Question

how does electronegativity change down the group? 1. label your x-axis as atomic number and the y-axis as the electronegativity. 2. go to table s. fill in the table below
element name | atomic number | electronegativity
lithium | |
beryllium | |
boron | |
fluorine | |

1. plot the data on your graph.

Explanation:

To solve this problem about electronegativity trends, we first need to fill in the table with the correct atomic numbers and electronegativity values for the given elements (using standard periodic table data) and then plot the graph. Here's the step - by - step process:

Step 1: Recall Atomic Numbers and Electronegativity Values

• Lithium (Li):
• The atomic number of lithium is 3.
• The electronegativity of lithium (on the Pauling scale) is approximately 0.98.
• Beryllium (Be):
• The atomic number of beryllium is 4.
• The electronegativity of beryllium (on the Pauling scale) is approximately 1.57.
• Boron (B):
• The atomic number of boron is 5.
• The electronegativity of boron (on the Pauling scale) is approximately 2.04.
• Fluorine (F):
• The atomic number of fluorine is 9.
• The electronegativity of fluorine (on the Pauling scale) is approximately 3.98.

Step 2: Fill in the Table

Element name	Atomic Number	Electronegativity
Beryllium	4	1.57
Boron	5	2.04
Fluorine	9	3.98

Step 3: Plot the Data on the Graph

• X - axis (Atomic Number): Mark the points 3 (for Li), 4 (for Be), 5 (for B), and 9 (for F) on the x - axis.
• Y - axis (Electronegativity): For each atomic number, find the corresponding electronegativity value on the y - axis and plot the points (3, 0.98), (4, 1.57), (5, 2.04), and (9, 3.98). Then, connect the points (if we consider the general trend, but note that fluorine is in a different period from Li, Be, and B. If we were looking at a group, we would have elements in the same group. However, for the purpose of plotting these given elements, we just plot the individual points).

Step 4: Analyze the Trend (Optional, but related to the initial question "How does electronegativity change down the group?")

If we consider elements in the same group (for example, Group 1: Li, Na, K, etc. or Group 2: Be, Mg, Ca, etc.), as we go down a group, the atomic radius increases. The valence electrons are further from the nucleus, and the shielding effect increases. This makes it harder for the nucleus to attract electrons, so electronegativity generally decreases down a group. But in our table, Li, Be, B are in the same period (Period 2), and F is also in Period 2. If we were to take a group, say Group 1 (Li, Na, K, Rb, Cs), as we go from Li to Na to K etc. down the group, electronegativity decreases (Li: ~0.98, Na: ~0.93, K: ~0.82, etc.).

Final Table (Filled)

Element name	Atomic Number	Electronegativity
Beryllium	4	1.57
Boron	5	2.04
Fluorine	9	3.98

(For the graph, you would have the plotted points as described above. The key part here was filling the table with the correct atomic numbers and electronegativity values based on standard chemical data.)

Answer:

To solve this problem about electronegativity trends, we first need to fill in the table with the correct atomic numbers and electronegativity values for the given elements (using standard periodic table data) and then plot the graph. Here's the step - by - step process:

Step 1: Recall Atomic Numbers and Electronegativity Values

• Lithium (Li):
• The atomic number of lithium is 3.
• The electronegativity of lithium (on the Pauling scale) is approximately 0.98.
• Beryllium (Be):
• The atomic number of beryllium is 4.
• The electronegativity of beryllium (on the Pauling scale) is approximately 1.57.
• Boron (B):
• The atomic number of boron is 5.
• The electronegativity of boron (on the Pauling scale) is approximately 2.04.
• Fluorine (F):
• The atomic number of fluorine is 9.
• The electronegativity of fluorine (on the Pauling scale) is approximately 3.98.

Step 2: Fill in the Table

Element name	Atomic Number	Electronegativity
Beryllium	4	1.57
Boron	5	2.04
Fluorine	9	3.98

Step 3: Plot the Data on the Graph

• X - axis (Atomic Number): Mark the points 3 (for Li), 4 (for Be), 5 (for B), and 9 (for F) on the x - axis.
• Y - axis (Electronegativity): For each atomic number, find the corresponding electronegativity value on the y - axis and plot the points (3, 0.98), (4, 1.57), (5, 2.04), and (9, 3.98). Then, connect the points (if we consider the general trend, but note that fluorine is in a different period from Li, Be, and B. If we were looking at a group, we would have elements in the same group. However, for the purpose of plotting these given elements, we just plot the individual points).

Step 4: Analyze the Trend (Optional, but related to the initial question "How does electronegativity change down the group?")

If we consider elements in the same group (for example, Group 1: Li, Na, K, etc. or Group 2: Be, Mg, Ca, etc.), as we go down a group, the atomic radius increases. The valence electrons are further from the nucleus, and the shielding effect increases. This makes it harder for the nucleus to attract electrons, so electronegativity generally decreases down a group. But in our table, Li, Be, B are in the same period (Period 2), and F is also in Period 2. If we were to take a group, say Group 1 (Li, Na, K, Rb, Cs), as we go from Li to Na to K etc. down the group, electronegativity decreases (Li: ~0.98, Na: ~0.93, K: ~0.82, etc.).

Final Table (Filled)

Element name	Atomic Number	Electronegativity
Beryllium	4	1.57
Boron	5	2.04
Fluorine	9	3.98

(For the graph, you would have the plotted points as described above. The key part here was filling the table with the correct atomic numbers and electronegativity values based on standard chemical data.)