Questiona. Which TWO of these elements would form
1. ionic compound
RS
2. covalent compound $Q R$ b. For the compounds in (a) above,
1. draw their electronic structures, showing electrons in the outermost shell
2. explain which compound is more volatile in terms of the forces between particles

Studdy Solution

STEP 1

What is this asking? We need to figure out which of these elements make ionic and covalent compounds, draw their electron diagrams, and explain why one is more volatile than the other! Watch out! Don't mix up ionic and covalent compounds!
Remember, ionic compounds are formed by transferring electrons, while covalent compounds share electrons.

STEP 2

1. Identify Ionic and Covalent Pairs
2. Draw Electronic Structures
3. Explain Volatility

STEP 3

Alright, let's look at element P with atomic number $\text{10}$ .
That means it has $\text{10}$ electrons, arranged as $2, 8$ .
It's stable and happy, like a noble gas!

STEP 4

Element Q has an atomic number of $\text{14}$ , so its electron configuration is $2, 8, 4$ .
It needs four more electrons to complete its outer shell.

STEP 5

R has an atomic number of $\text{17}$ , giving it an electron configuration of $2, 8, 7$ .
It's just one electron away from a full outer shell!

STEP 6

Finally, S has an atomic number of $\text{19}$ , with an electron configuration of $2, 8, 8, 1$ .
It has one extra electron it's itching to give away!

STEP 7

Ionic compounds form between elements that want to give away electrons and elements that want to take electrons.
S wants to give one away, and R wants to take one!
So, S and R will form an ionic compound, SR.

STEP 8

Covalent compounds form when elements share electrons to complete their outer shells.
Q needs four electrons, and R needs one.
If Q shares four electrons with four different R atoms, they can all be happy!
But, if we only have one Q and one R, they can share two electrons to form a covalent compound, QR.

STEP 9

For the ionic compound SR, S loses its one outer electron to become $S^{+}$ , with a configuration of $2, 8, 8$ .
R gains that electron to become $R^{-}$ , with a configuration of $2, 8, 8$ .
We can draw this with S having a plus sign and 8 dots around it, and R having a minus sign and 8 dots around it.

STEP 10

For the covalent compound QR, Q shares two of its four outer electrons with two of R's outer electrons.
We can draw this with overlapping circles.
Q has 6 dots around it, and R has 8 dots around it, with 2 dots in the overlapping section.

STEP 11

Volatility refers to how easily a substance turns into a gas.
This depends on the forces between the particles.

STEP 12

Ionic compounds like SR have strong electrostatic forces between the positive and negative ions.
These strong forces make it hard to separate the ions, so ionic compounds have low volatility.

STEP 13

Covalent compounds like QR have weaker intermolecular forces between the molecules.
These weaker forces make it easier to separate the molecules, so covalent compounds have higher volatility compared to ionic compounds.

STEP 14

a. 1. Ionic Compound: SR 2. Covalent Compound: QR
b. 1. Electronic structures are as described in the steps above (SR: S with + and 8 dots, R with - and 8 dots; QR: Q with 6 dots, R with 8 dots, 2 shared). 2. QR is more volatile than SR because it has weaker intermolecular forces compared to the strong electrostatic forces in the ionic compound SR.

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Questiona. Which TWO of these elements would form
1. ionic compound
RS
2. covalent compound $Q R$ b. For the compounds in (a) above,
1. draw their electronic structures, showing electrons in the outermost shell
2. explain which compound is more volatile in terms of the forces between particles

Studdy Solution

STEP 1

STEP 2

1. Identify Ionic and Covalent Pairs
2. Draw Electronic Structures
3. Explain Volatility

STEP 3

Alright, let's look at element P with atomic number $\text{10}$ .
That means it has $\text{10}$ electrons, arranged as $2, 8$ .
It's stable and happy, like a noble gas!

STEP 4

Element Q has an atomic number of $\text{14}$ , so its electron configuration is $2, 8, 4$ .
It needs four more electrons to complete its outer shell.

STEP 5

R has an atomic number of $\text{17}$ , giving it an electron configuration of $2, 8, 7$ .
It's just one electron away from a full outer shell!

STEP 6

Finally, S has an atomic number of $\text{19}$ , with an electron configuration of $2, 8, 8, 1$ .
It has one extra electron it's itching to give away!

STEP 7

Ionic compounds form between elements that want to give away electrons and elements that want to take electrons.
S wants to give one away, and R wants to take one!
So, S and R will form an ionic compound, SR.

STEP 8

STEP 9

STEP 10

For the covalent compound QR, Q shares two of its four outer electrons with two of R's outer electrons.
We can draw this with overlapping circles.
Q has 6 dots around it, and R has 8 dots around it, with 2 dots in the overlapping section.

STEP 11

Volatility refers to how easily a substance turns into a gas.
This depends on the forces between the particles.

STEP 12

Ionic compounds like SR have strong electrostatic forces between the positive and negative ions.
These strong forces make it hard to separate the ions, so ionic compounds have low volatility.

STEP 13

Covalent compounds like QR have weaker intermolecular forces between the molecules.
These weaker forces make it easier to separate the molecules, so covalent compounds have higher volatility compared to ionic compounds.

STEP 14

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Questiona. Which TWO of these elements would form1. ionic compoundRS2. covalent compound QRQ RQR b. For the compounds in (a) above,1. draw their electronic structures, showing electrons in the outermost shell2. explain which compound is more volatile in terms of the forces between particles

Studdy Solution

STEP 1

STEP 2

1. Identify Ionic and Covalent Pairs2. Draw Electronic Structures3. Explain Volatility

STEP 3

Alright, let's look at element P with atomic number 10\text{10}10.That means it has 10\text{10}10 electrons, arranged as 2,82, 82,8.It's stable and happy, like a noble gas!

STEP 4

Element Q has an atomic number of 14\text{14}14, so its electron configuration is 2,8,42, 8, 42,8,4.It needs four more electrons to complete its outer shell.

STEP 5

R has an atomic number of 17\text{17}17, giving it an electron configuration of 2,8,72, 8, 72,8,7.It's just one electron away from a full outer shell!

STEP 6

Finally, S has an atomic number of 19\text{19}19, with an electron configuration of 2,8,8,12, 8, 8, 12,8,8,1.It has one extra electron it's itching to give away!

STEP 7

Ionic compounds form between elements that want to give away electrons and elements that want to take electrons.S wants to give one away, and R wants to take one!So, S and R will form an **ionic compound**, SR.

STEP 8

STEP 9

STEP 10

For the **covalent compound** QR, Q shares two of its four outer electrons with two of R's outer electrons.We can draw this with overlapping circles.Q has 6 dots around it, and R has 8 dots around it, with 2 dots in the overlapping section.

STEP 11

**Volatility** refers to how easily a substance turns into a gas.This depends on the forces between the particles.

STEP 12

Ionic compounds like SR have strong **electrostatic forces** between the positive and negative ions.These strong forces make it hard to separate the ions, so ionic compounds have **low volatility**.

STEP 13

Covalent compounds like QR have weaker **intermolecular forces** between the molecules.These weaker forces make it easier to separate the molecules, so covalent compounds have **higher volatility** compared to ionic compounds.

STEP 14

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Questiona. Which TWO of these elements would form
1. ionic compound
RS
2. covalent compound $Q R$ b. For the compounds in (a) above,
1. draw their electronic structures, showing electrons in the outermost shell
2. explain which compound is more volatile in terms of the forces between particles

1. Identify Ionic and Covalent Pairs
2. Draw Electronic Structures
3. Explain Volatility

Alright, let's look at element P with atomic number $\text{10}$ .
That means it has $\text{10}$ electrons, arranged as $2, 8$ .
It's stable and happy, like a noble gas!

Element Q has an atomic number of $\text{14}$ , so its electron configuration is $2, 8, 4$ .
It needs four more electrons to complete its outer shell.

R has an atomic number of $\text{17}$ , giving it an electron configuration of $2, 8, 7$ .
It's just one electron away from a full outer shell!

Finally, S has an atomic number of $\text{19}$ , with an electron configuration of $2, 8, 8, 1$ .
It has one extra electron it's itching to give away!

Ionic compounds form between elements that want to give away electrons and elements that want to take electrons.
S wants to give one away, and R wants to take one!
So, S and R will form an ionic compound, SR.

For the covalent compound QR, Q shares two of its four outer electrons with two of R's outer electrons.
We can draw this with overlapping circles.
Q has 6 dots around it, and R has 8 dots around it, with 2 dots in the overlapping section.

Volatility refers to how easily a substance turns into a gas.
This depends on the forces between the particles.

Ionic compounds like SR have strong electrostatic forces between the positive and negative ions.
These strong forces make it hard to separate the ions, so ionic compounds have low volatility.

Covalent compounds like QR have weaker intermolecular forces between the molecules.
These weaker forces make it easier to separate the molecules, so covalent compounds have higher volatility compared to ionic compounds.