g. circle the element with the larger radius:
1. aluminum or sodium 2. barium or sodium
3. fluorine of chlorine 4. calcium or arsenic
h. circle the element with the lowest electronegativity:
1. sodium or magnesium 2. gallium or boron
3. iodine or fluorine 4. calcium or barium
i. cirlce correct answer:

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Accepted Answer

# Brief Explanations:
- **Atomic Radius Trends**:
    - In the periodic table, atomic radius increases down a group (due to more electron shells) and decreases across a period (as effective nuclear charge increases).
    - For G1: Sodium ($Na$) and Aluminum ($Al$) are in the same period ($3^{rd}$). Since atomic radius decreases across a period, $Na$ (group $1$) has a larger radius than $Al$ (group $13$).
    - For G2: Barium ($Ba$) is in period $6$ and Sodium ($Na$) in period $3$. As atomic radius increases down a group (more shells), $Ba$ has a larger radius.
    - For G3: Chlorine ($Cl$) and Fluorine ($F$) are in the same group ($17$). Since atomic radius increases down a group, $Cl$ (period $3$) has a larger radius than $F$ (period $2$).
    - For G4: Calcium ($Ca$) and Arsenic ($As$) are in the same period ($4^{th}$). As atomic radius decreases across a period, $Ca$ (group $2$) has a larger radius than $As$ (group $15$).
 - **Electronegativity Trends**:
    - Electronegativity increases across a period (due to increased nuclear charge) and decreases down a group (as atoms get larger, electrons are less tightly held).
    - For H1: Sodium ($Na$) and Magnesium ($Mg$) are in the same period ($3^{rd}$). As electronegativity increases across a period, $Na$ (group $1$) has lower electronegativity than $Mg$ (group $2$).
    - For H2: Gallium ($Ga$) is in period $4$ and Boron ($B$) in period $2$. As electronegativity decreases down a group, $Ga$ has lower electronegativity.
    - For H3: Iodine ($I$) and Fluorine ($F$) are in the same group ($17$). As electronegativity decreases down a group, $I$ (period $5$) has lower electronegativity than $F$ (period $2$).
    - For H4: Barium ($Ba$) is in period $6$ and Calcium ($Ca$) in period $4$. As electronegativity decreases down a group, $Ba$ has lower electronegativity.

# Answer:
- **G. Larger Radius**:
    - 1. Sodium
    - 2. Barium
    - 3. Chlorine
    - 4. Calcium
 - **H. Lowest Electronegativity**:
    - 1. Sodium
    - 2. Gallium
    - 3. Iodine
    - 4. Barium

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