Does Na2 gas posses metallic character? Explain your answer..​

Answer:

Cuando dos átomos se acercan entre sí, se genera un compuesto al compartir pares de electrones que cada uno de los átomos aporta, permitiéndoles alcanzar los 8 electrones de valencia (octeto) en su capa externa.

Explanation:

La configuración electrónica del elemento puede escribirse de la siguiente manera;

1s²2s²2p⁴

La configuración electrónica dada es equivalente a la del oxígeno, por lo tanto, tenemos;

El número de electrones en la capa de valencia = 2 + 4 = 6 electrones

Por consiguiente, cada átomo necesita 2 electrones para completar sus 8 electrones (octeto) en la capa externa.

Al acercarse los dos átomos, reaccionan y se combinan para formar un compuesto al compartir 4 electrones, 2 de cada átomo, de modo que cada átomo obtenga 2 electrones adicionales en su órbita externa en el nuevo compuesto y así se logre la configuración estable de octeto para cada uno de los átomos en el compuesto recién formado.

Answer:

1.5

Explanation:

It is given that:

Compound A and B originate from Sulfur + Oxygen.

Compound A:

6g sulfur + 5.99g Oxygen

Compound B:

8.6g sulfur + 12.88g oxygen

By comparing the ratios:

Compound A:

S: O = 6.00: 5.99

S/0 = 6.0g S / 5.99g O

Compound B:

S: O = 8.60: 12.88

S / O = 8.60g S / 12.88g O

The mass ratio of A and that of B

(6.0g S / 5.99g O) ÷ (8.60g S / 12.88g O)

(6.0 g S / 5.99g O) × (12.88g O / 8.60g S)

(6 × 12.88) / (5.99 × 8.60)

= 77.28 / 51.514

= 1.50017

= 1.5

(a)   Write the balanced half-reactions for the overall process:

Oxidation: Se^2- (aq) → Se (s) + 2e-

Reduction: 2So3^2- (aq) + 3H2O (l) + 4e- → S2O3^2- + 6OH- (aq)

(b)   Assuming E sulfite is 0.57 V, compute E selenium:

E anode = E cathode – E cell

= -0.57 – 0.35

= -.092

Solution:

The gas's new temperature is 604K

Justification:

Assuming standard temperature and pressure, we can determine the gas's temperature using the ideal gas law;

Step 1: Formulate the general gas law equation

P1V1/T1 = P2V2/T2

Step 2: Insert the values, converting as needed to standard units.

P1 = 0.800 atm

V1 = 0.180 L

T1 = 29°C = 273 + 29 = 302K

P2 = 3.20 atm

V2 = 90 mL = 90 * 10^-3 L = 0.09 L

Step 3: Solve for T2

The new gas temperature T2 is calculated as:

T2 = P2V2T1/(P1V1)

T2 = 3.20 * 0.09 * 302 / (0.800 * 0.180)

T2 = 86.976 / 0.144

T2 = 604K

The gas's new temperature is 604K.

Answer:

Number of moles of oxygen atoms that weigh the same as a glass of water = 3.12 moles

Note: This question lacks certain figures. Below is a complete similar question.

An oxygen atom weighs 2.66*10^-23 g and a glass of water weighs 0.050 kg. What is the weight of one mole of oxygen atoms? Round your result to three significant figures. How many moles of oxygen atoms have a weight equal to the weight of a glass of water? Round your answer to two significant figures.

Explanation:

One mole of a substance comprises the Avogadro number of particles, which is 6.02 * 10²³.

Hence, one mole of oxygen atoms contains 6.02*10²³ atoms.

Weight of a single oxygen atom = 2.66*10⁻²³ g

Weight of one mole of oxygen atoms = weight of a single atom multiplied by the number of atoms in one mole.

Weight of one mole of oxygen atoms = 2.66*10⁻²³ g * 6.02*10²³ = 16.01 g

A glass of water weighs = 0.050 kg or 50 g.

To calculate how many moles of oxygen atoms weigh the same as a glass of water (i.e., 50 g), the following formula is applied;

number of moles = mass/molar mass

mass of oxygen atoms = 50 g, molar mass or weight of one mole of oxygen atoms = 16.01 g

Thus, the number of moles of oxygen atoms = 50 g / 16.01 g = 3.12 moles