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3 years ago

What is true of a covalent bond? (03.03)

Chemistry

2 answers:

garri49 [273]3 years ago

6 0

Answer:

I think B..

Explanation:

It is the sharing of electrons from one atom to another .

Brrunno [24]3 years ago

5 0

Answer:

The answer is b: It is the sharing of electrons by overlapping orbitals

Explanation:

The ionic bong involves the exchange of electrons from one atom to another to keep eight particles in their outermost orbit. In this way the atoms become stable. This happens between a metal, which losing electrons becomes a cation that now has a positive charge, and a non-metal, which accepting electrons becomes an anion that now has a negative charge. So the ionic bond is the electrostatic attraction between oppositely charged particle (cation and anion).

No chemical bond involves sharing neutrons between two nuclei. Chemical bonds occur between the electrons of atoms, which are found in the outer layer around the nuclei.

So, the correct answer is b: It is the sharing of electrons by overlapping orbitals. This happens between two non-metallic elements.

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A gas at 89C occupies a volume of 0.67 L. At least what temperature will the volume increase to 1.12 L

dybincka [34]

At temperature 332.13 °C

<h3>Further explanation</h3>

Charles's Law stated that :

When the gas pressure is kept constant, the gas volume is proportional to the temperature

$\tt \dfrac{V_1}{T_1}=\dfrac{V_2}{T_2}$

T₁ = 89 °C=89+273=362 K

V₁ = 0.67 L

V₂ = 1.12 L

$\tt T_2=\dfrac{V_2.T_1}{V_1}\\\\T_2=\dfrac{1.12\times 362}{0.67}=605.13~K=332.13~^oC$

7 0

3 years ago

What is the answer please

lorasvet [3.4K]

Atomic radius, potassium is farther down on the table

6 0

3 years ago

The solid fuel in the booster stage of the space shuttle is a mix- ture of ammonium perchlorate and aluminum powder. Upon igni-

nataly862011 [7]

Answer:

For A: The mass of aluminium required will be 183 g

For B: The mass of alumina produced will be $6.63\times 10^6g$

Explanation:

To calculate the number of moles, we use the equation:

$\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}$ .....(1)

For a:

Given mass of $NH_4ClO_4$ = 1.325 kg = 1325 g (Conversion factor: 1 kg = 1000 g)

Molar mass of $NH_4ClO_4$ = 117.50 g/mol

Putting values in equation 1, we get:

$\text{Moles of }NH_4ClO_4=\frac{1325g}{117.50g/mol}=11.28mol$

For the given chemical reaction:

$6NH_4ClO_4(s)+10Al(s)\rightarrow 5Al_2O_3(s)+3N_2(g)+6HCl(g)+9H_2O(g)$

By stoichiometry of the reaction:

6 moles of $NH_4ClO_4$ reacts with 10 moles of aluminium

So, 11.28 moles of $NH_4ClO_4$ will react with = $\frac{10}{6}\times 11.28=6.77mol$ of aluminium

Now, calculating the mass of aluminium by using equation 1, we get:

Molar mass of aluminium = 27.00 g/mol

Moles of aluminium = 6.77 moles

Putting values in equation 1, we get:

$6.77mol=\frac{\text{Mass of aluminium}}{27.00g/mol}\\\\\text{Mass of aluminium}=(6.77mol\times 27.00g/mol)=183g$

Hence, the mass of aluminium required will be 183 g

For b:

Given mass of aluminium = $3.500\times 10^3=3.5\times 10^6g$ (Conversion factor: 1 kg = 1000 g)

Molar mass of aluminium = 27.00 g/mol

Putting values in equation 1, we get:

$\text{Moles of aluminium}=\frac{3.5\times 10^6g}{27.00g/mol}=1.3\times 10^5mol$

For the given chemical reaction:

$6NH_4ClO_4(s)+10Al(s)\rightarrow 5Al_2O_3(s)+3N_2(g)+6HCl(g)+9H_2O(g)$

By stoichiometry of the reaction:

10 moles of aluminium produces 5 moles of alumina

So, $1.3\times 10^5mol$ of aluminium will react with = $\frac{5}{10}\times 1.3\times 10^5=6.5\times 10^4mol$ of alumina

Now, calculating the mass of alumina by using equation 1, we get:

Molar mass of alumina = 101.96 g/mol

Moles of alumina = $6.5\times 10^4mol$

Putting values in equation 1, we get:

$6.5\times 10^4mol=\frac{\text{Mass of alumina}}{101.96g/mol}\\\\\text{Mass of alumina}=(6.5\times 10^4mol\times 101.96g/mol)=6.63\times 10^6g$

Hence, the mass of alumina produced will be $6.63\times 10^6g$

6 0

3 years ago

What is the hydroxide ion concentration of a solution whose pOH is 6.42?

Sergeeva-Olga [200]

Answer : The hydroxide ion concentration of a solution is, $3.8\times 10^{-7}M$

Explanation :

As we know that:

pH : It is defined as the negative logarithm of hydrogen ion concentration.

Mathematically,

$pH=-\log [H^+]$

Similarly,

pOH : It is defined as the negative logarithm of hydroxide ion concentration.

Mathematically,

$pOH=-\log [OH^-]$

Given:

pOH = 6.42

$6.42=-\log [OH^-]$

$[OH^-]=3.8\times 10^{-7}M$

Therefore, the hydroxide ion concentration of a solution is, $3.8\times 10^{-7}M$

7 0

3 years ago

What happens at a constant temperature, as time progresses?

Naddik [55]

4. it remains in its initial phase

4 0

3 years ago

Read 2 more answers