What element has the least metallic character B,C,F,Li or Na?

Answers

Answer 1

Answer: In the periodic table of the elements, the element from left to right at the same period, the metallic character decreases. And from up to down, at the same column, it increases. So the answer is Na.

Answer 2

Answer:

Final answer:

Among B, C, F, Li, and Na, Fluorine (F) has the least metallic character as it is the most nonmetallic element on the Periodic Table. This is related to its high electronegativity, which is a characteristic of nonmetals.

Explanation:

The element with the least metallic character out of B, C, F, Li, or Na would be Fluorine (F). In the Periodic Table, metallic character decreases as you move across a period from left to right and increases as you go down a group. Fluorine is located at the top right corner of the Periodic Table, which makes it the most nonmetallic element not only among B, C, F, Li and Na, but also in the entire Periodic Table.

This is because Fluorine has the highest electronegativity, meaning it has a high propensity to attract electrons in a bond. This is a property of nonmetals, in contrast to metals which tend to lose electrons.

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Gas occupies 30 Liters at 2.0 atm pressure and 27° Celsius. How many moles of gas are present

Answers

Your answer to this question is 2.44 mol.

The digestion process starts in the _____. A.esophagus
B.stomach
C.small intestine
D.mouth

Answers

The digestion process starts in the mouth first, with the mechanical digestion happening with your teeth. And then the saliva breaks down your food with its enzymes.

What is the temperature of 1.2 moles of Helium gas at 1950 mm Hg if it occupies 15,500 ml of volume?

Answers

Answer:

$T=404.16K=13.1^oC$

Explanation:

Hello,

In this case, we use the ideal gas equation to compute the requested temperature as shown below and considering the proper units:

$PV=nRT\nT=(PV)/(nR)=(1950mmHg*(1atm)/(760mmHg)*15500mL*(1L)/(1000mL) )/(1.2mol*0.082 (atm*L)/(mol*K) ) \nT=404.16K=13.1^oC$

Best regards.

Replace with

1950

1950mmHg and simplify.

1.2

1950

500

[17]. Trimix 10/50 is a gas mixture that contains 10% oxygen and 50% helium, and the rest is nitrogen. If a tank of Trinix 10/50 has a total pressure of 2.07 x 10^4 kPa, then what is the partial pressure of nitrogen? a). 1.04 x 10^4 kPa
x b). 8.3 x 10^3 kPa
c). 2.07 x 10^3 kPa
d). 2.07 x 10^4 kPa

Answers

The answer is B. 8.3x10^3 kPa. The partial pressure of a specific gas in a gas mixture is equivalent to product of its mole fraction and total pressure of the mixture. Since it was stated that the mixture is 10% oxygen, 50% helium, and the rest nitrogen, it can be determined that nitrogen is 40% of the mixture. So 40% of 2.07x10^4 kPa is 8.3x10^3 kPa.

Answer:

A) 1.04 x 10^4 kPa

Explanation:

I'm not exactly sure how but I took the test and this was the correct answer. My calculations said it was B as well but I guess not...

What is the total mass of oxygen in 1.00 mole of Al2(CrO4)3

Answers

1 mol of this atom would yield 12 moles of Oxygen, (using the number of atoms that they gave in 1 molecule of Al2(CrO4)3. Therefore, the atomic mass of Oxygen is 16, and there are 12 moles of Oxygen atoms. In total, the mass would be 12 * 16 = 192 grams of Oxygen.

Final answer:

The compound Al2(CrO4)3 contains 12 oxygen atoms per formula unit. Knowing that one mole of oxygen atoms has a mass of 16.00 grams, the total mass of oxygen in 1.00 mole of Al2(CrO4)3 is $12 * 16.00 = 192.00$ grams.

Explanation:

The primary task here is to find the total mass of oxygen in 1.00 mole of Al2(CrO4)3. This is a classic chemistry problem that involves understanding the composition and molar mass of compounds. In the compound Al2(CrO4)3, the subscript 3 after (CrO4) means there are three chrome tetraoxides in one formula unit of the compound.

Every CrO4 ion is composed of one chromium atom and four oxygen atoms. Therefore, three CrO4 ions will contain 3 * 4 = 12 oxygen atoms.

Knowing that one mole of oxygen atoms weighs approximately 16.00 grams, we can find the total mass of oxygen in the compound by multiplying this molar mass by the number of oxygen atoms. Again, in one mole of Al2(CrO4)3 we have 12 oxygen atoms, hence $12 * 16.00 g = 192.00$ grams.

So, the total mass of oxygen present in 1.00 mole of Al2(CrO4)3 is 192.00 grams.

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How many grams of hydrogen peroxide (H2O2) must be added to 1,500 ml of water to produce a concentration of 1.33 m (molal solution)

Answers

I hope it helped you out.

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