Question

question 24 (1 point)listenrank the following atoms in order of increasing first ionization energies ($ie_1$) (i.e., lowest to highest):calcium (ca)barium (ba)nitrogen (n)arsenic (as)question 25 (1 point)listenrank the following atoms in order of decreasing first ionization energies ($ie_1$) (i.e., highest to lowest):calcium (ca)oxygen (o)selenium (se)cesium (cs)

Explanation:

For Question 24: First ionization energy (IE₁) decreases down a group as atomic size increases, making it easier to remove an outer electron. It increases across a period as nuclear charge increases. Ba is below Ca in Group 2, so Ba < Ca. As is below N in Group 15, so As < N. Group 15 elements have higher IE₁ than Group 2 elements in lower periods due to smaller atomic size and higher nuclear charge relative to valence electrons.
For Question 25: IE₁ decreases down a group and increases across a period. O is in Period 2, Group 16 with high nuclear charge and small size. Se is below O in Group 16, so O > Se. Ca is in Group 2, Period 4, with higher IE₁ than Cs (Group 1, Period 6), which has the largest atomic size here, making it easiest to remove an electron.

Answer:

Question 24 (increasing IE₁, lowest to highest):

1. barium (Ba)
2. calcium (Ca)
3. arsenic (As)
4. nitrogen (N)

Question 25 (decreasing IE₁, highest to lowest):

1. oxygen (O)
2. selenium (Se)
3. calcium (Ca)
4. cesium (Cs)