Question

1. draw a line matching the following elements to the different groups on the periodic table. radium iodine krypton lithium alkali metal alkaline earth metal halogen noble gasses 7. sheldon finds a suspicious element on the ground after exploring a nuclear waste site. the element he finds is shiny, malleable, heavy and hard. after further testing at the lab, sheldon finds the element has a high boiling point, has 5 shells, and 74 protons. what element did he find? 8. which element has a higher effect nuclear charge and why? arsenic or antimony (min of 2 sentences) antimony has a higher effect nuclear charge. the proton 9. which element has a larger atomic radius and why? sulfur or chlorine (min of 2 sentences) the chlorine 10. which element has a higher electronegativity and why? platinum or mercury (min of 2 sentences) platinum 11. extra credit: using your knowledge of electronegativity and the octet rule. why do noble gases have no electronegativity? because

Explanation:

Step1: Match elements to groups

Radium is an Alkaline - Earth Metal, Iodine is a Halogen, Krypton is a Noble Gas, Lithium is an Alkali Metal.

Step2: Identify the element in question 7

The number of protons determines the element. The element with 74 protons is Tungsten (W). It is a shiny, malleable, heavy and hard metal with a high boiling - point.

Step3: Answer question 8

Antimony has a higher effective nuclear charge than Arsenic because antimony has more protons in its nucleus, and as we move down a group in the periodic table, the number of shielding electrons increases at a slower rate than the increase in nuclear charge.

Step4: Answer question 9

Sulfur has a larger atomic radius than Chlorine. In the same period, as we move from left to right, the nuclear charge increases while the number of electron shells remains the same. Chlorine has a greater nuclear charge which pulls the electrons closer, resulting in a smaller atomic radius.

Step5: Answer question 10

Platinum has a higher electronegativity than Mercury. Platinum has a greater effective nuclear charge and a stronger attraction for electrons in a chemical bond compared to Mercury due to its electron - configuration and position in the periodic table.

Step6: Answer extra - credit question

Noble gases have no (or very low) electronegativity because they have a full outer electron shell (octet or duet for helium). They are already in a stable state and have little tendency to attract additional electrons.

Answer:

1. Radium - Alkaline Earth Metal; Iodine - Halogen; Krypton - Noble Gases; Lithium - Alkali Metal
2. Tungsten
3. Antimony has a higher effective nuclear charge because it has more protons and the shielding effect does not fully counteract the increase in nuclear charge as we move down the group.
4. Sulfur has a larger atomic radius. As we move across a period, the nuclear charge increases and pulls electrons closer, making chlorine's atomic radius smaller.
5. Platinum has a higher electronegativity due to its greater effective nuclear charge and stronger electron - attracting ability in a bond.
6. Noble gases have no (or very low) electronegativity as they have a full outer electron shell and are in a stable state with little tendency to attract electrons.