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Bond [772]
3 years ago
8

Which trend is observed as the first four elements in group 17 on the periodic table are considered in order of increasing atomi

c number
Chemistry
1 answer:
ExtremeBDS [4]3 years ago
4 0

ANSWER:

The melting and boiling points increase in order of increasing atomic number.

The size of the nucleus increases in order of increasing atomic number.

Ionization energy decreases in order of increasing atomic number.

Electronegativity decreases in order of increasing atomic number.

Electron Affinity decreases in order of increasing atomic number.

The reactivities decrease in order of increasing atomic number.

EXPLANATION:

NAME     MELTING POINT    BOILING POINT

Fluorine    -220              -188

Chlorine          -101                       -35

Bromine           -7.2                58.8

Iodine            114                184

Melting and Boiling points increase as shown above.

NAME     COVALENT RADIUS    IONIC RADIUS

Fluorine    71                        133

Chlorine          99                          181

Bromine           114                  196

Iodine            133                 220

Size increases as shown above.

NAME            FIRST IONIZATION ENERGY

Fluorine              1681

Chlorine             1251

Bromine              1140

Iodine               1008

Ionization energy decreases as shown above.

NAME        ELECTRONEGATIVITY

Fluorine     4

Chlorine           3

Bromine           2.8

Iodine            2.5

Electronegativity decreases as shown above.

NAME      ELECTRON AFFINITY

Fluorine    -328.0

Chlorine    -349.0

Bromine    -324.6

Iodine     -295.2

Electron affinity decreases as shown above.

REACTIVITY

The reactivities of the halogens decrease. This is due to the fact that atomic radius increases in proportion with an increase of electronic energy levels. This decreases the pull for valence electrons of other atoms, minimizing reactivity.

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Calculate the volume (liters) of solution that can be prepared from 180. grams of K2Cr2O7 for a 0.200M solution.
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Answer:

The volume of the solution is 0.305 liters.

Explanation:

Molar mass is the amount of mass that a substance contains in one mole. The molar mass of K₂Cr₂O₇ is 294 g / mole. Then you can apply the following rule of three: if by definition of molar mass 294 grams of the compound are contained in 1 mole, 180 grams are contained in how many moles?

moles=\frac{180 grams*1mole}{294 grams}

moles= 0.61

Molarity is a measure of the concentration of a substance that is defined as the number of moles contained in a certain volume. So, the molarity of a solution is calculated by dividing the moles of the solute by the volume of the solution:

molarity=\frac{number of moles of solute}{volume}

Molarity is expressed in units \frac{moles}{liter}.

In this case:

  • molarity= 2 M
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Replacing in the definition of molarity:

2 M=\frac{0.61 moles}{volume}

Solving:

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<u><em>The volume of the solution is 0.305 liters.</em></u>

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3. Given 20g of Barium Hydroxide, how many grams of
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The number of grams of ammonium nitrate (NH₄NO₃) it would take for all the barium hydroxide to react is 18.7g

First, we will write the balanced chemical equation for the reaction

The balanced chemical equation for the reaction is

Ba(OH)₂ + 2NH₄NO₃ → 2NH₄OH + Ba(NO₃)₂

This means, 1 mole of barium hydroxide is required to react with 2 moles of ammonium nitrate

Now, we will calculate the number of moles of barium hydroxide present.

Mass of barium hydroxide (Ba(OH)₂) = 20 g

Using the formula

Number\ of\ moles = \frac{Mass}{Molar\ mass}

Molar mass of Ba(OH)₂ = 171.34 g/mol

∴ Number of moles of Ba(OH)₂ present =\frac{20}{171.34}

Number of moles of Ba(OH)₂ present = 0.116727 mole

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Since 1 mole of barium hydroxide is required to react with 2 moles of ammonium nitrate

Then,

0.116727 mole of barium hydroxide will react with 2 × 0.116727 mole of ammonium nitrate

2 × 0.116727 = 0.233454 mole

∴ Number of moles of NH₄NO₃ required is 0.233454 mole

Now, for the mass of ammonium nitrate (NH₄NO₃) required

From the formula

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Molar mass of NH₄NO₃ = 80.043 g/mol

∴ Mass of NH₄NO₃ required = 0.233454 × 80.043

Mass of NH₄NO₃ required = 18.68636 g

Mass of NH₄NO₃ required ≅ 18.7g

Hence, the number of grams of ammonium nitrate (NH₄NO₃) it would take for all the barium hydroxide to react is 18.7g

Learn more on determining mass of reactant required here: brainly.com/question/11232389

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