Question

ionization energy14. what trend in ionization energy do you see as you go down a group on the periodic table?15. what causes this trend?16. what trend in ionization energy do you see as you go left to right across a period?it increases17. what causes this trend?18. circle the atom with the greater ionization energy in each paira. ca gab. li oc. cl sd. br ase. ba srf. o sgeneral questions19. answer the following questions for li, be, mg, naa. which has the lowest electronegativity? nab. which is the largest atom? nac. which has the lowest ionization energy? na20. answer the following questions for p, s, cl, fa. which has the highest electronegativity? fb. which is the smallest atom? fc. which has the highest ionization energy? f21. answer the following questions for au, zn, si, sa. which has the lowest electronegativity?b. which is the largest atom?c. which has the lowest ionization energy?22. answer the following questions for f, ca, as, na. which has the highest electronegativity?b. which is the smallest atom?c. which has the highest ionization energy?23. answer the following questions for k, cr, rb, moa. which has the lowest electronegativity?b. which is the largest atom?c. which has the lowest ionization energy?

Explanation:

Questions 14-17:

1. Ionization energy follows a consistent trend down a group.
2. The trend arises from increasing atomic size and shielding.
3. Across a period, increasing nuclear charge drives the trend.

Question 18:

Ionization energy increases across a period and decreases down a group.

• a. Ca is above Ga (same group, lower period)
• b. Li is above O's period (Li has higher IE than O? Correction: O is to the right of Li, but Li's 2s orbital is full; Li has higher IE than O)
• c. Cl is to the right of S (same period, higher nuclear charge)
• d. Br is below As (As is in a higher period, smaller atomic size)
• e. Ba is below Sr (Sr is higher, smaller atomic size)
• f. O is above S (same group, lower period)

Questions 19-23:

Electronegativity increases right/up, atomic size increases left/down, ionization energy increases right/up.

1. Li, Be, Mg, Na: Na is leftmost/lowest in group.
2. P, S, Cl, F: F is rightmost/topmost.
3. Au, Zn, Si, S: Au is lowest in group/leftmost; S is rightmost/topmost.
4. F, Ca, As, N: F is rightmost/topmost.
5. K, Cr, Rb, Mo: Rb is lowest in group/leftmost.

Answer:

1. It decreases
2. Atomic size increases, shielding increases, so the outermost electron is held less tightly, requiring less energy to remove.
3. Atomic size decreases, nuclear charge increases, so the outermost electron is held more tightly, requiring more energy to remove.

18.
a. Ca
b. Li
c. Cl
d. As
e. Sr
f. O
19.
a. Na
b. Na
c. Na
20.
a. F
b. F
c. F
21.
a. Au
b. Au
c. Au
22.
a. F
b. F
c. F
23.
a. Rb
b. Rb
c. Rb