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3 years ago

Compare strontium with rubidium in terms of the following properties:

Chemistry

1 answer:

Ilya [14]3 years ago

6 0

Answer:

Strontium is smaller

Strontium has the higher ionization energy

Strontium has more valence electrons

Explanation:

It must be understood that both elements belong to the same period i.e the same horizontal band of the periodic table

While Rubidium is an alkali metal(group 1) while Strontium is an alkali earth metal(group 2)

Since they are in the same period, periodic trends would be useful in evaluating their properties

In terms of atomic radius, rubidium is larger meaning it has a bigger atomic size

Generally, across the periodic table, atomic radius is expected to decrease and thus Rubidium which is leftmost is expected to have the higher atomic radius

Since strontium belongs to group 2 of the periodic table, it has 2 valence electrons which is more than the single valence electron that rubidium which is in group 1 has

In terms of ionization energy, the atom with the higher number of valence electrons will have the higher ionization energy which is strontium in this case

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Newton's first law of motion states that an object at rest will remain at rest unless an unbalanced force acts on it. If you apply balanced forces on the object there would be no net force. The body does not accelerate but instead stays at rest.

Another way to look at this problem is to use Newton's second law of motion. The first law states that $F = m\times a$ , where $a$ is the acceleration $F$ is the net force and $m$ is the mass of the object.

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2 years ago

The metals in Groups 1A, 2A, and 3A ____.

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3 years ago

The water cycle imagine you are a rain drop

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2 years ago

What mass of iron is needed to react with sulfur in order to produce 96 grams of

fiasKO [112]

Answer:

51.69 g of Fe

Explanation:

We'll begin by writing the balanced equation for the reaction. This is illustrated below:

2Fe + 3S —> Fe₂S₃

Next, we shall determine the mass of Fe that reacted and the mass of Fe₂S₃ produced from the balanced equation. This can be obtained as follow:

Molar mass of Fe = 56 g/mol

Mass of Fe from the balanced equation = 2 × 56 = 112 g

Molar mass of Fe₂S₃ = (2×56) + (3×32)

= 112 + 96

= 208 g/mol

Mass of Fe₂S₃ from the balanced equation = 1 × 208 = 208 g

SUMMARY:

From the balanced equation above,

112 g of Fe reacted to produce 208 g of Fe₂S₃.

Finally, we shall determine the mass of Fe needed to produce 96 g of Fe₂S₃. This can be obtained as follow:

From the balanced equation above,

112 g of Fe reacted to produce 208 g of Fe₂S₃.

Therefore, Xg of Fe will react to produce 96 g of Fe₂S₃ i.e

Xg of Fe = (112 × 96)/208

Xg of Fe = 51.69 g

Thus, 51.69 g of Fe is needed for the reaction.

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3 years ago

Given the balanced equation, 2 H2 + O2 -> 2 H2O, answer the following

9966 [12]

Answer: $O_2$ is the limiting reagent

Explanation:

To calculate the moles :

$\text{Moles of solute}=\frac{\text{given mass}}{\text{Molar Mass}}$

$\text{Moles of} H_2=\frac{10.0g}{2g/mol}=5.00moles$

$\text{Moles of} O_2=\frac{20.0g}{32g/mol}=0.625moles$

The balanced chemical reaction is :

$2H_2+O_2\rightarrow 2H_2O$

According to stoichiometry :

1 moles of $O_2$ require = 2 moles of $H_2$

Thus 0.625 moles of $O_2$ will require= $\frac{2}{1}\times 0.625=1.25moles$ of $H_2$

Thus $O_2$ is the limiting reagent as it limits the formation of product and $H_2$ is the excess reagent as it is present more than the required amount.

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3 years ago