ so 7.4 moles of H₂ will react with 3.7 moles of O₂ but we only have 1.09 moles of O₂ available. The O₂ will be the limiting reactant. Knowing this we devise the following reasoning:

if 1 moles of O₂ produces 2 moles of H₂O

then 1.09 moles of O₂ produces X moles of H₂O

X = (1.09 × 2) / 1 = 2.18 moles of H₂O

mass = number of moles × molar weight

mass of H₂O = 2.18 × 18 = 39.25 g

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limiting reactant

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3 years ago

Need helpppppppppppppppppppppppppp with 3

ira [324]

Answer:

13. 8 hrs

12. 8.89 meters per second squared

11. -0.75 meters per second squared

7 0

2 years ago