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4 years ago

Which of the following Group 15 elements has the greatest metallic character?

Chemistry

2 answers:

vfiekz [6]4 years ago

8 0

Answer:

4. Bi

Explanation:

The elements in Group 15 (VA)show a marked progression from nonmetallic to metallic properties with increasing atomic number.

romanna [79]4 years ago

5 0

The answer is no. 4. Bismuth (Bi)
Across the period, from left to right, metallic character decreases, meaning, when it is going down, the last element in a group will have the most metallic character. Since Bismuth (bi) is the last element, it is the most metallic. The arrangement of the group 15 elements in ascending rate of metallic character is: N (Nitrogen) P (Phosphorus), As (Arsenic), Sb (Antimony) and Bi (Bismuth). Bismuth has the lowest rate of electronegativity and ionization energy thus, it is more likely to lose an e- than the rest of the elements of the said group, which is why it is considered the most metallic.

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Vikki [24]

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4 years ago

Predict (to 3 sig figs) the isochoric specific heat of gaseous SF6 (molar mass 146.06 g/mol) at 1200 K, assuming that at this te

bazaltina [42]

Explanation:

As it is known that $SF_{6}$ molecule is a non-linear molecule. Therefore, its isochoric heat capacity will be as follows.

$C_{v} = \frac{3}{2}R + \frac{3}{2}R + (3 \times 7 - 6)R$

= $\frac{3}{2}R + \frac{3}{2}R + 15R$

= 18 R

Also, $C_{V} = M \times C_{v}$

where, $C_{V}$ = molar heat capacity

M = molecular mass

$C_{v}$ = specific heat

Hence, calculate the value of $C_{v}$ as follows.

$C_{V} = M \times C_{v}$

$8 \times 8.314 \times 10^{7} = 146.06 \times C_{v}$

$C_{v} = 10.2 \times 10^{6} erg. K^{-1}. gm^{-1}$

This means that value of isochoric specific heat is $10.2 \times 10^{6} erg. K^{-1}. gm^{-1}$ .

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dU = $nC_{v}dT$

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3 years ago

The following forces act on an object: 3N left, 2N up, 1N right, 2N down.

Ymorist [56]

The answer is 2N left.

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4 years ago

Lime is a term that includes calcium oxide (cao, also called quicklime) and calcium hydroxide (ca(oh)2 also called slaked lime).

antiseptic1488 [7]

Answer: - 986.6 kj/mol

Explanation:

1) Equation given:

CaO(s) + H₂O (l) → Ca (OH)₂ (s) δh⁰ = −65.2 kj/mol

2) Standard enthalpies of formation given:

CaO, δhf⁰ = −635.6 kj/mol

H₂O, δhf⁰ = −285.8 kj/mol

3) Calculate the standard enthalpy of formation of Ca(OH)₂.

δh⁰ = ∑δh⁰f of products - ∑ δh⁰f of reactants

Using the mole coefficients of the balanced chemical equation:

δh⁰ = δh⁰f Ca(OH)₂ - δh⁰f CaO - δh⁰f H₂O

⇒ δh⁰f Ca(OH)₂ = δh⁰ + δh⁰f CaO + δh⁰f H₂O

⇒ δh⁰f Ca(OH)₂ = - 65.2 kj/mol − 635.6 kj/mol) − 285.8 kj/mol) = - 986.6 kj/mol.

4 0

3 years ago

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sdas [7]

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