Question

1. in the graph of atomic radius vs. atomic number what trend(s) is/are apparent?

a. does the graph support the statement that atomic radius is a periodic property?
b. where would you expect the next peak to appear?

1. given your definition of ionization energy and your knowledge of atomic structure, where on the periodic table would you expect to find the highest ionization energies?
2. using your 2nd graph, which elements have the highest ionization energies?
3. using your 2nd graph, which elements have the lowest ionization energies?
4. given your definition of electronegativity and your knowledge of atomic structure, where on the periodic table would you expect to find the highest electronegativity values?
5. according to your last graph, which elements have the highest electronegativities?
6. according to your last graph, which elements have the lowest electronegativities?
7. what (if any) relationship exists between atomic radius, ionization energy, and electronegativity?

Explanation:

Step1: Analyze atomic radius trend

As atomic number increases across a period, atomic radius generally decreases due to increasing nuclear - charge attracting electrons more strongly. Down a group, atomic radius increases as new electron shells are added. Since the pattern repeats with each period, atomic radius is a periodic property.

Step2: Predict next peak for atomic radius

The peaks in atomic radius occur for alkali metals. After francium (the last alkali metal in the known periodic table), if we assume the periodic table continues, the next alkali metal (with atomic number 119) would have the next peak.

Step3: Determine location of highest ionization energies

Ionization energy is the energy required to remove an electron from an atom. Noble gases have the highest ionization energies in each period because they have a full valence - shell configuration, making it difficult to remove an electron. So, the elements in the far - right group (Group 18) of the periodic table have the highest ionization energies.

Step4: Identify elements with highest ionization energies from graph

Based on the general trend, noble gases will show up as having the highest ionization energies on the graph.

Step5: Identify elements with lowest ionization energies from graph

Alkali metals have the lowest ionization energies in each period as they have only one valence electron which is easily removed. So, alkali metals will show up as having the lowest ionization energies on the graph.

Step6: Determine location of highest electronegativity values

Electronegativity is the ability of an atom to attract electrons in a chemical bond. Fluorine is the most electronegative element. Generally, electronegativity increases across a period and decreases down a group. So, elements in the top - right of the periodic table (excluding noble gases which do not usually form bonds) have high electronegativities.

Step7: Identify elements with highest electronegativities from graph

Fluorine and other halogens will show up as having high electronegativities on the graph.

Step8: Identify elements with lowest electronegativities from graph

Alkali metals and alkaline earth metals have low electronegativities as they tend to lose electrons rather than attract them. So, these elements will show up as having low electronegativities on the graph.

Step9: Analyze relationships

Atomic radius is inversely related to ionization energy and electronegativity. As atomic radius increases (down a group), ionization energy and electronegativity decrease. This is because with a larger atomic radius, the outermost electrons are farther from the nucleus, so it is easier to remove an electron (lower ionization energy) and the atom has a weaker ability to attract electrons (lower electronegativity).

Answer:

a. Yes, the graph supports that atomic radius is a periodic property as the trend repeats with each period.
b. For the next peak in atomic radius, we would expect it for the element with atomic number 119 (assuming the periodic table continues and following the pattern of alkali - metals having the largest atomic radius in each period).

1. Noble gases (Group 18) have the highest ionization energies in the periodic table.
2. Noble gases have the highest ionization energies on the graph.
3. Alkali metals have the lowest ionization energies on the graph.
4. Elements in the top - right of the periodic table (excluding noble gases), especially fluorine, have the highest electronegativities.
5. Fluorine and other halogens have the highest electronegativities on the graph.
6. Alkali metals and alkaline earth metals have the lowest electronegativities on the graph.
7. Atomic radius is inversely related to ionization energy and electronegativity. As atomic radius increases, ionization energy and electronegativity decrease.